# 8.38 What can be inferred from the magnetic moment values of the following complex species ?Example                                    Magnetic Moment (BM)$K_{4}[Mn(CN)_{6})$                                2.2$[Fe(H_{2}O)_{6}]^{2+}$                                          5.3$K_{2}[MnCl_{4}]$                                            5.9

M manish

Magnetic moment is given as - $\mu = \sqrt{n(n+2)}$
Putting the value on n = 1, 2, 3, 4, 5  (number of unpaired electrons in d-orbital)
we get the value of $\mu$ are 1.732, 2.83, 3.87, 4.899, 5.92 respectively.

$K_{4}[Mn(CN)_{6})$
By comparing with our calculation we get the values n nearest to 1. It means, in above compound d-orbital has one unpaired electron($Mn^{2+} = [d^{5}]$), which means $CN$ is astrong field ligand that cause force pairing of the electron.

$[Fe(H_{2}O)_{6}]^{2+}$
After comparing with our calculation the nearest value of n = 4. Here iron is in +2 oxidation state ($d^{6}$ configuration). So, we can say that $H_{2}O$ is a weak field ligand, which not cause any force pairing.

$K_{2}[MnCl_{4}]$
By observing we get the nearest value of n is 5. So, in this complex Manganese has $d^{5}$ configuration. So, we conclude that $Cl$  ligand does not cause any force pairing and hence it is a weak ligand.

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