General Chemistry II Exam Practice Tests - 3674 Verified Questions

General Chemistry II Exam Practice Tests

Course Introduction

General Chemistry II is a continuation of the foundational study of chemistry, building upon the concepts introduced in General Chemistry I. This course delves deeper into topics such as chemical kinetics, chemical equilibrium, acid-base reactions, thermodynamics, and electrochemistry. Additional subjects include solutions, solubility, and an introduction to nuclear and organic chemistry. Emphasis is placed on problem-solving, critical thinking, and laboratory techniques to develop a more thorough understanding of chemical phenomena and their applications in real-world situations. This course is essential for students pursuing further studies in science, engineering, and related fields.

Recommended Textbook

Chemistry The Central Science 14th Edition by Theodore E. Brown

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24 Chapters

3674 Verified Questions

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Chapter 1: Introduction: Matter, energy, and Measurement

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Sample Questions

Q1) The freezing point of water at 1 atm pressure is ________.

A)0 °F

B)0 K

C)0 °C

D)-273 °C

E)-32 °F

Answer: C

Q2) The density of a gold nugget is 19.3 g/cm³.If the volume of the gold nugget is 0.00369 L,the mass of the nugget is ________ g.

A)71.2

B)0.191

C)19.3

D)5.23

E)none of the above

Answer: A

Q3) 1.035 × 10^-4 L = ________ mL

Answer: 0.1035

Q4) Si is the symbol for the element ________. Answer: Silicon

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) Which atom has the smallest number of neutrons?

A)carbon-14

B)nitrogen-14

C)oxygen-16

D)fluorine-19

E)neon-20

Answer: B

Q2) Which metal does not form cations of differing charges?

A)Na

B)Cu

C)Co

D)Fe

E)Sn

Answer: A

Q3) What is the name of an alcohol derived from hexane?

Answer: hexanol

Q4) Which element is found in Period 2 and Group VIIA?

Answer: fluorine

Q5) The formula for potassium sulfide is ________. Answer: K₂S

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Chapter 3: Chemical Reactions and Reaction Stoichiometry

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Sample Questions

Q1) Which one of the following is not true concerning automotive air bags?

A)They are inflated as a result of a decomposition reaction.

B)They are loaded with sodium azide initially.

C)The gas used for inflating them is oxygen.

D)The two products of the decomposition reaction are sodium and nitrogen.

E)A gas is produced when the air bag activates.

Answer: C

Q2) Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s)+ 3O₂ (g) 2Al₂O₃(s)

In a particular experiment,the reaction of 2.5 g of Al with 2.5 g of O₂ produced 3.5 g of Al₂O₃.The % yield of the reaction is

A)74

B)37

C)47

D)66

E)29

Answer: A

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Page 5

Chapter 4: Reactions in Aqueous Solution

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Sample Questions

Q1) How many moles of Co²⁺ are present in 0.200 L of a 0.400 M solution of CoI₂?

A)2.00

B)0.500

C)0.160

D)0.0800

E)0.0400

Q2) Which of the following 0.300 M solutions would contain the highest concentration of potassium ions?

A)potassium phosphate

B)potassium hydrogen carbonate

C)potassium hypochlorite

D)potassium iodide

E)potassium bromide

Q3) What is the formula for phosphoric acid?

A)H₃PO₄

B)H₂PO₄

C)H₄PO₄

D)H₃PO₃

E)none of the above

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Chapter 5: Thermochemistry

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Sample Questions

Q1) H for an endothermic process is ________ while H for an exothermic process is

A)zero, positive

B)zero, negative

C)positive, zero

D)negative, positive

E)positive, negative

Q2) What is the molar heat capacity (in J/mol-K)of liquid bromine? The specific heat of liquid bromine is 0.226 J/g-K.

A)36.1 J/mol-K

B)707 J/mol-K

C)18.1 J/mol-K

D)9.05 J/mol-K

E)0.226 J/mol-K

Q3) The units of heat capacity are ________.

A)K/J or °C/J

B)J/K or J/°C

C)J/g-K or J/g-°C

D)J/mol

E)g-K/J or g-°C/J

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Chapter 6: Electronic Structure of Atoms

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Sample Questions

Q1) A mole of red photons of wavelength 725 nm has ________ kJ of energy.

A)2.74 × 10^-19

B)4.56 × 10^-46

C)6.05 × 10^-3

D)165

E)227

Q2) An electron cannot have the quantum numbers n = ________,l = ________,m_l= ________.

A)6, 1, 0

B)3, 2, 3

C)3, 2, -2

D)1, 0, 0

E)3, 2, 1

Q3) High energy and low wavelength light has the ability to eject electrons from metal surfaces.

A)True

B)False

Q4) Which group is represented by a ns²np⁶ valence shell electron configuration?

