# Graphite and diamond are both giant covalent structures made entirely of carbon atoms, yet they have very different properties. Explain why graphite can conduct electricity but diamond cannot.

> AQA GCSE Chemistry (8462) — 4.2.3 Structure and bonding of carbon · Explain · 4 marks

## Mark scheme (4 marks)

1. In graphite, each carbon atom forms three covalent bonds (with three other carbon atoms)
2. This leaves one electron per carbon atom that is delocalised / not used in bonding
3. These delocalised electrons are free to move through the structure and carry electrical charge
4. In diamond, each carbon forms four covalent bonds so there are no delocalised / free electrons to carry charge

## Key terms

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

## Related

- [Revision notes for AQA GCSE Chemistry (8462)](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/graphite-and-diamond-are-both-giant-45356255) · Published by Druglandscape Ltd.