Based on Crystal Field theory, match the Complex ions listed in Column I with the electronic configuration in the d orbitals of the central metal ion listed in Column II.
Let's analyze each complex ion to determine the correct electronic configuration based on Crystal Field Theory: (A) [Mn(CN)6]4− Mn in +2 oxidation state, so its electronic configuration is 3d5. CN−is a strong field ligand, causing a large splitting of the d orbitals. Therefore, all five electrons will occupy the lower energy t2g orbitals, leading to the configuration t2g5, which corresponds to (R). (B) [Co(H2O)6]2+ Co in +2 oxidation state, its electronic configuration is 3d7. H2O is a weak field ligand, resulting in a smaller splitting of the d orbitals. Therefore, the electronic configuration will be t2g5eg2, which corresponds to (S). (C) [Fe(H2O)6]2+ Fe in +2 oxidation state, its electronic configuration is 3d6. H2O is a weak field ligand, leading to a smaller splitting of the d orbitals. Therefore, the electronic configuration will be t2g4eg2, which corresponds to (Q). (D) [MnCl4]2− Mn in +2 oxidation state, its electronic configuration is 3d5. Cl−is a weak field ligand. The complex is tetrahedral, which results in a different splitting pattern than octahedral complexes. In a tetrahedral complex, the eg orbitals are lower in energy than the t2g orbitals. Therefore, the electronic configuration will be eg2t2g3, which corresponds to (P). Therefore, the correct matching is: ‌A=R ‌B=S ‌C=Q ‌D=P So the final answer is Option B.