Given below are two statements: Statement I: The magnetic nature of the octahedral complexes [ Fe ( CN )₆]⁴⁻ and [ Fe ( H ₂ O )₆]²⁺ is not the same, despite both having the central metal ion in the +2 oxidation state. Statement II: The presence of a strong field ligand in [ Fe ( CN )₆]⁴⁻ results in a diamagnetic complex, while the weak field ligand in [ Fe ( H ₂ O )₆]²⁺ leads to a paramagnetic complex. In the light o

Step-by-step solution

In [ Fe ( CN )₆]⁴⁻ , the oxidation state of Fe is +2 . The electronic configuration of Fe ²⁺ is 3d^6 . Since CN ⁻ is a strong field ligand, it causes pairing of electrons, resulting in a t_ 2g ^6 e_g^0 configuration with zero unpaired electrons. Hence, the complex is diamagnetic. In [ Fe ( H ₂ O )₆]²⁺ , the oxidation state of Fe is also +2 with a 3d^6 configuration. However, H ₂ O is a weak field ligand and does not cause pairing. The configuration is t_ 2g ^4 e_g^2 with four unpaired electrons. Hence, the complex