General Chemistry I Practice Exam
Course
Introduction
General Chemistry I provides a foundational introduction to the principles and concepts of chemistry, exploring the structure of matter, atomic theory, chemical bonding, stoichiometry, periodic trends, and the properties of gases, liquids, and solids. The course emphasizes quantitative problem-solving, laboratory techniques, and the application of chemical principles to real-world scenarios, preparing students for further study in chemistry and related scientific fields.
Recommended Textbook
General Chemistry 11th Edition by Darrell D. Ebbing
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Chapter 1: Chemistry and Measurement
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Sample Questions
Q1) The boiling point of chlorine is 172 K.This temperature corresponds to A)-82°C.
B)101°C.
C)172°C.
D)-172°C.
E)-101°C.
Answer: E
Q2) How many liters are in 15.1 fluid ounces of a soft drink? (1 fl oz = 28.35 mL)
A)5 × 10<sup>-4</sup> L
B)5 × 10<sup>2</sup> L
C)4 × 10<sup>5</sup> L
D)4 × 10<sup>2</sup> L
E)0.428 L
Answer: E
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Chapter 2: Atoms, molecules, and Ions
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Sample Questions
Q1) Which is a correct balanced chemical equation corresponding to the following description of a chemical reaction?
Hydrochloric acid reacts with magnesium metal to produce aqueous magnesium chloride and hydrogen gas.
A)2HCl(aq)+ Mg(s) MgCl<sub>2</sub>(aq)+ 2H(g)
B)2HCl(aq)+ Mg(s) MgCl<sub>2</sub>(aq)+ H<sub>2</sub>(g)
C)2HCl(aq)+ Mg(s) MgCl(aq)+ H<sub>2</sub>(g)
D)2HCl(aq)+ Mg(aq) MgCl<sub>2</sub>(s)+ H<sub>2</sub>(g)
E)HCl(aq)+ Mg(s) MgCl(aq)+ H(g)
Answer: B
Q2) Which of the following statements about different elements is incorrect?
A)Potassium is an alkali metal.
B)Fluorine is a halogen.
C)Aluminum is a transition element.
D)Barium is an alkaline earth metal.
E)Helium is a noble gas.
Answer: C
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Chapter 3: Calculations With Chemical Formulas and Equations
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Sample Questions
Q1) How many aluminum atoms are there in 52 g of Al<sub>2</sub>S<sub>3</sub>?
A)4.2 × 10<sup>23</sup>
B)1.6 × 10<sup>21</sup>
C)2.1 × 10<sup>23</sup>
D)1.1 × 10<sup>21</sup>
E)6.3 × 10<sup>23</sup>
Answer: A
Q2) Sulfur trioxide,SO<sub>3</sub>,is made from the oxidation of SO<sub>2</sub>,and the reaction is represented by the equation: 2SO<sub>2</sub> + O<sub>2</sub> 2SO<sub>3</sub>
A 25-g sample of SO<sub>2</sub> gives 18 g of SO<sub>3</sub>.The percent yield of SO<sub>3</sub> is .
A)9 %
B)58 %
C)14 %
D)31 %
E)100 %
Answer: B
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Chapter 4: Chemical Reactions
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Sample Questions
Q1) What mass of Na<sub>2</sub>CO<sub>3</sub> is present in 0.450 L of a 0.704 M Na<sub>2</sub>CO<sub>3</sub> solution?
A)33.5 g
B)47.6 g
C)74.6 g
D)67.7 g
E)165 g
Q2) In basic solution the chromate ion,CrO<sub>4</sub><sup>2-</sup>,can be converted to the chromite,CrO<sub>2</sub><sup>-</sup>,ion.The number of electrons gained or lost by the chromium atom is A)0.
B)3 electrons lost.
C)2 electrons lost.
D)3 electrons gained.
E)2 electrons gained.
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6
Chapter 5: The Gaseous State
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Sample Questions
Q1) A vessel with a volume of 12.4 L contains 2.80 g of nitrogen gas,0.403 g of hydrogen gas,and 79.9 g of argon gas.At 25°C,what is the pressure in the vessel?
A)164 atm
B)256.2 atm
C)4.54 atm
D)0.380 atm
E)2.27 atm
Q2) What does R denote in the ideal gas equation,PV = nRT?
