Question 1

Identify the complete electronic configuration for S2-.

Accepted Answer

A)  1s22s22p63s24p6 
B)  1s22s22p63s23p6 
C)  1s22s22p63s23p5 
D)  1s22s23p64s25p6 
E)  1s22s2p63s2p6 
A)  1s22s22p63s24p6 
B)  1s22s22p63s23p6 
C)  1s22s22p63s23p5 
D)  1s22s23p64s25p6 
E)  1s22s2p63s2p6

Question 2

Which of the following ionic compounds would be expected to have the highest lattice energy?

Accepted Answer

A)  Li Cl 
B)  Na Cl 
C)  K Cl 
D)  Rb Cl 
A)  Li Cl 
B)  Na Cl 
C)  K Cl 
D)  Rb Cl

Question 3

Match the following.
-Cs-I

Accepted Answer

A) strongest covalent bond 
B) longest covalent bond 
C) weakest ionic bond 
D) metallic bond 
E) highest melting point 
A) strongest covalent bond 
B) longest covalent bond 
C) weakest ionic bond 
D) metallic bond 
E) highest melting point

Question 4

Place the following in order of increasing magnitude of lattice energy. CaO MgO SrS

Accepted Answer

A)  MgO < CaO < SrS 
B)  SrS < MgO < CaO 
C)  SrS < CaO < MgO 
D)  CaO < MgO < SrS 
E)  CaO < SrS < MgO 
A)  MgO < CaO < SrS 
B)  SrS < MgO < CaO 
C)  SrS < CaO < MgO 
D)  CaO < MgO < SrS 
E)  CaO < SrS < MgO

Question 5

Identify the compound with ionic bonding.

Accepted Answer

A)  SrBr2 
B)  CH3CH2CH3 
C)  CH4 
D)  H2 
E)  CO2 
A)  SrBr2 
B)  CH3CH2CH3 
C)  CH4 
D)  H2 
E)  CO2

Question 6

Using Lewis structures and formal charge, which of the following ions is most stable? OCN⁻ ONC⁻ NOC⁻

Accepted Answer

A)  OCN⁻ 
B)  ONC⁻ 
C)  NOC⁻ 
D)  None of these ions is stable according to Lewis theory. 
A)  OCN⁻ 
B)  ONC⁻ 
C)  NOC⁻ 
D)  None of these ions is stable according to Lewis theory.

Question 7

Choose the bond below that is most polar.

Accepted Answer

A)  C-N 
B)  C-F 
C)  C-O 
D)  C-C 
E)  F-F 
A)  C-N 
B)  C-F 
C)  C-O 
D)  C-C 
E)  F-F

Question 8

The electronegativity is 2.1 for H and 1.9 for Pb. Based on these electronegativities, PbH4 would be expected to ________.

Accepted Answer

A)  be ionic and contain H- ions 
B)  be ionic and contain H+ ions 
C)  have polar covalent bonds with a partial negative charge on the H atoms 
D)  have polar covalent bonds with a partial positive charge on the H atoms 
A)  be ionic and contain H- ions 
B)  be ionic and contain H+ ions 
C)  have polar covalent bonds with a partial negative charge on the H atoms 
D)  have polar covalent bonds with a partial positive charge on the H atoms

Question 9

Identify the strongest bond.

Accepted Answer

A)  single covalent bond 
B)  double covalent bond 
C)  triple covalent bond 
D)  All of the above bonds are the same strength. 
A)  single covalent bond 
B)  double covalent bond 
C)  triple covalent bond 
D)  All of the above bonds are the same strength.

Question 10

Which of the following reactions is associated with the lattice energy of RbI (Δr)?

