metallic bonding

    Cards (8)

    • describe the structure of a pure metal
      layers of positive ions surrounded by delocalised electrons
    • describe the bonding in a pure metal
      strong electrostatic forces of attraction between metal ions and delocalised electrons
    • what are four properties of pure metals?
      1. malleable
      2. high melting and boiling point
      3. good conductors of electricity
      4. good conductors of thermal energy
    • why are pure metals malleable?
      the layers can slide over each other easily
    • explain why metals have high melting and boiling points
      the electrostatic force of attraction between positive metal ions and delocalised electrons is strong and requires a lot of energy to break
    • why are metals good conductors of electricity and thermal energy?
      the delocalised electrons are free to move through the metal and therefore are able to carry the charge
    • what is an alloy?
      a mixture of a metal with atoms of another element to harden a pure metal
    • why are alloys harder than pure metals?
      the different sized atoms disturb the layers, preventing them from sliding over each other