Why graphite is a conductor but not a diamond?

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Solution

Graphite:
Graphite is a crystalline allotropic form of carbon.
It is a soft black lustrous form of carbon that conducts electricity.
Graphite is a conductor but not diamond because:
In graphite, each carbon atom is linked to three carbon atoms via a $C - C$ covalent bond. The fourth electron is delocalized so it is mobile and can conduct electricity.
But diamonds have no free electrons because each carbon is four other carbon atoms covalently bonded in a tetrahedral manner.
So, it has been said that diamonds are bad conductors of electricity.

Hence, graphite is a conductor but diamond is a bad conductor.

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Similar questions

Q. (a) What is graphite? Of what substance is graphite made?
(b) Describe the structure of graphite with the help of a labelled diagram.
(c) Why is graphite a good conductor of electricity but diamond is a non-conductor of electricity?
(d) State any two uses of graphite.

(a) What is buckminsterfullerene? How is it related to diamond and graphite?
(b) Why is diamond used for making cutting tools (like glass cutters) but graphite is not?
(c) Why is graphite used for making dry cell electrodes but diamond is not?

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(a) Why is graphite a good conductor of electricity but not diamond ?

(b) Why is diamond very hard ?

(d) What impurity is present in black diamond ?

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