With respect to graphite and diamond, which of the statement(s) given below is/are correct?
With respect to graphite and diamond, which of the statement(s) given below is/are correct?
The correct options are
B Graphite has a higher electrical conductivity than diamond
D Graphite has a higher C – C bond order than diamond
Graphite is soft and is used as a lubricant. It is a poor thermal conductor whereas diamond is an excellent thermal conductor. In graphite, the structure is a layer of carbon atoms with sp2 hybridization. It has free delocalized electrons throughout the layer and this is why it is conducting. In diamond, there are no free electrons. Each carbon is sp3 hybridized and is attached to four other carbon atoms – giving rise to a hard, rigid crystalline structure. Because of the delocalization of electrons in graphite, the bond order is
4 bonds with 3 carbon atoms = 4 / 3 = 1.33
In diamond, the bond order is 4 bonds with 4 carbons = 4/4 = 1
B
Graphite has a higher electrical conductivity than diamond
D
Graphite has a higher C – C bond order than diamond
Graphite is soft and is used as a lubricant. It is a poor thermal conductor whereas diamond is an excellent thermal conductor. In graphite, the structure is a layer of carbon atoms with sp2 hybridization. It has free delocalized electrons throughout the layer and this is why it is conducting. In diamond, there are no free electrons. Each carbon is sp3 hybridized and is attached to four other carbon atoms – giving rise to a hard, rigid crystalline structure. Because of the delocalization of electrons in graphite, the bond order is
4 bonds with 3 carbon atoms = 4 / 3 = 1.33
In diamond, the bond order is 4 bonds with 4 carbons = 4/4 = 1
