Metallic bonding — AQA GCSE Chemistry
Test yourself on Metallic bonding with AQA GCSE practice questions.
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Metallic bonding explained
In a metal, the outer-shell electrons are not held by any one atom.
Read the full explanation
They become delocalised, meaning they are shared across the whole giant lattice and are free to move. The positive metal ions that remain are arranged in a regular pattern, and the sea of delocalised electrons is attracted to these ions in all directions. This electrostatic attraction between the positive ions and the shared electrons is the metallic bond, and because it acts throughout the structure it is strong. The model is often drawn as positive ions in a regular lattice with negative delocalised electrons between them. Moving electrons explain why metals conduct electricity and heat, while the strong bonding explains high melting points. When answering, refer to delocalised electrons, free movement, positive ions and strong electrostatic attraction.
Your focus
- Describe delocalised electrons as outer-shell electrons free to move through a metal.
- Explain metallic bonding as the attraction between positive ions and delocalised electrons.
- Use the metallic bonding model to explain conductivity and high melting points.
Metallic bonding exam tips
Marking Points
- States that outer-shell electrons in a metal become delocalised.
- Explains that delocalised electrons are free to move through the whole structure.
- Describes the metal as positive ions in a regular lattice surrounded by delocalised electrons.
- Identifies the metallic bond as the electrostatic attraction between positive ions and delocalised electrons.
- Links delocalised electrons to electrical or thermal conductivity.
- Links strong metallic bonding to high melting and boiling points.
Examiner Tips
- 💡Use the phrase sea of delocalised electrons when describing the model.
- 💡Always name the two charged species involved in the metallic bond before explaining the attraction.
- 💡When explaining conductivity, state that the delocalised electrons carry charge or energy through the metal.
Common Mistakes
- Saying that metal atoms share pairs of electrons in the same way as covalent bonds; correct this by describing delocalised electrons shared across the whole lattice.
- Describing the metal as negative ions; correct this by stating that the lattice contains positive metal ions.
- Claiming that the delocalised electrons are fixed in place; correct this by stating that they are free to move throughout the structure.