What can be inferred from the magnetic moment values of the following complex species? Example Magnetic Moment (BM)
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
Magnetic moment (μ) is given as μ = \(\sqrt{n(n+2)}\)
For value n = 1, μ = \(\sqrt{1(1+2)}\) = \(\sqrt{3}\) = 1.732
For value n = 2, μ = \(\sqrt{2(2+2)}\) = \(\sqrt{8}\) = 2.83
For value n = 3, μ = \(\sqrt{3(3+2)}\) = \(\sqrt{15}\) = 3.87
For value n = 4, μ = \(\sqrt{4(4+2)}\) = \(\sqrt{24}\) = 4.899
For value n = 5, μ = \(\sqrt{5(5+2)}\) = \(\sqrt{35}\) = 5.92
(i) K_{4}[Mn(CN)_{6}]
For in transition metals, the magnetic moment is calculated from the spinonly formula. Therefore,
\(\sqrt{n(n+2)}\) = 2.2
We can see from the above calculation that the given value is closest to n = 1. Also, in this complex, Mn is in the +2 oxidation state. This means that Mn has 5 electrons in the dorbital.
Hence, we can say that CN^{} is a strong field ligand that causes the pairing of electrons.
(ii) [Fe(H_{2}O)_{6}]^{2+}
\(\sqrt{n(n+2)}\) = 5.3
We can see from the above calculation that the given value is closest to n = 4. Also, in this complex, Fe is in the +2 oxidation state. This means that Fe has 6 electrons in the dorbital.
Hence, we can say that H_{2}O is a weak field ligand and does not cause the pairing of electrons.
(iii) K_{2}[MnCl_{4}]
\(\sqrt{n(n+2)}\) = 5.9
We can see from the above calculation that the given value is closest to n = 5. Also, in this complex, Mn is in the +2 oxidation state. This means that Mn has 5 electrons in the dorbital.
Hence, we can say that Cl^{} is a weak field ligand and does not cause the pairing of electrons.

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