General Chemistry II Study Guide Questions - 3323 Verified Questions

Course Introduction

General Chemistry II Study Guide Questions

General Chemistry II is a continuation of foundational chemical principles with an emphasis on topics such as chemical kinetics, chemical equilibria, acids and bases, thermodynamics, electrochemistry, and introductory concepts in coordination chemistry. This course deepens students' understanding of molecular structure, reactions in aqueous solutions, and the energetic changes involved in chemical processes. Laboratory exercises and problem-solving strategies are integrated to enhance practical skills, critical thinking, and application of theoretical concepts to real-world chemical phenomena.

Recommended Textbook

General Chemistry Principles and Modern Applications 11th Edition by Ralph H. Petrucci

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28 Chapters

3323 Verified Questions

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Page 2

Chapter 1: Matter: Its Properties and Measurement

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Sample Questions

Q1) Which of the following is a physical property?

A)the density of lead

B)sulfur burns in oxygen to form sulfur trioxide

C)ozone reacts with silver to give silver oxide

D)platinum metal does not react with hydrochloric acid

Answer: A

Q2) What is 21.1 miles/hour in furlongs/fortnight? (8 furlongs = 1 mile;14 days = 1 fortnight)

A)0.502 furlongs/fortnight

B)8.862 × 10³furlongs/fortnight

C)5.67 × 10⁴furlongs/fortnight

D)8.86 × 10³furlongs/fortnight

E)5.672 × 10⁴furlongs/fortnight

Answer: C

Q3) Round off 00907506 to four significant figures.

A)0091

B)9076

C)9100

D)9.075 × 10⁵

Answer: D

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Page 3

Chapter 2: Atoms and the Atomic Theory

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Sample Questions

Q1) What is the mass number of the most abundant form of oxygen atom?

A)15.9994

B)8

C)16

D)24

E)32

Answer: C

Q2) A certain mass of nickel reacts with sulphur to produce 2.83 g of NiS.The same mass of nickel reacts completely with 0.5 g of oxygen to produce 2.33 g of NiO.How many grams of sulfur reacted in the first reaction?

A)0.5 g

B)1 g

C)1.5 g

D)10^-1 g

E)1.25 g

Answer: B

Q3) Atoms combine in small,whole-numbered ratios.

A)True

B)False Answer: True

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Chapter 3: Chemical Compounds

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Sample Questions

Q1) The oxidation state of vanadium in VO²⁺ is ________.

A)-2

B)+2

C)+1

D)-4

E)+4

Answer: E

Q2) What is the mass of 8.50 × 10²² molecules of NH₃?

A)0.00829 g

B)0.417 g

C)2.40 g

D)121 g

Answer: C

Q3) What is the empirical formula of a substance that contains 5.28 g of C,1.11 g of H,and 3.52 g of O?

A)C₂HO₅

B)C₂H₄O₂

C)C₂H₄O₃

D)C₃H₄O₄

Answer: A

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Chapter 4: Chemical Reactions

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Sample Questions

Q1) When 31.2 mL of 0.500 mol L^-1 AgNO₃(aq)is added to 25.0 mL of 0.300 mol L^-1 NH₄Cl(aq),how many grams of AgCl are formed?

AgNO₃(aq)+

NH₄Cl(aq) AgCl(s)+ NH₄NO₃(aq)

A)1.07 g

B)2.24 g

C)3.31 g

D)6.44 g

Q2) A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150 mL of solution.She then took 15.0 mL of the stock solution and diluted it with enough water to make 65.0 mL of a final solution.What is the concentration of KOH for the final solution?

A)0.274 mol L^-1

B)0.356 mol L^-1

C)2.81 mol L^-1

D)3.65 mol L^-1

Q3) The reactant that is in excess determines the amount of products formed.

A)True

B)False

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Chapter 5: Introduction to Reactions in Aqueous Solutions

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Sample Questions

Q1) Write the net ionic equation for the reaction of lead(II)nitrate and sodium iodide.

