Test Bank for Chemistry 2nd Edition by OpenStax- by Flowers, Neth, Theopold & Langley - Updated

TEST BANK

TEST BANK

OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 01: Essential Ideas 1. A 0.150 kg metallic block measures 25.0 mm in length, 43.0 mm in width, and 19 .0 mm in height. What is the density of the metallic block in g/cm3? (Outcome # 3) (DOK 2) A. 7.34 x 10-6 g/cm3 B. 7.34 x 10-3 g/cm3 C. 7.34 g/cm3* 2. An object with a mass of 0.255 kg and density of 2.89 g/cm 3 measures 34 mm in length and 46 mm in width. What is the height of the object? (Outcome # 3) (DOK 3) A. 5.6 cm* B. 5.6 x 10-2 cm C. 7.2 x 10-4 cm 3. How would you determine the density of an irregular object? (Outcome # 3) (DOK 3) A. It would be impossible to determine the mass of the object without more information.

B. D = m/v, so measure the mass of the object using a balance. Then to find volume, measure the height, width, and length using an appropriate measuring tool.

C. D = m/v, so measure the mass of the object using a balance. Then to find volume, fill a graduated cylinder with a known amount of water and immerse the object in the water. The amount of displaced water is the volume in cm3 or mL.* 4. What is the base unit for length in the metric system? (Outcome # 6) (DOK 1) A. m* B. km C. mm 5. What is the base unit for mass in the metric system? (Outcome # 6) (DOK 1) A. kg B. g* C. mg 6. What is the base unit for volume in the metric system? (Outcome # 6) (DOK 1) A. L* B. mL C. dL 7. It is important that scientists use units that are understood on a global level. These units are referred to as SI units which stands for _____. (Outcome # 6) (DOK 1) A. standard international units Page 1 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

B. standard intercontinental units C. international system of units* 8. Convert 18.50 ft to the SI unit for length. (Outcome # 6) (DOK 2) A. 563.9 cm B. 5.639 m* C. 0.005639 km 9. An experimental mouse weighs about 4.41 x 10-2 lbs. What would the weight be in the SI unit for mass? (Outcome # 6) (DOK 2) A. 20.0 g B. 0.0200 kg* C. 20,003 mg 10. Accuracy is defined as how close a measured value comes to a _____. (Outcome # 6) (DOK 1) A. core value B. fixed value C. true value* 11. Precision is defined as how _____ the measured values are to one another. (Outcome # 6) (DOK 1) A. common B. reproducible* C. accurate 12. An experiment requires you to make several measurements. Based on the values in the table below, what would be the best statement that represents the data set if the true value is 0.2135? (Outcome # 11) (DOK 2) Trial A Trial B Trial C 0.2139 0.2893 0.2135 0.2130 0.3210 0.2134 0.2133 0.2999 0.3712 0.2135 0.2998 0.3715 A. The measurements in Trial A are accurate and precise, Trial B is neither accurate nor precise, and Trial C is accurate however, not precise.

B. The measurements in Trial A are accurate and precise, Trial B is neither accurate nor precise, and Trial C is precise however, not accurate.

C. The measurements in Trial A are accurate and precise, Trial’s B and C are neither accurate nor precise.* 13. An experiment requires you to make several measurements. Based on the values in the table below, what would be the best statement that represents the data set if the true value is 2.73? (Outcome # 11) (DOK 2) (Paired item 1) Page 2 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

Trial A Trial B Trial C 2.73 3.00 2.77 3.05 3.03 2.79 3.09 2.99 3.31 2.44 3.01 2.05 A. The measurements in Trial B are precise, however, not accurate. Trial’s A and C are neither accurate nor precise.* B. The measurements in Trial B are accurate, however, not precise. Trial’s A and C are neither accurate nor precise.

C. The measurements in Trial’s A, B, and C are neither accurate nor precise.

14. Which of the following would be considered a chemical change? (Outcome # 9) (DOK 1) A. a rusting nail* B. melting ice C. crushing an aluminum can 15. Which of the following would be considered a physical change? (Outcome # 9) (DOK 1) A. digesting food B. burning paper C. boiling water* 16. A salt water solution is classified as what type of matter? (Outcome # 9) (DOK 1) A. homogeneous mixture* B. heterogeneous mixture C. pure substance 17. How many significant figures are in 0.0000401 kg? (Outcome # 5) (DOK 1) A. 3* B. 7 C. 2 18. How many significant figures are in 0.20 L? (Outcome # 5) (DOK 1) (Paired item 1) A. 3 B. 1 C. 2* 19. Express 1.40 x 10-3 L in decimal notation. (Outcome # 5) (DOK 1) A. 0.00140 L* B. 0.0014 L C. 0.001 L 20. What is the answer for the following calculation: (1.249 - 0.0234) x 139.37? (Outcome # 5) (DOK 2) A. 170.812 B. 170.8* C. 170.81 Page 3 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

21. What is the SI unit for mass? (Outcome # 7) (DOK 1) A. kilogram* B. gram C. milligram 22. What is the SI unit for length? (Outcome # 7) (DOK 1) A. meter* B. kilometer C. millimeter 23. What is the SI unit for temperature? (Outcome # 7) (DOK 1) A. Celsius B. Fahrenheit C. kelvin* 24. How many grams of iron are in 350 mg of iron? (Outcome # 7) (DOK 1) A. 3.50 g B. 0.350 g* C. 35.0 g 25. The prefix milli- in the metric system represents a factor of _____. (Outcome # 7) (DOK 1) A. 103 B. 10-3* C. 1/10-3 26. The prefix kilo- in the metric system represents a factor of _____. (Outcome # 7) (DOK 1) A. 103* B. 10-3 C. 1/103 27. The prefix nano- in the metric system represents a factor of _____. (Outcome # 7) (DOK 1) A. 109 B. 10-6 C. 10-9* 28. An explanation for the collection of observations is considered a _____. (Outcome # 10) (DOK 1) A. theory* B. law C. hypothesis 29. A statement about mass always being conserved in a chemical reaction is an example of a _____. (Outcome # 10) (DOK 1) A. hypothesis B. theory C. law* Page 4 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

30. The scientific method involves various techniques which allow researchers to investigate scientific questions through _____ and _____. (Outcome # 10) (DOK 1) A. analysis and observations B. observations and experimentation* C. analysis and predictions 31. Why has Galileo been called the father of modern science? (Outcome # 10) (DOK 1) A. because he made observations and conducted experiments* B. because he discovered electrochemical cells C. because he was a philosopher 32. List the basic steps of the scientific method process in the order they must be carried out.

(Outcome # 10) (DOK 1) A. observation, hypothesis, prediction, experimentation, and conclusion* B. hypothesis, observation, prediction, experimentation, and conclusion C. prediction, observation, hypothesis, experimentation, and conclusion 33. Which of the following is not part of the scientific method process? (Outcome # 10) (DOK 1) A. observation B. prediction C. discussion* 34. Which of the following would be a good example of an observation in the scientific method process? (Outcome # 10) (DOK 2) A. a researcher watching a chemical reaction B. a researcher watching a chemical reaction and noting color and temperature changes* C. a researcher setting up a chemical reaction in a flask and allowing it to stir for 2 hours 35. Which of the following would be a good example of an observation in the scientific method process? (Outcome # 10) (DOK 2) (Paired item 1) A. a physician observing a patient's reaction to some medication* B. a physician observing his watch C. a physician speaking with and observing a patient in an examination room 36. Which of the following would be good tools for making scientific observations during a chemical reaction? (Outcome # 10) (DOK 2) A. barometer, thermometer, scale B. thermometer, your eyes, clock* C. thermometer, your eyes, tape measure 37. Which of the following would be a good tool for making scientific observations after isolating a solid product from a chemical reaction? (Outcome # 10) (DOK 2) A. balance* Page 5 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

B. clock C. tape measure 38. What can be used to measure the mass of an object? (Outcome # 10) (DOK 1) A. balance* B. tape measure C. caliper 39. Which of the following would be a good example of a hypothesis in the scientific method process? (Outcome # 10) (DOK 3) A. a researcher considers that the more sunlight a green plant receives, the larger the plant will grow* B. a researcher wonders amount the effect of more sunlight on green plant growth C. a researcher watches as a green plant exposed to more sunlight grows over a period of 1 month 40. Which of the following would be a good example of a hypothesis in the scientific method process? (Outcome # 10) (DOK 3) (Paired item 1) A. a clinician confirms that taking a vitamin every day will decrease the level of tiredness in people B. a clinician tells a patient that taking a vitamin every day, may decrease the level of tiredness in people C. a clinician contemplates that taking a vitamin every day, may decrease the level of tiredness in people* 41. Which of the following would be a good example of a hypothesis in the scientific method process? (Outcome # 10) (DOK 3) (Paired item 2) A. a botanist adds 20 mL of water to his plants on a daily basis and he notices a healthy growth, therefore, he believes that adding 40 mL of water on a daily basis will enhance their growth further* B. a botanist adds 20 mL of water to his plants on a daily basis and he notices a healthy growth C. a botanist adds 20 mL of water to his plants on a daily basis and he notices a healthy growth, therefore, adding 40 mL of water on a daily basis will definitely enhance their growth further 42. Once a hypothesis has been established, it can be tested by conducting an _____. (Outcome # 10) (DOK 1) A. observation B. experiment* C. analysis 43. Which statement is correct about the scientific method process? (Outcome # 10) (DOK 1) Page 6 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

A. after testing a hypothesis, a conclusion can be drawn on whether it will be accepted or rejected* B. after testing an observation, a conclusion can be drawn on whether it will be accepted or rejected C. after testing a conclusion, it can be predicted whether a hypothesis will be accepted or rejected 44. Why is chemistry considered a central science? (Outcome # 10) (DOK 1) A. because it is a core course required for most majors in college B. because it is the fundamental science for many other disciplines* C. because it is very important in medicine 45. What is applied research? (Outcome # 10) (DOK 1) A. it deals primarily with solving practical real-world problems* B. it deals primarily with solving practical laboratory problems C. it deals primarily with the fundamentals of science that may result in future applications 46. What is basic research? (Outcome # 10) (DOK 1) A. it deals primarily with solving practical real-world problems B. it deals primarily with the fundamentals of science that may result in future applications* C. it deals primarily with solving practical laboratory problems 47. Which of the following is an example of applied research? (Outcome # 10) (DOK 2) A. a researcher tries to develop a new anti-cancer drug* B. a researcher tries to extract a newly found natural product from plants to study its medicinal properties C. a researcher studies a hormone and its prospect as a cell signaling molecule 48. Which of the following is an example of applied research? (Outcome # 10) (DOK 2) (Paired item 1) A. a researcher tries to extract a newly found natural product from plants to study its medicinal properties B. a researcher tries to study the effect of a new drug on HIV-inhibition* C. a researcher studies a hormone and its prospect as a cell signaling molecule 49. Which of the following is an example of basic research? (Outcome # 10) (DOK 2) A. a researcher tries to study the effect of a new drug on HIV-inhibition B. a researcher tries to develop a new anti-cancer drug C. a researcher studies a hormone and its prospect as a cell signaling molecule* 50. Which is of the following is an example of a physical property? (Outcome # 10) (DOK 1) A. carbon monoxide is poisonous B. acids are sour and bases are bitter* Page 7 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

C. an iron nail rusts 51. Which is of the following is an example of a physical property? (Outcome # 10) (DOK 1) (Paired item 1) A. water freezes at 273.15 K* B. carbon monoxide is poisonous C. an iron nail rusts 52. Which is of the following is an example of a physical property? (Outcome # 10) (DOK 1) (Paired item 2) A. lead forming lead oxide in the presence of air B. the color of paint* C. digestion 53. Which is of the following is an example of a chemical property? (Outcome # 10) (DOK 1) A. water boils at 100 °C B. acids are sour and bases are bitter C. an iron nail rusts* 54. Which is of the following is an example of a chemical property? (Outcome # 10) (DOK 1) (Paired item 1) A. water boils at 100 °C B. carbon monoxide is poisonous* C. a copper penny weighs 3.00 g 55. The following is an example of a chemical change. (Outcome # 10) (DOK 1) A. cutting paper B. burning paper* C. folding paper 56. The following is an example of a chemical change. (Outcome # 10) (DOK 1) (Paired item 1) A. shredding paper B. decomposing waste* C. dissolving sugar 57. A website claims that there is a natural cure for all cancers; however, doctors do not want to recommend natural remedies because it would make them obsolete. Is this statement logical? (Outcome # 10) (DOK 3) A. yes, doctors can cure all patients B. yes, doctors can cure some patients with natural remedies C. no, doctors cannot cure all patients and regardless of treatment, some patients still remain ill and die*

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 02: Atoms, Molecules, and Ions 1. Structural isomers are considered molecules with the same ____________. (Outcome # 1,5,9) DOK 1 A. kinds and number of atoms but a different arrangement of these atoms* B. number of electrons and protons but a different number of neutrons C. molecular formula but with a different overall charge 2. Which of the following is not a correct element name-symbol combination? (Outcome # 1) DOK 1 A. copper, Cu B. arsenic, Ar* C. gold, Au 3. Isotopes of carbon differ with respect to the number of _________. (Outcome # 1,8) DOK 1 A. protons B. neutrons* C. electrons 4. Elements in group 17 are considered _____________. (Outcome # 1,2) DOK 1 A. alkali Metals B. halogens* C. noble Gases 5. Due to periodicity, which of the following elements has chemical behavior similar to that of Oxygen? (Outcome # 1,2,8) DOK 1 A. bromine B. sulfur* C. carbon 6. Where would you expect to find a stored bottle of HCl in the laboratory? (Outcome # 5) (DOK 1) A. in the storage cabinet labeled strong bases B. in the storage cabinet labeled strong acids* C. in the storage cabinet labeled solvents 7. Where would you expect to find a stored bottle of NaOH in the laboratory? (Outcome # 5) (DOK 1) (Paired item 1) A. in the storage cabinet labeled strong bases* B. in the storage cabinet labeled strong acids C. in the storage cabinet labeled solvents Page 1 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

8. Which of the following would be considered a caustic base? (Outcome # 5) (DOK 1) A. HNO3 B. H2SO4 C. NaOH* 9. Elements arranged horizontally in the periodic table are in the same_____? (Outcome # 2) (DOK 1) A. group or family B. period* C. column 10. Which elements are considered noble gases? (Outcome # 2) (DOK 1) A. He, Ne, Ar* B. H, N, O C. F, Cl, Br 11. Chlorine gas is considered a _____? (Outcome # 2) (DOK 1) A. noble gas B. halogen* C. chalcogen 12. Oxygen gas is considered a _____? (Outcome # 2) (DOK 1) (Paired item 1) A. noble gas B. halogen C. chalcogen* 13. What is the correct formula for acetic acid? (Outcome # 2) (DOK 1) A. CH3CO2H* B. CH3CO2C. CH3CO2H2 14. What is the correct formula for lead(II) nitrate? (Outcome # 2) (DOK 1) (Paired item 1) A. Pd(NO3)2 B. Pb(NO3) C. Pb(NO3)2* 15. What is the name for iron(III) chloride? (Outcome # 2) (DOK 1) A. FeCl2 B. FeCl3* C. FeCl4 16. What is the correct name for the precipitate formed when mixing potassium carbonate and nickel(II) chloride? (Outcome # 2) (DOK 2) A. potassium chloride B. nickel(II) carbonate* C. nickel(III) carbonate Page 2 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

17. Which of the following gases exists as a diatomic molecule? (Outcome # 9) (DOK 1) A. krypton B. hydrogen* C. argon 18. In mass spectrometry, species are separated based off their _____? (Outcome # 7) (DOK 2) A. mass-to-charge ratio* B. mass C. charge 19. Which statement is correct about chlorine-35 and chorine-37? (Outcome # 8) (DOK 1) A. They have the same number of protons and electrons, but a different number of neutrons.* B. They have a different number of protons and electrons, but the same number of neutrons.

C. They have the same number of protons, but a different number of electrons and neutrons.

20. What is the overall charge on a sulfate ion? (Outcome # 8) (DOK 1) A. 0 B. -1 C. -2* 21. What is the overall charge on a phosphate ion? (Outcome # 8) (DOK 1) A. -2 B. -3* C. -1 22. Which of the following would be considered a corrosive acid? (Outcome # 5) (DOK 1) A. HNO3* B. NaOH C. KOH 23. Which list of elements contains ONLY nonmetals? (Outcome # 1,9) (DOK 1) A. helium, carbon, gold B. sodium, chromium, copper C. phosphorus, nitrogen, oxygen* 24. The formula for potassium cyanide is KCN and the formula for calcium fluoride is CaF 2. What is the formula for calcium cyanide? (Outcome # 1,7,8,9) (DOK 2) A. Ca2CN B. CaCN C. Ca(CN)2* 25. Using the periodic table, what is the atomic number of argon? (Outcome # 1,9) (DOK 2) A. 26.98 Page 3 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

B. 13* C. 18 26. Which of the following is an ionic compound? (Outcome # 1,9) (DOK 1) A. CO B. HCl C. Na2O* 27. Structural isomers are considered molecules with the same ____________. (Outcome # 1,9) (DOK 2) A. kinds and number of atoms but a different arrangement of these atoms* B. number of electrons and protons but a different number of neutrons C. molecular formula but with a different overall charge 28. The Greek philosopher Democritus phrased what word for a tiny piece of matter that cannot be divided? (Outcome # 1,9) (DOK 1) A. element B. atom* C. electron 29. Who provided evidence for the existence of a nucleus in an atom? (Outcome # 1,9) (DOK 1) A. John Dalton B. J.J. Thomson C. Ernest Rutherford* 30. Within the nucleus, the positive charge is __________. (Outcome # 1,9) (DOK 2) A. concentrated in the center of an atom* B. spread evenly throughout an atom C. concentrated at multiple sites in an atom 31. Which statement about subatomic particles is NOT true? (Outcome # 1,9) (DOK 2) A. Protons and neutrons have almost the same mass.

B. Protons and electrons have opposite charges.

C. Protons and neutrons have the same charge* 32. The number of protons in one atom of an element is that element’s __________. (Outcome # 1,9) (DOK 1) A. mass number B. atomic mass C. atomic number* 33. To calculate the number of neutrons in an atom, you would subtract (Outcome # 1,9) (DOK 1) A. mass number from atomic number B. atomic number from mass number* C. atomic number from electron number Page 4 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

34. Which of the following is not a correct element name-symbol combination? (Outcome # 1,9) (DOK 1) A. copper, Cu B. arsenic, Ar* C. gold, Au 35. Isotopes of carbon differ with respect to the number of _________. (Outcome # 1,9) (DOK 1) A. protons B. neutrons* C. electrons 36. The fact that LiBr is 7.99 % lithium and 92.01 % bromine by mass regardless of its origin is an example of _____. (Outcome # 9) (DOK 1) A. law of definite proportions* B. law of conservation of mass C. Dalton’s atomic theory 37. Which of the following elements form +2 ions? (Outcome # 9) (DOK 1) A. strontium, magnesium, calcium* B. lithium, sodium, potassium C. sodium, magnesium, aluminum 38. Which of the following elements form +1 ions? (Outcome # 9) (DOK 1) A. strontium, magnesium, calcium B. lithium, sodium, potassium* C. sodium, magnesium, aluminum 39. How many neutrons are in carbon-12? (Outcome # 9) (DOK 1) A. 6* B. 7 C. 8 40. How many neutrons are in chlorine-37? (Outcome # 9) (DOK 1) A. 18 B. 20* C. 18.5 41. Identify the chalcogen that has 18 neutrons in the nucleus. (Outcome # 9) (DOK 2) A. sulfur-32 B. sulfur-33 C. sulfur-34* 42. The chemical symbol for cobalt is _____. (Outcome # 7) (DOK 1) A. Co* B. cO Page 5 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

C. CO 43. What is the chemical symbol for manganese? (Outcome # 7) (DOK 1) A. Mn* B. Mg C. mn 44. Which element is represented by the chemical symbol Th? (Outcome # 7) (DOK 1) A. thallium B. thorium* C. tantalum 45. Which element is represented by the chemical symbol Tl? (Outcome # 7) (DOK 1) A. tantalum B. thallium* C. thorium 46. What is an anion? (Outcome # 7) (DOK 1) A. An anion is defined as an atom that has lost electrons and forms a negative charge.

B. An anion is defined as an atom that has gained electrons and forms a negative charge.* C. An anion is defined as an atom that has gained electrons and forms a positive charge.

47. What is a cation? (Outcome # 7) (DOK 1) A. A cation is defined as an atom that has lost electrons and forms a positive charge.* B. A cation is defined as an atom that has gained electrons and forms a negative charge.

C. A cation is defined as an atom that has gained electrons and forms a positive charge.

48. Hafnium atom is located in which block on the periodic table? (Outcome # 7) (DOK 1) A. p-block B. d-block* C. f-block 49. Lanthanum atom is located in which block on the periodic table? (Outcome # 7) (DOK 1) A. p-block B. d-block C. f-block* 50. Determine the formula for copper(II) nitrate. (Outcome # 8) (DOK 2) A. Cu2NO3 B. CuNO3 C. Cu(NO3)2* 51. What is the name of Fe2O3? (Outcome # 8) (DOK 2) A. iron(II) oxide Page 6 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

B. iron(III) oxide* C. iron(IV) oxide 52. What is the correct formula for cobalt(III) chloride? (Outcome # 8) (DOK 2) A. CoCl2 B. CoCl3* C. Co3Cl 53. What is the correct formula for iodine monochloride? (Outcome # 8) (DOK 2) A. ICl2 B. I2Cl C. ICl*

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 03: Composition of Substances and Solutions 1. Which of the following compounds contains the largest number of atoms? (Outcome # 1,2) DOK 2 A. 1.00 mole of NH3 B. 1.00 mole of H2SO4* C. 1.00 mole of HBr 2. What is the molar mass of (NH4)3PO4? (Outcome # 1,2) DOK 2 A. 113 g B. 121 g C. 149 g* 3. What is the mass in grams of 6.022 x 1023 molecules of CO2? (Outcome # 1,2) DOK 3 A. 22 g B. 44 g* C. 66 g 4. What is the total number of atoms contained in 2.00 moles of iron? (Outcome # 1,2) DOK 2 A. 118 B. 6.02 x 1023 C. 1.2 x 1024* 5. What is the molar mass of K2CO3? (Outcome # 1,2) DOK 2 A. 138 g/mol * B. 106 g/mol C. 99 g/mol 6. What is the total number of atoms contained in 1.00 mole of sodium? (Outcome # 1,2,9) DOK 2 A. 118 B. 6.02 x 1023* C. 1.2 x 1024 7. If a hazardous bottle is labeled 20.2 percent by mass Hydrochloric Acid, HCl, with a density of 1.096 g/mL, calculate the molarity of the HCl solution. (Outcome # 1,2,5,8,9,10) (DOK 3) A. 6.07 M* B. 0.22 M C. 14.7 M 8. To dilute a HCl solution from 0.500 M to 0.100 M the final volume must be: (Outcome # 1,2,4,5,8) DOK 2 Page 1 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

A. 1/5 the original volume B. 5 times the original volume* C. 50 L 9. How would you prepare a 1 M solution of sodium hydroxide? (Outcome # 5) (DOK 3) A. add 40.0 grams of sodium hydroxide to 1 L of water* B. add 40.0 grams of sodium hydroxide to 100 L of water C. add 40.0 grams of sodium hydroxide to 10 L of water 10. How would you prepare a 0.5 M solution of sodium hydroxide? (Outcome # 5) (DOK 3) (Paired item 1) A. add 40.0 grams of sodium hydroxide to 1 L of water B. add 20.0 grams of sodium hydroxide to 1 L of water* C. add 20.0 grams of sodium hydroxide to 10 L of water 11. An experiment requires 15.0 mL of a 0.100 M solution of HCl. If you have a 12.0 M HCl stock solution in the laboratory, how would you prepare enough 0.1 M solution to run at least 3 experiments? (Outcome # 5) (DOK 3) A. add 0.833 mL 12 M HCl stock solution to 99.167 mL water* B. add 0.833 mL 12 M HCl stock solution to 49.167 mL water C. add 0.833 mL 12 M HCl stock solution to 199.167 mL water 12. What is the mass in grams of 1.59 moles of aluminum oxide? (Outcome # 2) (DOK 2) A. 162 g* B. 0.0156 g C. 64.1 g 13. What is the mass in grams of 0.852 moles of ferric oxide? (Outcome # 2) (DOK 3) (Paired item 1) A. 5.34 x 10-3 g B. 187 g C. 136 g* 14. How many moles are in 1.77 kg of cuprous sulfate? (Outcome # 2) (DOK 3) A. 7.93 x 10-3 moles B. 7.93 moles* C. 395 moles 15. How many grams are in 2.05 x 1023 molecules of dinitrogen pentoxide? (Outcome # 2) (DOK 3) A. 317 g B. 36.8 g* C. 0.00315 g 16. How many grams are in 1.02 x 1022 molecules of nitric acid? (Outcome # 2) (DOK 3) (Paired item 1) Page 2 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

A. 1.07 g* B. 3720 g C. 2.69 x 10-4 g 17. What is the total number of atoms contained in 2.11 moles of nickel? (Outcome # 2) (DOK 2) A. 2.85 x 1023 atoms B. 1.27 x 1024 atoms* C. 3.50 x 10-24 atoms 18. How many atoms are in 1.00 mole of Au? (Outcome # 2) (DOK 2) (Paired item 1) A. 6.02 x 1023 atoms* B. 1.66 x 10-24 atoms C. 197 atoms 19. A 44.8 g rhodium sample contains how many rhodium atoms? (Outcome # 2) (DOK 3) A. 2.62 x 1023 atoms* B. 6.02 x 1023 atoms C. 2.70 x 1025 atoms 20. What is the molar mass of potassium nitrate? (Outcome # 2) (DOK 2) A. 85.10 g/mol B. 140.20 g/mol C. 101.10 g/mol* 21. Commercial grade fuming nitric acid contains about 90% HNO 3 by mass with a density of 1.50 g/mL, calculate the molarity of the HNO3 solution. (Outcome # 9) (DOK 3) A. 0.214 M B. 21.4 M* C. 2.14 M 22. Which of the following is a method used to allow scientists to determine an empirical formula and identify an organic compound by combusting a sample and the resulting combustion products are quantitatively analyzed? (Outcome # 7) (DOK 1) A. gravimetric analysis B. combustion analysis* C. thermal analysis 23. A 3.00 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 8.80 g of CO2 and 5.40 g of H2O are produced. What is the empirical formula of the unknown? (Outcome # 7) (DOK 3) A. CH3* B. CH C. CH2 Page 3 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

24. A 0.125 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 0.4225 g of CO2 and 0.0865 g of H2O are produced. What is the empirical formula of the unknown? (Outcome # 7) (DOK 3) (Paired item 1) A. CH3 B. CH* C. CH2 25. An unknown organic compound (0.315 g) containing only C, H, and O produces 0.771 of CO 2 and 0.105 g of H2O when it undergoes complete combustion. The approximate molar mass is 108 g/mol. Which of the following compounds could be the identification of the unknown? (Outcome # 7) (DOK 3) A. para-Cresol, CH3C6H4(OH) B. Benzyl alcohol, C6H5CH2OH C. 1,2-Benzoquinone, C6H4O2* 26. Which of the following is an experimental technique used to determine the mass percent of elements found in a compound? (Outcome # 7) (DOK 1) A. gravimetric analysis B. mass analysis C. elemental analysis* 27. An unknown hydrocarbon compound was analyzed for hydrogen by elemental analysis and results show that it contains 15.88 % H. What is the empirical formula? (Outcome # 7) (DOK 2) A. C4H9* B. C8H18 C. C12H27 28. A 5.91 g unknown sample analyzed by elemental analysis revealed a composition of 37.51 % C. In addition, it was determined that the sample contains 1.4830 x 10 23 hydrogen atoms and 1.2966 x 1023 oxygen atoms. What is the empirical formula? (Outcome # 7) (DOK 3) A. C6H8O7* B. C5H6O3 C. C8H16O5 29. What is the concentration in ppm of a 3.7 L solution (d = 1.00 g/mL) containing 4.21 x 10 -7 kg of the pesticide DDT? (Outcome # 8) (DOK 2) A. 1.14 x 10-1 ppm* B. 1.14 x 102 ppm C. 1.14 x 101 ppm 30. When a salt is dissolved in water, it is represented by the following notation in a chemical reaction? (Outcome # 6) (DOK 1) Page 4 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

A. (aq)* B. (l) C. (s) 31. How is a solid phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s)* B. (g) C. (l) 32. How is a liquid phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s) B. (g) C. (l)* 33. How is a gas phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s) B. (g)* C. (l) 34. What are the proper units for molar mass in chemistry? (Outcome # 6) (DOK 1) A. amu B. g/mol* C. g/mmol 35. How many atoms can be found in a mole of mercury? (Outcome # 2) (DOK 2) A. 201 atoms B. 6.02 x 1023 atoms* C. 1.21 x 1026 atoms 36. A 21.8 g sample of water contains how many water molecules? (Outcome # 2) (DOK 3) A. 7.29 x 1023 molecules* B. 6.02 x 1023 molecules C. 2.01 x 10-24 molecules 37. A sample has a molar mass of 143 g/mol, identify the sample. (Outcome # 2) (DOK 1) A. AuCl B. AcCl C. AgCl* 38. What is the molar mass of 2.50 g of an unknown sample dissolved in 130. mL of water with a concentration of 0.480 M? (Outcome # 4) (DOK 3) A. 0.062 g/mol B. 8.65 g/mol C. 40.1 g/mol* 39. 2.50 g of an unknown base is dissolved in 289 mL of water and has a concentration of 0.216 M. What is the identification of the unknown base? (Outcome # 4) (DOK 3) Page 5 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

A. NaOH* B. LiOH C. KOH 40. How many grams of Hydrogen are present in three moles of Hydrogen? (Outcome # 1,5,9) (DOK 1) A. two grams B. six grams* C. one gram 41. Which of the following compounds contains the largest number of atoms? (Outcome # 1,9) (DOK 2) A. 1.00 mole of NH3 B. 1.00 mole of H2SO4* C. 1.00 mole of HBr 42. How many atoms are in 12.8 g of copper metal? (Outcome # 6) (DOK 2) A. 7.71 x 1024 atoms B. 1.21 x 1023 atoms* C. 3.34 x 10-25 atoms 43. How many grams contain 1.45 x 1021 zinc atoms? (Outcome # 6) (DOK 2) A. 1.57 x 10-1 g* B. 5.71 x 1046 g C. 2.41 x 10-3 g 44. How many moles are in 11.0 g of silver metal? (Outcome # 6) (DOK 1) A. 9.81 moles B. 1.19 x 103 moles C. 1.02 x 10-1 moles* 45. What is Avogadro’s number? (Outcome # 6) (DOK 1) A. 6.022 x 1023 particles/mole* B. 6.022 x 1022 particles/mole C. 6.022 x 1024 particles/mole 46. Which of the following 85.0 g samples contain the greatest number of atoms? (Outcome # 6) (DOK 3) A. zinc* B. gold C. zirconium 47. Which of the following 49.5 g samples contain the fewest number of atoms? (Outcome # 6) (DOK 3) (Paired item 1) A. lead* B. platinum Page 6 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

C. iron 48. How many atoms are in 1 mole of calcium? (Outcome # 6) (DOK 1) A. 6.022 x 1023 atoms* B. 6.022 x 10-23 atoms C. 6.022 x 1022 atoms 49. How many moles contain 6.022 x 1023 lithium atoms? (Outcome # 6) (DOK 1) A. 6.022 x 1023 moles B. 1 mole* C. 2 moles

Page 7 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 04: Stoichiometry of Chemical Reactions 1. When Mg(OH)2 reacts with H2SO4 what are the products? (Outcome # 1,2,6) DOK 2 A. Mg(OH)2 and H2SO4 B. MgSO4 and H2O* C. MgO and H2SO4 2. Which of the following is a strong acid? (Outcome # 1,3,5,9) DOK 1 A. HNO3* B. CaSO4 C. NH3 3. Which of the following is a strong acid when mixed in water? (Outcome # 1,2,5) DOK 1 A. HClO B. HBr* C. HNO2 4. What are the products of the reaction between barium hydroxide and hydrogen chloride?

(Outcome # 1,2,5,6,9) DOK 2 A. Barium chloride and water* B. Barium hydroxide and water C. Barium chloride and barium hydride 5. The symbol that separates the reactants from products in a reaction and means “to yield” is ________. (Outcome # 1,5,6,9) DOK 1 A. + B. (s) C. * 6. The chemical reaction CaCO3 CaO + CO2 is classified as a (Outcome # 1,9) DOK 1 A. synthesis reaction B. decomposition reaction* C. single-replacement reaction 7. How many mole ratios can be correctly obtained from the balanced chemical equation DOK 2 (Outcome # 1,2,8,9) 2Al2O3(l)  4Al(s) + 3O2(g)?

A. 3 B. 4 C. 6* Page 1 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

8. Fewer steps are required to solve stoichiometry problems when (Outcome # 1,2) (DOK 2) A. the amount of reactant is given in grams and the product is sought in grams.

