Philip DuttonUniversity of Windsor, Canada

N9B 3P4

Prentice-Hall © 2002

General ChemistryPrinciples and Modern Applications

Petrucci • Harwood • Herring

8th Edition

Chapter 13: Liquids, Solids and Intermolecular Forces

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Contents

13-1 Intermolecular Forces and some Properties of Liquids

13-2 Vaporization of Liquids: Vapor Pressure

13-3 Some Properties of Solids

13-4 Phase Diagrams

13-5 Van der Waals Forces

13-6 Hydrogen Bonding

13-7 Chemical Bonds as Intermolecular Forces

13-8 Crystal structures

13-8 Energy Changes in the Formation of Ionic Crystals

Focus on Liquid Crystals

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13-1 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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13-2 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

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Vapor Pressure and Boiling Point

(e) (d) (c) (b) (a)

Ln P = -A ( ) + B1T

A = ΔHvap

R

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Clausius-Clapeyron Equation

Ln P = -A ( ) + B1T

Ln = - ( - ) P2

P1

1T2

1T1

ΔHvap

R

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13-3 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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13-4 Phase Diagrams

Iodine

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Phase Diagrams

Carbon dioxide

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Supercritical Fluids

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The Critical Point

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Critical Temperatures and Pressures

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Water

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13-5 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

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Dipole Dipole Interactions

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13-6 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

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13-7 Chemical Bonds as Intermolecular Forces

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Other Carbon Allotropes

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Interionic Forces

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13-8 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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13-9 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