A)Pb(NO₃)₂(aq)+ 2 NaI(aq) PbI₂(s)+ 2 NaNO₃(aq)

B)Pb²⁺(aq)+ 2 NaI(aq) PbI₂(s)+ 2 Na

C)Pb²⁺(aq)+ 2 I^-(aq) PbI₂(s)

D)Pb²⁺(aq)+ 2 I^-(aq) Pb²⁺(aq)+ 2 I^-(aq)

E)no reaction

Q2) What reagent could be used to separate Br^- from CH₃CO₂^-when added to an aqueous solution containing both?

A)AgNO₃(aq)

B)Ba(OH)₂(aq)

C)CuSO₄(aq)

D)NaI_(aq)

Q3) An insoluble compound will dissolve to an appreciable amount in water.

A)True

B)False

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Chapter 6: Gases

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Sample Questions

Q1) The fact that a balloon filled with helium will leak more slowly than one filled with hydrogen is explained by citing:

A)Avogadro's Hypothesis

B)Dalton's Law

C)Graham's Law

D)van der Waals Theory

E)ideal gas law

Q2) A 34.8 mL sample of an unknown,water-insoluble gas was collected over water at 22.6 °C and a barometric pressure of 0.895 atm.When the gas was dried and chilled,it formed 114.6 mg of liquid.What was the molar mass of this substance? [The vapor pressure of water at 22.6 °C is 20.mmHg]

A)22.9 g/mol

B)38.4 g/mol

C)57.3 g/mol

D)84.2 g/mol

E)92.0 g/mol

Q3) Gas densities depend strongly on gas temperature and pressure.

A)True

B)False

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Page 8

Chapter 7: Thermochemistry

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Sample Questions

Q1) Calculate _fH° of octane,C₈H₁₈(l),given the enthalpy of combustion of octane to CO₂(g)and H₂O(l),-5471 kJ/mol,and the standard enthalpies of formation of CO₂(g)and H₂O(l),-393.5 kJ/mol and -285.8 kJ/mol,respectively.

A)-249.2 kJ/mol

B)+4792 kJ/mol

C)+249.2 kJ/mol

D)-4792 kJ/mol

Q2) Calculate the work needed to make room for products in the combustion of sulfur,S₈(s),to SO₂(g)at STP.

A)0 kJ

B)-2.27 kJ

C)-4.54 kJ

D)-18.2 kJ

E)+182 kJ

Q3) The enthalpy of a system is the internal energy minus the pressure-volume product.

A)True

B)False

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9

Chapter 8: Electrons in Atoms

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Sample Questions

Q1) The following orbitals are placed in the correct filling order: 6s,4f,5d,6p.

A)True

B)False

Q2) What is the energy in joules of the 656 nm spectral line of hydrogen?

A)4.35 × 10^-31J

B)3.03 × 10^-19J

C)1.30 × 10^-22J

D)3.03 × 10^-28J

E)1.45 × 10^-48J

Q3) Use the spdf notation to write out the complete electron configuration of Br.

A)[Ar] 3d¹⁰4s²4p⁵

B)[Kr] 3d¹⁰4s²4p⁴

C)[Ar] 3d⁹4s²4p⁶

D)[Ar] 3d¹⁰4p⁶5s²

E)[Ar] 4s²4p²4d⁹

Q4) When an electron in an atom goes from a high energy state to a low one,light is given off.

A)True

B)False

Page 10

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Chapter 9: The Periodic Table and Some Atomic Properties

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Sample Questions

Q1) List in order of increasing number of unpaired electrons: N,Na,Si,Cr,Ar.

A)Cr < Si < Na < N < Ar

B)Ar < Cr < N < Na < Si

C)Ar < Cr < Si < Na < N

D)N < Na < Cr < Si < Ar

E)Ar < Na < Si < N < Cr

Q2) Which of the following has the most unpaired electrons: Na,MnS1U1P12+ S1S1P0,S,N,Ar?

A)Na

B)MnS1U1P12+ S1S1P0

C)S

D)N

E)Ar

Q3) The similar chemical behavior of the elements in a given group in the periodic table is best accounted for by the fact that atoms of these elements have:

A)the same number of isotopes

B)the same number of electrons

C)the same number of electrons in the outermost (valence)shell

D)similar nuclear structures

E)the same number of protons

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Page 11

Chapter 10: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) After drawing the Lewis dot structure for PCl_3,determine the number of single bond(s),double bond(s),and lone pair(s)on the central atom.

