The major binding force in diamond is
A. Ionic bond
B. Covalent bond
C. Dipole-dipole interaction
D. Induced dipole interaction

Hint:Diamond is considered as one of hardest substances on the earth. This is due to their bonding structure. Also, diamond is the solid form of carbon where its atoms are arranged in a crystal form.

Complete answer:
As we said, diamond is the allotropes of carbon. Apart from diamond, graphite and fullerene are also some other allotropes of carbon. These are minerals consisting of carbon but show properties different from carbon.
Since we said it has a major component of carbon, carbon has a valency of four which means it has 4 valence electrons in its outer shell. In diamond these four valence electrons possess a strong chemical bond with the other carbon atoms present in it. They have the hybridization of $s{p^3}$, also the bond lengths of carbon-carbon atoms are equal. Hence we can say that diamond from a three dimensional network of covalent bonds.
Due to its strong covalent bonding it has a very high melting point of about 3843K and a high density also. Apart from that they are known to be poor conductors of electricity since its valence electrons get involved in C-C sigma covalent bonds. Hence we can say that they are localised and are not free to conduct electricity.

Therefore, option B is correct.

Note:
Like carbon, graphite is also a allotropes of carbon with stable bonds with that of other three carbon atoms. The carbon atoms present in graphite have a $s{p^2}$ hybridisation and are directed in the same plane thus forming hexagonal rings. They have low electrical conductivity and a low density.