Intermolecular and
Intramolecular Forces Review
In the compound PCl3, how many
valence electrons are present?
4
8
24
26
0%
26
0%
24
0%
8
0%
4
1.
2.
3.
4.
How many valence electrons are
available in the ion NO3 ?
16
9
22
24
0%
24
0%
22
0%
9
0%
16
1.
2.
3.
4.
Which type of bond has an electronegativity
difference greater than 1.8?
ionic
metallic
nonpolar covalent
polar covalent
no
np
o
co
va
le
nt
0%
ar
lar
m
co
v
et
al
ale
nt
lic
0%
po
l
0%
c
0%
io
ni
1.
2.
3.
4.
What molecular shape is the
compound CCl4?
trigonal planar
tetrahedral
octahedral
bent
0%
be
nt
ah
ed
ra
l
0%
oc
t
ah
ed
ra
l
0%
te
tr
al
p
lan
ar
0%
tri
go
n
1.
2.
3.
4.
How many bond pairs of electrons
exist in a molecule of ammonia
(NH
)?
3
1. 1
2. 2
3. 3
4. 4
0%
4
0%
3
0%
2
1
0%
What molecular shape is the
compound NH3?
trigonal planar
tetrahedral
trigonal pyramidal
bent
0%
be
nt
yr
a
m
...
0%
al
p
tri
go
n
ah
ed
ra
l
0%
te
tr
al
p
lan
a.
..
0%
tri
go
n
1.
2.
3.
4.
If the electronegativity of H is 2.20 and of Cl is
3.55, which type of bond is formed between H
and Cl, when they form hydrogen chloride?
1. Ionic
2. Polar ionic
3. Covalent
4. Polar covalent
0%
Po
l
ar
co
va
le
nt
en
t
0%
Co
va
l
ar
io
ni
c
0%
Po
l
Io
ni
c
0%
Which of the following is a polar
molecule?
CO2
Br2
BCl 3
NH3
CH4
0%
CH
4
0%
NH
3
0%
BC
l3
0%
Br
2
0%
CO
2
1.
2.
3.
4.
5.
Which of the following is a nonpolar
molecule?
CF4
H2O
NCl 3
NH3
NO30%
NO
3-
0%
NH
3
3
0%
NC
l
0%
H2
O
0%
CF
4
1.
2.
3.
4.
5.
Which is a typical characteristic of
an ionic compound?
0%
ha
s..
d.
..
po
un
d
om
io
ni
cc
io
ni
Th
e
cc
om
po
un
d
po
un
d
om
cc
io
ni
0%
is
ha
s.
..
sh
ar
e
ar
irs
pa
Th
e
ro
n
Ele
ct
0%
..
0%
Th
e
1. Electron pairs are shared
among atoms.
2. The ionic compound has a
low solubility in water.
3. The ionic compound is
described as a molecule.
4. The ionic compound has a
high melting point.
Why do atoms share electrons in
covalent bonds?
0%
0%
cr
ea
s
et
he
ir
a
to
m
i..
.
po
la
m
or
e
in
to
be
co
m
e
ega
s
no
bl
a
n
ta
i
at
to
el
e.
..
a.
.
at
tr
nd
ns
a
io
e
be
co
m
to
0%
r
0%
to
1. to become ions and
attract each other
2. to attain a noble-gas
electron configuration
3. to become more polar
4. to increase their
atomic numbers
en
0%
ni
tro
g
in
e
0%
flu
or
0%
ox
yg
en
bo
n
0%
ca
r
1.
2.
3.
4.
Which of the following elements can form
diatomic molecules held together by triple
covalent bonds?
carbon
oxygen
fluorine
nitrogen
The shape of the methane
molecule CH4 is called ____.
tetrahedral
square
four-cornered
planar
na
r
rn
er
ed
-co
fo
ur
0%
pl
a
0%
e
0%
sq
ua
r
ah
ed
ra
l
0%
te
tr
1.
2.
3.
4.
What causes water molecules to have a
bent shape, according to VSEPR theory?
0%
of
n
us
ua
l
lo
c
at
io
an
d
ac
t io
n
un
ttr
ca
io
ni
0%
t..
re
p.
..
th
e.
..
0%
be
tw
ee
n
t io
n
in
te
ra
c
re
pu
lsi
ve
fo
rc
es
b
et
w
ee
. ..
0%
th
e
1. repulsive forces between
unshared pairs of electrons
2. interaction between the
fixed orbitals of the
unshared pairs of oxygen
3. ionic attraction and
repulsion
4. the unusual location of the
free electrons
When placed between oppositely charged metal
plates, the region of a water molecule attracted
to the negative plate is the ____.
0%
re
gio
n
of
th
H
em
pl
o.
..
a.
.
0%
O&
#8
21
2;
he
.. .
0%
H&
#8
21
2;
en
te
ro
ft
cc
et
ri
ge
om
hy
dr
o
ge
n
re
gi
on
of
th
e
...
0%
ox
yg
en
1. hydrogen region of the
molecule
2. geometric center of the
molecule
3. H—O—H plane of the
molecule
4. oxygen region of the
molecule
What is thought to cause the
dispersion forces?
0%
n
el
ec
tr
n
on
e.
..
pa
ir s
0%
go
fe
le
ct
ro
of
el
ec
tro
ns
0%
sh
ar
in
m
ot
io
n
at
tra
ct
io
n
be
tw
ee
n
io
ns
0%
di
ffe
re
nc
es
i
1. attraction between
ions
2. motion of electrons
3. sharing of electron
pairs
4. differences in
electronegativity
Which of the forces of molecular
attraction is the weakest?
dipole interaction
dispersion
hydrogen bond
single covalent bond
nd
ale
nt
bo
sin
gle
co
v
ge
n
di
sp
er
sio
0%
bo
nd
0%
n
0%
hy
dr
o
ol
e
in
te
ra
ct
io
n
0%
di
p
1.
2.
3.
4.
What causes dipole interactions?
va
l
io
ns
0%
ee
n
ct
io
n
co
of
a
ng
bo
nd
i
be
tw
en
tly
po
l
ee
n
be
tw
0%
...
..
0%
n
ct
io
at
tra
sh
ar
in
go
fe
le
ct
ro
n
pa
ir s
0%
at
tra
1. sharing of electron pairs
2. attraction between polar
molecules
3. bonding of a covalently
bonded hydrogen to an
unshared electron pair
4. attraction between ions