Explain why graphite is:• a good electrical conductor• soft and slippery.You should answer in terms of structure and bonding.[6 marks]

1. Graphite is a good electrical conductor: Graphite has a unique structure where each carbon atom is covalently bonded to three other carbon atoms. This forms layers of hexagonal structures. The fourth electron of each carbon atom is not used in bonding and is free to move. These delocalized electrons can carry an electrical charge throughout the structure, making graphite a good conductor of electricity.

2. Graphite is soft and slippery: The covalent bonds within each layer of graphite are strong, but the forces between the layers (known as Van der Waals forces) are weak. This means the layers can slide over each other easily, making graphite soft and slippery. This is why graphite is used in pencils and as a lubricant.

In terms of bonding, graphite is made up of only carbon atoms, which form covalent bonds with each other. The delocalized electrons, which are free to move throughout the structure, also contribute to graphite's properties.