Metallic bonding and structure
Metals
Most metals are malleable – they can be bent and shaped without breaking. This is because they consist of layers of ions that can slide over one another when the metal is bent, hammered or pressed. Due to the ions sliding over each other, most metals are ductile – they can be drawn/pulled into wires, making them suitable for electric cables.
Metallic bonds
Metals form giant structures in which Subatomic particle, with a negative charge and a negligible mass relative to protons and neutrons. in the outer shells of the metal atoms are free to move. The metallic bond is the force of attraction between these free-moving (delocalised) electrons and positive metal Electrically charged particle, formed when an atom or molecule gains or loses an electron/electrons.. Metallic bonds are strong, so metals can maintain a regular structure and usually have high melting and boiling points.
Metals are good A material which allows charge to move easily through it. of electricity and heat. This is because the When an electron is not associated with a particular atom, eg the outer electrons in a metal can be free to move through the solid. electrons can move throughout the metal.
[Higher tier only]
The greater the number of outer electrons that the metal has, the higher its melting/boiling point. This is due to the increased positive charge on the metal ion and the increased number of electrons that are delocalised, resulting in stronger bonding.