general chemistry

1. Philip Dutton
University of Windsor, Canada
N9B 3P4
Prentice-Hall © 2002
General Chemistry
Principles and Modern Applications
Petrucci • Harwood • Herring
8th Edition
Chapter 12: Liquids, Solids and
Intermolecular Forces

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Contents
12-1 Intermolecular Forces and some Properties of Liquids
12-2 Vaporization of Liquids: Vapor Pressure
12-3 Some Properties of Solids
12-4 Phase Diagrams
12-5 Van der Waals Forces
12-6 Hydrogen Bonding
12-7 Chemical Bonds as Intermolecular Forces
12-8 Crystal structures
12-8 Energy Changes in the Formation of Ionic Crystals
Focus on Liquid Crystals

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12-1 Intermolecular Forces and Some
Properties of Liquids
• Cohesive Forces
– Intermolecular forces between like molecules.
• Adhesive Forces
– Intermolecular forces between unlike molecules.
• Surface Tension
– Energy or work required to increase the surface area
of a liquid.
• Viscosity
– A liquids resistance to flow

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Intermolecular Forces

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Intermolecular Forces

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12-2 Vaporization of Liquids:
Vapor Pressure

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Enthalpy of Vaporization
ΔHvap = Hvapor – Hliquid = - ΔHcondensation

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Boiling Point
Mercury
manometer
Vapor
pressure
of liquid
Pvap
independent
of Vliq
Pvap
independent
of Vgas
Pvap
dependent on
T

9. Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 9 of 35
Vapor Pressure and Boiling Point
(e) (d) (c) (b) (a)
Ln P = -A ( ) + B
1
T
A =
ΔHvap
R

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Clausius-Clapeyron Equation
Ln P = -A ( ) + B
1
T
Ln = - ( - )
P2
P1
1
T2
1
T1
ΔHvap
R
Example 12-1:
The vapor pressure is 5.08 kPa at 18.1 °C, the vaporization
enthalpy is 41.9 kJ/mol. What is the vapor pressure at 61.1 °C?
Example 12-2:
A compound has a 5.258 kPa vapor pressure at 15.80 °C. At 40.35
°C it has 45.61 kPa vapor pressure. What is the molar enthalpy of
vaporization in J mol-1 of this compound?

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12-3 Some Properties of Solids
Freezing Point Melting Point
ΔHfus(H2O) = +6.01 kJ/mol

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Sublimation
ΔHsub = ΔHfus + ΔHvap
= -ΔHdeposition

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12-4 Phase Diagrams
Iodine

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Phase Diagrams
Carbon dioxide

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Supercritical Fluids

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Phase Diagram of Water

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The Critical Point

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Critical Temperatures and Pressures

19. 3 dimension p-V-T surface
Csonka Gábor © 2008 Általános kémia: 3. fejezet Dia:19

20. Water 3 dimension p-V-T surface

21. Van der Waals Constants
• The Van der Waals constants can be obtained
from the critical data:
a = 3pc Vc
3 and b = Vc/3
Csonka Gábor © 2008 Általános kémia: 3. fejezet Dia:21

22. Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 22 of 35
12-5 Van der Waals Forces
• Instantaneous dipoles.
– Electrons move in an orbital to cause a polarization.
• Induced dipoles.
– Electrons move in response to an outside force.
• Dispersion or London forces.
– Instaneous dipole – induced dipole attraction.
– Related to polarizability.

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Phenomenon of Induction

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Instantaneous and Induced Dipoles

25. London dispersion in hydrocarbons
Slide 25 of 35
C5H12 C15H32 C18H38

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Dipole Dipole Interactions

27. The water molecule (dipole moment)
General Chemistry: Chapter 13 Slide 27 of 35
Dipole moment:  = 1.85 Debye
Polarizability: α = 1.48 x 10-24 cm3
δ-
δ+

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12-6 Hydrogen Bonding

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Hydrogen Bonding in HF(g)

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Hydrogen Bonding in Water
around a molecule in the solid in the liquid

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Other examples of H-Bonds
Viscosity

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12-7 Chemical Bonds as
Intermolecular Forces

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Other Carbon Allotropes

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Interionic Forces

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12-8 Crystal Structures

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Unit Cells in the Cubic Crystal System

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Holes in Crystals

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Hexagonal Close Packed (hcp)

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Coordination Number

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Counting Cell Occupancy

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X-Ray Diffraction

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X-Ray Diffraction

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Cesium Chloride

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Atomic Radii from Crystal Structures

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Sodium Chloride

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Holes in Crystals

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12-9 Energy Changes in the Formation of
Ionic Crystals

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Chapter 13 Questions
1, 3, 4, 13, 24, 26, 31,
45, 52, 61, 94, 107