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Nature of Solids

Nature of Solids. Objectives: 1.Compare the properties of crystalline solids with those of amorphous solids. 2.Foreach type of solid, relate its structure and bonding to its properties. KeyTerms : crystalline solid, anhydrous, amorphous solid, covalent-network solid. Nature of Solids.

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Nature of Solids

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  1. Nature of Solids Objectives: • 1.Compare the properties of crystalline solids with those of amorphous solids. • 2.Foreach type of solid, relate its structure and bonding to its properties. KeyTerms: • crystalline solid, anhydrous, amorphous solid, covalent-network solid

  2. Nature of Solids Basic Properties: • Solids, unlike liquids, have atoms and molecules in fixed positions • solids have strong intermolecular forces • Solids have a definite shape and volume • The density of most solids is only slightly greater than the liquid phase of the same material • Exception is with water • KE of Molecules (atoms) is less than the energy it takes to separate them • A solid become liquid at its melting point • KE = intermolecular forces

  3. Basic Physical Properties The physical properties solids of substances are dependent mostly on the intermolecular bonds. • hardness • melting point • electrical conductivity • luster • fracture • tensile strength • malleability • ductile

  4. Crystalline Solids A crystalline solid is one in which the molecules or atoms are arranged in highly ordered repeating patterns. • Most solids are crystalline • The smallest repeating unit is called a unit cell (think of a honeycomb) • Some crystals exist as hydrates (having water molecules) - CuSO4 * 5H2O (copper sulfate pentahydrate) has 5 water molecules included in each of its cells • Anhydrous crystalline solids are completely free of water

  5. Amorphous Solids Solids that do not form crystals and do not behave as solids are called amorphous (without form). • plastic, rubber, glass • Covalently bonded

  6. Allotropes • solid substances that are different molecular form but have the same composition

  7. Type of Solid - Metallic • Bond Type - Metallic bond • Hardness - Soft to hard • low to high melting point • Conductivity - electrical and thermal conductivity • Malleable & ductile

  8. Type of Solid - Molecular • Particles - atoms or molecules • Bond Type - Hydrogen bond, dipole-dipole, dispersion (temporary) • Hardness – soft • low to moderately high melting point • Conductivity - poor electrical and thermal conductivity • Other - most organic & inorganic compounds (methane, sugar, water)

  9. Type of Solid - Ionic • Particles - Positive & negative ions • Bonds - electrostatic attractions • Hardness - Hard, brittle • high melting point • Conductivity - poor electrical and thermal conductivity • Other - ionic salts (NaCl, KBr, MgSO4)

  10. Type of Solid - Covalent-Network • Particles – non-metals • Bonds - Covalent bonds • Hardness - very hard, brittle • very high melting point • Conductivity - often poor electrical and thermal conductivity • Other - diamond, Silicon, quartz, graphite

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