Chapter 12: Intermolecular Forces and Liquids and Solids

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Chapter 12Intermolecular Forces and Liquids and
Solids

• States of Matter
• Kinetic Energy vs. Attractive Forces
• Intermolecular Forces (Attractive, van der Waal
  Forces)
• Dipole-Dipole--- (Polar Molecules)
• Hydrogen Bonding
• Dispersion (London) Forces--- (NonPolar
  Molecules)
• Attractive Forces Involving Ions

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Intermolecular Forces and Liquids and Solids

• Properties of Liquids
• Viscosity
• Meniscus Formation
• Surface Tension
• Capillary Action
• Phase Changes
• Equilibrium Vapor Pressure
• Normal boiling point
• Phase Diagrams

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Intermolecular Forces and Liquids and Solids

• Crystalline Structure of Solids
• Unit Cells (Simple Cubic, BCC, FCC)
• Coordination Number
• Lattice Points in a Unit Cell
• Radius vs. Unit Cell Edge Length,a
• Density
• Types of Crystalline Solids
• Ionic, Molecular, Covalent, and Metallic

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Properties of Liquids

• Part III

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Properties of Liquid

• Viscosity Resistance to Flow
• Increase Intermolecular Force Increase Viscosity
• Increase Temperature Decrease Intermolecular
  Force Decrease Viscosity

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Properties of Liquids
Cohesion is the intermolecular attraction between
like molecules
Adhesion is an attraction between unlike molecules
11.3
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Concave Meniscus of Water
Chemistry The Science in Context by Thomas R
Gilbert, Rein V. Kirss, and Geoffrey Davies,
Norton Publisher, 2004, p 458
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• Surface Tension
• Attraction of surface
• molecules that cause the liquid
• surface to contract and become
• more spherical
• 2.Amount of energy required to
• stretch or increase the surface

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Consequences of Surface Tension
Chemistry The Science in Context by Thomas R
Gilbert, Rein V. Kirss, and Geoffrey Davies,
Norton Publisher, 2004, p 457
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Consequences of Surface Tension
Chemistry The Science in Context by Thomas R
Gilbert, Rein V. Kirss, and Geoffrey Davies,
Norton Publisher, 2004, p 458
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CapillaryAction Rise of Liquid up a Very Small
Diameter Glass Tube
Chemistry The Science in Context by Thomas R
Gilbert, Rein V. Kirss, and Geoffrey Davies,
Norton Publisher, 2004, p 459
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Increasing Strength of Intermolecular Force

• Higher Boiling and Melting Point
• Higher Surface Tension
• Higher Viscosity
• Lower Equilibrium Vapor Pressure

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Phase Changes

• Part IV

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Equilibrium Vapor Pressure

• Pressure exerted by gas vapor, in closed
  container, at a given temperature.

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Before Evaporation
At Equilibrium
11.8
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Why is the Boiling Point of Water Constant ?
Heat
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Phase Diagram
Increasing Pressure
Solid
Liquid
Increasing Temperature
Gas
Triple Point
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Solid
Liquid
Gas
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Phase Diagram of Water
Liquid
Solid
Gas
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Properties of Crystalline Solids

• Part V

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Unit Cells
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Simple Cubic Unit Cell
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Coordination

• of Lattice Points Surrounding Each Lattice
  Point

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Simple Cubic Unit Cells
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Crystalline Solids Differ in

• Lattice Point Representation
• Type of Force Holding Lattice Point Together

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Crystalline Solids
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Ionic Crystals
CsCl
ZnS
CaF2
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Molecular Crystals (Ice)
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Covalent Crystals
Graphite
Diamond
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Metallic Crystals
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Properties of Crystalline Solids
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Crystalline Solids
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