C2.3.2 - Graphite

• Structure and bonding

  Graphite has a giant covalent structure in which:

  • each carbon atom forms three covalent bonds with other carbon atoms
  • the carbon atoms form layers of hexagonal rings
  • there are no covalent bonds between the layers (weak bonds)
  • there is one non-bonded - or delocalised - electron from each atom

  
• Properties and uses

  Graphite has delocalised electrons, just like metals. These electrons are free to move between the layers in graphite, so graphite can conduct electricity. This makes graphite useful for electrodes in batteries and for electrolysis.

  The forces between the layers in graphite are weak. This means that the layers can slide over each other. This makes graphite slippery, so it is useful as a lubricant.