Section 4 - Metallic Bonding

Question 1

Describe the bonding of metal ions in a metal (3)

Answer 1

• In a metal, the outer electrons from each atom are delocalised (they’re not stuck on one atom) - this leaves positive metal ions.
• The positive metal ions are arranged regularly in a giant structure, surrounded by a ‘sea’ of delocalised electrons.
• Metals are held together because of the electrostatic attractions between the positive metal ions and the delocalised ‘sea’ of electrons. This is called metallic bonding.

Question 2

Metals melting points

Answer 2

Metals generally have high melting points. This is because a lot of energy is required to overcome the strong metallic bonding between the particles. The more electrons that are delocalised from each atom, the stronger the bonding will be and the higher the melting point.

Question 3

Metals - electrical conductivity

Answer 3

The delocalised electrons in metals are free to move around and can carry a charge. This makes good electrical conductors.