Question 1

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

Accepted Answer

A)  LiF 
B)  LiCl 
C)  LiBr 
D)  LiI 
A)  LiF 
B)  LiCl 
C)  LiBr 
D)  LiI

Question 2

The iodine atom in I2 would be expected to have a ________.

Accepted Answer

A)  charge of 1- 
B)  partial charge δ- 
C)  partial charge δ+ 
D)  charge of 0 
A)  charge of 1- 
B)  partial charge δ- 
C)  partial charge δ+ 
D)  charge of 0

Question 3

Use Lewis theory to determine the chemical formula for the compound formed between Ca and N.

Accepted Answer

A)  CaN 
B)  Ca3N2 
C)  CaN2 
D)  Ca2N 
E)  Ca2N3 
A)  CaN 
B)  Ca3N2 
C)  CaN2 
D)  Ca2N 
E)  Ca2N3

Question 4

Which molecule or compound below contains a pure covalent bond?

Accepted Answer

A)  Li2CO3 
B)  SCl6 
C)  Cl2 
D)  PF3 
E)  NaCl 
A)  Li2CO3 
B)  SCl6 
C)  Cl2 
D)  PF3 
E)  NaCl

Question 5

Define formal charge.

Accepted Answer

Formal charge is the charge of

Question 6

How many of the following elements can form hypercoordinate compounds? I O Cl Xe

Accepted Answer

A)  2 
B)  0 
C)  3 
D)  1 
E)  4 
A)  2 
B)  0 
C)  3 
D)  1 
E)  4

Question 7

Explain why the lattice energy of MgS is approximately four times as large as that of NaCl.

Accepted Answer

The Mg²⁺ and Na⁺ ions are similar in size

Question 8

Choose the best Lewis structure for CH2Cl2.

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 9

Which of the following processes is endothermic?

Accepted Answer

A)  the reaction associated with the lattice energy of LiCl 
B)  the reaction associated with the ionization energy of potassium 
C)  the reaction associated with the heat of formation of CaS 
D)  the formation of F2 from its elements in their standard states 
E)  None of the above processes is endothermic. 
A)  the reaction associated with the lattice energy of LiCl 
B)  the reaction associated with the ionization energy of potassium 
C)  the reaction associated with the heat of formation of CaS 
D)  the formation of F2 from its elements in their standard states 
E)  None of the above processes is endothermic.

Question 10

Choose the best Lewis structure for BeF2.

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 11

Which of the following processes is endothermic?

Accepted Answer

A)  K⁺(g) + I⁻(g) → KI(s) 
B)  2Br(g) → Br2(g) 
C)  Ca(s) → Ca(g) 
D)  2Na(s) +   O2(g) → Na2O(s) 
E)  None of the above processes is endothermic. 
A)  K⁺(g) + I⁻(g) → KI(s) 
B)  2Br(g) → Br2(g) 
C)  Ca(s) → Ca(g) 
D)  2Na(s) +   O2(g) → Na2O(s) 
E)  None of the above processes is endothermic.

Question 12

A double covalent bond contains ________ of electrons.

Accepted Answer

A)  0 pairs 
B)  1 pair 
C)  2 pairs 
D)  3 pairs 
E)  4 pairs 
A)  0 pairs 
B)  1 pair 
C)  2 pairs 
D)  3 pairs 
E)  4 pairs

Question 13

Of the following elements, which has the lowest electronegativity?

Accepted Answer

A)  Sr 
B)  I 
C)  Ba 
D)  At 
A)  Sr 
B)  I 
C)  Ba 
D)  At

Question 14

Identify the compound with covalent bonding.

Accepted Answer

A)  NaF 
B)  CaO 
C)  CH3NH2 
D)  K2O 
E)  SrBr2 
A)  NaF 
B)  CaO 
C)  CH3NH2 
D)  K2O 
E)  SrBr2

Question 15

Of the following elements, which has the highest electronegativity?

