Deck 9: Chemical Bonding I: Lewis Theory

Question 1

Identify the compound with covalent bonding.

A)NaCl
B)Li
C)H₂O
D)He
E)S

Answer 1

H₂O

Question 2

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.

Answer 2

A covalent bond has a lower potential energy than the two separate atoms.

Question 3

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

Answer 3

Al₂O₃

Question 4

Which of the following represent the Lewis structure for Cl?

A)
B)
C)
D)
E)

Question 5

Identify the compound with ionic bonding.

A)NaCl
B)Li
C)H₂O
D)He
E)S

Question 6

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

A)
B)
C)
D)
E)

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

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 9

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

Question 10

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

Question 11

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 12

Which of the following represent the Lewis structure for Mg?

A)
B)
C)
D)
E)

Question 13

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

A)
B)
C)
D)
E)

Question 14

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 15

Which of the following represent the Lewis structure for N?

A)
B)
C)
D)
E)

Question 16

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

A)
B)
C)
D)
E)

Question 17

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 18

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 19

Identify the compound with metallic bonding.

A)NaCl
B)Li
C)H₂O
D)He
E)S

Question 20

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 21

Which of the following reactions is associated with the lattice energy of RbI (Δ_{r NEWLINE} )?

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 22

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

Question 23

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

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

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 26

Identify the complete electronic configuration for S^2-.

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

Question 27

A single covalent bond contains ________ of electrons.

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

Question 28

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(l)→ 2Br(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 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 complete electronic configuration for Br^-.

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

Question 31

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 32

Identify the compound with the lowest magnitude of lattice energy.

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

Question 33

Identify the complete electronic configuration for Ca²⁺.

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

Question 34

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

Question 35

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 36

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 37

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

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

Question 38

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 39

Identify the compound with the highest magnitude of lattice energy.

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

Question 40

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 41

Which compound has the highest carbon-carbon bond strength?

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

Question 42

Which compound has the longest carbon-carbon bond length?

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

Question 43

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 44

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 45

Choose the best Lewis structure for NO₃⁻.

A)
B)
C)
D)
E)

Question 46

A triple covalent bond contains ________ of electrons.

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

Question 47

Choose the best Lewis structure for CH₂Cl₂.

A)
B)
C)
D)
E)

Question 48

Choose the best Lewis structure for NH₄⁺.

A)
B)
C)
D)
E)

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 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 51

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 52

Choose the bond below that is the strongest.

A)C-F
B)C=O
C)C-I
D)I-I
E)C≡N

Question 53

Choose the bond below that is the weakest.

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

Question 54

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 55

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 56

A double covalent bond contains ________ of electrons.

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

Question 57

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 58

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 59

Choose the bond below that is the weakest.

A)C≡O
B)N≡N
C)C-I
D)C=S
E)K-Cl

Question 60

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 61

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 62

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 63

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 64

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 65

List the following compounds in decreasing electronegativity difference. Cl₂ HCl NaCl

A)NaCl > Cl₂ > HCl
B)Cl₂ > HCl > NaCl
C)HCl > NaCl > Cl₂
D)NaCl > HCl > Cl₂

Question 66

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 67

Using periodic trends, place the following bonds in order of decreasing ionic character. Sb-Cl P-Cl As-Cl

A)Sb-Cl > As-Cl > P-Cl
B)As-Cl > Sb-Cl > P-Cl
C)P-Cl > Sb-Cl > As-Cl
D)P-Cl > As-Cl > Sb-Cl
E)Sb-Cl > P-Cl > As-Cl

Question 68

Choose the bond below that is least polar.

A)P-F
B)C-Br
C)C-F
D)C-I
E)C-Cl

Question 69

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 70

Using periodic trends, place the following bonds in order of increasing ionic character. S-F Se-F O-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 71

Use the bond energies provided to estimate Δ_rH° for the reaction below. XeF_{2 +} 2F₂ → XeF₆ Δ_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 72

Choose the bond below that is most polar.

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

Question 73

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 74

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 75

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 76

Choose the bond below that is most polar.

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

Question 77

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

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 78

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

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

Question 79

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 80

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.