General Chemistry II Exam Review - 3071 Verified Questions

General Chemistry II Exam Review

Course

Introduction

General Chemistry II builds upon foundational concepts introduced in the first semester, delving deeper into the principles of chemical reactions, thermodynamics, kinetics, equilibrium, and electrochemistry. This course explores topics such as acids and bases, solubility equilibria, chemical thermodynamics, reaction rates, and the behavior of electrons in chemical bonding. Laboratory work emphasizes experimental techniques, data analysis, and the application of theoretical concepts to practical situations, preparing students for advanced studies in chemistry and related scientific fields.

Recommended Textbook Chemistry Structure and Properties 2nd Edition by Nivaldo J. Tro

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Page 2

Chapter 1: Essentials: Units, Measurements, and Problem

Solving

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Sample Questions

Q1) A propane molecule contains 3 atoms of carbon.The number 3 represents how many significant figures?

A) one

B) two

C) three

D) infinite

Answer: D

Q2) Determine the mass of an object that has a volume of 88.6 mL and a density of 7.77 g/mL.

A) 96.4 g

B) 0.0877 g

C) 11.4 g

D) 80.8 g

E) 688 g

Answer: E

Q3) The correct answer (reported to the proper number of significant figures)to the following is

6.3 × 3.25 = ________

Answer: 20

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Chapter 2: Atoms

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Sample Questions

Q1) Give the composition of hydrogen peroxide.

A) two hydrogen atoms and two oxygen atoms

B) one hydrogen atom and one oxygen atom

C) two hydrogen atoms and one oxygen atom

D) one hydrogen atom and two oxygen atoms

Answer: A

Q2) Identify the characteristics of a solid.

A) definite volume and definite shape

B) definite volume and no definite shape

C) no definite shape and definite volume

D) no definite shape and no definite volume

Answer: A

Q3) What mass (in kg)does 4.77 moles of nickel have?

A) 0.352 kg

B) 0.122 kg

C) 0.820 kg

D) 0.280 kg

E) 0.632 kg

Answer: D

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Page 4

Chapter 3: The Quantum Mechanical Model of the Atom

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Sample Questions

Q1) Which of the following occur as the wavelength of a photon increases?

A) The frequency decreases.

B) The energy increases.

C) The speed decreases.

D) Planck's constant decreases.

E) None of the above occur as the wavelength of a photon increases.

Answer: A

Q2) Choose the transition (in a hydrogen atom)below that represents the absorption of the shortest wavelength photon.

A) n = 1 to n = 2

B) n = 2 to n = 3

C) n = 4 to n = 6

D) n = 6 to n = 5

E) n = 3 to n = 1

Answer: A

Q3) Give an example of a p orbital.

Answer: p_x,p_y,or p_z

Q4) Define constructive interference.

Answer: Waves that are in phase combine with each other.

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Chapter 4: Periodic Properties of the Elements

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Sample Questions

Q1) Place the following in order of increasing atomic radius. As O Br

A) As < Br < O

B) O < As < Br

C) Br < As < O

D) As < O < Br

E) O < Br < As

Q2) Are anions typically larger or smaller than their corresponding atom? Why?

Q3) Choose the ground state electron configuration for Cr³ .

A) [Ar]4s¹3d²

B) [Ar]

C) [Ar]4s²3d⁶

D) [Ar]3d³

E) [Ar]4s²3d¹

Q4) Define ionization energy.

Q5) In which of the following sets do all species have the same number of protons?

A) Cl^-, Ar, Ca²⁺

B) N, O^2-, F^-

C) Sc³⁺, Y³⁺, La³⁺

D) Cr, Cr²⁺, Cr³⁺

Page 6

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Chapter 5: Molecules and Compounds

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Sample Questions

Q1) What is the chemical formula for barium oxide?

A) BaO

B) BaO₂

C) Ba₂O₂

D) Ba₂O

E) Ba₂O₃

Q2) Which of the following is a molecular compound?