B. the amount of reactant is given in moles and the product is sought in moles.* C. the amount reactant is given in grams and the product is sought in liters.

9. Ozone, O3, is a product in automobile exhaust by the reaction represented by the equation NO2(g) + O2(g) NO(g) + O3(g). What mass of ozone is predicted to form from the reaction of 2.0 g NO2 in a car’s exhaust and excess oxygen? (Outcome # 1,2) (DOK 3) A. 1.1 g O3 B. 1.8 g O3 C. 2.1 g O3* 10. A 15.0 g sample of a white, solid substance, is heated in the presence of air. The solid remaining after heating has a mass of 12.6 g. The reaction that took place must have been a/an: (Outcome # 1,2) DOK 3 A. decomposition reaction* B. displacement reaction C. combination reaction 11. When mixing a strong acid and water together, it is recommended that you do which of the following? (Outcome # 5) (DOK 1) A. add water to the strong acid B. add the strong acid to water* C. add them in any order 12. What are the products when reacting potassium hydroxide and hydrogen chloride?

(Outcome # 5) (DOK 2) A. potassium chloride and water* B. potassium hydroxide and water C. no reaction 13. What precipitate forms when mixing copper(II) sulfate and sodium sulfate? (Outcome # 5) (DOK 2) A. copper(I) sulfate B. copper(III) sulfate C. no precipitate forms* 14. What precipitate forms when mixing silver(I) nitrate and sodium chloride? (Outcome # 5) (DOK 2) (Paired item 1) A. silver(I) chloride* B. sodium nitrate C. no precipitate forms 15. What precipitate forms when mixing lead(II) nitrate and sodium iodide? (Outcome # 5) (DOK 2) (Paired item 2) A. sodium nitrate Page 2 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

B. lead(II) iodide* C. no precipitate forms 16. Which of the following reactions are written correctly? (Outcome # 5) (DOK 2) A. H2SO4(aq) + 2 NaOH(aq)  Na2SO4(aq) + 2H2O(l)* B. 2HCl(aq) + K2OH(aq)  2KCl(aq) + H2O(l) C. 2HSO4(aq) + 2NaOH(aq)  2NaSO4(aq) + 2H2O(l) 17. Which of the following reactions are written correctly? (Outcome # 5) (DOK 2) (Paired item 1) A. H2NO3(aq) + 2NaOH(aq)  Na2NO3(aq) + 2H2O(l) B. HNO3(aq) + K2OH(aq)  K2NO3(aq) + H2O(l) C. HNO3(aq) + NaOH(aq)  NaNO3(aq) + H2O(l)* 18. What is the correct name for the precipitate formed when mixing potassium carbonate and nickel(II) chloride? (Outcome # 2) (DOK 2) A. potassium chloride B. nickel(II) carbonate* C. nickel(III) carbonate 19. The reaction HNO3(aq) + NaOH(aq)  NaNO3(aq) + H2O(l) is an example of _____?

(Outcome # 9) (DOK 1) A. an acid-base reaction* B. a combustion reaction C. a precipitation reaction 20. The reaction CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) is an example of _____? (Outcome # 9) (DOK 1) (Paired item 1) A. an acid-base reaction B. a combustion reaction* C. a precipitation reaction 21. Which is the correct balanced reaction for the combustion of octane? (Outcome # 9) (DOK 2) A. 2C8H18(g) + 25O2(g)  16CO2(g) + 18H2O(g)* B. C8H18(g) + 12.5O2(g)  8CO2(g) + 9H2O(g) C. C8H18(g) + 25O(g)  8CO2(g) + 9H2O(g) 22. If 1.50 moles of nitrogen gas reacts with an excess of hydrogen gas, what mass of ammonia would be produced? (Outcome # 9) (DOK 3) A. 34.1 g B. 51.1 g* C. 25.5 g 23. If 250.3 L of hydrogen gas (d = 0.0899 g/L) reacts with an excess of nitrogen gas, what mass of ammonia would be produced? (Outcome # 9) (DOK 3) Page 3 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

A. 253 g B. 380 g C. 127 g* 24. What instrument is used during an acid-base titration experiment to deliver the titrant?

(Outcome # 4) (DOK 1) A. buret* B. syringe C. pipette 25. The combustion of 0.136 kg of methane in the presence of excess oxygen produces 353 g of carbon dioxide. What is the percent yield? (Outcome # 8) (DOK 3) A. 38.5 % B. 94.6 %* C. 0.946 % 26. The combustion of 0.374 kg of methane in the presence of excess oxygen produces 0.983 kg of carbon dioxide. What is the percent yield? (Outcome # 8) (DOK 3) (Paired item 1) A. 38.1 % B. 95.8 %* C. 0.958 % 27. What mass of methane is required to produce 1.130 kg of carbon dioxide during combustion? (Assume the reaction undergoes complete combustion.) (Outcome # 8) (DOK 3) A. 41.18 g B. 0.4118 g C. 411.8 g* 28. The combustion of 0.1240 kg of propane in the presence of excess oxygen produces 0.3110 kg of carbon dioxide. What is the theoretical yield? (Outcome # 8) (DOK 3) A. 371.2 g* B. 0.8377 g C. 0.3712 g 29. Which is the correct balanced reaction for the combustion of octane? (Outcome # 8) (DOK 2) A. 2C8H18(l) + 25O2(g)  16CO2(g) + 18H2O(g)* B. C8H18(l) + 25O(g)  8CO2(g) + 9H2O(g) C. C8H18(l) + 12.5O2(g)  8CO2(g) + 9H2O(g) 30. Which is the correct balanced reaction for the combustion of methane? (Outcome # 8) (DOK 2) (Paired item 1) A. CH4(g) + O2(g)  CO2(g) + H2O(g) B. CH4(g) + 4O(g)  CO2(g) + 2H2O(g) Page 4 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

C. CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)* 31. Write a balanced reaction for the neutralization of HBr upon the addition of KOH. (Outcome # 8) (DOK 2) A. HBr(aq) + KOH(aq)  KBr(aq) + H2O(l)* B. HBr(aq) + KOH(aq)  KBr(s) + H2O(l) C. HBr(aq) + KOH(aq)  KBr(l) + H2O(l) 32. The combustion of 0.296 kg of propane produces 713 g of carbon dioxide. What is the percent yield? (Outcome # 8) (DOK 3) A. 80.5 %* B. 0.805 % C. 124 % 33. 0.450 kg of octane burned during combustion produces 1.25 kg of carbon dioxide. What is the percent yield? (Outcome # 8) (DOK 3) A. 0.901 % B. 90.1 %* C. 36.0 % 34. How many moles of HCl are needed to completely react with 50.0 mL of 0.250 M NaOH solution? (Outcome # 8) (DOK 2) A. 1.25 x 10-2 moles* B. 1.25 x 101 moles C. 2.50 x 10-1 moles 35. How many moles of KOH are needed to neutralize 35.0 mL of 0.115 M HNO 3 solution?

(Outcome # 8) (DOK 2) A. 4.03 x 10-3 moles* B. 4.03 x 101 moles C. 1.15 x 10-1 moles 36. How many moles of NaOH are needed to neutralize 15.0 mL of 0.235 M HCl solution?

(Outcome # 8) (DOK 2) (Paired item 1) A. 3.53 x 101 moles B. 2.35 x 10-1 moles C. 3.53 x 10-3 moles* 37. What is the oxidation number of Cr in a dichromate anion? (Outcome # 8) (DOK 2) A. +6* B. +3 C. +2 38. What is the oxidation number of Mn in a permanganate anion? (Outcome # 8) (DOK 2) A. +4 B. +7* Page 5 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

C. +2 39. How many electrons are transferred during the oxidation of iron metal to form rust?

(Outcome # 8) (DOK 2) A. 3 electrons B. 6 electrons C. 12 electrons* 40. What is the oxidation number of free elements? (Outcome # 8) (DOK 1) A. 0* B. +1 C. +2 41. What is the oxidation number of diatomic elements? (Outcome # 8) (DOK 1) A. 0* B. +1 C. +2 42. What is the oxidation number of hydrogen in H2O2? (Outcome # 8) (DOK 1) A. +2 B. +1* C. 0 43. What is the oxidation number of oxygen in H2O2? (Outcome # 8) (DOK 2) A. -2 B. -1* C. 0 44. What is the net ionic equation for the reaction between CoCl2 and an alkali hydroxide?

(Outcome # 3) (DOK 2) A. Co2+(aq) + 2OH-(aq)  Co(OH)2(s)* B. Na+(aq) + Cl-(aq)  NaCl(s) C. Co3+(aq) + 3OH-(aq)  Co(OH)3(s) 45. Write the net ionic equation for a reaction between a strong acid and strong base.

(Outcome # 3) (DOK 3) A. HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l) B. H+(aq) + OH-(aq)  H2O(l)* C. H2O(l)  H+(aq) + OH-(aq) 46. Identify the reactants in the following reaction: 2 CH3OH(l) + 3 O2(g)  2 CO2(g) + 4 H2O(g) (Outcome # 6) (DOK 1) A. CH3OH B. CH3OH and O2* C. CO2 and H2O Page 6 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

47. If 23.6 g of hydrogen gas reacts with 28.3 g of nitrogen gas, what is the maximum amount of product that can be produced? (Outcome # 6) (DOK 3) A. 34.4 g* B. 133 g C. 68.8 g 48. The catalytic decomposition of hydrogen peroxide occurs with the addition of KI. If 10 mL of a saturated KI solution was added to 315 g of hydrogen peroxide, how much oxygen gas would be produced? (Outcome # 6) (DOK 3) A. 296 g B. 593 g C. 148 g* 49. What is the oxidation number of oxygen gas in the combustion of pentane reaction?

(Outcome # 6) (DOK 3) A. 0* B. -1 C. -2 50. Which is the reducing agent in the combustion of methanol? (Outcome # 6) (DOK 3) A. CH3OH* B. O2 C. CO2 51. Which is the oxidizing agent in the combustion of methanol? (Outcome # 6) (DOK 3) A. CH3OH B. O2* C. CO2 52. Propane is used as a fuel source on many barbeque grills. What is undergoing oxidation during the burning of propane while grilling? (Outcome # 6) (DOK 3) A. CH3CH2CH3* B. O2 C. CO2 53. Propane is used as a fuel source on many barbeque grills. What is undergoing reduction during the burning of propane while grilling? (Outcome # 6) (DOK 3) (Paired item 1) A. CH3CH2CH3 B. O2* C. CO2 54. When a salt is dissolved in water, it is represented by the following notation in a chemical reaction? (Outcome # 6) (DOK 1) A. (aq)* B. (l) Page 7 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

C. (s) 55. How is a solid phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s)* B. (g) C. (l) 56. How is a liquid phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s) B. (g) C. (l)* 57. How is a gas phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s) B. (g)* C. (l) 58. The reaction NH3(aq) + H2O(l)  OH-(aq) + NH4+(aq) is an example of _____? (Outcome # 9) (DOK 1) A. a combustion reaction B. an acid-base reaction* C. a precipitation reaction 59. Which of the following is a strong acid? (Outcome # 1,3,9) (DOK 1) A. HNO3* B. CaSO4 C. NH3 60. Which of the following is a strong acid when mixed in water? (Outcome # 1,5,9) (DOK 2) A. HClO B. HBr* C. HNO2 61. When Ca(OH)2 reacts with H2SO4 what are the products? (Outcome # 1,5,6,9) (DOK 2) A. Ca(OH)2 and H2SO4 B. CaSO4 and H2O* C. CaO and H2SO4 62. What are the products of the reaction between barium hydroxide and hydrogen chloride?

(Outcome # 1,5,6,9) (DOK 2) A. barium chloride and water* B. barium hydroxide and water C. barium chloride and barium hydride 63. The symbol that separates the reactants from products in a reaction and means “to yield” is ________. (Outcome # 1,5,6,9) (DOK 1) A. + Page 8 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

B. (s) C. * 64. The chemical reaction CaCO3 CaO + CO2 is classified as a (Outcome # 1,5,9) (DOK 1) A. synthesis reaction B. decomposition reaction * C. single-replacement reaction 65. What is the correct name for the salt formed between KOH and HCl? (Outcome # 9) (DOK 2) A. potassium hydride B. potassium chloride* C. potassium hydroxide 66. What is the correct formula for the precipitate formed between NaNO 3 and mercury nitrate? (Outcome # 9) (DOK 3) A. Hg2NO3 B. Hg(NO3)2 C. no reaction between NaNO3 and mercury nitrate* 67. Which compound is insoluble in water? (Outcome # 2) (DOK 2) A. CaCO3* B. LiOH C. Na2S 68. In a chemical reaction, the right side of the yield arrow is where the _____ can be found.

(Outcome # 2) (DOK 1) A. reactants B. products* C. both reactant and products 69. The coefficients in front of the substances in a chemical reaction indicate the number of each type of _____. (Outcome # 2) (DOK 1) A. ionic bond B. covalent bond C. molecule* 70. When balancing a chemical reaction, the following may need to be changed? (Outcome # 2) (DOK 1) A. subscripts B. coefficients* C. phases 71. What is the oxidation state of oxygen in H2O2? (Outcome # 2) (DOK 2) A. 0 B. -1* C. -2 Page 9 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

72. Which of the following is a weak acid? (Outcome # 2) (DOK 1) A. acetic acid* B. sulfuric acid C. perchloric acid 73. Which of the following is a weak base? (Outcome # 2) (DOK 1) A. sodium hydroxide B. potassium hydroxide C. ammonia* 74. Hydrogen gas can react with some halogen to produce hydrogen chloride. Write a correct balanced reaction and identify the oxidizing agent. (Outcome # 2) (DOK 3) A. H2(g) + Cl2(g)  2HCl(g) and Cl2 is the oxidizing agent* B. H2(g) + Cl2(g)  2HCl(g) and H2 is the oxidizing agent C. H2(g) + Cl2(g)  2HCl(g) and HCl is the oxidizing agent 75. Which of the following is a redox reaction? (Outcome # 2) (DOK 2) A. Zn(s) + 2 HCl(aq)  ZnCl2(aq) + H2(g)* B. HNO3(aq) + KOH(aq)  KNO3(aq) + H2O(l) C. ZnSO4(aq) + Hg2(NO3)2(aq)  Hg2SO4(s) + Zn(NO3)2(aq) 76. Which of the following is an acid-base reaction? (Outcome # 2) (DOK 2) A. Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g) B. HClO4(aq) + NaOH(aq)  NaClO4(aq) + H2O(l)* C. Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq) 77. Which of the following is a precipitation reaction? (Outcome # 2) (DOK 2) A. Ca(s) + 2HCl(aq)  CaCl2(aq) + H2(g) B. H2SO4(aq) + 2NaOH(aq)  Na2SO4(aq) + 2H2O(l) C. 2NaOH(aq) + MgCl2(aq)  2 NaCl(aq) + Mg(OH)2(s)* 78. Solid potassium chlorate readily decomposes in the presence of a catalyst and heat to form oxygen gas and potassium salt. What is the correct balanced reaction? (Outcome # 5) (DOK 3) A. 2KClO3(s)  2KCl(s) + 3O2(g)* B. KClO4(s)  KCl(s) + 2O2(g) C. KClO3(s)  KCl(s) + 3O(g) 79. Hydrogen peroxide readily decomposes in the presence of a catalyst to form oxygen gas and water. What is the correct balanced reaction? (Outcome # 5) (DOK 3) A. 4HO2(aq)  3O2(g) + 2H2O(l) B. H2O2(aq)  O(g) + H2O(l) C. 2H2O2(aq)  O2(g) + 2H2O(l)* 80. The combustion of propane produced 8.53 g of carbon dioxide. What mass of propane is required if the yield is 93 %. (Outcome # 5) (DOK 3) Page 10 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

A. 3.06 g* B. 9.19 g C. 27.6 g 81. The combustion of butane produced 0.0243 kg of carbon dioxide. What mass of butane is required if the yield is 89 %. (Outcome # 5) (DOK 3) (Paired item 1) A. 36.1 g B. 9.01 g* C. 144.2 g 82. A reaction with an unknown theoretical yield was carried out and the amount of product obtained was a third of the theoretical yield. What is the percent yield? (Outcome # 5) (DOK 3) A. 33.3 %* B. 66.6 % C. cannot be determined 83. A reaction with an unknown percent yield was carried out and the amount of product obtained was a fourth of the theoretical yield. What is the percent yield? (Outcome # 5) (DOK 3) (Paired item 1) A. 75.0 % B. 25.0 %* C. cannot be determined 84. What is the density of a 0.354 M solution of ammonium phosphate? (Outcome # 7) (DOK 3) A. 0.0523 g/mL* B. 5.23 g/mL C. 52.3 g/mL 85. What is the mass of ammonium chloride is 500.0 mL of a 0.198 M solution? (Outcome # 7) (DOK 3) A. 10.6 g B. 5.30 g* C. 5.30 x 103 g 86. How many μL are in 0.239 mL of solvent? (Outcome # 7) (DOK 1) A. 2.39 x 105 μL B. 2.39 x 102 μL* C. 2.39 x 10-5 μL 87. How many grams are in an 81 mg aspirin sample? (Outcome # 7) (DOK 1) A. 0.081 g* B. 0.81 g C. 8.1 g 88. What is the product of hydrogen gas and oxygen gas? (Outcome # 8) (DOK 2) Page 11 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

A. H2O2 B. H2O* C. H3O+ 89. Classify the following type of reaction: Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g). (Outcome # 3) (DOK 1) A. redox reaction* B. combustion reaction C. acid/base reaction 90. Classify the following type of reaction: C3H8(l) + 5O2(g)  3CO2(g) + 4H2O(g). (Outcome # 3) (DOK 1) A. redox reaction B. combustion reaction* C. acid/base reaction 91. Classify the following type of reaction: NaCl(aq) + AgNO3(aq)  AgCl(s) + NaNO3(aq).

(Outcome # 3) (DOK 1) A. redox reaction B. acid/base reaction C. precipitation reaction* 92. Balance the following reaction: CaO + C  CaC2 + CO2. (Outcome # 3) (DOK 1) A. CaO2 + 3C  CaC2 + CO2 B. 2CaO2 + 6C  2CaC2 + 2CO2 C. 2CaO + 5C  2CaC2 + CO2* 93. Ammonia reacts with oxygen in the air. Write a balanced chemical reaction. (Outcome # 3) (DOK 2) A. 4NH3(g) + 5O2(g)  4NO(g) + 6H2O(l)* B. 2NH3(g) + 5O(g)  2NO(g) + 3H2O(l) C. 2NH3(g) + 3O2(g)  2H3NO3(aq) 94. What is the percent yield of a reaction if the product recovered is 89.4 g and the theoretical yield is 128.4 g? (Outcome # 4) (DOK 1) A. 144 % B. 69.6 %* C. 0.696 % 95. What is the percent yield of a reaction if the product recovered is 21.2 g and the theoretical yield is 28.4 g? (Outcome # 4) (DOK 1) (Paired item 1) A. 74.6 %* B. 134 % C. 0.746 % Page 12 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

96. What is the percent yield of a reaction if the actual yield is 80.6 % of the 42.4 g theoretical yield? (Outcome # 4) (DOK 2) A. 34.2 % B. 19.4 % C. 80.6 %* 97. What is the theoretical yield of a reaction if the percent yield 92.4 % and product recovered is 89.3 g? (Outcome # 4) (DOK 2) A. 89.3 g B. 96.6 g* C. 82.5 g 98. What is the limiting reactant in the combustion of 159 g of methane in an open atmosphere? (Outcome # 4) (DOK 1) A. methane* B. oxygen C. carbon dioxide 99. What is the excess reactant in the combustion of 211 g of methane in an open atmosphere?

(Outcome # 4) (DOK 1) A. water B. methane C. oxygen* 100. How many moles are in 1.25 g of calcium chloride? (Outcome # 4) (DOK 1) A. 8.88 x 101 moles B. 1.39 x 102 moles C. 1.13 x 10-2 moles* 101. How many moles are in 4.50 g of Na2SO4? (Outcome # 4) (DOK 1) A. 3.17 x 10-2 moles* B. 6.39 x 102 moles C. 3.16 x 101 moles 102. How many grams are in 12.5 moles of Ba(OH)2? (Outcome # 4) (DOK 1) A. 7.30 x 10-2 g B. 2.14 x 103 g* C. 2.14 x 104 g 103. How many grams are in 2.57 moles of iron oxide? (Outcome # 4) (DOK 2) A. 4.10 x 102 g* B. 6.21 x 101 g C. 1.61 x 10-2 g 104. What is the molar mass of laughing gas, N2O? (Outcome # 4) (DOK 1) A. 46.0 g/mol Page 13 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

105.

B. 30.0 g/mol C. 44.0 g/mol* What salt is formed between LiOH and HBr? (Outcome # 9) (DOK 1) A. LiBr* B. LiBr2 C. Li2Br

Page 14 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 05: Thermochemistry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 05: Thermochemistry 1. If ΔH = -54.74 kJ for a chemical reaction, that reaction _____________. (Outcome # 1,2) DOK 1 A. is exothermic* B. is endothermic C. cannot occur 2. A _____ is an experimental set-up that can be used to measure the heat of a chemical reaction or a physical change and determine the specific heat capacity of a substance.

(Outcome # 10) (DOK 1) A. manometer B. thermometer C. calorimeter* 3. The following can be used to measure the heat of combustion for an unknown sample?

(Outcome # 10) (DOK 2) A. bomb manometer B. bomb calorimeter* C. coffee-cup calorimeter 4. Coffee-cup calorimetry is carried out at _____. (Outcome # 10) (DOK 1) A. constant-volume B. constant-pressure* C. constant-mass 5. Bomb calorimetry is carried out at _____. (Outcome # 10) (DOK 1) A. constant-volume* B. constant-pressure C. constant-mass 6. You are asked to design an experiment to measure the enthalpy of a given reaction. The reaction needs to be at atmospheric pressure so which of the following techniques would be ideal for this experiment? (Outcome # 10) (DOK 3) A. bomb manometry B. bomb calorimetry C. coffee-cup calorimetry* 7. Your task is to measure the amount of energy evolved during the combustion of some hydrocarbon. Which of the following would be the ideal technique for this experiment?

(Outcome # 10) (DOK 3) Page 1 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 05: Thermochemistry

A. coffee-cup calorimetry B. bomb calorimetry* C. bomb manometry 8. 100 mL of a 0.300 M solution of AgNO3 reacts with 100 mL of a 0.300 M solution of HCl in a coffee-cup calorimeter and the temperature rises from 21.80 °C to 23.20 °C. Assuming the density and specific heat of the resulting solution is 1.00 g/mL and 4.18 J/g ∙ °C, respectfully, what is the ΔH°rxn? (Outcome # 11) (DOK 3) A. -39.0 kJ/mol* B. +39.0 kJ/mol C. +1.17 kJ/mol 9. Given the ∆H°f, calculate the ∆H°rxn for the formation of diamond from graphite. (Outcome # 11) (DOK 2) ∆H°f (C, graphite) = 0 kJ/mol ∆H°f (C, diamond) = 2 kJ/mol A. 0 kJ/mol B. +2 kJ/mol* C. -2 kJ/mol 10. Calculate the ∆H°rxn for the combustion of methane using the given ∆H°f. (Outcome # 11) (DOK 3) ∆H°f, methane(g) = -74.60 kJ/mol ∆H°f, water(l) = -285.8 kJ/mol ∆H°f, carbon dioxide(g) = -393.5 kJ/mol A. -1.04 x 10+3 kJ/mol B. -890.5 kJ/mol* C. 890.5 kJ/mol 11. A drop in water temperature is observed when 0.873 g of ammonium nitrate is added. The enthalpy change for this reaction is +0.280 kJ. Which of the statements is accurate?

(Outcome # 11) (DOK 3) A. The ∆H°soln for ammonium nitrate is +25.7 kJ/mol so this is an endothermic process where energy in the form of heat is absorbed from the surroundings.* B. The ∆H°soln for ammonium nitrate is -25.7 kJ/mol so this is an exothermic process where energy in the form of heat is released into the surroundings.

C. The ∆H°soln for ammonium nitrate is +25.7 kJ/mol so this is an endothermic process where energy in the form of heat is released into the surroundings.

Page 2 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 05: Thermochemistry

12. An increase in water temperature is observed when 1.97 g of NaOH is added. The enthalpy change for this reaction is -2.19 kJ. Which of the statements is accurate? (Outcome # 11) (DOK 3) (Paired item 1) A. The ∆H°soln for NaOH is +44.5 kJ/mol so this is an endothermic process where energy in the form of heat is absorbed from the surroundings.

B. The ∆H°soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is released into the surroundings.* C. The ∆H°soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is absorbed from the surroundings.

13. If ∆H = -73.54 kJ for a chemical reaction, that reaction _____________. (Outcome # 1,5,9) (DOK 2) A. is exothermic* B. is endothermic C. cannot occur 14. A chemical reaction that gives off energy in the form of heat is considered _____. (Outcome # 5) (DOK 2) A. exothermic* B. endothermic C. exergonic 15. A chemical reaction that absorbs energy in the form of heat is considered _____. (Outcome # 5) (DOK 2) (Paired item 1) A. exothermic B. endothermic* C. exergonic 16. A reaction requires a sample to be heated using a water bath near boiling temperature.

Which statement below would be accurate? (Outcome # 5) (DOK 3) A. Boiling water is an endothermic process and to break apart the intermolecular forces that hold together the water molecules requires -40.7 kJ of energy.

B. Boiling water is an exothermic process and to break apart the intermolecular forces that hold together the water molecules requires +40.7 kJ of energy.

C. Boiling water is an endothermic process and to break apart the intermolecular forces that hold together the water molecules requires +40.7 kJ of energy.* 17. A reaction where the products are lower in energy than the reactants is an example of an _____. (Outcome # 6) (DOK 1) A. endothermic process B. exothermic process* C. endergonic process Page 3 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 05: Thermochemistry

18. A reaction where the products are higher in energy than the reactants is an example of an _____. (Outcome # 6) (DOK 1) A. endothermic process* B. exothermic process C. exergonic process 19. An _____ reaction results when the energy required to break bonds in the reactants is greater than the energy released by the formation of products. (Outcome # 3) (DOK 1) A. exergonic B. endothermic* C. exothermic 20. An _____ reaction results when the energy released by the formation of products is greater than the energy required to break the bonds in the reactants. (Outcome # 3) (DOK 1) A. exergonic B. endothermic C. exothermic*

Page 4 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 06: Electronic Structure and Periodic Properties of Elements 1. Provide the element name with a ground-state electron configuration of 1s 22s2p4 (Outcome # 1,5) DOK 1 A. Potassium B. carbon C. oxygen* 2. What is the ground-state electron configuration of calcium? (Outcome # 1,5) DOK 1 A. 1s22s22p63s23p64s2* B. 1s22s22p6 C. 1s22s22p63s2 3. Due to periodicity, which element would you expect to behave most like sodium?

(Outcome # 1,2) DOK 2 A. calcium B. aluminum C. potassium* 4. Which of the following has the longest wavelength? (Outcome # 1,2) DOK 1 A. x rays B. microwaves* C. UV light 5. Elements in group 17 are considered _____________. (Outcome # 1,2) DOK 1 A. alkali Metals B. halogens* C. noble Gases 6. Due to periodicity, which of the following elements has chemical behavior similar to that of Oxygen? (Outcome # 1,2,8) DOK 1 A. bromine B. sulfur* C. carbon 7. Which of the following sets of elements are the most similar to each other? (Outcome # 2) (DOK 1) A. F, Cl, Br, I* B. C, N, O, F C. H, He Page 1 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements

8. According to periodic trends, arrange the following ions, potassium, magnesium, and aluminum in order of increasing ionic size. (Outcome # 2) (DOK 2) A. potassium ion, magnesium ion, and aluminum ion B. aluminum ion, magnesium ion, and potassium ion* C. aluminum ion, potassium ion, and magnesium ion 9. During a UV-Visible spectroscopy experiment, a student notes a wavelength peak measurement at 280 nm. What region of the electromagnetic spectrum was this peak observed? (Outcome # 7) (DOK 1) A. visible region B. ultra-violet region* C. both ultra-violet and visible region 10. During a UV-Visible spectroscopy experiment, a student notes 2 wavelength peak measurements at 580nm and 685nm. What region of the electromagnetic spectrum were these peaks observed? (Outcome # 7) (DOK 1) (Paired item 1) A. visible region* B. ultra-violet region C. both ultra-violet and visible region 11. Provide the element name with a ground-state electron configuration of 1s 22s2p4 (Outcome # 1,7,9) (DOK 1) A. potassium B. carbon C. oxygen* 12. What is the ground-state electron configuration of Calcium? (Outcome # 1,7,9) (DOK 1) A. 1s22s22p63s23p64s2* B. 1s22s22p6 C. 1s22s22p63s2 13. As you move down a group of elements (family), the number of valence electrons (Outcome # 1,9) (DOK 1) A. increases.* B. stays the same.

C. increases and then decreases.

14. Due to periodicity, which element would you expect to behave most like sodium?

(Outcome # 1,9) (DOK 2) A. calcium B. aluminum C. potassium* 15. Which of the following has the longest wavelength? (Outcome # 1,9) (DOK 1) A. x rays Page 2 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements

B. microwaves* C. UV light 16. What is the maximum number of electrons that can occupy the 4th energy level or shell?

(Outcome # 9) (DOK 2) A. 4 B. 16 C. 32* 17. How many subshells are found in the 2nd energy level or shell? (Outcome # 9) (DOK 2) A. 2* B. 4 C. 8 18. What is the maximum number of orbitals found in the 3rd energy level or shell?

(Outcome # 9) (DOK 2) A. 3 B. 9* C. 18 19. Based on the following electron configuration, [Kr]5s24d105p5, this element would most likely _____. (Outcome # 9) (DOK 3) A. gain an electron to form a -1 anion and could form an ionic bond with a metal* B. loss an electron to form a -1 anion and could form an ionic bond with a metal C. gain an electron to form a -1 anion and could form an ionic bond with a nonmetal 20. Based on the following electron configuration, [Xe]6s 2, this element would most likely _____. (Outcome # 9) (DOK 3) (Paired item 1) A. loss 2 electrons to form a +2 cation and could form an ionic bond with a metal B. loss 2 electrons to form a +2 cation and could form an ionic bond with a nonmetal* C. gain 2 electrons to form a +2 cation and could form an ionic bond with a nonmetal 21. Identify the transition metal ion and the number of electrons with the following electron configuration, [Ar]4s03d7. (Outcome # 9) (DOK 3) A. cobalt (I) ion and 25 electrons B. cobalt (II) ion and 25 electrons* C. cobalt (III) ion and 25 electrons 22. UV-Visible spectroscopy can be used to study chromophores such as C=C-C=C which absorb in the UV region of the electromagnetic spectrum ranging from _____. (Outcome # 2) (DOK 2) A. 100 - 300 nm* Page 3 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements

B. 400 - 600 nm C. 600 - 800 nm 23. What is the electron configuration of a copper atom? (Outcome # 7) (DOK 2) A. [Ar]4s23d9 B. [Ar]4s13d10* C. [Ar]4s03d11 24. What is the electron configuration of a copper (II) ion? (Outcome # 7) (DOK 2) A. [Ar]4s23d7 B. [Ar]4s13d8 C. [Ar]3d9* 25. What is the ground-state electron configuration of carbon? (Outcome # 7) (DOK 1) A. 1s22s12p3 B. 1s22s22p2* C. 1s22s32p1 26. In which orbital does an electron add to in chlorine to form an octet? (Outcome # 7) (DOK 2) A. 3s B. 3p* C. 3d 27. What is the ms value for an electron added to bromine to form an octet? (Outcome # 7) (DOK 3) A. +1/2 B. -1/2* C. 0 28. In what block, group, and period on the periodic table can the atom with a 1s22s22p63s23p64s23d104p5 ground-state electron configuration be found? (Outcome # 7) (DOK 3) A. p-block, group 7A, and period 3 B. p-block, group 7A, and period 4* C. p-block, group 7A, and period 5 29. In what block, group, and period on the periodic table can the atom with a 1s 22s22p63s1 ground-state electron configuration be found? (Outcome # 7) (DOK 3) (Paired item 1) A. s-block, group 1A, and period 2 B. s-block, group 1A, and period 3* C. s-block, group 1A, and period 4 30. How many electrons are in the most likely ion formed from an atom located in group 6A and period 3? (Outcome # 7) (DOK 3) A. 16 electrons Page 4 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements

B. 17 electrons C. 18 electrons* 31. How many electrons are in the most likely ion formed from an atom located in group 2A and period 5? (Outcome # 7) (DOK 3) (Paired item 1) A. 36 electrons* B. 38 electrons C. 37 electrons 32. Which of the following sources of radiation is higher in energy? (Outcome # 3) (DOK 1) A. visible light B. ultra violet light* C. infrared light 33. Which of the following sources of radiation has a longer wavelength? (Outcome # 3) (DOK 1) A. visible light B. infrared light* C. ultra violet light 34. 23.1 L of an unknown gas has a mass of 28.85 g at STP. What is the identity of the unknown gas? (Outcome # 4) (DOK 3) (Paired item 1) A. SO2 B. CO* C. NO 35. According to periodic trends, which metal has the lowest ionization energy? (Outcome # 2) (DOK 2) A. Li B. Cs* C. Rb 36. According to periodic trends, which metal has the highest ionization energy? (Outcome # 2) (DOK 2) (Paired item 1) A. Li* B. Cs C. Rb 37. Which nonradioactive group I metal would be the most reactive in water and why?

