The oxidation state of Fe in browns ring complex $\left[Fe\right(H_{2}O{)}_{5}N{O}^{+}]S{O}_4$ is:

The correct option is A 1

Let oxidation state of Fe = $x$

$x+5\left(0\right)+1+(-2)=0$

$x$ + 1 - 2= 0

$x$ = 1

The oxidation state of Fe in browns ring complex $\left[Fe\right(H_{2}O\left)5N{O}^{+}\right]S{O}_4$ is +1 as oxidation of NO is +1 and that of $S{O}_4^{-2}$ is -2.