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Chem I Chapter 8
Matching
Match each item with the correct statement below
...
coordinate covalent bond
d
...
double covalent bond
e
...
structural formula
f
...
a depiction of the arrangement of atoms in molecules and polyatomic ions

____

2
...
a covalent bond in which two pairs of electrons are shared

____

4
...
a covalent bond between two atoms of significantly different electronegativities

____

6
...

a
...
tetrahedral angle
b
...
VSEPR theory
c
...
sigma bond
d
...
energy needed to break a single bond between two covalently bonded atoms

____

8
...
molecular orbital that can be occupied by two electrons of a covalent bond

____ 10
...
5
____ 11
...
attraction between polar molecules
____ 13
...

____ 14
...
the number and kind of atoms that are bonded by the transfer of electrons
b
...
information about a molecule’s structure
d
...
What is shown by the structural formula of a molecule or polyatomic ion?
a
...
the number of ionic bonds

c
...
the shapes of molecular orbitals
____ 16
...
What information does the molecular
formula provide about hydrogen cyanide?
a
...

b
...

c
...

d
...

____ 17
...
One atom completely loses two electrons to the other atom in the bond
...
Two atoms share two pairs of electrons
...
Two atoms share two electrons
...
Two atoms share one electron
...
Why do atoms share electrons in covalent bonds?
a
...
to attain a noble-gas electron configuration
c
...
to increase their atomic numbers
____ 19
...
carbon
b
...
fluorine
d
...
Which noble gas has the same electron configuration as the oxygen in a water molecule?
a
...
neon
c
...
xenon
____ 21
...
hydrogen only
b
...
halogens and members of the oxygen group only
d
...
What is the representative unit in a molecular compound?
a
...
an ion
c
...
shared electrons

____ 23
...
2s 2p
b
...
2s 2p 3s
d
...
Which of the following diatomic molecules is joined by a double covalent bond?
a
...

c
...

____ 25
...
CO
b
...
CO
d
...
The chemical formula of an ionic compound shows
a
...

b
...

c
...

d
...

____ 27
...
They are stronger
...
They are more ionic in character
...
They are weaker
...
There is no difference
...
When H forms a bond with H O to form the hydronium ion H O , this bond is called a coordinate
covalent bond because
a
...

b
...

c
...

d
...

____ 29
...
C—C
b
...
O—H
d
...
How many valid electron dot formulas—having the same number of electron pairs for a molecule or ion—can
be written when a resonance structure occurs?
a
...
1 only
c
...
2 or more

____ 31
...
H S
b
...
PCl
d
...
A resonance structure, like the one above, represents
a
...

b
...

c
...

d
...

____ 33
...
classical mechanical model
b
...
quantum mechanical model
d
...
A bond that is not symmetrical along the axis between two atomic nuclei is a(n) ____
...
alpha bond
b
...
pi bond
d
...
A pair of molecular orbitals is formed by the
a
...

b
...

c
...

d
...

____ 36
...
alpha bond
b
...
pi bond
d
...
Where are the electrons most probably located in a molecular bonding orbital?
a
...
between the two atomic nuclei
c
...
in circular orbits around each nucleus
____ 38
...
s only
b
...
d only
d
...
Which of the following bond types is normally the weakest?
a
...
sigma bond formed by the overlap of two p orbitals
c
...
pi bond formed by the overlap of two p orbitals
____ 40
...
pairs of valence electrons
b
...
mobile electrons
d
...
The shape of the methane molecule is ____
...
tetrahedral
b
...
four-cornered
d
...
What causes water molecules to have a bent shape, according to VSEPR theory?
a
...
interaction between the fixed orbitals of the unshared pairs of oxygen
c
...
the unusual location of the free electrons
____ 43
...
molecular orbital theory
b
...
orbital hybridization theory
d
...
Experimental evidence suggests that the H—C—H bond angles in ethene, C H , are ____
...
90
b
...
5
c
...
180
____ 45
...
sp
b
...
sp
d
...
What is the shape of a molecule with a triple bond?
a
...
pyramidal
c
...
linear

____ 47
...

b
...

