(a)Draw the molecule structure of the following compounds :
(i)`N_(2)O_(5)`
(ii)`XeOF_(4)`
(b)Despite lower value of its electron gain enthalpy with negative sign, fluorine `(F_(2))` is a stronger oxidising agent than `Cl_(2)`.

Answer

(a)(i)`(##RES_INO_CHM_XII_V02_C03_E01_186_A01##)`
(b)(i)It is because sulphur forms single bonds whereas oxygen forms double bond.Secondly S-S bond is stronger than O-O bond because there is more repulsion between electrons of oxygen as it is smaller in size than sulphur.
(ii)It is because ICl is more polar and has less effective overlapping than I_(2).
(iii)It is due to higher standard reduction potential of `F_(2)` which is due to low bond dissociation energy of F-F bond due to repulsion among small size F atoms, high electron gain enthalpy and highest hydration enthalpy.