Based on Valence Bond Theory, match the complexes listed in Column I with the number of unpaired electrons on the central metal ion, given in Column II
| No. | Complex ions | No. | Number of unpaired electrons |
|---|---|---|---|
| (A) | $$ \left[\mathrm{Fe} \mathrm{F}_6\right]^{3-} $$ |
(P) | 0 |
| (B) | $$ \left[\mathrm{Fe}(\mathrm{CN})_6\right]^{4-} $$ |
(P) | 1 |
| (C) | $$ \left[\mathrm{Fe}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+} $$ |
(R) | 5 |
| (D) | $$ \left[\mathrm{Fe}(\mathrm{CN})_6\right]^{3-} $$ |
(S) | 4 |
Given below are 4 statements. Two of these are correct statements. Identify them.
A. $$\mathrm{Co}^{2+}$$ is easily oxidised to $$\mathrm{Co}^{3+}$$ in the presence of a strong ligand like $$\mathrm{CN}^{-}$$
B. $$[\mathrm{Fe}(\mathrm{CN})_6]^{4-}$$ is an octahedral complex ion which is paramagnetic in nature.
C. Removal of $$\mathrm{H}_2 \mathrm{O}$$ molecules from $$[\mathrm{Ti}(\mathrm{H}_2 \mathrm{O})_6] \mathrm{Cl}_3$$ on strong heating converts it to a colourless compound.
D. Crystal Field splitting in Octahedral and Tetrahedral complexes is given by the equation $$\Delta_0=4 / 9 \Delta_t$$
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. | Complexion | No. | d orbital configuration of central metal ion. |
|---|---|---|---|
| (A) | $$ \left[M n(C N)_6\right]^{4-} $$ |
(P) | $$ e_g^2 t_{2 g}^3 $$ |
| (B) | $$ \left[\mathrm{Co}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+} $$ |
(Q) | $$ t_{2 g}^4 e_g^2 $$ |
| (C) | $$ \left[\mathrm{Fe}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+} $$ |
(R) | $$ t_{2 g}^5 $$ |
| (D) | $$ \left[\mathrm{MnCl}_4\right]^{2-} $$ |
(S) | $$ t_{2 g}^5 e_g^2 $$ |
A d - block metal $$\mathrm{X}(\mathrm{Z}=26)$$ forms a compound $$[\mathrm{X}(\mathrm{CN})_2(\mathrm{CO})_4]^{+}$$. Calculate its spin magnetic moment value.