[Co(NH$_3$)$_6$]$^{3+}$
-Oxidation state of Co: $+3$
-Electronic configuration of Co$^{3+}$: $3d^6$
-NH$_3$ is a strong field ligand, causing pairing of electrons in the $t_{2g}$ orbitals.
-Distribution: $t_{2g}^6 e_g^0$
-Unpaired electrons: 0
[NiCl$_4$]$^{2-}$
-Oxidation state of Ni: $+2$
-Electronic configuration of Ni$^{2+}$: $3d^8$
-Cl$^-$ is a weak field ligand, causing no pairing of electrons.
-Distribution: $e_g^2 t_{2g}^6$
-Unpaired electrons: 2
Total unpaired electrons: $0 + 2 = 2$
Match List - I with List - II:
List - I:
(A) \([ \text{MnBr}_4]^{2-}\)
(B) \([ \text{FeF}_6]^{3-}\)
(C) \([ \text{Co(C}_2\text{O}_4)_3]^{3-}\)
(D) \([ \text{Ni(CO)}_4]\)
List - II:
(I) d²sp³ diamagnetic
(II) sp²d² paramagnetic
(III) sp³ diamagnetic
(IV) sp³ paramagnetic