Chapter 13: Liquids, Solids and Intermolecular Forces : Philip Dutton
University of Windsor, Canada
N9B 3P4
Prentice-Hall © 2002
General Chemistry
Principles and Modern Applications
Petrucci • Harwood • Herring
8th Edition Chapter 13: Liquids, Solids and Intermolecular Forces
Contents : 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
13-1 Intermolecular Forces and Some Properties of Liquids : 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
Intermolecular Forces : Intermolecular Forces
Intermolecular Forces : Intermolecular Forces
13-2 Vaporization of Liquids: Vapor Pressure : 13-2 Vaporization of Liquids: Vapor Pressure
Enthalpy of Vaporization : Enthalpy of Vaporization ΔHvap = Hvapor – Hliquid = - ΔHcondensation
Boiling Point : Boiling Point Mercury manometer Vapor pressure of liquid Pvap independent of Vliq Pvap independent of Vgas Pvap dependent on T
Vapor Pressure and Boiling Point : Vapor Pressure and Boiling Point
Clausius-Clapeyron Equation : Clausius-Clapeyron Equation
13-3 Some Properties of Solids : 13-3 Some Properties of Solids Freezing Point ΔHfus(H2O) = +6.01 kJ/mol
Sublimation : Sublimation ΔHsub = ΔHfus + ΔHvap
= -ΔHdeposition
13-4 Phase Diagrams : 13-4 Phase Diagrams Iodine
Phase Diagrams : Phase Diagrams Carbon dioxide
Supercritical Fluids : Supercritical Fluids
The Critical Point : The Critical Point
Critical Temperatures and Pressures : Critical Temperatures and Pressures
Water : Water
13-5 Van der Waals Forces : 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.
Phenomenon of Induction : Phenomenon of Induction
Instantaneous and Induced Dipoles : Instantaneous and Induced Dipoles
Dipole Dipole Interactions : Dipole Dipole Interactions
13-6 Hydrogen Bonding : 13-6 Hydrogen Bonding
Hydrogen Bonding in HF(g) : Hydrogen Bonding in HF(g)
Hydrogen Bonding in Water : Hydrogen Bonding in Water around a molecule in the solid in the liquid
Other examples of H-Bonds : Other examples of H-Bonds
13-7 Chemical Bonds as Intermolecular Forces : 13-7 Chemical Bonds as Intermolecular Forces
Other Carbon Allotropes : Other Carbon Allotropes
Interionic Forces : Interionic Forces
13-8 Crystal Structures : 13-8 Crystal Structures
Unit Cells in the Cubic Crystal System : Unit Cells in the Cubic Crystal System
Holes in Crystals : Holes in Crystals
Hexagonal Close Packed (hcp) : Hexagonal Close Packed (hcp)
Coordination Number : Coordination Number
Counting Cell Occupancy : Counting Cell Occupancy
X-Ray Diffraction : X-Ray Diffraction
X-Ray Diffraction : X-Ray Diffraction
Cesium Chloride : Cesium Chloride
Atomic Radii from Crystal Structures : Atomic Radii from Crystal Structures
Sodium Chloride : Sodium Chloride
Holes in Crystals : Holes in Crystals
13-9 Energy Changes in the Formation of Ionic Crystals : 13-9 Energy Changes in the Formation of Ionic Crystals
Chapter 13 Questions : Chapter 13 Questions 1, 3, 4, 13, 24, 26, 31, 45, 52, 61, 94, 107