The electronic configurations of Cr^{2+}, Mn^ | vedclass

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(A) Paramagnetic behavior is directly proportional to the number of unpaired electrons $(n)$.For $[Cr(H_2O)_6]^{2+}$,$Cr^{2+}$ is $3d^4$,so $n = 4$.Fo

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$[Ni(H_2O)_6]^{2+}$

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(A) Paramagnetic behavior is directly proportional to the number of unpaired electrons $(n)$.For $[Cr(H_2O)_6]^{2+}$,$Cr^{2+}$ is $3d^4$,so $n = 4$.For $[Mn(H_2O)_6]^{2+}$,$Mn^{2+}$ is $3d^5$,so $n = 5$.For $[Fe(H_2O)_6]^{2+}$,$Fe^{2+}$ is $3d^6$,so $n = 4$.For $[Ni(H_2O)_6]^{2+}$,$Ni^{2+}$ is $3d^8$,so $n = 2$.Since $[Ni(H_2O)_6]^{2+}$ has the minimum number of unpaired electrons $(n = 2)$,it exhibits the minimum paramagnetic behavior.

The electronic configurations of $Cr^{2+}, Mn^{2+}, Fe^{2+},$ and $Ni^{2+}$ are $3d^4, 3d^5, 3d^6,$ and $3d^8$ respectively. Which one of the following aqua complexes will exhibit the minimum paramagnetic behavior?

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