(Outcome # 2) (DOK 3) A. Cesium would be the most reactive group I metal in water because it has only one valence electron.

B. Cesium would be the most reactive group I metal in water because it’s one valence electron is the closest to the nucleus compared to the other metals.

Page 5 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements

C. Cesium would be the most reactive group I metal in water because it’s one valence electron is the farthest from the nucleus compared to the other metals.* 38. Which of the following elements have a tendency to gain electrons? (Outcome # 9) (DOK 1) A. Cl, O, F* B. N, O, Al C. Cl, F, Ga

Page 6 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 07: Chemical Bonding and Molecular Geometry 1. According to the octet rule, a magnesium atom has a tendency to (Outcome # 1,2,9) DOK 1 A. lose one electron.

B. lose two electrons.* C. gain one electron.

2. A molecule that has a single covalent bond is _____. (Outcome # 1,2,9) DOK 1 A. CO2 B. CO C. Cl2* 3. A diatomic molecule with a triple covalent bond is _____. (Outcome # 1,2,9) DOK 1 A. O2 B. F2 C. N2 * 4. Which of the following diatomic molecules is joined by a double covalent bond? (Outcome # 1,2,9) DOK 1 A. Cl2 B. O2 * C. N2 5. Which of the following pairs of elements can be joined by a covalent bond? (Outcome # 1,2,9) DOK 1 A. N and C* B. Na and C C. Mg and C 6. Which one of the following elements does not exist as a diatomic molecule in nature?

(Outcome # 1,2,9) DOK 1 A. hydrogen B. nitrogen C. neon* 7. Which of the following is an ionic compound? (Outcome # 1,2) DOK 1 A. CO B. HCl C. Na2O* 8. Which one of these compounds is an ionic compound? (Outcome # 1,2) DOK 1 A. Na2O* Page 1 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

B. CO2 C. N2 9. According to VSEPR theory, the shape of an ammonium ion, NH4+, is most similar to __________. (Outcome # 1,2) DOK 2 A. CH4* B. BH3 C. N2 10. According to periodic trends, which element is the most electronegative? (Outcome # 2) (DOK 1) A. Ne B. O C. F* 11. What is the electron group (EG) and molecular geometry (MG) of an ammonium ion?

(Outcome # 2) (DOK 2) A. (EG) tetrahedral and (MG) tetrahedral* B. (EG) tetrahedral and (MG) trigonal pyramidal C. (EG) tetrahedral and (MG) bent 12. What is the electron group (EG) and molecular geometry (MG) of an ammonia molecule?

(Outcome # 2) (DOK 2) (Paired item 1) A. (EG) tetrahedral and (MG) tetrahedral B. (EG) tetrahedral and (MG) trigonal pyramidal* C. (EG) tetrahedral and (MG) bent 13. According to the octet rule, which of elements will have a tendency to loss 2 electrons?

(Outcome # 9) (DOK 1) A. strontium* B. oxygen C. cesium 14. Which of the following molecules has the greatest bond energy? (Outcome # 9) (DOK 2) A. H2 B. N2* C. O2 15. What type of bond will typically form between boron and hydrogen based on their electronegativity? (Outcome # 9) (DOK 2) A. metallic B. ionic C. covalent* 16. Based off periodic trends, which of the following has the strongest lattice energy? (Outcome # 9) (DOK 3) Page 2 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

A. aluminum chloride* B. calcium chloride C. sodium chloride 17. Construct the molecule IF5 using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles of the equatorial fluorine’s in the structure?

(Outcome # 12) (DOK 3) A. 90°* B. 120° C. 109.5° 18. Construct the molecule IF5 and PF5 using a molecular modeling software such as Spartan or 3D-ChemDraw. How do the molecular shapes differ? (Outcome # 12) (DOK 3) A. In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on phosphorus. As a result, the molecular shape of IF5 is square pyramidal and PF5 is trigonal bipyramidal.* B. In PF5 there is a lone pair of electrons on phosphorus where as in IF5 there are no lone pairs on iodine. As a result, the molecular shape of PF5 is square pyramidal and IF5 is trigonal bipyramidal.

C. In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on phosphorus. As a result, the molecular shape of IF5 is octahedral and PF5 is trigonal bipyramidal.

19. Construct the molecule PF5 using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles of the equatorial fluorine’s in the structure?

(Outcome # 12) (DOK 3) A. 90° B. 120°* C. 109.5° 20. Construct the molecule PF5 using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles of the axial fluorine’s in the structure? (Outcome # 12) (DOK 3) A. 90°* B. 120° C. 109.5° 21. Using VSEPR theory, predict the molecule shape of a molecule that contains 2 electron groups. (Outcome # 12) (DOK 1) A. trigonal planar B. linear* C. bent Page 3 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

22. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond angles in a molecule that contains 4 electron groups (3 bonds and 1 lone pair electrons).

(Outcome # 12) (DOK 2) A. tetrahedral, trigonal pyramidal, >109.5° B. tetrahedral, trigonal pyramidal, <109.5°* C. tetrahedral, trigonal pyramidal, 109.5° 23. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond angles in a molecule that contains 5 electron groups (2 bonds and 3 lone pair electrons).

(Outcome # 12) (DOK 2) (Paired item 1) A. trigonal bipyramidal, linear, 180°* B. trigonal bipyramidal, trigonal bipyramidal, 90° and 120° C. trigonal bipyramidal, trigonal bipyramidal, 180° 24. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond angles in a molecule that contains 6 electron groups (5 bonds and 1 lone pair electrons).

(Outcome # 12) (DOK 2) (Paired item 2) A. octahedral, octahedral, 90° B. octahedral, square planar, 90° C. octahedral, square pyramidal, 90°* 25. Using VSEPR theory, predict the molecular shape and bond angles in BCl3. (Outcome # 12) (DOK 2) A. trigonal planer, 120°* B. trigonal pyramidal, 120° C. trigonal bent, 120° 26. Construct the molecule H2O using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles in the structure? (Outcome # 12) (DOK 2) A. 104.5°* B. 107° C. 109.5° 27. Construct the molecule NH3 using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles in the structure? (Outcome # 12) (DOK 2) A. 104.5° B. 107°* C. 109.5° 28. Construct the molecule CH4 using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles in the structure? (Outcome # 12) (DOK 2) A. 104.5° B. 107° C. 109.5°* Page 4 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

29. The bond angles in CH4, NH3, and H2O are 109.5°, 107°, and 104.5°, respectfully. Which of the statements best describes the variance in bond angles? (Outcome # 12) (DOK 3) A. CH4 has no lone pairs of electrons on the central atom so the optimal molecular shape would be tetrahedral with bond angles of 109.5°. In NH3 and H2O there are 1 and 2 lone pairs, respectfully, so more repulsion exists between the bonds and lone pairs, as a result, the bond angles are less than 109.5°.* B. NH3 and H2O have a trigonal pyramidal and bent molecular shape, respectfully, which is the reason why the bond angles are less than 109.5°.

C. CH4 only has nonpolar bonds while NH3 and H2O have polar bonds which results in the difference in bond angels.

30. Based off the following data, what is the lattice energy of sodium chloride? (Outcome # 11) (DOK 2) ΔHsub of Na = 108 kJ/mol Do of Cl2 = 243 kJ/mol IE of Na(g) = 496 kJ/mol EA of Cl(g) = -349 kJ/mol ΔHf of NaCl = -411 kJ/mol A. -1490 kJ/mol B. -909 kJ/mol C. -788 kJ/mol* 31. In an ionic bond, the charge on the cation (i.e. the metal) is (Outcome # 1,7,9) (DOK 1) A. always positive.* B. always negative.

C. either positive or negative.

32. According to the octet rule, a magnesium atom has a tendency to (Outcome # 1,9) (Dok 2) A. lose one electron.

B. lose two electrons.* C. gain one electron.

33. A covalent bond is formed when two atoms (Outcome # 1,9) (DOK 2) A. share an electron with each other.

B. share one or more pairs of electrons with each other.* C. gain electrons.

34. According to the octet rule, a bromine atom has a tendency to (Outcome # 1,9) (DOK 2) A. lose one electron.

B. lose two electrons.

C. gain one electron.* 35. The halogens have how many valence electrons? (Outcome # 1,9) (DOK 1) Page 5 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

A. 4 B. 6 C. 7* 36. How many electrons are shared in a single covalent bond? (Outcome # 1,9) (DOK 1) A. 2* B. 3 C. 1 37. How many electrons are shared in a double covalent bond? (Outcome # 1,9) (DOK 1) A. 3 B. 4* C. 2 38. A molecule that has a single covalent bond is _____. (Outcome # 1,9) (DOK 1) A. CO2 B. CO C. Cl2* 39. A diatomic molecule with a triple covalent bond is _____. (Outcome # 1,9) (DOK 2) A. O2 B. F2 C. N2 * 40. Which of the following diatomic molecules is joined by a double covalent bond? (Outcome # 1,9) (DOK 2) A. Cl2 B. O2 * C. N2 41. Which of the following pairs of elements can be joined by a covalent bond? (Outcome # 1,9) (DOK 2) A. N and C* B. Na and C C. Mg and C 42. _____ is a diatomic molecule that has a double covalent bond. (Outcome # 9) (DOK 2) A. Br2 B. I2 C. O2* 43. Which element contains triple covalent bonds? (Outcome # 9) (DOK 1) A. oxygen B. nitrogen* C. iodine 44. What is the molecular shape of CO2? (Outcome # 9) (DOK 1) Page 6 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

A. linear* B. bent C. trigonal planar 45. How many polar bonds does CH4 contain? (Outcome # 9) (DOK 1) A. 0* B. 2 C. 4 46. Which molecule has only covalent bonds? (Outcome # 9) (DOK 1) A. CO2* B. Al2O3 C. Mg3N2 47. Which compound has only ionic bonds? (Outcome # 9) (DOK 1) (Paired item 1) A. CO2 B. Al2O3* C. H2O2 48. The octet rule states that main group elements in the periodic table react to achieve a filled valence shell which consists of how many electrons? (Outcome # 9) (DOK 1) A. 2 B. 4 C. 8* 49. What is the molecular shape and polarity for xenon tetrafluoride? (Outcome # 9) (DOK 3) A. square-planar and polar B. square-planar and non-polar* C. tetrahedral and non-polar 50. Which of the following elements are found in the p-block and can form an octet? (Outcome # 7) (DOK 1) A. He, P, S, As B. P, S, O, C* C. He, Ar, Kr, Ne 51. Based off molecular polarity determined by VSEPR theory, which of the following would be soluble in methanol? (Outcome # 8) (DOK 3) A. heptane B. ethanol* C. pentane 52. Based off molecular polarity determined by VSEPR theory, which of the following would be insoluble in CCl4? (Outcome # 8) (DOK 3) A. methanol* B. octane Page 7 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

C. hexane 53. Based off molecular polarity determined by VSEPR theory, in which solvent would NaCl be the most soluble? (Outcome # 8) (DOK 3) A. CH3OH B. CH3CH2OH C. H2O* 54. Based off molecular polarity determined by VSEPR theory, in which solvent would glucose be the least soluble? (Outcome # 8) (DOK 3) A. CH3CH2OCH2CH3* B. CH3OH C. H2O 55. Which statement best describes a bond forming between fluorine and iodine? (Outcome # 8) (DOK 3) A. fluorine and iodine are in the same group so the electron density in the bond is equaling shared giving rise to a non-polar bond B. fluorine is more electronegative than iodine so it will attract the electron density in the bond giving rise to a polar bond* C. fluorine is less electronegative than iodine so it will attract the electron density in the bond giving rise to a polar bond 56. Why are detergents and soaps good at cleaning up oily stains from dishes or clothing?

(Outcome # 8) (DOK 3) 1. Detergents and soaps work well to clean up oily messes because they are amphiphilic in nature so they contain both hydrophilic (polar) and hydrophobic (nonpolar) ends. The hydrophobic end attaches to oils via hydrogen bonds creating micelles which leave the hydrophilic part exposed and can be washed away by water.

2. Detergents and soaps work well to clean up oily messes because they are amphiphilic in nature so they contain both hydrophilic (non-polar) and hydrophobic (polar) ends. The hydrophobic end attaches to oils via London forces creating micelles which leave the hydrophilic part exposed and can be washed away by water.

3. Detergents and soaps work well to clean up oily messes because they are amphiphilic in nature so they contain both hydrophilic (polar) and hydrophobic (nonpolar) ends. The hydrophobic end attaches to oils via London forces creating micelles which leave the hydrophilic part exposed and can be washed away by water.* 57. Is it true that a molecule with polar bonds will always be polar? (Outcome # 8) (DOK 2) A. that is false, molecular polarity is determined by molecular shape* B. that is true, molecular polarity is determined by bond polarity only Page 8 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

C. that is false, molecular polarity is determined by electron group geometry 58. An _____ reaction results when the energy required to break bonds in the reactants is greater than the energy released by the formation of products. (Outcome # 3) (DOK 1) A. exergonic B. endothermic* C. exothermic 59. An _____ reaction results when the energy released by the formation of products is greater than the energy required to break the bonds in the reactants. (Outcome # 3) (DOK 1) A. exergonic B. endothermic C. exothermic* 60. How many non-polar bonds does CH3OH contain? (Outcome # 9) (DOK 1) A. 2 B. 3* C. 4 61. How many polar bonds does CCl4 have in its structure? (Outcome # 9) (DOK 1) A. 0 B. 2 C. 4*

Page 9 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 08: Advanced Theories of Covalent Bonding Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 08: Advanced Theories of Covalent Bonding 1. Based on valence bond theory, which statement best describes the electron geometry, bonding and hybridization of the central atom in carbon tetrachloride? (Outcome # 12) (DOK 3) A. The electron geometry of carbon in carbon tetrachloride is tetrahedral with a sp 3 hybridization. The C-Cl bond is of σ-character.* B. The electron geometry of carbon in carbon tetrachloride is tetrahedral with a sp 2 hybridization. The C-Cl bond is of σ-character.

C. The electron geometry of carbon in carbon tetrachloride is tetrahedral with a sp 3 hybridization. The C-Cl bond is of π-character.

2. Based on valence bond theory, which statement best describes the electron geometry and hybridization of the central atom(s) in acetylene? (Outcome # 12) (DOK 2) A. The electron geometry of the 2 carbons in acetylene is tetrahedral with a sp 3 hybridization.

B. The electron geometry of the 2 carbons in acetylene is trigonal planar with a sp 2 hybridization.

C. The electron geometry of the 2 carbons in acetylene is linear with a sp hybridization.* 3. Which statement best describe the structure of a carbonate anion? (Outcome # 12) (DOK 3) A. The electron geometry of carbon in a carbonate anion is trigonal planar with a sp 2 hybridization and bond angles are 120°. There is a π-bond formed between a nonhybridized “C” p-orbital overlapping with an “O” p-orbital.* B. The electron geometry of carbon in a carbonate anion is trigonal planar with a sp 2 hybridization and bond angles are <120°. There is a π-bond formed between a nonhybridized “C” p-orbital overlapping with an “O” p-orbital.* C. The electron geometry of carbon in a carbonate anion is trigonal planar with a sp 2 hybridization and bond angles are <120°. There is a π-bond formed between a hybridized “C” p-orbital overlapping with an “O” p-orbital.* 4. Based on valence bond theory, what is the hybridization of the central atom(s) in C 2F4?

(Outcome # 12) (DOK 1) A. both carbons are sp2* B. both carbons are sp3 C. one carbon is sp3 and the other carbon is sp2 5. Which element contains triple covalent bonds? (Outcome # 9) (DOK 1) Page 1 of 2

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OpenStax Chemistry Supplemental Test Items Chapter 08: Advanced Theories of Covalent Bonding

A. oxygen B. nitrogen* C. iodine

Page 2 of 2

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OpenStax Chemistry Supplemental Test Items Chapter 09: Gases Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 09: Gases 1. On a very cold day, you notice that your tires look a bit deflated than warmer days. This observation can be explained by _____. (Outcome # 8) (DOK 2) A. Boyles law B. Ideal gas law C. Charles law* 2. What is the relationship between pressure and volume of a gas at constant temperature?

(Outcome # 8) (DOK 2) A. as volume decreases, pressure increases* B. as volume decreases, pressure decreases C. as volume increases, pressure increases 3. How many mm Hg are in 0.890 atm of pressure? (Outcome # 8) (DOK 1) A. 854 mm Hg B. 676 mm Hg* C. 1.17 x 10-3 mm Hg 4. How many atmospheres are in 710 mm Hg? (Outcome # 8) (DOK 1) A. 0.934 atm* B. 1.07 atm C. 5.40 x 105 atm 5. The average tire pressure for an automobile is 38.5 psi which is how many atmospheres of pressure? (Outcome # 8) (DOK 1) A. 1.77 x 10-3 atm B. 566 atm C. 2.62 atm* 6. What is the volume for 1.00 mole of gas at STP? (Outcome # 3) (DOK 2) A. 24.5 L B. 22.4 L* C. 2.05 L 7. What is the standard pressure for 1.00 mole of gas at STP? (Outcome # 3) (DOK 2) A. 760 mm Hg* B. 1.03 atm C. 103 kPa 8. 286 L of hydrogen gas at STP reacts with excess chorine gas. What is the maximum amount of gas product that can be formed at STP? (Outcome # 3) (DOK 3) Page 1 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 09: Gases

A. 572 L* B. 143 L C. 286 L 9. 159 L of hydrogen gas at STP reacts with excess chorine gas. What is the maximum amount of gas product that can be formed at STP? (Outcome # 3) (DOK 3) (Paired item 1) A. 159 L B. 79.5 L C. 318 L* 10. A _____ is an instrument used to measure atmospheric pressure specifically in the area of meteorology. (Outcome # 10) (DOK 1) A. barometer* B. manometer C. altimeter 11. A _____ is a general instrument that utilizes a liquid column, typically mercury, to measure pressure. (Outcome # 10) (DOK 1) A. barometer B. manometer* C. altimeter 12. How many psi are in 760. mm Hg? (Outcome # 7) (DOK 1) A. 1.47 x 101 psi* B. 3.93 x 104 psi C. 2.54 x 10-5 psi 13. A sample of nitrogen gas occupies 9.20 L at 21 °C and 0.959 atm. If the pressure is increased to 1.15 atm at constant temperature, what is the newly occupied volume? (Outcome # 6) (DOK 1) A. 11.0 L B. 7.67 L* C. 9.20 L 14. The pressure of a gas in a container is 1.85 atm and occupies a volume of 12.5 L. If the original volume is reduced by half at constant temperature, what would happen to the pressure? (Outcome # 6) (DOK 2) A. the pressure would double* B. the pressure would reduce by half C. the pressure would remain the same 15. The pressure of a gas in a container is 1.23 atm and occupies a volume of 1.5 L. If the original volume is doubled at constant temperature, what would happen to the pressure?

(Outcome # 6) (DOK 2) A. the pressure would remain the same Page 2 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 09: Gases

B. the pressure would double C. the pressure would reduce by half* 16. Suppose your car is equipped with tire pressure monitoring system (TPMS) and the tire pressure is 34.0 psi on a 98 °F day in California. You decided to take a road trip to Alaska where the temperature drops to 20 °F. As you arrived in Alaska, you noticed that the tire pressure monitoring system alert light is illuminated. Why did this happen? (Outcome # 6) (DOK 3) A. as temperature decreases, gas molecules lose kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated* B. as temperature decreases, gas molecules gain kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated C. as temperature decreases, gas molecules lose kinetic energy and the volume of gas increases thus reducing the overall pressure in the tire which results in the TPMS to become activated 17. On a hot summer day, you notice that a bag of chips left in your vehicle has inflated. Why did this happen? (Outcome # 6) (DOK 3) A. as temperature increases, gas molecules gain kinetic energy and the volume of gas decreases inside the bag of chips B. as temperature increases, gas molecules lose kinetic energy and the volume of gas increases inside the bag of chips C. as temperature increases, gas molecules gain kinetic energy and the volume of gas increases inside the bag of chips* 18. What mass of nitrogen is needed to fill an 855 L tank at STP? (Outcome # 6) (DOK 3) A. 0.978 kg B. 1.07 kg* C. 0.533 kg 19. What mass of oxygen is needed to fill a 585 L tank at STP? (Outcome # 6) (DOK 3) (Paired item 1) A. 0.835 kg* B. 0.765 kg C. 0.417 kg 20. What is the pressure in a 5.80 L container that has 0.545 moles of oxygen gas at 22.0 °C? (Outcome # 6) (DOK 1) A. 0.170 atm B. 2.28 atm* C. 231 atm Page 3 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 09: Gases

21. What is the pressure in a 3.41 L container that has 0.741 moles of oxygen gas at 26.0 °C? (Outcome # 6) (DOK 1) (Paired item 1) A. 5.34 atm* B. 0.464 atm C. 62.0 atm 22. How many moles of CO2 gas are present in a 9.1 L container at 25 °C and 1.35 atm?

(Outcome # 6) (DOK 1) A. 4.96 x 10-3 moles B. 5.99 moles C. 0.502 moles* 23. Oxygen gas (PO2 = 1.10 atm), nitrogen gas (PN2 = 0.840 atm), and carbon dioxide gas (PCO2 = 0.125 atm) occupy the same container. What is the total pressure in the container?

(Outcome # 6) (DOK 1) A. 2.07 atm* B. 1.94 atm C. 0.135 atm 24. A container filled with neon and argon gas is 25.00% by volume neon. What is the partial pressure of argon if the total pressure inside the container is 5.500 atm? (Outcome # 6) (DOK 2) A. 412.5 atm B. 1.375 atm C. 4.125 atm* 25. A container filled with helium and argon gas is 8.00% by volume argon. What is the partial pressure of argon if the total pressure inside the container is 4.100 atm? (Outcome # 6) (DOK 2) (Paired item 1) A. 0.328 atm* B. 3.77 atm C. 32.8 atm 26. What is the temperature for STP conditions? (Outcome # 4) (DOK 1) A. 273.15 K* B. 298.15 K C. 0 K 27. What is the pressure for STP conditions? (Outcome # 4) (DOK 1) A. 740 mm Hg B. 780 mm Hg C. 760 mm Hg* 28. 28.5 L of an unknown gas has a mass of 55.92 g at STP. What is the identity of the unknown gas? (Outcome # 4) (DOK 3) Page 4 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 09: Gases

A. CO2* B. O2 C. N2

Page 5 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 10: Liquids and Solids Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 10: Liquids and Solids 1. Which statement accurately depicts what happens to water on the molecular level in a tea pot when it begins to boil? (Outcome # 9) (DOK 3) A. The molecules begin to move farther apart decreasing their intermolecular forces and they escape the liquid state to enter the gas state.* B. The molecules begin to move closer together overcoming their intermolecular forces which holds them together and they escape the liquid state to enter the gas state.

C. The molecules begin to move farther apart decreasing their intramolecular forces and they escape the liquid state to enter the gas state.

2. At what temperature does water boil in kelvin? (Outcome # 7) (DOK 1) A. 373.15 K* B. 273.15 K C. 173.15 K 3. Which phases change is an exothermic process? (Outcome # 8) (DOK 1) A. freezing* B. melting C. evaporation 4. Which phases change is an endothermic process? (Outcome # 8) (DOK 1) A. freezing B. evaporation* C. deposition 5. Water changing from ice to a liquid is an example of _____. (Outcome # 8) (DOK 1) A. melting* B. evaporation C. freezing 6. Sodium chloride changing from a solid to a gas is an example of _____. (Outcome # 8) (DOK 1) A. evaporation B. sublimation* C. boiling 7. What predominate intermolecular force is in HCl? (Outcome # 8) (DOK 1) A. dipole-dipole* B. hydrogen bonding C. London forces Page 1 of 3

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OpenStax Chemistry Supplemental Test Items Chapter 10: Liquids and Solids

8. What predominate intermolecular force is in NH3? (Outcome # 8) (DOK 1) (Paired item 1) A. dipole-dipole B. hydrogen bonding* C. London forces 9. What predominate intermolecular force is in CO2? (Outcome # 8) (DOK 1) (Paired item 2) A. dipole-dipole B. hydrogen bonding C. London forces* 10. What predominate intermolecular force is in CH3OH? (Outcome # 8) (DOK 1) (Paired item 3) A. dipole-dipole B. hydrogen bonding* C. London forces 11. What predominate intermolecular force is in CH3CH2CH3? (Outcome # 8) (DOK 1) (Paired item 4) A. dipole-dipole B. hydrogen bonding C. London forces* 12. Based off of the principles of intermolecular forces, which liquid has a higher vapor pressure? (Outcome # 8) (DOK 2) A. water B. methanol C. ethyl ether* 13. Based off of the principles of intermolecular forces, which liquid has the lowest vapor pressure? (Outcome # 8) (DOK 2) (Paired item 1) A. water* B. ethanol C. ethyl ether 14. If it takes you 10 min. to boil an egg to perfection at sea level, how long would it take to boil an egg to your taste in the Carpathian Mountains at elevations of 8,500 ft? (Outcome # 8) (DOK 3) A. The boiling point of water in the Carpathian Mountains is less than 100 °C because of lower atmospheric pressure which results in reduced intermolecular forces, so it would take a longer time to boil the egg.* B. The boiling point of water in the Carpathian Mountains is greater than 100 °C because of lower atmospheric pressure which results in increased intermolecular forces, so it would take less time to boil the egg.

C. The boiling point of water is always 100 °C regardless of elevation so it would take the same amount of time to boil the egg.

Page 2 of 3

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OpenStax Chemistry Supplemental Test Items Chapter 10: Liquids and Solids

15. Which alkane would have a higher boiling point? (Outcome # 8) (DOK 1) A. heptane* B. ethane C. pentane 16. Which alkane would have a lower boiling point? (Outcome # 8) (DOK 1) A. CH3CH3 B. CH4* C. CH3CH2CH3 17. Which of the following halogens would have stronger intermolecular forces? (Outcome # 8) (DOK 1) A. Br2 B. Cl2 C. I2* 18. Which of the following molecules would have weaker intermolecular forces? (Outcome # 8) (DOK 1) A. I2* B. NH3 C. H2O

Page 3 of 3

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OpenStax Chemistry Supplemental Test Items Chapter 11: Solutions and Colloids Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 11: Solutions and Colloids 1. Based off the molecular polarity of water, which of the following molecules would be soluble in water? (Outcome # 4) (DOK 2) A. glucose, methanol, and ethanol* B. carbon dioxide, methane, methanol C. glucose, carbon dioxide, ethanol 2. Which of the following would be a strong electrolyte in solution? (Outcome # 6) (DOK 2) A. PbI2 B. KCl* C. Al(OH)3 3. Which of the following would be a weak electrolyte in solution? (Outcome # 6) (DOK 2) A. acetic acid* B. sulfuric acid C. hydroiodic acid 4. Which of the following when dissolved in deionized water would make a poor conducting solution? (Outcome # 6) (DOK 2) A. baking soda B. sugar* C. salt 5. Which of the following when dissolved in deionized water would make a good conducting solution? (Outcome # 6) (DOK 2) (Paired item 1) A. methanol B. sugar C. baking soda* 6. For an experiment, you are asked to prepare a 2 m strong electrolytic solution. Which of the following salts would you use? (Outcome # 6) (DOK 3) A. an alkali salt* B. an alkaline salt C. either an alkali or an alkaline salt 7. Which of the following substances would be a poor choice for making conductive solutions?

(Outcome # 6) (DOK 3) A. C6H12O6, CH3OH, CH3CH2OH* B. HCl, KBr, HNO3 C. NaOH, KOH, LiOH Page 1 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 11: Solutions and Colloids

8. Which of the following would be soluble in water? (Outcome # 9) (DOK 2) A. sugar, NaCl, HCl* B. sugar, NaOH, ethane C. sugar, HNO3, methane 9. How would you purify salt water so that it becomes potable? (Outcome # 2) (DOK 1) A. gravity filtration B. vacuum filtration C. distillation* 10. Which of the following would conduct electricity? (Outcome # 2) (DOK 3) A. solid NaCl B. NaCl solution* C. both solid NaCl and a NaCl solution 11. At what temperature does salt water freeze? (Outcome # 7) (DOK 1) A. 0 °C B. below 0 °C* C. above 0 °C 12. If you want to boil a pot of water containing salt, at what temperature would boiling begin?

(Outcome # 7) (DOK 1) A. 100 °C B. below 100 °C C. above 100 °C* 13. What happens to the freezing point of water when ethylene glycol is added? (Outcome # 8) (DOK 2) A. Ethylene glycol has no effect on the freezing point of water.

B. Ethylene glycol will interfere with the organization of water molecules during the freezing process therefore increasing the freezing point of water.

C. Ethylene glycol will interfere with the organization of water molecules during the freezing process therefore reducing the freezing point of water.* 14. Which of the following is a colligative property? (Outcome # 8) (DOK 1) A. boiling-point elevation* B. temperature of a solution C. color of a solution 15. Which of the following is a not a colligative property? (Outcome # 8) (DOK 1) (Paired item 1) A. boiling-point elevation B. temperature of a solution* C. Freezing-point depression 16. Assuming all the salts below are the same concentration, which salt would lower the freezing point of water the most? (Outcome # 8) (DOK 1) Page 2 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 11: Solutions and Colloids

A. NaCl B. KBr C. CaCl2* 17. Which salt would lower the freezing point of a solvent the most? (Outcome # 8) (DOK 2) A. 1.5m NaCl B. 0.5m CaCl2 C. 1.25m Na2SO4* 18. What would be the best method for raising the boiling point of water in a kettle by a few degrees Celsius? (Outcome # 8) (DOK 3) A. increase the temperature of the stove B. add some table salt to the water* C. increase the temperature of the stove and increase the surface area by transferring the water to a larger kettle 19. What would be the best method for lowering the freezing point of water in an ice tray that is in the freezer? (Outcome # 8) (DOK 3) A. decrease the temperature of the freezer B. decrease the temperature of the freezer and increase the surface area by transferring the water to a larger ice tray C. add some table salt to the water* 20. Patients who enter the emergency room dehydrated are usually given sterile saline solution intravenously. The solution administered is isotonic to prevent cell damage. What would happen if the solution was hypotonic? (Outcome # 6) (DOK 3) A. Hypotonic solutions have a higher osmotic pressure than that within cells so hemolysis can occur.

B. Hypotonic solutions have a lower osmotic pressure than that within cells so hemolysis can occur.* C. Hypotonic solutions have the same osmotic pressure as that within cells so hemolysis can occur.

21. Patients who enter the emergency room dehydrated are usually given sterile saline solution intravenously. The solution administered is isotonic to prevent cell damage. What would happen if the solution was hypertonic? (Outcome # 6) (DOK 3) (Paired item 1) A. Hypertonic solutions have the same osmotic pressure as that within cells so crenation can occur.

B. Hypertonic solutions have a lower osmotic pressure than that within cells so crenation can occur.

C. Hypertonic solutions have a higher osmotic pressure than that within cells so crenation can occur.* Page 3 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 11: Solutions and Colloids

22. Which type of solution has a lower osmotic pressure than that within cells? (Outcome # 6) (DOK 1) A. hypertonic B. hypotonic* C. isotonic 23. Which type of solution has a higher osmotic pressure than that within cells? (Outcome # 6) (DOK 1) A. isotonic B. hypertonic* C. hypotonic 24. Which type of solution has the same osmotic pressure as that within cells? (Outcome # 6) (DOK 1) A. hypertonic B. isotonic* C. hypotonic 25. What is the osmolarity of a 2 M NaCl solution? (Outcome # 6) (DOK 1) A. 2 osmol B. 6 osmol C. 4 osmol* 26. A KCl solution is 0.500 M. What is the osmolarity? (Outcome # 6) (DOK 1) (Paired item 1) A. 1 osmol* B. 2 osmol C. 4 osmol 27. 45.8 g of NaCl is dissolved in 500. mL of a water (d = 1.00 g/mL) and is placed in the freezer at -1 °C overnight. Which statement best describes what would happen to the solution?

(Outcome # 3) (DOK 3) A. The freezing point of the NaCl solution would be -5.83 °C, so the solution would not freeze.* B. The freezing point of the NaCl solution would be 5.83 °C, so the solution would freeze.

C. The freezing point of the NaCl solution would be -2.92 °C, so the solution would not freeze.

28. 17.1 g of calcium chloride is dissolved in 750. mL of a water (d = 1.00 g/mL) and is placed in the freezer at -2 °C overnight. Which statement best describes what would happen to the solution? (Outcome # 3) (DOK 3) (Paired item 1) A. The freezing point of the calcium chloride solution would be 1.15 °C, so the solution would freeze.

