# Explain why graphite can conduct electricity but most other giant covalent structures, such as diamond, cannot.

> OCR GCSE Chemistry A: Gateway Science (J248) — C2.2 Bonding · Explain · 4 marks

> Graphite is used as an electrode material in industrial electrolysis cells. Diamond, despite also being a giant covalent structure made entirely of carbon atoms, is used as an electrical insulator in cutting tools.

## Mark scheme (4 marks)

1. Graphite has delocalised electrons (one per carbon atom) that are free to move
2. These delocalised electrons can carry charge through the structure, allowing electrical conduction
3. In diamond, each carbon atom forms four covalent bonds, so all electrons are involved in bonding / there are no delocalised electrons
4. Without delocalised electrons there are no charge carriers, so diamond cannot conduct electricity

## Key terms

- [giant covalent structure](https://www.gradenine.co.uk/glossary/giant-covalent-structure)

## Related

- [Revision notes for OCR GCSE Chemistry A: Gateway Science (J248)](https://www.gradenine.co.uk/learn)
- [How to answer "Explain" questions](https://www.gradenine.co.uk/tools/command-word-cheatsheet)
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Source: [GradeNine](https://www.gradenine.co.uk/q/explain-why-graphite-can-conduct-electricity-282d900a) · Published by Druglandscape Ltd.