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(D) The magnetic moment is calculated using the formula $\mu = \sqrt{n(n+2)} 	ext{ B.M.}$,where $n$ is the number of unpaired electrons.$1$. $[Cr(H_2

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

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(D) The magnetic moment is calculated using the formula $\mu = \sqrt{n(n+2)} 	ext{ B.M.}$,where $n$ is the number of unpaired electrons.$1$. $[Cr(H_2O)_6]^{2+}$: $Cr$ is in $+2$ oxidation state $(3d^4)$. It has $4$ unpaired electrons $(n=4)$.$2$. $[Fe(H_2O)_6]^{2+}$: $Fe$ is in $+2$ oxidation state $(3d^6)$. In a weak field ligand like $H_2O$,it has $4$ unpaired electrons $(n=4)$.$3$. $[Mn(H_2O)_6]^{2+}$: $Mn$ is in $+2$ oxidation state $(3d^5)$,having $5$ unpaired electrons $(n=5)$.$4$. $[CoCl_4]^{2-}$: $Co$ is in $+2$ oxidation state $(3d^7)$,having $3$ unpaired electrons $(n=3)$.Since $[Cr(H_2O)_6]^{2+}$ and $[Fe(H_2O)_6]^{2+}$ both have $4$ unpaired electrons,they have the same magnetic moment.

The pair having the same magnetic moment is $:$
[At. No.$: $ $Cr= 24, Mn= 25, Fe= 26, Co= 27$]

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The pair having the same magnetic moment is $:$[At. No.$: $ $Cr= 24, Mn= 25, Fe= 26, Co= 27$]