Q5) A line spectrum contains radiation of ________ wavelengths.

Page 8

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Chapter 7: Periodic Properties of the Elements

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Sample Questions

Q1) In the generation of most anions,the energy change (kJ/mol)that ________ an electron is ________.

A)removes, positive

B)adds, positive

C)removes, negative

D)adds, negative

E)None of the above is correct.

Q2) Which of the following species has the smallest ionic radius?

A)Al³⁺

B)Na⁺

C)Mg²⁺

D)S^2-

E)Cl^-

Q3) ________ is isoelectronic with argon,and ________ is isoelectronic with neon.

A)P^3-, N^3-

B)P^2-, N^2-

C)P³⁺, N³⁺

D)N^3-, P^3-

E)P, N

Q4) What are the elements called that are located between the metals and nonmetals?

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Chapter 8: Basic Concepts of Chemical Bonding

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Sample Questions

Q1) Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration?

O Sr Na Se Br

A)Br

B)Sr

C)Na

D)O, Se

E)Sr, O, Se

Q2) For ________ forms of a molecule or ion,the observed structure is an average of the ________ forms.

A)resonance, covalent

B)resonance, resonance

C)ionic, resonance

D)resonance, ionic

E)resonance, metallic

Q3) An exothermic reaction should have ________ chemical bonds and decompose to a molecule with ________ bonds.

Q4) If the bonds in the reactants of a reaction are weaker than the bonds in the product,the reaction is ________.

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Chapter 9: Molecular Geometry and Bonding Theories

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Sample Questions

Q1) The electron-domain geometry of a sulfur-centered compound is trigonal bipyramidal.The hybridization of the central sulfur atom is ________.

A)sp

B)sp²

C)sp³

D)sp³d

E)sp³d²

Q2) The electron-domain geometry and the molecular geometry of a molecule of the general formula AB_n are ________.

A)never the same

B)always the same

C)sometimes the same

D)not related

E)mirror images of one another

Q3) XeF₄ is a polar molecule.

A)True

B)False

Q4) Three molecules have similar electron domains,but different molecular shapes.Why?

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11

Chapter 10: Gases

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Sample Questions

Q1) A sample of hydrogen gas (3.2 L)at 3.5 atm and 25 °C was combined with 5.2 L of nitrogen gas at 7.3 atm and 25 °C at constant temperature in a 15.0 L flask.Assuming the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C,what is the total pressure (atm)in the flask?

A)3.28

B)5.85

C)9.45

D)15.4

E)10.8

Q2) A 0.133 mol sample of gas in a 525 mL container has a pressure of 312 torr.The temperature of the gas is ________ °C.

A)20.3

B)-253

C)-20.3

D)203

E)22.4

Q3) The deviation from ideal behavior of a gas is most evident at ________ and/or low temperature.

Q4) What is the rms speed (m/s)of oxygen molecules at 36.0 °C?

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Chapter 11: Liquids and Intermolecular Forces

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Sample Questions

Q1) Viscosity is ________.

A)the "skin" on a liquid surface caused by intermolecular attraction

B)the resistance to flow

C)the same as density

D)inversely proportional to molar mass

E)unaffected by temperature

Q2) The intermolecular force(s)responsible for the fact that CH₄ has the lowest boiling point in the set

CH₄,CH₃CH₃,CH₃CH₂CH< sub>3</sub>,CH₃CH₂CH₂CH₃ is/are

A)hydrogen bonding

B)London dispersion forces

C)mainly hydrogen bonding but also dipole-dipole interactions

D)dipole-dipole interactions

E)mainly London-dispersion forces but also dipole-dipole interactions

Q3) The initial discovery of a liquid crystal resulted from studies of a ________ derivative.

Q4) The conversion of a solid to a liquid is called ________.

Q5) London Dispersion Forces tend to ________ in strength with increasing molecular weight.

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Chapter 12: Solids and Modern Materials

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Sample Questions

Q1) Which statement best describes the classification of Sterling silver?

A)It is pure silver.

B)It is oxidized silver.

C)It is an alloy of silver.

D)It is a mixture of silver and gold.

E)It is a liquid at room temperature.

Q2) The unit cell with all sides the same length and all angles equal to 90° that has lattice points only at the corners is called ________.

A)monoclinic

B)body-centered cubic

C)primitive cubic

D)face-centered cubic

E)spherical cubic

Q3) What is the percent gold in a 10 karat gold necklace?

A)10

B)58

C)90

D)1.0 × 10²

E)42

Q4) What are semiconductors?

Page 14

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Chapter 13: Properties of Solutions

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Sample Questions

Q1) A solution contains 11% by mass of sodium chloride.This means that ________.

