What is the bonding in metals like?

The atoms in metals are closely packed and regularly arranged.

The atoms lose their outer electrons and form a giant lattice of regularly arranged positive icons.

Like charges repel, so you might expect the metal icons to fly apart from each other.

This does not happen of course. Why not?

The outer electrons from the metal atoms are free to move randomly throughout the lattice of metal icons.

As the electrons do not belong to any particular metal ion, they are called delocalised electrons.

The metallic bond is the electrostatic force of attraction between the metal Ions and the delocalised electrons.

Aluminium has stronger metallic bonds than sodium and magnesium, so it has a higher boiling point.

Aluminium has stronger metallic bonds than sodium and magnesium, so it has a higher boiling point.

Aluminium has stronger metallic bonds than sodium and magnesium, so it has a higher boiling point.

Aluminium has stronger metallic bonds than sodium and magnesium, so it has a higher boiling point.

The strength of the metallic bond depends on several factors.

Aluminium ions have a greater positive charge than sodium or magnesium ions.

They are smaller and there are more delocalised electrons.

Aluminium conducts electricity better than sodium and magnesium.

Each aluminium atom contributes more delocalised electrons than sodium or magnesium atoms.