Identify the homoleptic complexes with odd number of $d$ electrons in the central metal :

(A) $\left[\mathrm{FeO}_4\right]^{2-}$

(B) $\left[\mathrm{Fe}(\mathrm{CN})_6\right]^{3-}$

(C) $\left[\mathrm{Fe}(\mathrm{CN})_5 \mathrm{NO}\right]^{2-}$

(D) $\left[\mathrm{CoCl}_4\right]^{2-}$

(E) $\left[\mathrm{Co}\left(\mathrm{H}_2 \mathrm{O}\right)_3 \mathrm{~F}_3\right]$

Choose the correct answer from the options given below :

<p>Homoleptic complexes are complexes with identical ligands attached to the central metal atom.</p> <p>(A) ${[Fe{O_4}]^{2 - }}$ - Homdeptic</p> <p>Central metal : Fe</p> <p>IN this complex, Fe is in +6 oxidation state.</p> <p>{oxidation state : $x + 4( - 2) = - 2$</p> <p>$x - 8 = - 2$</p> <p>$x = - 2 + 6 = + 6$</p> <p>Configuration of $Fe - {d^6}{s^2}$</p> <p>Configuration of $Fe( + 6) - c{l^2}$</p> <p>Iron has even number of d electrons. So, it is not correct.</p> <p>(B) ${[Fe{(N)_6}]^{3 - }}$ - Homoleptic</p> <p>Central metal : Fe</p> <p>In this complex, the oxidation state of Fe is +3</p> <p>Oxidation state :</p> <p>$x + 6( - 1) - 3$</p> <p>$x - 6 = - 3$</p> <p>$x = - 3 + 6 = + 3$</p> <p>Configuration of $Fe - {d^6}{s^2}$</p> <p>Configuration of $Fe( + 3) - {d^5}$</p> <p>Iron has odd number of d electrons.</p> <p>So, it is correct.</p> <p>(C) ${[Fe{(CN)_5}NO]^{2 - }}$ - Not homoleptic</p> <p>This complex has different type of ligands.</p> <p>${[CoC{l_4}]^{2 - }}$ - Homoleptic</p> <p>Central metal - Co</p> <p>In this complex, the oxidation state of Co is +2</p> <p>Oxidation state:</p> <p>$x + 4( - 1) = - 2$</p> <p>$x - 4 = - 2$</p> <p>$x = - 2 + 4 = + 2$</p> <p>Configuration of $Co - {d^7}{s^2}$</p> <p>Configuration of $Co( + 2) - {d^7}$</p> <p>Cobalt has odd number of d electrons.</p> <p>So, it is correct.</p> <p>(E) $[Co{({H_2}O)_3}{F_3}]$ - Not homoleptic,</p> <p>It has different type of ligands.</p> <p>Complexes B and D are homoleptic complexes with odd number of d electrons in the central metal. So, correct answer is</p> <p>(B) and (D) only.</p>