structure and bonding of carbon

• Diamond


  Each carbon is joined to 4 other carbons covalently
• Graphite(structure)


  Each carbon is covalently bonded to 3 other carbons, forming layers of hexagonal rings which have no covalent bonds between the layers
• Graphite(structure and properties)


  • The layers can slide over each other due to no covalent bonds between the layers, but weak intermolecular forces
  • Soft and slippery
• Graphite


  One electron from each carbon atom is delocalised
• Graphite(electrons and conductivity)


  • Similar to metals because of its delocalised electrons
  • Can conduct electricity - unlike Diamond, because the delocalised electrons can move
• Graphene


  Single layer of graphite
• Graphene


  • Has properties that make it useful in electronics and composites
  • Very strong because atoms within its layers are very tightly bonded
  • Elastic because the planes of atoms can flex relatively easily without the atoms breaking apart
• Fullerenes


  Molecules of carbon atoms with hollow shapes
• Fullerenes


  • hollow shapes
  • Based on hexagonal rings of carbon atoms, but may also contain rings with five or seven carbon atoms
  • The first fullerene to be discovered was Buckminsterfullerene (C60), which has a spherical shape
• Carbon nanotubes


  Cylindrical fullerenes with very high length to diameter ratios
• Carbon nanotubes(uses)


  • Their properties make them useful for nanotechnology, electronics and materials
• Uses of carbon-based materials

  • Can be used as lubricants, to deliver drugs in the body and catalysts
  • Nanotubes can be used for reinforcing materials, for example tennis rackets
• giant covalent structures:

  1. diamond
  2. graphite
  3. graphene
  4. fullerenes
• diamond's properties:

  1. very hard
  2. very high melting point
  3. does not conduct electricity