Deck 9: Chemical Bonding I: Lewis Theory

Question 1

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

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

Answer 1

Rb₂S

Question 2

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.

Answer 2

An ionic bond is much stronger than most covalent bonds.

Question 3

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

A) CaN
B) Ca₃N₂
C) CaN₂
D) Ca₂N
E) Ca₂N₃

Answer 3

Ca₃N₂

Question 4

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

A)
B)
C)
D)
E)

Question 5

Which of the following represent the Lewis structure for Cl?

A)
B)
C)
D)
E)

Question 6

Identify the compound with ionic bonding.

A) NaCl
B) CH₄
C) H₂O
D) H₂
E) CO₂

Question 7

Identify an ionic bond.

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

Question 8

Identify the compound with covalent bonding.

A) NaF
B) CaO
C) CH₃NH₂
D) K₂O
E) SrBr₂

Question 9

Identify the compound or element with metallic bonding.

A) NaCl
B) Li
C) H₂O
D) He
E) S

Question 10

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

A)
B)
C)
D)
E)

Question 11

Which of the following represent the Lewis structure for Mg?

A)
B)
C)
D)
E)

Question 12

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

A)
B)
C)
D)
E)

Question 13

Identify the compound with ionic bonding.

A) H₂O
B) CH₄
C) H₂
D) CO₂
E) RbF

Question 14

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 are sometimes referred to as "lone pairs."
C) It is not possible for two atoms to share more than two electrons.
D) Single bonds are shorter than double bonds.
E) A covalent bond has a lower potential energy than the two separate atoms.

Question 15

Identify the compound with covalent bonding.

A) NaCl
B) KCl
C) H₂O
D) CaO
E) SrBr₂

Question 16

Use Lewis theory to determine the chemical formula for the compound formed between Mg and Br.

A) MgBr
B) Mg₂Br₃
C) Mg₃Br₂
D) MgBr₂
E) Mg₂Br

Question 17

Identify the substance that conducts electricity.

A) NaCl dissolved in water
B) solid NaCl
C) water
D) solid sugar
E) sugar dissolved in water

Question 18

Identify the compound with covalent bonding.

A) Li₂S
B) SrO
C) CaI₂
D) C₂Cl₄
E) SrBr₂

Question 19

Identify the compound with ionic bonding.

A) SrBr₂
B) CH₃CH₂CH₃
C) CH₄
D) H₂
E) CO₂

Question 20

Which of the following represent the Lewis structure for N?

A)
B)
C)
D)
E)

Question 21

Identify the compound with the highest magnitude of lattice energy.

A) CsF
B) BaO
C) SrO
D) CaO

Question 22

Place the following in order of increasing magnitude of lattice energy. MgO LiI CaS

A) CaS < MgO < LiI
B) LiI < CaS < MgO
C) MgO < CaS < LiI
D) LiI < MgO < CaS
E) MgO < LiI < CaS

Question 23

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 24

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 25

Identify the compound with the lowest magnitude of lattice energy.

A) CsF
B) BaO
C) SrO
D) CaO

Question 26

Choose the compound below that should have the highest melting point according to the ionic bonding model.

A) AlN
B) MgO
C) NaF
D) CaS
E) RbI

Question 27

Choose the compound below that should have the lowest melting point according to the ionic bonding model.

A) LiF
B) NaCl
C) CsI
D) KBr
E) RbI

Question 28

Identify the compound with the lowest magnitude of lattice energy.

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

Question 29

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

Question 30

Identify the compound with the highest magnitude of lattice energy.

A) MgO
B) BaO
C) SrO
D) CaO

Question 31

Which of the following reactions is associated with the lattice energy of RbI (Δ_r)?

A) Rb(s) + I₂(g) → RbI(s)
B) RbI(s) → Rb⁺(g) + I⁻(g)
C) RbI(s) → Rb(s) + I₂(g)
D) RbI(s) → Rb⁺(aq) + I⁻(aq)
E) Rb⁺(g) + I⁻(g) → RbI(s)

Question 32

Choose the compound below that should have the highest melting point according to the ionic bonding model.

A) SrI₂
B) MgF₂
C) CaCl₂
D) SrF₂
E) SrBr₂

Question 33

Place the following in order of decreasing magnitude of lattice energy. KF MgS RbI

A) RbI > KF > MgS
B) RbI > MgS > KF
C) MgS > RbI > KF
D) KF > RbI > MgS
E) MgS > KF > RbI

Question 34

Identify the complete electronic configuration for Br^-.

A) 1s²2s²2p⁶3s²3p⁶4s²4p⁶
B) 1s²2s²2p⁶3s²3p⁶4s²4d¹⁰4p⁶
C) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶
D) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁵
E) 1s²2s^2p63s^2p64s²3d¹⁰4p⁶

Question 35

Which of the following reactions is associated with the lattice energy of Li₂O (Δ_r)?

A) Li₂O(s) → 2Li⁺(g) + O²⁻(g)
B) 2Li⁺(aq) + O²⁻(aq) → Li₂O(s)
C) 2Li⁺(g) + O²⁻(g) → Li₂O(s)
D) Li₂O(s) → 2Li⁺(aq) + O²⁻(aq)
E) 2Li(s) + O₂(g) → Li₂O(s)

Question 36

Identify the compound with the lowest magnitude of lattice energy.

A) BaO
B) MgO
C) SrO
D) CaO

Question 37

Identify the compound with the highest magnitude of lattice energy.

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

Question 38

Which of the following reactions is associated with the lattice energy of CaS (Δ_r)?

