Graphite

• Carbon atom in graphite


  • Able to form three covalent bonds to other carbon atoms forming layers of hexagons
  • Leaving one free electron per carbon atom
• Free electrons in graphite

  Migrate along the layers and are free to move and carry charge
• Covalent bonds within the layers

  Very strong
• Layers in graphite


  • Attracted to each other by weak intermolecular forces
  • Can slide over each other making graphite soft and slippery
• Diagram showing the structure and bonding arrangement in graphite
• Properties of Graphite


  • Conducts electricity and heat
  • Has a very high melting point
  • Is soft and slippery and less dense than diamond (2.25 g/cm3)
• Graphite's weak intermolecular forces


  Make it a useful material
• Uses of graphite


  • Pencils
  • Industrial lubricant
  • Engines
  • Locks
  • Inert electrodes for electrolysis, which is particularly important in the extraction of metals such as aluminium