Graphite

• Graphite


  Another form of carbon, a giant covalent molecule
• Graphite


  • Soft and slippery
  • High melting and boiling point
  • Good conductor of electricity and heat
• Structure of graphite


  1. Carbon atoms form covalent bonds to 3 other carbon atoms

  2. Carbon atoms form hexagonal rings

  3. Hexagonal rings arranged into layers

  4. No covalent bonds between layers
• No covalent bonds between layers in graphite


  Layers can slide over each other, making graphite soft and slippery
• Graphite contains many strong covalent bonds


  Requires a lot of energy to melt graphite, explaining its high melting and boiling point
• Delocalized electrons in graphite

  Electrons in the outer energy level of carbon atoms that are not in covalent bonds, can move and conduct electricity and heat
• Graphite has delocalized electrons


  Makes graphite a good conductor of electricity and heat, similar to metals
• Graphite is formed from the element carbon, so it is not a metal