Foundations of Chemistry Test Questions
Course Introduction
Foundations of Chemistry introduces students to the fundamental principles underlying the science of chemistry. Topics include atomic and molecular structure, chemical bonding, stoichiometry, states of matter, thermochemistry, and the periodic table. The course emphasizes problem-solving skills, laboratory techniques, and the development of a conceptual understanding of how chemical processes impact the natural and technological world. Designed for students beginning their studies in chemistry or related sciences, this course prepares learners for more advanced topics and provides a solid base for laboratory investigations and real-world applications.
Recommended Textbook
Introductory Chemistry An Atoms First Approach 1st Edition by Julia Burdge
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Page 2
Chapter 1: Atoms and Elements
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Sample Questions
Q1) The elements in Group 2A are known by what name?
A)Transition metals
B)Halogens
C)Alkali metals
D)Alkaline earth metals
E)Noble gases
Answer: D
Q2) Which of the following is an example of an observation?
A)Gases expand as their temperature increases because the gas molecules are moving more rapidly.
B)Paraffin wax begins to melt at 57°C.
C)Three samples of wax are heated to 75°C.
D)The force acting on an object is equal to its mass times its acceleration.
E)Will all waxes melt at the same temperature?
Answer: B
Q3) Lead (Pb) is a main group element.
A)True
B)False
Answer: True
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Page 3
Chapter 2: Electrons and the Periodic Table
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Sample Questions
Q1) Atomic orbitals developed using quantum mechanics
A)describe regions of space in which one is most likely to find an electron.
B)describe exact paths for electron motion.
C)give a description of the atomic structure which is essentially the same as the Bohr model.
D)allow scientists to calculate an exact volume for the hydrogen atom.
E)are in conflict with the Heisenberg uncertainty principle.
Answer: A
Q2) Using the periodic table, predict the charge on the common ion of selenium.
A)+1
B)+2
C) 1
D) 2
Answer: D
Q3) For all atoms of the same element, the 2s orbital is larger than the 1s orbital.
A)True
B)False
Answer: True
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Chapter 3: Compounds and Chemical Bonds
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Sample Questions
Q1) What types of elements undergo ionic bonding?
A)two metals
B)a nonmetal and a metal
C)two nonmetals
D)two Group 1A elements
E)two noble gases
Answer: B
Q2) The formula for sodium sulfide is
A)NaS
B)K<sub>2</sub>S
C)NaS<sub>2</sub>
D)Na<sub>2</sub>S
E)SeS
Answer: D
Q3) Determine the charge on the unknown ion, A, in the compound ACl2.
A)+2
B)+1
C)-1
D)-2
Answer: A
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Chapter 4: How Chemists Use Numbers
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Sample Questions
Q1) The SI prefix nano- (n) means
A)10<sup> </sup><sup>9</sup>
B)10<sup> </sup><sup>6</sup>
C)10<sup> </sup><sup>3</sup>
D)10<sup>+6</sup>
E)10<sup>+9</sup>
Q2) The SI prefix mega- (M) means
A)10<sup> </sup><sup>6</sup>
B)10<sup> </sup><sup>3</sup>
C)10<sup>3</sup>
D)10<sup>6</sup>
E)10<sup>9</sup>
Q3) How many micrograms are in 65.3 kg?
A)0.653 g
B)6.53 × 10<sup>7</sup> g
C)6.53 × 10<sup>4</sup> g
D)6.53× 10<sup> </sup><sup>8</sup> g
E)6.53 × 10<sup>10</sup> g
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Chapter 5: The Mole and Chemical Formulas
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Sample Questions
Q1) A rock contains an element with a molar mass of 40.08 g/mol.If 9.28 × 10<sup>24</sup> atoms of this element were found in the rock, how many grams of the unknown element are present in the rock?
A)618 g
B)1.49 × 10<sup>28</sup> g
C)2.24 × 10<sup>50</sup> g
D)0.38 g
E)3.80 g
Q2) Determine the mass of Sr(C<sub>2</sub>H<sub>3</sub>O<sub>2</sub>)<sub>2</sub> that contains 2.780 10<sup>23</sup> atoms of carbon.
A)205.7 g
B)57.19 g
C)46.16 g
D)94.96 g
E)23.74 g
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Chapter 6: Molecular Shape
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Sample Questions
Q1) Which is the most reasonable prediction for the H-N-H bond angle in NH<sub>3</sub>?
A)90°
B)109.5°
C)120°
D)107°
E)105°
Q2) In which one of the following species is the central atom (the first atom in the formula) likely to violate the octet rule?
