Question 1

Place the following elements in order of increasing electronegativity. 
K$\quad$ Cs$\quad$ P

Accepted Answer

A) P < K < Cs 
B) K < P < Cs 
C) Cs < P < K 
D) Cs < K < P 
E) P < Cs < K 
A) P < K < Cs 
B) K < P < Cs 
C) Cs < P < K 
D) Cs < K < P 
E) P < Cs < K

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

Choose the best Lewis structure for BF3.

Accepted Answer

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

Question 4

Define bond energy.

Accepted Answer

Bond energy is the e

Question 5

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 6

Identify the compound with the highest magnitude of lattice energy.

Accepted Answer

A) NaCl 
B) KCl 
C) LiCl 
D) CsCl 
A) NaCl 
B) KCl 
C) LiCl 
D) CsCl

Question 7

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

Question 8

Choose the best Lewis structure for SF4.

Accepted Answer

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

Question 9

Describe the difference between a pure covalent bond and a polar covalent bond.

Accepted Answer

A pure covalent bond occurs when bonding

Question 10

Give the number of valence electrons for SO42-.

Accepted Answer

A) 32 
B) 30 
C) 34 
D) 28 
E) 36 
A) 32 
B) 30 
C) 34 
D) 28 
E) 36

Question 11

Identify the weakest 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 12

Identify the compound with the lowest magnitude of lattice energy.

Accepted Answer

A) KCl 
B) KBr 
C) SrO 
D) CaO 
A) KCl 
B) KBr 
C) SrO 
D) CaO

Question 13

Which compound has the highest carbon-carbon bond strength?

Accepted Answer

A) CH3CH3 
B) CH2CH2 
C) HCCH 
D) All bond strengths are the same. 
A) CH3CH3 
B) CH2CH2 
C) HCCH 
D) All bond strengths are the same.

Question 14

Choose the best Lewis structure for NH4+.

Accepted Answer

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

Question 15

Use Lewis theory to determine the chemical formula for the compound formed between Rb and S.

Accepted Answer

A) RbS 
B) RbS2 
C) Rb2S 
D) Rb2S3 
E) Rb3S2 
A) RbS 
B) RbS2 
C) Rb2S 
D) Rb2S3 
E) Rb3S2

Question 16

Draw the best Lewis structure for CH3+.What is the formal charge on the C?

Accepted Answer

A) 0 
B) 1 
C) -1 
D) 2 
E) -2 
A) 0 
B) 1 
C) -1 
D) 2 
E) -2

Question 17

Using periodic trends,place the following bonds in order of decreasing ionic character. 
Sb-Cl $\quad$P-Cl $\quad$As-Cl

Accepted Answer

A) Sb-Cl > As-Cl > P-Cl 
B) As-Cl > Sb-Cl > P-Cl 
C) P-Cl > Sb-Cl > As-Cl 
D) P-Cl > As-Cl > Sb-Cl 
E) Sb-Cl > P-Cl > As-Cl 
A) Sb-Cl > As-Cl > P-Cl 
B) As-Cl > Sb-Cl > P-Cl 
C) P-Cl > Sb-Cl > As-Cl 
D) P-Cl > As-Cl > Sb-Cl 
E) Sb-Cl > P-Cl > As-Cl

Question 18

Use the data given below to construct a Born-Haber cycle to determine the heat of formation of KCl. 
$$\begin{array} { l c } 
& \Delta H ^ { \circ } \left( \mathrm { kJ } \text { mol} ^ { - 1 } \right) \
\mathrm { K } ( s ) \rightarrow \mathrm { K } ( g ) & 89 \
\mathrm {~K} ( g ) \rightarrow \mathrm { K } ^ { + } ( g ) + \mathrm { e } ^ { - } & 418 \
\mathrm { Cl } 2 ( g ) \rightarrow 2 \mathrm { Cl } ( g ) & 244 \
\mathrm { Cl } ( g ) + \mathrm { e } ^ { - } \rightarrow \mathrm { Cl } ^ { - } ( g ) & - 349 \
\mathrm { KCl } ( s ) \rightarrow \mathrm { K } ^ { + } ( g ) + \mathrm { Cl } ^ { - } ( g ) & 717
\end{array}$$

Accepted Answer

A) -1119 kJ mol-1 
B) -997 kJ mol-1 
C) -437 kJ mol-1 
D) +631 kJ mol-1 
E) +158 kJ mol-1 
A) -1119 kJ mol-1 
B) -997 kJ mol-1 
C) -437 kJ mol-1 
D) +631 kJ mol-1 
E) +158 kJ mol-1

Question 19

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 20

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

Exam 9: Chemical Bonding I: Lewis Theory

Place the following elements in order of increasing electronegativity. K \quad Cs \quad P

The iodine atom in I2 would be expected to have a

Choose the best Lewis structure for BF3.

Define bond energy.

Which molecule or compound below contains a pure covalent bond?

Identify the compound with the highest magnitude of lattice energy.

Choose the best Lewis structure for SF4.

Describe the difference between a pure covalent bond and a polar covalent bond.

Give the number of valence electrons for SO42-.

Identify the weakest bond.

Identify the compound with the lowest magnitude of lattice energy.

Which compound has the highest carbon-carbon bond strength?

Choose the best Lewis structure for NH4+.

Use Lewis theory to determine the chemical formula for the compound formed between Rb and S.

Draw the best Lewis structure for CH3+.What is the formal charge on the C?

Using periodic trends,place the following bonds in order of decreasing ionic character. Sb-Cl \quad P-Cl \quad As-Cl

Use the data given below to construct a Born-Haber cycle to determine the heat of formation of KCl. \Delta (s)\rightarrow(g) 89 (g)\rightarrow(g)+ 418 2(g)\rightarrow2(g) 244 (g)+\rightarrow(g) -349 (s)\rightarrow(g)+(g) 717

Choose the bond below that is the strongest.

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

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

Place the following elements in order of increasing electronegativity. K $\quad$ Cs $\quad$ P

The iodine atom in I₂ would be expected to have a

Choose the best Lewis structure for BF₃.

Choose the best Lewis structure for SF₄.

Give the number of valence electrons for SO₄^2-.

Choose the best Lewis structure for NH₄⁺.

Draw the best Lewis structure for CH₃⁺.What is the formal charge on the C?

Using periodic trends,place the following bonds in order of decreasing ionic character. Sb-Cl $\quad$ P-Cl $\quad$ As-Cl

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