Metallic bonding

• Metals also consist of a giant structure.
• What is metallic bonding?


  Metallic bonding is the electrostatic attraction between positively charged metal ions and a sea of delocalized electrons.
• What are examples of substances held together by metallic bonding?


  Elements and alloys.
• What produces the properties of metals?

  Delocalised electrons.
• Why are most metals solid at room temperature?

  Strong electrostatic forces between metal atoms and delocalised electrons are hard to break down.
• Why are metals good conductors of electricity and heat?


  Delocalised electrons carry electric charge and thermal energy.
• Why are most metals malleable?

  Layers of atoms can slide over eachother.
• Why do we not use pure metals often?


  They are too soft due to layered structure.
• We use alloys instead of pure metals because they are stronger.
• Why are alloys harder than pure metals?


  Different sized atoms makes it more difficult to slide over eachother.