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(C) The magnetic moment (spin only) is given by the formula $\mu = \sqrt{n(n+2)} 	ext{ BM}$,where $n$ is the number of unpaired electrons.For $[Cr(H_

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$[Cr(H_2O)_6]^{2+}$ and $[Fe(H_2O)_6]^{2+}$

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(C) The magnetic moment (spin only) is given by the formula $\mu = \sqrt{n(n+2)} 	ext{ BM}$,where $n$ is the number of unpaired electrons.For $[Cr(H_2O)_6]^{2+}$,$Cr^{2+}$ is $d^4$. Since $H_2O$ is a weak field ligand,the configuration is $t_{2g}^3 e_g^1$,giving $n = 4$.For $[Fe(H_2O)_6]^{2+}$,$Fe^{2+}$ is $d^6$. Since $H_2O$ is a weak field ligand,the configuration is $t_{2g}^4 e_g^2$,giving $n = 4$.Since both complexes have $n = 4$ unpaired electrons,they have the same magnetic moment.Thus,the correct pair is $[Cr(H_2O)_6]^{2+}$ and $[Fe(H_2O)_6]^{2+}$.

The pair in which both the species have the same magnetic moment (spin only) is :

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