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GCSE Chemistry Revision
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GCSE Chemistry revision
Graphite
Structure and bonding of carbon
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Structure of Graphite
- In graphite, each carbon atom is covalently bonded to only three other carbon atoms, forming hexagonal rings that make up large, flat sheets called layers.
- The layers in graphite are held together only by weak intermolecular forces, allowing them to slide over one another, making graphite relatively soft.
- Despite being soft, graphite still has a very high melting point because the covalent bonds within each layer are very strong.
Delocalised Electrons in Graphite
- Because each carbon atom in graphite forms only three covalent bonds, it has one spare electron that becomes delocalised, meaning it is free to move throughout the structure.
- These delocalised electrons allow graphite to conduct both electricity and heat, unlike diamond.
Comparing Diamond and Graphite
- Diamond is harder than graphite because all four of its carbon bonds are used in a rigid 3D structure, whereas graphite's layers can slide due to weak forces between them.
- Both allotropes share a very high melting point due to the strong covalent bonds present within their structures, but only graphite conducts electricity.
Introduction to Graphene and Fullerenes
- A single isolated layer of graphite is known as graphene, which is an incredibly thin and strong material.
- Scientists can use graphene layers to construct other structures such as spheres and tubes, which are collectively known as fullerenes.