(a) Draw the molecular structures of the following compounds :
(i) `N_(2)O_(5) " "` (ii) `XeOF_(4)`
(b) Explain the following observations :
(i) Sulphur has a greater tendency for catenation than oxygen.
(ii) ICI is more reactive than `I_(2)`.
(iii) Despite lower value of its electron gain enthalpy with negative sign, fluorine `(F_(2))` is a stronger oxidizing agent than `Cl_(2)`.

Explanation

(b) (i) Due to small size of oxygen, lone pair of electron on oxygen atom repel the bond pair of O-O bond to greater extent than the lone pairs of electrons on the S atom is S-S bond .
Hence S-Sbond is much stronger and hence much stronger tendency of for catenation than O
(ii) ICI is more reactive than `I_(2)` because `I-Cl` bond is weaker than I-I bond because of less effective overlapping between orbitals of dissimilar atoms than those between similar atoms Consequently , ICI breaks easily to form halogen atoms which readily bring about the reactions.
(iii) It is due to
Low enthalpy of dissociation of F-F bond .
High hydration enthalpy of `F^(-)`.