A)there are 11 g of sodium chloride in in 1.0 mL of this solution

B)100 g of the solution contains 11 g of sodium chloride

C)100 mL of the solution contains 11 g of sodium chloride

D)the density of the solution is 11 g/mL

E)the molality of the solution is 11

Q2) A 0.200 m solution of which one of the following solutes will have the lowest vapor pressure?

A)LiCl

B)AlCl₃

C)CaCl₂

D)glucose

E)KCl

Q3) Which of the following liquids will have the lowest freezing point?

A)pure H₂O

B)aqueous glucose (0.60 m)

C)aqueous sucrose (0.60 m)

D)aqueous FeI₃ (0.24 m)

E)aqueous KF (0.50 m)

Q4) What is the formula weight of iron(III)chloride hexahydrate?

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Chapter 14: Chemical Kinetics

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Sample Questions

Q1) As the temperature of a reaction is increased,the rate of the reaction increases because the ________.

A)reactant molecules collide less frequently

B)reactant molecules collide more frequently and with greater energy per collision

C)activation energy is lowered

D)reactant molecules collide with greater energy

E)reactant molecules collide more frequently

Q2) At elevated temperatures,methylisonitrile (CH₃NC)isomerizes to acetonitrile (CH₃CN): CH₃NC (g) CH₃CN (g)

At the start of an experiment,there are 0.200 mol of reactant and 0 mol of product in the reaction vessel.After 25 min,0.121 mol of reactant (CH₃NC)remain.There are ________ mol of product (CH₃CN)in the reaction vessel.

A)0.022

B)0.121

C)0.200

D)0.321

E)0.079

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Page 16

Chapter 15: Chemical Equilibrium

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Sample Questions

Q1) Define the reaction quotient.

Q2) If the value for the equilibrium constant is much less than 1,then the equilibrium mixture contains mostly ________.

Q3) If Reaction A + Reaction B = Reaction C,then K_c for Reaction C is ________.

Q4) If the reaction quotient Q for a reaction is equal to the value of the equilibrium constant K for that reaction at a given temperature,then the reaction is at ________.

Q5) The relationship between the concentrations of reactants and products of a system at equilibrium is given by the law of energy.

A)True

B)False

Q6) Which one of the following will change the value of an equilibrium constant?

A)changing temperature

B)adding other substances that do not react with any of the species involved in the equilibrium

C)varying the initial concentrations of reactants

D)varying the initial concentrations of products

E)changing the volume of the reaction vessel

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) Of the following,which is the strongest acid?

A)HIO₄

B)HIO₃

C)HIO₂

D)HIO

E)The acid strength of all of the above is the same.

Q2) A Br nsted-Lowry base is defined as a substance that ________.

A)increases [H⁺] when placed in H₂O

B)decreases [H⁺] when placed in H₂O

C)increases [OH^-] when placed in H₂O

D)acts as a proton acceptor

E)acts as a proton donor

Q3) Calculate the concentration (in M)of hydronium ions in a solution at 25.0 °C with a pOH of 3.58.

A)2.63 × 10^-4

B)2.63 × 10¹⁰

C)3.80 × 10^-11

D)3.80 × 10³

E)1.00 × 10^-7

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Page 18

Chapter 17: Additional Aspects of Aqueous Equilibria

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Sample Questions

Q1) In which of the following aqueous solutions would you expect AgF to have the highest solubility?

A)0.00750 M LiF

B)0.030 M AgNO₃

C)0.023 M NaF

D)0.015 M KF

E)AgF will have the same solubility in all solutions.

Q2) What is the molar solubility of calcium carbonate ( CaCO₃ )in water? The solubility-product constant for CaCO₃ is 4.5 × 10^-9 at 25 °C.

A)2.3 × 10^-9

B)9.0 × 10^-9

C)8.35

D)9.5 × 10^-5

E)6.7 × 10^-5

Q3) Metal oxides and hydroxides that are relatively insoluble in neutral water,but are soluble in both strongly acidic and strongly basic solutions are said to be ________.

Q4) ________ analysis determines how much of a given substance is present.

Q5) CaCO₃ is very soluble in the presence of ________.

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Chapter 18: Chemistry of the Environment

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Sample Questions

Q1) In the troposphere,temperature ________ with increasing altitude,while in the stratosphere,temperature ________ with increasing altitude.

A)increases, increases

B)decreases, decreases C)increases, decreases

D)decreases, increases E)decreases, remains constant

Q2) In the past,CFCs were used in which of the following?

A)spray cans

B)plastic manufacturing

C)air conditioners

D)refrigerators

E)all of the above

Q3) Which of the following is released by the combustion of fossil fuels?

A)N₂

B)CO₂

C)H₂

D)O₂

E)O₃

Q4) The stratosphere contains approximately ________ of the earth's ozone.