A) CuCl₂

B) KI

C) NaNO₃

D) CH₂Cl₂

E) RbBr

Q3) Give the structure for lithium hypo iodite.

A) LI IO

B) LI IO₂

C) LI IO₃

D) LI IO₄

Q4) Calculate the mass percent composition of oxygen in Al₂(SO₄)₃.

Q5) Why aren't prefixes used in naming ionic compounds?

Page 7

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Chapter 6: Chemical Bonding I

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Sample Questions

Q1) Determine the electron geometry (eg)and molecular geometry (mg)of CO₂.

A) eg = tetrahedral, mg = tetrahedral

B) eg = linear, mg = trigonal planar

C) eg = trigonal planar, mg = bent

D) eg = linear, mg = linear

E) eg = trigonal planar, mg = trigonal planar

Q2) Define dipole moment.

Q3) Give the number of valence electrons for CH₂Cl₂.

A) 16

B) 18

C) 20

D) 22

E) 12

Q4) Which molecule or compound below contains a pure covalent bond?

A) Li₂CO₃

B) SCl₆

C) Cl₂

D) P Br₃

E) Li F

Page 8

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Chapter 7: Chemical Bonding Ii

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Sample Questions

Q1) How many of the following molecules have sp³d² hybridization on the central atom?

Se Cl₆ Xe Cl₄ IF₅ As Cl₅

A) 1

B) 3

C) 0

D) 2

E) 4

Q2) Draw the molecular orbital diagram shown to determine which of the following is MOST stable.

A) C₂²

B) N₂²

C) B₂

D) C₂²

E) B₂²

Q3) List the number of sigma bonds and pi bonds in a triple bond.

A) 1 sigma, 1 pi

B) 2 sigma, 1 pi

C) 2 sigma, 2 pi

D) 1 sigma, 2 pi

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Chapter 8: Chemical Reactions and Chemical Quantities

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Sample Questions

Q1) How many moles of SnCl₂ will be produced if 85.3 g of FeCl₃ is reacted with an excess of Sn for the following reaction: 2 FeCl₃(s)+ 3 Sn(s) 3 SnCl₂(s)+ 2 Fe(s)

A) 0.526 mol

B) 0.789 mol

C) 1.20 mol

D) 1.58 mol

E) 2.43 mol

Q2) How many grams of calcium chloride are needed to produce 5.00 g of potassium chloride?

CaCl₂(aq)+ K₂CO₃(aq) 2 KCl(aq)+ CaCO₃(aq)

A) 0.269 g

B) 3.72 g

C) 7.44 g

D) 14.9 g

Q3) Balance the following equation. ________ C₉H₂₀+ ________ O₂ ________ H₂O + ________ CO₂

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Page 10

Chapter 9: Introduction to Solutions and Aqueous Reactions

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Sample Questions

Q1) 6.74 g of the monoprotic acid KHP (MW = 204.2 g/mol)is dissolved into water.The sample is titrated with a 0.703 M solution of calcium hydroxide to the equivalence point.What volume of base was used?

A) 8.64 mL

B) 11.8 mL

C) 23.5 mL

D) 47.0 mL

E) 93.9 mL

Q2) Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of K₂S and Fe(NO₃)₂ are mixed.

A) K⁺(aq) + NO₃^-(aq) KNO₃(s)

B) Fe²⁺(aq) + S^2-(aq) + 2 K⁺(aq) + 2 NO₃^-(aq) FeS(s) + 2 K⁺(aq) + 2 NO₃^-(aq)

C) Fe²⁺(aq) + S^2-(aq) + 2 K⁺(aq) + 2 NO₃^-(aq) Fe²⁺(aq) + S^2-(aq) + 2 KNO₃(s)

D) Fe²⁺(aq) + S^2-(aq) FeS(s)

E) No reaction occurs.

