Which one of the following arrangements does not give the correct picture of the trends indicated against it ?

Options

A. `F_(2) gt Cl_(2) gt Br_(2) gt I_(2)` Oxidising power
B. `F_(2), Cl_(2) gt Br_(2) gt I_(2)` Electron gain enthaply
C. `F_(2) gt Cl_(2) gt Br_(2) gt I_(2)`
D. `F_(2) gt Cl_(2) gt Br_(2) gt I_(2)` Electronegtivity

Answer

C

Explanation

Generally as the size of the atom increases bond dissociation energy decreases, so in halogens `I_(2)` have lowest bond dissociation energy, but the bond dissocitation energy of chlorine is higher than that of fluorine because in fluorine there is a greater repulsion between non-bonding electrons `(2p)`. Hence, the order of bond dissociation energy is
`{:(,Cl_(2),gt,F_(2),gt,Br_(2),gt,I_(2)),(underset("energy" (kJ//mol))("Bond dissociation"),243,,153,,193,,151):}`