Metallic bonding

What is a metallic bond?

The electrostatic force of attraction between positive metal ions & a sea of negative electrons

Describe the structure of a metallic bond

A giant 3 dimensional lattice of positive metal ions surrounded by a sea of delocalised electrons

How are the positive metal ions kept close together?

By the sea of delocalised electrons

More delocalised electrons means a stronger metallic bond

Why do metallic bonds have high melting & boiling points?

Because the bonds between the positive metal ions & the negative delocalised electrons are very strong, allowing the metal to maintain a giant regular structure

This requires a lot of energy to overcome, therefore high temperatures are needed to break the bonds, giving metallic bonds high melting & boiling points

Why are metallic bonds good conductors of heat & electricity?

Because they have a sea of delocalised electrons, meaning that they have charged particles that are free to move

What are the properties of metals?

- Ductile (can be drawn / pulled into a wire)

- Malleable (can be bent & shaped without breaking)

- Conductors of heat & electricity

- High melting & boiling points

- Shiny

- Sonorous (clangs when hit)

Why are metals malleable?

Because their layers can slide over each due the sea of delocalised electrons