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OpenStax Chemistry Supplemental Test Items Chapter 11: Solutions and Colloids

B. The freezing point of the calcium chloride solution would be -1.15 °C, so the solution would freeze.* C. The freezing point of the calcium chloride solution would be -0.382 °C, so the solution would freeze.

29. How would you be able to increase the boiling point of water on a hotplate? (Outcome # 3) (DOK 2) A. increase the temperature of the hotplate B. add less water and increase the temperature of the hotplate C. add some NaCl to the water* 30. How would you increase the concentration of a 1 M NaCl solution? (Outcome # 3) (DOK 1) A. decant some of the solution down the sink B. bring the solution to near boiling until desired volume is achieved* C. decrease the temperature of the salt solution to near freezing 31. The solubility of NaCH3CO2 in water is ~1.23 g/mL. What would be the best method for preparing a supersaturated NaCH3CO2 solution? (Outcome # 3) (DOK 2) A. add 130 g of NaCH3CO2 to 100 mL of H2O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature* B. add 123 g of NaCH3CO2 to 200 mL of H2O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature C. add 130 g of NaCH3CO2 to 100 mL of H2O at room temperature while stirring until all the solid dissolves 32. The solubility of KCl in water is ~344 g/L. What would be the best method for preparing a 100 mL saturated KCl solution? (Outcome # 3) (DOK 2) A. add 38.0 g of KCl to 100 mL of H2O at room temperature while stirring* B. add 30.0 g of KCl to 100 mL of H2O at room temperature while stirring C. add 34.0 g of KCl to 100 mL of H2O at room temperature while stirring

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OpenStax Chemistry Supplemental Test Items Chapter 12: Kinetics Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 12: Kinetics 1. _____ energy is the minimum amount of energy that colliding molecules must possess in order for a chemical reaction to occur. (Outcome # 6) (DOK 1) A. activation* B. bond C. collision 2. A reaction where the products are lower in energy than the reactants is an example of an _____. (Outcome # 6) (DOK 1) A. endothermic process B. exothermic process* C. endergonic process 3. A reaction where the products are higher in energy than the reactants is an example of an _____. (Outcome # 6) (DOK 1) A. endothermic process* B. exothermic process C. exergonic process 4. Which of the following affects the rate of a reaction? (Outcome # 6) (DOK 1) A. concentration, temperature, nature of reactants, presence of solvents B. concentration, temperature, molecular size, presence of catalysts C. concentration, temperature, nature of reactants, presence of catalysts* 5. What affect does temperature have on the rate of a reaction? (Outcome # 6) (DOK 2) A. the lower the temperature, the lower the kinetic energy which results in more effective collisions therefore increasing the rate of a reaction B. the higher the temperature, the greater the kinetic energy which results in more effective collisions therefore increasing the rate of a reaction* C. the higher the temperature, the greater the kinetic energy which results in more effective collisions therefore decreasing the rate of a reaction 6. Which statement best describes the effect of concentration on the rate of a reaction?

(Outcome # 6) (DOK 2) A. higher concentrations result in more effective collisions therefore increasing the rate of a reaction* B. higher concentrations result in less effective collisions therefore increasing the rate of a reaction Page 1 of 2

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OpenStax Chemistry Supplemental Test Items Chapter 12: Kinetics

C. higher concentrations result in more collisions therefore increasing the rate of a reaction* 7. What is the overall rate order of a reaction A + B  C which has the following rate equation: rate = k[A][B]? (Outcome # 4) (DOK 1) A. 2* B. 1 C. 0 8. What is the rate order with respect to [A] in the reaction A + B  C which has following rate equation: rate = k[B]? (Outcome # 4) (DOK 1) A. 2 B. 1 C. 0* 9. What is the rate order with respect to [B] in the reaction A + B  C which has following rate equation: rate = k[B]? (Outcome # 4) (DOK 1) A. 2 B. 1* C. 0 10. What is the rate equation of a reaction A + B  C which has a first-rate order for [A] and zero-rate order for [B]? (Outcome # 4) (DOK 2) A. rate = k[A]* B. rate = k[A][B] C. rate = k[B]

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OpenStax Chemistry Supplemental Test Items Chapter 13: Fundamental Equilibrium Concepts Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 13: Fundamental Equilibrium Concepts 1. Consider the following equilibrium mixture in a closed system: H 2O(g) + CO(g) ⇌ H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas?

(Outcome # 3) (DOK 3) A. The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved.* B. The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right which would result in more CO2 being produced until equilibrium is achieved.

C. The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen.

2. Consider the following equilibrium mixture in a closed system: H 2O(g) + CO(g) ⇌ H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of carbon monoxide gas? (Outcome # 3) (DOK 3) A. The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved.

B. The addition of carbon monoxide gas would not disrupt the equilibrium, so nothing would happen.

C. The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the right which would result in more products being produced until equilibrium is achieved.* 3. Write the equilibrium expression for H2O(g) + CO(g) ⇌ H2(g) + CO2(g). (Outcome # 3) (DOK 1) A. Kc = [CO2] [H2] / [H2O] [CO]* B. Kc = [H2O] [CO] / [CO2] [H2] C. Kc = [CO2] [H2] / [CO] 4. Write the equilibrium expression for 2NO(g) + 2H2(g) ⇌ N2(g) + 2H2O(g). (Outcome # 3) (DOK 1) A. Kc = [NO]2 [H2]2 / [H2O]2 [N2] B. Kc = [H2O]2 [N2] / [NO]2 [H2]2* C. Kc = [N2] / [NO]2 [H2]2 Page 1 of 2

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OpenStax Chemistry Supplemental Test Items Chapter 13: Fundamental Equilibrium Concepts

5. The Kc for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I2, and H2 are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct?

(Outcome # 4) (DOK 2) A. Q = 5.15 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium* B. Q = 15.2 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium C. Q = 0.194 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium 6. If the reaction quotient is greater than the equilibrium constant, which statement would be correct? (Outcome # 4) (DOK 1) A. If Q > K, then the reaction needs to proceed towards the right to reach equilibrium.

B. If Q > K, then the reaction needs to proceed towards the left to reach equilibrium.* C. If Q > K, then the reaction is at equilibrium.

7. If the reaction quotient is less than the equilibrium constant, which statement would be correct? (Outcome # 4) (DOK 1) A. If Q < K, then the reaction needs to proceed towards the left to reach equilibrium.

B. If Q < K, then the reaction is at equilibrium.

C. If Q < K, then the reaction needs to proceed towards the right to reach equi librium.*

Page 2 of 2

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 14: Acid-Base Equilibria 1. Which of the following is an electronic device used to measure the hydrogen ion activity in aqueous solutions? (Outcome # 7) (DOK 1) A. pH meter* B. potentiometer C. ammeter 2. Which of the following is a typical type of electrode found on a pH meter? (Outcome # 7) (DOK 1) A. gold electrode B. glass electrode* C. silver electrode 3. When titrating a weak acid with a strong base, approximately where would the pH be observed when reaching the equivalence point? (Outcome # 4) (DOK 2) A. at the equivalence point, the pH is greater than 7* B. at the equivalence point, the pH is equal to 7 C. at the equivalence point, the pH is less than 7 4. When titrating a weak base with a strong acid, approximately where would the pH be observed when reaching the equivalence point? (Outcome # 4) (DOK 2) (Paired item 1) A. at the equivalence point, the pH is greater than 7 B. at the equivalence point, the pH is equal to 7 C. at the equivalence point, the pH is less than 7* 5. When titrating a strong acid with a strong base, approximately where would the pH be observed when reaching the equivalence point? (Outcome # 4) (DOK 2) (Paired item 2) A. at the equivalence point, the pH is greater than 7 B. at the equivalence point, the pH is equal to 7* C. at the equivalence point, the pH is less than 7 6. What are the products formed at the equivalence point when titrating a strong acid with a strong base? (Outcome # 4) (DOK 2) A. salt and water* B. the solution is neutral, so water only C. no products are formed 7. Phenolphthalein can be used as an _____ in acid-base titrations. (Outcome # 4) (DOK 1) A. equivalence point B. end-point Page 1 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

C. indicator* 8. Phenolphthalein can be used as an indicator in acid-base titrations. When a few drops are added to an acidic solution which is then titrated with a strong base, the color of the solution changes from _____ to _____. (Outcome # 4) (DOK 1) A. colorless; pink* B. pink; colorless C. colorless; red 9. When blue litmus paper is in contact with an acid, the litmus paper will turn _____.

(Outcome # 4) (DOK 1) A. orange B. red* C. green 10. When red litmus paper is in contact with a base, the litmus paper will turn _____.

(Outcome # 4) (DOK 1) (Paired item 1) A. orange B. green C. blue* 11. Which of the following is a diprotic acid? (Outcome # 3) (DOK 1) A. H3PO4 B. H2PO4-* C. HPO4212. Which of the following is an amphiprotic substance? (Outcome # 3) (DOK 1) A. H3PO4 B. PO43C. HPO42-* 13. What is the conjugate base that is formed when carbonic acid is dissolved in water?

(Outcome # 3) (DOK 2) A. H3O+ B. HCO3-* C. CO3214. When phosphoric acid is dissolved in water, what is the conjugate acid that is formed?

(Outcome # 3) (DOK 2) A. H2PO4B. H3O+* C. HPO4215. What is the conjugate base that is formed upon the addition of carbonic acid to water?

(Outcome # 3) (DOK 2) A. HCO3-* Page 2 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

B. H3O+ C. CO3216. Rank the following oxyanions in order of increasing basicity: ClO 4-, ClO2-, ClO-, ClO3-.

(Outcome # 3) (DOK 2) A. ClO4-, ClO-, ClO2-, ClO3B. ClO-, ClO2-, ClO3-, ClO4C. ClO4-, ClO3-, ClO2-, ClO-* 17. Rank the following oxoacids in order of increasing acidity: HClO 2, HClO4, HClO, HClO3.

(Outcome # 3) (DOK 2) A. HClO, HClO2, HClO3, HClO4* B. HClO4, HClO2, HClO, HClO3 C. HClO4, HClO3, HClO2, HClO 18. What is the pH of a solution if 10 mL of a 1 M HCl solution is added to 10 mL of a 1 M NaOH solution? (Outcome # 10) (DOK 2) A. 14 B. 7* C. 0 19. If 10 mL of a 1 M HI solution is added to 5 mL of a 1 M KOH solution, the resulting solution would be _____. (Outcome # 10) (DOK 2) A. acidic* B. basic C. neutral 20. If 3 mL of a 0.5 M HBr solution is added to 20 mL of a 0.5 M NaOH solution, the resulting solution would be _____. (Outcome # 10) (DOK 2) (Paired item 1) A. acidic B. basic* C. neutral 21. What is the hydronium concentration of a solution at pH 7? (Outcome # 10) (DOK 1) A. 1 x 10+7 M B. 1 x 10-14 M C. 1 x 10-7 M* 22. A student titrates 50.0 mL of an unknown concentration of HI with 85 mL of a 1.0 M solution of NaOH to reach the equivalence point. What is the pH of the HI solution?

(Outcome # 10) (DOK 3) A. -0.23* B. 0.23 C. 1.7 Page 3 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

23. A student titrates a 25 mL of an unknown concentration of HCl with 35 mL of a 0.890 M solution of KOH to reach the equivalence point. What is the pH of the HCl solution?

(Outcome # 10) (DOK 3) (Paired item 1) A. -0.10* B. 0.10 C. 1.2 24. A student discovers a bottle of a highly corrosive monoprotic acid with the label partially destroyed. How can the concentration of the unknown acid be determined without using a pH meter? (Outcome # 10) (DOK 3) A. The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The moles of OH- added would be equal to moles of H+ in the unknown at the half-way point, therefore, the concentration of the unknown can be calculated.

B. The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The moles of OH- added would be equal to moles of H+ in the unknown at the equivalence point, therefore, the concentration of the unknown can be calculated.* C. The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The pH at the equivalence point should be 7 since this is a neutralization reaction, therefore, the concentration of the unknown acid is 1 x 10-7 M. 25. A student discovers a bottle of NaOH with a partially destroyed label. How can the concentration be determined without using a pH meter? (Outcome # 10) (DOK 3) A. The student can set-up a titration experiment, where a standardized HCl solution is used to titrate the NaOH. The moles of H+ and OH- are equal at the equivalence point, therefore, the concentration of NaOH can be calculated.* B. The student can set-up a titration experiment, where a standardized HCl solution is used to titrate the NaOH. The pH at the equivalence point should be 7 since this is a neutralization reaction, therefore, the concentration of NaOH is 1 x 10 -7 M. C. The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate HCl. The moles of H+ and OH- are equal at the equivalence point, therefore, the concentration of NaOH can be calculated.

26. What is the pH of 0.048 M solution of hydrochloric acid? (Outcome # 7) (DOK 1) A. 0.32 B. 4.8 C. 1.3* Page 4 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

27. What is the pH of 0.014 M solution of hydroiodic acid? (Outcome # 7) (DOK 1) (Paired item 1) A. 1.4 B. 1.9* C. 0.85 28. What is the pH of deionized water? (Outcome # 7) (DOK 1) A. pH = 7* B. pH < 7 C. pH > 7 29. What is the pH of 0.48 M HCl solution? (Outcome # 2) (DOK 1) A. 0.32* B. -0.32 C. 13.68 30. What is the pH of 8.1 x 10-5 M HClO4 solution? (Outcome # 2) (DOK 1) (Paired item 1) A. 9.91 B. 4.09* C. -4.09 31. What is the hydroxide ion concentration for a 23 % (m/v) HNO3 solution? (Outcome # 2) (DOK 3) A. 10.35 M B. 3.65 M C. 2.74 x 10-15 M* 32. Blood is considered a buffered solution. What is the pH range of blood? (Outcome # 2) (DOK 1) A. 7.35 - 7.45* B. 6.35 - 6.45 C. 8.35 - 8.45 33. What instrument can be used to measure the hydrogen ion concentration in solutions?

(Outcome # 2) (DOK 1) A. ammeter B. pH meter* C. potentiometer 34. Which acid has a lower pH? (Outcome # 5) (DOK 2) A. 1.0 M acetic acid* B. 0.50 M acetic acid C. 0.25 M acetic acid 35. Which acid has a higher hydrogen ion concentration? (Outcome # 5) (DOK 2) A. 1.0 M HCl Page 5 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

B. 0.050 M HNO3 C. 1.25 M HBr* 36. What is the base in the following reaction: HCl (aq) + H 2O (l)  Cl- (aq) + H3O+ (aq)?

(Outcome # 5) (DOK 2) A. ClB. H3O+ C. H2O* 37. What is the conjugate acid in the following reaction: HCl (aq) + H2O (l)  Cl- (aq) + H3O+ (aq)? (Outcome # 5) (DOK 2) A. ClB. H3O+* C. H2O 38. What is the conjugate base in the following reaction: HCl (aq) + H 2O (l)  Cl- (aq) + H3O+ (aq)? (Outcome # 5) (DOK 2) (Paired item 1) A. Cl-* B. H3O+ C. H2O 39. What is the conjugate base of HSO4-? (Outcome # 5) (DOK 2) A. H2SO4 B. SO42-* C. SO440. What is the conjugate acid of HSO4-? (Outcome # 5) (DOK 2) A. H2SO4* B. SO42C. H2SO441. Write the equilibrium expression for the autoionization of water. (Outcome # 3) (DOK 3) A. Kw = [H3O+] [OH-] / [H2O]2 B. Kw = [H3O+] [OH-]* C. Kw = [H2O]2 / [H3O+] [OH-] 42. What is the pOH of a solution that has a pH of 7? (Outcome # 2) (DOK 1) A. 7* B. 14 C. 0 43. What is the pOH of a solution that has a pH of 2? (Outcome # 2) (DOK 1) (Paired item 1) A. 12* B. 7 C. 14 44. Which acid has the lowest hydroxide ion concentration? (Outcome # 5) (DOK 2) Page 6 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

A. 0.010 M HCl B. 0.050 M HNO3* C. 0.015 M HBr* 45. What is the conjugate base in the following reaction: HI (aq) + H2O (l)  I- (aq) + H3O+ (aq)? (Outcome # 5) (DOK 2) A. I-* B. H3O+ C. H2O 46. What is the acid in the following reaction: NH3 (aq) + H2O (l)  NH4+ (aq) + OH- (aq)?

(Outcome # 5) (DOK 2) A. NH3 B. NH4+ C. H2O*

Page 7 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 15: Equilibria of Other Reaction Classes Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 15: Equilibria of Other Reaction Classes [No items]

Page 1 of 1

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OpenStax Chemistry Supplemental Test Items Chapter 16: Thermodynamics Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 16: Thermodynamics 1. At what temperature are the standard Gibbs free energy of formations reported? (Outcome # 11) (DOK 1) A. 20.0 °C B. 0 °C C. 25.0 °C* 2. What is the ∆G° if ∆H° is +58.7 kJ and ∆S° is +129 J/K? (Outcome # 11) (DOK 1) A. +20.2 kJ* B. -20.2 kJ C. +55.5 kJ 3. What is the ∆G° if ∆H° is +72.7 kJ and ∆S° is +112 J/K? (Outcome # 11) (DOK 1) (Paired item 1) A. -39.3 kJ B. +39.3 kJ* C. +70.0 kJ 4. What is the ∆S° if the ∆H° is +88.00 kJ and ∆G ° is +11.21 kJ? (Outcome # 11) (DOK 1) A. -258 J B. +258 J* C. +0.258 J 5. What is the ∆S° if the ∆H° is +48.90 kJ and ∆G ° is +19.01 kJ? (Outcome # 11) (DOK 1) (Paired item 1) A. -0.1003 J B. +0.1003 J C. +100.3 J* 6. An _____ reaction is a nonspontaneous reaction in which the standard change in free energy is positive. (Outcome # 3) (DOK 1) A. exergonic B. endergonic* C. exothermic 7. An _____ reaction is a spontaneous reaction in which the standard change in free energy is negative. (Outcome # 3) (DOK 1) A. exergonic* B. endergonic C. exothermic Page 1 of 1

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OpenStax Chemistry Supplemental Test Items Chapter 17: Electrochemistry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 17: Electrochemistry 1. Write a balanced redox reaction for the formation of rust on iron metal and identify the correct oxidizing agent and/or reducing agent. (Outcome # 6) (DOK 3) A. Iron is the oxidizing agent and O2 is neither a reducing agent nor an oxidizing agent B. Iron is the oxidizing agent and O2 is the reducing agent C. Iron is the reducing agent and O2 is the oxidizing agent* 2. Which is the reducing agent in the combustion of methanol? (Outcome # 6) (DOK 3) A. CH3OH* B. O2 C. CO2 3. Which is the oxidizing agent in the combustion of methanol? (Outcome # 6) (DOK 3) A. CH3OH B. O2* C. CO2 4. Propane is used as a fuel source on many barbeque grills. What is undergoing oxidation during the burning of propane while grilling? (Outcome # 6) (DOK 3) A. CH3CH2CH3* B. O2 C. CO2 5. Propane is used as a fuel source on many barbeque grills. What is undergoing reduction during the burning of propane while grilling? (Outcome # 6) (DOK 3) (Paired item 1) A. CH3CH2CH3 B. O2* C. CO2 6. Automobiles from northern states tend to show more signs of rust formation than southern states. The reason for this is that the rate of corrosion is affected by _____, which is more common during winter months especially in northern states. (Outcome # 6) (DOK 1) A. the cold air and clouds B. rain clouds C. snow, ice, and salt mixtures* 7. Certain anaerobic organisms such as methanogens have the ability to metabolize carbon dioxide into methane in the presence of hydrogen. Methane is produced by the oxidation of _____? (Outcome # 6) (DOK 3) A. H2* Page 1 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 17: Electrochemistry

B. CO2 C. CH4 8. A voltaic cell must be split into two separate cells, an oxidation and reduction half-cells. The two half-cells must be connected by a _____ so ions can freely flow between the two halfcells to balance the charges or the voltaic cell cannot function. (Outcome # 10) (DOK 2) A. metallic wire B. salt bridge* C. membrane 9. In a voltaic cell, oxidation occurs at the _____. (Outcome # 10) (DOK 1) A. anode terminal* B. cathode terminal C. positive terminal 10. In a voltaic cell, reduction occurs at the _____. (Outcome # 10) (DOK 1) A. anode terminal B. cathode terminal* C. negative terminal 11. Electron flow in a voltaic cell is always from _____ to _____. (Outcome # 10) (DOK 2) A. anode to cathode* B. cathode to anode C. anode to negative terminal 12. The following can be used as an electrolyte for a salt bridge in a voltaic cell? (Outcome # 10) (DOK 1) A. KNO3(aq)* B. H2O(l) C. CH3OH(l) 13. The following can be used as an electrolyte for a salt bridge in a voltaic cell? (Outcome # 10) (DOK 1) (Paired item 1) A. CCl4(l) B. CH3CH2OH(l) C. Na2SO4(aq)* 14. In a voltaic cell, electrons are produced at the _____. (Outcome # 10) (DOK 1) A. positive terminal B. anode terminal* C. cathode terminal 15. The anode terminal in a voltaic cell is the _____ terminal. (Outcome # 10) (DOK 1) A. (-)* B. (+) C. Neutral Page 2 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 17: Electrochemistry

16. The cathode terminal in a voltaic cell is the _____ terminal. (Outcome # 10) (DOK 1) A. (-) B. (+)* C. neutral 17. In a voltaic cell, electrons are received at the _____. (Outcome # 10) (DOK 1) A. cathode terminal* B. negative terminal C. anode terminal 18. Based on the reduction potential data, what is the standard cell potential for the following electrochemical cell reaction: Zn(s) + Cu2+(aq)  Zn2+(aq) + Cu(s)? (Outcome # 11) (DOK 2) E°red = -0.763 V for Zn2+(aq) + 2e-  Zn(s) E°red = +0.340 V for Cu2+(aq) + 2e-  Cu(s) A. +1.103 V* B. -0.423 V C. +0.423 V 19. Based on the reduction potential data, what is the standard cell potential for the following electrochemical cell reaction: Cu(s) + 2Ag+  Cu2+(aq) + 2Ag(s)? (Outcome # 11) (DOK 2) (Paired item 1) E°red = +0.800 V for Ag+(aq) + e-  Ag(s) E°red = +0.340 V for Cu2+(aq) + 2e-  Cu(s) A. +1.14 V B. +0.460 V* C. +1.26 V 20. Based on the following reduction potential data, which is the strongest reducing agent?

(Outcome # 11) (DOK 1) E°red = +1.78 V for H2O2(aq) + 2H+(aq) + 2e-  2H2O(l) E°red = +0.800 V for Ag+(aq) + e-  Ag(s) E°red = -0.130 V for Pb2+(aq) + 2e-  Pb(s) A. Pb(s)* B. Ag(s) C. H2O(l) Page 3 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 17: Electrochemistry

21. Based on the following reduction potential data, which is the strongest oxidizing agent?

(Outcome # 11) (DOK 1) E°red = +1.78 V for H2O2(aq) + 2H+(aq) + 2e-  2H2O(l) E°red = +0.800 V for Ag+(aq) + e-  Ag(s) E°red = -0.130 V for Pb2+(aq) + 2e-  Pb(s) A. Pb2+(aq) B. H2O2(aq)* C. Ag+(aq) 22. The standard cell potential is +0.460 V for the following electrochemical cell reaction: Cu(s) + 2Ag+(aq)  Cu2+(aq) + 2Ag(s). What is the ∆G°rxn? (Outcome # 11) (DOK 2) A. -88.8 kJ/mol* B. -44.4 kJ/mol C. +44.4 kJ/mol 23. What is the ∆G°rxn for a 2 electron transfer electrochemical cell with a standard cell potential of +0.770 V. (Outcome # 11) (DOK 2) A. -74.3 kJ/mol B. -149 kJ/mol* C. +74.3 kJ/mol 24. Based on the following reduction potential data, what is the ∆G° rxn for the following electrochemical cell reaction: Zn(s) + Cu2+(aq)  Zn2+(aq) + Cu(s)? (Outcome # 11) (DOK 3) E°red = -0.763 V for Zn2+(aq) + 2e-  Zn(s) E°red = +0.340 V for Cu2+(aq) + 2e-  Cu(s) A. +106 kJ/mol B. -106 kJ/mol C. -213 kJ/mol* 25. Which of the following acids is a strong oxidant? (Outcome # 5) (DOK 1) A. HCl B. HNO3* C. HI 26. Which strong acid is commonly used in automobile batteries? (Outcome # 2) (DOK 2) A. HCl B. H2SO4* C. HNO3 Page 4 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 17: Electrochemistry

27. Cell phones batteries are typically rechargeable. How do they differ from non-rechargeable batteries? (Outcome # 2) (DOK 3) A. A rechargeable battery has the ability to undergo a double replacement reaction while non-rechargeable batteries do not. Therefore, the forward direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.

B. A rechargeable battery has the ability to undergo a reversible redox reaction while non-rechargeable batteries do not. Therefore, the forward direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.* C. A rechargeable battery has the ability to undergo a redox reaction while nonrechargeable batteries do not. Therefore, the reverse direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.

28. The process of corrosion involves what type of reaction? (Outcome # 2) (DOK 2) A. double displacement reaction B. acid-base reaction C. redox reaction* 29. What is the oxidation state of oxygen in K2O2? (Outcome # 2) (DOK 2) A. 0 B. -1* C. -2 30. Which of the following is a strong oxidizing agent? (Outcome # 2) (DOK 2) A. N2 B. O2* C. H2

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OpenStax Chemistry Supplemental Test Items Chapter 18: Representative Metals, Metalloids, and Nonmetals Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 18: Representative Metals, Metalloids, and Nonmetals 1. What is one of the primary components in our atmosphere that leads to acidic rain?

(Outcome # 5) (DOK 1) A. SO B. SO2* C. both SO and SO2 2. Which of the following gases are flammable? (Outcome # 5) (DOK 1) A. helium B. hydrogen* C. nitrogen 3. Which of the following gases are considered inert? (Outcome # 5) (DOK 1) (Paired item 1) A. oxygen B. hydrogen C. nitrogen* 4. Which one of the following elements does not exist as a diatomic molecule in nature?

(Outcome # 1,9) (DOK 2) A. hydrogen B. nitrogen C. neon* 5. Which diatomic element is considered an inert gas? (Outcome # 9) (DOK 1) A. H2 B. N2* C. F2 6. What is the active ingredient in most solid antacids? (Outcome # 2) (DOK 2) A. CaCO3* B. Ca(OH)2 C. KOH 7. Which of the following are considered toxic heavy metals? (Outcome # 5) (DOK 2) A. lead, cadmium, and mercury* B. lead, iron, and mercury C. arsenic, mercury, and calcium 8. What compound does magnesium and nitrogen form? (Outcome # 8) (DOK 1) A. Mg3N2* B. Mg2N3 Page 1 of 2

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OpenStax Chemistry Supplemental Test Items Chapter 18: Representative Metals, Metalloids, and Nonmetals

C. MgN

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OpenStax Chemistry Supplemental Test Items Chapter 19: Transition Metals and Coordination Chemistry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 19: Transition Metals and Coordination Chemistry [No items]

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OpenStax Chemistry Supplemental Test Items Chapter 20: Organic Chemistry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 20: Organic Chemistry

1. What is the molar mass of isopropyl alcohol? (Outcome # 4) (DOK 2) A. 60.1 g/mol* B. 32.0 g/mol C. 46.1 g/mol

Page 1 of 1

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OpenStax Chemistry Supplemental Test Items Chapter 21: Nuclear Chemistry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 21: Nuclear Chemistry 1. Which of the following is emitted by radioactive nuclei and contains two protons and two neutrons? (Outcome # 3) (DOK 1) A. alpha particles* B. beta particles C. gamma rays 2. Which of the following is emitted by radioactive nuclei and is a type of high energy radiation that does not contain mass or charge? (Outcome # 3) (DOK 1) A. alpha particles B. beta particles C. gamma rays* 3. Which of the following is emitted by radioactive nuclei and has a mass and charge that is identical to an electron? (Outcome # 3) (DOK 1) A. alpha particles B. beta particles* C. gamma rays 4. Gamma Ray Emission is represented by which symbol? (Outcome # 3) (DOK 1) A. β B. α C. γ* 5. Beta particle emission is represented by which symbol? (Outcome # 3) (DOK 1) A. β* B. α C. γ 6. Alpha particle emission is represented by which symbol? (Outcome # 3) (DOK 1) A. β B. α* C. γ 7. Which of the following sources of radiation is higher in energy? (Outcome # 3) (DOK 1) A. visible light B. ultra violet light* C. infrared light 8. Which of the following sources of radiation has a longer wavelength? (Outcome # 3) (DOK 1) A. visible light Page 1 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 21: Nuclear Chemistry

B. infrared light* C. ultra violet light 9. Which is an example of nonionizing radiation? (Outcome # 3) (DOK 1) A. radiowaves* B. x-rays C. cosmic rays 10. Which is an example of ionizing radiation? (Outcome # 3) (DOK 1) A. radiowaves B. infrared light C. cosmic rays* 11. Which is an example of ionizing radiation? (Outcome # 3) (DOK 1) (Clone 1) A. ultra violet light* B. visible light C. infrared light 12. What is nonionizing radiation? (Outcome # 3) (DOK 1) A. radiation that does not have a sufficient amount of energy to remove an electron from an atom or molecule* B. radiation that has sufficient amount of energy to remove an electron from an atom or molecule C. radiation that does not have a sufficient amount of energy to gain an electron from an atom or molecule 13. What is ionizing radiation? (Outcome # 3) (DOK 1) A. radiation that does not have a sufficient amount of energy to remove an electron from an atom or molecule B. radiation that has sufficient amount of energy to gain an electron from an atom or molecule C. radiation that has sufficient amount of energy to remove an electron from an atom or molecule* 14. Which type of radiation has sufficient energy to penetrate into organs, tissue, and bone?

(Outcome # 3) (DOK 2) A. gamma radiation* B. alpha radiation C. beta radiation 15. Which type of radiation has insufficient energy and cannot penetrate the outer layers of human skin? (Outcome # 3) (DOK 2) A. gamma radiation B. alpha radiation* C. beta radiation Page 2 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 21: Nuclear Chemistry

16. Which is a type of nuclear reaction where two small nuclei are merged together to generate a larger nuclei and a tremendous amount of energy? (Outcome # 3) (DOK 1) A. nuclear fission B. nuclear fusion* C. neutron scattering 17. Which is a type of nuclear reaction where a large nucleus splits into two smaller nuclei with the release of a large amount of energy?(Outcome # 3) (DOK 1) A. neutron scattering B. nuclear fusion C. nuclear fission* 18. Through what process does the sun generate its energy? (Outcome # 3) (DOK 1) A. nuclear fusion* B. nuclear fission C. neutron scattering 19. _____ is an instrument used to measure levels of ionizing radiation. (Outcome # 3) (DOK 1) A. radio counter B. Geiger counter* C. radiation counter 20. Technetium-99m is commonly used as a medical radioisotope in numerous medical diagnostic procedures yearly. The half-life of technetium-99m is 6.00 hours. After 1 day, a medical sample was found to contain 0.05 grams of technetium-99m. How many grams of technetium-99m were present initially? (Outcome # 3) (DOK 3) A. 0.8 g* B. 0.2 g C. 0.1 g 21. Before the use of technetium-99m, patients with high risk coronary artery disease were evaluated using thallium-201 which has a half-life of 73.00 hours. If a person is exposed to 5.000 μg of thallium-201, how many hours would it take to reach 10.00 % of its original mass? (Outcome # 3) (DOK 3) A. 3.322 hours B. 242.5 hours* C. 21.98 hours 22. How much of a 0.230 g radioactive sample with a half-life of 8 hours would remain after a period of 2.50 days? (Outcome # 3) (DOK 3) A. 8.98 x 10-4 g B. 1.80 x 10-3 g C. 1.27 x 10-3 g* Page 3 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 21: Nuclear Chemistry

23. What is the half-life of a radioactive sample if 0.892 g would take 3.73 days to decay to 0.114 g? (Outcome # 3) (DOK 3) A. 0.331 hours B. 2.96 hours C. 30.1 hours*

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TEST BANK

TEST BANK

TEST BANK

TEST BANK

OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 01: Essential Ideas 1. A 0.150 kg metallic block measures 25.0 mm in length, 43.0 mm in width, and 19 .0 mm in height. What is the density of the metallic block in g/cm3? (Outcome # 3) (DOK 2) A. 7.34 x 10-6 g/cm3 B. 7.34 x 10-3 g/cm3 C. 7.34 g/cm3* 2. An object with a mass of 0.255 kg and density of 2.89 g/cm 3 measures 34 mm in length and 46 mm in width. What is the height of the object? (Outcome # 3) (DOK 3) A. 5.6 cm* B. 5.6 x 10-2 cm C. 7.2 x 10-4 cm 3. How would you determine the density of an irregular object? (Outcome # 3) (DOK 3) A. It would be impossible to determine the mass of the object without more information.

B. D = m/v, so measure the mass of the object using a balance. Then to find volume, measure the height, width, and length using an appropriate measuring tool.