d
...
How many pi bonds are formed when sp hybridization occurs in ethene, C H ?
a
...
1
c
...
3
____ 49
...
C
b
...
O
d
...
A bond formed between a silicon atom and an oxygen atom is likely to be ____
...
ionic
b
...
polar covalent
d
...
Which of the following covalent bonds is the most polar?
a
...
H—C
c
...
H—N
____ 52
...

a
...
geometric center of the molecule
c
...
oxygen region of the molecule
____ 53
...
attraction between ions
b
...
sharing of electron pairs
d
...
Which of the forces of molecular attraction is the weakest?
a
...
dispersion
c
...
single covalent bond
____ 55
...
sharing of electron pairs

b
...
bonding of a covalently bonded hydrogen to an unshared electron pair
d
...
What are the weakest attractions between molecules?
a
...
Van der Waals forces
c
...
hydrogen forces
____ 57
...
attraction between ions
b
...
sharing of electron pairs
d
...
Why is hydrogen bonding only possible with hydrogen?
a
...

b
...

c
...

d
...

____ 59
...
ionic solid
b
...
metal
d
...
What is required in order to melt a network solid?
a
...
breaking ionic bonds
c
...
breaking covalent bonds
Numeric Response
61
...
What is the total number of covalent bonds normally associated with a single carbon atom in a compound?
63
...
How many electrons does a nitrogen atom need to gain in order to attain a noble-gas electron configuration?
65
...
How many electrons does carbon need to gain in order to obtain a noble-gas electron configuration?
67
...
How many covalent bonds are in a covalently bonded molecule containing 1 phosphorus atom and 3 chlorine
atoms?
69
...
What is the bond angle in a water molecule?
Essay
71
...
Can some atoms exceed the limits of the octet rule in bonding? If so, give an example
...
Indicate how bonding is explained in terms of molecular orbitals
...
Explain a pi bond and a sigma bond
...
Explain what is meant by VSEPR theory
...

76
...
Give an example of a molecule in which orbital hybridization
occurs
...
Choose a molecule which displays an exception to the octet rule and illustrate clearly, using Lewis dot
structures, why it is considered an exception
...

78
...

79
...

80
...


Chem I Chapter 8
Answer Section
MATCHING
1
...
227
OBJ: 8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
ANS: D
PTS: 1
DIF: L1
REF: p
...
2
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: knowledge
3
...
230
OBJ: 8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
ANS: A
PTS: 1
DIF: L1
REF: p
...
2
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: knowledge
5
...
248
OBJ: 8
...
1 Describe how electronegativity values determine the charge distribution in a polar molecule
...
3
...
3
...
3
...
ANS: F
PTS: 1
DIF: L1
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: knowledge
7
...
236
OBJ: 8
...
4 Explain how the strength of a covalent bond is related to its bond dissociation energy
...
3
...
3
...
3
...
ANS: G
PTS: 1
DIF: L1
REF: p
...
3
...

STA: C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: knowledge
9
...
238
OBJ: 8
...
1 Describe the relationship between atomic and molecular orbitals
...
3
...
3
...
3
...
3
...
ANS: E
PTS: 1
DIF: L1
REF: p
...
3
...

STA: C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: knowledge
11
...
240
OBJ: 8
...
2 Describe how VSEPR theory helps predict the shapes of molecules
...
3
...
3
...
3
...
3
...
ANS: C
PTS: 1
DIF: L1
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: knowledge
13
...
252
OBJ: 8
...
3 Explain why the properties of covalent compounds are so diverse
...
3
...
3
...
3
...
ANS:
OBJ:
STA:
15
...
ANS:
OBJ:
STA:
17
...
ANS:
OBJ:
STA:
19
...
ANS:
OBJ:
STA:
21
...
ANS:
OBJ:
STA:
23
...
ANS:
OBJ:
STA:
25
...
ANS:
OBJ:
STA:
27
...
ANS:
OBJ:
STA:
29
...
222
8
...
1 Identify the information a molecular formula provides
...
3
...
3
...
3
...
227
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
223
8
...
1 Identify the information a molecular formula provides
...
3
...
3
...
3
...
226
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
226
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
230
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
227
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
226 | p
...
2
...