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Chapter 10: Thermochemistry

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Sample Questions

Q1) Give the equation with the elements in MgSO₄ in their standard state as the reactants and MgSO₄ as the product.

Q2) Use the bond energies provided to estimate H°_rxn for the reaction below. PCl₃(g)+ Cl₂(g) PCl₅(l) H°_rxn= ?

Bond Bond Energy (kJ/mol)

Cl-Cl 243

P-Cl 331

A) -243 kJ

B) -419 kJ

C) -662 kJ

D) -67 kJ

E) -905 kJ

Q3) Which of the following is TRUE if E_sys = - 115 J?

A) The system is gaining 115 J, while the surroundings are losing 115 J.

B) The system is losing 115 J, while the surroundings are gaining 115 J.

C) Both the system and the surroundings are gaining 115 J.

D) Both the system and the surroundings are losing 115 J.

E) None of the above are true.

Q4) Give the temperature and pressure for the standard state for a liquid.

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Chapter 11: Gases

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Sample Questions

Q1) How many moles of Ar are contained in a 5.00 L tank at 155°C and 2.80 atm?

A) 0.399 moles

B) 1.10 moles

C) 2.51 moles

D) 0.455 moles

E) 0.289 moles

Q2) A syringe contains 0.65 moles of He gas that occupy 750.0 mL.What volume (in L)of gas will the syringe hold if 0.35 moles of Ne is added?

A) 0.87 L

B) 4.9 L

C) 1.2 L

D) 2.1 L

E) 1.9 L

Q3) Define hypoxia.

A) oxygen starvation

B) increased oxygen concentration in body tissues

C) increased nitrogen concentration in body tissues and fluids

D) nitrogen starvation

Q4) Give the major gas in dry air.

Q5) Define pressure.

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Chapter 12: Liquids, Solids, and Intermolecular Forces

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Sample Questions

Q1) Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.

A) absolute temperature

B) definite temperature

C) fluid temperature

D) critical temperature

E) solid temperature

Q2) Which substance below has the strongest intermolecular forces?

A) A₂X, H_vap= 39.6 kJ/mol

B) BY₂, H_vap= 26.7 kJ/mol

C) C₃X₂, H_vap= 36.4 kJ/mol

D) DX₂, H_vap= 23.3 kJ/mol

E) EY₃, H_vap= 21.5 kJ/mol

Q3) Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.

A) O₂

B) CO

C) HF

D) NaCl

E) All of these have intermolecular forces stronger than dispersion.

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Chapter 13: Crystalline Solids and Modern Materials

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Sample Questions

Q1) Nickel has a face-centered cubic structure and has a density of 8.90 g/cm³.What is its atomic radius?

A) 125 pm

B) 249 pm

C) 353 pm

D) 997 pm

Q2) In a semiconductor,the bonding molecular orbitals that contain electrons are referred to as the ________,while the antibonding orbitals that are completely empty are referred to as the ________.

A) single bond, antibond

B) conduction band, valence band

C) valence band, conduction band

D) n-type, p-type

E) p-type, n-type

Q3) All of the following are examples of allotropes of carbon EXCEPT

A) graphite

B) glass

C) diamond

D) graphine

E) all of the above

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Chapter 14: Solutions

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Sample Questions

Q1) Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈,molar mass = 128.16 g/mol)dissolved in 722 mL of benzene (d = 0.877 g/mL).Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m.

A) 4.76°C

B) 4.17°C

C) 0.74°C

D) 1.33°C

E) 1.68°C

Q2) Define osmosis.

Q3) Identify the compound whose solubility is least affected by temperature.

A) KCl

B) K₂Cr₂O₇

C) NaNO₃

D) Pb(NO₃)₃

E) NaCl

Q4) Why isn't pentanol (CH₃CH₂CH₂CH₂CH₂OH) very soluble in water?

Q5) Explain why water does not dissolve in gasoline.

Q6) Give the preparation of rock candy.

