General Chemistry II Exam Solutions - 4331 Verified Questions

General Chemistry II

Exam Solutions

Course Introduction

General Chemistry II builds on foundational concepts from introductory chemistry, exploring more advanced topics such as chemical kinetics, chemical equilibrium, acid-base theories, thermodynamics, electrochemistry, and coordination compounds. The course emphasizes problem-solving and the application of theoretical principles to real-world chemical systems. Laboratory experiments complement lecture material, providing hands-on experience with quantitative analysis, reaction mechanisms, and the interpretation of experimental data. This course prepares students for further study in chemistry and related scientific fields.

Recommended Textbook Chemistry 6th Edition by John E. McMurry

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23 Chapters

4331 Verified Questions

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Page 2

Chapter 1: Chemistry: Matter and Measurement

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Sample Questions

Q1) If hitting the bull's-eye is the desired result,Figure (b)represents

A)good accuracy and good precision.

B)good accuracy and poor precision.

C)poor accuracy and good precision.

D)poor accuracy and poor precision.

Answer: A

Q2) A preliminary explanation of the results of many experiments that can be used to make predictions and suggest further experimentations is a ________.

Answer: hypothesis

Q3) The number of significant digits in 0.07090 g is ________. Answer: four

Q4) Which of the following is the smallest volume?

A)44 cm³

B)1)0 dL

C)5)5 × 10³ mL

D)1)0 × 10⁸ nL

Answer: A

Q5) The quantity 1.0567 qt rounded to two significant figures is ________ qt. Answer: 1.1

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) Beta decay of ³²P produces a beta particle and A)(²⁸Al.)

B)(³¹P.)

C)(³²Si.)

D)(³²S.)

Answer: D

Q2) If shaded and unshaded spheres represent atoms of different elements,which of the above drawings most likely represents an ionic compound at room temperature and a pressure of 1 atm?

A)drawing (a)

B)drawing (b)

C)drawing (c)

D)drawing (d)

Answer: A

Q3) Gamma radiation can be described as

A)a helium nucleus.

B)a negatively charged free electron.

C)high energy electromagnetic radiation.

D)a positively charged free electron.

Answer: C

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Chapter 3: Formulas, equations, and Moles

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Sample Questions

Q1) Balance the chemical equation given below,and determine the number of grams of MgO are needed to produce 10.0 g of Fe₂O₃.

_____ MgO(s)+ _____ Fe(s) _____ Fe₂O₃(s)+ _____ Mg(s)

A)0)312 g

B)0)841 g

C)2)52 g

D)7)57 g

Answer: D

Q2) Which one of the following contains 39% carbon by mass?

A)C₂H₂

B)CH₄

C)CH₃NH₂

D)CO₂

Answer: C

Q3) What is the mass of 8.50 x 10²² molecules of NH₃?

A)0)00 829 g

B)0)417 g

C)2)40 g

D)121 g

Answer: C

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Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) Predict the products of a reaction between AgNO₃(aq)and KBr(aq).

A)Ag(s)and NO(g)

B)Ag(s)and Br₂(l)

C)AgBr(s)and KNO₃(aq)

D)AgNO₃(aq)and KBr(aq)

Q2) The compound K₂S is predicted to be soluble based on the solubility guideline that all ________ are soluble.

Q3) What is the oxidation number of the oxygen atom in H₂O₂?

A)-2

B)-1

C)+1 D)+2

Q4) Which outcome corresponds to the mixing of potassium and sulfide ions shown in the following equation?

2 K⁺(aq)+ S^2-(aq) ?

A)box (a)

B)box (b)

C)box (c)

D)None of these

Q5) The oxidation number of hydrogen in CaH₂ is ________.

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Chapter 5: Periodicity and the Atomic Structure of Atoms

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Sample Questions

Q1) How many unpaired electrons are in an atom of Co in its ground state?

A)1

B)2

C)3

D)7

Q2) The laser used to read Blu-Ray discs have a wavelength of 405 nm.405 nm photons have of an energy of ________ J,and a mole of 405 nm photons has an energy of ________ kJ/mol.

Q3) Which of the following elements would you predict to have an anomalous electron configuration?

