What is the structural difference between diamond and graphite?
What is the structural difference between diamond and graphite?
There are many structural differences between diamond and graphite, due to which they show different physical properties.
In diamond, each C atom is bonded with 4 other C atoms i.e. each carbon atom is tetravalent. While in graphite, each C atom is bonded to 3 other C atoms i.e. each carbon atom is trivalent.
In diamond there is 3-D cross linked network of C atoms, with shape of every set of C atom is tetrahedral while in graphite the shape of the structure is hexagonal, with every side of hexagon representing a C atom.
In diamond every layer of C atom is bonded with strong sigma bonds, while in graphite different layers of C atoms are bonded with weak Van-der-Waal forces.
Diamond doesn’t have any valence electron left after bonding with other 4 C atoms, while in graphite each C atom is bonded with 3 other C atoms, so it has a mobile electron due to which it conduct electricity and heat.
In diamond every C atom is sp3 hybridised, while in graphite every C atom is sp2 hybridised.
There are many structural differences between diamond and graphite, due to which they show different physical properties.
In diamond, each C atom is bonded with 4 other C atoms i.e. each carbon atom is tetravalent. While in graphite, each C atom is bonded to 3 other C atoms i.e. each carbon atom is trivalent.
In diamond there is 3-D cross linked network of C atoms, with shape of every set of C atom is tetrahedral while in graphite the shape of the structure is hexagonal, with every side of hexagon representing a C atom.
In diamond every layer of C atom is bonded with strong sigma bonds, while in graphite different layers of C atoms are bonded with weak Van-der-Waal forces.
Diamond doesn’t have any valence electron left after bonding with other 4 C atoms, while in graphite each C atom is bonded with 3 other C atoms, so it has a mobile electron due to which it conduct electricity and heat.
In diamond every C atom is sp3 hybridised, while in graphite every C atom is sp2 hybridised.
