Deck 9: Chemical Bonding I: Basic Concepts

Question 1

The Lewis dot symbol for the calcium ion is

A) $\text{: Ca :}^{2+}$
B) -Ca-
C)
D) Ca²⁺
E) Ca

Answer 1

Ca²⁺

Question 2

Which one of the following is most likely to be a covalent compound

A) Rb₂O
B) BaO
C) SrO
D) SeO₂
E) MnO₂

Answer 2

SeO₂

Question 3

Which one of the following compounds utilizes both ionic and covalent bonding

A) Na₂SO₄
B) AlCl₃
C) PO₄^3-
D) NH₄⁺
E) CaO

Answer 3

Na₂SO₄

Question 4

Complete this statement: Coulomb's law states that the magnitude of the $\underline{\text{force of interaction}}$ between two charged bodies is

A) directly proportional to the product of the charges on the bodies and directly proportional to the distance separating them.
B) directly proportional to the product of the charges on the bodies, and inversely proportional to the square of the distance separating them.
C) inversely proportional to the product of the charges on the bodies, and directly proportional to the square of the distance separating them.
D) directly proportional to the sum of the charges on the bodies, and inversely proportional to the square of the distance separating them.

Question 5

Calculate the energy change for the reaction K(g) + Br(g) $\rarr$ K⁺(g) + Br^- (g)
Given the following ionization energy (IE) and electron affinity (EA) values. $\begin{array}{cc}\text { IE } & \text { EA } \\\text { K: }: 419 \mathrm{~kJ} / \mathrm{mol} & 48 \mathrm{~kJ} / \mathrm{mol} \\\mathrm{Br}: 1140 \mathrm{~kJ} / \mathrm{mol} & 324 \mathrm{~kJ} / \mathrm{mol}\end{array}$

A) -1,092 kJ/mol
B) -95 kJ/mol
C) 95 kJ/mol
D) 1,092 kJ/mol
E) 1,187 kJ/mol

Question 6

Which of the following solids would have the highest melting point

A) NaF
B) NaCl
C) NaBr
D) NaI

Question 7

Which one of the following is most likely to be a covalent compound

A) KF
B) CaCl₂
C) SF₄
D) Al₂O₃
E) CaSO₄

Question 8

The Lewis dot symbol for the chloride ion is

A)
B)
C) $\text{: Cl}^-$
D)
E) Cl^-

Question 9

Which of the following solids would have the lowest melting point

A) KI
B) KBr
C) KCl
D) KF

Question 10

The Lewis dot symbol for the S ^2- ion is

A)
B)
C) S^2-
D)
E)

Question 11

Which one of the following is most likely to be an ionic compound

A) ClF₃
B) FeCl₃
C) NH₃
D) PF₃
E) SO₃

Question 12

Which one of the following compounds utilizes both ionic and covalent bonding

A) C₁₀H₂₂O
B) NH₃
C) Na₂S
D) NH₄NO₃
E) K₃N

Question 13

Which one of the following is most likely to be a covalent compound

A) CsOH
B) NF₃
C) Sr(NO₃)₂
D) CaO
E) LiF

Question 14

Which of the following solids would have the highest melting point

A) NaI
B) NaF
C) MgO
D) MgCl₂
E) KF

Question 15

Which one of the following compounds utilizes both ionic and covalent bonding

A) CO₃^2-
B) Al₂(SO₄)₃
C) CO₂
D) C₆H₁₂O₆
E) MgCl₂

Question 16

Which one of the following is most likely to be an ionic compound

A) NCl₃
B) BaCl₂
C) CO
D) SO₂
E) SF₄

Question 17

Which of the following ionic solids would have the largest lattice energy

A) KF
B) KI
C) LiF
D) LiI
E) NaF

Question 18

Which of the following ionic solids would have the largest lattice energy

A) SrO
B) NaF
C) CaBr₂
D) CsI
E) BaSO₄

Question 19

Which one of the following is most likely to be an ionic compound

A) CaCl₂
B) CO₂
C) CS₂
D) SO₂
E) OF₂

Question 20

Which one of the following ionic solids would have the largest lattice energy

A) NaCl
B) NaF
C) CaBr₂
D) CsI
E) CaCl₂

Question 21

Which of the elements listed below would most likely form an ionic bond when bonded to oxygen

