The document discusses intermolecular forces, liquids, and solids. It defines intermolecular forces as attractive forces between molecules, and describes different types including dipole-dipole forces, ion-dipole forces, and dispersion forces. Hydrogen bonding is discussed as a special type of dipole-dipole force. Solids are described as possessing rigid, long-range molecular order and defined unit cells, while liquids and amorphous solids lack long-range order.

1. Intermolecular Forces
and
Liquids and Solids
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2. A phase is a homogeneous part of the system in
contact with other parts of the system but
separated from them by a well-defined boundary.
2 Phases
Solid phase - ice
Liquid phase - water
11.1

3. Intermolecular Forces
Intermolecular forces are attractive forces between molecules.
Intramolecular forces hold atoms together in a molecule.
Intermolecular vs Intramolecular
• 41 kJ to vaporize 1 mole of water (inter)
• 930 kJ to break all O-H bonds in 1 mole of water (intra)
“Measure” of intermolecular force
Generally,
boiling point
intermolecular
forces are much melting point
weaker than ∆Hvap
intramolecular
∆Hfus
forces.
∆Hsub 11.2

4. Intermolecular Forces
Dipole-Dipole Forces
Attractive forces between polar molecules
Orientation of Polar Molecules in a Solid
11.2

5. Intermolecular Forces
Ion-Dipole Forces
Attractive forces between an ion and a polar molecule
Ion-Dipole Interaction
11.2

6. 11.2

7. Intermolecular Forces
Dispersion Forces
Attractive forces that arise as a result of temporary
dipoles induced in atoms or molecules
11.2

8. What type(s) of intermolecular forces exist between
each of the following molecules?
HBr
HBr is a polar molecule: dipole-dipole forces. There are
also dispersion forces between HBr molecules.
CH4
CH4 is nonpolar: dispersion forces.
S O
SO2 O
SO2 is a polar molecule: dipole-dipole forces. There are
also dispersion forces between SO2 molecules.
11.2

9. Intermolecular Forces
Hydrogen Bond
The hydrogen bond is a special dipole-dipole interaction
between they hydrogen atom in a polar N-H, O-H, or F-H bond
and an electronegative O, N, or F atom.
A H…B or A H…A
A & B are N, O, or F
11.2

10. Hydrogen Bond
11.2

11. Why is the hydrogen bond considered a
“special” dipole-dipole interaction?
Decreasing molar mass
Decreasing boiling point
11.2

12. A crystalline solid possesses rigid and long-range order. In a
crystalline solid, atoms, molecules or ions occupy specific
(predictable) positions.
An amorphous solid does not possess a well-defined
arrangement and long-range molecular order.
A unit cell is the basic repeating structural unit of a crystalline
solid.
lattice At lattice points:
point • Atoms
• Molecules
• Ions
Unit Cell Unit cells in 3 dimensions 11.4

13. When silver crystallizes, it forms face-centered cubic
cells. The unit cell edge length is 409 pm. Calculate
the density of silver.
m
d= V = a3 = (409 pm)3 = 6.83 x 10-23 cm3
V
4 atoms/unit cell in a face-centered cubic cell
107.9 g 1 mole Ag
m = 4 Ag atoms x x = 7.17 x 10-22 g
mole Ag 6.022 x 1023 atoms
m 7.17 x 10-22 g
d= = = 10.5 g/cm3
V 6.83 x 10-23 cm3
11.4

14. An amorphous solid does not possess a well-defined
arrangement and long-range molecular order.
A glass is an optically transparent fusion product of inorganic
materials that has cooled to a rigid state without crystallizing
Crystalline Non-crystalline
quartz (SiO2) quartz glass 11.7