C. D = m/v, so measure the mass of the object using a balance. Then to find volume, fill a graduated cylinder with a known amount of water and immerse the object in the water. The amount of displaced water is the volume in cm3 or mL.* 4. What is the base unit for length in the metric system? (Outcome # 6) (DOK 1) A. m* B. km C. mm 5. What is the base unit for mass in the metric system? (Outcome # 6) (DOK 1) A. kg B. g* C. mg 6. What is the base unit for volume in the metric system? (Outcome # 6) (DOK 1) A. L* B. mL C. dL 7. It is important that scientists use units that are understood on a global level. These units are referred to as SI units which stands for _____. (Outcome # 6) (DOK 1) A. standard international units Page 1 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

B. standard intercontinental units C. international system of units* 8. Convert 18.50 ft to the SI unit for length. (Outcome # 6) (DOK 2) A. 563.9 cm B. 5.639 m* C. 0.005639 km 9. An experimental mouse weighs about 4.41 x 10-2 lbs. What would the weight be in the SI unit for mass? (Outcome # 6) (DOK 2) A. 20.0 g B. 0.0200 kg* C. 20,003 mg 10. Accuracy is defined as how close a measured value comes to a _____. (Outcome # 6) (DOK 1) A. core value B. fixed value C. true value* 11. Precision is defined as how _____ the measured values are to one another. (Outcome # 6) (DOK 1) A. common B. reproducible* C. accurate 12. An experiment requires you to make several measurements. Based on the values in the table below, what would be the best statement that represents the data set if the true value is 0.2135? (Outcome # 11) (DOK 2) Trial A Trial B Trial C 0.2139 0.2893 0.2135 0.2130 0.3210 0.2134 0.2133 0.2999 0.3712 0.2135 0.2998 0.3715 A. The measurements in Trial A are accurate and precise, Trial B is neither accurate nor precise, and Trial C is accurate however, not precise.

B. The measurements in Trial A are accurate and precise, Trial B is neither accurate nor precise, and Trial C is precise however, not accurate.

C. The measurements in Trial A are accurate and precise, Trial’s B and C are neither accurate nor precise.* 13. An experiment requires you to make several measurements. Based on the values in the table below, what would be the best statement that represents the data set if the true value is 2.73? (Outcome # 11) (DOK 2) (Paired item 1) Page 2 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

Trial A Trial B Trial C 2.73 3.00 2.77 3.05 3.03 2.79 3.09 2.99 3.31 2.44 3.01 2.05 A. The measurements in Trial B are precise, however, not accurate. Trial’s A and C are neither accurate nor precise.* B. The measurements in Trial B are accurate, however, not precise. Trial’s A and C are neither accurate nor precise.

C. The measurements in Trial’s A, B, and C are neither accurate nor precise.

14. Which of the following would be considered a chemical change? (Outcome # 9) (DOK 1) A. a rusting nail* B. melting ice C. crushing an aluminum can 15. Which of the following would be considered a physical change? (Outcome # 9) (DOK 1) A. digesting food B. burning paper C. boiling water* 16. A salt water solution is classified as what type of matter? (Outcome # 9) (DOK 1) A. homogeneous mixture* B. heterogeneous mixture C. pure substance 17. How many significant figures are in 0.0000401 kg? (Outcome # 5) (DOK 1) A. 3* B. 7 C. 2 18. How many significant figures are in 0.20 L? (Outcome # 5) (DOK 1) (Paired item 1) A. 3 B. 1 C. 2* 19. Express 1.40 x 10-3 L in decimal notation. (Outcome # 5) (DOK 1) A. 0.00140 L* B. 0.0014 L C. 0.001 L 20. What is the answer for the following calculation: (1.249 - 0.0234) x 139.37? (Outcome # 5) (DOK 2) A. 170.812 B. 170.8* C. 170.81 Page 3 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

21. What is the SI unit for mass? (Outcome # 7) (DOK 1) A. kilogram* B. gram C. milligram 22. What is the SI unit for length? (Outcome # 7) (DOK 1) A. meter* B. kilometer C. millimeter 23. What is the SI unit for temperature? (Outcome # 7) (DOK 1) A. Celsius B. Fahrenheit C. kelvin* 24. How many grams of iron are in 350 mg of iron? (Outcome # 7) (DOK 1) A. 3.50 g B. 0.350 g* C. 35.0 g 25. The prefix milli- in the metric system represents a factor of _____. (Outcome # 7) (DOK 1) A. 103 B. 10-3* C. 1/10-3 26. The prefix kilo- in the metric system represents a factor of _____. (Outcome # 7) (DOK 1) A. 103* B. 10-3 C. 1/103 27. The prefix nano- in the metric system represents a factor of _____. (Outcome # 7) (DOK 1) A. 109 B. 10-6 C. 10-9* 28. An explanation for the collection of observations is considered a _____. (Outcome # 10) (DOK 1) A. theory* B. law C. hypothesis 29. A statement about mass always being conserved in a chemical reaction is an example of a _____. (Outcome # 10) (DOK 1) A. hypothesis B. theory C. law* Page 4 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

30. The scientific method involves various techniques which allow researchers to investigate scientific questions through _____ and _____. (Outcome # 10) (DOK 1) A. analysis and observations B. observations and experimentation* C. analysis and predictions 31. Why has Galileo been called the father of modern science? (Outcome # 10) (DOK 1) A. because he made observations and conducted experiments* B. because he discovered electrochemical cells C. because he was a philosopher 32. List the basic steps of the scientific method process in the order they must be carried out.

(Outcome # 10) (DOK 1) A. observation, hypothesis, prediction, experimentation, and conclusion* B. hypothesis, observation, prediction, experimentation, and conclusion C. prediction, observation, hypothesis, experimentation, and conclusion 33. Which of the following is not part of the scientific method process? (Outcome # 10) (DOK 1) A. observation B. prediction C. discussion* 34. Which of the following would be a good example of an observation in the scientific method process? (Outcome # 10) (DOK 2) A. a researcher watching a chemical reaction B. a researcher watching a chemical reaction and noting color and temperature changes* C. a researcher setting up a chemical reaction in a flask and allowing it to stir for 2 hours 35. Which of the following would be a good example of an observation in the scientific method process? (Outcome # 10) (DOK 2) (Paired item 1) A. a physician observing a patient's reaction to some medication* B. a physician observing his watch C. a physician speaking with and observing a patient in an examination room 36. Which of the following would be good tools for making scientific observations during a chemical reaction? (Outcome # 10) (DOK 2) A. barometer, thermometer, scale B. thermometer, your eyes, clock* C. thermometer, your eyes, tape measure 37. Which of the following would be a good tool for making scientific observations after isolating a solid product from a chemical reaction? (Outcome # 10) (DOK 2) A. balance* Page 5 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

B. clock C. tape measure 38. What can be used to measure the mass of an object? (Outcome # 10) (DOK 1) A. balance* B. tape measure C. caliper 39. Which of the following would be a good example of a hypothesis in the scientific method process? (Outcome # 10) (DOK 3) A. a researcher considers that the more sunlight a green plant receives, the larger the plant will grow* B. a researcher wonders amount the effect of more sunlight on green plant growth C. a researcher watches as a green plant exposed to more sunlight grows over a period of 1 month 40. Which of the following would be a good example of a hypothesis in the scientific method process? (Outcome # 10) (DOK 3) (Paired item 1) A. a clinician confirms that taking a vitamin every day will decrease the level of tiredness in people B. a clinician tells a patient that taking a vitamin every day, may decrease the level of tiredness in people C. a clinician contemplates that taking a vitamin every day, may decrease the level of tiredness in people* 41. Which of the following would be a good example of a hypothesis in the scientific method process? (Outcome # 10) (DOK 3) (Paired item 2) A. a botanist adds 20 mL of water to his plants on a daily basis and he notices a healthy growth, therefore, he believes that adding 40 mL of water on a daily basis will enhance their growth further* B. a botanist adds 20 mL of water to his plants on a daily basis and he notices a healthy growth C. a botanist adds 20 mL of water to his plants on a daily basis and he notices a healthy growth, therefore, adding 40 mL of water on a daily basis will definitely enhance their growth further 42. Once a hypothesis has been established, it can be tested by conducting an _____. (Outcome # 10) (DOK 1) A. observation B. experiment* C. analysis 43. Which statement is correct about the scientific method process? (Outcome # 10) (DOK 1) Page 6 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

A. after testing a hypothesis, a conclusion can be drawn on whether it will be accepted or rejected* B. after testing an observation, a conclusion can be drawn on whether it will be accepted or rejected C. after testing a conclusion, it can be predicted whether a hypothesis will be accepted or rejected 44. Why is chemistry considered a central science? (Outcome # 10) (DOK 1) A. because it is a core course required for most majors in college B. because it is the fundamental science for many other disciplines* C. because it is very important in medicine 45. What is applied research? (Outcome # 10) (DOK 1) A. it deals primarily with solving practical real-world problems* B. it deals primarily with solving practical laboratory problems C. it deals primarily with the fundamentals of science that may result in future applications 46. What is basic research? (Outcome # 10) (DOK 1) A. it deals primarily with solving practical real-world problems B. it deals primarily with the fundamentals of science that may result in future applications* C. it deals primarily with solving practical laboratory problems 47. Which of the following is an example of applied research? (Outcome # 10) (DOK 2) A. a researcher tries to develop a new anti-cancer drug* B. a researcher tries to extract a newly found natural product from plants to study its medicinal properties C. a researcher studies a hormone and its prospect as a cell signaling molecule 48. Which of the following is an example of applied research? (Outcome # 10) (DOK 2) (Paired item 1) A. a researcher tries to extract a newly found natural product from plants to study its medicinal properties B. a researcher tries to study the effect of a new drug on HIV-inhibition* C. a researcher studies a hormone and its prospect as a cell signaling molecule 49. Which of the following is an example of basic research? (Outcome # 10) (DOK 2) A. a researcher tries to study the effect of a new drug on HIV-inhibition B. a researcher tries to develop a new anti-cancer drug C. a researcher studies a hormone and its prospect as a cell signaling molecule* 50. Which is of the following is an example of a physical property? (Outcome # 10) (DOK 1) A. carbon monoxide is poisonous B. acids are sour and bases are bitter* Page 7 of 8

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OpenStax Chemistry Supplemental Test Items Chapter 01: Essential Ideas

C. an iron nail rusts 51. Which is of the following is an example of a physical property? (Outcome # 10) (DOK 1) (Paired item 1) A. water freezes at 273.15 K* B. carbon monoxide is poisonous C. an iron nail rusts 52. Which is of the following is an example of a physical property? (Outcome # 10) (DOK 1) (Paired item 2) A. lead forming lead oxide in the presence of air B. the color of paint* C. digestion 53. Which is of the following is an example of a chemical property? (Outcome # 10) (DOK 1) A. water boils at 100 °C B. acids are sour and bases are bitter C. an iron nail rusts* 54. Which is of the following is an example of a chemical property? (Outcome # 10) (DOK 1) (Paired item 1) A. water boils at 100 °C B. carbon monoxide is poisonous* C. a copper penny weighs 3.00 g 55. The following is an example of a chemical change. (Outcome # 10) (DOK 1) A. cutting paper B. burning paper* C. folding paper 56. The following is an example of a chemical change. (Outcome # 10) (DOK 1) (Paired item 1) A. shredding paper B. decomposing waste* C. dissolving sugar 57. A website claims that there is a natural cure for all cancers; however, doctors do not want to recommend natural remedies because it would make them obsolete. Is this statement logical? (Outcome # 10) (DOK 3) A. yes, doctors can cure all patients B. yes, doctors can cure some patients with natural remedies C. no, doctors cannot cure all patients and regardless of treatment, some patients still remain ill and die*

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 02: Atoms, Molecules, and Ions 1. Structural isomers are considered molecules with the same ____________. (Outcome # 1,5,9) DOK 1 A. kinds and number of atoms but a different arrangement of these atoms* B. number of electrons and protons but a different number of neutrons C. molecular formula but with a different overall charge 2. Which of the following is not a correct element name-symbol combination? (Outcome # 1) DOK 1 A. copper, Cu B. arsenic, Ar* C. gold, Au 3. Isotopes of carbon differ with respect to the number of _________. (Outcome # 1,8) DOK 1 A. protons B. neutrons* C. electrons 4. Elements in group 17 are considered _____________. (Outcome # 1,2) DOK 1 A. alkali Metals B. halogens* C. noble Gases 5. Due to periodicity, which of the following elements has chemical behavior similar to that of Oxygen? (Outcome # 1,2,8) DOK 1 A. bromine B. sulfur* C. carbon 6. Where would you expect to find a stored bottle of HCl in the laboratory? (Outcome # 5) (DOK 1) A. in the storage cabinet labeled strong bases B. in the storage cabinet labeled strong acids* C. in the storage cabinet labeled solvents 7. Where would you expect to find a stored bottle of NaOH in the laboratory? (Outcome # 5) (DOK 1) (Paired item 1) A. in the storage cabinet labeled strong bases* B. in the storage cabinet labeled strong acids C. in the storage cabinet labeled solvents Page 1 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

8. Which of the following would be considered a caustic base? (Outcome # 5) (DOK 1) A. HNO3 B. H2SO4 C. NaOH* 9. Elements arranged horizontally in the periodic table are in the same_____? (Outcome # 2) (DOK 1) A. group or family B. period* C. column 10. Which elements are considered noble gases? (Outcome # 2) (DOK 1) A. He, Ne, Ar* B. H, N, O C. F, Cl, Br 11. Chlorine gas is considered a _____? (Outcome # 2) (DOK 1) A. noble gas B. halogen* C. chalcogen 12. Oxygen gas is considered a _____? (Outcome # 2) (DOK 1) (Paired item 1) A. noble gas B. halogen C. chalcogen* 13. What is the correct formula for acetic acid? (Outcome # 2) (DOK 1) A. CH3CO2H* B. CH3CO2C. CH3CO2H2 14. What is the correct formula for lead(II) nitrate? (Outcome # 2) (DOK 1) (Paired item 1) A. Pd(NO3)2 B. Pb(NO3) C. Pb(NO3)2* 15. What is the name for iron(III) chloride? (Outcome # 2) (DOK 1) A. FeCl2 B. FeCl3* C. FeCl4 16. What is the correct name for the precipitate formed when mixing potassium carbonate and nickel(II) chloride? (Outcome # 2) (DOK 2) A. potassium chloride B. nickel(II) carbonate* C. nickel(III) carbonate Page 2 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

17. Which of the following gases exists as a diatomic molecule? (Outcome # 9) (DOK 1) A. krypton B. hydrogen* C. argon 18. In mass spectrometry, species are separated based off their _____? (Outcome # 7) (DOK 2) A. mass-to-charge ratio* B. mass C. charge 19. Which statement is correct about chlorine-35 and chorine-37? (Outcome # 8) (DOK 1) A. They have the same number of protons and electrons, but a different number of neutrons.* B. They have a different number of protons and electrons, but the same number of neutrons.

C. They have the same number of protons, but a different number of electrons and neutrons.

20. What is the overall charge on a sulfate ion? (Outcome # 8) (DOK 1) A. 0 B. -1 C. -2* 21. What is the overall charge on a phosphate ion? (Outcome # 8) (DOK 1) A. -2 B. -3* C. -1 22. Which of the following would be considered a corrosive acid? (Outcome # 5) (DOK 1) A. HNO3* B. NaOH C. KOH 23. Which list of elements contains ONLY nonmetals? (Outcome # 1,9) (DOK 1) A. helium, carbon, gold B. sodium, chromium, copper C. phosphorus, nitrogen, oxygen* 24. The formula for potassium cyanide is KCN and the formula for calcium fluoride is CaF 2. What is the formula for calcium cyanide? (Outcome # 1,7,8,9) (DOK 2) A. Ca2CN B. CaCN C. Ca(CN)2* 25. Using the periodic table, what is the atomic number of argon? (Outcome # 1,9) (DOK 2) A. 26.98 Page 3 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

B. 13* C. 18 26. Which of the following is an ionic compound? (Outcome # 1,9) (DOK 1) A. CO B. HCl C. Na2O* 27. Structural isomers are considered molecules with the same ____________. (Outcome # 1,9) (DOK 2) A. kinds and number of atoms but a different arrangement of these atoms* B. number of electrons and protons but a different number of neutrons C. molecular formula but with a different overall charge 28. The Greek philosopher Democritus phrased what word for a tiny piece of matter that cannot be divided? (Outcome # 1,9) (DOK 1) A. element B. atom* C. electron 29. Who provided evidence for the existence of a nucleus in an atom? (Outcome # 1,9) (DOK 1) A. John Dalton B. J.J. Thomson C. Ernest Rutherford* 30. Within the nucleus, the positive charge is __________. (Outcome # 1,9) (DOK 2) A. concentrated in the center of an atom* B. spread evenly throughout an atom C. concentrated at multiple sites in an atom 31. Which statement about subatomic particles is NOT true? (Outcome # 1,9) (DOK 2) A. Protons and neutrons have almost the same mass.

B. Protons and electrons have opposite charges.

C. Protons and neutrons have the same charge* 32. The number of protons in one atom of an element is that element’s __________. (Outcome # 1,9) (DOK 1) A. mass number B. atomic mass C. atomic number* 33. To calculate the number of neutrons in an atom, you would subtract (Outcome # 1,9) (DOK 1) A. mass number from atomic number B. atomic number from mass number* C. atomic number from electron number Page 4 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

34. Which of the following is not a correct element name-symbol combination? (Outcome # 1,9) (DOK 1) A. copper, Cu B. arsenic, Ar* C. gold, Au 35. Isotopes of carbon differ with respect to the number of _________. (Outcome # 1,9) (DOK 1) A. protons B. neutrons* C. electrons 36. The fact that LiBr is 7.99 % lithium and 92.01 % bromine by mass regardless of its origin is an example of _____. (Outcome # 9) (DOK 1) A. law of definite proportions* B. law of conservation of mass C. Dalton’s atomic theory 37. Which of the following elements form +2 ions? (Outcome # 9) (DOK 1) A. strontium, magnesium, calcium* B. lithium, sodium, potassium C. sodium, magnesium, aluminum 38. Which of the following elements form +1 ions? (Outcome # 9) (DOK 1) A. strontium, magnesium, calcium B. lithium, sodium, potassium* C. sodium, magnesium, aluminum 39. How many neutrons are in carbon-12? (Outcome # 9) (DOK 1) A. 6* B. 7 C. 8 40. How many neutrons are in chlorine-37? (Outcome # 9) (DOK 1) A. 18 B. 20* C. 18.5 41. Identify the chalcogen that has 18 neutrons in the nucleus. (Outcome # 9) (DOK 2) A. sulfur-32 B. sulfur-33 C. sulfur-34* 42. The chemical symbol for cobalt is _____. (Outcome # 7) (DOK 1) A. Co* B. cO Page 5 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

C. CO 43. What is the chemical symbol for manganese? (Outcome # 7) (DOK 1) A. Mn* B. Mg C. mn 44. Which element is represented by the chemical symbol Th? (Outcome # 7) (DOK 1) A. thallium B. thorium* C. tantalum 45. Which element is represented by the chemical symbol Tl? (Outcome # 7) (DOK 1) A. tantalum B. thallium* C. thorium 46. What is an anion? (Outcome # 7) (DOK 1) A. An anion is defined as an atom that has lost electrons and forms a negative charge.

B. An anion is defined as an atom that has gained electrons and forms a negative charge.* C. An anion is defined as an atom that has gained electrons and forms a positive charge.

47. What is a cation? (Outcome # 7) (DOK 1) A. A cation is defined as an atom that has lost electrons and forms a positive charge.* B. A cation is defined as an atom that has gained electrons and forms a negative charge.

C. A cation is defined as an atom that has gained electrons and forms a positive charge.

48. Hafnium atom is located in which block on the periodic table? (Outcome # 7) (DOK 1) A. p-block B. d-block* C. f-block 49. Lanthanum atom is located in which block on the periodic table? (Outcome # 7) (DOK 1) A. p-block B. d-block C. f-block* 50. Determine the formula for copper(II) nitrate. (Outcome # 8) (DOK 2) A. Cu2NO3 B. CuNO3 C. Cu(NO3)2* 51. What is the name of Fe2O3? (Outcome # 8) (DOK 2) A. iron(II) oxide Page 6 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 02: Atoms, Molecules, and Ions

B. iron(III) oxide* C. iron(IV) oxide 52. What is the correct formula for cobalt(III) chloride? (Outcome # 8) (DOK 2) A. CoCl2 B. CoCl3* C. Co3Cl 53. What is the correct formula for iodine monochloride? (Outcome # 8) (DOK 2) A. ICl2 B. I2Cl C. ICl*

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 03: Composition of Substances and Solutions 1. Which of the following compounds contains the largest number of atoms? (Outcome # 1,2) DOK 2 A. 1.00 mole of NH3 B. 1.00 mole of H2SO4* C. 1.00 mole of HBr 2. What is the molar mass of (NH4)3PO4? (Outcome # 1,2) DOK 2 A. 113 g B. 121 g C. 149 g* 3. What is the mass in grams of 6.022 x 1023 molecules of CO2? (Outcome # 1,2) DOK 3 A. 22 g B. 44 g* C. 66 g 4. What is the total number of atoms contained in 2.00 moles of iron? (Outcome # 1,2) DOK 2 A. 118 B. 6.02 x 1023 C. 1.2 x 1024* 5. What is the molar mass of K2CO3? (Outcome # 1,2) DOK 2 A. 138 g/mol * B. 106 g/mol C. 99 g/mol 6. What is the total number of atoms contained in 1.00 mole of sodium? (Outcome # 1,2,9) DOK 2 A. 118 B. 6.02 x 1023* C. 1.2 x 1024 7. If a hazardous bottle is labeled 20.2 percent by mass Hydrochloric Acid, HCl, with a density of 1.096 g/mL, calculate the molarity of the HCl solution. (Outcome # 1,2,5,8,9,10) (DOK 3) A. 6.07 M* B. 0.22 M C. 14.7 M 8. To dilute a HCl solution from 0.500 M to 0.100 M the final volume must be: (Outcome # 1,2,4,5,8) DOK 2 Page 1 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

A. 1/5 the original volume B. 5 times the original volume* C. 50 L 9. How would you prepare a 1 M solution of sodium hydroxide? (Outcome # 5) (DOK 3) A. add 40.0 grams of sodium hydroxide to 1 L of water* B. add 40.0 grams of sodium hydroxide to 100 L of water C. add 40.0 grams of sodium hydroxide to 10 L of water 10. How would you prepare a 0.5 M solution of sodium hydroxide? (Outcome # 5) (DOK 3) (Paired item 1) A. add 40.0 grams of sodium hydroxide to 1 L of water B. add 20.0 grams of sodium hydroxide to 1 L of water* C. add 20.0 grams of sodium hydroxide to 10 L of water 11. An experiment requires 15.0 mL of a 0.100 M solution of HCl. If you have a 12.0 M HCl stock solution in the laboratory, how would you prepare enough 0.1 M solution to run at least 3 experiments? (Outcome # 5) (DOK 3) A. add 0.833 mL 12 M HCl stock solution to 99.167 mL water* B. add 0.833 mL 12 M HCl stock solution to 49.167 mL water C. add 0.833 mL 12 M HCl stock solution to 199.167 mL water 12. What is the mass in grams of 1.59 moles of aluminum oxide? (Outcome # 2) (DOK 2) A. 162 g* B. 0.0156 g C. 64.1 g 13. What is the mass in grams of 0.852 moles of ferric oxide? (Outcome # 2) (DOK 3) (Paired item 1) A. 5.34 x 10-3 g B. 187 g C. 136 g* 14. How many moles are in 1.77 kg of cuprous sulfate? (Outcome # 2) (DOK 3) A. 7.93 x 10-3 moles B. 7.93 moles* C. 395 moles 15. How many grams are in 2.05 x 1023 molecules of dinitrogen pentoxide? (Outcome # 2) (DOK 3) A. 317 g B. 36.8 g* C. 0.00315 g 16. How many grams are in 1.02 x 1022 molecules of nitric acid? (Outcome # 2) (DOK 3) (Paired item 1) Page 2 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

A. 1.07 g* B. 3720 g C. 2.69 x 10-4 g 17. What is the total number of atoms contained in 2.11 moles of nickel? (Outcome # 2) (DOK 2) A. 2.85 x 1023 atoms B. 1.27 x 1024 atoms* C. 3.50 x 10-24 atoms 18. How many atoms are in 1.00 mole of Au? (Outcome # 2) (DOK 2) (Paired item 1) A. 6.02 x 1023 atoms* B. 1.66 x 10-24 atoms C. 197 atoms 19. A 44.8 g rhodium sample contains how many rhodium atoms? (Outcome # 2) (DOK 3) A. 2.62 x 1023 atoms* B. 6.02 x 1023 atoms C. 2.70 x 1025 atoms 20. What is the molar mass of potassium nitrate? (Outcome # 2) (DOK 2) A. 85.10 g/mol B. 140.20 g/mol C. 101.10 g/mol* 21. Commercial grade fuming nitric acid contains about 90% HNO 3 by mass with a density of 1.50 g/mL, calculate the molarity of the HNO3 solution. (Outcome # 9) (DOK 3) A. 0.214 M B. 21.4 M* C. 2.14 M 22. Which of the following is a method used to allow scientists to determine an empirical formula and identify an organic compound by combusting a sample and the resulting combustion products are quantitatively analyzed? (Outcome # 7) (DOK 1) A. gravimetric analysis B. combustion analysis* C. thermal analysis 23. A 3.00 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 8.80 g of CO2 and 5.40 g of H2O are produced. What is the empirical formula of the unknown? (Outcome # 7) (DOK 3) A. CH3* B. CH C. CH2 Page 3 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

24. A 0.125 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 0.4225 g of CO2 and 0.0865 g of H2O are produced. What is the empirical formula of the unknown? (Outcome # 7) (DOK 3) (Paired item 1) A. CH3 B. CH* C. CH2 25. An unknown organic compound (0.315 g) containing only C, H, and O produces 0.771 of CO 2 and 0.105 g of H2O when it undergoes complete combustion. The approximate molar mass is 108 g/mol. Which of the following compounds could be the identification of the unknown? (Outcome # 7) (DOK 3) A. para-Cresol, CH3C6H4(OH) B. Benzyl alcohol, C6H5CH2OH C. 1,2-Benzoquinone, C6H4O2* 26. Which of the following is an experimental technique used to determine the mass percent of elements found in a compound? (Outcome # 7) (DOK 1) A. gravimetric analysis B. mass analysis C. elemental analysis* 27. An unknown hydrocarbon compound was analyzed for hydrogen by elemental analysis and results show that it contains 15.88 % H. What is the empirical formula? (Outcome # 7) (DOK 2) A. C4H9* B. C8H18 C. C12H27 28. A 5.91 g unknown sample analyzed by elemental analysis revealed a composition of 37.51 % C. In addition, it was determined that the sample contains 1.4830 x 10 23 hydrogen atoms and 1.2966 x 1023 oxygen atoms. What is the empirical formula? (Outcome # 7) (DOK 3) A. C6H8O7* B. C5H6O3 C. C8H16O5 29. What is the concentration in ppm of a 3.7 L solution (d = 1.00 g/mL) containing 4.21 x 10 -7 kg of the pesticide DDT? (Outcome # 8) (DOK 2) A. 1.14 x 10-1 ppm* B. 1.14 x 102 ppm C. 1.14 x 101 ppm 30. When a salt is dissolved in water, it is represented by the following notation in a chemical reaction? (Outcome # 6) (DOK 1) Page 4 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

A. (aq)* B. (l) C. (s) 31. How is a solid phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s)* B. (g) C. (l) 32. How is a liquid phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s) B. (g) C. (l)* 33. How is a gas phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s) B. (g)* C. (l) 34. What are the proper units for molar mass in chemistry? (Outcome # 6) (DOK 1) A. amu B. g/mol* C. g/mmol 35. How many atoms can be found in a mole of mercury? (Outcome # 2) (DOK 2) A. 201 atoms B. 6.02 x 1023 atoms* C. 1.21 x 1026 atoms 36. A 21.8 g sample of water contains how many water molecules? (Outcome # 2) (DOK 3) A. 7.29 x 1023 molecules* B. 6.02 x 1023 molecules C. 2.01 x 10-24 molecules 37. A sample has a molar mass of 143 g/mol, identify the sample. (Outcome # 2) (DOK 1) A. AuCl B. AcCl C. AgCl* 38. What is the molar mass of 2.50 g of an unknown sample dissolved in 130. mL of water with a concentration of 0.480 M? (Outcome # 4) (DOK 3) A. 0.062 g/mol B. 8.65 g/mol C. 40.1 g/mol* 39. 2.50 g of an unknown base is dissolved in 289 mL of water and has a concentration of 0.216 M. What is the identification of the unknown base? (Outcome # 4) (DOK 3) Page 5 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

A. NaOH* B. LiOH C. KOH 40. How many grams of Hydrogen are present in three moles of Hydrogen? (Outcome # 1,5,9) (DOK 1) A. two grams B. six grams* C. one gram 41. Which of the following compounds contains the largest number of atoms? (Outcome # 1,9) (DOK 2) A. 1.00 mole of NH3 B. 1.00 mole of H2SO4* C. 1.00 mole of HBr 42. How many atoms are in 12.8 g of copper metal? (Outcome # 6) (DOK 2) A. 7.71 x 1024 atoms B. 1.21 x 1023 atoms* C. 3.34 x 10-25 atoms 43. How many grams contain 1.45 x 1021 zinc atoms? (Outcome # 6) (DOK 2) A. 1.57 x 10-1 g* B. 5.71 x 1046 g C. 2.41 x 10-3 g 44. How many moles are in 11.0 g of silver metal? (Outcome # 6) (DOK 1) A. 9.81 moles B. 1.19 x 103 moles C. 1.02 x 10-1 moles* 45. What is Avogadro’s number? (Outcome # 6) (DOK 1) A. 6.022 x 1023 particles/mole* B. 6.022 x 1022 particles/mole C. 6.022 x 1024 particles/mole 46. Which of the following 85.0 g samples contain the greatest number of atoms? (Outcome # 6) (DOK 3) A. zinc* B. gold C. zirconium 47. Which of the following 49.5 g samples contain the fewest number of atoms? (Outcome # 6) (DOK 3) (Paired item 1) A. lead* B. platinum Page 6 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 03: Composition of Substances and Solutions

C. iron 48. How many atoms are in 1 mole of calcium? (Outcome # 6) (DOK 1) A. 6.022 x 1023 atoms* B. 6.022 x 10-23 atoms C. 6.022 x 1022 atoms 49. How many moles contain 6.022 x 1023 lithium atoms? (Outcome # 6) (DOK 1) A. 6.022 x 1023 moles B. 1 mole* C. 2 moles

Page 7 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 04: Stoichiometry of Chemical Reactions 1. When Mg(OH)2 reacts with H2SO4 what are the products? (Outcome # 1,2,6) DOK 2 A. Mg(OH)2 and H2SO4 B. MgSO4 and H2O* C. MgO and H2SO4 2. Which of the following is a strong acid? (Outcome # 1,3,5,9) DOK 1 A. HNO3* B. CaSO4 C. NH3 3. Which of the following is a strong acid when mixed in water? (Outcome # 1,2,5) DOK 1 A. HClO B. HBr* C. HNO2 4. What are the products of the reaction between barium hydroxide and hydrogen chloride?

(Outcome # 1,2,5,6,9) DOK 2 A. Barium chloride and water* B. Barium hydroxide and water C. Barium chloride and barium hydride 5. The symbol that separates the reactants from products in a reaction and means “to yield” is ________. (Outcome # 1,5,6,9) DOK 1 A. + B. (s) C. * 6. The chemical reaction CaCO3 CaO + CO2 is classified as a (Outcome # 1,9) DOK 1 A. synthesis reaction B. decomposition reaction* C. single-replacement reaction 7. How many mole ratios can be correctly obtained from the balanced chemical equation DOK 2 (Outcome # 1,2,8,9) 2Al2O3(l)  4Al(s) + 3O2(g)?

A. 3 B. 4 C. 6* Page 1 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

8. Fewer steps are required to solve stoichiometry problems when (Outcome # 1,2) (DOK 2) A. the amount of reactant is given in grams and the product is sought in grams.

B. the amount of reactant is given in moles and the product is sought in moles.* C. the amount reactant is given in grams and the product is sought in liters.

9. Ozone, O3, is a product in automobile exhaust by the reaction represented by the equation NO2(g) + O2(g) NO(g) + O3(g). What mass of ozone is predicted to form from the reaction of 2.0 g NO2 in a car’s exhaust and excess oxygen? (Outcome # 1,2) (DOK 3) A. 1.1 g O3 B. 1.8 g O3 C. 2.1 g O3* 10. A 15.0 g sample of a white, solid substance, is heated in the presence of air. The solid remaining after heating has a mass of 12.6 g. The reaction that took place must have been a/an: (Outcome # 1,2) DOK 3 A. decomposition reaction* B. displacement reaction C. combination reaction 11. When mixing a strong acid and water together, it is recommended that you do which of the following? (Outcome # 5) (DOK 1) A. add water to the strong acid B. add the strong acid to water* C. add them in any order 12. What are the products when reacting potassium hydroxide and hydrogen chloride?