A) Cl
B) C
C) O
D) H
E) Ca

Question 22

Which of the bonds below would have the greatest polarity (i.e., highest percent ionic character)

A) Si - P
B) Si - S
C) Si - Se
D) Si - Cl
E) Si - I

Question 23

Calculate the energy change for the reaction K(g) + I(g) $\rarr$ K⁺(g) + I ^- (g)
Given the following ionization energy (IE) and electron affinity (EA) values. $\begin{array}{cc}\text { IE } & \text { EA } \\\text { K: } 419 \mathrm{~kJ} / \mathrm{mol} & 48 \mathrm{~kJ} / \mathrm{mol} \\\text { I: } 1,010 \mathrm{~kJ} / \mathrm{mol} & 295 \mathrm{~kJ} / \mathrm{mol}\end{array}$

A) -124 kJ/mol
B) -715 kJ/mol
C) 715 kJ/mol
D) 1429 kJ/mol
E) None of these

Question 24

Use the Born-Haber cycle to calculate the lattice energy of MgO (s) given the following data: $\Delta$ H(sublimation) Mg = 130 kJ/mol
I₁ (Mg) = 738.1 kJ/mol
I₂ (Mg) = 1450 kJ/mol
Bond energy (O=O) = 498.7 kJ/mol
EA (O) = 141 kJ/mol
EA (O^-) = -780 kJ/mol
$\Delta{H}^{\circ}_f$ (MgO(s)) = -601.8 kJ/mol

A) 2200 kJ/mol
B) 2800 kJ/mol
C) 3200 kJ/mol
D) 3800 kJ/mol
E) 4100 kJ/mol

Question 25

Use the Born-Haber cycle to calculate the standard enthalpy of formation ( $\Delta{H}^{\circ}_f$ ) for LiCl(s) given the following data: $\Delta$ H(sublimation) Li = 155.2 kJ/mol
I₁ (Li) = 520 kJ/mol
Bond energy (Cl-Cl) = 242.7 kJ/mol
EA (Cl) = 349 kJ/mol
Lattice energy (LiCl(s)) = 828 kJ/mol

A) 440 kJ/mol
B) 320 kJ/mol
C) -260 kJ/mol
D) -380 kJ/mol
E) -1420 kJ/mol

Question 26

The covalent bond with the greatest polarity would form in which of the atom pairs below

A) Br - Br
B) S - O
C) C - P
D) C - O
E) B - O

Question 27

Arrange the elements Ba, Br, and Ga in order of increasing electronegativity.

A) Ba < Br < Ga
B) Br < Ga < Ba
C) Ba < Ga < Br
D) Ga < Ba < Br
E) Ga < Br < Ba

Question 28

Which of the elements listed below would most likely form a polar covalent bond when bonded to oxygen

A) Mg
B) H
C) Al
D) O
E) Na

Question 29

A polar covalent bond would form in which one of the following pairs of atoms

A) Cl - Cl
B) Si - Si
C) Ca - Cl
D) Cr - Br
E) P - Cl

Question 30

What type of chemical bond holds the atoms together within a water molecule

A) Ionic bond
B) Nonpolar covalent bond
C) Polar covalent bond
D) Coordinate covalent bond

Question 31

Which of the elements listed below would most likely form a nonpolar covalent bond when bonded to bromine

A) Rb
B) Br
C) C
D) O
E) H

Question 32

A nonpolar covalent bond (i.e., pure covalent) would form in which one of the following pairs of atoms

A) Na - Cl
B) H - Cl
C) Li - Br
D) Se - Br
E) Br - Br

Question 33

Arrange the following bonds in order of increasing ionic character:
$B - C$
$C - N$
$C - O$
$C - C$

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

Question 34

Which one of these polar covalent bonds would have the greatest percent ionic character

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

Question 35

Define electronegativity:

A) an atoms ability to attract electrons that are shared in a chemical bond
B) an atoms ability to form an ionic bond with another atom
C) an atoms ability to donate valence electrons to another atom
D) an atoms ability to form a cation
E) an atoms ability to form double and triple bonds

Question 36

Arrange the elements F, P, and Cl in order of increasing electronegativity.

