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Solids and the Kinetic Molecular Theory

Solids and the Kinetic Molecular Theory. Ryan Rowland AJ Rosciszewski David Milostan Toni Lukic Allison Koch. Vocabulary. Crystalline Solids: Solids consisting of solids Crystals: a substance in which the particles are arranged in an orderly, geometric, repeating pattern.

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Solids and the Kinetic Molecular Theory

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  1. Solids and the Kinetic Molecular Theory Ryan Rowland AJ Rosciszewski David Milostan Toni Lukic Allison Koch

  2. Vocabulary • Crystalline Solids: Solids consisting of solids • Crystals: a substance in which the particles are arranged in an orderly, geometric, repeating pattern. • Amorphous Solids: solid in which the particles are arranged randomly • Melting: physical change of a solid to a liquid by the addition of energy as heat • Melting Point: the temperature at which a solid becomes a liquid • Super cooled Liquids: substances that retain certain liquids properties even at temperatures at which they appear to be solid • Crystal Structure: total three dimensional arrangement of particles of a crystal

  3. Types of Solids • Amorphous Solids: • Particles are not arranged in a regular pattern. • Crystalline Solids: • Exist as single crystals, or groups of crystals fused together. • Crystal structure, and crystal lattice.

  4. Crystalline Systems • Cubic • Tetragonal • Hexagonal • Trigonal • Orthorhombic • Monoclinic • Triclinic

  5. Characteristics of Solids • Definite shape and volume: • Solids maintain a definite shape without a container. Solids have a definite volume because their particles are packed tightly together. • Definite melting point: • At melting point, kinetic energies of the particles over come the attractive forces holding them together. • High density and incompressibility: • Substances are most dense in the solid state. For practical purposes, solids can be considered incompressible. • Low rate of diffusion: • Rate of diffusion is millions of times slower in solids.

  6. Products of Binding Forces in Crystals • Ionic Crystals: • NaCl, MgF2 • Covalent Network Crystals: • (SiO2)x, Cx (Diamond) • Metallic Crystals: • Hg, Cu, Fe, W • Covalent Molecular Crystals: • Nonpolar: H2, O2, CH4, CCl4, C6H6 • Polar: NH3, H2O

  7. Understand • Ionic or network covalent substances have stronger forces and are not as likely to volatilize. • These substances often have little if any color.

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