Introductory Chemistry Test Bank - 3115 Verified Questions

Introductory Chemistry Test Bank

Course Introduction

Introductory Chemistry provides a foundational understanding of the principles and concepts that underlie chemical phenomena. This course covers topics such as the structure of atoms and molecules, chemical bonding, states of matter, stoichiometry, chemical reactions, the periodic table, and basic thermochemistry. Students learn how to apply scientific reasoning, perform calculations involving chemical quantities, and safely conduct experiments in a laboratory setting. The course is designed for those new to chemistry and prepares students for more advanced study in the sciences while emphasizing the relevance of chemistry in everyday life and various professional fields.

Recommended Textbook Chemistry 11th Edition by Raymond Chang

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25 Chapters

3115 Verified Questions

3115 Flashcards

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Chapter 1: Chemistry: the Study of Change

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Sample Questions

Q1) Radio waves travel at the speed of light, which is 3.00 × 10⁸ m/s.How many minutes does it take for a radio message to reach Earth from Saturn if Saturn is 7.9 × 10⁸ km from Earth?

A)4.4 × 10^-2 min

B)1.6 × 10⁵ min

C)4.0 × 10¹⁵ min

D)44 min

E)2.6 min

Answer: D

Q2) Express the number 26.7 in scientific notation.

A)2.67 × 10^-2

B)2.67 × 10^-1

C)2.67 × 10¹

D)2.67 × 10²

E)26.7 is already written in scientific notation

Answer: C

Q3) Define element.

Answer: An element is a substance that cannot be separated into simpler substances by chemical means.

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Page 3

Chapter 2: Atoms, Molecules, and Ions

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Sample Questions

Q1) Name the compound CuSO₄

A)Copper (I)sulfate

B)Copper (I)sulfite

C)Copper (II)sulfite

D)Copper (II)sulfate

E)Copper (IV)sulfate

Answer: D

Q2) Name the following binary compound: NaH.

Answer: sodium hydride

Q3) Give the formula of copper(II)bromide.

Answer: CuBr₂

Q4) Write the formula of a cation that contains a nonmetal. Answer: NH₄⁺

Q5) An iron(II)ion has:

A)24 electrons and a charge of 2+

B)24 electrons and a charge of 2-

C)26 electrons and a charge of 2+

D)28 electrons and a charge of 2+

E)28 electrons and a charge of 2-

Answer: A

Page 4

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) How many sulfur atoms are present in 25.6 g of Al₂(S₂O₃)₃?

A)0.393

B)6.00

C)3.95 × 10²²

D)7.90 × 10²²

E)2.37 × 10²³

Answer: E

Q2) What is the average mass, in grams, of one Rb atom?

A)6.02 x 10²³ g

B)1.42 x 10^-22g

C)5.15 x 10²⁵ g

D)85.47 g

E)85.47 amu

Answer: B

Q3) Oxidation of a hydrocarbon gave a product composed of carbon, hydrogen, and oxygen.The product that was purified and sent off for elemental analysis giving the following mass percents: 68.85% C and 4.95% H.Determine the empirical formula of this compound.

Answer: C₇H₆O₂

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Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) During a titration the following data were collected.A 10.mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40.mL of the base were required to neutralize the sample.How many moles of acid are present in 2.0 liters of this unknown solution?

Q2) Determine the oxidation number of each of the elements in Cs₂Cr₂O₇?

Q3) Hydrogen is oxidized in the following chemical reaction. H₂ + Cl₂\(\rarr\)2HCl

A)True

B)False

Q4) In the following chemical reaction the oxidizing agent is 5H₂O₂ + 2MnO₄^- + 6H⁺ \(\rarr\)2Mn²⁺ + 8H₂O + 5O₂

A)H₂O₂

B)MnO₄^-

C)H⁺

D)Mn²⁺

E)O₂

Q5) Name and give the formulas for six strong acids.

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Chapter 5: Gases

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Sample Questions

Q1) If the pressure of a gas sample is quadrupled and the absolute temperature is doubled, by what factor does the volume of the sample change?

A)8

B)2

C)1/2

D)1/4

E)1/8

Q2) Calculate the volume occupied by 56.5 g of argon gas at STP.

A)22.4 L

B)31.7 L

C)34.6 L

D)1,270 L

E)1,380 L

Q3) A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21°C is allowed to rise to the stratosphere where the temperature is -5°C and the pressure is 1.0 millibar.What is the final volume of the balloon in Liters? 1.000 atm = 1.013 bar.

Q4) How many grams of N₂O, nitrous oxide, are contained in 500.mL of the gas at STP?

