Explain the difference between Diamond and graphite.

Open in App

Solution

Diamond

Graphite

(i) Diamond is a brilliant, hard, and crystalline allotrope of carbon.

(i) Graphite is a black, soft, brittle, and slippery crystalline allotrope of carbon.

(ii) In diamonds, every carbon atom is bonded to four neighbouring atoms by covalent bonds forming a tetragonal three-dimensional structure which makes it very hard.

(ii) In graphite, every carbon atom is bonded to three other carbon atoms by covalent bonds in such a way that a hexagonal layered structure is formed. A graphite crystal is made of many such layers of carbon atoms. These layers slip over each other on applying pressure.

(iii) Diamond is a bad conductor of electricity as it does not have free electrons.

(iii) Inside each layer of graphite, free electrons move continuously within the entire layer. Hence, graphite is a good conductor of electricity.

Suggest Corrections

Similar questions

Explain the difference between Diamond and graphite.

Write three differences between graphite and diamond.

Explain the difference in properties of diamond and graphite on the basis of their structures.

Join BYJU'S Learning Program

Diamond	Graphite
(i) Diamond is a brilliant, hard, and crystalline allotrope of carbon.	(i) Graphite is a black, soft, brittle, and slippery crystalline allotrope of carbon.
(ii) In diamonds, every carbon atom is bonded to four neighbouring atoms by covalent bonds forming a tetragonal three-dimensional structure which makes it very hard.	(ii) In graphite, every carbon atom is bonded to three other carbon atoms by covalent bonds in such a way that a hexagonal layered structure is formed. A graphite crystal is made of many such layers of carbon atoms. These layers slip over each other on applying pressure.
(iii) Diamond is a bad conductor of electricity as it does not have free electrons.	(iii) Inside each layer of graphite, free electrons move continuously within the entire layer. Hence, graphite is a good conductor of electricity.