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Intermolecular Forces Practice #1
1. Why are the intermolecular attractions in H
2
O
(g)
much weaker than the
attractions in H
2
O
(l)
or H
2
O
(s)
?
The particles in a H
2
O
g
gas are further apart, so there would not be as
much attraction between the particles
2. Consider the following: Br
2
, Ne, HCl, and N
2
.
a. Which of the above would have the largest dispersion forces?
Why?
Bromine, because it has the largest mass.
b. Which of the above would have the largest dipole-dipole
attractions? Why?
HCl, because it is the only molecule that is polar
3. Which of the following molecules would exhibit hydrogen bonding:
methane (CH
4
), hydrazine (H
2
NNH
2
),
Hydrazine would form hydrogen bonds
4. List the type(s) of intermolecular forces that are present in each of the
following examples:
a. HBr dipole / LDF

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b. I
2
LDF (dispersion)
c. CS
2
LDF
d. H
2
O Hydrogen bonding/Dipole
e. CH
2
Cl
2
Dipole-dipole
f. C
2
H
6
LDF
g. NH
3
dipole/Hydrogen
h. H
2
S Dipole
i. ClF
3
LDF
5. For each of the following, select the molecule that you would expect to
have the higher boiling point and explain your reasoning:
a. HF or HCl
HF would have the higher boiling point because it forms hydrogen bonds.

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Intermolecular Forces Practice #1 1. Why are the intermolecular attractions in H2O (g) much weaker than the attractions in H2O (l) or H2O (s)? The particles in a H2Og gas are further apart, so there would not be as much attraction between the particles 2. Consider the following: Br2, Ne, HCl, and N2. a. Which of the above would have the largest dispersion forces? Why? Bromine, because it has the largest mass. b. Which of the above would have the largest dipole-dipole attractions? Why? HCl, because it is the only molecule that is polar 3. Which of the following molecules would exhibit hydrogen bonding: methane (CH4), hydrazine (H2NNH2), Hydrazine would form hydrogen bonds 4. List the type(s) of intermolecular forces that are present in each of the following examples: a. HBr dipole / LDF b. I2 LDF (dispersion) c. CS2 LDF d. H2O Hydrogen bonding/Dipole e. CH2Cl2 Dipole-dipole f. C2H6 LDF g. NH3 dipole/Hydrogen h. H2S Dipole i. ClF3 LDF 5. For each of the following, select the molecule that you would expect to have the higher boiling point and explain your reasoning: a. HF or HCl HF would have the higher boiling point because it forms hydrogen bonds. b. CH4 or C3H8 C3H8 would have the higher boiling point because it has a greater mass / more dispersion. Consider the heating curve on the previous page, and explain the following observations from a molecular standpoint: 1. Segments AB, CD, and EF have a positive slope. The heat energy that is being added is bei ...
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