Metallic bonding

• • consists of giant structure of metal atoms
  • all give away outer electrons and share them with the other atoms
  • all ions become positive because all lost an electron
  • free delocalised electrons = strong electrostatic forces between - electrons and + metal ions
• • the very strong electrostatic forces is what holds the atoms together in a regular structure

  
• • electrostatic forces are very strong so needs lots of energy to break them
  • = high melting / boiling points
  • solid at room temp
• • Delocalised electrons can carry electric charge and current so good conductors of electricity and heat
• Malleable

  • layers in the regular structure means layers can slide over eachother so can be bent or hammered
• Alloys

  • mixing 2 metals or metal and a non metal
  • have to be 2 diff sized atoms to change the regular structure so the layers cant slide
  • = much harder than pure metal