Accepted Answer

A)  S 
B)  Cl 
C)  Ti 
D)  Se 
A)  S 
B)  Cl 
C)  Ti 
D)  Se

Question 16

Give the number of valence electrons for SF4.

Accepted Answer

A)  28 
B)  30 
C)  32 
D)  34 
A)  28 
B)  30 
C)  32 
D)  34

Question 17

Use the bond energies provided to estimate ΔrH° for the reaction below. CH3OH(l) + 2O2(g) → CO2(g) + 2H2O(g) ΔrH° = ?
Bond Bond Energy (kJ mol-1)
C-H 414
C-O 360
C=O 799
O=O 498
O-H 464

Accepted Answer

A)  +473 kJ mol-1 
B)  -91 kJ mol-1 
C)  -486 kJ mol-1 
D)  -392 kJ mol-1 
E)  +206 kJ mol-1 
A)  +473 kJ mol-1 
B)  -91 kJ mol-1 
C)  -486 kJ mol-1 
D)  -392 kJ mol-1 
E)  +206 kJ mol-1

Question 18

Identify the complete electronic configuration for Ca2+.

Accepted Answer

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

Question 19

List the following compounds in decreasing electronegativity difference. Cl2 HCl NaCl

Accepted Answer

A)  NaCl > Cl2 > HCl 
B)  Cl2 > HCl > NaCl 
C)  HCl > NaCl > Cl2 
D)  NaCl > HCl > Cl2 
A)  NaCl > Cl2 > HCl 
B)  Cl2 > HCl > NaCl 
C)  HCl > NaCl > Cl2 
D)  NaCl > HCl > Cl2

Question 20

Choose the compound below that should have the highest melting point according to the ionic bonding model.

Accepted Answer

A)  AlN 
B)  MgO 
C)  NaF 
D)  CaS 
E)  RbI 
A)  AlN 
B)  MgO 
C)  NaF 
D)  CaS 
E)  RbI

Exam 9: Chemical Bonding I: Lewis Theory

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

The iodine atom in I2 would be expected to have a ________.

Use Lewis theory to determine the chemical formula for the compound formed between Ca and N.

Which molecule or compound below contains a pure covalent bond?

Define formal charge.

How many of the following elements can form hypercoordinate compounds? I O Cl Xe

Explain why the lattice energy of MgS is approximately four times as large as that of NaCl.

Choose the best Lewis structure for CH2Cl2.

Which of the following processes is endothermic?

Choose the best Lewis structure for BeF2.

Which of the following processes is endothermic?

A double covalent bond contains ________ of electrons.

Of the following elements, which has the lowest electronegativity?

Identify the compound with covalent bonding.

Of the following elements, which has the highest electronegativity?

Give the number of valence electrons for SF4.

Use the bond energies provided to estimate ΔrH° for the reaction below. CH3OH(l) + 2O2(g) → CO2(g) + 2H2O(g) ΔrH° = ? Bond Bond Energy (kJ mol-1) C-H 414 C-O 360 C=O 799 O=O 498 O-H 464

Identify the complete electronic configuration for Ca2+.

List the following compounds in decreasing electronegativity difference. Cl2 HCl NaCl

Choose the compound below that should have the highest melting point according to the ionic bonding model.

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

The iodine atom in I₂ would be expected to have a ________.

Choose the best Lewis structure for CH₂Cl₂.

Choose the best Lewis structure for BeF₂.

Give the number of valence electrons for SF₄.

Use the bond energies provided to estimate Δ_rH° for the reaction below. CH₃OH(l) + 2O₂(g) → CO₂(g) + 2H₂O(g) Δ_rH°= ? Bond Bond Energy (kJ mol^-1) C-H 414 C-O 360 C=O 799 O=O 498 O-H 464

Identify the complete electronic configuration for Ca²⁺.

List the following compounds in decreasing electronegativity difference. Cl₂ HCl NaCl