Accepted Answer

A)  Rb(s) +   I2(g) → RbI(s) 
B)  RbI(s) → Rb⁺(g) + I⁻(g) 
C)  RbI(s) → Rb(s) +   I2(g) 
D)  RbI(s) → Rb⁺(aq) + I⁻(aq) 
E)  Rb⁺(g) + I⁻(g) → RbI(s) 
A)  Rb(s) +   I2(g) → RbI(s) 
B)  RbI(s) → Rb⁺(g) + I⁻(g) 
C)  RbI(s) → Rb(s) +   I2(g) 
D)  RbI(s) → Rb⁺(aq) + I⁻(aq) 
E)  Rb⁺(g) + I⁻(g) → RbI(s)

Question 11

The phosphorus atom in PCl3 would be expected to have a ________.

Accepted Answer

A)  partial positive (δ+) charge 
B)  partial negative (δ-) charge 
C)  3+ charge 
D)  3- charge 
A)  partial positive (δ+) charge 
B)  partial negative (δ-) charge 
C)  3+ charge 
D)  3- charge

Question 12

Use the bond energies provided to estimate ?S1U1B1rS1U1B0H° for the reaction below. XeFS1U1B12S1U1B0 +2FS1U1B12S1U1B0 ? XeFS1U1B16 S1U1B0?S1U1B1rS1U1B0H°= ?
Bond Bond Energy (kJ molS1U1P1-1S1S1P0)
Xe-F 147
F-F 159

Accepted Answer

A)  -429 kJ molS1U1P1-1S1S1P0 
B)  +159 kJ molS1U1P1-1S1S1P0 
C)  -660 kJ molS1U1P1-1S1S1P0 
D)  +176 kJ molS1U1P1-1S1S1P0 
E)  -270 kJ molS1U1P1-1S1S1P0 
A)  -429 kJ molS1U1P1-1S1S1P0 
B)  +159 kJ molS1U1P1-1S1S1P0 
C)  -660 kJ molS1U1P1-1S1S1P0 
D)  +176 kJ molS1U1P1-1S1S1P0 
E)  -270 kJ molS1U1P1-1S1S1P0

Question 13

Use the data given below to construct a Born-Haber cycle to determine the electron affinity of Br.

Accepted Answer

A)  -885 kJ mol-1 
B)  -325 kJ mol-1 
C)  +367 kJ mol-1 
D)  -464 kJ mol-1 
E)  +246 kJ mol-1 
A)  -885 kJ mol-1 
B)  -325 kJ mol-1 
C)  +367 kJ mol-1 
D)  -464 kJ mol-1 
E)  +246 kJ mol-1

Question 14

Draw the Lewis structure for SO42⁻. How many equivalent resonance structures can be drawn?

Accepted Answer

A)  6 
B)  2 
C)  4 
D)  3 
E)  8 
A)  6 
B)  2 
C)  4 
D)  3 
E)  8

Question 15

Identify the compound with the highest magnitude of lattice energy.

Accepted Answer

A)  CsF 
B)  BaO 
C)  SrO 
D)  CaO 
A)  CsF 
B)  BaO 
C)  SrO 
D)  CaO

Question 16

How many lone pairs are on the Br atom in BrCl2-?

Accepted Answer

A)  0 
B)  1 
C)  2 
D)  3 
A)  0 
B)  1 
C)  2 
D)  3

Question 17

Choose the bond below that is the strongest.

Accepted Answer

A)  N=O 
B)  N-I 
C)  N-O 
D)  N-S 
E)  N=N 
A)  N=O 
B)  N-I 
C)  N-O 
D)  N-S 
E)  N=N

Question 18

Use the data given below to construct a Born-Haber cycle to determine the second ionization energy of Ca.

Accepted Answer

A)  1010 kJ mol-1 
B)  1757 kJ mol-1 
C)  1508 kJ mol-1 
D)  -3027 kJ mol-1 
E)  -1514 kJ mol-1 
A)  1010 kJ mol-1 
B)  1757 kJ mol-1 
C)  1508 kJ mol-1 
D)  -3027 kJ mol-1 
E)  -1514 kJ mol-1

Question 19

Which of the following processes is exothermic?

