In graphite, each carbon atom forms three sigma bonds to 3 other carbon atoms forming interlocking hexagonal rings with bond angles 120°. The fourth electron is in a p orbital and p orbitals of adjacent carbon atoms are close enough to overlap and produce a cloud of delocalised electrons above and below the plane of the rings. Graphite is a solid lubricant as the layers can slide over each other easily and there are weak London forces between the layers. The lubricating properties are also helped by adsorbed gases on the surface of the carbon atoms.Graphene is a single layer of graphite.
Graphite is a giant covalent structure. It is made of hexagonally arranged carbon atoms covalently bonded together. Each carbon atom uses three of the outer electrons to form three covalent bonds with three other carbon atoms.The layers are held together by weak London forces.The spare electron is delocalised within each layer, above and below the plane of the rings. The delocalised electrons can move along the layers, so graphite is an electrical conductor.
Graphite is a giant covalent structure. It is made of hexagonally arranged carbon atoms covalently bonded together. Each carbon atom uses three of the outer electrons to form three covalent bonds with three other carbon atoms.The layers are held together by weak London forces.The spare electron is delocalised within each layer, above and below the plane of the rings. The delocalised electrons can move along the layers, so graphite is an electrical conductor.