Question

$\left[Fe\right(H_{2}O{)}_{5}NO{]}^{2+}$ is a complex formed during the brown ring test for $N{O}_3^{-}$ ion. In this complex :

• A. There are three unpaired electrons so that its magnetic moment is 3.87 BM
• B. NO transfer its electron to $F{e}^{2+}$ so that iron as $F{e}^{(-)}$ and $NO$ as $N{O}^{+}$
• C. The colour is because of charge transfer
• D. All of the above statements are correct

Answer 1

Answer: (D)

All of the above statements are correct

In brown ring complex, iron exists in $+1$ due to transfer of one electron from $NO$ and in $+1$ oxidation state iron has 3 unpaired electrons. The color of the complex is due to the charge transfer.