Question 1

Choose the best Lewis structure for SF4.

Accepted Answer

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

Question 2

Which of the following represent the Lewis structure for Ca2⁺?

Accepted Answer

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

Question 3

A single 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 B

Question 4

Identify the shortest bond.

Accepted Answer

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

Question 5

Use the bond energies provided to estimate ΔrH° for the reaction below. C2H4(g)+ H2(g)→ C2H6(g)ΔrH° = ?
Bond Bond Energy (kJ mol-1)
C-C 347
C-H 414
C=C 611
C≡C 837
H-H 436

Accepted Answer

A) -128 kJ mol-1 
B) +98 kJ mol-1 
C) +700 kJ mol-1 
D) -102 kJ mol-1 
E) -166 kJ mol-1 
A) -128 kJ mol-1 
B) +98 kJ mol-1 
C) +700 kJ mol-1 
D) -102 kJ mol-1 
E) -166 kJ mol-1

Question 6

Which of the following represent the Lewis structure for S2⁻?

Accepted Answer

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

Question 7

Use the data given below to construct a Born-Haber cycle to determine the heat of formation of KCl. ΔH°(kJ mol-1)
K(s)→ K(g)89
K(g)→ K⁺(g)+ e⁻ 418
Cl2(g)→ 2Cl(g)244
Cl(g)+ e⁻ → Cl⁻(g)-349
KCl(s)→ K⁺(g)+ Cl⁻(g)717

Accepted Answer

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

Question 8

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 9

Identify the number of valence electrons for XeI2.

Accepted Answer

A) 22 
B) 20 
C) 18 
D) 24 
A) 22 
B) 20 
C) 18 
D) 24

Question 10

Define dipole moment.

Accepted Answer

Dipole moment is the measured

Question 11

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

Accepted Answer

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

Question 12

Which of the following represent the Lewis structure for N?

Accepted Answer

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

Question 13

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 14

Identify the compound with metallic bonding.

Accepted Answer

A) NaCl 
B) Li 
C) H2O 
D) He 
E) S 
A) NaCl 
B) Li 
C) H2O 
D) He 
E) S

Question 15

Use the bond energies provided to estimate ΔrH° for the reaction below. PCl3(g)+ Cl2(g)→ PCl5(l)ΔrH° = ?
Bond Bond Energy (kJ mol-1)
Cl-Cl 243
P-Cl 331

Accepted Answer

A) -243 kJ mol-1 
B) -419 kJ mol-1 
C) -662 kJ mol-1 
D) -67 kJ mol-1 
E) -905 kJ mol-1 
A) -243 kJ mol-1 
B) -419 kJ mol-1 
C) -662 kJ mol-1 
D) -67 kJ mol-1 
E) -905 kJ mol-1

Question 16

Draw the best Lewis structure for CH3+1. 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 17

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 18

Choose the bond below that is the strongest.

Accepted Answer

A) C-F 
B) C=O 
C) C-I 
D) I-I 
E) C≡N 
A) C-F 
B) C=O 
C) C-I 
D) I-I 
E) C≡N

Question 19

38)Use the data given below to construct a Born-Haber cycle to determine the bond energy of O2. ΔH°(kJ mol-1)
Na(s)→ Na(g)107
Na(g)→ Na⁺(g)+ e⁻ 496
O(g)+ e⁻ → O⁻(g)-141
O⁻(g)+ e⁻ → O2⁻(g)878
2Na(s)+   O2(g)→ Na2O(s)-416
2Na⁺(g)+ O2⁻(g)→ Na2O(s)-2608

Accepted Answer

A) 426 kJ 
B) 249 kJ 
C) 852 kJ 
D) 498 kJ 
E) 356 kJ 
A) 426 kJ 
B) 249 kJ 
C) 852 kJ 
D) 498 kJ 
E) 356 kJ

Question 20

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.