(Outcome # 5) (DOK 2) A. potassium chloride and water* B. potassium hydroxide and water C. no reaction 13. What precipitate forms when mixing copper(II) sulfate and sodium sulfate? (Outcome # 5) (DOK 2) A. copper(I) sulfate B. copper(III) sulfate C. no precipitate forms* 14. What precipitate forms when mixing silver(I) nitrate and sodium chloride? (Outcome # 5) (DOK 2) (Paired item 1) A. silver(I) chloride* B. sodium nitrate C. no precipitate forms 15. What precipitate forms when mixing lead(II) nitrate and sodium iodide? (Outcome # 5) (DOK 2) (Paired item 2) A. sodium nitrate Page 2 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

B. lead(II) iodide* C. no precipitate forms 16. Which of the following reactions are written correctly? (Outcome # 5) (DOK 2) A. H2SO4(aq) + 2 NaOH(aq)  Na2SO4(aq) + 2H2O(l)* B. 2HCl(aq) + K2OH(aq)  2KCl(aq) + H2O(l) C. 2HSO4(aq) + 2NaOH(aq)  2NaSO4(aq) + 2H2O(l) 17. Which of the following reactions are written correctly? (Outcome # 5) (DOK 2) (Paired item 1) A. H2NO3(aq) + 2NaOH(aq)  Na2NO3(aq) + 2H2O(l) B. HNO3(aq) + K2OH(aq)  K2NO3(aq) + H2O(l) C. HNO3(aq) + NaOH(aq)  NaNO3(aq) + H2O(l)* 18. What is the correct name for the precipitate formed when mixing potassium carbonate and nickel(II) chloride? (Outcome # 2) (DOK 2) A. potassium chloride B. nickel(II) carbonate* C. nickel(III) carbonate 19. The reaction HNO3(aq) + NaOH(aq)  NaNO3(aq) + H2O(l) is an example of _____?

(Outcome # 9) (DOK 1) A. an acid-base reaction* B. a combustion reaction C. a precipitation reaction 20. The reaction CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) is an example of _____? (Outcome # 9) (DOK 1) (Paired item 1) A. an acid-base reaction B. a combustion reaction* C. a precipitation reaction 21. Which is the correct balanced reaction for the combustion of octane? (Outcome # 9) (DOK 2) A. 2C8H18(g) + 25O2(g)  16CO2(g) + 18H2O(g)* B. C8H18(g) + 12.5O2(g)  8CO2(g) + 9H2O(g) C. C8H18(g) + 25O(g)  8CO2(g) + 9H2O(g) 22. If 1.50 moles of nitrogen gas reacts with an excess of hydrogen gas, what mass of ammonia would be produced? (Outcome # 9) (DOK 3) A. 34.1 g B. 51.1 g* C. 25.5 g 23. If 250.3 L of hydrogen gas (d = 0.0899 g/L) reacts with an excess of nitrogen gas, what mass of ammonia would be produced? (Outcome # 9) (DOK 3) Page 3 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

A. 253 g B. 380 g C. 127 g* 24. What instrument is used during an acid-base titration experiment to deliver the titrant?

(Outcome # 4) (DOK 1) A. buret* B. syringe C. pipette 25. The combustion of 0.136 kg of methane in the presence of excess oxygen produces 353 g of carbon dioxide. What is the percent yield? (Outcome # 8) (DOK 3) A. 38.5 % B. 94.6 %* C. 0.946 % 26. The combustion of 0.374 kg of methane in the presence of excess oxygen produces 0.983 kg of carbon dioxide. What is the percent yield? (Outcome # 8) (DOK 3) (Paired item 1) A. 38.1 % B. 95.8 %* C. 0.958 % 27. What mass of methane is required to produce 1.130 kg of carbon dioxide during combustion? (Assume the reaction undergoes complete combustion.) (Outcome # 8) (DOK 3) A. 41.18 g B. 0.4118 g C. 411.8 g* 28. The combustion of 0.1240 kg of propane in the presence of excess oxygen produces 0.3110 kg of carbon dioxide. What is the theoretical yield? (Outcome # 8) (DOK 3) A. 371.2 g* B. 0.8377 g C. 0.3712 g 29. Which is the correct balanced reaction for the combustion of octane? (Outcome # 8) (DOK 2) A. 2C8H18(l) + 25O2(g)  16CO2(g) + 18H2O(g)* B. C8H18(l) + 25O(g)  8CO2(g) + 9H2O(g) C. C8H18(l) + 12.5O2(g)  8CO2(g) + 9H2O(g) 30. Which is the correct balanced reaction for the combustion of methane? (Outcome # 8) (DOK 2) (Paired item 1) A. CH4(g) + O2(g)  CO2(g) + H2O(g) B. CH4(g) + 4O(g)  CO2(g) + 2H2O(g) Page 4 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

C. CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)* 31. Write a balanced reaction for the neutralization of HBr upon the addition of KOH. (Outcome # 8) (DOK 2) A. HBr(aq) + KOH(aq)  KBr(aq) + H2O(l)* B. HBr(aq) + KOH(aq)  KBr(s) + H2O(l) C. HBr(aq) + KOH(aq)  KBr(l) + H2O(l) 32. The combustion of 0.296 kg of propane produces 713 g of carbon dioxide. What is the percent yield? (Outcome # 8) (DOK 3) A. 80.5 %* B. 0.805 % C. 124 % 33. 0.450 kg of octane burned during combustion produces 1.25 kg of carbon dioxide. What is the percent yield? (Outcome # 8) (DOK 3) A. 0.901 % B. 90.1 %* C. 36.0 % 34. How many moles of HCl are needed to completely react with 50.0 mL of 0.250 M NaOH solution? (Outcome # 8) (DOK 2) A. 1.25 x 10-2 moles* B. 1.25 x 101 moles C. 2.50 x 10-1 moles 35. How many moles of KOH are needed to neutralize 35.0 mL of 0.115 M HNO 3 solution?

(Outcome # 8) (DOK 2) A. 4.03 x 10-3 moles* B. 4.03 x 101 moles C. 1.15 x 10-1 moles 36. How many moles of NaOH are needed to neutralize 15.0 mL of 0.235 M HCl solution?

(Outcome # 8) (DOK 2) (Paired item 1) A. 3.53 x 101 moles B. 2.35 x 10-1 moles C. 3.53 x 10-3 moles* 37. What is the oxidation number of Cr in a dichromate anion? (Outcome # 8) (DOK 2) A. +6* B. +3 C. +2 38. What is the oxidation number of Mn in a permanganate anion? (Outcome # 8) (DOK 2) A. +4 B. +7* Page 5 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

C. +2 39. How many electrons are transferred during the oxidation of iron metal to form rust?

(Outcome # 8) (DOK 2) A. 3 electrons B. 6 electrons C. 12 electrons* 40. What is the oxidation number of free elements? (Outcome # 8) (DOK 1) A. 0* B. +1 C. +2 41. What is the oxidation number of diatomic elements? (Outcome # 8) (DOK 1) A. 0* B. +1 C. +2 42. What is the oxidation number of hydrogen in H2O2? (Outcome # 8) (DOK 1) A. +2 B. +1* C. 0 43. What is the oxidation number of oxygen in H2O2? (Outcome # 8) (DOK 2) A. -2 B. -1* C. 0 44. What is the net ionic equation for the reaction between CoCl2 and an alkali hydroxide?

(Outcome # 3) (DOK 2) A. Co2+(aq) + 2OH-(aq)  Co(OH)2(s)* B. Na+(aq) + Cl-(aq)  NaCl(s) C. Co3+(aq) + 3OH-(aq)  Co(OH)3(s) 45. Write the net ionic equation for a reaction between a strong acid and strong base.

(Outcome # 3) (DOK 3) A. HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l) B. H+(aq) + OH-(aq)  H2O(l)* C. H2O(l)  H+(aq) + OH-(aq) 46. Identify the reactants in the following reaction: 2 CH3OH(l) + 3 O2(g)  2 CO2(g) + 4 H2O(g) (Outcome # 6) (DOK 1) A. CH3OH B. CH3OH and O2* C. CO2 and H2O Page 6 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

47. If 23.6 g of hydrogen gas reacts with 28.3 g of nitrogen gas, what is the maximum amount of product that can be produced? (Outcome # 6) (DOK 3) A. 34.4 g* B. 133 g C. 68.8 g 48. The catalytic decomposition of hydrogen peroxide occurs with the addition of KI. If 10 mL of a saturated KI solution was added to 315 g of hydrogen peroxide, how much oxygen gas would be produced? (Outcome # 6) (DOK 3) A. 296 g B. 593 g C. 148 g* 49. What is the oxidation number of oxygen gas in the combustion of pentane reaction?

(Outcome # 6) (DOK 3) A. 0* B. -1 C. -2 50. Which is the reducing agent in the combustion of methanol? (Outcome # 6) (DOK 3) A. CH3OH* B. O2 C. CO2 51. Which is the oxidizing agent in the combustion of methanol? (Outcome # 6) (DOK 3) A. CH3OH B. O2* C. CO2 52. Propane is used as a fuel source on many barbeque grills. What is undergoing oxidation during the burning of propane while grilling? (Outcome # 6) (DOK 3) A. CH3CH2CH3* B. O2 C. CO2 53. Propane is used as a fuel source on many barbeque grills. What is undergoing reduction during the burning of propane while grilling? (Outcome # 6) (DOK 3) (Paired item 1) A. CH3CH2CH3 B. O2* C. CO2 54. When a salt is dissolved in water, it is represented by the following notation in a chemical reaction? (Outcome # 6) (DOK 1) A. (aq)* B. (l) Page 7 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

C. (s) 55. How is a solid phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s)* B. (g) C. (l) 56. How is a liquid phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s) B. (g) C. (l)* 57. How is a gas phase represented in a chemical reaction? (Outcome # 6) (DOK 1) A. (s) B. (g)* C. (l) 58. The reaction NH3(aq) + H2O(l)  OH-(aq) + NH4+(aq) is an example of _____? (Outcome # 9) (DOK 1) A. a combustion reaction B. an acid-base reaction* C. a precipitation reaction 59. Which of the following is a strong acid? (Outcome # 1,3,9) (DOK 1) A. HNO3* B. CaSO4 C. NH3 60. Which of the following is a strong acid when mixed in water? (Outcome # 1,5,9) (DOK 2) A. HClO B. HBr* C. HNO2 61. When Ca(OH)2 reacts with H2SO4 what are the products? (Outcome # 1,5,6,9) (DOK 2) A. Ca(OH)2 and H2SO4 B. CaSO4 and H2O* C. CaO and H2SO4 62. What are the products of the reaction between barium hydroxide and hydrogen chloride?

(Outcome # 1,5,6,9) (DOK 2) A. barium chloride and water* B. barium hydroxide and water C. barium chloride and barium hydride 63. The symbol that separates the reactants from products in a reaction and means “to yield” is ________. (Outcome # 1,5,6,9) (DOK 1) A. + Page 8 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

B. (s) C. * 64. The chemical reaction CaCO3 CaO + CO2 is classified as a (Outcome # 1,5,9) (DOK 1) A. synthesis reaction B. decomposition reaction * C. single-replacement reaction 65. What is the correct name for the salt formed between KOH and HCl? (Outcome # 9) (DOK 2) A. potassium hydride B. potassium chloride* C. potassium hydroxide 66. What is the correct formula for the precipitate formed between NaNO 3 and mercury nitrate? (Outcome # 9) (DOK 3) A. Hg2NO3 B. Hg(NO3)2 C. no reaction between NaNO3 and mercury nitrate* 67. Which compound is insoluble in water? (Outcome # 2) (DOK 2) A. CaCO3* B. LiOH C. Na2S 68. In a chemical reaction, the right side of the yield arrow is where the _____ can be found.

(Outcome # 2) (DOK 1) A. reactants B. products* C. both reactant and products 69. The coefficients in front of the substances in a chemical reaction indicate the number of each type of _____. (Outcome # 2) (DOK 1) A. ionic bond B. covalent bond C. molecule* 70. When balancing a chemical reaction, the following may need to be changed? (Outcome # 2) (DOK 1) A. subscripts B. coefficients* C. phases 71. What is the oxidation state of oxygen in H2O2? (Outcome # 2) (DOK 2) A. 0 B. -1* C. -2 Page 9 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

72. Which of the following is a weak acid? (Outcome # 2) (DOK 1) A. acetic acid* B. sulfuric acid C. perchloric acid 73. Which of the following is a weak base? (Outcome # 2) (DOK 1) A. sodium hydroxide B. potassium hydroxide C. ammonia* 74. Hydrogen gas can react with some halogen to produce hydrogen chloride. Write a correct balanced reaction and identify the oxidizing agent. (Outcome # 2) (DOK 3) A. H2(g) + Cl2(g)  2HCl(g) and Cl2 is the oxidizing agent* B. H2(g) + Cl2(g)  2HCl(g) and H2 is the oxidizing agent C. H2(g) + Cl2(g)  2HCl(g) and HCl is the oxidizing agent 75. Which of the following is a redox reaction? (Outcome # 2) (DOK 2) A. Zn(s) + 2 HCl(aq)  ZnCl2(aq) + H2(g)* B. HNO3(aq) + KOH(aq)  KNO3(aq) + H2O(l) C. ZnSO4(aq) + Hg2(NO3)2(aq)  Hg2SO4(s) + Zn(NO3)2(aq) 76. Which of the following is an acid-base reaction? (Outcome # 2) (DOK 2) A. Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g) B. HClO4(aq) + NaOH(aq)  NaClO4(aq) + H2O(l)* C. Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq) 77. Which of the following is a precipitation reaction? (Outcome # 2) (DOK 2) A. Ca(s) + 2HCl(aq)  CaCl2(aq) + H2(g) B. H2SO4(aq) + 2NaOH(aq)  Na2SO4(aq) + 2H2O(l) C. 2NaOH(aq) + MgCl2(aq)  2 NaCl(aq) + Mg(OH)2(s)* 78. Solid potassium chlorate readily decomposes in the presence of a catalyst and heat to form oxygen gas and potassium salt. What is the correct balanced reaction? (Outcome # 5) (DOK 3) A. 2KClO3(s)  2KCl(s) + 3O2(g)* B. KClO4(s)  KCl(s) + 2O2(g) C. KClO3(s)  KCl(s) + 3O(g) 79. Hydrogen peroxide readily decomposes in the presence of a catalyst to form oxygen gas and water. What is the correct balanced reaction? (Outcome # 5) (DOK 3) A. 4HO2(aq)  3O2(g) + 2H2O(l) B. H2O2(aq)  O(g) + H2O(l) C. 2H2O2(aq)  O2(g) + 2H2O(l)* 80. The combustion of propane produced 8.53 g of carbon dioxide. What mass of propane is required if the yield is 93 %. (Outcome # 5) (DOK 3) Page 10 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

A. 3.06 g* B. 9.19 g C. 27.6 g 81. The combustion of butane produced 0.0243 kg of carbon dioxide. What mass of butane is required if the yield is 89 %. (Outcome # 5) (DOK 3) (Paired item 1) A. 36.1 g B. 9.01 g* C. 144.2 g 82. A reaction with an unknown theoretical yield was carried out and the amount of product obtained was a third of the theoretical yield. What is the percent yield? (Outcome # 5) (DOK 3) A. 33.3 %* B. 66.6 % C. cannot be determined 83. A reaction with an unknown percent yield was carried out and the amount of product obtained was a fourth of the theoretical yield. What is the percent yield? (Outcome # 5) (DOK 3) (Paired item 1) A. 75.0 % B. 25.0 %* C. cannot be determined 84. What is the density of a 0.354 M solution of ammonium phosphate? (Outcome # 7) (DOK 3) A. 0.0523 g/mL* B. 5.23 g/mL C. 52.3 g/mL 85. What is the mass of ammonium chloride is 500.0 mL of a 0.198 M solution? (Outcome # 7) (DOK 3) A. 10.6 g B. 5.30 g* C. 5.30 x 103 g 86. How many μL are in 0.239 mL of solvent? (Outcome # 7) (DOK 1) A. 2.39 x 105 μL B. 2.39 x 102 μL* C. 2.39 x 10-5 μL 87. How many grams are in an 81 mg aspirin sample? (Outcome # 7) (DOK 1) A. 0.081 g* B. 0.81 g C. 8.1 g 88. What is the product of hydrogen gas and oxygen gas? (Outcome # 8) (DOK 2) Page 11 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

A. H2O2 B. H2O* C. H3O+ 89. Classify the following type of reaction: Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g). (Outcome # 3) (DOK 1) A. redox reaction* B. combustion reaction C. acid/base reaction 90. Classify the following type of reaction: C3H8(l) + 5O2(g)  3CO2(g) + 4H2O(g). (Outcome # 3) (DOK 1) A. redox reaction B. combustion reaction* C. acid/base reaction 91. Classify the following type of reaction: NaCl(aq) + AgNO3(aq)  AgCl(s) + NaNO3(aq).

(Outcome # 3) (DOK 1) A. redox reaction B. acid/base reaction C. precipitation reaction* 92. Balance the following reaction: CaO + C  CaC2 + CO2. (Outcome # 3) (DOK 1) A. CaO2 + 3C  CaC2 + CO2 B. 2CaO2 + 6C  2CaC2 + 2CO2 C. 2CaO + 5C  2CaC2 + CO2* 93. Ammonia reacts with oxygen in the air. Write a balanced chemical reaction. (Outcome # 3) (DOK 2) A. 4NH3(g) + 5O2(g)  4NO(g) + 6H2O(l)* B. 2NH3(g) + 5O(g)  2NO(g) + 3H2O(l) C. 2NH3(g) + 3O2(g)  2H3NO3(aq) 94. What is the percent yield of a reaction if the product recovered is 89.4 g and the theoretical yield is 128.4 g? (Outcome # 4) (DOK 1) A. 144 % B. 69.6 %* C. 0.696 % 95. What is the percent yield of a reaction if the product recovered is 21.2 g and the theoretical yield is 28.4 g? (Outcome # 4) (DOK 1) (Paired item 1) A. 74.6 %* B. 134 % C. 0.746 % Page 12 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

96. What is the percent yield of a reaction if the actual yield is 80.6 % of the 42.4 g theoretical yield? (Outcome # 4) (DOK 2) A. 34.2 % B. 19.4 % C. 80.6 %* 97. What is the theoretical yield of a reaction if the percent yield 92.4 % and product recovered is 89.3 g? (Outcome # 4) (DOK 2) A. 89.3 g B. 96.6 g* C. 82.5 g 98. What is the limiting reactant in the combustion of 159 g of methane in an open atmosphere? (Outcome # 4) (DOK 1) A. methane* B. oxygen C. carbon dioxide 99. What is the excess reactant in the combustion of 211 g of methane in an open atmosphere?

(Outcome # 4) (DOK 1) A. water B. methane C. oxygen* 100. How many moles are in 1.25 g of calcium chloride? (Outcome # 4) (DOK 1) A. 8.88 x 101 moles B. 1.39 x 102 moles C. 1.13 x 10-2 moles* 101. How many moles are in 4.50 g of Na2SO4? (Outcome # 4) (DOK 1) A. 3.17 x 10-2 moles* B. 6.39 x 102 moles C. 3.16 x 101 moles 102. How many grams are in 12.5 moles of Ba(OH)2? (Outcome # 4) (DOK 1) A. 7.30 x 10-2 g B. 2.14 x 103 g* C. 2.14 x 104 g 103. How many grams are in 2.57 moles of iron oxide? (Outcome # 4) (DOK 2) A. 4.10 x 102 g* B. 6.21 x 101 g C. 1.61 x 10-2 g 104. What is the molar mass of laughing gas, N2O? (Outcome # 4) (DOK 1) A. 46.0 g/mol Page 13 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 04: Stoichiometry of Chemical Reactions

105.

B. 30.0 g/mol C. 44.0 g/mol* What salt is formed between LiOH and HBr? (Outcome # 9) (DOK 1) A. LiBr* B. LiBr2 C. Li2Br

Page 14 of 14

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OpenStax Chemistry Supplemental Test Items Chapter 05: Thermochemistry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 05: Thermochemistry 1. If ΔH = -54.74 kJ for a chemical reaction, that reaction _____________. (Outcome # 1,2) DOK 1 A. is exothermic* B. is endothermic C. cannot occur 2. A _____ is an experimental set-up that can be used to measure the heat of a chemical reaction or a physical change and determine the specific heat capacity of a substance.

(Outcome # 10) (DOK 1) A. manometer B. thermometer C. calorimeter* 3. The following can be used to measure the heat of combustion for an unknown sample?

(Outcome # 10) (DOK 2) A. bomb manometer B. bomb calorimeter* C. coffee-cup calorimeter 4. Coffee-cup calorimetry is carried out at _____. (Outcome # 10) (DOK 1) A. constant-volume B. constant-pressure* C. constant-mass 5. Bomb calorimetry is carried out at _____. (Outcome # 10) (DOK 1) A. constant-volume* B. constant-pressure C. constant-mass 6. You are asked to design an experiment to measure the enthalpy of a given reaction. The reaction needs to be at atmospheric pressure so which of the following techniques would be ideal for this experiment? (Outcome # 10) (DOK 3) A. bomb manometry B. bomb calorimetry C. coffee-cup calorimetry* 7. Your task is to measure the amount of energy evolved during the combustion of some hydrocarbon. Which of the following would be the ideal technique for this experiment?

(Outcome # 10) (DOK 3) Page 1 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 05: Thermochemistry

A. coffee-cup calorimetry B. bomb calorimetry* C. bomb manometry 8. 100 mL of a 0.300 M solution of AgNO3 reacts with 100 mL of a 0.300 M solution of HCl in a coffee-cup calorimeter and the temperature rises from 21.80 °C to 23.20 °C. Assuming the density and specific heat of the resulting solution is 1.00 g/mL and 4.18 J/g ∙ °C, respectfully, what is the ΔH°rxn? (Outcome # 11) (DOK 3) A. -39.0 kJ/mol* B. +39.0 kJ/mol C. +1.17 kJ/mol 9. Given the ∆H°f, calculate the ∆H°rxn for the formation of diamond from graphite. (Outcome # 11) (DOK 2) ∆H°f (C, graphite) = 0 kJ/mol ∆H°f (C, diamond) = 2 kJ/mol A. 0 kJ/mol B. +2 kJ/mol* C. -2 kJ/mol 10. Calculate the ∆H°rxn for the combustion of methane using the given ∆H°f. (Outcome # 11) (DOK 3) ∆H°f, methane(g) = -74.60 kJ/mol ∆H°f, water(l) = -285.8 kJ/mol ∆H°f, carbon dioxide(g) = -393.5 kJ/mol A. -1.04 x 10+3 kJ/mol B. -890.5 kJ/mol* C. 890.5 kJ/mol 11. A drop in water temperature is observed when 0.873 g of ammonium nitrate is added. The enthalpy change for this reaction is +0.280 kJ. Which of the statements is accurate?

(Outcome # 11) (DOK 3) A. The ∆H°soln for ammonium nitrate is +25.7 kJ/mol so this is an endothermic process where energy in the form of heat is absorbed from the surroundings.* B. The ∆H°soln for ammonium nitrate is -25.7 kJ/mol so this is an exothermic process where energy in the form of heat is released into the surroundings.

C. The ∆H°soln for ammonium nitrate is +25.7 kJ/mol so this is an endothermic process where energy in the form of heat is released into the surroundings.

Page 2 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 05: Thermochemistry

12. An increase in water temperature is observed when 1.97 g of NaOH is added. The enthalpy change for this reaction is -2.19 kJ. Which of the statements is accurate? (Outcome # 11) (DOK 3) (Paired item 1) A. The ∆H°soln for NaOH is +44.5 kJ/mol so this is an endothermic process where energy in the form of heat is absorbed from the surroundings.

B. The ∆H°soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is released into the surroundings.* C. The ∆H°soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is absorbed from the surroundings.

13. If ∆H = -73.54 kJ for a chemical reaction, that reaction _____________. (Outcome # 1,5,9) (DOK 2) A. is exothermic* B. is endothermic C. cannot occur 14. A chemical reaction that gives off energy in the form of heat is considered _____. (Outcome # 5) (DOK 2) A. exothermic* B. endothermic C. exergonic 15. A chemical reaction that absorbs energy in the form of heat is considered _____. (Outcome # 5) (DOK 2) (Paired item 1) A. exothermic B. endothermic* C. exergonic 16. A reaction requires a sample to be heated using a water bath near boiling temperature.

Which statement below would be accurate? (Outcome # 5) (DOK 3) A. Boiling water is an endothermic process and to break apart the intermolecular forces that hold together the water molecules requires -40.7 kJ of energy.

B. Boiling water is an exothermic process and to break apart the intermolecular forces that hold together the water molecules requires +40.7 kJ of energy.

C. Boiling water is an endothermic process and to break apart the intermolecular forces that hold together the water molecules requires +40.7 kJ of energy.* 17. A reaction where the products are lower in energy than the reactants is an example of an _____. (Outcome # 6) (DOK 1) A. endothermic process B. exothermic process* C. endergonic process Page 3 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 05: Thermochemistry

18. A reaction where the products are higher in energy than the reactants is an example of an _____. (Outcome # 6) (DOK 1) A. endothermic process* B. exothermic process C. exergonic process 19. An _____ reaction results when the energy required to break bonds in the reactants is greater than the energy released by the formation of products. (Outcome # 3) (DOK 1) A. exergonic B. endothermic* C. exothermic 20. An _____ reaction results when the energy released by the formation of products is greater than the energy required to break the bonds in the reactants. (Outcome # 3) (DOK 1) A. exergonic B. endothermic C. exothermic*

Page 4 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 06: Electronic Structure and Periodic Properties of Elements 1. Provide the element name with a ground-state electron configuration of 1s 22s2p4 (Outcome # 1,5) DOK 1 A. Potassium B. carbon C. oxygen* 2. What is the ground-state electron configuration of calcium? (Outcome # 1,5) DOK 1 A. 1s22s22p63s23p64s2* B. 1s22s22p6 C. 1s22s22p63s2 3. Due to periodicity, which element would you expect to behave most like sodium?

(Outcome # 1,2) DOK 2 A. calcium B. aluminum C. potassium* 4. Which of the following has the longest wavelength? (Outcome # 1,2) DOK 1 A. x rays B. microwaves* C. UV light 5. Elements in group 17 are considered _____________. (Outcome # 1,2) DOK 1 A. alkali Metals B. halogens* C. noble Gases 6. Due to periodicity, which of the following elements has chemical behavior similar to that of Oxygen? (Outcome # 1,2,8) DOK 1 A. bromine B. sulfur* C. carbon 7. Which of the following sets of elements are the most similar to each other? (Outcome # 2) (DOK 1) A. F, Cl, Br, I* B. C, N, O, F C. H, He Page 1 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements

8. According to periodic trends, arrange the following ions, potassium, magnesium, and aluminum in order of increasing ionic size. (Outcome # 2) (DOK 2) A. potassium ion, magnesium ion, and aluminum ion B. aluminum ion, magnesium ion, and potassium ion* C. aluminum ion, potassium ion, and magnesium ion 9. During a UV-Visible spectroscopy experiment, a student notes a wavelength peak measurement at 280 nm. What region of the electromagnetic spectrum was this peak observed? (Outcome # 7) (DOK 1) A. visible region B. ultra-violet region* C. both ultra-violet and visible region 10. During a UV-Visible spectroscopy experiment, a student notes 2 wavelength peak measurements at 580nm and 685nm. What region of the electromagnetic spectrum were these peaks observed? (Outcome # 7) (DOK 1) (Paired item 1) A. visible region* B. ultra-violet region C. both ultra-violet and visible region 11. Provide the element name with a ground-state electron configuration of 1s 22s2p4 (Outcome # 1,7,9) (DOK 1) A. potassium B. carbon C. oxygen* 12. What is the ground-state electron configuration of Calcium? (Outcome # 1,7,9) (DOK 1) A. 1s22s22p63s23p64s2* B. 1s22s22p6 C. 1s22s22p63s2 13. As you move down a group of elements (family), the number of valence electrons (Outcome # 1,9) (DOK 1) A. increases.* B. stays the same.

C. increases and then decreases.

14. Due to periodicity, which element would you expect to behave most like sodium?

(Outcome # 1,9) (DOK 2) A. calcium B. aluminum C. potassium* 15. Which of the following has the longest wavelength? (Outcome # 1,9) (DOK 1) A. x rays Page 2 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements

B. microwaves* C. UV light 16. What is the maximum number of electrons that can occupy the 4th energy level or shell?

(Outcome # 9) (DOK 2) A. 4 B. 16 C. 32* 17. How many subshells are found in the 2nd energy level or shell? (Outcome # 9) (DOK 2) A. 2* B. 4 C. 8 18. What is the maximum number of orbitals found in the 3rd energy level or shell?

(Outcome # 9) (DOK 2) A. 3 B. 9* C. 18 19. Based on the following electron configuration, [Kr]5s24d105p5, this element would most likely _____. (Outcome # 9) (DOK 3) A. gain an electron to form a -1 anion and could form an ionic bond with a metal* B. loss an electron to form a -1 anion and could form an ionic bond with a metal C. gain an electron to form a -1 anion and could form an ionic bond with a nonmetal 20. Based on the following electron configuration, [Xe]6s 2, this element would most likely _____. (Outcome # 9) (DOK 3) (Paired item 1) A. loss 2 electrons to form a +2 cation and could form an ionic bond with a metal B. loss 2 electrons to form a +2 cation and could form an ionic bond with a nonmetal* C. gain 2 electrons to form a +2 cation and could form an ionic bond with a nonmetal 21. Identify the transition metal ion and the number of electrons with the following electron configuration, [Ar]4s03d7. (Outcome # 9) (DOK 3) A. cobalt (I) ion and 25 electrons B. cobalt (II) ion and 25 electrons* C. cobalt (III) ion and 25 electrons 22. UV-Visible spectroscopy can be used to study chromophores such as C=C-C=C which absorb in the UV region of the electromagnetic spectrum ranging from _____. (Outcome # 2) (DOK 2) A. 100 - 300 nm* Page 3 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements

B. 400 - 600 nm C. 600 - 800 nm 23. What is the electron configuration of a copper atom? (Outcome # 7) (DOK 2) A. [Ar]4s23d9 B. [Ar]4s13d10* C. [Ar]4s03d11 24. What is the electron configuration of a copper (II) ion? (Outcome # 7) (DOK 2) A. [Ar]4s23d7 B. [Ar]4s13d8 C. [Ar]3d9* 25. What is the ground-state electron configuration of carbon? (Outcome # 7) (DOK 1) A. 1s22s12p3 B. 1s22s22p2* C. 1s22s32p1 26. In which orbital does an electron add to in chlorine to form an octet? (Outcome # 7) (DOK 2) A. 3s B. 3p* C. 3d 27. What is the ms value for an electron added to bromine to form an octet? (Outcome # 7) (DOK 3) A. +1/2 B. -1/2* C. 0 28. In what block, group, and period on the periodic table can the atom with a 1s22s22p63s23p64s23d104p5 ground-state electron configuration be found? (Outcome # 7) (DOK 3) A. p-block, group 7A, and period 3 B. p-block, group 7A, and period 4* C. p-block, group 7A, and period 5 29. In what block, group, and period on the periodic table can the atom with a 1s 22s22p63s1 ground-state electron configuration be found? (Outcome # 7) (DOK 3) (Paired item 1) A. s-block, group 1A, and period 2 B. s-block, group 1A, and period 3* C. s-block, group 1A, and period 4 30. How many electrons are in the most likely ion formed from an atom located in group 6A and period 3? (Outcome # 7) (DOK 3) A. 16 electrons Page 4 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements

B. 17 electrons C. 18 electrons* 31. How many electrons are in the most likely ion formed from an atom located in group 2A and period 5? (Outcome # 7) (DOK 3) (Paired item 1) A. 36 electrons* B. 38 electrons C. 37 electrons 32. Which of the following sources of radiation is higher in energy? (Outcome # 3) (DOK 1) A. visible light B. ultra violet light* C. infrared light 33. Which of the following sources of radiation has a longer wavelength? (Outcome # 3) (DOK 1) A. visible light B. infrared light* C. ultra violet light 34. 23.1 L of an unknown gas has a mass of 28.85 g at STP. What is the identity of the unknown gas? (Outcome # 4) (DOK 3) (Paired item 1) A. SO2 B. CO* C. NO 35. According to periodic trends, which metal has the lowest ionization energy? (Outcome # 2) (DOK 2) A. Li B. Cs* C. Rb 36. According to periodic trends, which metal has the highest ionization energy? (Outcome # 2) (DOK 2) (Paired item 1) A. Li* B. Cs C. Rb 37. Which nonradioactive group I metal would be the most reactive in water and why?

(Outcome # 2) (DOK 3) A. Cesium would be the most reactive group I metal in water because it has only one valence electron.

B. Cesium would be the most reactive group I metal in water because it’s one valence electron is the closest to the nucleus compared to the other metals.

