give any two differences between the properits of a diamnond and graphine. What causes these differences
give any two differences between the properits of a diamnond and graphine. What causes these differences
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.
All these structural differences has made diamond and graphite to show different properties. As diamond is crystalline, hard, transparent, insulator while graphite is amorphous, soft, opaque, conducts heat and electricity.
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.
All these structural differences has made diamond and graphite to show different properties. As diamond is crystalline, hard, transparent, insulator while graphite is amorphous, soft, opaque, conducts heat and electricity.
