Question 1

Which of the following statements is true?

Accepted Answer

A) An ionic bond is much stronger than most covalent bonds. 
B) An ionic bond is formed through the sharing of electrons. 
C) Ionic compounds at room temperature typically conduct electricity. 
D) Once dissolved in water,ionic compounds rarely conduct electricity. 
E) None of the above are true. 
A) An ionic bond is much stronger than most covalent bonds. 
B) An ionic bond is formed through the sharing of electrons. 
C) Ionic compounds at room temperature typically conduct electricity. 
D) Once dissolved in water,ionic compounds rarely conduct electricity. 
E) None of the above are true.

Question 2

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

Question 3

How many of the following elements can form compounds with an expanded octet?
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 4

Use Lewis theory to determine the chemical formula for the compound formed between Al and O.

Accepted Answer

A) Al3O2 
B) Al2O3 
C) AlO2 
D) Al2O 
E) AlO 
A) Al3O2 
B) Al2O3 
C) AlO2 
D) Al2O 
E) AlO

Question 5

Choose the best Lewis structure for SeO42⁻.

Accepted Answer

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

Question 6

Place the following elements in order of increasing electronegativity.
K Cs 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 7

Match the following.
-Cs-I

Accepted Answer

A) weakest ionic bond 
B) strongest covalent bond 
C) metallic bond 
D) highest melting point 
E) longest covalent bond
F)Na-Br
G)C-F 
A) weakest ionic bond 
B) strongest covalent bond 
C) metallic bond 
D) highest melting point 
E) longest covalent bond
F)Na-Br
G)C-F

Question 8

Using periodic trends,place the following bonds in order of increasing ionic character.
Si-P Si-Cl Si-S

Accepted Answer

A) Si-P < Si-Cl < Si-S 
B) Si-P < Si-S < Si-Cl 
C) Si-S < Si-Cl < Si-P 
D) Si-Cl < Si-P < Si-S 
E) Si-Cl < Si-S < Si-P 
A) Si-P < Si-Cl < Si-S 
B) Si-P < Si-S < Si-Cl 
C) Si-S < Si-Cl < Si-P 
D) Si-Cl < Si-P < Si-S 
E) Si-Cl < Si-S < Si-P

Question 9

Use Lewis theory to determine the chemical formula for the compound formed between K and I.

Accepted Answer

A) KI2 
B) K2I 
C) KI 
D) K2I2 
A) KI2 
B) K2I 
C) KI 
D) K2I2

Question 10

Choose the bond below that is the weakest.

Accepted Answer

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

Question 11

How many of the following elements can form compounds with an expanded octet?
Pb Kr Si B

Accepted Answer

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

Question 12

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 13

The compound ClF contains

Accepted Answer

A) ionic bonds. 
B) nonpolar covalent bonds. 
C) polar covalent bonds with partial negative charges on the F atoms. 
D) polar covalent bonds with partial negative charges on the Cl atoms. 
A) ionic bonds. 
B) nonpolar covalent bonds. 
C) polar covalent bonds with partial negative charges on the F atoms. 
D) polar covalent bonds with partial negative charges on the Cl atoms.

Question 14

Choose the best Lewis structure for SF4.

Accepted Answer

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

Question 15

Using periodic trends,place the following bonds in order of increasing ionic character.
S-F Se-F O-F

Accepted Answer

A) Se-F < S-F < O-F 
B) S-F < Se-F < O-F 
C) O-F < Se-F < S-F 
D) Se-F < O-F < S-F 
E) O-F < S-F < Se-F 
A) Se-F < S-F < O-F 
B) S-F < Se-F < O-F 
C) O-F < Se-F < S-F 
D) Se-F < O-F < S-F 
E) O-F < S-F < Se-F