A)Coulomb's constant
B)Rydberg constant
C)Boltzmann constant
D)Atomic mass constant
E)Molar gas constant
Q3) The density of O<sub>2</sub> gas at 16°C and 1.27 atm is A)31 g/L.
B)28.4 g/L.
C)1.71 g/L.
D)88.7 g/mL.
E)0.584 g/L.
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Chapter 6: Thermochemistry
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Sample Questions
Q1) Which of the following statements about enthalpy is false?
A)Enthalpy is a state function.
B)At constant pressure,the enthalpy change is equal to the heat absorbed or released.
C)Enthalpy is an extensive property.
D)The change in enthalpy of a process cannot be negative.
E)The SI unit of enthalpy is J.
Q2) The heat required to raise the temperature of 54.94 g of manganese by 1°C is called its
A)heat of vaporization.
B)specific heat.
C)heat of fusion.
D)entropy.
E)molar heat capacity.
Q3) Which of the following statements is not true for an exothermic reaction?
A)The products have a higher heat content than the reactants.
B)The temperature of the reaction system increases.
C)The temperature of the surroundings increases.
D)Heat passes from the reaction system to the surroundings.
E)The enthalpy change for the reaction is negative.
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Chapter 7: Quantum Theory of the Atom
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Sample Questions
Q1) Which type of electromagnetic radiation has the longest wavelength?
A)red light
B)x rays
C)gamma rays
D)microwaves
E)blue light
Q2) Which hydrogen atom orbital has an energy essentially identical to a 3d orbital?
A)5d
B)4d
C)2s
D)1s
E)3p
Q3) In Bohr's atomic theory,when an electron moves from one energy level to another energy level more distant from the nucleus,
A)energy is absorbed.
B)light is emitted.
C)energy is emitted.
D)no change in energy occurs.
E)none of these
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Chapter 8: Electron Configurations and Periodicity
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Sample Questions
Q1) What is the maximum number of electrons in an atom that have the set of quantum numbers n= 2 and l= 1?
A)10
B)2
C)14
D)18
E)6
Q2) What is the maximum number of electrons that can occupy one p orbital?
A)14
B)2
C)10
D)1
E)6
Q3) The quantum numbers of an atom's highest-energy valence electrons are n = 5 and l = 1.The element to which this atom belongs could be a
A)inner transition metal.
B)alkali metal.
C)s-block main-group element.
D)transition metal.
E)p-block main-group element.
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Chapter 9: Ionic and Covalent Bonding
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Sample Questions
Q1) The Cr<sup>2+</sup> ion would be expected to have ____ unpaired electrons.
A)4
B)2
C)3
D)0
E)1
Q2) In the Lewis dot formula that minimizes formal charge,how many bonds are there in the tetrathionate ion,S<sub>4</sub>O<sub>6</sub><sup>2-</sup> ?
A)7
B)9
C)15
D)11
E)13
Q3) The octet rule is violated by at least one atom in all the following compounds except
A)SiF<sub>5</sub><sup>-</sup>.
B)SCl<sub>6</sub>.
C)BrF<sub>5</sub>.
D)SiF<sub>6</sub><sup>2-</sup>.
E)NF<sub>3</sub>.
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Page 11
Chapter 10: Molecular Geometry and Chemical Bonding Theory
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Sample Questions
Q1) Which molecule or ion has a trigonal pyramidal molecular geometry?
A)BF<sub>3</sub>
B)C<sub>2</sub>H<sub>4</sub>
C)SO<sub>3</sub>
D)SO<sub>3</sub><sup>2-</sup>
E)CO<sub>3</sub><sup>2-</sup>
Q2) Which of the following electron distributions among the molecular orbitals best describes the NO molecule?
<sub>2s</sub> <sub>2s</sub><sup>*</sup>
<sub>2py</sub>= <sub>2px</sub> <sub>2pz</sub> <sub>2py</sub><sup>*</sup>= <sub>2px</sub><sup>*</sup> <sub>2pz</sub><sup>*</sup>
A)2 2 4 1 3 0
B)2 2 4 2 4 1
C)2 2 4 2 1 0
D)2 2 4 2 2 0
E)2 2 4 2 4 2
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Chapter 11: States of Matter; Liquids and Solids
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Sample Questions
Q1) Rank the following molecules in order of increasing normal boiling point: CH<sub>3</sub>CH<sub>2</sub>OH,CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>O H,CH<sub>3</sub>CH<sub>2</sub>OCH<sub>3</sub>.
