Question 1

Which of the following represent the Lewis structure for Cl?

Accepted Answer

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

Question 2

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 3

Draw the best Lewis structure for BrO4⁻. What is the formal charge on bromine?

Accepted Answer

A) -1 
B) +1 
C) 0 
D) +2 
E) +3 
A) -1 
B) +1 
C) 0 
D) +2 
E) +3

Question 4

How many of the following elements can form hypercoordinate compounds? 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 5

Which ionic compound would be expected to have the highest lattice energy?

Accepted Answer

A) Rb2O 
B) SrO  
C) In2O3 
D) CO2 
A) Rb2O 
B) SrO  
C) In2O3 
D) CO2

Question 6

Identify the complete electronic configuration for Br-.

Accepted Answer

A) 1s22s22p63s23p64s24p6 
B) 1s22s22p63s23p64s24d104p6 
C) 1s22s22p63s23p64s23d104p6 
D) 1s22s22p63s23p64s23d104p5 
E) 1s22s2p63s2p64s23d104p6 
A) 1s22s22p63s23p64s24p6 
B) 1s22s22p63s23p64s24d104p6 
C) 1s22s22p63s23p64s23d104p6 
D) 1s22s22p63s23p64s23d104p5 
E) 1s22s2p63s2p64s23d104p6

Question 7

Place the following in order of decreasing magnitude of lattice energy. NaF RbBr KCl

Accepted Answer

A) RbBr > NaF > KCl 
B) NaF > KCl > RbBr 
C) KCl > NaF > RbBr 
D) NaF > RbBr > KCl 
E) RbBr > KCl > NaF 
A) RbBr > NaF > KCl 
B) NaF > KCl > RbBr 
C) KCl > NaF > RbBr 
D) NaF > RbBr > KCl 
E) RbBr > KCl > NaF

Question 8

Which element can act as the centre atom in a hypercoordinate compound?

Accepted Answer

A) N 
B) O 
C) Br 
D) He 
A) N 
B) O 
C) Br 
D) He

Question 9

How many lone pairs of electrons are on the S atom in SF4?

Accepted Answer

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

Question 10

Match the following.

-C=N

Accepted Answer

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

Question 11

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

Question 12

Choose the best Lewis structure for OCl2.

Accepted Answer

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

Question 13

Choose the bond below that is the weakest.

Accepted Answer

A) Na-Cl 
B) I-I 
C) C=N 
D) Li-F 
E) C=O 
A) Na-Cl 
B) I-I 
C) C=N 
D) Li-F 
E) C=O

Question 14

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 15

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 16

Place the following elements in order of increasing electronegativity. Sr N Na

Accepted Answer

A) Sr < Na < N 
B) Na < N < Sr 
C) Sr < N < Na 
D) N < Sr < Na 
E) N < Na < Sr 
A) Sr < Na < N 
B) Na < N < Sr 
C) Sr < N < Na 
D) N < Sr < Na 
E) N < Na < Sr

Question 17

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 18

Which of the following compounds is hypercoordinate?

Accepted Answer

A) CsI 
B) SnO2 
C) ClF5 
D) ClF 
A) CsI 
B) SnO2 
C) ClF5 
D) ClF

Question 19

Identify an ionic bond.

Accepted Answer

A) Electrons are pooled. 
B) Electrons are shared. 
C) Electrons are transferred. 
D) Electrons are gained. 
E) Electrons are lost. 
A) Electrons are pooled. 
B) Electrons are shared. 
C) Electrons are transferred. 
D) Electrons are gained. 
E) Electrons are lost.

Question 20

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.

Exam 9: Chemical Bonding I: Lewis Theory

Which of the following represent the Lewis structure for Cl?

Which of the following processes is endothermic?

Draw the best Lewis structure for BrO4⁻. What is the formal charge on bromine?

How many of the following elements can form hypercoordinate compounds? Pb Kr Si B

Which ionic compound would be expected to have the highest lattice energy?

Identify the complete electronic configuration for Br-.

Place the following in order of decreasing magnitude of lattice energy. NaF RbBr KCl

Which element can act as the centre atom in a hypercoordinate compound?

How many lone pairs of electrons are on the S atom in SF4?

Match the following. -C=N

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

Choose the best Lewis structure for OCl2.

Choose the bond below that is the weakest.

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

Identify the strongest bond.

Place the following elements in order of increasing electronegativity. Sr N Na

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

Which of the following compounds is hypercoordinate?

Identify an ionic bond.

The compound ClF contains

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 Metallury

Transition Metals and Coordination Compounds

Filters

Draw the best Lewis structure for BrO₄⁻. What is the formal charge on bromine?

Identify the complete electronic configuration for Br^-.

How many lone pairs of electrons are on the S atom in SF₄?

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

Choose the best Lewis structure for OCl₂.

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