Which of the following bonds require the largest amount of bond energy to dissociate the atoms concerned ?

Options

A. `H H` bon in `H_2`
B. `C - C` bond in `CH_4`
C. `N -= N` bond in `N_2`
D. `O - O` bond in `O_2`

Answer

C

Explanation

Hydrogen atom has only 1s orbital which overlap with another 1s orbital of H atom to form `H_2` molecule.
There is sufficient overlap between spherical orbitals. Also there is no repulsion due to other electrons as it has only one electron which is being used in the `sigma` bonding. So the bond is very strong.
In the formation of `N_2` molecule, p orbitals of N atom overlap axially (to form a `sigma` bond) and laterally (to form two `pi`- bonds). N atom experience repulsion due to other electrons which do not take part in bonding. But the combined effect of 3 bonds overcome the repulsion effect, so the bond dissociation energy of `N -= N ` is more than `H - H`.