A)lowest
CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>OH,CH<sub>3</sub>CH<sub>2</sub>O CH<sub>3</sub>,CH<sub>3</sub>CH<sub>2</sub>OH highest.
B)lowest
CH<sub>3</sub>CH<sub>2</sub>OH,CH<sub>3</sub>CH<sub>2</sub>OCH<sub>3</sub> ,CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>OH highest.
C)lowest
CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>OH,CH<sub>3</sub>CH<sub>2</sub>O H,CH<sub>3</sub>CH<sub>2</sub>OCH<sub>3</sub> highest.
D)lowest
CH<sub>3</sub>CH<sub>2</sub>OCH<sub>3</sub>,CH<sub>3</sub>CH<sub>2</sub>OH ,CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>OH highest.
E)lowest
CH<sub>3</sub>CH<sub>2</sub>OCH<sub>3</sub>,CH<sub>3</sub>CH<sub>2</sub>CH <sub>2</sub>OH,CH<sub>3</sub>CH<sub>2</sub>OH highest.
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Chapter 12: Solutions
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Sample Questions
Q1) A cucumber is placed in a concentrated salt solution.What is most likely to happen?
A)Water will flow from the solution to the cucumber.
B)No change will occur.
C)Salt will flow into the cucumber.
D)Salt will precipitate out.
E)Water will flow from the cucumber to the solution.
Q2) A concentrated hydrofluoric acid solution is 49.0% HF by mass and has a density of 1.3406 g/mL at 25°C.What is the mass of HF per L of solution?
A)637 g HF /L soln
B)0.0013 g HF /L soln
C)376 g HF /L soln
D)0.265 g HF /L soln
E)3.76 g HF /L soln
Q3) The solubility of a gas in a liquid can always be increased by
A)decreasing the pressure of the gas above the solvent.
B)increasing the pressure of the gas above the solvent.
C)increasing the temperature of the solvent.
D)decreasing the polarity of the solvent.
E)decreasing the temperature of the gas above the solvent.
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Page 14
Chapter 13: Rates of Reaction
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Sample Questions
Q1) The nuclide <sup>188</sup>W decays by a first-order process with a rate constant of 1.0 × 10<sup>-2</sup> d<sup>-1</sup>.How long will it take for 88% of the initial amount of <sup>188</sup>W to be consumed?
A)6 d
B)240 d
C)12 d
D)210 d
E)92 d
Q2) At 500<sup>o</sup>C,cyclopropane (C<sub>3</sub>H<sub>6</sub>)reacts to form its isomer,propene (C<sub>3</sub>H<sub>6</sub>).The reaction is first-order,and the rate constant is 6.7 × 10<sup>-4</sup> s<sup>-1</sup>.If the initial concentration of cyclopropane is 0.500 M and the initial concentration of propene is 0,determine the time required for the concentration of propene to reach 0.100 M.
A)3.4 × 10<sup>3</sup> s
B)3.3 × 10<sup>2</sup> s
C)1.2 × 10<sup>4</sup> s
D)7.5 × 10<sup>2</sup> s
E)2.4 × 10<sup>3</sup> s
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) For a specific reaction,which of the following statements can be made about the equilibrium constant?
A)It can be changed by the addition of a catalyst.
B)It increases when the concentration of one of the products is increased.
C)It increases when the concentration of one of the reactants is increased.
D)It always remains the same.
E)It changes with changes in the temperature.
Q2) Which of the following is the main step in the contact process for the industrial production of sulfuric acid?
A)Oxidation of SO<sub>2</sub> in the presence of a catalyst
B)Oxidation of SO<sub>3</sub> in the presence of a catalyst
C)Oxidation of SO in the presence of a catalyst
D)Reduction of SO<sub>2</sub> in the presence of a catalyst
E)Reduction of SO<sub>4</sub> in the presence of a catalyst
Q3) Which of the following represents a dynamic equilibrium?
A)a stoppered flask half full of water
B)a coin spinning in mid-air
C)two people of equal mass balanced on the ends of a seesaw
D)an open pan of boiling water
E)an object traveling at a constant speed
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Chapter 15: Acids and Bases
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Sample Questions
Q1) What pH should a solution have if its pH is about the same as that of vinegar?
A)about 8
B)about 11
C)about 1
D)about 6
E)about 3
Q2) A solution in which the pH is 1.5 would be described as
A)neutral.
B)very acidic.
