The oxidation state of nitrogen varies from:

The correct option is A $-3$ to $+5$
Nitrogen ($2s^{2}2p^3$) can obtain inert gas configuration by either gaining 3 electrons ($2s^{2}2p^6$) thereby attaining oxidation state of -3, or losing all the 5 valence shell electrons and thus attaining oxidation state of +5.
Nitrogen oxidation state varies from $-3$ to $+5$ . It posseses $-3$ oxidation state in ammonia $\left(N{H}_3\right)$ and $+5$ oxidation state in dinitrogen pentoxide $\left(N_2{O}_5\right)$. Other oxidation states (between -3 and +5) are also possible and hence they can act as both an oxidising and reducing agents.