A)Ag

B)Ce

C)Se

D)Sr

Q4) If wave (a)represents green light,wave (b)might represent A)blue light.

B)red light.

C)ultraviolet radiation.

D)X-rays.

Q5) The number of orbitals in the n = 3 shell is ________.

Page 7

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Chapter 6: Ionic Bonds and Some Main-Group Chemistry

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Sample Questions

Q1) Which sphere most likely represents the Cl ion?

A)A

B)B

C)A or B

D)C or D

Q2) How many electrons does magnesium lose and nitrogen need to form Mg₃N₂?

A)magnesium loses 2 and nitrogen gains 2

B)magnesium loses 2 and nitrogen gains 3

C)magnesium loses 3 and nitrogen gains 2

D)magnesium loses 3 and nitrogen gains 3

Q3) When the equation for the reaction of KBr(aq)with MnO₂(s)to produce Br₂ and Mn²⁺(aq)in acidic solution is balanced,the coefficient in front of the Br₂ is ________.

Q4) Using shorthand notation,the ground-state electron configuration for Tl⁺ is predicted to be ________.

Q5) Lattice energy increases with ________ cation and anion charges and ________ cation and anion radii.

Q6) The element in period 4 with the smallest first ionization energy is ________.

Page 8

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Chapter 7: Covalent Bonds and Molecular Structure

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Sample Questions

Q1) In which will the O-O bond be made stronger by removing an electron?

A)Only O₂

B)Only O₂^-

C)Only O₂^2-

D)All of these

Q2) Compare the energies of molecular orbitals of homonuclear diatomic molecules with the energies of the atomic orbitals with which they correlate.

A)Both bonding and antibonding molecular orbitals lie lower in energy than the atomic orbitals.

B)Bonding orbitals are lower and antibonding orbitals are higher in energy than the atomic orbitals.

C)Bonding orbitals are higher and antibonding orbitals are lower in energy than the atomic orbitals.

D)Both bonding and antibonding molecular orbitals are higher in energy than the atomic orbitals.

Q3) Based on formal charges,the P-O bond order in POCl₃ is expected to be

Q4) Which compound is most likely to exist as a gas at room temperature?

Q5) Of the bonds C-C,C-N,C-O,and C-F,the bond that is most polar is ________.

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Chapter 8: Thermochemistry: Chemical Energy

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Sample Questions

Q1) For a system at constant pressure,12,400 calories of heat are released.This quantity of heat is equivalent to

A)1)92 × 10^-5 J.

B)2)96 × 10³ J.

C)1)24 × 10⁴ J. D)5)19 × 10⁴ J.

Q2) At 25°C the heat of fusion of aluminum is 10.6 kJ/mol and the heat of sublimation is 326.4 kJ/mol.What is the heat of vaporization of aluminum at 25°C?

A)158.2 kJ/mol

B)168.5 kJ/mol

C)315.8 kJ/mol

D)337.0 kJ/mol

Q3) What is the thermodynamic criterion for equilibrium for a reaction at constant temperature and pressure (PV work only)?

A) S = 0

B) G = 0

C) S > 0

D) G < 0

Q4) Is chemical energy a form of kinetic or potential molecular energy?

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Chapter 9: Gases: Their Properties and Behavior

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Sample Questions

Q1) A steel bottle contains argon gas at STP.What is the final pressure if the temperature is changed to 115°C?

A)0)704 atm

B)0)768 atm

C)1)30 atm

D)1)42 atm

Q2) An "empty" aerosol can at 25°C still contains gas at 1.00 atmosphere pressure.If an "empty" can is thrown into a 475°C fire,what is the final pressure in the heated can?

A)5)26 × 10^-2 atm

B)0)398 atm

C)2)51 atm

D)19.0 atm

Q3) What is the total pressure in a 6.00-L flask which contains 0.127 mol of H₂(g)and 0.288 mol of N₂(g)at 20.0°C?

A)0)510 atm

B)0)681 atm

C)1)16 atm

D)1)66 atm

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Chapter 10: Liquids,solids,and Phase Changes

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Sample Questions

Q1) In the drawing of acetic acid,CH₃CO₂H,a partial positive charge ( +)occurs on

A)only atom (a).