C)slightly basic.
D)slightly acidic.
E)very basic.
Q3) Which of the following statements does not describe a characteristic of an Arrhenius acid?
A)An Arrhenius acid reacts with an Arrhenius base to produce a salt.
B)An Arrhenius acid turns red litmus blue.
C)An Arrhenius acid is an electrolyte.
D)An Arrhenius acid reacts with CaCO<sub>3</sub> to produce CO<sub>2</sub>.
E)An Arrhenius acid tastes sour.
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Chapter 16: Acid-Base Equilibria
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Sample Questions
Q1) The K<sub>a</sub> for hydrofluoric acid is 6.8 × 10<sup>-4</sup>.What is K<sub>b</sub> for the fluoride ion?
A)1.5 × 10<sup>-11</sup>
B)6.8 × 10<sup>-4</sup>
C)1.5 × 10<sup>3</sup>
D)6.8 × 10<sup>10</sup>
E)6.8 × 10<sup>-18</sup>
Q2) What is the pH of a 0.35 M solution of methylamine (CH<sub>3</sub>NH<sub>2</sub>,K<sub>b</sub> = 4.4 × 10<sup>-4</sup>)at 25<sup>o</sup>C?
A)5.55
B)0.46
C)12.09
D)13.54
E)1.91
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Chapter 17: Solubility and Complex-Ion Equilibria
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Sample Questions
Q1) After mixing an excess PbCl<sub>2</sub> with a fixed amount of water,it is found that the equilibrium concentration of Pb<sup>2+</sup> is 1.6 × 10<sup>-2</sup> M.What is K<sub>sp</sub> for PbCl<sub>2</sub>?
A)4.0 × 10<sup>-6</sup>
B)1.6 × 10<sup>-5</sup>
C)2.5 × 10<sup>-4</sup>
D)4.8 × 10<sup>-2</sup>
E)1.0 × 10<sup>-6</sup>
Q2) K<sub>sp</sub> for PbF<sub>2</sub> is 4.0 ×10<sup>-8</sup>.If a 0.032 M NaF solution is saturated with PbF<sub>2</sub>,what is [Pb<sup>2+</sup>] in solution?
A)4.1 × 10<sup>-11</sup> M
B)1.3 × 10<sup>-9</sup> M
C)1.3 × 10<sup>-6</sup> M
D)1.2 × 10<sup>-3</sup> M
E)3.9 × 10<sup>-5</sup> M
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Chapter 18: Thermodynamics and Equilibrium
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Sample Questions
Q1) The reaction Br<sub>2</sub>(g) 2Br(g)is spontaneous only at temperatures in excess of 1600°C.We can conclude that
A) H is + and S is + for the reaction.
B) H is - and S is + for the reaction.
C) G is + for all temperatures.
D) H is - and S is - for the reaction.
E) H is + and S is - for the reaction.
Q2) Which of the following has the lowest entropy per mole?
A)liquid sodium at 100°C
B)gaseous sodium at 900°C and 0.5 atm
C)a solid solution of sodium in potassium at 30°C
D)gaseous sodium at 900°C and 1 atm
E)solid sodium at 30°C
Q3) The reaction C(s)+ CO<sub>2</sub>(g) 2CO(g)is spontaneous only at temperatures in excess of 1100 K.We can conclude that
A) G° is negative for all temperatures.
B) H° is negative and S° is negative.
C) H° is positive and S° is positive.
D) H° is negative and S° is positive.
E) H° is positive and S° is negative.
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Chapter 19: Electrochemistry
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Q1) A cell consists of a magnesium electrode immersed in a solution of magnesium chloride and a silver electrode immersed in a solution of silver nitrate.The two half-cells are connected by means of a salt bridge.It is possible to increase the voltage of the cell by
A)decreasing the concentration of Mg<sup>2+</sup> and increasing the concentration of Ag<sup>+</sup>.
B)adding sodium chloride to both half-cells.
C)increasing the size of the Mg electrode and decreasing the size of the Ag electrode. D)decreasing the size of the Mg electrode and increasing the size of the Ag electrode. E)increasing the concentration of Mg<sup>2+</sup>.
Q2) Which of the following is true for a reaction that is nonspontaneous as written?
