Draw the structure of : `{:((i)BrF_(3),(ii)XeOF_(4)):}`
(b) Explain giving reason in each case :
(i) Why `H_(2)` Te is more acidic than `H_(2)S`?
(ii) Why are halogens strong oxidising agents ?
(iii) Why does nitrogen show catenation tendentcy less than phosphorus ?

Explanation

(i) As the size of element increase down the group bond length increases and hence, bond dissociation energy decreases. Hence H-S bond dissociation energy is higher than that of H- Te bond dissociation energy and hence H- S bond breakes less easily than H- Te bond. Hence `H_(2)` Te is strong acid than `H_(2)S.`
(ii) See Q. 25, (or) (b) (i) Delhi Board (Comptt.) 2016.
(iii) N-N single bond is weaker than P - P single bond because Nitrogen has smaller size, due to that lone pair of electrons on two N-atom repel the bond of N-N bond and hence, it makes N-N single ond weakeer than P-P bond in which the lone pair of electrons fo not replel the bond pair electrons because bigger size of phosphorus. Consequently, Nitrogen shows the little tendency for catenation than phosphorous.