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Chapter 15: Chemical Kinetics

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Sample Questions

Q1) Give the characteristic of a first order reaction having only one reactant.

A) The rate of the reaction is not proportional to the concentration of the reactant.

B) The rate of the reaction is proportional to the square of the concentration of the reactant.

C) The rate of the reaction is proportional to the square root of the concentration of the reactant.

D) The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant.

E) The rate of the reaction is directly proportional to the concentration of the reactant.

Q2) What data should be plotted to show that experimental concentration data fits a second-order reaction?

A) ln[reactant] vs. time

B) [reactant] vs. time

C) ln(k) vs. 1/T

D) 1/[reactant] vs. time

E) ln(k) vs. E_a

Q3) Explain how the order of a reaction can be determined.

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Chapter 16: Chemical Equilibrium

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Sample Questions

Q1) Consider the following reaction at equilibrium.What effect will removing NO₂ have on the system?

SO₂(g)+ NO₂(g) SO₃(g)+ NO(g)

A) The reaction will shift in the direction of products.

B) The reaction will shift to decrease the pressure.

C) No change will occur since SO₃ is not included in the equilibrium expression.

D) The reaction will shift in the direction of reactants.

E) The equilibrium constant will decrease.

Q2) Consider the following reaction: CO₂(g)+ C(graphite) 2 CO(g)

A reaction mixture initially contains 0.56 atm CO₂ and 0.32 atm

CO.Determine the equilibrium pressure of CO if K_p for the reaction at this temperature is 2.25.

A) 0.83 atm

B) 0.31 atm

C) 0.26 atm

D) 0.58 atm

E) 0.42 atm

Q3) Why aren't solids or liquids included in an equilibrium expression?

Q4) Define Le Chatelier's Principle.

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Chapter 17: Acids and Bases

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Sample Questions

Q1) Identify the base that is in baking soda.

A) RbOH

B) NaOH

C) NaHCO₃

D) K₂CO₃

E) NH₃

Q2) Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.24.

A) 5.8 × 10^-4

B) 10.76

C) 1.7 × 10^-11

D) 3.2 × 10^-14

E) 1.1 × 10^-13

Q3) Which of the following is not a conjugate acid-base pair?

A) NH₄⁺/NH₃

B) H₃O /OH

C) H₂SO₃/HSO₃

D)

C₂H₃O₂ /HC₂H₃O<sub>2< /sub>

E) All of the above are conjugate acid-base pairs.

Page 19

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Chapter 18: Aqueous Ionic Equilibrium

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Sample Questions

Q1) Animals will lick up ethylene glycol (antifreeze)due to its sweet taste.The antidote for ethylene glycol poisoning is the administration of

A) ethyl alcohol ( alcoholic drinks).

B) isopropyl alcohol (rubbing alcohol).

C) mineral oil (laxative).

D) vinegar.

E) sodium bicarbonate (baking soda).

Q2) What is the pH of a solution made by mixing 20.00 mL of 0.100 M HCl with 40.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.

A) 0.48

B) 1.48

C) 12.52

D) 13.52

Q3) Sketch the titration curve for a strong acid titrated with a strong base.Make sure to indicate the equivalence point (and whether it is acidic,basic or neutral)and the buffer region.

Q4) Explain the common ion effect with respect to molar solubility.

Q5) Identify the compound that is in stalactites and stalagmites.

Q6) Give the name of the compound that is in antifreeze and is toxic to pets.

Page 20

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Chapter 19: Free Energy and Thermodynamics

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Sample Questions

Q1) The ________ Law of Thermodynamics states that for any spontaneous reaction,the entropy of the universe increases.

A) Zero

B) First

C) Second

D) Third

E) Fourth

Q2) Place the following in order of decreasing molar entropy at 298 K. HCl N₂H₄ He

A) He > N₂H₄> HCl

B) He > HCl > N₂H₄

C) N₂H₄ > He > HCl

D) N₂H₄ > HCl > He

E) HCl > N₂H₄ > He

Q3) Give the standard states for a gas,liquid,solid,and solution.

