Covalent Bonding Chemistry Worksheet With Answers Page 2
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6CHAPTER
8
CHAPTER
8
Assessment
Assessment
Reviewing Content
8.1 Molecular Compounds
51.
Explain what is meant by bond dissociation
energy.
The melting point of a compound is 1240°C. Is
39.
39. ionic
this compound most likely an ionic or a molecu-
What is the relationship between the magnitude
52.
40. a. 6 C, 8 H, 6 O b. 12 C, 22 H, 11 O
lar compound?
of a molecule’s bond dissociation energy and its
expected chemical reactivity?
c. 7 C, 5 H, 3 N, 6 O
Identify the number and kinds of atoms present
40.
in a molecule of each compound.
41. Nitrogen and oxygen achieve sta-
8.3 Bonding Theories
a.
ascorbic acid (vitamin C), C
H
O
6
8
6
bility as diatomic molecules. Argon
What is a pi bond? Describe, with the aid of a
53.
sucrose (table sugar), C
H
O
b.
12
22
11
diagram, how the overlap of two half-filled p
exists as individual atoms because
trinitrotoluene (TNT), C
H
N
O
c.
7
5
3
6
atomic orbitals produces a pi bond.
it has a stable noble-gas electron
Which of the following gases in Earth’s atmo-
41.
54.
Use VSEPR theory to predict the shapes of the
configuration.
sphere would you expect to find as molecules
following species.
42. Neon has an octet of electrons. A
and which as individual atoms? Explain.
CO
SiCl
SO
a.
b.
c.
2
4
3
nitrogen
oxygen
argon
a.
b.
c.
chlorine atom achieves an octet by
SCl
CO
H
Se
d.
e.
f.
2
2
sharing an electron with another
8.2 The Nature of Covalent Bonding
The molecule CO
has two carbon–oxygen dou-
55.
2
ble bonds. Describe the bonding in the CO
chlorine atom.
42.
Explain why neon is monatomic but chlorine is
2
molecule, which involves hybridized orbitals for
diatomic.
43. a. ionic b. ionic
c. covalent
carbon and oxygen.
Classify the following compounds as ionic or
43.
d. covalent
What types of hybrid orbitals are involved in the
56.
covalent.
44. Ionic bonds depend on electro-
bonding of the carbon atoms in the following
MgCl
Na
S
H
O
H
S
a.
b.
c.
d.
2
2
2
2
static attraction between ions.
molecules?
Describe the difference between an ionic and a
44.
CH
Covalent bonds depend on elec-
a.
b.
H
C “ CH
covalent bond.
4
2
2
HC { CH
c.
d.
N { C ¬ C { N
trostatic attraction between
45.
How many electrons do two atoms in a double
8.4 Polar Bonds and Molecules
shared electrons and nuclei of
covalent bond share? How many in a triple cova-
lent bond?
How must the electronegativies of two atoms
combining atoms.
57.
compare if a covalent bond between them is to
Write plausible electron dot structures for the
46.
45. A double covalent bond has four
be polar?
following substances. Each substance contains
shared electrons (two bonding pairs);
only single covalent bonds.
The bonds between the following pairs of ele-
58.
a triple covalent bond has six shared
I
OF
H
S
NI
a.
b.
c.
d.
ments are covalent. Arrange them according to
2
2
2
3
electrons (three bonding pairs).
polarity, naming the most polar bond first.
Characterize a coordinate covalent bond and
47.
I
N
I
H⎯Cl
H⎯C
H⎯F
a.
b.
c.
give an example.
46. a.
I I
b.
O
c.
d.
F
F
S
H
H
I
H⎯O
H⎯H
S⎯Cl
d.
e.
f.
Explain why compounds containing C⎯N and
48.
47. One atom contributes both elec-
59.
What is a hydrogen bond?
C⎯O single bonds can form coordinate covalent
trons to a coordinate covalent
bonds with H but compounds containing only
Depict the hydrogen bonding between two
60.
bond, as in CO.
C⎯H and C⎯C single bonds cannot.
ammonia molecules and between one ammonia
molecule and one water molecule.
48. An unshared pair of electrons is
Using electron dot structures, draw at least
49.
needed for a coordinate covalent
two resonance structures for the nitrite ion
61.
Why do compounds with strong intermolecular
(NO
). The oxygens in NO
are attached to the
attractive forces have higher boiling points than
bond. There are no unshared pairs
2
2
nitrogen.
compounds with weak intermolecular attractive
in compounds with only C-H and
forces?
Which of these compounds contain elements
50.
C-C bonds.
that do not follow the octet rule? Explain.
↔ O
49.
NF
PCl
F
SF
SCl
O
N
O
N
O
a.
b.
c.
d.
3
2
3
4
2
50. b and c; assuming only single
bonds, the P and S atoms each
have 10 valence electrons.
Assessment
247
51. Bond dissociation energy is
defined as the energy needed to
break one covalent bond.
54. a. linear
b. tetrahedral c. trigonal
59. A hydrogen bond is formed by an electro-
52. Increasing bond dissociation
planar
d. bent e. linear
f. bent
static interaction between a hydrogen
energy is linked to lower chemical
55. The 2s and the 2p orbitals form two sp
atom that is covalently bonded to an elec-
reactivity.
hybrid orbitals on the carbon atom.
tronegative atom, and an unshared elec-
53. A pi bond is formed by the side-by
One sp hybrid orbital forms a sigma bond
tron pair of a nearby atom.
side overlap of two half-filled p
between the carbon atom and each oxy-
60.
atomic orbitals to produce a pi
H
H
gen atom. Pi bonds between each oxygen
molecular orbital. In a pi bond, the
H
N
H
N
H
H
atom and the carbon are formed by the
bonding electrons are most likely
H
H
unhybridized 2p orbitals.
to be found in sausage-shaped
O
H
N
3
2
56. a. sp
b. sp
c. sp d. sp
regions above and below the bond
H
H
57. The electronegativities of the two atoms
axis of the bonded atoms. See Fig-
61. More energy is required to separate the
will differ by about 0.4 to 2.0.
ure 8.15.
molecules.
58. c, d, a, f, b, e
Covalent Bonding
247
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