GCSE Chemistry · AQA 8462 · Topic 4.2.3
Structure and bonding of carbon
Key points
- Diamond: each carbon is bonded to four others in a giant covalent structure. It is very hard, has a very high melting point and does not conduct electricity.
- Graphite: each carbon is bonded to three others in hexagonal layers with weak forces between layers, so it is soft and slippery. One electron per atom is delocalised, so graphite conducts electricity and heat.
- Graphene is a single layer of graphite, one atom thick. It is very strong, light and conducts well, so it is useful in electronics and composites.
- Fullerenes are hollow carbon molecules based on rings of five, six or seven carbon atoms. The first found was buckminsterfullerene, , which is spherical.
- Carbon nanotubes are cylindrical fullerenes with a very high length to diameter ratio. They are strong and conduct, so they are used in nanotechnology, electronics and to reinforce materials.
- Fullerenes can also be used to deliver drugs in the body, as lubricants and as catalysts because of their large surface area.
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Carbon forms more different structures than any other element. All its forms are made only of carbon atoms, but the way the atoms are bonded gives very different properties.
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