GCSE-ready- Home
- Lessons
- GCSE & IGCSE Chemistry
- Metallic bonding
Metallic bonding
🎬 The doodle video for this lesson is coming soon. Subscribe on YouTube to see it first.
Metals have their own kind of bonding, which explains why they conduct electricity and can be hammered into shape.
The metallic lattice
In a 2-D diagram, a metal is drawn as rows of positive ions surrounded by a 'sea' of delocalised electrons (the outer electrons that have left the atoms).
The ions are arranged in a regular pattern (a lattice).
The ions are arranged in a regular pattern (a lattice).
Metallic bonding
Metallic bonding is the strong electrostatic attraction between the positive metal ions and the delocalised electrons.
This attraction is strong, so most metals have high melting points.
This attraction is strong, so most metals have high melting points.
Explaining properties
Electrical conductivity: the delocalised electrons can move through the structure, carrying charge.
Malleability: the layers of positive ions can slide over each other when a force is applied. The delocalised electrons still hold them together, so the metal changes shape instead of breaking.
Malleability: the layers of positive ions can slide over each other when a force is applied. The delocalised electrons still hold them together, so the metal changes shape instead of breaking.
Explain why copper can be hammered into a thin sheet without breaking.
- Copper has layers of positive ions in a sea of delocalised electrons.
- The layers can slide over each other.
- The metallic bonding is not broken because the electrons still attract the ions.
Answer: Layers of ions slide over each other while the delocalised electrons keep holding them together.
Metals are lattices of positive ions in a sea of delocalised electrons. Metallic bonding is the electrostatic attraction between them. Delocalised electrons move to conduct electricity; layers of ions slide, making metals malleable.
Check you have got it
Answer 6 quick questions with instant marking. If you get one wrong, GCSE-ready shows you why and gives you another go. It is free, and you do not need an account.