Question

In graphite, electrons are

• A. localised on each C-atom
• B. localised on every third C-atom
• C. spread out between the structure
• D. Both (b) and (c)

Answer 1

Answer: (D)

Both (b) and (c)

Answer 2

Structure of graphite consist of a two dimensional sheet like network joined together in hexagonal rings. These layers are held together by weak van der Waals' forces. In graphite each carbon atom is bonded to three others, forming $sp^2$ hybrid bonds. The fourth electron forms a $\pi$-bond. Graphite is a conductor of electricity which is due to the fact that all the carbon bonds being not satisfied. Thus, some of the electrons are free to move through the crystal.