A) Ca(s) + S(s) → CaS(s)
B) CaS(s) → Ca(s) + S(s)
C) Ca²⁺(aq) + S²⁻(aq) → CaS(s)
D) Ca²⁺(g) + S²⁻(g) → CaS(s)
E) CaS(s) → Ca²⁺(aq) + S²⁻(aq)

Question 39

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

A) KI₂
B) K₂I
C) KI
D) K₂I₂

Question 40

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 41

Use the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO. ΔH°(kJ mol^-1)
Ca(s) → Ca(g) 193
Ca(g) → Ca⁺(g) + e⁻ 590
Ca⁺(g) → Ca²⁺(g) + e⁻ 1010
2O(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 mol^-1
B) +1397 kJ mol^-1
C) -2667 kJ mol^-1
D) +3028 kJ mol^-1
E) -2144 kJ mol^-1

Question 42

Choose the best Lewis structure for NO₃⁻.

A)
B)
C)
D)
E)

Question 43

Identify the longest bond.

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

Question 44

Choose the best Lewis structure for CH₂Cl₂.

A)
B)
C)
D)
E)

Question 45

A double covalent bond contains ________ of electrons.

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

Question 46

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

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 47

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

A) 426 kJ mol^-1
B) 249 kJ mol^-1
C) 852 kJ mol^-1
D) 498 kJ mol^-1
E) 356 kJ mol^-1

Question 48

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 49

Choose the bond below that is the strongest.

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

Question 50

Identify the complete electronic configuration for S^2-.

A) 1s²2s²2p⁶3s²4p⁶
B) 1s²2s²2p⁶3s²3p⁶
C) 1s²2s²2p⁶3s²3p⁵
D) 1s²2s²3p⁶4s²5p⁶
E) 1s²2s^2p63s^2p6

Question 51

Use the data given below to construct a Born-Haber cycle to determine the second ionization energy of Ca. ΔH°(kJ mol^-1)
Ca(s) → Ca(g) 193
Ca(g) → Ca⁺(g) + e⁻ 590.
2O(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 mol^-1
B) 1757 kJ mol^-1
C) 1508 kJ mol^-1
D) -3027 kJ mol^-1
E) -1514 kJ mol^-1

Question 52

A single covalent bond contains ________ of electrons.

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

Question 53

Choose the bond below that is the strongest.

A) C-F
B) C=O
C) C-I
D) I-I
E) C≡N

Question 54

Use the data given below to construct a Born-Haber cycle to determine the electron affinity of Br. ΔH°(kJ mol^-1)
K(s) → K(g) 89
K(g) → K⁺(g) + e⁻ 419
Br₂(g) → 2Br(g) 193
K(s) + Br₂(g) → KBr (s) -394
KBr(s) → K⁺(g) + Br⁻(g) 674

A) -885 kJ mol^-1
B) -325 kJ mol^-1
C) +367 kJ mol^-1
D) -464 kJ mol^-1
E) +246 kJ mol^-1

Question 55

Identify the complete electronic configuration for Ca²⁺.

A) 1s²2s²2p⁶3s²4p⁶
B) 1s²2s²2p⁶3s²3p⁶
C) 1s²2s²2p⁶3s²3p⁵
D) 1s²2s²3p⁶4s²5p⁶
E) 1s²2s^2p63s^2p6

Question 56

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 57

A triple covalent bond contains ________ of electrons.

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

Question 58

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 59

Choose the best Lewis structure for NH₄⁺.

A)
B)
C)
D)
E)

Question 60

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 61

Place the following in order of increasing bond length. C-F C-S C-Cl

A) C-S < C-Cl < C-F
B) C-Cl < C-F < C-S
C) C-F < C-S < C-Cl
D) C-F < C-Cl < C-S
E) C-S < C-F < C-Cl

Question 62

Place the following elements in order of decreasing electronegativity. S Cl Se

A) Se > S > Cl
B) Cl > Se > S
C) Se > Cl > S
D) S > Cl > Se
E) Cl > S > Se

Question 63

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 64

Which compound has the highest carbon-carbon bond strength?

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

Question 65

Use the bond energies provided to estimate ?_rH° for the reaction below. XeF₂ +2F₂ ? XeF₆ ?_rH°= ?
Bond Bond Energy (kJ mol^-1)
Xe-F 147
F-F 159

A) -429 kJ mol^-1
B) +159 kJ mol^-1
C) -660 kJ mol^-1
D) +176 kJ mol^-1
E) -270 kJ mol^-1

Question 66

Choose the bond below that is the weakest.

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

Question 67

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 68

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

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 69

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

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

Question 70

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 71

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 72

Which of the following processes is exothermic?

A) the second ionization energy of Mg
B) the sublimation of Li
C) the breaking of the bond of I₂
D) the formation of NaBr from its constituent elements in their standard state
E) None of the above processes is exothermic

Question 73

Which of the following processes is endothermic?

A) K⁺(g) + I⁻(g) → KI(s)
B) 2Br(g) → Br₂(g)
C) Ca(s) → Ca(g)
D) 2Na(s) + O₂(g) → Na₂O(s)
E) None of the above processes is endothermic.

Question 74

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

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 75

Which of the following 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 76

Choose the bond below that is the weakest.

A) C≡O
B) N≡N
C) C-I
D) C=S
E) K-Cl

Question 77

Which of the following 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 78

Use the bond energies provided to estimate Δ_rH° for the reaction below. CH₃OH(l) + 2O₂(g) → CO₂(g) + 2H₂O(g) Δ_rH° = ?
Bond Bond Energy (kJ mol^-1)
C-H 414
C-O 360
C=O 799
O=O 498
O-H 464

A) +473 kJ mol^-1
B) -91 kJ mol^-1
C) -486 kJ mol^-1
D) -392 kJ mol^-1
E) +206 kJ mol^-1

Question 79

Which compound has the longest carbon-carbon bond length?

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

Question 80

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

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