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SO_(2) is reducing while TeO_(2) is an oxidising agent. Give reasons. |
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Answer» Solution :Since +6 oxidation state of S is more STABLE than +4, therefore, it can readily donate electrons an hence acts as a reducing AGENT. For example, it reduces ferric to FERROUS salts. `underset("Ferric sulphate")(Fe_(2)(SO_(4))_(3)) + SO_(2) + 2H_(2)O rarr underset("Ferrous sulphate")(2FeSO_(4)) + 2H_(2)SO_(4)` Since due to inert pair effect, the stability of +6 oxidation state DECREASES while the stability of +4 and +2 oxidation states increases down the group. Thus, +4 oxidation state of `TiO_(2)` is less stable than its +2 oxidation state. As a result, it accepts electrons and thus acts an oxidising agent. |
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