GCSE Combined Science (AQA)

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Graphite

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Bonding, structure, and the properties of matter Structure and bonding of carbon

Graphite

3:08 Carbon Structures and Bonding
Spec 4.2.3.2 4.2.2.1
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  • Graphite is a giant covalent structure consisting of carbon atoms.
  • Writing with a pencil involves using graphite, which is made entirely of carbon atoms.
  • Each carbon atom in graphite is bonded to three other carbon atoms.
  • Graphite forms layers of hexagonal rings with no covalent bonds between the layers.
  • The layers in graphite are held together by weak forces of attraction.
  • Graphite has a high melting point, around 4,000 degrees Celsius, due to strong covalent bonds within each layer.
  • Graphite is slippery because of weak forces of attraction between layers, allowing them to slide.
  • The sliding layers allow a pencil to draw on paper as layers of graphite slide off the tip.
  • Graphite can conduct electricity because each carbon atom is bonded to three others, leaving one unbonded electron.
  • These unbonded electrons are delocalized and free to move between layers, enabling electrical conductivity.
  • Delocalized electrons in graphite are similar to those in metals, allowing both to conduct electricity.
  • Both graphite and metals have structures containing delocalized electrons, facilitating electrical conductivity.

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