|
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
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) Density of diamond is 3.5 g/cm3. |
(iii) Density of graphite is 1.9 to 2.3 g/cm3 . |
| (iv) Diamond is a bad conductor of electricity as it does not have free electrons. |
(iv) Inside each layer of graphite, free electrons move continuously within the entire layer. Hence, graphite is a good conductor of electricity. |
