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

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(C) The paramagnetic behaviour depends on the number of unpaired electrons $(n)$.$1$. For $[Cr(H_2O)_6]^{2+}$,$Cr^{2+}$ is $d^4$. In a weak field liga

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

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(C) The paramagnetic behaviour depends on the number of unpaired electrons $(n)$.$1$. For $[Cr(H_2O)_6]^{2+}$,$Cr^{2+}$ is $d^4$. In a weak field ligand like $H_2O$,$n = 4$.$2$. For $[Mn(H_2O)_6]^{2+}$,$Mn^{2+}$ is $d^5$. In a weak field ligand like $H_2O$,$n = 5$.$3$. For $[Fe(H_2O)_6]^{2+}$,$Fe^{2+}$ is $d^6$. In a weak field ligand like $H_2O$,$n = 4$.$4$. For $[Co(H_2O)_6]^{2+}$,$Co^{2+}$ is $d^7$. In a weak field ligand like $H_2O$,$n = 3$.Since $[Co(H_2O)_6]^{2+}$ has the minimum number of unpaired electrons $(n = 3)$,it exhibits the minimum paramagnetic behaviour.The magnetic moment is given by $\mu = \sqrt{n(n+2)} 	ext{ BM}$.

Complex	Magnetic Moment $(BM)$
$K_4[Mn(CN)_6]$	$2.2$
$[Fe(H_2O)_6]^{2+}$	$5.3$
$K_2[MnCl_4]$	$5.9$

The $d-$electron configurations of $Cr^{2+}, Mn^{2+}, Fe^{2+}$ and $Co^{2+}$ are $d^4, d^5, d^6$ and $d^7$ respectively. Which one of the following will exhibit minimum paramagnetic behaviour?
(At. nos. $Cr = 24, Mn = 25, Fe = 26, Co = 27$)

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Complex Magnetic Moment $(BM)$

$K_4[Mn(CN)_6]$ $2.2$

$[Fe(H_2O)_6]^{2+}$ $5.3$

$K_2[MnCl_4]$ $5.9$

Select the correct statement about the given square planar complex.

The pair not correctly matched is:

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The $d-$electron configurations of $Cr^{2+}, Mn^{2+}, Fe^{2+}$ and $Co^{2+}$ are $d^4, d^5, d^6$ and $d^7$ respectively. Which one of the following will exhibit minimum paramagnetic behaviour?(At. nos. $Cr = 24, Mn = 25, Fe = 26, Co = 27$)