What is the structure of graphite?

Graphite is composed of layers of carbon atoms arranged in a hexagonal lattice.

Graphite, a naturally occurring form of crystalline carbon, is a unique material due to its structure. It is composed of carbon atoms, which are arranged in a hexagonal lattice or honeycomb pattern. This pattern forms layers, or sheets, that are loosely bonded together by weak Van der Waals forces.

Each carbon atom in graphite is covalently bonded to three other carbon atoms. This leaves one electron free, which can move along the layers, making graphite a good conductor of electricity. The covalent bonds within the layers are very strong, but the bonds between the layers are weak. This means the layers can slide over each other easily, which is why graphite is slippery and is used as a lubricant.

The layers in graphite are spaced further apart compared to other forms of carbon, like diamond. This makes graphite less dense and softer. The structure of graphite also makes it highly resistant to heat and most chemicals, which is why it's used in things like pencils, batteries, and as a moderator in nuclear reactors.

In summary, the structure of graphite is unique and gives it a range of useful properties. It's composed of layers of carbon atoms arranged in a hexagonal lattice, with weak bonds between the layers. This structure makes graphite a good conductor of electricity, slippery, less dense, soft, and resistant to heat and most chemicals.