Deck 9: Chemical Bonding I: Lewis Theory

Question 1

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

A)
B)
C)
D)
E)

Answer 1

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

Which of the following reactions is associated with the lattice energy of RbI (ΔH°_latt)?

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)

Answer 3

Rb⁺(g)+ I^⁻(g)→ RbI(s)

Question 4

Which of the following reactions is associated with the lattice energy of CaS (ΔH°_latt)?

A)Ca(s)+ S(s)→ CaS(s)
B)CaS(s)→ Ca(s)+ S(s)
C)Ca²⁺(aq)+ S^2⁻(aq)→ CaS(s)
D)Ca²⁺(g)+ S^2⁻(g)→ CaS(s)
E)CaS(s)→ Ca²⁺(aq)+ S²⁻(aq)

Question 5

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

A)
B)
C)
D)
E)

Question 6

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 7

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 8

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 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

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

A)
B)
C)
D)
E)

Question 11

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 12

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 13

Which of the following represent the Lewis structure for Mg?

A)
B)
C)
D)
E)

Question 14

Which of the following reactions is associated with the lattice energy of Li₂O (ΔH°_latt)?

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

Question 15

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 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

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

A)Mg₃N₂
B)Mg₂N₃
C)MgN₂
D)MgN

Question 18

Which of the following represent the Lewis structure for N?

A)
B)
C)
D)
E)

Question 19

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 20

Which of the following represent the Lewis structure for Cl?

A)
B)
C)
D)
E)

Question 21

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 22

In the Lewis structure of CH₃OH,how many bonding pairs of electrons are there?

A)2
B)7
C)5
D)3

Question 23

Which molecule or compound below contains a pure covalent bond?

A)Li₂CO₃
B)SCl₆
C)Cl₂
D)PF₃
E)NaCl

Question 24

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 25

Choose the bond below that is most polar.

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

Question 26

Choose the bond below that is least polar.

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

Question 27

Identify the most electronegative element.

A)Fr
B)At
C)H
D)F

Question 28

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 29

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 30

In the Lewis structure of CH₃OH,how many lone pairs of electrons are there?

A)5
B)7
C)3
D)2

Question 31

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 are true.

Question 32

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 33

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)Sb-Cl > P-Cl > As-Cl
D)P-Cl > As-Cl > Sb-Cl
E)P-Cl > Sb-Cl > As-Cl

Question 34

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 35

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 36

Choose the bond below that is most polar.

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

Question 37

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 38

Which molecule or compound below contains a polar covalent bond?

A)C₂H₄
B)ZnS
C)LiI
D)NCl₃
E)AgCl

Question 39

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 40

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 41

Choose the best Lewis structure for XeI₂.

A)
B)
C)
D)
E)

Question 42

Give the number of valence electrons for SF₄.

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

Question 43

Choose the best Lewis structure for BF₃.

A)
B)
C)
D)
E)

Question 44

Choose the best Lewis structure for NO₃⁻.

A)
B)
C)
D)
E)

Question 45

Which molecule or compound below contains an ionic bond?

A)CO₂
B)C₂Cl₄
C)SiF₄
D)OCl₂
E)NH₄NO₃

Question 46

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

Question 47

Choose the best Lewis structure for BeF₂.

A)
B)
C)
D)
E)

Question 48

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 49

Choose the best Lewis structure for SO₄²⁻.

A)
B)
C)
D)
E)

Question 50

Choose the best Lewis structure for ICl₅.

A)
B)
C)
D)
E)

Question 51

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

A)O(2 lone pairs)=C=N (2 lone pairs)
B)O(1 lone pair)≡C-N(3 lone pairs)
C)O(1 lone pair)=C(2 lp)=N(1 lone pair)
D)O(3 lone pairs)-C≡N(with 1 lone pair)
E)They all contribute equally to the correct structure of OCN⁻.

Question 52

Choose the best Lewis structure for SeO₄²⁻.

A)
B)
C)
D)
E)

Question 53

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 54

Draw the Lewis structure for NO₂⁻ including any valid resonance structures.Which of the following statements is true?

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 1.5 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 are true.

Question 55

Choose the best Lewis structure for OCl₂.

A)
B)
C)
D)
E)

Question 56

Choose the best Lewis structure for PO₄³⁻.

A)
B)
C)
D)
E)

Question 57

Choose the best Lewis structure for CH₂Cl₂.

A)
B)
C)
D)
E)

Question 58

Choose the best Lewis structure for NH₄⁺.

A)
B)
C)
D)
E)

Question 59

Give the number of valence electrons for XeI₂.

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

Question 60

Choose the best Lewis structure for SF₄.

A)
B)
C)
D)
E)

Question 61

Choose the bond below that is the weakest.

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

Question 62

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 are endothermic.

Question 63

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

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

Question 64

Draw the best Lewis structure for CH₃^-.What is the formal charge on the C?

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

Question 65

Choose the bond below that is the weakest.

A)C≡O
B)N≡N
C)C-I
D)C=S
E)K-Cl

Question 66

Which of the following processes are 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 are exothermic.

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

How many of the following elements can form compounds with an expanded octet?
Pb Kr Si B

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

Question 69

Which of the following processes is exothermic?

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

Question 70

Choose the bond below that is the strongest.

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

Question 71

Which of the following elements can form compounds with an expanded octet?

A)Se
B)C
C)Li
D)F
E)All of the above elements can form compounds with an expanded octet.

Question 72

Draw the best Lewis structure for the free radical,NO₂.What is the formal charge on the N?

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

Question 73

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 74

Choose the bond below that is the strongest.

A)C-F
B)C=O
C)C-I
D)I-I
E)C≡N

Question 75

How many of the following elements can form compounds with an expanded octet?
I O Cl Xe

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

Question 76

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

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

Question 77

Which of the following processes is endothermic?

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

Question 78

Which of the following elements can form compounds with an expanded octet?

A)N
B)Br
C)F
D)Be
E)None of the above can form compounds with an expanded octet.

Question 79

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 80

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