A) F < P < Cl
B) P < Cl < F
C) Cl < P < F
D) P < F < Cl
E) Cl < F < P

Question 37

Arrange the elements C, O, and H in order of increasing electronegativity.

A) C < O < H
B) H < C < O
C) C < H < O
D) O < C < H
E) H < O < C

Question 38

Which of the elements listed below would most likely form an ionic bond when bonded to chlorine

A) H
B) Br
C) O
D) Sr
E) N

Question 39

Use the Born-Haber cycle to calculate the lattice energy of KCl(s) given the following data: $\Delta$ H(sublimation) K = 79.2 kJ/mol
I₁ (K) = 418.7 kJ/mol
Bond energy (Cl-Cl) = 242.8 kJ/mol
EA (Cl) = 348 kJ/mol
$\Delta{H}^{\circ}_f$ (KCl(s)) = -435.7 kJ/mol

A) -165 kJ/mol
B) 288 kJ/mol
C) 629 kJ/mol
D) 707 kJ/mol
E) 828 kJ/mol

Question 40

Which of the following covalent bonds is the most polar (i.e., highest percent ionic character)

A) Al - I
B) Si - I
C) Al - Cl
D) Si - Cl
E) Si - P

Question 41

Classify the C - Cl bond in CCl₄ as ionic, polar covalent, or nonpolar covalent.

A) ionic
B) polar covalent
C) nonpolar covalent

Question 42

The electron dot formula for O₂ shows

A) a single covalent bond.
B) a double covalent bond.
C) an ionic bond.
D) a total of 8 x 2 = 16 electron dots.
E) a total of 32 electron dots.

Question 43

Classify the O - H bond in CH₃OH as ionic, polar covalent, or nonpolar covalent.

A) ionic
B) polar covalent
C) nonpolar covalent

Question 44

The Lewis structure reveals a triple bond in which of the following molecules

A) Br₂
B) O₂
C) N₂
D) H₂
E) CH₄

Question 45

The total number of valence electrons in the molecule P₂O₅ is

A) 11.
B) 22.
C) 23.
D) 40.
E) 70.

Question 46

Arrange the following bonds in order of increasing ionic character:
C - F
O - F
H - F

Na - F

A) C - F < O - F < H - F < Na - F
B) C - F < H - F < O - F < Na - F
C) O - F < C - F < H - F < Na - F
D) H - F < C - F < O - F < Na - F
E) Na - F < H - F < C - F < O - F

Question 47

Classify the Ca - Cl bond in CaCl₂ as ionic, polar covalent, or nonpolar covalent.

A) ionic
B) polar covalent
C) nonpolar covalent

Question 48

Arrange the following bonds in order of increasing ionic character:
H - Cl
C - H
H - H
O - H

A) H - Cl < C - H < H - H < O - H
B) H - H < C - H < O - H < H - Cl
C) H - H < C - H < H - Cl < O - H
D) C - H < O - H < H - Cl < H - H
E) C - H < H - Cl < O - H < H - H

Question 49

The number of lone electron pairs in the N₂ molecule is ___.

A) 1
B) 2
C) 3
D) 4
E) 5

Question 50

The total number of valence electrons in the compound NH₄NO₃ is

A) 28.
B) 30.
C) 32.
D) 42.
E) 80.

Question 51

The total number of valence electrons in the ion SO₄^2- is

A) 24.
B) 26.
C) 28.
D) 30.
E) 32.

Question 52

List all types of bonding present in the ion SO₄^2-.
I. ionic bond
II. polar covalent bond
III. nonpolar covalent bond

A) I only
B) II only
C) III only
D) I and II
E) II and III

Question 53

List all types of bonding present in the molecule S₈.
I. ionic bond
II. polar covalent bond
III. nonpolar covalent bond

A) I only
B) II only
C) III only
D) I and II
E) II and III

Question 54

List all types of bonding present in the compound CaCO₃.
I. ionic bond
II. polar covalent bond
III. nonpolar covalent bond

A) I only
B) II only
C) III only
D) I and II
E) II and III

Question 55

List all types of bonding present in the molecule SO₃.
I. ionic bond
II. polar covalent bond
III. nonpolar covalent bond

A) I only
B) II only
C) III only
D) I and II
E) II and III

Question 56

The Lewis structure reveals only single bonds in which of the following species

A) CO₂
B) CO
C) CO₃^2-
D) Cl₂CO
E) CCl₄

Question 57

The total number of valence electrons in the molecule CO₂ is

A) 4.
B) 10.
C) 14.
D) 16.
E) 20.