A)single bond(s)= 2,double bond(s)= 1,lone pair(s)= 1

B)single bond(s)= 3,double bond(s)= 0,lone pair(s)= 1

C)single bond(s)= 2,double bond(s)= 0,lone pair(s)= 2

D)single bond(s)= 3,double bond(s)= 1,lone pair(s)= 0

E)single bond(s)= 3,double bond(s)= 1,lone pair(s)= 1

Q2) Arrange the following in order of increasing electronegativity: Cs,F,As,Cl.

A)As < Cl < Cs < F

B)Cl < As < F < Cs

C)As < F < Cs < Cl

D)Cl < Cs < F < As

E)Cs < As < Cl < F

Q3) Which of the following species has a trigonal pyramidal structure?

A)ClO₃^-

B)ClO₄^-

C)ClO₂^-

D)ClO₂

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Page 12

Chapter 11: Chemical Bonding Ii: Valence Bond and

Molecular Orbital Theories

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Sample Questions

Q1) Three of the molecular shapes which a sp³^d hybridized molecule can have are:

A)triangular,trigonal bipyramid,linear

B)linear,square planar,T-shaped

C)irregular tetrahedron,T-shaped,bent

D)T-shaped,linear,trigonal bipyramid

E)linear,tetragonal pyramid,octahedral

Q2) Using the VSEPR model,the molecular geometry of the central atom in NCl₃ is:

A)linear

B)trigonal planar

C)tetrahedral

D)bent

E)trigonal pyramidal

Q3) What geometric arrangement of charge clouds is expected for an atom that has four charge clouds?

A)trigonal bipyramidal

B)octahedral

C)tetrahedral

D)square planar

Page 13

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Chapter 12: Intermolecular Forces: Liquids and Solids

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Sample Questions

Q1) A crystal and its melt readily conduct electricity.The crystal also has a luster and is easily deformed.Thus,it is:

A)a covalent network crystal

B)an ionic crystal

C)a metallic crystal

D)a molecular crystal

E)a covalent crystal

Q2) The property of a liquid that measures its resistance to flow is called resistivity.

A)True

B)False

Q3) The phenomenon in which a steel needle can,with proper care,be made to float on the surface of some water illustrates a property of liquids known as:

A)compressibility

B)polarizability

C)surface tension

D)triple point

E)viscosity

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14

Chapter 13: Spontaneous Change: Entropy and Gibbs Energy

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Sample Questions

Q1) How much heat is released when 85.0 g of steam at 100.0 °C is cooled to ice at -15.0 °C? The enthalpy of vaporization of water is 40.67 kJ mol^-1,the enthalpy of fusion for water is 6.01 kJ mol^-1,the molar heat capacity of liquid water is 75.4 J mol^-1 °C^-1,and the molar heat capacity of ice is 36.4 J mol^-1 °C^-1.

A)54.8 kJ

B)221 kJ

C)258 kJ

D)281 kJ

Q2) For CdO(s)+ SO₃(g) CdSO₄(s), _rH° = -279.4 kJ/mol,and _rS° = -118.4 J/mol K.What is the temperature at which K_eq is 1.0 × 10⁴?

A)1890 °C

B)6950 °C

C)1160 °C

D)1710 °C

E)6410 °C

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Chapter 14: Solutions and Their Physical Properties

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Sample Questions

Q1) A solution composed of 5 moles of acetone (CH₃COCH₃,P°_A = 324 mmHg)and 5 moles of chloroform (CHCl₃,P° = 274 mmHg)has a vapor pressure of 236 mmHg.Which one of the following statements is completely true about this solution?

A)The solution shows a negative deviation from Raoult's law and thus possesses a maximum boiling azeotrope.

B)The solution process is exothermic because the forces between unlike molecules are weaker than those between like molecules.

C)The solution shows a positive deviation from Raoult's law.

D)The solution possesses a minimum boiling azeotrope because it shows a negative deviation from Raoult's law.

E)The solution obeys Raoult's Law.

Q2) Which of the following is a true solution with particles less than 1 nm in size?

