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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

Answers (1)

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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 values of \mu are 1.732, 2.83, 3.87, 4.899, and 5.92, respectively.

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