Q5) What is standard temperature and standard pressure in units of °C and atm?

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Chapter 6: Thermochemistry

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Sample Questions

Q1) The heat of solution of calcium chloride CaCl₂ is -82.8 kJ/mol, and the combined heats of hydration of 1.00 mole of gaseous calcium ions and 2.00 mole of gaseous chloride ions is -2327 kJ.What is the lattice energy of calcium chloride?

Q2) The heat absorbed by a system at constant pressure is equal to \(\Delta\)E + P\(\Delta\)V.

A)True

B)False

Q3) When 18.5 g of HgO(s)is decomposed to form Hg(l)and O₂(g), 7.75 kJ of heat is absorbed at standard-state conditions.What is the standard enthalpy of formation (\(\Delta\)H°_f)of HgO(s)?

A)-90.7 kJ/mol

B)-7.75 kJ/mol

C)0.419 kJ/mol

D)27.9 kJ/mol

E)143 kJ/mol

Q4) The heat of solution of NH₄NO₃ is 26.2 kJ/mol.Is heat evolved or absorbed when a solution of NH₄NO₃ is diluted by addition of more water?

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Chapter 7: Quantum Theory and the Electronic Structure of Atoms

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Sample Questions

Q1) The longest wavelength of light that causes electrons to be ejected from the surface of a copper plate is 243 nm.What is the maximum velocity of the electrons ejected when light of wavelength 200.nm shines on a copper plate?

A)1.97 × 10⁴ m/s

B)4.67 × 10⁴ m/s

C)6.22 × 10⁵ m/s

D)1.34 × 10⁶ m/s

E)1.48 × 10⁶ m/s

Q2) What is the energy in joules of a mole of photons associated with red light of wavelength 7.00 × 10² nm?

A)4.72 × 10^-43 J

B)1.71 × 10⁵ J

C)12.4 kJ

D)256 kJ

E)2.12 × 10⁴² J

Q3) Write the ground state electron configuration for the selenium atom.

Q4) What is the total number of electrons possible in the 6s orbital?

Q5) Calculate the energy of a photon of light with a wavelength of 360 nm.

Q6) Write the ground state electron configuration for Ni.

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Chapter 8: Periodic Relationships Among the Elements

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Sample Questions

Q1) The effective nuclear charge (Z_eff)felt by the outermost electrons is the strongest for which of the following elements?

A)B

B)C

C)N

D)O

E)F

Q2) Write the ground-state electron configuration for Cr³⁺.

Q3) Which of the following is the general electron configuration for the outermost electrons of the elements in Group 5A?

A)ns²np⁶

B)ns²np⁵

C)ns²np⁴

D)ns²np³

E)ns²np¹

Q4) Amphoteric oxides exhibit both acidic and basic properties.

A)True

B)False

Q5) Write the ground-state electron configuration for Br^-.

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Chapter 9: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) Use the bond enthalpy data given to estimate the heat released when 25.0 g of acetylene gas, C₂H₂, burns in excess oxygen to yield carbon dioxide and water vapor at 25°C. BE(C-C)= 347 kJ/mol

BE(C=C)= 812 kJ/mol

BE(C=O in CO₂)= 799 kJ/mol

BE(C-H)= 414 kJ/mol

BE(O-H)= 460 kJ/mol

BE(O=O)= 498.7 kJ/mol

A)16.8 kJ

B)364 kJ

C)447 kJ

D)1180 kJ

E)1230 kJ

Q2) The Lewis structure reveals a triple bond in which of the following molecules?

A)Br₂

B)O₂

C)N₂

D)H₂

E)CH₄

Q3) Write a Lewis structure for OF₂.

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Chapter 10: Chemical Bonding Ii: Molecular Geometry and Hybridization

of Atomic

Orbitals

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Sample Questions

Q1) Indicate the type of hybrid orbitals used by the central atom in TeF₄.

A)sp

B)sp²

C)sp³

D)sp³d

E)sp³d²

Q2) According to VSEPR theory, which one of the following molecules is trigonal bipyramidal?

A)SF₄

B)XeF₄

C)NF₃

D)SF₆

E)PF₅

Q3) Which one of the following molecules has a zero dipole moment?

A)CO

B)CH₂Cl₂

C)SO₃

D)SO₂

E)NH₃

Page 12

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Chapter 11: Intermolecular Forces and Liquids and Solids

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Sample Questions

Q1) Indicate all the types of intermolecular forces of attraction in CF₄(g).