A)BF<sub>4</sub><sup> </sup>
B)XeO<sub>3</sub>
C)SiCl<sub>4</sub>
D)NH<sub>3</sub>
E)CH<sub>2</sub>Cl<sub>2</sub>
Q3) What is the molecular geometry of HOF as predicted by the VSEPR model?
A)trigonal pyramidal
B)bent
C)tetrahedral
D)linear
E)trigonal planar
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Chapter 7: Solids, Liquids, and Phase Changes
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Sample Questions
Q1) Ethanol (C<sub>2</sub>H<sub>5</sub>-OH) will have a greater viscosity than ethylene glycol (HO-CH<sub>2</sub>CH<sub>2</sub>-OH) at the same temperature.
A)True
B)False
Q2) Which one of the following crystallizes in a metallic lattice?
A)C
B)NaMnO<sub>4</sub>
C)K
D)LiClO<sub>4</sub>
E)K<sub>2</sub>Cr<sub>2</sub>O<sub>7</sub>
Q3) What amount of energy (heat) is required to warm a 73.5-g sample of liquid ethanol from 15.0ºC to 29.5ºC? The specific heat capacity of ethanol is 2.46 J/gºC.
A)0.485 J
B)433 J
C)2.62 × 10<sup>3</sup> J
D)5.33 × 10<sup>3</sup> J
E)238 J
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9
Chapter 8: Gases
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Sample Questions
Q1) A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275
L.What will the gas pressure be if the volume is increased to 321 L at 125°C?
A)212 torr
B)289 torr
C)356 torr
D)441 torr
E)359 torr
Q2) What is the mass, in grams, of 2.74 L of CO gas measured at 33°C and 945 mmHg?
(R = 0.08206 L atm/mol K, 1 atm = 760 mmHg)
A)0.263 g
B)2.46 g
C)3.80 g
D)35.2 g
E)206 g
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Chapter 9: Physical Properties of Solutions
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Sample Questions
Q1) Determine the boiling point of a solution formed by dissolving 0.187 moles of glucose in 456 grams of water.(For water, K<sub>b</sub> = 0.512°C/m)
A)100.957°C
B)101.25°C
C)100.210°C
D)100.476°C
E)100.365°C
Q2) The distinguishing characteristic of all nonelectrolyte solutions is that they A)contain ions.
B)do not conduct electricity.
C)react with other solutions.
D)always contain acids.
E)conducts heat.
Q3) Based on the solubility rules, which one of these compounds is soluble in water?
A)CaSO<sub>4</sub>
B)BaSO<sub>4</sub>
C)PbSO<sub>4</sub>
D)K<sub>2</sub>SO<sub>4</sub>
E)Ag<sub>2</sub>SO<sub>4</sub>
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Page 11
Chapter 10: Chemical Reactions and Chemical Equations
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Sample Questions
Q1) What is the coefficient of O<sub>2</sub> when the following equation is properly balanced with the smallest set of whole numbers? __ C<sub>2</sub>H<sub>4</sub> + __ O<sub>2</sub> __ CO<sub>2</sub> + __ H<sub>2</sub>O
A)1
B)2
C)3
D)4
E)6
Q2) What is reduced in the following reaction? Cu(NO<sub>3</sub>)<sub>2</sub> + Zn
Zn(NO<sub>3</sub>)<sub>2</sub> + Cu
A)Cu(NO<sub>3</sub>)<sub>2</sub>
B)N
C)O
D)Zn
E)NO<sub>3</sub>
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Chapter 11: Using Balanced Chemical Equations
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Sample Questions
Q1) Ammonia reacts with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in the production of aluminum, in uranium processing, and in the frosting of light bulbs). 2NH<sub>3</sub>(g) + 5F<sub>2</sub>(g) N<sub>2</sub>F<sub>4</sub>(g) + 6HF(g)
How many moles of NH<sub>3</sub> are needed to react completely with 13.6 mol of F<sub>2</sub>?
A)34.0 mol
B)27.2 mol
C)6.80 mol
D)5.44 mol
E)2.27 mol
Q2) What is the maximum number of grams of ammonia, NH<sub>3</sub>, which can be obtained from the reaction of 10.0 g of H<sub>2</sub> and 80.0 g of N<sub>2</sub>? N<sub>2</sub> + 3H<sub>2</sub> 2NH<sub>3</sub>
A)34.1 g
B)48.6 g
C)56.3 g
D)90.0 g
E)97.3 g
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Chapter 12: Acids and Bases
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Sample Questions
Q1) Complete the following reaction and identify the Brønsted base: NaOH(aq) + HCl(aq)
A)Na(aq) + HOCl(aq); NaOH is the base.
