Deck 9: Chemical Bonding I: Lewis Theory

Question 1

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

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

Answer 1

NaF > KCl > RbBr

Question 2

Use the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO. DH°(kJ)
Ca(s)→ Ca(g)193
Ca(g)→ Ca⁺(g)+ e⁻ 590
Ca⁺(g)→ Ca²⁺(g)+ e⁻ 1010
2 O(g)→ O₂(g)-498
O(g)+ e⁻ → O⁻(g)-141
O⁻(g)+ e⁻ → O²⁻(g)878
Ca(s)+ O₂(g)→ CaO(s)-635

A) -3414 kJ
B) +1397 kJ
C) -2667 kJ
D) +3028 kJ
E) -2144 kJ

Answer 2

-3414 kJ

Question 3

Give the complete electronic configuration for Ca²⁺.

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

Answer 3

1s²2s²2p⁶3s²3p⁶

Question 4

Give the complete electronic configuration for Br^-.

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

Question 5

Give the complete electronic configuration for S^2-.

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

Question 6

Use the data given below to construct a Born-Haber cycle to determine the second ionization energy of Ca. DH°(kJ)
Ca(s)→ Ca(g)193
Ca(g)→ Ca⁺(g)+ e⁻ 590.
2 O(g)→ O₂(g)-498
O(g)+ e⁻ → O⁻(g)-141
O⁻(g)+ e⁻ → O²⁻(g)878
Ca(s)+ O₂(g)→ CaO(s)-635
Ca²⁺(g)+ O²⁻(g)→ CaO(s)-3414

A) 1010 kJ
B) 1757 kJ
C) 1508 kJ
D) -3027 kJ
E) -1514 kJ

Question 7

Place the following in order of increasing magnitude of lattice energy. CaO MgO SrS

A) MgO < CaO < SrS
B) SrS < MgO < CaO
C) SrS < CaO < MgO
D) CaO < MgO < SrS
E) CaO < SrS < MgO

Question 8

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

A)
B)
C)
D)
E)

Question 9

Which of the following represents the Lewis structure for Cl?

A)
B)
C)
D)
E)

Question 10

Which of the following represents the Lewis structure for Br⁻?

A)
B)
C)
D)
E)

Question 11

Place the following in order of decreasing magnitude of lattice energy. K₂O Rb₂S Li₂O

A) Li₂O > K₂O > Rb₂S
B) Li₂O > Rb₂S > K₂O
C) Rb₂S > K₂O > Li₂O
D) Rb₂S > Li₂O > K₂O
E) K₂O > Li₂O > Rb₂S

Question 12

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

A)
B)
C)
D)
E)

Question 13

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

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

Question 14

Use the data given below to construct a Born-Haber cycle to determine the electron affinity of Br. DH°(kJ)
K(s)→ K(g)89
K(g)→ K⁺(g)+ e⁻ 419
Br₂(l)→ 2 Br(g)193
K(s)+ Br₂(g)→ KBr(s)-394
KBr(s)→ K⁺(g)+ Br⁻(g)674

A) -885 kJ
B) -325 kJ
C) +367 kJ
D) -464 kJ
E) +246 kJ

Question 15

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

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

Question 16

Which of the following represents the Lewis structure for N?

A)
B)
C)
D)
E)

Question 17

Which of the following statements is TRUE?

A) A covalent bond is formed through the transfer of electrons from one atom to another.
B) A pair of electrons involved in a covalent bond is sometimes referred to as a "lone pair."
C) It is not possible for two atoms to share more than two electrons.
D) Single bonds are shorter than double bonds.
E) In a covalent bond, the shared electrons interact with the nuclei of both of the bonding atoms, thus lowering their potential energy.

Question 18

Which of the following statements is 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 is true.

Question 19

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

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

Question 20

Which of the following represents the Lewis structure for Mg?

A)
B)
C)
D)
E)

Question 21

Choose the best Lewis structure for SF₄.

A)

B)

C)

D)

E)

Question 22

Choose the best Lewis structure for SeO₄²⁻.

A)

B)

C)

D)

E)

Question 23

Identify the shortest bond.

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

Question 24

Choose the best Lewis structure for PO₄³⁻.

A)

B)

C)

D)

E)

Question 25

Choose the best Lewis structure for OCl₂.

A)
B)
C)
D)
E)

Question 26

Identify the number of bonding pairs and lone pairs of electrons in water.

A) 1 bonding pair and 1 lone pair
B) 1 bonding pair and 2 lone pairs
C) 2 bonding pairs and 2 lone pairs
D) 2 bonding pairs and 1 lone pair
E) 3 bonding pairs and 2 lone pairs

Question 27

Define electronegativity.