Q2) The normal boiling point of methanol (CH₃OH)is 64.6°C.Given that the vapor pressure of methanol is 75.0 torr at 15.2°C, calculate the molar enthalpy of vaporization of methanol.

A)0.383 kJ/mol

B)3.00 kJ/mol

C)27.5 kJ/mol

D)38.0 kJ/mol

E)74.7 kJ/mol

Q3) Identify the dominant (strongest)type of intermolecular force present in RbCl(s).

Q4) Each of the following substances is a gas at 25°C and 1 atmosphere pressure.Which one will liquefy most easily when compressed at a constant temperature?

A)F₂

B)H₂

C)HF

D)SiH₄

E)Ar

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13

Chapter 12: Physical Properties of Solutions

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Sample Questions

Q1) Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

A)2.45 × 10^-4 m

B)5.80 × 10^-4 m

C)2.45 × 10^-1 m

D)103 m

E)5.80 m

Q2) What is the boiling point of an aqueous solution of a nonelectrolyte that has an osmotic pressure of 10.50 atm at 25°C? K_b of water is 0.52°C/m.Assume the density of the solution is the same as that of pure water.

A)0.22°C

B)0.429°C

C)99.78°C

D)100.22°C

E)100.43°C

Q3) A 100.-mL sample of water is taken from the Pacific Ocean, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 3.85 g.Calculate the original concentration of NaCl, in g per liter, in the water sample.

Q4) What is the mole fraction of NaOH in a 32.0 % by mass NaOH aqueous solution?

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Page 14

Chapter 13: Chemical Kinetics

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Sample Questions

Q1) The reaction 2A \(\rarr\) products is second order with respect to A.If the concentration of A drops from 1.05 M to 0.815 M in a time of 15.0 min, what is the rate constant for this reaction (the same time units may be used)?

Q2) For the first-order reaction 2N₂O₅ \(\rarr\)2N₂O₄ + O₂ at a particular temperature, the half-life of N₂O₅ is 0.90 hr.What fraction of the initial concentration of N₂O₅ will remain after 2.4 hours?

Q3) The reaction A + 2B \(\rarr\) products was found to follow the rate law: rate = k[A]²[B].Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

A)5

B)6

C)12

D)18

E)None of these.

Q4) Given the rate law for a reaction, rate = k[A]², where rate is measured in units of M min^-1, what are the units for the rate constant k?

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Page 15

Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) What conditions are used in the Haber process to enhance the yield of ammonia? Explain why each condition affects the yield in terms of the Le Châtelier principle.

Q2) A reaction with an equilibrium constant K_c = 1.5 x 10²¹ would consist of which of the following at equilibrium:

A)approximately equal reactants and products

B)some reactants and products with reactants slightly favored

C)some reactants and products with products slightly favored

D)essentially all reactants

E)essentially all products

Q3) A reaction with an equilibrium constant K_c = 1.5 x 10^-25 would consist of which of the following at equilibrium:

A)approximately equal reactants and products

B)some reactants and products with reactants slightly favored

C)some reactants and products with products slightly favored

D)essentially all reactants

E)essentially all products

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Chapter 15: Acids and Bases

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Sample Questions

Q1) Write the chemical formula for the acid formed when Cl₂O₇ is dissolved in water.

Q2) Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

A)2.9 × 10^-2M

B)5.7 × 10^-2M

C)1.3 × 10^-3M

D)2.9 × 10^-3M

E)5.7 × 10^-4M

Q3) Calculate the pH of a 0.021 M NaCN solution.[K_a(HCN)= 4.9 × 10^-10]

A)1.68

B)3.18

Q4) Calculate the pH of a 0.15 M solution of HOI (K_a = 2.3 x 10^-11)

Q5) HCN is classified as a weak acid in water.What does this classification mean?

Q6) Calculate the pOH of a solution containing 0.25 g of HCl in 800.mL of solution.

Page 17

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Chapter 16: Acid-Base Equilibria and Solubility Equilibria

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Sample Questions

Q1) Calculate the molar solubility of AgBr in a 0.25M solution of NH₃(aq)(K_sp (AgBr)= 7.7 x 10^-13 ; K_f (Ag(NH₃)₂⁺)= 1.5 x 10⁷.

A)8.8 x 10^-7 M

B)3.4 x 10^-3 M

C)8.4 x 10^-4 M

D)2.5 x 10^-1 M

E)9.7 x 10² M

Q2) Bromothymol blue is a common acid-base indicator.It has a K_a equal to 1.6 × 10^-7.Its un-ionized form is yellow and its conjugate base is blue.What color would a solution have at pH = 5.8?

