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 ?

Draw the structure of : {:((i)BrF_(3),(ii)XeOF_(4)):} (b) Explain giv

1.	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 ?
Answer» Solution : (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.