Explain the following :
(a) The electron gain enthalpy with negative sign for fluorine is less than for chlorine, still fluorine is a stronger oxidising agent than chlorine.
(b) `XeF_(2)` is linear molecule without a bend.
(c) `NCl_(3)` is an endothermic compound while `NF_(3)` is an exothermic one.

Explanation

(a) The electron gain enthalpy of flurine is less negative than of chlorine due to the samll size of F and the election electron repulsion in the small 2p subshell of F learge due to that incoming e-is not accepted with the same ease. But the bond dissociation enthalpy of `F_(2)` is less than the of `Cl_(2)` due to small size, lone pairs of F-atons repel the bond pair hence bond dissociates easily. Hence the electrode potential of `F_(2)(+2.87 V)` is higher than that of `Cl_(2)(+1.36 V)`
(b) Since there are two Xe-F covalent bonds and 3 lone pairs -in `XeF_(2)`. According to VSEPR they. the shape of ` XeF_(2)` is linear
(c) Because bond energy of `F_(2)` is lower than `Cl_(2) ` and N-F bond is smaller and stronger than N-Cl bond.