Q4) How many microstates are possible in a collection of four particles that are present,with two particles each in two connected flasks?

Sketch them below.

Q5) Why can endothermic reactions be spontaneous?

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Chapter 20: Electrochemistry

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Q1) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced.) Mg(s)+ Cu²⁺(aq) Cu(s)+ Mg²⁺(aq) Mg²⁺(aq)+ 2 e Mg(s)E° = -2.38 V Cu²⁺(aq)+ 2 e Cu(s)E° = +0.34 V

A) +2.04 V

B) -2.04 V

C) +2.72 V

D) -1.36 V

E) +1.36 V

Q2) CuHow many electrons are transferred in the following reaction? (The reaction is unbalanced.)

V⁵⁺(aq)+ Mg(s) V(s)+ Mg²⁺(aq)

A) 1

B) 2

C) 4

D) 5

E) 10

Q3) What is electrolysis?

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Chapter 21: Radioactivity and Nuclear Chemistry

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Q1) Define chain reaction in terms of the fission of uranium nucleus.

Q2) The splitting of a heavy nucleus to form two or more lighter ones is called

A) radioactive cleavage.

B) nuclear fission.

C) nuclear fusion.

D) radioactive merge.

E) half life.

Q3) Samarium-158 undergoes beta emission with a half-life of 5.30 minutes.If you start with 76.2 mg of the material,how long will it take until you have 18.9 mg of the sample?

A) 3.51 minutes

B) 5.30 minutes

C) 10.6 minutes

D) 18.4 minutes

E) 26.3 minutes

Q4) Describe what is meant by the term "valley of stability"?

Q5) List two problems associated with nuclear power.

Q6) Define radioactivity.

Q7) How does a dosimeter measure exposure to radioactivity?

Q8) What is the "mass defect"?

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Chapter 22: Organic Chemistry

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Q1) Write a balanced chemical reaction to represent the combustion of 2,2-dimethylpropane.

A) C₅H₁₂ + 8 O₂ 5 CO₂ + 6 H₂O

B) C₃H₈ + 5 O₂ 3 CO₂ + 4 H₂O

C) C₅H₁₂ + H₂ CH₄ + 2

C₂H₆

D) C₃H₈ + H₂ CH₄ + C₂H₆

E) 2 C₃H₈ + O₂ 3 CH₄ + 2 H₂O

Q2) Which of the following compounds exhibit geometric isomerism?

A) CH₂=CH-CH₃

B) CCl₂=CBr₂

C) CH₃-CH=CH-CH₃

D) CCl₂=CHBr

E) All of the above exhibit geometric isomerism.

Q3) What does the term "racemic mixture" mean?

Q4) Why doesn't benzene typically undergo addition reactions like the alkenes do?

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Chapter 23: Transition Metals and Coordination Compounds

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Q1) Which of the following compounds can exhibit fac-mer isomerism?

A) [Cu(CO)₅Cl]⁺

B) [Co(H₂O)₃(CO)₃]³⁺

C) [Fe(CO)₅NO₂]²⁺

D) [Fe(NH₃)₂(H₂O)₄]²⁺

E) [Cr(H₂O)₄Br₂]⁺

Q2) How many d electrons are there in Cr₂O₇^2-?

A) 0

B) 1

C) 2

D) 3

Q3) Determine the chemical formula for the compound,diamminetetraaquairon(II)chloride.

A) [Fe(NH₃)₂(H₂O)₄Cl]

B) [Fe(NH₃)₂][(H₂O)₄Cl]

C) [Fe(NH₃)₂(H₂O)₄]Cl₂

D) [Fe(H₂O)₄][(NH₃)₂Cl]

E) [Fe(NH₃)₂(H₂O)₄]Cl₃

Q4) What is the Lanthanide contraction?

Q5) What is a coordinate covalent bond?

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