A)calcium chloride in water

B)oil in water

C)whipped cream

D)milk

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Page 16

Chapter 15: Principles of Chemical Equilibrium

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Sample Questions

Q1) Large value for equilibrium constant K means the reaction will be less complete at the equilibrium point.

A)True

B)False

Q2) At a certain temperature,K_c = 0.0500 and _rH° = +39.6 kJ for the reaction below.

2 MgCl₂(s)+ O₂(g) 2 MgO(s)+ 2 Cl₂(g)

Calculate K_c for the reaction MgO(s)+ Cl₂(g) MgCl₂(s)+ 1/2 O₂(g)

And indicate whether its value will be larger or smaller at a lower temperature.

A)4.47,larger

B)400,smaller

C)0.224,larger

D)0.224,smaller

E)0.0025,smaller

Q3) Both products and reactants will be present in an equilibrium reaction unless K is very small or very large.

A)True

B)False

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Page 17

Chapter 16: Acids and Bases

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Sample Questions

Q1) Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.010 mol L^-1aqueous H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

A)6.6 × 10^-⁵ mol L^-1

B)4.3 × 10^-7 mol L^-1

C)4.3 × 10^-⁹ mol L^-1

D)5.6 × 10^-11 mol L^-1

Q2) Choose the strongest acid.

A)HF

B)H₂CO₃

C)HCN

D)HC₂H₃O₂

E)HClO₄

Q3) What is the hydroxide ion concentration of a lye solution that has a pH of 9.20?

A)6.3 × 10^-¹⁰ mol L^-1

B)1.6 × 10^-⁵ mol L^-1

C)4.8 mol L^-1

D)9.2 mol L^-1

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Page 18

Chapter 17: Additional Aspects of Acidbase Equilibria

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Q1) What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 NH₃ with 5.00 mL of 0.10 mol L^-1 NH₄Cl?

Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

A)8.25

B)9.28

C)10.26

D)11.13

Q2) What is the pH of a solution made by dissolving 2.16 g of sodium benzoate (NaC₆H₅CO₂)in a sufficient volume of 0.033 M aqueous benzoic acid solution to prepare 500.0 mL of buffer? [K_a for benzoic acid is 6.3 × 10^-5]

A)4.16

B)4.37

C)4.64

D)5.77

E)6.30

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Chapter 18: Solubility and Complex-Ion Equilibria

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Sample Questions

Q1) Predict the molar solubility of the following salt in an aqueous solution that contains the given concentration of one of its ions:

BaSO₄;[SO₄^2-] = 4.3 × 10^-5 M;K_sp = 1.1 × 10^-10

A)4.7 × 10^-15 M

B)6.9 × 10^-8 M

C)8.0 × 10^-4 M

D)2.6 × 10^-6 M

E)1.6 × 10^-3 M

Q2) If iron(III)acetate is added to be 1 × 10^-10 M in an aqueous solution that is 0.10 M NH₃,what is Q_spand will Fe(OH)₃ precipitate? The K_sp of Fe(OH)₃(s)is 4 × 10^-38 and K_b for NH₃ is 1.8 × 10^-5.

A)1.3 × 10^-13,yes

B)1.7 × 10^-16,yes

C)1.7 × 10^-16,no

D)2.4 × 10^-19,yes

E)2.4 × 10^-19,no

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Chapter 19: Electrochemistry

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Sample Questions

Q1) What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below?

Al(s) Al³⁺(aq) Fe²⁺(aq) Fe(s)

A)2 Al(s)+ 3 Fe²⁺(aq) 2 Al³⁺(aq)+ 3Fe(s)

B)3 Al(s)+ 2 Fe²⁺(aq) 3 Al³⁺(aq)+ 2 Fe(s)

C)2 Fe(s)+ 3 Al³⁺(aq) 2 Fe²⁺(aq)+ 3 Al(s)

D)3 Fe(s)+ 2 Al³⁺(aq) 3 Fe²⁺(aq)+ 2 Al(s)

Q2) Choose the INCORRECT statement.

A)SHE stands for Standard Helium Electrodes.

B)E° is the standard electrode potential.

C)The standard electrode potential is the reduction potential of a half cell.

