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The Nature of Solids Chapter 10
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Solids: Gases = very free to move Liquids = relatively free to move Solids = not very free to move
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Solids: Solids do not move freely like liquids and gases Rather, they vibrate about fixed points
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Solids: Do not take the shape or volume of the container They are dense and incompressible
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Solids and kinetic energy: Increase in average kinetic energy = increase in particle vibration = increase in temperature
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Melting Point: Mp = Solid turning to liquid Vibrations are strong enough to overcome the intermolecular interactions
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Freezing Point: Opposite of melting point Liquid turns into a solid because the particles slow down and intermolecular forces are stronger
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Equilibrium: A solid will melt and freeze at the same temperature This is the point of equilibrium, assuming temperature is remaining constant
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Solids: Ionic Solids (ex: NaCl) = high melting points They have relatively strong forces holding them together
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This is table salt
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Solids: Molecular compounds = low melting temperatures Example – hydrogen chloride has a melting temperature of -112 0 C
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Solids: Not all solids melt, some will decompose Example: wood, cane sugar
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Sugar or Rock Candy MMMMMM
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Crystal structure: Crystalline (crystals) = atoms, ions or molecules are arranged in a repeated, three dimensional pattern called a crystal lattice
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Crystals:
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Diamond Structure
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Crystals: Have regular shape Shape reflects the arrangement of the particles within the solid Types of bonds determines the melting point Ionic = high melting point Molecular = low melting point
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Graphite Structure
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Crystals: Have sides or faces Angles of the sides for a given crystal are always the same
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Crystal Classification: Galena –Cubic
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Crystal Classification: Zircon –Tetragonal
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Crystal Classification: Blue Topaz –Orthorhombic
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Crystal Classification: Gypsum –Monoclinic
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Crystal Classification: Amazonite –Triclinic
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Crystal Classification: Tourmaline –Hexagonal
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Crystal Classification: Calcite –Rhombohedral
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Shape of Crystals: Shape depends on arrangement of crystals Unit cell = smallest group of particles that retains geometric shape
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More than one Form? Carbon is an example of a crystal that can exist in more than one form
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Many forms of carbon: Diamonds Graphite Buckyball or Buckminsterfullerene- 60 + carbon atoms shaped like a soccer ball
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Many forms of Carbon: Allotropes –Two or more molecular forms of the same element in the same physical state (diamond, graphite & buckyballs)
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Example: diamonds and graphite
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Amorphous Solids: Lack ordered internal structure Non- crystalline Example- rubber, plastics, asphalt and glasses –Glasses are sometimes called super cooled liquids
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Nature of Liquids Now, go on to the Nature of Liquids Power Point Click Here Click Here to go to go to Nature of Liquids Nature of Liquids
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