Explain why `[Fe(H_(2)O)_(6)]^(3+)` has magnetic moment value of 5.92 BM whereas `[Fe(CN)_(6)]^(3-)` has a value of only 1.74 BM ?

Explanation

To explain why the magnetic moment value of `[Fe(H₂O)₆]^(3+)` is 5.92 BM while that of `[Fe(CN)₆]^(3-)` is only 1.74 BM, we can break down the explanation into several steps:

### Step 1: Determine the Oxidation State of Iron
For both complexes, we need to determine the oxidation state of iron (Fe).

- In `[Fe(H₂O)₆]^(3+)`, the overall charge is +3. Since water (H₂O) is a neutral ligand, the oxidation state of Fe is +3.
- In `[Fe(CN)₆]^(3-)`, the overall charge is -3. The cyanide ion (CN⁻) has a charge of -1, and since there are six cyanide ligands, the total contribution from ligands is -6. Thus, the oxidation state of Fe is +3 as well.

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