Covalent Bonding

• Covalent Bonding 


  The bonding between non-metal atoms
• Simple covalent bond


  a shared pair of electrons
• Double covalent bond


  two shared pairs of electrons
• Simple covalent bonds do not conduct electricity as they don't have any free electrons or ions to move
• Diamond

  • Diamond is a form of carbon
  • Each carbon is joined to 4 other carbon atoms
  • Does not conduct electricity
  • High melting and boiling points
  • used as drill bits
  • Strong and hard
• Graphite

  • Graphite is a form of carbon
  • Each carbon is joined to 3 carbon atoms
  • The 4th electron is delocalised (free)
  • Conducts electricity
  • The layers can slide over each other because there are no covalent bonds between them
  • Used in Pencils
• Fullerenes 


  Molecules of carbon atoms with hollow shapes such as cages and tubes with a different number of carbon atoms
• Buckminster fullerene

  • Spherical
  • 60 carbon atoms
• Nanotubes

  • Conducts electricity
  • Small diameter
  • large surface area
  • Low density
  • Very strong
  • used in small electronic circuits
• Fullerenes may be used for drug delivery systems in the body, in lubricants and as catalyst
• Nanotubes are useful in reinforcing structures where lightness and strength are needed