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Livro Prentice-Hall 2002
Citation preview
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
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 2 of 35
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
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 3 of 35
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
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 4 of 35
Intermolecular Forces
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 5 of 35
Intermolecular Forces
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 6 of 35
13-2 Vaporization of Liquids:Vapor Pressure
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 7 of 35
Enthalpy of Vaporization
ΔHvap = Hvapor – Hliquid = - ΔHcondensation
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 8 of 35
Boiling Point
Mercury manometer
Vapor pressure of liquid
Pvap independent
of Vliq
Pvap independent
of Vgas
Pvap dependent on
T
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 9 of 35
Vapor Pressure and Boiling Point
(e) (d) (c) (b) (a)
Ln P = -A ( ) + B1T
A = ΔHvap
R
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 10 of 35
Clausius-Clapeyron Equation
Ln P = -A ( ) + B1T
Ln = - ( - ) P2
P1
1T2
1T1
ΔHvap
R
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 11 of 35
13-3 Some Properties of Solids
Freezing Point Melting Point
ΔHfus(H2O) = +6.01 kJ/mol
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 12 of 35
Sublimation
ΔHsub = ΔHfus + ΔHvap
= -ΔHdeposition
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 13 of 35
13-4 Phase Diagrams
Iodine
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 14 of 35
Phase Diagrams
Carbon dioxide
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 15 of 35
Supercritical Fluids
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 16 of 35
The Critical Point
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 17 of 35
Critical Temperatures and Pressures
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 18 of 35
Water
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 19 of 35
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.
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 20 of 35
Phenomenon of Induction
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 21 of 35
Instantaneous and Induced Dipoles
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 22 of 35
Dipole Dipole Interactions
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 23 of 35
13-6 Hydrogen Bonding
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 24 of 35
Hydrogen Bonding in HF(g)
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 25 of 35
Hydrogen Bonding in Water
around a molecule in the solid in the liquid
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 26 of 35
Other examples of H-Bonds
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 27 of 35
13-7 Chemical Bonds as Intermolecular Forces
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 28 of 35
Other Carbon Allotropes
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 29 of 35
Interionic Forces
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 30 of 35
13-8 Crystal Structures
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 31 of 35
Unit Cells in the Cubic Crystal System
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 32 of 35
Holes in Crystals
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 33 of 35
Hexagonal Close Packed (hcp)
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 34 of 35
Coordination Number
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 35 of 35
Counting Cell Occupancy
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 36 of 35
X-Ray Diffraction
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 37 of 35
X-Ray Diffraction
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 38 of 35
Cesium Chloride
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 39 of 35
Atomic Radii from Crystal Structures
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 40 of 35
Sodium Chloride
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 41 of 35
Holes in Crystals
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 42 of 35
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 43 of 35
13-9 Energy Changes in the Formation of Ionic Crystals
Prentice-Hall © 2002 General Chemistry: Chapter 13 Slide 44 of 35
Chapter 13 Questions
1, 3, 4, 13, 24, 26, 31, 45, 52, 61, 94, 107