B)NaCl(aq) + OH<sup> </sup>(aq); HCl is the base.
C)NaCl(aq) + OH<sup> </sup>(aq); NaOH is the base.
D)H<sub>2</sub>O(l) + NaCl(aq); HCl is the base.
E)NaCl(aq)+ H<sub>2</sub>O(l); NaOH is the base.
Q2) Identify the major ions present in an aqueous LiOH solution.
A)Li<sup>2+</sup>, O<sup> </sup>, H<sup> </sup>
B)Li<sup>+</sup>, OH<sup> </sup>
C)LiO<sup> </sup>, H<sup>+</sup>
D)Li<sup>+</sup>, O<sup>2 </sup>, H<sup>+</sup>
E)Li<sup> </sup>, OH<sup>+</sup>
Q3) What is the conjugate base of water?
A)H<sub>3</sub>O<sup>+</sup>
B)OH<sup> </sup>
C)H<sub>3</sub>O
D)OH
E)H<sub>2</sub>O<sub>2</sub>
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Page 14
Chapter 13: Equilibrium
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Sample Questions
Q1) At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.
A)True
B)False
Q2) Which substances are included in the equilibrium constant expression, K<sub>c</sub>?
A)Only pure solids
B)Only pure liquids
C)Only pure solids and liquids
D)Only gases and dissolved substances
E)All participating substances
Q3) If, in a particular process, reactants are able to form products, and products are also able to form reactants, then this process may be described as
A)a reversible process.
B)an elementary process.
C)at equilibrium.
D)forbidden.
E)a forward process.
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Chapter 14: Organic Chemistry
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Sample Questions
Q1) What name is given to a compound containing a hydroxyl group?
A)Aldehyde
B)Ketone
C)Alcohol
D)Amine
E)Ester
Q2) Organic chemistry is defined as the study of compounds containing which element?
A)Carbon
B)Silicon
C)Hydrogen
D)Sodium
E)Carbon and hydrogen
Q3) Which type of organic compound does not contain a carbonyl group?
A)Ethers
B)Carboxylic acids
C)Ketones
D)Aldehydes
E)Esters
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Chapter 15: Biochemistry
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Sample Questions
Q1) Which of the following is not a carbohydrate?
A)C<sub>6</sub>H<sub>12</sub>O<sub>6</sub>
B)C<sub>5</sub>H<sub>10</sub>O<sub>5</sub> C)C<sub>10</sub>H<sub>18</sub>O<sub>9</sub>
D)C<sub>6</sub>H<sub>14</sub>O<sub>6</sub> E)C<sub>12</sub>H<sub>22</sub>O<sub>11</sub>
Q2) A peptide bond (also called an amide bond) joins two amino acids together.What atoms are linked by this bond?
A)C - O
B)C - H
C)C - N
D)N - S
E)S - C
Q3) Which of the following refers to a primary structure?
A)The shape the protein chain adopts as the result of hydrogen bonding.
B)The sequence of amino acids that make up a protein chain.
C)The folding of a protein into a characteristic shape.
D)The shape formed by two or more folded protein chains coming together.
E)None of the above.
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Page 17
Chapter 16: Nuclear Chemistry
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Sample Questions
Q1) The half-life of <sup>14</sup>C is 5730 yr.Assuming some charcoal from a campfire 29,000 years old was found, what fraction of the original C-14 would remain today?
A)3.0 × 10<sup> 2</sup>
B)0.20
C)3.5
D)0.33
E)0.29
Q2) Beta particles are identical to A)protons.
B)helium atoms.
C)hydrogen atoms.
D)helium nuclei.
E)electrons.
Q3) Alpha particles are identical to A)protons.
B)helium atoms.
C)hydrogen atoms.
D)helium nuclei.
E)electrons.
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Page 18
Chapter 17: Electrochemistry
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Sample Questions
Q1) Complete and balance the following redox equation using the set of smallest whole numbers coefficients.What is the sum of the coefficients? HI + HNO<sub>3</sub> I<sub>2</sub> + NO (acidic solution)
A)5
B)7
C)14
D)17
E)None of these choices is correct.
Q2) When the following redox equation is balanced with the smallest whole number coefficients, what is the coefficient of Sb<sup>3</sup><sup>+</sup>(aq)? BrO<sub>3</sub><sup> </sup>(aq) + Sb<sup>3+</sup>(aq) Br<sup> </sup>(aq) + Sb<sup>5+</sup>(aq) (acidic solution)
A)1
B)2
C)3
D)4
E)6
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