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

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(B) Paramagnetic behaviour is directly proportional to the number of unpaired electrons present in the metal ion.$H_2O$ is a weak field ligand,so it d

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

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(B) Paramagnetic behaviour is directly proportional to the number of unpaired electrons present in the metal ion.$H_2O$ is a weak field ligand,so it does not cause pairing of electrons in these $3d$ metal ions.$1$. For $[Cr(H_2O)_6]^{2+}$: $Cr^{2+}$ is $3d^4$,having $4$ unpaired electrons.$2$. For $[Mn(H_2O)_6]^{2+}$: $Mn^{2+}$ is $3d^5$,having $5$ unpaired electrons.$3$. For $[Fe(H_2O)_6]^{2+}$: $Fe^{2+}$ is $3d^6$,having $4$ unpaired electrons.$4$. For $[Ni(H_2O)_6]^{2+}$: $Ni^{2+}$ is $3d^8$,having $2$ unpaired electrons.Since $[Ni(H_2O)_6]^{2+}$ has the minimum number of unpaired electrons $(2)$,it exhibits the minimum paramagnetic behaviour.

The $d$ electron 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 behaviour?
(At. No. $Cr = 24, Mn = 25, Fe = 26, Ni = 28$)

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The $d$ electron 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 behaviour?(At. No. $Cr = 24, Mn = 25, Fe = 26, Ni = 28$)