D)The standard cell potential is the potential difference between two half cells.

E)E°_cell is the standard cell potential.

Q3) Choose the INCORRECT statement.

A)Corrosion of metals is an oxidation reduction process.

B)Rust is a form of corrosion.

C)Metals can be protected by cathodic protection.

D)Cathodic protection is attaching a more active metal to the protected metal.

E)The active metal is called a sacrificial cathode.

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Page 21

Chapter 20: Chemical Kinetics

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Q1) For the reaction: C₂H₄Br₂ + 3 KI

C₂H₄+ 2 KBr + KI₃,when the rate of disappearance of C₂H₄Br₂ is 2.0 × 10^-5 M/s,what is the rate of appearance of C₂H₄?

A)0.67 × 10^-5 M/s

B)2.0 × 10^-5 M/s

C)4.0 × 10^-5 M/s

D)6.0 × 10^-5 M/s

E)1.0 × 10^-5 M/s

Q2) For the second order reaction A products,the following data are obtained:

[A] = 1.512 M,t = 0 min

[A] = 1.490 M,t = 1.0 min

[A] = 1.469 M,t = 2.0 min

What is the concentration of [A] in the experiment after 4.0 min for the reaction?

A)1.43 M

B)1.35 M

C)1.61 M

D)1.39 M

E)1.37 M

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Page 22

Chapter 21: Chemistry of the Main-Group Elements I:

Groups 1,2,13,and 14

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Q1) What potential would be expected from a galvanic cell using a solid magnesium/0.20 M Mg²⁺(aq)half-cell with a solid thallium/0.010 M Tl⁺(aq)half-cell [for Mg²⁺(aq)+ 2 e^- = Mg(s),E° = -2.36 V;for Tl⁺(aq)+ e^- = Tl(s),E° = -0.34 V]?

A)3.04 V

B)1.92 V

C)1.68 V

D)2.70 V

E)2.02 V

Q2) Write the general reaction for a group 1 (1A)metal with water.

A)2 M(s)+ 2 H₂O(l) H₂O₂(aq)+ 2 MH(s)

B)2 M(s)+ 2 H₂O(l) 2 MOH(aq)+ H₂(g)

C)M(s)+ H₂O(l) MO(s)+ H₂(g)

D)2 M(s)+ H₂O(l) M₂O(s)+ H₂(g)

E)2 M(s)+ 2H₂O(l) M(OH)₂(s)+ H₂(g)

Q3) In a nonmetal hydroxide the oxygen-hydrogen bond is generally less polar than the nonmetal-oxygen bond.

A)True

B)False

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Chapter 22: Chemistry of the Main-Group Elements Ii:

Groups 18,17,16,15,and Hydrogen

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Q1) Write the equation for commercially extracting bromine from seawater.

A)Br₂(l)+ 2 Cl(aq) Cl₂(g)+ 2 Br^-(aq)

B)2 Br^-(aq)+ I₂(s) Br₂(l)+ 2 I^-(aq)

C)4 Br^-(aq)+ Cl₂(g) Br₂(l)+ 2 BrCl(aq)

D)2 Br^-(aq)+ F₂(g) Br₂(l)+ 2 F^-(aq)

E)2 Br^-(aq)+ Cl₂(g) Br₂(l)+ 2 Cl^-(aq)

Q2) In the compound dinitrogen monoxide,sometimes used as a dental anesthetic,the oxidation state of nitrogen is ________. A)+1

B)-1

C)+2 D)-2

E)0

Q3) Which of the following oxides is neither acidic nor amphoteric?

A)As₂O₅

B)Bi₂O₃

C)N₂O₃

D)P₄O₆

E)Sb₂O₃

Page 24

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Chapter 23: The Transition Elements

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Q1) The coinage metals are copper,silver,and zinc.

A)True

B)False

Q2) Which of the following forms a colorless aqueous solution?

A)CuClO₄

B)CoSO₄

C)NiCl₂

D)FeCl₃

Q3) List the following in order of increasing number of unpaired electrons: Fe,V,Sc,Mn

A)Mn < Fe < V < Sc

B)Sc < V < Fe < Mn

C)Fe < V < Sc < Mn

D)V < Sc < Mn < Fe

E)Sc < Mn < Fe < V

Q4) Pig iron comes from the blast furnace.

