• In graphite each of carbon atom, shown in grey balls ..are arranged in hexagonal rings. These hexagonal rings are weakly attracted by weak Vander Waals forces, which makes it slippery in nature. The carbon atom in graphite is SP2 hybridized and is bonded two three adjacent carbon atoms.
•While, the 4th Valence Electrons of graphite lies in the unhybridized - 2P orbital of each carbon atom, it loosely held and free to move in crystalline solid lattice
•As this 4th Valence Electrons of graphite is loosely held, it moves freely between the hexagonal rings. Due to presence of freely moving valence electron in between the hexagonal rings, graphite acts as a good conductor

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