B)only atom (b).

C)atoms (a)and (c).

D)atoms (b)and (d).

Q2) How many cations M are in the unit cell?

A)1

B)2

C)4

D)8

Q3) The wavelength of light used to observe an object must be ________ than the object itself.

A)larger

B)smaller

C)of higher energy

D)of lower energy

Q4) The HBr bond has a length of 141 pm and 12.1% ionic character.What is the dipole moment of HBr?

Q5) The coordination number of each atom in a simple cubic unit cell is ________.

Page 12

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Chapter 11: Solutions and Their Properties

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Sample Questions

Q1) KBr does not dissolve well in nonpolar solvents because

A)solute-solute interactions are much larger than solvent-solvent or solute-solvent interactions.

B)solvent-solvent interactions are much larger than solute-solvent or solute-solute interactions.

C)solute-solvent interactions are much larger than solvent-solvent or solute-solute interactions.

D)solute-solvent interactions are similar to solvent-solvent and solute-solute interactions.

Q2) In most liquid solutions,the component present in the larger amount is called the A)dispersed medium.

B)emulsifying agent.

C)solute.

D)solvent.

Q3) At 80.0°C benzene has a vapor pressure of 96.0 mm Hg and toluene has a vapor pressure of 30.3 mm Hg.If a mixture of benzene and toluene has a vapor pressure of 54.6 mm Hg,what are the mole fractions of benzene and toluene?

Q4) Molarity is defined as ________,whereas molality is defined as ________.

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Page 13

Chapter 12: Chemical Kinetics

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Sample Questions

Q1) What is the order of reaction with respect to B₂?

A)0

B)1

C)2

D)3

Q2) What is the overall reaction order for the reaction that has the rate law: Rate = k[H₂][NO]²?

A)zero order

B)first order

C)second order

D)third order

Q3) A reaction occurs by a two-step mechanism,shown below.

Step 1: AX₂(g) AX(g)+ X(g)

Step 2: AX₂(g)+ X(g) AX + X₂(g)

The intermediate in this reaction is ________,and the molecularity of the second step is ________.

Q4) A reaction with an activation energy,E_a = 51.2 kJ/mol will proceed ________ times faster when the temperature is raised from 20 °C to 30 °C.

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Page 14

Chapter 13: Chemical Equilibrium

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Sample Questions

Q1) The dissolution of calcium hydroxide is exothermic.

Ca(OH)₂(s) Ca²⁺(aq)+ 2 OH^-(aq)What happens when the solution of Ca(OH)₂ is heated?

A)The amount of Ca(OH)₂(s)decreases.

B)The amount of Ca(OH)₂(s)increases.

C)The amount of Ca(OH)₂(s)remains unchanged.

D)The Ca(OH)₂(s)completely dissolves.

Q2) Which reaction has the smallest equilibrium constant?

A)A₂ + B₂ 2 AB

B)A₂ + C₂ 2 AC

C)A₂ + D₂ 2 AD

D)A₂ + E₂ 2 AE

Q3) For the reaction shown below,N₂O₄ and NO₂ have equilibrium concentrations,[N₂O₄]_eq = 2.160 × 10^-⁴ and [NO₂]_eq = 1.001 × 10^-³,respectively.The equilibrium constant,K_c,for this reaction equals ________. N₂O₄(g) 2 NO₂(g)

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Chapter 14: Aqueous Equilibria: Acids and Bases

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Sample Questions

Q1) Calculate the pH of a 0.020 M carbonic acid solution,H₂CO₃(aq),that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

A)1)70

B)4)03

C)6)37

D)10.25

Q2) In order for the reaction HA + HSO₃^- A^- + H₂SO₃ to have an equilibrium constant K_c < 1,the K_a of HA must be ________ (greater,less)than the K_a of HSO₃^-.

Q3) Calculate the pH of a 1.60 M KBrO solution.K_a for hypobromous acid,HBrO,is 2.0 × 10^-9.

A)2)55

B)4)25

C)9)75

D)11.45

Q4) A proton hydrated by four water molecules has the formula ________.

Q5) A 0.10 M KNO₂ solution will have a pH ________ seven.

