Metals as conductors

• • Metals consist of giant structures
  • Within the metal lattice, the atoms lose their outer electrons and become positively charged metal ions
  • The outer electrons no longer belong to any specific metal atom and are said to be delocalised
• • Metals can conduct electricity because the delocalised electrons are able to move through the structure and carry a charge 
• • The metallic bond is the strong force of attraction between the positive metal ions and the delocalised electrons
  • This type of bonding occurs in metals and metal alloys, which are mixtures of metal
• When explaining why metals conduct electricity in an exam, be careful that you don't write electrons move 'throughout' the structure, but say 'through' the structure.
• • Metals are also good conductors of heat
  • The delocalised electrons are free to move and transfer thermal energy through the structure
  • Some metals are better conductors of heat energy than others