# Compare the electrical conductivity of graphite and diamond, and explain the difference in terms of their structures and bonding.

> Cambridge International IGCSE Chemistry (0620) — 2.6 Giant covalent structures · Compare · 4 marks

## Mark scheme (4 marks)

1. Graphite conducts electricity but diamond does not
2. In graphite, each carbon atom forms only three covalent bonds, leaving one outer (delocalised) electron per atom
3. These delocalised electrons in graphite are free to move through the structure and carry charge
4. In diamond, every outer electron is used in four covalent bonds so there are no free/delocalised electrons to carry charge

## Key terms

- [electrical conductivity](https://www.gradenine.co.uk/glossary/electrical-conductivity)

## Related

- [Revision notes for Cambridge International IGCSE Chemistry (0620)](https://www.gradenine.co.uk/learn)
- [How to answer "Compare" questions](https://www.gradenine.co.uk/tools/command-word-cheatsheet)
- [Practice this with AI marking (free)](https://www.gradenine.co.uk/start)

---
Source: [GradeNine](https://www.gradenine.co.uk/q/compare-the-electrical-conductivity-of-graphite-31a3fb58) · Published by Druglandscape Ltd.