Exam 9: Chemical Bonding I: Lewis Theory

Choose the best Lewis structure for SF4.

Which of the following represent the Lewis structure for Ca2⁺?

A single covalent bond contains ________ of electrons.

Identify the shortest bond.

Use the bond energies provided to estimate ΔrH° for the reaction below. C2H4(g)+ H2(g)→ C2H6(g)ΔrH° = ? Bond Bond Energy (kJ mol-1) C-C 347 C-H 414 C=C 611 C≡C 837 H-H 436

Which of the following represent the Lewis structure for S2⁻?

Use the data given below to construct a Born-Haber cycle to determine the heat of formation of KCl. ΔH°(kJ mol-1) K(s)→ K(g)89 K(g)→ K⁺(g)+ e⁻ 418 Cl2(g)→ 2Cl(g)244 Cl(g)+ e⁻ → Cl⁻(g)-349 KCl(s)→ K⁺(g)+ Cl⁻(g)717

Which of the following processes is exothermic?

Identify the number of valence electrons for XeI2.

Define dipole moment.

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

Which of the following represent the Lewis structure for N?

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

Identify the compound with metallic bonding.

Use the bond energies provided to estimate ΔrH° for the reaction below. PCl3(g)+ Cl2(g)→ PCl5(l)ΔrH° = ? Bond Bond Energy (kJ mol-1) Cl-Cl 243 P-Cl 331

Draw the best Lewis structure for CH3+1. What is the formal charge on the C?

Identify the complete electronic configuration for Ca2+.

Choose the bond below that is the strongest.

38)Use the data given below to construct a Born-Haber cycle to determine the bond energy of O2. ΔH°(kJ mol-1) Na(s)→ Na(g)107 Na(g)→ Na⁺(g)+ e⁻ 496 O(g)+ e⁻ → O⁻(g)-141 O⁻(g)+ e⁻ → O2⁻(g)878 2Na(s)+ O2(g)→ Na2O(s)-416 2Na⁺(g)+ O2⁻(g)→ Na2O(s)-2608

The iodine atom in I2 would be expected to have a

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Filters

Choose the best Lewis structure for SF₄.

Which of the following represent the Lewis structure for Ca²⁺?

Use the bond energies provided to estimate Δ_rH° for the reaction below. C₂H₄(g)+ H₂(g)→ C₂H₆(g)Δ_rH°= ? Bond Bond Energy (kJ mol^-1) C-C 347 C-H 414 C=C 611 C≡C 837 H-H 436

Which of the following represent the Lewis structure for S²⁻?

Use the data given below to construct a Born-Haber cycle to determine the heat of formation of KCl. ΔH°(kJ mol^-1) K(s)→ K(g)89 K(g)→ K⁺(g)+ e⁻ 418 Cl₂(g)→ 2Cl(g)244 Cl(g)+ e⁻ → Cl⁻(g)-349 KCl(s)→ K⁺(g)+ Cl⁻(g)717

Identify the number of valence electrons for XeI₂.

Use the bond energies provided to estimate Δ_rH° for the reaction below. PCl₃(g)+ Cl₂(g)→ PCl₅(l)Δ_rH°= ? Bond Bond Energy (kJ mol^-1) Cl-Cl 243 P-Cl 331

Draw the best Lewis structure for CH₃⁺¹. What is the formal charge on the C?

Identify the complete electronic configuration for Ca²⁺.

38)Use the data given below to construct a Born-Haber cycle to determine the bond energy of O₂. ΔH°(kJ mol^-1) Na(s)→ Na(g)107 Na(g)→ Na⁺(g)+ e⁻ 496 O(g)+ e⁻ → O⁻(g)-141 O⁻(g)+ e⁻ → O²⁻(g)878 2Na(s)+ O₂(g)→ Na₂O(s)-416 2Na⁺(g)+ O²⁻(g)→ Na₂O(s)-2608

The iodine atom in I₂ would be expected to have a