1. Metallic bonding Metals conduct electricity
There must be charged particles that can move
Metals (usually) have high melting points
There must be strong forces holding the particles together

2. What does it look like inside a metal?
The atoms are in a lattice
Each atom loses its valence (outer) electrons to a delocalised ‘sea’
So we have a “lattice of positive ions in a sea of free electrons”
This would be a Group 1 metal as each atom has lost one electron
A Group 2 metal would be a better conductor

3. Why do metals conduct?
Because the delocalised electrons are free to move
Why do metals have high melting points?
Because there is a strong force between all the positive ions and the sea of free electrons
Why are metals malleable (can be bent into shape)?
atoms are arranged in layers
layers can slide over each other