C
...
1 | C
...
2 | C
...
3
BLM: comprehension
A
PTS: 1
DIF: L2
REF: p
...
1
...

C
...
1 | C
...
2 | C
...
3
BLM: comprehension
D
PTS: 1
DIF: L2
REF: p
...
244
8
...
1 Describe the relationship between atomic and molecular orbitals
...
3
...
3
...
3
...
3
...
230
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
230
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
224
8
...
2 Describe the representative units that define molecular compounds and ionic compounds
...
3
...
3
...
3
...
232
8
...
2 Describe how coordinate covalent bonds are different from other covalent bonds
...
3
...
3
...
3
...
233
8
...
4 Explain how the strength of a covalent bond is related to its bond dissociation energy
...
3
...
3
...
3
...
236 | p
...
2
...

C
...
1 | C
...
2 | C
...
3
BLM: application

30
...
ANS:
OBJ:
BLM:
32
...
ANS:
OBJ:
STA:
34
...
ANS:
OBJ:
STA:
36
...
ANS:
OBJ:
STA:
38
...
ANS:
OBJ:
STA:
40
...
ANS:
OBJ:
STA:
42
...
ANS:
OBJ:
STA:
44
...
ANS:
OBJ:
STA:
46
...
237
8
...
5 Describe how resonance structures are used
...
3
...
3
...
3
...
235
8
...
3 Identify some exceptions to the octet rule
...
3
...
3
...
3
...
237
8
...
5 Describe how resonance structures are used
...
3
...
3
...
3
...
240
8
...
1 Describe the relationship between atomic and molecular orbitals
...
3
...
3
...
3
...
3
...
241
8
...
1 Describe the relationship between atomic and molecular orbitals
...
3
...
3
...
3
...
3
...
240
8
...
1 Describe the relationship between atomic and molecular orbitals
...
3
...
3
...
3
...
3
...
241
8
...
1 Describe the relationship between atomic and molecular orbitals
...
3
...
3
...
3
...
3
...
241
8
...
1 Describe the relationship between atomic and molecular orbitals
...
3
...
3
...
3
...
3
...
240 | p
...
3
...

C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: comprehension
D
PTS: 1
DIF: L2
REF: p
...
3
...

C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: comprehension
A
PTS: 1
DIF: L1
REF: p
...
3
...

C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: knowledge
A
PTS: 1
DIF: L1
REF: p
...
3
...

C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: knowledge
A
PTS: 1
DIF: L2
REF: p
...
3
...

C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: comprehension
C
PTS: 1
DIF: L1
REF: p
...
3
...

C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: knowledge
C
PTS: 1
DIF: L1
REF: p
...
3
...

C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: knowledge
C
PTS: 1
DIF: L1
REF: p
...
3
...

C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: knowledge
D
PTS: 1
DIF: L2
REF: p
...


48
...


50
...


52
...


54
...


56
...


58
...


60
...
3
...

STA: C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: comprehension
ANS: C
PTS: 1
DIF: L2
REF: p
...
3
...

STA: C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: application
ANS: B
PTS: 1
DIF: L2
REF: p
...
3
...

STA: C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: application
ANS: C
PTS: 1
DIF: L2
REF: p
...
249
OBJ: 8
...
1 Describe how electronegativity values determine the charge distribution in a polar molecule
...
3
...
3
...
3
...
248 | p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: application
ANS: A
PTS: 1
DIF: L3
REF: p
...
249
OBJ: 8
...
1 Describe how electronegativity values determine the charge distribution in a polar molecule
...
3
...
3
...
3
...
248 | p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: comprehension
ANS: B
PTS: 1
DIF: L1
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: knowledge
ANS: B
PTS: 1
DIF: L1
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: knowledge
ANS: B
PTS: 1
DIF: L1
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: knowledge
ANS: B
PTS: 1
DIF: L1
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: knowledge
ANS: D
PTS: 1
DIF: L2
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: comprehension
ANS: A
PTS: 1
DIF: L2
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: comprehension
ANS: B
PTS: 1
DIF: L1
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: knowledge
ANS: D
PTS: 1
DIF: L2
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: comprehension