Q3) Calculate the pH of a solution that is 0.15 M CH₃COOH and 0.75 M CH₃COONa.

Q4) A 50.0 mL sample of 2.0 × 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN.The formation constant of the complex ion Cu(CN)₃^2- is 1.0 × 10⁹.What is the copper(I)ion concentration in this system at equilibrium?

Q5) Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH)buffer that has a pH of 4.77.

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Chapter 17: Entropy Free Energy and Equilibrium

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Sample Questions

Q1) Arrange the following substances in the order of increasing entropy at 25°C. HF(g), NaF(s), SiF₄(g), SiH₄(g), Al(s)

Lowest \(\rarr\) highest

A)SiF₄(g)< SiH₄(g)< NaF(s)< HF(g)< Al(s)

B)HF(g)< Al(s)< NaF(s)< SiF₄(g)< SiH₄(g)

C)Al(s)< NaF(s)< HF(g)< SiH₄(g)< SiF₄(g)

D)Al(s)< HF(g)< NaF(s)< SiF₄(g)< SiH₄(g)

E)NaF(s)< Al(s)< HF(g)< SiF₄(g)< SiH₄(g)

Q2) Which of the following is consistent with an exothermic reaction that is nonspontaneous at high temperatures?

A)(\(\Delta\)H > 0, \(\Delta\)S < 0, \(\Delta\)G < 0)

B)(\(\Delta\)H > 0, \(\Delta\)S > 0, \(\Delta\)G < 0)

C)(\(\Delta\)H < 0, \(\Delta\)S > 0, \(\Delta\)G < 0)

D)(\(\Delta\)H < 0, \(\Delta\)S > 0, \(\Delta\)G > 0)

E)(\(\Delta\)H < 0, \(\Delta\)S < 0, \(\Delta\)G > 0)

Q3) Dissolving an ionic solid in water always results in an increase in entropy.

A)True

B)False

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19

Chapter 18: Electrochemistry

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Sample Questions

Q1) The half-reaction that occurs at the cathode during electrolysis of an aqueous sodium iodide solution is

A)Na⁺ + e^- \(\rarr\) Na.

B)Na \(\rarr\) Na⁺ + e^-.

C)2H₂O + 2e^- \(\rarr\) H₂ + 2OH^-.

D)I₂ + 2e^- \(\rarr\) 2I^-.

E)2I^- \(\rarr\)I₂ + 2e^-.

Q2) Iron objects such as storage tanks and underground pipelines can be protected from corrosion by connecting them through a wire to a piece of A)Pb

B)Ag

C)Sn

D)Mg

E)Cu

Q3) Calculate E°_cell for the following electrochemical cell: Ni(s)| Ni²⁺(aq)|| Hg₂²⁺(aq)| Hg(l)| Pt(s)

Q4) Aluminum metal is formed by the electrolysis of Al₂O₃in molten cryolite.How many grams of Al are produced when 6.50 × 10³ C pass through the cell?

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Chapter 19: Nuclear Chemistry

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Sample Questions

Q1) When a ¹⁶²Re nucleus emits an alpha particle, the nuclear species that results is _____________.

Q2) The energy released by the sun is the result of A)natural radioactivity.

B)nuclear fusion.

C)combustion of hydrogen.

D)photosynthesis.

E)nuclear fission.

Q3) Present-day plant life has a carbon-14 decay rate of 16 disintegrations per minute (dpm)per gram of carbon.If a contemporary wooden chair were somehow preserved for the next 3,900 years, what ¹⁴C decay rate should be expected from the wood used to make the chair? (t_1/2= 5,730 yr)

A)26 dpm

B)12 dpm

C)11 dpm

D)10 dpm

E)8 dpm

Q4) Determine the decay rate for a radioisotope sample with an activity of 12 microcuries? [1 curie = 3.7 × 10¹⁰disintegrations/s]

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Chapter 20: Chemistry in the Atmosphere

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Q1) One of the steps in the fixation of nitrogen by lightening is given below. 2NO₂(g)+ H₂O(l)\(\rarr\)HNO₂(aq)+ HNO₃(aq)

In this reaction, is the element nitrogen oxidized or reduced?

A)Nitrogen is oxidized in this reaction.

B)Nitrogen is reduced in this reaction.

C)Nitrogen is oxidized and reduced in this reaction.

D)Nitrogen is neither oxidized nor reduced in this reaction.

Q2) Write out the reaction that shows how the acidic oxide N₂O₅ combines with water to generate nitric acid leading to acid rain.

