Graphite has layer structure. Each layer is a planar sheet, composed of hexagonal rings of carbon atoms, with 3 electrons of each atom involved in single bonds with three adjacent atoms of hexagonal ring. The extra electron makes a very weak bond with the adjacent layer. The inter-layer distance can be easily changed. This makes graphite very soft.
Graphite is used as a lubricant due to its slippery nature.
The layers in graphite can slide over each other because the forces between them are weak
Due to its loosely intact carbon atoms or free electrons, they can move around easily from one place to another, making graphite a good conductor of electricity.
