Chapter 09 – Chemical Bonding I: Basic Concepts
40. Arrange the following bonds in order of increasing ionic character:
B — C
C — N
C — O
C — C
41. Arrange the following bonds in order of increasing ionic character:
C — F
O — F
H — F
Na — F
Chapter 09 – Chemical Bonding I: Basic Concepts
42. Arrange the following bonds in order of increasing ionic character:
H — Cl
C — H
H — H
O — H
43. Classify the O — H bond in CH3OH as ionic, polar covalent, or nonpolar covalent.
Chapter 09 – Chemical Bonding I: Basic Concepts
44. Classify the C — Cl bond in CCl4 as ionic, polar covalent, or nonpolar covalent.
45. Classify the Ca — Cl bond in CaCl2 as ionic, polar covalent, or nonpolar covalent.
Chapter 09 – Chemical Bonding I: Basic Concepts
46. List all types of bonding present in the compound CaCO3.
I. ionic bond
II. polar covalent bond
III. nonpolar covalent bond
47. List all types of bonding present in the compound NH4NO3.
I. ionic bond
II. polar covalent bond
III. nonpolar covalent bond
Chapter 09 – Chemical Bonding I: Basic Concepts
48. List all types of bonding present in the molecule SO3.
I. ionic bond
II. polar covalent bond
III. nonpolar covalent bond
49. List all types of bonding present in the ion SO42-.
I. ionic bond
II. polar covalent bond
III. nonpolar covalent bond
Chapter 09 – Chemical Bonding I: Basic Concepts
50. List all types of bonding present in the molecule S8.
I. ionic bond
II. polar covalent bond
III. nonpolar covalent bond
51. The total number of valence electrons in the molecule CO2 is
Chapter 09 – Chemical Bonding I: Basic Concepts
52. The total number of valence electrons in the molecule P2O5 is
53. The total number of valence electrons in the compound NH4NO3 is
54. The total number of valence electrons in the ion NH4+ is
Chapter 09 – Chemical Bonding I: Basic Concepts
55. The total number of valence electrons in the ion SO42- is
56. The electron dot formula for O2 shows
57. The number of lone electron pairs in the N2 molecule is ___.
Chapter 09 – Chemical Bonding I: Basic Concepts
58. The Lewis structure reveals a double bond in which of the following molecules?
59. The Lewis structure reveals a triple bond in which of the following molecules?
Chapter 09 – Chemical Bonding I: Basic Concepts
60. The Lewis structure reveals only single bonds in which of the following species?
61. The Lewis structure reveals an unpaired electron (free radical) in which of the following
species?
Chapter 09 – Chemical Bonding I: Basic Concepts
63. The number of lone electron pairs in the ClO4– ion is ___.
Chapter 09 – Chemical Bonding I: Basic Concepts
64. The total number of bonding electrons in a molecule of formaldehyde (H2CO) is
65. The total number of lone pairs in NCl3 is
Chapter 09 – Chemical Bonding I: Basic Concepts
66.
The Lewis structure for CS2 is:
Chapter 09 – Chemical Bonding I: Basic Concepts
67. Which of the following Lewis structures is incorrect?
Chapter 09 – Chemical Bonding I: Basic Concepts
68. The number of resonance structures for the sulfur dioxide molecule that satisfy the octet
rule is
69. The number of resonance structures for the nitrate ion that satisfy the octet rule is
Chapter 09 – Chemical Bonding I: Basic Concepts
70. The azide ion, N3–, is very reactive although it is isoelectronic with the very stable CO2
molecule. This reactivity is reasonable considering that
71. Assuming the octet rule is obeyed, how many covalent bonds will a nitrogen atom form to
give a formal charge of zero?
Chapter 09 – Chemical Bonding I: Basic Concepts
72. Assuming the octet rule is obeyed, how many covalent bonds will an oxygen atom form to
give a formal charge of zero?
73. Assuming the octet rule is obeyed, how many covalent bonds will a carbon atom form to
Chapter 09 – Chemical Bonding I: Basic Concepts
74. Assuming the octet rule is obeyed, how many covalent bonds will a neon atom form to
give a formal charge of zero?
75. Which of the following is a useful guideline for the application of formal charges in
neutral molecules?
Chapter 09 – Chemical Bonding I: Basic Concepts
76. What is the formal charge on the oxygen atom in N2O (the atomic order is N–N–O)?
77. The formal charge on the bromine atom in BrO3– drawn with three single bonds is
Chapter 09 – Chemical Bonding I: Basic Concepts
78. 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)?
79. How many covalent bonds will be drawn to phosphorous in PO43– 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)?