A) the ability of an atom to repel neutrons in a chemical bond
B) the ability of an atom to repel electrons in a chemical bond
C) the ability of an atom to attract protons to itself in a chemical bond
D) the ability of an atom to attract neutrons to itself in a chemical bond
E) the ability of an atom to attract electrons to itself in a chemical bond

Question 28

Choose the best Lewis structure for BeF₂.

A)
B)
C)
D)
E)

Question 29

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

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

Question 30

Give the number of valence electrons for ICl₅.

A) 36
B) 40
C) 42
D) 44
E) 46

Question 31

Choose the best Lewis structure for XeI₂.

A)
B)
C)
D)
E)

Question 32

Choose the best Lewis structure for ICl₅.

A)

B)

C)

D)

E)

Question 33

Give the number of valence electrons for XeI₂.

A) 22
B) 20
C) 18
D) 24
E) 16

Question 34

Choose the best Lewis structure for SO₄²⁻.

A)

B)

C)

D)

E)

Question 35

Identify the strongest bond.

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

Question 36

Choose the best Lewis structure for NO₃⁻.

A)

B)

C)

D)

E)

Question 37

Identify the weakest bond.

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

Question 38

Choose the best Lewis structure for CH₂Cl₂.

A)

B)

C)

D)

E)

Question 39

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

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 40

Choose the best Lewis structure for BF₃.

A)

B)

C)

D)

E)

Question 41

Draw the Lewis structure for CO₃^2- including any valid resonance structures.Which of the following statements is TRUE?

A) The CO₃^2- ion contains one C-O single bond and two C O double bonds.
B) The CO₃^2- ion contains two C-O single bonds and one C O double bond.
C) The CO₃^2- ion contains three C-O double bonds.
D) The CO₃^2- ion contains two C-O single bonds and one C O triple bond.
E) None of the above is true.

Question 42

Place the following in order of decreasing bond length. H-F H-I H-Br

A) H-F > H-Br > H-I
B) H-I > H-F > H-Br
C) H-I > H-Br > H-F
D) H-Br > H-F > H-I
E) H-F > H-I > H-Br

Question 43

Rank the following molecules in decreasing bond energy. Cl₂ Br₂ F₂ I₂

A) I₂ > Br₂ > Cl₂ > F₂
B) Cl₂ > Br₂ > F₂ > I₂
C) I₂ > Cl₂ > Br₂ > F₂
D) Cl₂ > I₂ > F₂ > Br₂

Question 44

Draw the best Lewis structure for Cl₃⁻.What is the formal charge on the central Cl atom?

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

Question 45

Place the following in order of increasing bond length. C-O C-C C-N

A) C-C < C-N < C-O
B) C-N < C-O < C-C
C) C-O < C-C < C-N
D) C-O < C-N < C-C
E) C-C < C-O < C-N

Question 46

Which compound has the shortest carbon-carbon bond length?

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

Question 47

Using Lewis structures and formal charge,which of the following ions is most stable,? OCN⁻ ONC⁻ NOC⁻

A) OCN⁻
B) ONC⁻
C) NOC⁻
D) None of these ions are stable according to Lewis theory.
E) All of these compounds are equally stable according to Lewis theory.

Question 48

Which of the following resonance structures for OCN⁻ will contribute most to the correct structure of OCN⁻?

A) O C
N, with two lone pairs on O and two lone pairs on N
B) O C-N, with one lone pair on O and three lone pairs on N
C) O C
N, with one lone pair on O, two lone pairs on C, and one lone pair on N
D) O-C N, with three lone pairs on O and one lone pair on N
E) They all contribute equally to the correct structure of OCN⁻.

Question 49

Choose the best Lewis structure for NH₄⁺.

A)

B)

C)

D)

E)

Question 50

Identify the bond with the highest bond energy.

A) Si=O
B) N=N
C) C=C
D) C=N
E) O=O

Question 51

Define bond energy.

A) energy required to form 1 mole of the bond in the solid phase
B) energy required to form 1 mole of the bond in the gas phase
C) energy required to break 1 mole of the bond in the liquid phase
D) energy required to break 1 mole of the bond in the gas phase
E) energy required to break 1 mole of the bond in the solid phase

Question 52

Place the following in order of decreasing XO bond length,where "X" represents the central atom in each of the following compounds or ions. SiO₃²⁻ CO₂ CO₃²⁻

A) CO₂ > SiO₃²⁻ > CO₃²⁻
B) CO₂ > CO₃²⁻ > SiO₃²⁻
C) CO₃²⁻ > CO₂ > SiO₃²⁻
D) CO₃²⁻ > SiO₃²⁻ > CO₂
E) SiO₃²⁻ > CO₃²⁻ > CO₂

Question 53

The Lewis structure of sulfuric acid contains

A) 2 double bonds, 4 single bonds, and 8 lone pairs.
B) 4 double bonds, and two single bonds.
C) 2 double bonds and 4 single bonds.
D) 6 single bonds and 4 lone pairs.
E) 2 double bonds, 4 single bonds, and 4 lone pairs.