A)True

B)False

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25

Chapter 24: Complex Ions and Coordination Compounds

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Q1) Choose the correct shape,weak or strong field,and number of unpaired electrons for [CoCl₄]^2-.

A)square planar,strong,3

B)square planar,strong,0

C)tetrahedral,strong,1

D)tetrahedral,weak,3

E)square planar,weak,0

Q2) Which of the following is a bidentate ligand?

A)H₂O

B)NO₂^-

C)NH₃

D)H₂NCH₂CH₂NH₂

E)[(O₂C)₂NCH₂CH₂N(CO<sub>2</sub >)₂]^4-

Q3) Choose the INCORRECT statement about isomers.

A)Structural isomers differ in structure or bond type.

B)stereoisomers differ in the spatial arrangements among the ligands.

C)Ionization isomers differ in the charge on the central ion.

D)Linkage isomers differ in which atom is bonded to the central atom.

E)Geometric isomerism is cis-trans isomerism.

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Chapter 25: Nuclear Chemistry

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Q1) Choose the INCORRECT statement.

A)Radioactive ³²P as a phosphate can be used to trace the uptake of phosphorus in plants.

B)The thyroid gland can be studied by the use of radioactive iodine.

C)There is no difference in physical properties between isotopes.

D)The mechanism of a chemical reaction can be followed by a radioactive tracer such as ³⁵S.

E)Industrial catalysts can be followed by a tracer such as ¹⁹²Ir.

Q2) Choose the correct word to describe the nuclear stability of the following isotope.If it is radioactive,choose the most likely mode of decay. ¹⁹F

A)radioactive,beta

B)radioactive,fission

C)radioactive,alpha

D)radioactive,neutron

E)stable

Q3) Ion production is the way radiation causes the most damage.

A)True

B)False

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Page 27

Chapter 26: Structures of Organic Compounds

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99 Verified Questions

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Sample Questions

Q1) Which of the following has the lowest melting point: cyclohexane,hexane,benzene?

A)cyclohexane

B)hexane

C)benzene

D)They have approximately the same melting point.

E)There is not enough information to determine.

Q2) A solid wedge line denotes a bond that sticks back behind the plane of the paper.

A)True

B)False

Q3) A conformation is a set of all possible optical isomers of an organic compound of a given molecular formula.

A)True

B)False

Q4) Name the following compound:

CH₃CH₂NHCH₃.

A)aminopropane

B)aminomethylethane

C)methylaminoethane

D)propylamine

E)ethylmethylamine

28

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Chapter 27: Reactions of Organic Compounds

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Sample Questions

Q1) Which of the following are nucleophiles?

I.CH₃COCH₃

II.CH₃Br

III.CH₃CH₂C C^-

A)I

B)II

C)III

D)I + II

E)I + III

Q2) S_N2 reactions are nucleophilic substitution reactions for which the rate determining step is bimolecular.

A)True

B)False

Q3) The initiation step in chain reaction for alkene substitution produces:

A)free halogen radicals

B)free alkyl radicals

C)both free halogen and alkyl radicals

D)free halonium ions

E)free halide ions

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Chapter 28: Chemistry of the Living State

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104 Verified Questions

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Sample Questions

Q1) Choose the INCORRECT statement.

A)Lipids are hydrocarbons with basic properties.

B)The acyl groups of triglycerides are fatty acids.

C)A mixed triglyceride has different acyl groups.

D)Lipids are constituents of plant and animal tissues that are soluble in solvents of low polarity.

E)Triglycerides are esters of glycerol with long-chain monocarboxylic acids.

Q2) Which of the following structural elements cannot be found in DNA?

A)purine

B)pentose

C)phosphate

D)heme

E)pyrimidine

Q3) Find a mismatch in the following body part - food metabolism pairs:

A)mouth - starch

B)small intestine - polysaccharides

C)small intestine - fats and oils

D)stomach - proteins

E)stomach - small peptides

Q4) The hydrolysis of tristearin produces the soap potassium stearate and ________.

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