Page 5 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 06: Electronic Structure and Periodic Properties of Elements

C. Cesium would be the most reactive group I metal in water because it’s one valence electron is the farthest from the nucleus compared to the other metals.* 38. Which of the following elements have a tendency to gain electrons? (Outcome # 9) (DOK 1) A. Cl, O, F* B. N, O, Al C. Cl, F, Ga

Page 6 of 6

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 07: Chemical Bonding and Molecular Geometry 1. According to the octet rule, a magnesium atom has a tendency to (Outcome # 1,2,9) DOK 1 A. lose one electron.

B. lose two electrons.* C. gain one electron.

2. A molecule that has a single covalent bond is _____. (Outcome # 1,2,9) DOK 1 A. CO2 B. CO C. Cl2* 3. A diatomic molecule with a triple covalent bond is _____. (Outcome # 1,2,9) DOK 1 A. O2 B. F2 C. N2 * 4. Which of the following diatomic molecules is joined by a double covalent bond? (Outcome # 1,2,9) DOK 1 A. Cl2 B. O2 * C. N2 5. Which of the following pairs of elements can be joined by a covalent bond? (Outcome # 1,2,9) DOK 1 A. N and C* B. Na and C C. Mg and C 6. Which one of the following elements does not exist as a diatomic molecule in nature?

(Outcome # 1,2,9) DOK 1 A. hydrogen B. nitrogen C. neon* 7. Which of the following is an ionic compound? (Outcome # 1,2) DOK 1 A. CO B. HCl C. Na2O* 8. Which one of these compounds is an ionic compound? (Outcome # 1,2) DOK 1 A. Na2O* Page 1 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

B. CO2 C. N2 9. According to VSEPR theory, the shape of an ammonium ion, NH4+, is most similar to __________. (Outcome # 1,2) DOK 2 A. CH4* B. BH3 C. N2 10. According to periodic trends, which element is the most electronegative? (Outcome # 2) (DOK 1) A. Ne B. O C. F* 11. What is the electron group (EG) and molecular geometry (MG) of an ammonium ion?

(Outcome # 2) (DOK 2) A. (EG) tetrahedral and (MG) tetrahedral* B. (EG) tetrahedral and (MG) trigonal pyramidal C. (EG) tetrahedral and (MG) bent 12. What is the electron group (EG) and molecular geometry (MG) of an ammonia molecule?

(Outcome # 2) (DOK 2) (Paired item 1) A. (EG) tetrahedral and (MG) tetrahedral B. (EG) tetrahedral and (MG) trigonal pyramidal* C. (EG) tetrahedral and (MG) bent 13. According to the octet rule, which of elements will have a tendency to loss 2 electrons?

(Outcome # 9) (DOK 1) A. strontium* B. oxygen C. cesium 14. Which of the following molecules has the greatest bond energy? (Outcome # 9) (DOK 2) A. H2 B. N2* C. O2 15. What type of bond will typically form between boron and hydrogen based on their electronegativity? (Outcome # 9) (DOK 2) A. metallic B. ionic C. covalent* 16. Based off periodic trends, which of the following has the strongest lattice energy? (Outcome # 9) (DOK 3) Page 2 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

A. aluminum chloride* B. calcium chloride C. sodium chloride 17. Construct the molecule IF5 using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles of the equatorial fluorine’s in the structure?

(Outcome # 12) (DOK 3) A. 90°* B. 120° C. 109.5° 18. Construct the molecule IF5 and PF5 using a molecular modeling software such as Spartan or 3D-ChemDraw. How do the molecular shapes differ? (Outcome # 12) (DOK 3) A. In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on phosphorus. As a result, the molecular shape of IF5 is square pyramidal and PF5 is trigonal bipyramidal.* B. In PF5 there is a lone pair of electrons on phosphorus where as in IF5 there are no lone pairs on iodine. As a result, the molecular shape of PF5 is square pyramidal and IF5 is trigonal bipyramidal.

C. In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on phosphorus. As a result, the molecular shape of IF5 is octahedral and PF5 is trigonal bipyramidal.

19. Construct the molecule PF5 using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles of the equatorial fluorine’s in the structure?

(Outcome # 12) (DOK 3) A. 90° B. 120°* C. 109.5° 20. Construct the molecule PF5 using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles of the axial fluorine’s in the structure? (Outcome # 12) (DOK 3) A. 90°* B. 120° C. 109.5° 21. Using VSEPR theory, predict the molecule shape of a molecule that contains 2 electron groups. (Outcome # 12) (DOK 1) A. trigonal planar B. linear* C. bent Page 3 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

22. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond angles in a molecule that contains 4 electron groups (3 bonds and 1 lone pair electrons).

(Outcome # 12) (DOK 2) A. tetrahedral, trigonal pyramidal, >109.5° B. tetrahedral, trigonal pyramidal, <109.5°* C. tetrahedral, trigonal pyramidal, 109.5° 23. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond angles in a molecule that contains 5 electron groups (2 bonds and 3 lone pair electrons).

(Outcome # 12) (DOK 2) (Paired item 1) A. trigonal bipyramidal, linear, 180°* B. trigonal bipyramidal, trigonal bipyramidal, 90° and 120° C. trigonal bipyramidal, trigonal bipyramidal, 180° 24. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond angles in a molecule that contains 6 electron groups (5 bonds and 1 lone pair electrons).

(Outcome # 12) (DOK 2) (Paired item 2) A. octahedral, octahedral, 90° B. octahedral, square planar, 90° C. octahedral, square pyramidal, 90°* 25. Using VSEPR theory, predict the molecular shape and bond angles in BCl3. (Outcome # 12) (DOK 2) A. trigonal planer, 120°* B. trigonal pyramidal, 120° C. trigonal bent, 120° 26. Construct the molecule H2O using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles in the structure? (Outcome # 12) (DOK 2) A. 104.5°* B. 107° C. 109.5° 27. Construct the molecule NH3 using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles in the structure? (Outcome # 12) (DOK 2) A. 104.5° B. 107°* C. 109.5° 28. Construct the molecule CH4 using a molecular modeling software such as Spartan or 3DChemDraw. What are the bond angles in the structure? (Outcome # 12) (DOK 2) A. 104.5° B. 107° C. 109.5°* Page 4 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

29. The bond angles in CH4, NH3, and H2O are 109.5°, 107°, and 104.5°, respectfully. Which of the statements best describes the variance in bond angles? (Outcome # 12) (DOK 3) A. CH4 has no lone pairs of electrons on the central atom so the optimal molecular shape would be tetrahedral with bond angles of 109.5°. In NH3 and H2O there are 1 and 2 lone pairs, respectfully, so more repulsion exists between the bonds and lone pairs, as a result, the bond angles are less than 109.5°.* B. NH3 and H2O have a trigonal pyramidal and bent molecular shape, respectfully, which is the reason why the bond angles are less than 109.5°.

C. CH4 only has nonpolar bonds while NH3 and H2O have polar bonds which results in the difference in bond angels.

30. Based off the following data, what is the lattice energy of sodium chloride? (Outcome # 11) (DOK 2) ΔHsub of Na = 108 kJ/mol Do of Cl2 = 243 kJ/mol IE of Na(g) = 496 kJ/mol EA of Cl(g) = -349 kJ/mol ΔHf of NaCl = -411 kJ/mol A. -1490 kJ/mol B. -909 kJ/mol C. -788 kJ/mol* 31. In an ionic bond, the charge on the cation (i.e. the metal) is (Outcome # 1,7,9) (DOK 1) A. always positive.* B. always negative.

C. either positive or negative.

32. According to the octet rule, a magnesium atom has a tendency to (Outcome # 1,9) (Dok 2) A. lose one electron.

B. lose two electrons.* C. gain one electron.

33. A covalent bond is formed when two atoms (Outcome # 1,9) (DOK 2) A. share an electron with each other.

B. share one or more pairs of electrons with each other.* C. gain electrons.

34. According to the octet rule, a bromine atom has a tendency to (Outcome # 1,9) (DOK 2) A. lose one electron.

B. lose two electrons.

C. gain one electron.* 35. The halogens have how many valence electrons? (Outcome # 1,9) (DOK 1) Page 5 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

A. 4 B. 6 C. 7* 36. How many electrons are shared in a single covalent bond? (Outcome # 1,9) (DOK 1) A. 2* B. 3 C. 1 37. How many electrons are shared in a double covalent bond? (Outcome # 1,9) (DOK 1) A. 3 B. 4* C. 2 38. A molecule that has a single covalent bond is _____. (Outcome # 1,9) (DOK 1) A. CO2 B. CO C. Cl2* 39. A diatomic molecule with a triple covalent bond is _____. (Outcome # 1,9) (DOK 2) A. O2 B. F2 C. N2 * 40. Which of the following diatomic molecules is joined by a double covalent bond? (Outcome # 1,9) (DOK 2) A. Cl2 B. O2 * C. N2 41. Which of the following pairs of elements can be joined by a covalent bond? (Outcome # 1,9) (DOK 2) A. N and C* B. Na and C C. Mg and C 42. _____ is a diatomic molecule that has a double covalent bond. (Outcome # 9) (DOK 2) A. Br2 B. I2 C. O2* 43. Which element contains triple covalent bonds? (Outcome # 9) (DOK 1) A. oxygen B. nitrogen* C. iodine 44. What is the molecular shape of CO2? (Outcome # 9) (DOK 1) Page 6 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

A. linear* B. bent C. trigonal planar 45. How many polar bonds does CH4 contain? (Outcome # 9) (DOK 1) A. 0* B. 2 C. 4 46. Which molecule has only covalent bonds? (Outcome # 9) (DOK 1) A. CO2* B. Al2O3 C. Mg3N2 47. Which compound has only ionic bonds? (Outcome # 9) (DOK 1) (Paired item 1) A. CO2 B. Al2O3* C. H2O2 48. The octet rule states that main group elements in the periodic table react to achieve a filled valence shell which consists of how many electrons? (Outcome # 9) (DOK 1) A. 2 B. 4 C. 8* 49. What is the molecular shape and polarity for xenon tetrafluoride? (Outcome # 9) (DOK 3) A. square-planar and polar B. square-planar and non-polar* C. tetrahedral and non-polar 50. Which of the following elements are found in the p-block and can form an octet? (Outcome # 7) (DOK 1) A. He, P, S, As B. P, S, O, C* C. He, Ar, Kr, Ne 51. Based off molecular polarity determined by VSEPR theory, which of the following would be soluble in methanol? (Outcome # 8) (DOK 3) A. heptane B. ethanol* C. pentane 52. Based off molecular polarity determined by VSEPR theory, which of the following would be insoluble in CCl4? (Outcome # 8) (DOK 3) A. methanol* B. octane Page 7 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

C. hexane 53. Based off molecular polarity determined by VSEPR theory, in which solvent would NaCl be the most soluble? (Outcome # 8) (DOK 3) A. CH3OH B. CH3CH2OH C. H2O* 54. Based off molecular polarity determined by VSEPR theory, in which solvent would glucose be the least soluble? (Outcome # 8) (DOK 3) A. CH3CH2OCH2CH3* B. CH3OH C. H2O 55. Which statement best describes a bond forming between fluorine and iodine? (Outcome # 8) (DOK 3) A. fluorine and iodine are in the same group so the electron density in the bond is equaling shared giving rise to a non-polar bond B. fluorine is more electronegative than iodine so it will attract the electron density in the bond giving rise to a polar bond* C. fluorine is less electronegative than iodine so it will attract the electron density in the bond giving rise to a polar bond 56. Why are detergents and soaps good at cleaning up oily stains from dishes or clothing?

(Outcome # 8) (DOK 3) 1. Detergents and soaps work well to clean up oily messes because they are amphiphilic in nature so they contain both hydrophilic (polar) and hydrophobic (nonpolar) ends. The hydrophobic end attaches to oils via hydrogen bonds creating micelles which leave the hydrophilic part exposed and can be washed away by water.

2. Detergents and soaps work well to clean up oily messes because they are amphiphilic in nature so they contain both hydrophilic (non-polar) and hydrophobic (polar) ends. The hydrophobic end attaches to oils via London forces creating micelles which leave the hydrophilic part exposed and can be washed away by water.

3. Detergents and soaps work well to clean up oily messes because they are amphiphilic in nature so they contain both hydrophilic (polar) and hydrophobic (nonpolar) ends. The hydrophobic end attaches to oils via London forces creating micelles which leave the hydrophilic part exposed and can be washed away by water.* 57. Is it true that a molecule with polar bonds will always be polar? (Outcome # 8) (DOK 2) A. that is false, molecular polarity is determined by molecular shape* B. that is true, molecular polarity is determined by bond polarity only Page 8 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 07: Chemical Bonding and Molecular Geometry

C. that is false, molecular polarity is determined by electron group geometry 58. An _____ reaction results when the energy required to break bonds in the reactants is greater than the energy released by the formation of products. (Outcome # 3) (DOK 1) A. exergonic B. endothermic* C. exothermic 59. An _____ reaction results when the energy released by the formation of products is greater than the energy required to break the bonds in the reactants. (Outcome # 3) (DOK 1) A. exergonic B. endothermic C. exothermic* 60. How many non-polar bonds does CH3OH contain? (Outcome # 9) (DOK 1) A. 2 B. 3* C. 4 61. How many polar bonds does CCl4 have in its structure? (Outcome # 9) (DOK 1) A. 0 B. 2 C. 4*

Page 9 of 9

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OpenStax Chemistry Supplemental Test Items Chapter 08: Advanced Theories of Covalent Bonding Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 08: Advanced Theories of Covalent Bonding 1. Based on valence bond theory, which statement best describes the electron geometry, bonding and hybridization of the central atom in carbon tetrachloride? (Outcome # 12) (DOK 3) A. The electron geometry of carbon in carbon tetrachloride is tetrahedral with a sp 3 hybridization. The C-Cl bond is of σ-character.* B. The electron geometry of carbon in carbon tetrachloride is tetrahedral with a sp 2 hybridization. The C-Cl bond is of σ-character.

C. The electron geometry of carbon in carbon tetrachloride is tetrahedral with a sp 3 hybridization. The C-Cl bond is of π-character.

2. Based on valence bond theory, which statement best describes the electron geometry and hybridization of the central atom(s) in acetylene? (Outcome # 12) (DOK 2) A. The electron geometry of the 2 carbons in acetylene is tetrahedral with a sp 3 hybridization.

B. The electron geometry of the 2 carbons in acetylene is trigonal planar with a sp 2 hybridization.

C. The electron geometry of the 2 carbons in acetylene is linear with a sp hybridization.* 3. Which statement best describe the structure of a carbonate anion? (Outcome # 12) (DOK 3) A. The electron geometry of carbon in a carbonate anion is trigonal planar with a sp 2 hybridization and bond angles are 120°. There is a π-bond formed between a nonhybridized “C” p-orbital overlapping with an “O” p-orbital.* B. The electron geometry of carbon in a carbonate anion is trigonal planar with a sp 2 hybridization and bond angles are <120°. There is a π-bond formed between a nonhybridized “C” p-orbital overlapping with an “O” p-orbital.* C. The electron geometry of carbon in a carbonate anion is trigonal planar with a sp 2 hybridization and bond angles are <120°. There is a π-bond formed between a hybridized “C” p-orbital overlapping with an “O” p-orbital.* 4. Based on valence bond theory, what is the hybridization of the central atom(s) in C 2F4?

(Outcome # 12) (DOK 1) A. both carbons are sp2* B. both carbons are sp3 C. one carbon is sp3 and the other carbon is sp2 5. Which element contains triple covalent bonds? (Outcome # 9) (DOK 1) Page 1 of 2

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OpenStax Chemistry Supplemental Test Items Chapter 08: Advanced Theories of Covalent Bonding

A. oxygen B. nitrogen* C. iodine

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OpenStax Chemistry Supplemental Test Items Chapter 09: Gases Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 09: Gases 1. On a very cold day, you notice that your tires look a bit deflated than warmer days. This observation can be explained by _____. (Outcome # 8) (DOK 2) A. Boyles law B. Ideal gas law C. Charles law* 2. What is the relationship between pressure and volume of a gas at constant temperature?

(Outcome # 8) (DOK 2) A. as volume decreases, pressure increases* B. as volume decreases, pressure decreases C. as volume increases, pressure increases 3. How many mm Hg are in 0.890 atm of pressure? (Outcome # 8) (DOK 1) A. 854 mm Hg B. 676 mm Hg* C. 1.17 x 10-3 mm Hg 4. How many atmospheres are in 710 mm Hg? (Outcome # 8) (DOK 1) A. 0.934 atm* B. 1.07 atm C. 5.40 x 105 atm 5. The average tire pressure for an automobile is 38.5 psi which is how many atmospheres of pressure? (Outcome # 8) (DOK 1) A. 1.77 x 10-3 atm B. 566 atm C. 2.62 atm* 6. What is the volume for 1.00 mole of gas at STP? (Outcome # 3) (DOK 2) A. 24.5 L B. 22.4 L* C. 2.05 L 7. What is the standard pressure for 1.00 mole of gas at STP? (Outcome # 3) (DOK 2) A. 760 mm Hg* B. 1.03 atm C. 103 kPa 8. 286 L of hydrogen gas at STP reacts with excess chorine gas. What is the maximum amount of gas product that can be formed at STP? (Outcome # 3) (DOK 3) Page 1 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 09: Gases

A. 572 L* B. 143 L C. 286 L 9. 159 L of hydrogen gas at STP reacts with excess chorine gas. What is the maximum amount of gas product that can be formed at STP? (Outcome # 3) (DOK 3) (Paired item 1) A. 159 L B. 79.5 L C. 318 L* 10. A _____ is an instrument used to measure atmospheric pressure specifically in the area of meteorology. (Outcome # 10) (DOK 1) A. barometer* B. manometer C. altimeter 11. A _____ is a general instrument that utilizes a liquid column, typically mercury, to measure pressure. (Outcome # 10) (DOK 1) A. barometer B. manometer* C. altimeter 12. How many psi are in 760. mm Hg? (Outcome # 7) (DOK 1) A. 1.47 x 101 psi* B. 3.93 x 104 psi C. 2.54 x 10-5 psi 13. A sample of nitrogen gas occupies 9.20 L at 21 °C and 0.959 atm. If the pressure is increased to 1.15 atm at constant temperature, what is the newly occupied volume? (Outcome # 6) (DOK 1) A. 11.0 L B. 7.67 L* C. 9.20 L 14. The pressure of a gas in a container is 1.85 atm and occupies a volume of 12.5 L. If the original volume is reduced by half at constant temperature, what would happen to the pressure? (Outcome # 6) (DOK 2) A. the pressure would double* B. the pressure would reduce by half C. the pressure would remain the same 15. The pressure of a gas in a container is 1.23 atm and occupies a volume of 1.5 L. If the original volume is doubled at constant temperature, what would happen to the pressure?

(Outcome # 6) (DOK 2) A. the pressure would remain the same Page 2 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 09: Gases

B. the pressure would double C. the pressure would reduce by half* 16. Suppose your car is equipped with tire pressure monitoring system (TPMS) and the tire pressure is 34.0 psi on a 98 °F day in California. You decided to take a road trip to Alaska where the temperature drops to 20 °F. As you arrived in Alaska, you noticed that the tire pressure monitoring system alert light is illuminated. Why did this happen? (Outcome # 6) (DOK 3) A. as temperature decreases, gas molecules lose kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated* B. as temperature decreases, gas molecules gain kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated C. as temperature decreases, gas molecules lose kinetic energy and the volume of gas increases thus reducing the overall pressure in the tire which results in the TPMS to become activated 17. On a hot summer day, you notice that a bag of chips left in your vehicle has inflated. Why did this happen? (Outcome # 6) (DOK 3) A. as temperature increases, gas molecules gain kinetic energy and the volume of gas decreases inside the bag of chips B. as temperature increases, gas molecules lose kinetic energy and the volume of gas increases inside the bag of chips C. as temperature increases, gas molecules gain kinetic energy and the volume of gas increases inside the bag of chips* 18. What mass of nitrogen is needed to fill an 855 L tank at STP? (Outcome # 6) (DOK 3) A. 0.978 kg B. 1.07 kg* C. 0.533 kg 19. What mass of oxygen is needed to fill a 585 L tank at STP? (Outcome # 6) (DOK 3) (Paired item 1) A. 0.835 kg* B. 0.765 kg C. 0.417 kg 20. What is the pressure in a 5.80 L container that has 0.545 moles of oxygen gas at 22.0 °C? (Outcome # 6) (DOK 1) A. 0.170 atm B. 2.28 atm* C. 231 atm Page 3 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 09: Gases

21. What is the pressure in a 3.41 L container that has 0.741 moles of oxygen gas at 26.0 °C? (Outcome # 6) (DOK 1) (Paired item 1) A. 5.34 atm* B. 0.464 atm C. 62.0 atm 22. How many moles of CO2 gas are present in a 9.1 L container at 25 °C and 1.35 atm?

(Outcome # 6) (DOK 1) A. 4.96 x 10-3 moles B. 5.99 moles C. 0.502 moles* 23. Oxygen gas (PO2 = 1.10 atm), nitrogen gas (PN2 = 0.840 atm), and carbon dioxide gas (PCO2 = 0.125 atm) occupy the same container. What is the total pressure in the container?

(Outcome # 6) (DOK 1) A. 2.07 atm* B. 1.94 atm C. 0.135 atm 24. A container filled with neon and argon gas is 25.00% by volume neon. What is the partial pressure of argon if the total pressure inside the container is 5.500 atm? (Outcome # 6) (DOK 2) A. 412.5 atm B. 1.375 atm C. 4.125 atm* 25. A container filled with helium and argon gas is 8.00% by volume argon. What is the partial pressure of argon if the total pressure inside the container is 4.100 atm? (Outcome # 6) (DOK 2) (Paired item 1) A. 0.328 atm* B. 3.77 atm C. 32.8 atm 26. What is the temperature for STP conditions? (Outcome # 4) (DOK 1) A. 273.15 K* B. 298.15 K C. 0 K 27. What is the pressure for STP conditions? (Outcome # 4) (DOK 1) A. 740 mm Hg B. 780 mm Hg C. 760 mm Hg* 28. 28.5 L of an unknown gas has a mass of 55.92 g at STP. What is the identity of the unknown gas? (Outcome # 4) (DOK 3) Page 4 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 09: Gases

A. CO2* B. O2 C. N2

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OpenStax Chemistry Supplemental Test Items Chapter 10: Liquids and Solids Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 10: Liquids and Solids 1. Which statement accurately depicts what happens to water on the molecular level in a tea pot when it begins to boil? (Outcome # 9) (DOK 3) A. The molecules begin to move farther apart decreasing their intermolecular forces and they escape the liquid state to enter the gas state.* B. The molecules begin to move closer together overcoming their intermolecular forces which holds them together and they escape the liquid state to enter the gas state.

C. The molecules begin to move farther apart decreasing their intramolecular forces and they escape the liquid state to enter the gas state.

2. At what temperature does water boil in kelvin? (Outcome # 7) (DOK 1) A. 373.15 K* B. 273.15 K C. 173.15 K 3. Which phases change is an exothermic process? (Outcome # 8) (DOK 1) A. freezing* B. melting C. evaporation 4. Which phases change is an endothermic process? (Outcome # 8) (DOK 1) A. freezing B. evaporation* C. deposition 5. Water changing from ice to a liquid is an example of _____. (Outcome # 8) (DOK 1) A. melting* B. evaporation C. freezing 6. Sodium chloride changing from a solid to a gas is an example of _____. (Outcome # 8) (DOK 1) A. evaporation B. sublimation* C. boiling 7. What predominate intermolecular force is in HCl? (Outcome # 8) (DOK 1) A. dipole-dipole* B. hydrogen bonding C. London forces Page 1 of 3

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OpenStax Chemistry Supplemental Test Items Chapter 10: Liquids and Solids

8. What predominate intermolecular force is in NH3? (Outcome # 8) (DOK 1) (Paired item 1) A. dipole-dipole B. hydrogen bonding* C. London forces 9. What predominate intermolecular force is in CO2? (Outcome # 8) (DOK 1) (Paired item 2) A. dipole-dipole B. hydrogen bonding C. London forces* 10. What predominate intermolecular force is in CH3OH? (Outcome # 8) (DOK 1) (Paired item 3) A. dipole-dipole B. hydrogen bonding* C. London forces 11. What predominate intermolecular force is in CH3CH2CH3? (Outcome # 8) (DOK 1) (Paired item 4) A. dipole-dipole B. hydrogen bonding C. London forces* 12. Based off of the principles of intermolecular forces, which liquid has a higher vapor pressure? (Outcome # 8) (DOK 2) A. water B. methanol C. ethyl ether* 13. Based off of the principles of intermolecular forces, which liquid has the lowest vapor pressure? (Outcome # 8) (DOK 2) (Paired item 1) A. water* B. ethanol C. ethyl ether 14. If it takes you 10 min. to boil an egg to perfection at sea level, how long would it take to boil an egg to your taste in the Carpathian Mountains at elevations of 8,500 ft? (Outcome # 8) (DOK 3) A. The boiling point of water in the Carpathian Mountains is less than 100 °C because of lower atmospheric pressure which results in reduced intermolecular forces, so it would take a longer time to boil the egg.* B. The boiling point of water in the Carpathian Mountains is greater than 100 °C because of lower atmospheric pressure which results in increased intermolecular forces, so it would take less time to boil the egg.

C. The boiling point of water is always 100 °C regardless of elevation so it would take the same amount of time to boil the egg.

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OpenStax Chemistry Supplemental Test Items Chapter 10: Liquids and Solids

15. Which alkane would have a higher boiling point? (Outcome # 8) (DOK 1) A. heptane* B. ethane C. pentane 16. Which alkane would have a lower boiling point? (Outcome # 8) (DOK 1) A. CH3CH3 B. CH4* C. CH3CH2CH3 17. Which of the following halogens would have stronger intermolecular forces? (Outcome # 8) (DOK 1) A. Br2 B. Cl2 C. I2* 18. Which of the following molecules would have weaker intermolecular forces? (Outcome # 8) (DOK 1) A. I2* B. NH3 C. H2O

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OpenStax Chemistry Supplemental Test Items Chapter 11: Solutions and Colloids Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 11: Solutions and Colloids 1. Based off the molecular polarity of water, which of the following molecules would be soluble in water? (Outcome # 4) (DOK 2) A. glucose, methanol, and ethanol* B. carbon dioxide, methane, methanol C. glucose, carbon dioxide, ethanol 2. Which of the following would be a strong electrolyte in solution? (Outcome # 6) (DOK 2) A. PbI2 B. KCl* C. Al(OH)3 3. Which of the following would be a weak electrolyte in solution? (Outcome # 6) (DOK 2) A. acetic acid* B. sulfuric acid C. hydroiodic acid 4. Which of the following when dissolved in deionized water would make a poor conducting solution? (Outcome # 6) (DOK 2) A. baking soda B. sugar* C. salt 5. Which of the following when dissolved in deionized water would make a good conducting solution? (Outcome # 6) (DOK 2) (Paired item 1) A. methanol B. sugar C. baking soda* 6. For an experiment, you are asked to prepare a 2 m strong electrolytic solution. Which of the following salts would you use? (Outcome # 6) (DOK 3) A. an alkali salt* B. an alkaline salt C. either an alkali or an alkaline salt 7. Which of the following substances would be a poor choice for making conductive solutions?

(Outcome # 6) (DOK 3) A. C6H12O6, CH3OH, CH3CH2OH* B. HCl, KBr, HNO3 C. NaOH, KOH, LiOH Page 1 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 11: Solutions and Colloids

8. Which of the following would be soluble in water? (Outcome # 9) (DOK 2) A. sugar, NaCl, HCl* B. sugar, NaOH, ethane C. sugar, HNO3, methane 9. How would you purify salt water so that it becomes potable? (Outcome # 2) (DOK 1) A. gravity filtration B. vacuum filtration C. distillation* 10. Which of the following would conduct electricity? (Outcome # 2) (DOK 3) A. solid NaCl B. NaCl solution* C. both solid NaCl and a NaCl solution 11. At what temperature does salt water freeze? (Outcome # 7) (DOK 1) A. 0 °C B. below 0 °C* C. above 0 °C 12. If you want to boil a pot of water containing salt, at what temperature would boiling begin?

(Outcome # 7) (DOK 1) A. 100 °C B. below 100 °C C. above 100 °C* 13. What happens to the freezing point of water when ethylene glycol is added? (Outcome # 8) (DOK 2) A. Ethylene glycol has no effect on the freezing point of water.

B. Ethylene glycol will interfere with the organization of water molecules during the freezing process therefore increasing the freezing point of water.

C. Ethylene glycol will interfere with the organization of water molecules during the freezing process therefore reducing the freezing point of water.* 14. Which of the following is a colligative property? (Outcome # 8) (DOK 1) A. boiling-point elevation* B. temperature of a solution C. color of a solution 15. Which of the following is a not a colligative property? (Outcome # 8) (DOK 1) (Paired item 1) A. boiling-point elevation B. temperature of a solution* C. Freezing-point depression 16. Assuming all the salts below are the same concentration, which salt would lower the freezing point of water the most? (Outcome # 8) (DOK 1) Page 2 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 11: Solutions and Colloids

A. NaCl B. KBr C. CaCl2* 17. Which salt would lower the freezing point of a solvent the most? (Outcome # 8) (DOK 2) A. 1.5m NaCl B. 0.5m CaCl2 C. 1.25m Na2SO4* 18. What would be the best method for raising the boiling point of water in a kettle by a few degrees Celsius? (Outcome # 8) (DOK 3) A. increase the temperature of the stove B. add some table salt to the water* C. increase the temperature of the stove and increase the surface area by transferring the water to a larger kettle 19. What would be the best method for lowering the freezing point of water in an ice tray that is in the freezer? (Outcome # 8) (DOK 3) A. decrease the temperature of the freezer B. decrease the temperature of the freezer and increase the surface area by transferring the water to a larger ice tray C. add some table salt to the water* 20. Patients who enter the emergency room dehydrated are usually given sterile saline solution intravenously. The solution administered is isotonic to prevent cell damage. What would happen if the solution was hypotonic? (Outcome # 6) (DOK 3) A. Hypotonic solutions have a higher osmotic pressure than that within cells so hemolysis can occur.

B. Hypotonic solutions have a lower osmotic pressure than that within cells so hemolysis can occur.* C. Hypotonic solutions have the same osmotic pressure as that within cells so hemolysis can occur.

21. Patients who enter the emergency room dehydrated are usually given sterile saline solution intravenously. The solution administered is isotonic to prevent cell damage. What would happen if the solution was hypertonic? (Outcome # 6) (DOK 3) (Paired item 1) A. Hypertonic solutions have the same osmotic pressure as that within cells so crenation can occur.

B. Hypertonic solutions have a lower osmotic pressure than that within cells so crenation can occur.

C. Hypertonic solutions have a higher osmotic pressure than that within cells so crenation can occur.* Page 3 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 11: Solutions and Colloids

22. Which type of solution has a lower osmotic pressure than that within cells? (Outcome # 6) (DOK 1) A. hypertonic B. hypotonic* C. isotonic 23. Which type of solution has a higher osmotic pressure than that within cells? (Outcome # 6) (DOK 1) A. isotonic B. hypertonic* C. hypotonic 24. Which type of solution has the same osmotic pressure as that within cells? (Outcome # 6) (DOK 1) A. hypertonic B. isotonic* C. hypotonic 25. What is the osmolarity of a 2 M NaCl solution? (Outcome # 6) (DOK 1) A. 2 osmol B. 6 osmol C. 4 osmol* 26. A KCl solution is 0.500 M. What is the osmolarity? (Outcome # 6) (DOK 1) (Paired item 1) A. 1 osmol* B. 2 osmol C. 4 osmol 27. 45.8 g of NaCl is dissolved in 500. mL of a water (d = 1.00 g/mL) and is placed in the freezer at -1 °C overnight. Which statement best describes what would happen to the solution?

(Outcome # 3) (DOK 3) A. The freezing point of the NaCl solution would be -5.83 °C, so the solution would not freeze.* B. The freezing point of the NaCl solution would be 5.83 °C, so the solution would freeze.

C. The freezing point of the NaCl solution would be -2.92 °C, so the solution would not freeze.

28. 17.1 g of calcium chloride is dissolved in 750. mL of a water (d = 1.00 g/mL) and is placed in the freezer at -2 °C overnight. Which statement best describes what would happen to the solution? (Outcome # 3) (DOK 3) (Paired item 1) A. The freezing point of the calcium chloride solution would be 1.15 °C, so the solution would freeze.

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OpenStax Chemistry Supplemental Test Items Chapter 11: Solutions and Colloids

B. The freezing point of the calcium chloride solution would be -1.15 °C, so the solution would freeze.* C. The freezing point of the calcium chloride solution would be -0.382 °C, so the solution would freeze.