A) G° > 0; E°<sub>cell</sub> < 0
B) G° < 0; E°cell < 0
C) G° < 0; E°<sub>cell</sub> < 0
D) G° > 0; E°<sub>cell</sub> > 0
E) G° > 0; E°<sub>cell</sub> = 0
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Chapter 20: Nuclear Chemistry
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Sample Questions
Q1) Iodine-131,which is used to treat thyroid cancer,has a half-life of 8.04 days.How much time is required for 68% of the isotope to decay?
A)13 days
B)7 days
C)43 days
D)53 days
E)4 days
Q2) When a nucleus undergoes radioactive decay,its new mass number is
A)always less than its original mass number.
B)never more than its original mass number.
C)never less than its original mass number.
D)always the same as its original mass number.
E)always more than its original mass number.
Q3) <sup>55</sup>Mn can be prepared by electron capture from which of the following?
A)(<sup>56</sup>Mn)
B)(<sup>55</sup>Fe)
C)(<sup>55</sup>Cr)
D)(<sup>51</sup>V)
E)(<sup>57</sup>Co)
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Page 22
Chapter 21: Chemistry of the Main-Group Metals
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Q1) Which of the following statements concerning lead is false?
A)Lead is predominantly used to make electrodes in batteries.
B)Lead ions exist only in the +4 oxidation state.
C)Lead reacts with hydrochloric acid,but because lead(II)chloride is insoluble in water,the reaction soon stops.
D)Lead is commercially prepared by reducing lead(II)oxide with carbon monoxide.
E)Lead is commonly found in galena,a lead(II)sulfide mineral.
Q2) Which of the following statements about sodium is false?
A)Sodium reacts with oxygen to produce sodium peroxide.
B)Sodium ions are a significant component of seawater.
C)Sodium reacts with water to produce sodium hydride and oxygen gas.
D)Sodium metal is produced by electrolysis of sodium chloride.
E)Sodium metal is a strong reducing agent.
Q3) Which of the following elements is least likely to form a stable oxide?
A)Fe
B)Ca
C)S<sub>8</sub>
D)P<sub>4</sub>
E)He
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Page 23
Chapter 22: The Transition Elements and Coordination Compounds
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Q1) Which of the following is a product of the acidification of sodium chromate?
A)CrO<sub>4</sub><sup>2-</sup>(aq)
B)Cr<sub>2</sub>O<sub>7</sub><sup>2-</sup>(aq)
C)Cr<sup>3+</sup>(aq)
D)CrO<sub>3</sub>(s)
E)Cr(s)
Q2)
1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>4s<sup> 2</sup>3d<sup>2</sup> is the correct electron configuration for which of the following atoms?
A)Ti
B)Ca
C)Ge
D)Zr
E)none of these
Q3) In which compound is cobalt in the highest oxidation state?
A)Co<sub>2</sub>(CO)<sub>8</sub>
B)[Co(NH<sub>3</sub>)<sub>6</sub>]Cl<sub>2</sub>
C)[Co(NH<sub>3</sub>)<sub>4</sub>Cl<sub>2</sub>]Cl
D)Na<sub>2</sub>[CoCl<sub>4</sub>]
E)K<sub>4</sub>[CoF<sub>6</sub>]
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Chapter 23: Organic Chemistry
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Q1) Which of the following names may represent either a cis or a trans isomer?
A)1-butene
B)1,2-dibromoethene
C)1,1,2-tribromoethene
D)1,1-dibromoethene
E)1-bromo-1-chloroethene
Q2) Which of the following is not a structural isomer of 1-pentene?
A)1-methyl-cyclobutene
B)2-methyl-2-butene
C)3-methyl-1-butene
D)2-pentene
E)cyclopentane
Q3) Carbon,a Group 4A element of the periodic table,has _____ valence electrons.
A)five
B)one
C)three
D)two
E)four
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Chapter 24: Polymer Materials: Synthetic and Biological
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Sample Questions
Q1) The sequence of amino acids held together by peptide bonds in a protein is the A)tertiary structure.
B)hydrogen bonding.
C)primary structure.
D)quaternary structure.
E)secondary structure.
Q2) What is the charge on each phosphate group in DNA in an aqueous solution near physiological pH?
A)0
B)1
C)2
D) 1
E) 2
Q3) Which of the following combinations can produce a condensation polymer? (R and R' are alkyl groups)
A)R OH + HOOC R' COOH
B)HO R OH + R' COOH
C)H<sub>2</sub>N R NH<sub>2</sub> + HOOC R' COOH
D)A and C
E)A,B,and C
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