Page 20

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Chapter 19: Chemical Thermodynamics

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Sample Questions

Q1) The value of S° for the catalytic hydrogenation of acetylene to ethene, C₂H₂ (g)+ H₂ (g) C₂H₄ (g)

Is ________ J/K mol.

A)+18.6

B)+550.8

C)+112.0

D)-112.0

E)-18.6

Q2) The value of H° for the formation of calcium chloride from its constituent elements, Ca (s)+ Cl₂ (g) CaCl₂ (s) Is ________ kJ/mol.

A)0.00

B)-397.9

C)+397.9

D)-795.8

E)+795.8

Q3) What is the G° (kJ/mol)for the formation of silver chloride at 25 °C? K_sp = 1.8 × 10^-10

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Page 21

Chapter 20: Electrochemistry

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Sample Questions

Q1) Define a coulomb.

Q2) In a voltaic cell,electrons flow from the ________ to the ________.

A)salt bride, anode

B)anode, salt bridge

C)cathode, anode

D)salt bridge, cathode

E)anode, cathode

Q3) What is the correct coefficient for the electrons in the following half-reaction: Ni⁶⁺ + ___e^- Ni

A)6

B)1

C)2

D)3

E)5

Q4) The loss of electrons by an element is called ________.

A)fractionation

B)reduction

C)disproportionation

D)oxidation

E)sublimation

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Chapter 21: Nuclear Chemistry

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Sample Questions

Q1) The basis for the carbon-14 dating method is that ________.

A)the amount of carbon-14 in all objects is the same

B)carbon-14 is very unstable and is readily lost from the atmosphere

C)the ratio of carbon-14 to carbon-12 in the atmosphere is a constant

D)living tissue will not absorb carbon-14 but will absorb carbon-12

E)All of the above are correct.

Q2) The product of the nuclear reaction in which ²⁸Si is subjected to neutron capture followed by alpha emission is ________.

A).³¹S

B).³³S

C).²³Mg

D).²⁵Mg

E).²⁵Al

Q3) Due to the nature of the positron,________ is actually detected in positron emission tomography.

A)alpha radiation

B)beta radiation

C)gamma radiation

D)x-ray emission

E)neutron emission

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Chapter 22: Chemistry of the Nonmetals

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Sample Questions

Q1) D₂O,deuterium oxide,is also known as ________.

Q2) What process replenishes O₂?

Q3) What group 5A element is the least metallic?

Q4) Hydrogen peroxide is a highly polar and strongly hydrogen-bonded liquid.It decomposes to form water and ________.

Q5) Group 8A elements are all gases at room temperature except for ________.

Q6) What is the primary commercial source of elemental nitrogen?

Q7) What sulfur gas is used to sterilize wine?

Q8) The oxidation numbers of nitrogen in the nitride ion,hydrazine,ammonium cation,and nitrate ion are ________,________,________,and ________,respectively.

A)-3, -2, -3, +5

B)+3, -2, -3, +5

C)+3, -2, +1, +3

D)-3, +2, +1, +5

E)-3, +2, -3, +3

Q9) In oxygen compounds,a disproportionation reaction is a reaction in which oxygen is simultaneously ________.

Q10) What noble gas is radioactive?

Q11) Compounds containing only boron and hydrogen are called ________. Page 24

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Page 25

Chapter 23: Transition Metals and Coordination Chemistry

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Sample Questions

Q1) What is the ligand in Ca₃[Fe(CN)₆]₂?

A)Ca²⁺

B)Fe³⁺

C)CN^-

D)Fe(CN)₆^3-

E)Fe²⁺

Q2) Name the compound:

K₂[Cr(H₂O)₄(CO₃)₂].

Q3) Non superimposable isomers are ________ isomers.

Q4) Complexes containing metals with d¹⁰ electron configurations are typically ________.

A)violet

B)blue

C)green

D)yellow

E)white/colorless

Q5) Green and orange are complementary colors.

A)True

B)False

Q6) A substance is ________ if its ions or atoms have zero unpaired electrons.

Page 26

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Chapter 24: The Chemistry of Life: Organic and Biological Chemistry

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Sample Questions

Q1) ________ could be the formula of an alkene.

A)C₃H₈

B)C₃H₆

C)C₆H₆

D)C₁₇H₃₆

E)CH₈

Q2) Which one of the following could be a cycloalkane?

A)C₆H₅

B)C₃H₅

C)C₂H₆

D)C₁₀H₂₂

E)C₅H₁₀

Q3) The minimum number of carbons necessary for a hydrocarbon to form a branched structure is ________.

A)4

B)6

C)3

D)9

E)12

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Q4) What is the electron group geometry surrounding the carbon atoms in alkanes?