29. How would you be able to increase the boiling point of water on a hotplate? (Outcome # 3) (DOK 2) A. increase the temperature of the hotplate B. add less water and increase the temperature of the hotplate C. add some NaCl to the water* 30. How would you increase the concentration of a 1 M NaCl solution? (Outcome # 3) (DOK 1) A. decant some of the solution down the sink B. bring the solution to near boiling until desired volume is achieved* C. decrease the temperature of the salt solution to near freezing 31. The solubility of NaCH3CO2 in water is ~1.23 g/mL. What would be the best method for preparing a supersaturated NaCH3CO2 solution? (Outcome # 3) (DOK 2) A. add 130 g of NaCH3CO2 to 100 mL of H2O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature* B. add 123 g of NaCH3CO2 to 200 mL of H2O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature C. add 130 g of NaCH3CO2 to 100 mL of H2O at room temperature while stirring until all the solid dissolves 32. The solubility of KCl in water is ~344 g/L. What would be the best method for preparing a 100 mL saturated KCl solution? (Outcome # 3) (DOK 2) A. add 38.0 g of KCl to 100 mL of H2O at room temperature while stirring* B. add 30.0 g of KCl to 100 mL of H2O at room temperature while stirring C. add 34.0 g of KCl to 100 mL of H2O at room temperature while stirring

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OpenStax Chemistry Supplemental Test Items Chapter 12: Kinetics Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 12: Kinetics 1. _____ energy is the minimum amount of energy that colliding molecules must possess in order for a chemical reaction to occur. (Outcome # 6) (DOK 1) A. activation* B. bond C. collision 2. A reaction where the products are lower in energy than the reactants is an example of an _____. (Outcome # 6) (DOK 1) A. endothermic process B. exothermic process* C. endergonic process 3. A reaction where the products are higher in energy than the reactants is an example of an _____. (Outcome # 6) (DOK 1) A. endothermic process* B. exothermic process C. exergonic process 4. Which of the following affects the rate of a reaction? (Outcome # 6) (DOK 1) A. concentration, temperature, nature of reactants, presence of solvents B. concentration, temperature, molecular size, presence of catalysts C. concentration, temperature, nature of reactants, presence of catalysts* 5. What affect does temperature have on the rate of a reaction? (Outcome # 6) (DOK 2) A. the lower the temperature, the lower the kinetic energy which results in more effective collisions therefore increasing the rate of a reaction B. the higher the temperature, the greater the kinetic energy which results in more effective collisions therefore increasing the rate of a reaction* C. the higher the temperature, the greater the kinetic energy which results in more effective collisions therefore decreasing the rate of a reaction 6. Which statement best describes the effect of concentration on the rate of a reaction?

(Outcome # 6) (DOK 2) A. higher concentrations result in more effective collisions therefore increasing the rate of a reaction* B. higher concentrations result in less effective collisions therefore increasing the rate of a reaction Page 1 of 2

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OpenStax Chemistry Supplemental Test Items Chapter 12: Kinetics

C. higher concentrations result in more collisions therefore increasing the rate of a reaction* 7. What is the overall rate order of a reaction A + B  C which has the following rate equation: rate = k[A][B]? (Outcome # 4) (DOK 1) A. 2* B. 1 C. 0 8. What is the rate order with respect to [A] in the reaction A + B  C which has following rate equation: rate = k[B]? (Outcome # 4) (DOK 1) A. 2 B. 1 C. 0* 9. What is the rate order with respect to [B] in the reaction A + B  C which has following rate equation: rate = k[B]? (Outcome # 4) (DOK 1) A. 2 B. 1* C. 0 10. What is the rate equation of a reaction A + B  C which has a first-rate order for [A] and zero-rate order for [B]? (Outcome # 4) (DOK 2) A. rate = k[A]* B. rate = k[A][B] C. rate = k[B]

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OpenStax Chemistry Supplemental Test Items Chapter 13: Fundamental Equilibrium Concepts Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 13: Fundamental Equilibrium Concepts 1. Consider the following equilibrium mixture in a closed system: H 2O(g) + CO(g) ⇌ H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas?

(Outcome # 3) (DOK 3) A. The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved.* B. The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right which would result in more CO2 being produced until equilibrium is achieved.

C. The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen.

2. Consider the following equilibrium mixture in a closed system: H 2O(g) + CO(g) ⇌ H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of carbon monoxide gas? (Outcome # 3) (DOK 3) A. The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved.

B. The addition of carbon monoxide gas would not disrupt the equilibrium, so nothing would happen.

C. The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the right which would result in more products being produced until equilibrium is achieved.* 3. Write the equilibrium expression for H2O(g) + CO(g) ⇌ H2(g) + CO2(g). (Outcome # 3) (DOK 1) A. Kc = [CO2] [H2] / [H2O] [CO]* B. Kc = [H2O] [CO] / [CO2] [H2] C. Kc = [CO2] [H2] / [CO] 4. Write the equilibrium expression for 2NO(g) + 2H2(g) ⇌ N2(g) + 2H2O(g). (Outcome # 3) (DOK 1) A. Kc = [NO]2 [H2]2 / [H2O]2 [N2] B. Kc = [H2O]2 [N2] / [NO]2 [H2]2* C. Kc = [N2] / [NO]2 [H2]2 Page 1 of 2

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OpenStax Chemistry Supplemental Test Items Chapter 13: Fundamental Equilibrium Concepts

5. The Kc for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I2, and H2 are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct?

(Outcome # 4) (DOK 2) A. Q = 5.15 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium* B. Q = 15.2 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium C. Q = 0.194 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium 6. If the reaction quotient is greater than the equilibrium constant, which statement would be correct? (Outcome # 4) (DOK 1) A. If Q > K, then the reaction needs to proceed towards the right to reach equilibrium.

B. If Q > K, then the reaction needs to proceed towards the left to reach equilibrium.* C. If Q > K, then the reaction is at equilibrium.

7. If the reaction quotient is less than the equilibrium constant, which statement would be correct? (Outcome # 4) (DOK 1) A. If Q < K, then the reaction needs to proceed towards the left to reach equilibrium.

B. If Q < K, then the reaction is at equilibrium.

C. If Q < K, then the reaction needs to proceed towards the right to reach equi librium.*

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 14: Acid-Base Equilibria 1. Which of the following is an electronic device used to measure the hydrogen ion activity in aqueous solutions? (Outcome # 7) (DOK 1) A. pH meter* B. potentiometer C. ammeter 2. Which of the following is a typical type of electrode found on a pH meter? (Outcome # 7) (DOK 1) A. gold electrode B. glass electrode* C. silver electrode 3. When titrating a weak acid with a strong base, approximately where would the pH be observed when reaching the equivalence point? (Outcome # 4) (DOK 2) A. at the equivalence point, the pH is greater than 7* B. at the equivalence point, the pH is equal to 7 C. at the equivalence point, the pH is less than 7 4. When titrating a weak base with a strong acid, approximately where would the pH be observed when reaching the equivalence point? (Outcome # 4) (DOK 2) (Paired item 1) A. at the equivalence point, the pH is greater than 7 B. at the equivalence point, the pH is equal to 7 C. at the equivalence point, the pH is less than 7* 5. When titrating a strong acid with a strong base, approximately where would the pH be observed when reaching the equivalence point? (Outcome # 4) (DOK 2) (Paired item 2) A. at the equivalence point, the pH is greater than 7 B. at the equivalence point, the pH is equal to 7* C. at the equivalence point, the pH is less than 7 6. What are the products formed at the equivalence point when titrating a strong acid with a strong base? (Outcome # 4) (DOK 2) A. salt and water* B. the solution is neutral, so water only C. no products are formed 7. Phenolphthalein can be used as an _____ in acid-base titrations. (Outcome # 4) (DOK 1) A. equivalence point B. end-point Page 1 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

C. indicator* 8. Phenolphthalein can be used as an indicator in acid-base titrations. When a few drops are added to an acidic solution which is then titrated with a strong base, the color of the solution changes from _____ to _____. (Outcome # 4) (DOK 1) A. colorless; pink* B. pink; colorless C. colorless; red 9. When blue litmus paper is in contact with an acid, the litmus paper will turn _____.

(Outcome # 4) (DOK 1) A. orange B. red* C. green 10. When red litmus paper is in contact with a base, the litmus paper will turn _____.

(Outcome # 4) (DOK 1) (Paired item 1) A. orange B. green C. blue* 11. Which of the following is a diprotic acid? (Outcome # 3) (DOK 1) A. H3PO4 B. H2PO4-* C. HPO4212. Which of the following is an amphiprotic substance? (Outcome # 3) (DOK 1) A. H3PO4 B. PO43C. HPO42-* 13. What is the conjugate base that is formed when carbonic acid is dissolved in water?

(Outcome # 3) (DOK 2) A. H3O+ B. HCO3-* C. CO3214. When phosphoric acid is dissolved in water, what is the conjugate acid that is formed?

(Outcome # 3) (DOK 2) A. H2PO4B. H3O+* C. HPO4215. What is the conjugate base that is formed upon the addition of carbonic acid to water?

(Outcome # 3) (DOK 2) A. HCO3-* Page 2 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

B. H3O+ C. CO3216. Rank the following oxyanions in order of increasing basicity: ClO 4-, ClO2-, ClO-, ClO3-.

(Outcome # 3) (DOK 2) A. ClO4-, ClO-, ClO2-, ClO3B. ClO-, ClO2-, ClO3-, ClO4C. ClO4-, ClO3-, ClO2-, ClO-* 17. Rank the following oxoacids in order of increasing acidity: HClO 2, HClO4, HClO, HClO3.

(Outcome # 3) (DOK 2) A. HClO, HClO2, HClO3, HClO4* B. HClO4, HClO2, HClO, HClO3 C. HClO4, HClO3, HClO2, HClO 18. What is the pH of a solution if 10 mL of a 1 M HCl solution is added to 10 mL of a 1 M NaOH solution? (Outcome # 10) (DOK 2) A. 14 B. 7* C. 0 19. If 10 mL of a 1 M HI solution is added to 5 mL of a 1 M KOH solution, the resulting solution would be _____. (Outcome # 10) (DOK 2) A. acidic* B. basic C. neutral 20. If 3 mL of a 0.5 M HBr solution is added to 20 mL of a 0.5 M NaOH solution, the resulting solution would be _____. (Outcome # 10) (DOK 2) (Paired item 1) A. acidic B. basic* C. neutral 21. What is the hydronium concentration of a solution at pH 7? (Outcome # 10) (DOK 1) A. 1 x 10+7 M B. 1 x 10-14 M C. 1 x 10-7 M* 22. A student titrates 50.0 mL of an unknown concentration of HI with 85 mL of a 1.0 M solution of NaOH to reach the equivalence point. What is the pH of the HI solution?

(Outcome # 10) (DOK 3) A. -0.23* B. 0.23 C. 1.7 Page 3 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

23. A student titrates a 25 mL of an unknown concentration of HCl with 35 mL of a 0.890 M solution of KOH to reach the equivalence point. What is the pH of the HCl solution?

(Outcome # 10) (DOK 3) (Paired item 1) A. -0.10* B. 0.10 C. 1.2 24. A student discovers a bottle of a highly corrosive monoprotic acid with the label partially destroyed. How can the concentration of the unknown acid be determined without using a pH meter? (Outcome # 10) (DOK 3) A. The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The moles of OH- added would be equal to moles of H+ in the unknown at the half-way point, therefore, the concentration of the unknown can be calculated.

B. The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The moles of OH- added would be equal to moles of H+ in the unknown at the equivalence point, therefore, the concentration of the unknown can be calculated.* C. The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The pH at the equivalence point should be 7 since this is a neutralization reaction, therefore, the concentration of the unknown acid is 1 x 10-7 M. 25. A student discovers a bottle of NaOH with a partially destroyed label. How can the concentration be determined without using a pH meter? (Outcome # 10) (DOK 3) A. The student can set-up a titration experiment, where a standardized HCl solution is used to titrate the NaOH. The moles of H+ and OH- are equal at the equivalence point, therefore, the concentration of NaOH can be calculated.* B. The student can set-up a titration experiment, where a standardized HCl solution is used to titrate the NaOH. The pH at the equivalence point should be 7 since this is a neutralization reaction, therefore, the concentration of NaOH is 1 x 10 -7 M. C. The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate HCl. The moles of H+ and OH- are equal at the equivalence point, therefore, the concentration of NaOH can be calculated.

26. What is the pH of 0.048 M solution of hydrochloric acid? (Outcome # 7) (DOK 1) A. 0.32 B. 4.8 C. 1.3* Page 4 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

27. What is the pH of 0.014 M solution of hydroiodic acid? (Outcome # 7) (DOK 1) (Paired item 1) A. 1.4 B. 1.9* C. 0.85 28. What is the pH of deionized water? (Outcome # 7) (DOK 1) A. pH = 7* B. pH < 7 C. pH > 7 29. What is the pH of 0.48 M HCl solution? (Outcome # 2) (DOK 1) A. 0.32* B. -0.32 C. 13.68 30. What is the pH of 8.1 x 10-5 M HClO4 solution? (Outcome # 2) (DOK 1) (Paired item 1) A. 9.91 B. 4.09* C. -4.09 31. What is the hydroxide ion concentration for a 23 % (m/v) HNO3 solution? (Outcome # 2) (DOK 3) A. 10.35 M B. 3.65 M C. 2.74 x 10-15 M* 32. Blood is considered a buffered solution. What is the pH range of blood? (Outcome # 2) (DOK 1) A. 7.35 - 7.45* B. 6.35 - 6.45 C. 8.35 - 8.45 33. What instrument can be used to measure the hydrogen ion concentration in solutions?

(Outcome # 2) (DOK 1) A. ammeter B. pH meter* C. potentiometer 34. Which acid has a lower pH? (Outcome # 5) (DOK 2) A. 1.0 M acetic acid* B. 0.50 M acetic acid C. 0.25 M acetic acid 35. Which acid has a higher hydrogen ion concentration? (Outcome # 5) (DOK 2) A. 1.0 M HCl Page 5 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

B. 0.050 M HNO3 C. 1.25 M HBr* 36. What is the base in the following reaction: HCl (aq) + H 2O (l)  Cl- (aq) + H3O+ (aq)?

(Outcome # 5) (DOK 2) A. ClB. H3O+ C. H2O* 37. What is the conjugate acid in the following reaction: HCl (aq) + H2O (l)  Cl- (aq) + H3O+ (aq)? (Outcome # 5) (DOK 2) A. ClB. H3O+* C. H2O 38. What is the conjugate base in the following reaction: HCl (aq) + H 2O (l)  Cl- (aq) + H3O+ (aq)? (Outcome # 5) (DOK 2) (Paired item 1) A. Cl-* B. H3O+ C. H2O 39. What is the conjugate base of HSO4-? (Outcome # 5) (DOK 2) A. H2SO4 B. SO42-* C. SO440. What is the conjugate acid of HSO4-? (Outcome # 5) (DOK 2) A. H2SO4* B. SO42C. H2SO441. Write the equilibrium expression for the autoionization of water. (Outcome # 3) (DOK 3) A. Kw = [H3O+] [OH-] / [H2O]2 B. Kw = [H3O+] [OH-]* C. Kw = [H2O]2 / [H3O+] [OH-] 42. What is the pOH of a solution that has a pH of 7? (Outcome # 2) (DOK 1) A. 7* B. 14 C. 0 43. What is the pOH of a solution that has a pH of 2? (Outcome # 2) (DOK 1) (Paired item 1) A. 12* B. 7 C. 14 44. Which acid has the lowest hydroxide ion concentration? (Outcome # 5) (DOK 2) Page 6 of 7

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OpenStax Chemistry Supplemental Test Items Chapter 14: Acid-Base Equilibria

A. 0.010 M HCl B. 0.050 M HNO3* C. 0.015 M HBr* 45. What is the conjugate base in the following reaction: HI (aq) + H2O (l)  I- (aq) + H3O+ (aq)? (Outcome # 5) (DOK 2) A. I-* B. H3O+ C. H2O 46. What is the acid in the following reaction: NH3 (aq) + H2O (l)  NH4+ (aq) + OH- (aq)?

(Outcome # 5) (DOK 2) A. NH3 B. NH4+ C. H2O*

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OpenStax Chemistry Supplemental Test Items Chapter 15: Equilibria of Other Reaction Classes Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 15: Equilibria of Other Reaction Classes [No items]

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OpenStax Chemistry Supplemental Test Items Chapter 16: Thermodynamics Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 16: Thermodynamics 1. At what temperature are the standard Gibbs free energy of formations reported? (Outcome # 11) (DOK 1) A. 20.0 °C B. 0 °C C. 25.0 °C* 2. What is the ∆G° if ∆H° is +58.7 kJ and ∆S° is +129 J/K? (Outcome # 11) (DOK 1) A. +20.2 kJ* B. -20.2 kJ C. +55.5 kJ 3. What is the ∆G° if ∆H° is +72.7 kJ and ∆S° is +112 J/K? (Outcome # 11) (DOK 1) (Paired item 1) A. -39.3 kJ B. +39.3 kJ* C. +70.0 kJ 4. What is the ∆S° if the ∆H° is +88.00 kJ and ∆G ° is +11.21 kJ? (Outcome # 11) (DOK 1) A. -258 J B. +258 J* C. +0.258 J 5. What is the ∆S° if the ∆H° is +48.90 kJ and ∆G ° is +19.01 kJ? (Outcome # 11) (DOK 1) (Paired item 1) A. -0.1003 J B. +0.1003 J C. +100.3 J* 6. An _____ reaction is a nonspontaneous reaction in which the standard change in free energy is positive. (Outcome # 3) (DOK 1) A. exergonic B. endergonic* C. exothermic 7. An _____ reaction is a spontaneous reaction in which the standard change in free energy is negative. (Outcome # 3) (DOK 1) A. exergonic* B. endergonic C. exothermic Page 1 of 1

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OpenStax Chemistry Supplemental Test Items Chapter 17: Electrochemistry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 17: Electrochemistry 1. Write a balanced redox reaction for the formation of rust on iron metal and identify the correct oxidizing agent and/or reducing agent. (Outcome # 6) (DOK 3) A. Iron is the oxidizing agent and O2 is neither a reducing agent nor an oxidizing agent B. Iron is the oxidizing agent and O2 is the reducing agent C. Iron is the reducing agent and O2 is the oxidizing agent* 2. Which is the reducing agent in the combustion of methanol? (Outcome # 6) (DOK 3) A. CH3OH* B. O2 C. CO2 3. Which is the oxidizing agent in the combustion of methanol? (Outcome # 6) (DOK 3) A. CH3OH B. O2* C. CO2 4. Propane is used as a fuel source on many barbeque grills. What is undergoing oxidation during the burning of propane while grilling? (Outcome # 6) (DOK 3) A. CH3CH2CH3* B. O2 C. CO2 5. Propane is used as a fuel source on many barbeque grills. What is undergoing reduction during the burning of propane while grilling? (Outcome # 6) (DOK 3) (Paired item 1) A. CH3CH2CH3 B. O2* C. CO2 6. Automobiles from northern states tend to show more signs of rust formation than southern states. The reason for this is that the rate of corrosion is affected by _____, which is more common during winter months especially in northern states. (Outcome # 6) (DOK 1) A. the cold air and clouds B. rain clouds C. snow, ice, and salt mixtures* 7. Certain anaerobic organisms such as methanogens have the ability to metabolize carbon dioxide into methane in the presence of hydrogen. Methane is produced by the oxidation of _____? (Outcome # 6) (DOK 3) A. H2* Page 1 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 17: Electrochemistry

B. CO2 C. CH4 8. A voltaic cell must be split into two separate cells, an oxidation and reduction half-cells. The two half-cells must be connected by a _____ so ions can freely flow between the two halfcells to balance the charges or the voltaic cell cannot function. (Outcome # 10) (DOK 2) A. metallic wire B. salt bridge* C. membrane 9. In a voltaic cell, oxidation occurs at the _____. (Outcome # 10) (DOK 1) A. anode terminal* B. cathode terminal C. positive terminal 10. In a voltaic cell, reduction occurs at the _____. (Outcome # 10) (DOK 1) A. anode terminal B. cathode terminal* C. negative terminal 11. Electron flow in a voltaic cell is always from _____ to _____. (Outcome # 10) (DOK 2) A. anode to cathode* B. cathode to anode C. anode to negative terminal 12. The following can be used as an electrolyte for a salt bridge in a voltaic cell? (Outcome # 10) (DOK 1) A. KNO3(aq)* B. H2O(l) C. CH3OH(l) 13. The following can be used as an electrolyte for a salt bridge in a voltaic cell? (Outcome # 10) (DOK 1) (Paired item 1) A. CCl4(l) B. CH3CH2OH(l) C. Na2SO4(aq)* 14. In a voltaic cell, electrons are produced at the _____. (Outcome # 10) (DOK 1) A. positive terminal B. anode terminal* C. cathode terminal 15. The anode terminal in a voltaic cell is the _____ terminal. (Outcome # 10) (DOK 1) A. (-)* B. (+) C. Neutral Page 2 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 17: Electrochemistry

16. The cathode terminal in a voltaic cell is the _____ terminal. (Outcome # 10) (DOK 1) A. (-) B. (+)* C. neutral 17. In a voltaic cell, electrons are received at the _____. (Outcome # 10) (DOK 1) A. cathode terminal* B. negative terminal C. anode terminal 18. Based on the reduction potential data, what is the standard cell potential for the following electrochemical cell reaction: Zn(s) + Cu2+(aq)  Zn2+(aq) + Cu(s)? (Outcome # 11) (DOK 2) E°red = -0.763 V for Zn2+(aq) + 2e-  Zn(s) E°red = +0.340 V for Cu2+(aq) + 2e-  Cu(s) A. +1.103 V* B. -0.423 V C. +0.423 V 19. Based on the reduction potential data, what is the standard cell potential for the following electrochemical cell reaction: Cu(s) + 2Ag+  Cu2+(aq) + 2Ag(s)? (Outcome # 11) (DOK 2) (Paired item 1) E°red = +0.800 V for Ag+(aq) + e-  Ag(s) E°red = +0.340 V for Cu2+(aq) + 2e-  Cu(s) A. +1.14 V B. +0.460 V* C. +1.26 V 20. Based on the following reduction potential data, which is the strongest reducing agent?

(Outcome # 11) (DOK 1) E°red = +1.78 V for H2O2(aq) + 2H+(aq) + 2e-  2H2O(l) E°red = +0.800 V for Ag+(aq) + e-  Ag(s) E°red = -0.130 V for Pb2+(aq) + 2e-  Pb(s) A. Pb(s)* B. Ag(s) C. H2O(l) Page 3 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 17: Electrochemistry

21. Based on the following reduction potential data, which is the strongest oxidizing agent?

(Outcome # 11) (DOK 1) E°red = +1.78 V for H2O2(aq) + 2H+(aq) + 2e-  2H2O(l) E°red = +0.800 V for Ag+(aq) + e-  Ag(s) E°red = -0.130 V for Pb2+(aq) + 2e-  Pb(s) A. Pb2+(aq) B. H2O2(aq)* C. Ag+(aq) 22. The standard cell potential is +0.460 V for the following electrochemical cell reaction: Cu(s) + 2Ag+(aq)  Cu2+(aq) + 2Ag(s). What is the ∆G°rxn? (Outcome # 11) (DOK 2) A. -88.8 kJ/mol* B. -44.4 kJ/mol C. +44.4 kJ/mol 23. What is the ∆G°rxn for a 2 electron transfer electrochemical cell with a standard cell potential of +0.770 V. (Outcome # 11) (DOK 2) A. -74.3 kJ/mol B. -149 kJ/mol* C. +74.3 kJ/mol 24. Based on the following reduction potential data, what is the ∆G° rxn for the following electrochemical cell reaction: Zn(s) + Cu2+(aq)  Zn2+(aq) + Cu(s)? (Outcome # 11) (DOK 3) E°red = -0.763 V for Zn2+(aq) + 2e-  Zn(s) E°red = +0.340 V for Cu2+(aq) + 2e-  Cu(s) A. +106 kJ/mol B. -106 kJ/mol C. -213 kJ/mol* 25. Which of the following acids is a strong oxidant? (Outcome # 5) (DOK 1) A. HCl B. HNO3* C. HI 26. Which strong acid is commonly used in automobile batteries? (Outcome # 2) (DOK 2) A. HCl B. H2SO4* C. HNO3 Page 4 of 5

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OpenStax Chemistry Supplemental Test Items Chapter 17: Electrochemistry

27. Cell phones batteries are typically rechargeable. How do they differ from non-rechargeable batteries? (Outcome # 2) (DOK 3) A. A rechargeable battery has the ability to undergo a double replacement reaction while non-rechargeable batteries do not. Therefore, the forward direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.

B. A rechargeable battery has the ability to undergo a reversible redox reaction while non-rechargeable batteries do not. Therefore, the forward direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.* C. A rechargeable battery has the ability to undergo a redox reaction while nonrechargeable batteries do not. Therefore, the reverse direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.

28. The process of corrosion involves what type of reaction? (Outcome # 2) (DOK 2) A. double displacement reaction B. acid-base reaction C. redox reaction* 29. What is the oxidation state of oxygen in K2O2? (Outcome # 2) (DOK 2) A. 0 B. -1* C. -2 30. Which of the following is a strong oxidizing agent? (Outcome # 2) (DOK 2) A. N2 B. O2* C. H2

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OpenStax Chemistry Supplemental Test Items Chapter 18: Representative Metals, Metalloids, and Nonmetals Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 18: Representative Metals, Metalloids, and Nonmetals 1. What is one of the primary components in our atmosphere that leads to acidic rain?

(Outcome # 5) (DOK 1) A. SO B. SO2* C. both SO and SO2 2. Which of the following gases are flammable? (Outcome # 5) (DOK 1) A. helium B. hydrogen* C. nitrogen 3. Which of the following gases are considered inert? (Outcome # 5) (DOK 1) (Paired item 1) A. oxygen B. hydrogen C. nitrogen* 4. Which one of the following elements does not exist as a diatomic molecule in nature?

(Outcome # 1,9) (DOK 2) A. hydrogen B. nitrogen C. neon* 5. Which diatomic element is considered an inert gas? (Outcome # 9) (DOK 1) A. H2 B. N2* C. F2 6. What is the active ingredient in most solid antacids? (Outcome # 2) (DOK 2) A. CaCO3* B. Ca(OH)2 C. KOH 7. Which of the following are considered toxic heavy metals? (Outcome # 5) (DOK 2) A. lead, cadmium, and mercury* B. lead, iron, and mercury C. arsenic, mercury, and calcium 8. What compound does magnesium and nitrogen form? (Outcome # 8) (DOK 1) A. Mg3N2* B. Mg2N3 Page 1 of 2

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OpenStax Chemistry Supplemental Test Items Chapter 18: Representative Metals, Metalloids, and Nonmetals

C. MgN

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OpenStax Chemistry Supplemental Test Items Chapter 19: Transition Metals and Coordination Chemistry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 19: Transition Metals and Coordination Chemistry [No items]

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OpenStax Chemistry Supplemental Test Items Chapter 20: Organic Chemistry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 20: Organic Chemistry

1. What is the molar mass of isopropyl alcohol? (Outcome # 4) (DOK 2) A. 60.1 g/mol* B. 32.0 g/mol C. 46.1 g/mol

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OpenStax Chemistry Supplemental Test Items Chapter 21: Nuclear Chemistry Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 21: Nuclear Chemistry 1. Which of the following is emitted by radioactive nuclei and contains two protons and two neutrons? (Outcome # 3) (DOK 1) A. alpha particles* B. beta particles C. gamma rays 2. Which of the following is emitted by radioactive nuclei and is a type of high energy radiation that does not contain mass or charge? (Outcome # 3) (DOK 1) A. alpha particles B. beta particles C. gamma rays* 3. Which of the following is emitted by radioactive nuclei and has a mass and charge that is identical to an electron? (Outcome # 3) (DOK 1) A. alpha particles B. beta particles* C. gamma rays 4. Gamma Ray Emission is represented by which symbol? (Outcome # 3) (DOK 1) A. β B. α C. γ* 5. Beta particle emission is represented by which symbol? (Outcome # 3) (DOK 1) A. β* B. α C. γ 6. Alpha particle emission is represented by which symbol? (Outcome # 3) (DOK 1) A. β B. α* C. γ 7. Which of the following sources of radiation is higher in energy? (Outcome # 3) (DOK 1) A. visible light B. ultra violet light* C. infrared light 8. Which of the following sources of radiation has a longer wavelength? (Outcome # 3) (DOK 1) A. visible light Page 1 of 4

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OpenStax Chemistry Supplemental Test Items Chapter 21: Nuclear Chemistry

B. infrared light* C. ultra violet light 9. Which is an example of nonionizing radiation? (Outcome # 3) (DOK 1) A. radiowaves* B. x-rays C. cosmic rays 10. Which is an example of ionizing radiation? (Outcome # 3) (DOK 1) A. radiowaves B. infrared light C. cosmic rays* 11. Which is an example of ionizing radiation? (Outcome # 3) (DOK 1) (Clone 1) A. ultra violet light* B. visible light C. infrared light 12. What is nonionizing radiation? (Outcome # 3) (DOK 1) A. radiation that does not have a sufficient amount of energy to remove an electron from an atom or molecule* B. radiation that has sufficient amount of energy to remove an electron from an atom or molecule C. radiation that does not have a sufficient amount of energy to gain an electron from an atom or molecule 13. What is ionizing radiation? (Outcome # 3) (DOK 1) A. radiation that does not have a sufficient amount of energy to remove an electron from an atom or molecule B. radiation that has sufficient amount of energy to gain an electron from an atom or molecule C. radiation that has sufficient amount of energy to remove an electron from an atom or molecule* 14. Which type of radiation has sufficient energy to penetrate into organs, tissue, and bone?

(Outcome # 3) (DOK 2) A. gamma radiation* B. alpha radiation C. beta radiation 15. Which type of radiation has insufficient energy and cannot penetrate the outer layers of human skin? (Outcome # 3) (DOK 2) A. gamma radiation B. alpha radiation* C. beta radiation Page 2 of 4

Credit: Modification of assessment items provided by Lumen Learning, with generous funding from the William and Flora Hewlett Foundation. Licensed Creative Commons Attribution 4.0.

OpenStax Chemistry Supplemental Test Items Chapter 21: Nuclear Chemistry

16. Which is a type of nuclear reaction where two small nuclei are merged together to generate a larger nuclei and a tremendous amount of energy? (Outcome # 3) (DOK 1) A. nuclear fission B. nuclear fusion* C. neutron scattering 17. Which is a type of nuclear reaction where a large nucleus splits into two smaller nuclei with the release of a large amount of energy?(Outcome # 3) (DOK 1) A. neutron scattering B. nuclear fusion C. nuclear fission* 18. Through what process does the sun generate its energy? (Outcome # 3) (DOK 1) A. nuclear fusion* B. nuclear fission C. neutron scattering 19. _____ is an instrument used to measure levels of ionizing radiation. (Outcome # 3) (DOK 1) A. radio counter B. Geiger counter* C. radiation counter 20. Technetium-99m is commonly used as a medical radioisotope in numerous medical diagnostic procedures yearly. The half-life of technetium-99m is 6.00 hours. After 1 day, a medical sample was found to contain 0.05 grams of technetium-99m. How many grams of technetium-99m were present initially? (Outcome # 3) (DOK 3) A. 0.8 g* B. 0.2 g C. 0.1 g 21. Before the use of technetium-99m, patients with high risk coronary artery disease were evaluated using thallium-201 which has a half-life of 73.00 hours. If a person is exposed to 5.000 μg of thallium-201, how many hours would it take to reach 10.00 % of its original mass? (Outcome # 3) (DOK 3) A. 3.322 hours B. 242.5 hours* C. 21.98 hours 22. How much of a 0.230 g radioactive sample with a half-life of 8 hours would remain after a period of 2.50 days? (Outcome # 3) (DOK 3) A. 8.98 x 10-4 g B. 1.80 x 10-3 g C. 1.27 x 10-3 g* Page 3 of 4

Credit: Modification of assessment items provided by Lumen Learning, with generous funding from the William and Flora Hewlett Foundation. Licensed Creative Commons Attribution 4.0.

OpenStax Chemistry Supplemental Test Items Chapter 21: Nuclear Chemistry

23. What is the half-life of a radioactive sample if 0.892 g would take 3.73 days to decay to 0.114 g? (Outcome # 3) (DOK 3) A. 0.331 hours B. 2.96 hours C. 30.1 hours*

Page 4 of 4

Credit: Modification of assessment items provided by Lumen Learning, with generous funding from the William and Flora Hewlett Foundation. Licensed Creative Commons Attribution 4.0.

TEST BANK

TEST BANK

The title documents are available in full on the following links

Title: Test Bank for OpenStax Chemistry 2E by Paul Flowers, Klaus Theopold, Richard Langley & William Robinson - Complete, Elaborated & Latest Solution Manual. ALL Chapters (1-21) Included & Updated

Link I: https://scholarfriends.com/singlePaper/404765/test-bank-for-chemistry-2e-by-openstax-2ndedition-by-openstaxpaul-flowers-edward-j-neth-robins

Link II: https://scholarfriends.com/singlePaper/423835/test-bank-for-chemistry-2nd-edition-byopenstaxpaul-flowers-edward-j-neth-robinson-klaus-theopo