Metallic bonding

• Metallic bonding is the electrostatic attraction between positive nuclei and delocalised negatively charged electrons, this occurs between metal atoms in a pure or alloy metal.
• What does metallic bonding feature the electrostatic attraction of?

  Delocalized electrons and positive nuclei.
• Where is metallic bonding found?

  Metals
• To melt a metal you need to overcome all of the forces of attraction between nuclei and delocalised electrons. Metals with more delocalised electrons tend to have a greater melting point. Another factor that affects melting point is ion size. The smaller an ion the closer the electrons are leading to an overall increase in attraction strength.
• Metals can conduct electricity due to delocalised electrons being attracted to the positive charge.
• Metals can conduct heat by 2 ways. Delocalised electrons passing kinetic energy along the metal. Cations passing kinetic energy to each other due to them being highly packed.
• Metals are malleable and ductile. This is because when layers of cations are moved over each other delocalised electrons move with them to prevent strong repulsion.