Graphite

• Graphite exists as a giant covalent structure in which each atom is carbon atom is bonded to just three other carbon atoms.
• In graphite, there is one electron in the outer shell which is not involved in bonding, so this becomes delocalised. Instead, the dilocalised electrons in graphite is free to move through the structure so graphite conducts electricity even though it's not metal.
• Graphite has a layered structure. The atoms in each layer form interlocking hexagons like the knots in Chicken wire. The many strong covalent bonds in the layers give graphite a very high melting point. However, the forces between each layer a week so layers can slide over each other easily. This is why graphite is slippery and some of the graphite tip in a pencil rubs off on paper.