Question

What are the differences between the structures of Diamond and Graphite?

Answer 1

* Diamond is the hardest mineral known to man, Graphite is one of the softest.
* Diamond is an excellent electrical insulator, Graphite is a good conductor of electricity.
* Diamond is the ultimate abrasive, Graphite is a very good lubricant.
* Diamond is usually transparent, Graphite is opaque.
* Diamond crystallizes in the Isometric system and graphite crystallizes in the hexagonal system.
* Diamond Carbon is SP3 hybridization and in case of Graphite Carbon is SP2 hybridization

Answer 2

well i can understand the first five differences can u describe the 6th difference mentioned by u @chmvijay

Answer 3

Diamond has rigid covalent (strong bonds) in which all four electrons of the carbon atoms are bonded by sharing. This makes diamond very hard to break or shatter.
Graphite also has these bonds, although only three electrons of the carbon atoms are bonded together covalently. This allows the fourth for each atom,able to become delocalised and can move within the two dimensional hexagonal sheets (this is how the structure is created).
In contrast diamond is three dimentional.
Because of the delocalised electrons, graphite is able to conduct electricity. If you put a current (made up of fast moving electrons) through it roughly the same number will leave the structure.
Diamond cannot because there are no delcolalised electrons, they are shared between the many carbon atoms making up the covalent network.
This would also mean that graphite is a good thermal conductor because of the ability of electrons to move freely and vibrate (gain kenetic energy) and pass that onto nearby electrons as heat is passed through the structure, so eventually it turns hot.
This makes diamond a good insulator.