Answer:
(i)\[HN{{O}_{3}}\]: Oxidation number of N is \[HN{{O}_{3}}=+5\]
Maximum oxidation number of N = + 5
Minimum oxidation number of N = -3
Since the oxidation number of N in \[HN{{O}_{3}}\]is maximum (+5), therefore, it can only decrease by accepting electrons. Hence, \[HN{{O}_{3}}\] acts only as an oxidising agent.
(ii)\[HN{{O}_{2}}\]: Oxidation number of N in \[HN{{O}_{2}}=+3\]
Maximum oxidation number of N = + 5
Minimum oxidation number of N = - 3
Thus, the oxidation number of N can either increase by losing electrons or can decrease its O.N by accepting electrons. Therefore, \[HN{{O}_{2}}\] acts both as an oxidising as well as a reducing agent.
You need to login to perform this action.
You will be redirected in
3 sec