Accepted Answer

A)  Cl2(g) → 2Cl(g) 
B)  Br(g) + e⁻ → Br⁻(g) 
C)  Li(s) → Li(g) 
D)  NaF(s) → Na⁺(g) + F⁻(g) 
E)  None of the above processes is exothermic. 
A)  Cl2(g) → 2Cl(g) 
B)  Br(g) + e⁻ → Br⁻(g) 
C)  Li(s) → Li(g) 
D)  NaF(s) → Na⁺(g) + F⁻(g) 
E)  None of the above processes is exothermic.

Question 20

Use the bond energies provided to estimate ΔrH° for the reaction below. 2Br2(l) + C2H2(g) → C2H2Br4(l) ΔrH° = ?
Bond Bond Energy (kJ mol-1)
Br-Br 193
C≡C 837
C-C 347
C-Br 276
C-H 414

Accepted Answer

A)  +407 kJ mol-1 
B)  -324 kJ mol-1 
C)  -228 kJ mol-1 
D)  +573 kJ mol-1 
E)  -648 kJ mol-1 
A)  +407 kJ mol-1 
B)  -324 kJ mol-1 
C)  -228 kJ mol-1 
D)  +573 kJ mol-1 
E)  -648 kJ mol-1

Exam 9: Chemical Bonding I: Lewis Theory

Identify the complete electronic configuration for S2-.

Which of the following ionic compounds would be expected to have the highest lattice energy?

Match the following. -Cs-I

Place the following in order of increasing magnitude of lattice energy. CaO MgO SrS

Identify the compound with ionic bonding.

Using Lewis structures and formal charge, which of the following ions is most stable? OCN⁻ ONC⁻ NOC⁻

Choose the bond below that is most polar.

The electronegativity is 2.1 for H and 1.9 for Pb. Based on these electronegativities, PbH4 would be expected to ________.

Identify the strongest bond.

Which of the following reactions is associated with the lattice energy of RbI (Δr)?

The phosphorus atom in PCl3 would be expected to have a ________.

Use the bond energies provided to estimate ?rH° for the reaction below. XeF2 +2F2 ? XeF6 ?rH°= ? Bond Bond Energy (kJ mol-1) Xe-F 147 F-F 159

Use the data given below to construct a Born-Haber cycle to determine the electron affinity of Br.

Draw the Lewis structure for SO42⁻. How many equivalent resonance structures can be drawn?

Identify the compound with the highest magnitude of lattice energy.

How many lone pairs are on the Br atom in BrCl2-?

Choose the bond below that is the strongest.

Use the data given below to construct a Born-Haber cycle to determine the second ionization energy of Ca.

Which of the following processes is exothermic?

Use the bond energies provided to estimate ΔrH° for the reaction below. 2Br2(l) + C2H2(g) → C2H2Br4(l) ΔrH° = ? Bond Bond Energy (kJ mol-1) Br-Br 193 C≡C 837 C-C 347 C-Br 276 C-H 414

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Identify the complete electronic configuration for S^2-.

The electronegativity is 2.1 for H and 1.9 for Pb. Based on these electronegativities, PbH₄ would be expected to ________.

Which of the following reactions is associated with the lattice energy of RbI (Δ_r)?

The phosphorus atom in PCl₃ would be expected to have a ________.

Use the bond energies provided to estimate ?_rH° for the reaction below. XeF₂ +2F₂ ? XeF₆?_rH°= ? Bond Bond Energy (kJ mol^-1) Xe-F 147 F-F 159

Draw the Lewis structure for SO₄²⁻. How many equivalent resonance structures can be drawn?

How many lone pairs are on the Br atom in BrCl₂^-?

Use the bond energies provided to estimate Δ_rH° for the reaction below. 2Br₂(l) + C₂H₂(g) → C₂H₂Br₄(l) Δ_rH°= ? Bond Bond Energy (kJ mol^-1) Br-Br 193 C≡C 837 C-C 347 C-Br 276 C-H 414