Question 58

The Lewis structure reveals a double bond in which of the following molecules

A) Br₂
B) O₂
C) N₂
D) H₂
E) CH₄

Question 59

The total number of valence electrons in the ion NH₄⁺ is

A) 8.
B) 9.
C) 10.
D) 17.
E) 18.

Question 60

List all types of bonding present in the compound NH₄NO₃.
I. ionic bond
II. polar covalent bond
III. nonpolar covalent bond

A) I only
B) II only
C) III only
D) I and II
E) II and III

Question 61

The formal charge on the sulfur atom in the resonance structure of sulfur dioxide which has one single bond and one double bond is

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

Question 62

The Lewis structure reveals an unpaired electron (free radical) in which of the following species

A) NO₃^-
B) N₂O
C) NO₂
D) NO₂^-
E) HNO₃

Question 63

The number of resonance structures for the sulfur dioxide molecule that satisfy the octet rule is

A) 1.
B) 2.
C) 3.
D) 4.
E) None of these.

Question 64

Assuming the octet rule is obeyed, how many covalent bonds will an oxygen atom form to give a formal charge of zero

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

Question 65

How many covalent bonds will be drawn to phosphorous in PO₄^3- for the dot structure that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s)

A) 4
B) 5
C) 6
D) 7
E) 8

Question 66

The Lewis structure for CS₂ is:

A)
B)
C)
D)

Question 67

The azide ion, N₃^-, is very reactive although it is isoelectronic with the very stable CO₂ molecule. This reactivity is reasonable considering that

A) a Lewis structure cannot be written for the azide ion that has nitrogen formal charges of zero.
B) there is no valid Lewis structure possible for the azide ion.
C) there are resonance structures for azide ion but not for carbon dioxide.
D) nitrogen cannot form multiple bonds.
E) charged species always decompose in solution.

Question 68

The formal charge on the bromine atom in BrO₃^- drawn with three single bonds is

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

Question 69

Assuming the octet rule is obeyed, how many covalent bonds will a nitrogen atom form to give a formal charge of zero

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

Question 70

The number of lone electron pairs in the NH₄⁺ ion is ___.

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

Question 71

Which of the following is a useful guideline for the application of formal charges in neutral molecules

A) A Lewis structure in which there are no formal charges is preferred.
B) Lewis structures with large formal charges are preferred.
C) The preferred Lewis structure is one in which positive formal charges are on the most electronegative atoms.

Question 72

Assuming the octet rule is obeyed, how many covalent bonds will a carbon atom form to give a formal charge of zero

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

Question 73

The number of lone electron pairs in the ClO₄^- ion is ___.

A) 3
B) 4
C) 6
D) 12
E) 24

Question 74

How many covalent bonds will be drawn to bromine in BrO₃^- for the dot structure that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s)

A) 3
B) 4
C) 5
D) 6
E) 7

Question 75

What is the formal charge on the oxygen atom in N₂O (the atomic order is N-N-O)

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

Question 76

What is the formal charge on sulfur in the most favorable Lewis structure for the SCN^- (thiocyanate) ion based on minimizing formal charge overall

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

Question 77

The total number of lone pairs in NCl₃ is

A) 6.
B) 8.
C) 9.
D) 10.
E) 13.

Question 78

The total number of bonding electrons in a molecule of formaldehyde (H₂CO) is

A) 3.
B) 4.
C) 6.
D) 8.
E) 18.

Question 79

Assuming the octet rule is obeyed, how many covalent bonds will a neon atom form to give a formal charge of zero

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

Question 80

The number of resonance structures for the nitrate ion that satisfy the octet rule is

A) 1
B) 2
C) 3
D) 4
E) None of these