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Chapter 15: Applications of Aqueous Equilibria

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Sample Questions

Q1) What is the characteristic pH-titration curve for the titration of a weak acid by a strong base?

A)A

B)B

C)C

D)D

Q2) What is the pH of a buffered system made by dissolving 17.42 g of KH₂PO₄ and 20.41 g of K₂HPO₄ in water to give a volume of 200.0 mL? The K_a2 for dihydrogen phosphate is 6.2 × 10^-8 and the equilibrium reaction of interest is H₂PO₄^-(aq)+ H₂O(l) H₃O⁺(aq)+ HPO₄^-(aq).

A)7)03

B)7)17

C)7)38

D)7)58

Q3) The solution formed upon adding 50.00 mL of 0.10 M NH₄Cl to 50.00 mL of 0.10 M NH₃ will have a pH that is ________ the pH of the original NH₃ solution.

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Page 17

Chapter 16: Thermodynamics: Entropy, free Energy, and Equilibrium

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Q1) By what factor does the entropy increase for a collection of 100 molecules from a system of 1 × 10⁵ boxes to 1 × 10⁶ boxes?

Q2) Which of the above reaction mixtures is G of reaction = G °?

A)(1)

B)(2)

C)(3)

D)(4)

Q3) For the reaction N₂(g)+ O₂(g) 2NO(g), H° = 180.4 kJ/mol and S° = 24.9 J/K.Is there a temperature at which the spontaneity of this reaction be changed,either from spontaneous to nonspontaneous or nonspontaneous to spontaneous? If so,estimate the temperature.

Q4) Entropy is a measure of A)free energy.

B)the heat of a reaction. C)molecular randomness.

D)the rate of a reaction.

Q5) For the vaporization of solid rhombic sulfur,S(s,rhombic) S(g), G° = 236.7 kJ/mol.At 25 °C the vapor pressure of rhombic sulfur is ________ atm.

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Chapter 17: Electrochemistry

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Sample Questions

Q1) Which statement concerning overvoltage is false?

A)Overvoltage is the additional voltage above the calculated voltage required to bring about electrolysis.

B)Overvoltage is often due to a high activation energy for the reaction at one electrode.

C)Overvoltage is small for half-reactions involving the formation of O₂(g)or H₂(g).

D)Overvoltage must be experimentally determined.

Q2) The cell reaction 2 Fe³⁺(aq)+ Zn(s) Zn²⁺(aq)+ 2 Fe²⁺(aq)occurs in the galvanic cell shown above.Which would be the most appropriate choices for the solid electrode in half-cell (A)and in half-cell (B)?

A)Fe(s)for half-cell (A)and Zn(s)for half-cell (B)

B)Pt(s)for half-cell (A)and Zn(s)for half-cell (B)

C)Fe(s)for half-cell (A)and Fe(s)for half-cell (B)

D)Zn(s)for half-cell (A)and Pt(s)for half-cell (B)

Q3) Electrolysis of a metal nitrate solution M(NO₃)₂(aq)for 3.00 hours with a constant current of 20.0 A gives 119 g of the metal M.The identity of the metal M in the metal ion M²⁺ is ________.

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Page 19

Chapter 18: Hydrogen, oxygen, and Water

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Q1) What is not a good laboratory method for the preparation of oxygen?

A)photosynthesis of sugars: 6 CO₂(g)+ 6 H₂O(l) 6 O₂(g)+ ₆H₁₂O₆(s)

B)electrolysis of water: 2 H₂O(l) 2 H₂(g)+ O₂(g)

C)catalytic decomposition of hydrogen peroxide: 2 H₂O₂(aq) 2 H₂O(l)+ O₂(g)

D)thermal decomposition of potassium chlorate: 2 KClO₃(s) 2 KCl(s)+ 3 O₂(g)

Q2) How many mL of O₂ gas at 25°C and 755 mm Hg pressure can be produced from the thermal decomposition of 0.300 grams of KClO₃(s)according to the chemical equation shown below? 2 KClO₃(s) 2 KCl(s)+ 3 O₂(g)

A)30.1 mL

B)40.2 mL

C)90.4 mL

D)181 mL

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Page 20

Chapter 19: The Main-Group Elements

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Q1) Which of these molecules is most likely to contain good overlap of p orbitals,as shown in figure (a),rather than poor overlap of p orbitals,as shown in figure (b)?

