solid

• Solids


  One of the four fundamental states of matter, where the molecules are closely packed together and contain the least amount of kinetic energy
• Properties of solids


  • Definite shape and volume
  • Melting point - temperature at which a solid changes into a liquid
  • Malleability - ability to hammer a solid into a sheet without breaking it
  • Ductility - whether a solid can be stretched to form a wire
  • Solubility - extent to which a solid dissolves in a particular solvent
  • Density - amount of mass that exists in a certain volume
  • Conductivity - flow of electrons from one place to another
• Crystalline solids


  Solids whose atoms, ions, or molecules are ordered in well-defined arrangements, usually with flat surfaces and sharp angles

  
• Amorphous solids


  Solids whose particles do not have orderly structures, with poorly-defined shapes

  
• Types of crystalline solids

  • Ionic solids
  • Molecular solids
  • Metallic solids
  • Network solids

  
• Ionic solids


  • Hard, high melting point, insulating as a solid but conducting when dissolved
• Molecular solids


  • Soft, low melting point, poor thermal and electrical conductors
• Metallic solids


  • Wide range of hardness and melting points, good thermal and electrical conductors
• Network solids


  • Hard, high melting point, poor thermal and electrical conductors
• Crystal structure


  Smallest repeating unit lattice, a three-dimensional system of points designating the position of the components (atoms, ions, or molecules) that make up a crystal

  
• Types of unit cell

  • Cubic
  • Tetragonal
  • Orthorhombic
  • Monoclinic
  • Rhombohedral
  • Hexagonal
  • Triclinic
• Specific heat


  Amount of heat needed to raise the temperature of one gram of a substance by one degree Celsius
• Heat of fusion


  Energy absorbed to break the bonds that hold water molecules in the solid structure of ice
• Heat of freezing


  Amount of heat given up or released when 1 gram of water changes to 1 gram of ice
• Heat of vaporization


  Energy absorbed to change 1 gram of liquid to gas at its boiling point
• Heat of condensation


  Heat released when 1 gram of a gas condenses to a liquid at its boiling point
• Specific heat values for water: ice = 2.03 J/g°C, liquid = 4.18 J/g°C, steam = 1.99 J/g°C
• Heat of fusion of water = 333 J/g, heat of vaporization of water = 2260 J/g
• Sample problem: Calculating heat absorbed by skin from 150 g steam at 100°C

  1. Given: m = 150 g, c = 4.18 J/g°C, ΔT = 63°C

  2. Equation: Q = mcΔT

  3. Solution: Q = (150 g)(4.18 J/g°C)(63°C) = 39,501 J

  4. Heat absorbed = mΔHvap = (150 g)(2260 J/g) = 339,000 J

  5. Total Q = 39,501 J + 339,000 J = 378,501 J
• Phase diagram of water shows transitions between solid, liquid, and gas phases
• Phase diagram of CO2 shows critical point and triple point
• Ability of water to undergo phase changes is significant
• Students will answer a 20-item multiple-choice quiz to evaluate their understanding
• Labster simulation is provided to extend learning