C2 - Metallic Bonding

How are atoms arranged in metals?

Atoms are arranged in a giant structure, electrons in outer shells are delocalised, strong forces of electrostatic attraction between positive metal ions and shared negative electrons, forces of attraction hold atoms together in a regular structure and are known as metallic bonding which is very strong, substances held together by metallic bonding are either metal elements or alloys, and delocalised electrons produce many of the properties of metals.

Why are most metals solid at room temperature?

It requires a lot of energy to break the electrostatic forces between metal ions and the sea of delocalised electrons, so most metals have very high melting and boiling points.

Why are metals good conductors of electricity and thermal energy?

The delocalised electrons can move through the entire structure and carry electrical charge and thermal energy.

Why are most metals malleable?

Layers of atoms can slide over each other.

Why are alloys harder than pure metals?

Different elements have different sized elements which disrupt the regular lattice structure when they are put in mixture. Therefore, layers can’t easily slide over each other so they are harder than pure metals.