Graphite

• Formed by layers of carbon atoms
• Each carbon atom forms three covalent bonds
• Graphite has high melting and boiling points
• Graphite is soft and slippery
• It requires lots of energy to break graphite because of its strong covalent bonds
• Graphite has delocalised electrons which can move allowing graphite to conduct heat and electricity
• Graphite is an excellent conductor of heat and electricity
• 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
• Layers in graphite structure

  Can slide over each other
• 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
• Delocalized electrons in graphite

  Make graphite similar to metals
• Graphite is not a metal, it is formed from the element carbon