General Chemistry
Principles & Modern Applications
9th Edition
Petrucci/Harwood/Herring/Madura
Chapter 12
Liquids, Solids and Intermolecular Forces
Dr. Travis D. Fridgen
Memorial University of Newfoundland
© 2007 Pearson Education
Which row do you think has the correct heats of vaporization associated
with the compound (in its liquid form)?
1.
0.5
10.4
2.8
3.4
2.
10.4
0.5
3.4
2.8
3.
2.8
3.4
0.5
10.4
All values are in kJ mol-1.
Which row do you think has the correct heats of vaporization associated
with the compound (in its liquid form)?
1.
0.5
10.4
2.8
3.4
2.
10.4
0.5
3.4
2.8
3.
2.8
3.4
0.5
10.4
All values are in kJ mol-1.
1. Compound A has a higher vapor
pressure than compound B.
2. More energy is required to vaporize
1 mole of A than one mole of B.
3. On average, at a given temperature, B
has more kinetic energy than A.
number of molecules
The lines marked A and B represent the point where each of the molecules for
two different liquids (A and B) have enough kinetic energy to escape into the gas
phase. Which of the following statements is correct?
A
B
kinetic energy
4. On average, at a given temperature, A has more kinetic energy than B.
5. The intermolecular forces between molecules of A are stronger than
those between molecules of B.
1. Compound A has a higher vapor
pressure than compound B.
2. More energy is required to vaporize
1 mole of A than one mole of B.
3. On average, at a given temperature, B
has more kinetic energy than A.
number of molecules
The lines marked A and B represent the point where each of the molecules for
two different liquids (A and B) have enough kinetic energy to escape into the gas
phase. Which of the following statements is correct?
A
B
kinetic energy
4. On average, at a given temperature, A has more kinetic energy than B.
5. The intermolecular forces between molecules of A are stronger than
those between molecules of B.
Choose the incorrect statement,
number of molecules
The lines marked A and B represent the
point where each of the molecules for
two different liquids (A and B) have
enough kinetic energy to escape into the
gas phase.
A
B
kinetic energy
1. There would be more A than B molecules in the gas phase.
2. There are stronger intermolecular forces between molecules of A than
molecules of B.
3. Increasing the temperature would result in more molecules of both A and B
in the gas phase.
Choose the incorrect statement,
number of molecules
The lines marked A and B represent the
point where each of the molecules for
two different liquids (A and B) have
enough kinetic energy to escape into the
gas phase.
A
B
kinetic energy
1. There would be more A than B molecules in the gas phase.
2. There are stronger intermolecular forces between molecules of A than
molecules of B.
3. Increasing the temperature would result in more molecules of both A and B
in the gas phase.
To the right is the phase diagram
for iodine. Which of the following
transitions occur when the
temperature and pressure
conditions are changed from A to
B to C to D?
1.
l
s
g
l
2.
s
l
g
s
3.
g
s
l
g
4.
s
l
g
l
5.
s
g
l
g
s
s
A
D
B
C
To the right is the phase diagram
for iodine. Which of the following
transitions occur when the
temperature and pressure
conditions are changed from A to
B to C to D?
1.
l
s
g
l
2.
s
l
g
s
3.
g
s
l
g
4.
s
l
g
l
5.
s
g
l
g
s
s
A
D
B
C
Butane has a much higher melting point than ethane
because (choose the best answer)
1. butane is heavier than ethane.
2. butane has more electrons and is therefore
more polarizable than ethane.
ethane
Tboil = 185 K
3. butane has more hydrogens and therefore can
make more hydrogen bonds than ethane.
4. butane is more polar than ethane and therefore
has stronger dipole-dipole interactions.
5. butane has more protons than ethane.
butane
Tboil = 273 K
Butane has a much higher melting point than ethane
because (choose the best answer)
1. butane is heavier than ethane.
