Question

Calculate the Oxidation number of $Fe$ in the compound.
$\left[Fe\left(No\right){\left(H_{2}O\right)}_5\right]{SO}_4$

• A. 3
• B. 2
• C. 1
• D. 0

Answer 1

The correct option is A 3

Let the oxidation number of Fe in the given compound $\left[Fe\right(No\left)\right(H_{2}O{)}_5]S{O}_4$ be x

As it dissociated into ions then we get, $\left[Fe\right(No\left)\right(H_{2}O{)}_5{]}^{2+}$ and $S{O}_4^{2-}$

We know No exists as $N{o}^{-}$ and hence oxidation state of Fe is,

$x-1=+2⟹x=+3$