Q3) List the following greenhouse gases in order of their overall magnitude of contribution to global warming: N₂O, CFCs, CO₂, CH₄

A)N₂O < CFCs < CO₂ < CH₄

B)N₂O < CH₄ < CFCs < CO₂

C)CO₂ < N₂O < CFCs < CH₄

D)CH₄ < CFCs < N₂O < CO₂

E)N₂O < CFCs < CH₄ < CO₂

Q4) List three primary pollutants removed from automobile exhaust by catalytic converters.

Page 22

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Chapter 21: Metallurgy and the Chemistry of Metals

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Sample Questions

Q1) Which two compounds are produced by the Solvay process?

A)CaCO₃ and CaO

B)CaCO₃ and Na₂CO₃

C)NaHCO₃ and NaCl

D)NH₃ and NH₄Cl

E)NaHCO₃ and Na₂CO₃

Q2) According to the band theory, which of these statements provide(s)an explanation for the high electrical conductivity of metals? I.a partly filled conduction band

II.a valence band overlapping an empty conduction band

III.a filled valence band

IV.a large gap between the valence band and the conduction band

A)I and II

B)I and III

C)III

D)III and IV

E)IV

Q3) Potassium superoxide, KO₂(s), is used in the breathing systems of biohazard suits.Write separate chemical equations showing how KO₂(s)reacts with moisture and carbon dioxide in exhaled air to generate oxygen gas.

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Chapter 22: Nonmetallic Elements and Their Compounds

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Sample Questions

Q1) Which of these reactions is an example of nitrogen fixation?

A)2N₂O \(\rarr\)2N₂ + O₂

B)NH₃ + H₂O \(\rarr\)NH₄⁺ + OH^-

C)N₂ + O₂ \(\rarr\) 2NO

D)2NO₂ + H₂O \(\rarr\) HNO₂ + HNO₃

E)2NO + O₂ \(\rarr\) 2NO₂

Q2) Hydrogen plays an important role in many industrial processes.Write a balanced chemical equation for its production by the water gas reaction.

Q3) Write the chemical formula of the superoxide ion.

Q4) When phosphate rock, Ca₃(PO₄)₂(s), is converted to phosphorus,

A)one of the products of the reaction is water.

B)sulfuric acid is added to generate insoluble calcium sulfate.

C)hydrogen is used to reduce the phosphate to phosphorus.

D)silica is added to form a calcium silicate slag.

E)oxygen must be added to prevent reaction of P₄.

Q5) Write an equation for a laboratory preparation of nitrogen gas.

Q6) Write the chemical formula of the peroxide ion.

Page 24

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Chapter 23: Transition Metal Chemistry and Coordination Compounds

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Sample Questions

Q1) Which of the following complexes has optical (chiral)isomers?

A)[Co(NH₃)₄Br₂]⁺

B)[Co(en)₃]³⁺

C)Co(NH₃)₃Br₃

D)[Co(en)Br₄]^-

E)[Co(en)(NH₃)₄]³⁺

Q2) Predict the number of unpaired electrons in the [CrCl₆]^4- ion.

Q3) In Na₃[Ni(SCN)₅], how many 3d electrons does nickel have?

Q4) The total number of electrons in the 3d orbitals of a copper atom is

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Chapter 24: Organic Chemistry

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Q1) How many structural isomers are there of C₄H₁₀?

A)4

B)6

C)2

D)8

E)10

Q2) "Wood alcohol" is the common name for A)methanol. B)ethanol. C)propyl alcohol. D)ethylene. E)acetylene.

Q3) The oxidation product of 1-propanol when using Cr₂O₇^2- as the oxidizing agent is acetone.

A)True

B)False

Q4) A compound with the formula C₆H₁₂ may or may not be a saturated hydrocarbon.Explain.

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Page 26

Chapter 25: Synthetic and Natural Organic Polymers

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Q1) Both DNA and RNA have double-helical structures.

A)True

B)False

Q2) What structural feature is required to have an isotactic or syndiotactic carbon-based polymer?

A)A repeating unit that contains an asymmetric carbon

B)A repeating unit that contains a double bond

C)A repeating unit that contains a triple bond

D)A repeating unit that contains an aromatic hydrocarbon

E)A repeating unit that contains an atom other than carbon

Q3) The primary structure of a protein refers to the unique amino acid sequence of the polypeptide chain.

A)True

B)False

Q4) Which nitrogen base is found in RNA but not in DNA?

A)adenine

B)cytosine

C)guanine

D)thymine

E)uracil

To view all questions and flashcards with answers, click on the resource link above. Page 27