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. No. Complex No. d orbital configuration of central metal ion A [Mn(CN)₆]⁴⁻ P e_g^2 t_ 2g ^3 B [Co(H₂O)₆]²⁺ Q t_ 2g ^4 e_g^2 C [Fe(H₂O)₆]²⁺ R t_ 2g ^5 D [MnCl₄]²⁻ S t_ 2g ^5 e_g^2

Step-by-step solution

For [Mn(CN)₆ ]⁴⁻ , the oxidation state of Mn is +2 . The electronic configuration of Mn²⁺ is 3d^5 . Since CN⁻ is a strong field ligand, pairing occurs. The configuration is t_ 2g ^5 e_g^0 , which is represented by (R). For [Co(H₂O)₆ ]²⁺ , the oxidation state of Co is +2 . The electronic configuration of Co²⁺ is 3d^7 . Since H₂O is a weak field ligand, the configuration is t_ 2g ^5 e_g^2 , which is represented by (S). For [Fe(H₂O)₆ ]²⁺ , the oxidation state of Fe is +2 . The electronic configuration of Fe²⁺ is 3d^6