Account for the following:
(i) is a stronger base than
(ii) Sulphur has a greater tendency for catenation than oxygen.
(iii) Bond dissociation energy of is less than that of
(i) Since both P and N contain lone pairs of electrons but due to small size and high electronegativity of Nitrogen in the electron density is much higher than therefore it can easily donate electrons and acts as strong Lewis base than
(ii) The greater catenation tendency of sulphur is due to two reasons :
(a) The lone pair of electrons feels more repulsion in O-O bond than S-S bond due to its small size and thus S-S forms strong bond.
(b) As the size of atom increases down the group from O-PO, the strength of bond increases and therefore catenation tendency also increases.
(iii) Due to smaller size of F than Cl as a result of which electron-electron repulsions between the lone pairs of electrons are very large than that of Cl, hence bond dissociation energy of is less than that of