Question 16

Place the following in order of increasing bond length.
NO2⁻ NO3⁻ NO

Accepted Answer

A) NO 2⁻ 3⁻ 
B) NO2⁻ 3⁻ 3⁻ 2⁻ 
D) NO 3⁻ 2⁻ 
E) NO3⁻ 2⁻ < NO 
A) NO 2⁻ 3⁻ 
B) NO2⁻ 3⁻ 3⁻ 2⁻ 
D) NO 3⁻ 2⁻ 
E) NO3⁻ 2⁻ < NO

Question 17

Use the bond energies provided to estimate ΔH°rxn for the reaction below.
PCl3(g)+ Cl2(g)→ PCl5(l)ΔH°rxn = ?
Bond Bond Energy (kJ/mol)
Cl-Cl 243
P-Cl 331

Accepted Answer

A) -243 kJ 
B) -419 kJ 
C) -662 kJ 
D) -67 kJ 
E) -905 kJ 
A) -243 kJ 
B) -419 kJ 
C) -662 kJ 
D) -67 kJ 
E) -905 kJ

Question 18

In the Lewis structure of CH3OH,how many bonding pairs of electrons are there?

Accepted Answer

A) 2 
B) 7 
C) 5 
D) 3 
A) 2 
B) 7 
C) 5 
D) 3

Question 19

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 20

How many lone pairs of electrons are on the As atom in AsCl3?

Accepted Answer

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

Which of the following statements is true?

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

How many of the following elements can form compounds with an expanded octet? I O Cl Xe

Use Lewis theory to determine the chemical formula for the compound formed between Al and O.

Choose the best Lewis structure for SeO₄²⁻.

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

Match the following. -Cs-I

Using periodic trends,place the following bonds in order of increasing ionic character. Si-P Si-Cl Si-S

Use Lewis theory to determine the chemical formula for the compound formed between K and I.

Choose the bond below that is the weakest.

How many of the following elements can form compounds with an expanded octet? Pb Kr Si B

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

The compound ClFcontains

Choose the best Lewis structure for SF₄.

Using periodic trends,place the following bonds in order of increasing ionic character. S-F Se-F O-F

Place the following in order of increasing bond length. NO₂⁻ NO₃⁻ NO

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. PCl₃(g)+ Cl₂(g)→ PCl₅(l)ΔH°_rxn= ? Bond Bond Energy (kJ/mol) Cl-Cl 243 P-Cl 331

In the Lewis structure of CH₃OH,how many bonding pairs of electrons are there?

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

How many lone pairs of electrons are on the As atom in AsCl₃?

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

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Filters

Exam 9: Chemical Bonding I: Lewis Theory

Which of the following statements is true?

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

How many of the following elements can form compounds with an expanded octet? I O Cl Xe

Use Lewis theory to determine the chemical formula for the compound formed between Al and O.

Choose the best Lewis structure for SeO42⁻.

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

Match the following. -Cs-I

Using periodic trends,place the following bonds in order of increasing ionic character. Si-P Si-Cl Si-S

Use Lewis theory to determine the chemical formula for the compound formed between K and I.

Choose the bond below that is the weakest.

How many of the following elements can form compounds with an expanded octet? Pb Kr Si B

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

The compound ClF contains

Choose the best Lewis structure for SF4.

Using periodic trends,place the following bonds in order of increasing ionic character. S-F Se-F O-F

Place the following in order of increasing bond length. NO2⁻ NO3⁻ NO

Use the bond energies provided to estimate ΔH°rxn for the reaction below. PCl3(g)+ Cl2(g)→ PCl5(l)ΔH°rxn = ? Bond Bond Energy (kJ/mol) Cl-Cl 243 P-Cl 331

In the Lewis structure of CH3OH,how many bonding pairs of electrons are there?

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

How many lone pairs of electrons are on the As atom in AsCl3?

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

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

Choose the best Lewis structure for SeO₄²⁻.

The compound ClFcontains

Choose the best Lewis structure for SF₄.

Place the following in order of increasing bond length. NO₂⁻ NO₃⁻ NO

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. PCl₃(g)+ Cl₂(g)→ PCl₅(l)ΔH°_rxn= ? Bond Bond Energy (kJ/mol) Cl-Cl 243 P-Cl 331

In the Lewis structure of CH₃OH,how many bonding pairs of electrons are there?

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

How many lone pairs of electrons are on the As atom in AsCl₃?