Metallic bonding

• Structure and bonding of metals

  Metals have a giant structure

  The metal atoms give up their outer shell electrons which become delocalised

  Regular lattice structure

  Strong electrostatic forces of attraction between positive metal ions and the negative delocalised electrons
• Why are metals good at conducting electricity and heat

  Delocalised electrons

  Strong intermolecular bonds
• Why are metals malleable

  Layers of metal ions can slide over one another which allows the structure to bend
• Ductile

  Able to be deformed without losing toughness
• Alloy

  Mixture of 2 or more metals (may be a metal and a non-metal)
• Why are alloys harder than pure metals

  Different elements have different-sized atoms

  This disrupts the regular layered structure

  The layers can’t slide over one another anymore

  This makes them less malleable, so harder
• Disadvantage of pure metals

  Pure metals are often too soft so an alloy must be used instead