2. butane has more electrons and is therefore
more polarizable than ethane.
ethane
Tboil = 185 K
3. butane has more hydrogens and therefore can
make more hydrogen bonds than ethane.
4. butane is more polar than ethane and therefore
has stronger dipole-dipole interactions.
5. butane has more protons than ethane.
butane
Tboil = 273 K
The boiling points of some rare gases are provided to
the right. This trend in boiling points is best explained
with reference to
Tboil = -269 oC
Tboil = -246 oC
1. the masses of the atoms.
2. the polarizabilities of the atoms.
Tboil = -186 oC
3. the dipole moment of the atoms.
4. the number of neutrons in the nuclei of the atoms.
5. the trend in melting points of the solid rare gases.
Tboil = -153 oC
The boiling points of some rare gases are provided to
the right. This trend in boiling points is best explained
with reference to
Tboil = -269 oC
Tboil = -246 oC
1. the masses of the atoms.
2. the polarizabilities of the atoms.
Tboil = -186 oC
3. the dipole moment of the atoms.
4. the number of neutrons in the nuclei of the atoms.
5. the trend in melting points of the solid rare gases.
Tboil = -153 oC
Two C3H6O isomers, acetone and methoxy ethene are
shown below. Being isomers, the molar masses and
the number of electrons are equal. Their boiling points,
however, are quite different. The best reason for the
difference in boiling points is?
1. Methoxy ethane is much more polarizable.
acetone
Tboil = 330 K
2. Acetone molecules can participate in hydrogen
bonding with one another.
3. Methoxy ethane molecules can participate in
hydrogen bonding with one another.
4. Acetone has a higher dipole moment.
5. Methoxy methane has a higher dipole moment.
methoxy ethene
Tboil = 279 K
Two C3H6O isomers, acetone and methoxy ethene are
shown below. Being isomers, the molar masses and
the number of electrons are equal. Their boiling points,
however, are quite different. The best reason for the
difference in boiling points is?
1. Methoxy ethane is much more polarizable.
acetone
Tboil = 330 K
2. Acetone molecules can participate in hydrogen
bonding with one another.
3. Methoxy ethane molecules can participate in
hydrogen bonding with one another.
4. Acetone has a higher dipole moment.
5. Methoxy methane has a higher dipole moment.
methoxy ethene
Tboil = 279 K
Propanol is a relatively volatile liquid while glycerol is
a very viscous liquid much like syrop. The difference
in the viscosity of these liquids is best explained by
1. the fact that glycerol is much heavier than
1-propanol.
1-propanol
2. the fact that glycerol is a more polar molecule
than 1-propanol.
3. the fact that glycerol can form more hydrogen
bonds than 1-propanol.
4. the higher polarizability of 1-propanol.
5. the higher polarizability of glycerol.
glycerol
Propanol is a relatively volatile liquid while glycerol is
a very viscous liquid much like syrop. The difference
in the viscosity of these liquids is best explained by
1. the fact that glycerol is much heavier than
1-propanol.
1-propanol
2. the fact that glycerol is a more polar molecule
than 1-propanol.
3. the fact that glycerol can form more hydrogen
bonds than 1-propanol.
4. the higher polarizability of 1-propanol.
5. the higher polarizability of glycerol.
glycerol
Which process would you expect to require the most energy?
1. The conversion of 1 mole of solid ethanol to 1 mole of
liquid ethanol.
2. The conversion of 1 mole of solid chloroethane to 1
mole of liquid chloroethane.
3. The conversion of 1 mole of solid ethane to 1 mole of
liquid ethane.
4. The conversion of 1 mole of liquid ethanol to 1 mole of
gaseous ethanol.
5. The conversion of 1 mole of liquid chloroethane to 1
mole of gaseous chloroethane.
Which process would you expect to require the most energy?
1. The conversion of 1 mole of solid ethanol to 1 mole of
liquid ethanol.