Question 54

Which compound has the highest carbon-carbon bond strength?

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

Question 55

How many electrons does an hydroxyl radical contain?

A) 7 electrons
B) 6 electrons
C) 8 electrons
D) 9 electrons
E) 5 electrons

Question 56

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

A) NO < NO₂⁻ < NO₃⁻
B) NO₂⁻ < NO₃⁻ < NO
C) NO₃⁻ < NO < NO₂⁻
D) NO < NO₃⁻ < NO₂⁻
E) NO₃⁻ < NO₂⁻ < NO

Question 57

Draw the Lewis structure for NO₂⁻ including any valid resonance structures.Describe the resonance hybrid of the nitrite ion.

A) The nitrite ion contains one N-O single bond and one N O double bond.
B) The nitrite ion contains two N-O bonds that are equivalent to 1 bonds.
C) The nitrite ion contains two N O double bonds.
D) The nitrite ion contains two N-O single bonds.
E) None of the above is true.

Question 58

A reaction is exothermic when

A) weak bonds break and strong bonds form.
B) strong bonds break and weak bonds form.
C) weak bonds break and weak bonds form.
D) strong bonds break and strong bonds form.

Question 59

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

A) 6
B) 2
C) 4
D) 3
E) 8

Question 60

Which compound has the longest carbon-carbon bond length?

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

Question 61

Identify the compound with ionic bonding.

A) LiBr
B) Na
C) H₂O
D) Ne
E) O

Question 62

Identify the compound with covalent bonding.

A) KBr
B) K
C) H₂Se
D) Ne
E) O

Question 63

Identify the property of metals that is NOT explained by the electron sea model.

A) metals conduct heat
B) metals conduct electricity
C) malleability of metals
D) most metals are liquids
E) ductility of metals

Question 64

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

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

Question 65

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

A) LiS
B) LiS₂
C) Li₂S
D) Li₂S₃
E) Li₃S₂

Question 66

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. XeF_{2 +} 2 F₂ → XeF₆ ΔH°_rxn = ?
Bond Bond Energy (kJ/mol)
Xe-F 147
F-F 159

A) -429 kJ
B) +159 kJ
C) -660 kJ
D) +176 kJ
E) -270 kJ

Question 67

Identify the bond with the lowest bond energy.

A) Si=O
B) N=N
C) C=C
D) C=N
E) O=O

Question 68

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

A) Al₃F₂
B) Al₂F₃
C) AlF₂
D) AlF
E) AlF₃

Question 69

Identify an ionic bond.

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

Question 70

Identify the compound with metallic bonding.

A) LiI
B) Na
C) H₂O
D) He
E) S

Question 71

Ozone absorbs

A) infrared light entering Earth's atmosphere.
B) ultraviolet light exiting Earth's atmosphere.
C) ultraviolet light entering Earth's atmosphere.
D) visible light entering Earth's atmosphere.
E) infrared light exiting Earth's atmosphere.

Question 72

Use Lewis theory to determine the chemical formula for the compound formed between Ba and F.

A) BaF
B) Ba₂F₃
C) Ba₃F₂
D) BaF₂
E) Ba₂F

Question 73

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

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

Question 74

Identify the bond with the highest bond energy.

A) C≡O
B) C≡C
C) C≡N
D) N≡N

Question 75

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

A) SrN
B) Sr₃N₂
C) SrN₂
D) Sr₂N
E) Sr₂N₃

Question 76

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

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

Question 77

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. 2 Br₂(l)+ C₂H₂(g)→ C₂H₂Br₄(l)ΔH°_rxn = ?
Bond Bond Energy (kJ/mol)
Br-Br 193
C≡C 837
C-C 347
C-Br 276
C-H 414

A) +407 kJ
B) -324 kJ
C) -228 kJ
D) +573 kJ
E) -648 kJ

Question 78

Identify the bond with the highest bond energy.

A) C≡O
B) C≡C
C) C≡N
D) N≡N

Question 79

Identify the substance that conducts electricity.

A) KBr dissolved in water
B) solid KBr
C) rubbing alcohol
D) solid baking soda
E) sugar dissolved in water.

Question 80

Identify the chemical formula for ozone.

A) O₃
B) O₂
C) O
D) O^2-
E) O^-