With respect to diamond and graphite, which of the statement(s) given below is/are correct?
With respect to diamond and graphite, which of the statement(s) given below is/are correct?
The correct options are
B Graphite has higher electrical conductivity than diamond
D Graphite has higher C - C bond order than diamond
Diamond has a three-dimensional network of strong covalent bonds. This makes it extremely hard.
In diamond, all four valence electrons are involved in covalent bonding and are not free to conduct electricity. This makes diamond a bad conductor of electricity. On the other hand, in graphite, each carbon atom is bonded to only three other carbon atoms. Thus, each carbon atoms utilizes only three valence electrons for forming covalent bonds, the fourth valence electron is mobile, and hence is responsible for conducting electricity. Hence, graphite is a good conductor of electricity.
B
Graphite has higher electrical conductivity than diamond
D
Graphite has higher C - C bond order than diamond
Diamond has a three-dimensional network of strong covalent bonds. This makes it extremely hard.
In diamond, all four valence electrons are involved in covalent bonding and are not free to conduct electricity. This makes diamond a bad conductor of electricity. On the other hand, in graphite, each carbon atom is bonded to only three other carbon atoms. Thus, each carbon atoms utilizes only three valence electrons for forming covalent bonds, the fourth valence electron is mobile, and hence is responsible for conducting electricity. Hence, graphite is a good conductor of electricity.