A)Cl₂

B)N₂

C)P₄

D)S₈

Q2) Using principles discussed in chapters 15 and 19,determine which of the following is the strongest acid.

A)HClO₂

B)HClO₃

C)HBrO₃

D)HIO₃

Q3) What is the oxidation number of carbon in CaC₂?

A)+ 4

B)+ 1

C)- 1

D)- 2

Q4) The fullerene C₆₀ is an ________ (allotrope,isotope,isomer)of carbon.

Q5) The number of nonmetals in group 4A of the periodic table is ________.

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Chapter 20: Transition Elements and Coordination Chemistry

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Q1) What is the ground-state electron configuration for the element chromium (Z = 24)?

A)[Ne] 4s² 3d⁴

B)[Ar] 4s² 3d⁴

C)[Ar] 4s¹ 3d⁵

D)[Ar] 3d⁶

Q2) Which element indicated on the above periodic table has the electron configuration [Xe] 4f⁷ 5d¹ 6s²?

A)element A

B)element B

C)element C

D)element D

Q3) Which of the following complex ions is colorless?

A)[Co(H₂O)₆]²⁺

B)[Mn(CN)₆]^3-

C)[CrCl₃(H₂O)₃]

D)[Ag(NH₃)₂]⁺

Q4) The oxidation state of palladium in K₂[PdCl₄] is ________.

Page 22

Q5) The first transition series element expected to have the lowest second ionization energy is ________.

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Chapter 21: Metals and Solid-State Materials

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Q1) What is not a metallurgy process?

A)environmental reconstruction of the landscape

B)extraction of metals from their ores

C)making of alloys and metallic composites

D)reduction of the mineral to the free metal

Q2) An AlGaAs diode laser pointer emits 532 nm light and appears ________ (blue,green,red)in color.

Q3) Which of these elements is likely to be found in nature as a sulfide?

A)element A

B)element B

C)element C

D)element D

Q4) A silicon carbide ceramic has a unit cell with carbon atoms in a cubic closest packed arrangement with carbon atoms occupying one-half of the tetrahedral holes.The empirical formula of this ceramic is ________.

Q5) Which substance is the best conductor of electricity?

A)arsenic

B)boron

C)silver

D)tellurium

Page 23

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Chapter 22: Nuclear Chemistry

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Q1) Oxygen-16 (15.994915 amu)is synthesized in the sun by fusion of ¹²C (12.000000 amu)and ⁴He (4.00260 amu).How much energy is released in this nuclear reaction?

A)2)48 × 10³ kJ/mol

B)2)30 × 10⁶ kJ/mol

C)6)92 × 10⁸ kJ/mol

D)7)20 × 10¹¹ kJ/mol

Q2) Radium occurs only in uranium ores,typically with an observed Ra/U ratio of 1mg/3kg.Uranium ores normally contain only about 200 ppm of U.How many kilograms of uranium ore must be processed to obtain 1 mg of radium?

A)1700 kg ore

B)15,000 kg ore

C)6)0 × 10⁸ kg ore

D)None of these

Q3) What type of shielding can be used to protect against gamma rays?

A)cloth

B)lead

C)wood

D)No shielding is effective against gamma rays.

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Page 24

Chapter 23: Organic and Biological Chemistry

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Sample Questions

Q1) Which name is not correct?

A)1,2-dichloropentane

B)2,3-dimethylbutane

C)2-ethylbutane

D)4-propylheptane

Q2) Which one of the following behaves like a base?

A)CH₃CONHCH₃

B)(CH₃)₂NH

C)C₂H₅CONHCH₃

D)All of these are bases.

Q3) Cellulose is a polymer consisting of thousands of A) -glucose molecules.

B) -glucose molecules.

C)long chain fatty acids.

D)amino acids.

Q4) What hybrid orbitals are used by carbon to form covalent bonds with hydrogen?

A)sp

B)sp²

C)sp³

D)sp³^d

Page 25

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