Give reasons : (i) `SO_(2)` is reducing while `TeO_(2)` is an oxidizing agent.
(ii) Nitrogen does not form pentahalide.
(iii) ICl is more reactive than `I_(2)`.

Explanation

(i) + 6 oxidation state of S is more stable than +4. Hence, `SO_(2)` act as reducing agent. Since stability of +6 oxidation decreases from S to Te. Hence, reducing character of dioxide decreases while oxidising character increases. Thus, `TeO_(2)` acts as an oxidising agent.
(ii) Nitrogen does not form Pentahalides due to the absence of empty d-orbital.
(iii) ICl is more reactive than `I_(2)` because the over lapping of orbitals of two dissimilar atoms is less effective than the overlapping of orbitals of similar atoms. Hence, I-Cl bond is weaker and more reactive.