NUMERIC RESPONSE
61
...
ANS:

1
DIF: L2
REF: p
...
2
...

C
...
1 | C
...
2 | C
...
3
BLM: application
4

PTS:
OBJ:
STA:
63
...
228
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
ANS:

1
DIF: L1
REF: p
...
2
...

C
...
1 | C
...
2 | C
...
3
BLM: knowledge
3

PTS:
OBJ:
STA:
65
...
228
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
ANS:

1
DIF: L2
REF: p
...
2
...

C
...
1 | C
...
2 | C
...
3
BLM: comprehension
4

PTS:
OBJ:
STA:
67
...
228
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
ANS:

1
DIF: L2
REF: p
...
2
...

C
...
1 | C
...
2 | C
...
3
BLM: comprehension
3

PTS:
OBJ:
STA:
69
...
228
8
...
1 Explain the result of electron sharing in covalent bonds
...
3
...
3
...
3
...
ANS:

1
DIF: L3
REF: p
...
2
...

C
...
1 | C
...
2 | C
...
3
BLM: application
105

PTS: 1
DIF: L1
REF: p
...
3
...

STA: C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: knowledge

ESSAY
71
...
The greater the bond dissociation
energy, the more stable the compound
...

PTS: 1
DIF: L3
REF: p
...
237
OBJ: 8
...
4 Explain how the strength of a covalent bond is related to its bond dissociation energy
...
3
...
3
...
3
...
ANS:
Yes, sulfur and phosphorus can expand the octet
...
In PCl , phosphorus has 10 valence electrons
...
235
OBJ: 8
...
3 Identify some exceptions to the octet rule
...
3
...
3
...
3
...
ANS:
When two atoms combine, the overlap of their atomic orbitals produces molecular orbitals
...
Much like an
atomic orbital, two electrons are required to fill a molecular orbital
...

PTS: 1
DIF: L3
REF: p
...
3
...

STA: C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: application
74
...
A sigma bond is the
bond that results from a combination of two s orbitals, two p orbitals, or a p and an s orbital
...
Therefore, pi bonds tend to be weaker than sigma
bonds
...
240 | p
...
3
...

STA: C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: analysis
75
...

Methane, CH , for example, has four bonding electron pairs and no unshared pairs
...
5
...

PTS: 1
DIF: L3
REF: p
...
3
...

STA: C
...
1 | C
...
2 | C
...
3 | C
...
4
BLM: application
76
...
For instance, the s and p orbitals of an atom combine to make hybrid orbitals
having the character of both the s orbital and the p orbital
...
Orbital
hybridization occurs in the methane molecule in which one 2s orbital and three 2p orbitals hybridize to form
four sp orbitals
...
244
OBJ: 8
...
3 Identify the ways in which orbital hybridization is useful in describing molecules
...
3
...
3
...
3
...
3
...
ANS:
Sample Answer: NO2 is an molecule that does not satisfy the octet rule
...


This molecule can be represented by a resonance structure in which the nitrogen atom and one oxygen atom at
a time appear to have a stable octet
...


PTS: 1
DIF: L3
REF: p
...
237
OBJ: 8
...
3 Identify some exceptions to the octet rule
...
2
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: evaluation
78
...
If the difference in
electronegativities between the two atoms is less than 0
...
If the difference in
electronegativities between the two atoms is 0
...
0, the bond is moderately polar covalent
...
0 to 2
...
If the
difference in electronegativities between the two atoms is more than 2
...

PTS: 1
DIF: L3
REF: p
...
280 | p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: analysis
79
...
Generally, the strength of dispersion forces increases as the number of electrons in a molecule
increases
...

PTS: 1
DIF: L3
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: synthesis
80
...
Melting these
substances requires breaking covalent bonds throughout the solid
...

PTS: 1
DIF: L2
REF: p
...
4
...

STA: C
...
1 | C
...
2 | C
...
3
BLM: comprehension



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