The magnetic moment of potassium salt of [Fe(CN)6]3– is 2.3 µB. Choose the correct statement from the following :
The increase in magnetic moment because of spin-orbit coupling
K3[Fe(CN)6] contains Fe(III), a d5 ion. Cyanide is a strong-field ligand, so the complex is low spin with the configuration t2g5, leaving exactly one unpaired electron.
Step 1 — Spin-only moment for one unpaired electron: \(\mu_{s} = \sqrt{n(n+2)} = \sqrt{1 \times 3} = 1.73\ \mu_B\). Step 2 — The observed value, 2.3 µB, is clearly larger. The ground term of a low-spin t2g5 ion is 2T2g; a T ground term retains unquenched orbital angular momentum, and spin-orbit coupling mixes this orbital contribution into the moment, raising it above the spin-only figure.
The spin-only value of one unpaired electron is 1.73 µB, not 2.3 µB, so the moment is not a pure spin-only value. Spin-only moments are fixed by a whole number of unpaired electrons, so a value lying between one and two unpaired electrons has no meaning. Ferromagnetic coupling would need cooperative interaction between neighbouring paramagnetic centres, which does not operate in this magnetically dilute salt; the excess comes from the single ion itself.
The increase in magnetic moment because of spin-orbit coupling option is correct.
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