# Graphite is a giant covalent structure. 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 / free to move through the structure
3. These delocalised electrons can carry electrical charge / current through graphite
4. In diamond, each carbon atom 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)

## Related

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Source: [GradeNine](https://www.gradenine.co.uk/q/graphite-is-a-giant-covalent-structure-7a26f0ce) · Published by Druglandscape Ltd.