metallic bonding

What is metallic bonding?

The electrostatic attraction between delocalised electrons and fixed positive metal ions in giant lattice.

Give two properties of metal due to metallic bonding

High melting/boiling point; good electrical/thermal conductivity

Why do metals have a high melting point

Strong electrons forces between positive ions and delocalised electrons require a lot of energy

Why are metal good conductors of elecricity

Delocalised electrons are free to move and carry electric current through the metal

Describe the structure of a metal

A giant lattice of positive metal ions surrounded by a ‘sea’ of delocalised electrons

Why can metals be hammered into shapes

Layers of metal ions can slide over each other without breaking the metallic bonds, as delocalised electrons hold the structure together.

Why can metal be drawn into wires

The uniform metallic bonding allows the layers of ions to slide past each other when pulled, without the structure breaking

Which particles are delocalised in metallic bonding

Electrons

Why don’t metallic bonds form between non-metal atoms

They don’t have delocalised electrons; they form covalent or ionic bonds instead

Explain why alloys are harder than pure metals

Atoms of different sizes distort the regular lattice, making it harder for layers to slide over each other