2. The conversion of 1 mole of solid chloroethane to 1
mole of liquid chloroethane.
3. The conversion of 1 mole of solid ethane to 1 mole of
liquid ethane.
4. The conversion of 1 mole of liquid ethanol to 1 mole of
gaseous ethanol.
5. The conversion of 1 mole of liquid chloroethane to 1
mole of gaseous chloroethane.
True or false. At 370 K the vapor
pressure of benzene is the greatest
of the three substances shown and
Toluene has the lowest whereas at
313 K benzene still has the higher
vapor pressure but water has the
lowest.
1. True
2. False
370 K
313 K
True or false. At 370 K the vapor
pressure of benzene is the greatest
of the three substances shown and
Toluene has the lowest whereas at
313 K benzene still has the higher
vapor pressure but water has the
lowest.
1. True
2. False
370 K
313 K
To the left is a cartoon diagram of a particular
unit cell. How many atoms would there be in 1
mole of these unit cells?
1. 6.022 x 1023 atoms.
2. 4 moles of atoms
3. 2 x (6.022 x 1023) atoms.
4. 4 x (6.022 x 1023) atoms.
5. 1.875 moles
To the left is a cartoon diagram of a particular
unit cell. How many atoms would there be in 1
mole of these unit cells?
1. 6.022 x 1023 atoms.
2. 4 moles of atoms
3. 2 x (6.022 x 1023) atoms.
4. 4 x (6.022 x 1023) atoms.
5. 1.875 moles
scc
bcc
fcc
512 pm
627 pm
If Ba were to solidify with
the crystal structures to
the right, the edge
lengths would be as
given below
444 pm
This means that the bcc and fcc unit cells have volumes which are roughly 1.5
and 3 times as large, respectively, as the scc unit cell. Which of the following
statements is best,
1. The density of the fcc unit cell is larger because the volume is larger.
2. The density of the fcc unit cell is smaller because the volume is larger.
3. The density of the scc unit is larger because the volume is smaller.
4. The density of the fcc unit cell is larger because the mass is larger.
5. The density of the scc unit cell is larger because the mass is larger.
scc
bcc
fcc
512 pm
627 pm
If Ba were to solidify with
the crystal structures to
the right, the edge
lengths would be as
given below
444 pm
This means that the bcc and fcc unit cells have volumes which are roughly 1.5
and 3 times as large, respectively, as the scc unit cell. Which of the following
statements is best,
1. The density of the fcc unit cell is larger because the volume is larger.
2. The density of the fcc unit cell is smaller because the volume is larger.
3. The density of the scc unit is larger because the volume is smaller.
4. The density of the fcc unit cell is larger because the mass is larger.
5. The density of the scc unit cell is larger because the mass is larger.
Which of the following would you expect to have the largest lattice energy?
1. MgCl2
2. MgBr2
3. NaBr
4. CaCl2
5. CaBr2
∆ lattace H o ∝
cation charge × anion charge
cation radius + anion radius
Which of the following would you expect to have the largest lattice energy?
1. MgCl2
2. MgBr2
3. NaBr
4. CaCl2
5. CaBr2
∆ lattace H o ∝
cation charge × anion charge
cation radius + anion radius
Which of the following ionic compounds would you expect to require more energy
to decompose to gaseous ions than CaS(s)?
1. NaF(s)
2. SrS(s)
3. AlN(s)
4. MgBr2(s)
5. SrSe(s)
Which of the following ionic compounds would you expect to require more energy
to decompose to gaseous ions than CaS(s)?
1. NaF(s)
2. SrS(s)
3. AlN(s)
4. MgBr2(s)
5. SrSe(s)
Which of the following ionic compounds would you expect to have the lowest
boiling point?
1. KF
2. BeO
3. BN
4. KBr
5. NaCl
Which of the following ionic compounds would you expect to have the lowest
boiling point?
1. KF
2. BeO
3. BN
4. KBr
5. NaCl