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PSHS WV Beryllium
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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
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
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
Properties of Liquids
Part III
Properties of Liquid
• Viscosity – Resistance to Flow– Increase Intermolecular Force; Increase
Viscosity– Increase Temperature; Decrease Intermolecular
Force; Decrease Viscosity
Properties of Liquids
Cohesion is the intermolecular attraction between like molecules
11.3
Adhesion is an attraction between unlike molecules
Adhesion
Cohesion
Concave Meniscus of Water
Chemistry; The Science in Context; by Thomas R Gilbert, Rein V. Kirss, and Geoffrey Davies, Norton Publisher, 2004, p 458
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
Consequences of Surface Tension
Chemistry; The Science in Context; by Thomas R Gilbert, Rein V. Kirss, and Geoffrey Davies, Norton Publisher, 2004, p 457
Consequences of Surface Tension
Chemistry; The Science in Context; by Thomas R Gilbert, Rein V. Kirss, and Geoffrey Davies, Norton Publisher, 2004, p 458
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
Increasing Strength of Intermolecular Force
• Higher Boiling and Melting Point
• Higher Surface Tension
• Higher Viscosity
• Lower Equilibrium Vapor Pressure
Phase Changes
Part IV
Equilibrium Vapor Pressure
• Pressure exerted by gas vapor, in closed container, at a given temperature.
BeforeEvaporation
At Equilibrium
11.8
Why is the Boiling Point of Water Constant ?
Heat
Solid Liquid
Gas
Triple Point
Increasing Temperature
Increasing Pressure
Phase Diagram
Solid Liquid
Gas
Phase Diagram of Water
Solid
Liquid
Gas
Properties of Crystalline Solids
Part V
Simple Cubic Unit Cell
Coordination #
# of Lattice Points Surrounding Each Lattice Point
Simple Cubic Unit Cells
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
Crystalline Solids Differ in …
1. Lattice Point Representation
2. Type of Force Holding Lattice Point Together
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
Ionic Crystals
CsCl ZnS CaF2
Molecular Crystals (Ice)
Covalent Crystals
Diamond
Graphite
Metallic Crystals
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
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