Intermolecular Forces
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Transcript of Intermolecular Forces
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Chapter 12:Intermolecular Forces and
Liquids and SolidsI. States of Matter
a) Kinetic Energy vs. Attractive Forces
II. Intermolecular Forces (Attractive, van der Waal Forces)a) Dipole-Dipole--- (Polar Molecules)
i. Hydrogen Bonding
b) Dispersion (London) Forces--- (NonPolar Molecules)
c) Attractive Forces Involving Ions
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Intermolecular Forces and Liquids and Solids
III. Properties of Liquidsa) Viscosityb) Meniscus Formationc) Surface Tensiond) Capillary Action
IV. Phase Changesa) Equilibrium Vapor Pressure
i. Normal boiling point
b) Phase Diagrams
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Intermolecular Forces and Liquids and Solids
V. Crystalline Structure of Solidsa) Unit Cells (Simple Cubic, BCC, FCC)
i. Coordination Number
ii. # Lattice Points in a Unit Cell
VI. Radius vs. Unit Cell Edge Length,aa) Density
VII. Types of Crystalline Solidsa) 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
11.3
Adhesion is an attraction between unlike molecules
Adhesion
Cohesion
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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 Tension1. Attraction of surfacemolecules that cause the liquidsurface to contract and becomemore 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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BeforeEvaporation
At Equilibrium
11.8
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Why is the Boiling Point of Water Constant ?
Heat
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Solid Liquid
Gas
Triple Point
Increasing Temperature
Increasing Pressure
Phase Diagram
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Solid Liquid
Gas
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Phase Diagram of Water
Solid
Liquid
Gas
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Properties of Crystalline Solids
Part V
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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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Unit Cell Type Coordinaton # # Lattice Pts In Unit Cell
Simple Cubic 6 1
Body Centered Cubic (BCC)
8 2
Face Centered Cubic (FCC)
12 4
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Crystalline Solids Differ in …
1. Lattice Point Representation
2. Type of Force Holding Lattice Point Together
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Crystalline Solids
Solid Type Composition Lattice Point Attractive Force
Ionic + & - ions Ion Electrostatic Attraction
Molecular 2 or more nonmetals
Molecule Intermolecular Force
Covalent 2 or more nonmetals
Nonmetal Atom
Covalent Bond
Metallic Metal atoms Metal Cation Metallic Bond
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Ionic Crystals
CsCl ZnS CaF2
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Molecular Crystals (Ice)
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Covalent Crystals
Diamond
Graphite
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Metallic Crystals
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Properties of Crystalline SolidsSolid Type High Melting
Pt?Conduct electricity as solid?
Conduct electricity dissolved in water?
Ionic YES NO YES
Molecular NO NO NO
Covalent YES NO NO
Metallic YES YES N/A
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Crystalline Solids
Solid Type Composition Lattice Point Attractive Force
Ionic + & - ions Ion Ionic Bond
Molecular 2 or more nonmetals
Molecule Intermolecular Force
Covalent 2 or more nonmetals
Nonmetal Atom
Covalent Bond
Metallic Metal atoms Metal Cation Metallic Bond
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