The hybridization and magnetic nature of ${\left[\mathrm{Mn}\right(\mathrm{CN}{)}_6]}^{-4}\text{\hspace{0.17em}and\hspace{0.17em}}{\left[\mathrm{Fe}\right(\mathrm{CN}{)}_6]}^{3-}$, respectively are:

1. $\begin{array}{l}{\mathrm{d}}^2{\mathrm{sp}}^3\end{array}$and diamagnetic

2. $\begin{array}{l}{\mathrm{sp}}^3{\mathrm{d}}^2\end{array}$and diamagnetic

3. ${\mathrm{d}}^2{\mathrm{sp}}^3$ and paramagnetic

4.  ${\mathrm{sp}}^3{\mathrm{d}}^2$ and paramagnetic

Given below are two statements :

1. Statement I is false but Statement II is true.

2. Both Statement I and Statement II are false.

3. Statement I is true but Statement II is false.

4. Both Statement I and Statement II are true.

Number of bridging CO ligands in [Mn₂(CO)₁₀] is:

Simplified absorption spectra of three complexes ((i), (ii) and (iii)) of Mⁿ⁺ ion are provided below; their $\lambda$_max values are marked as A, B and C respectively. The correct match between the complexes and their $\lambda$_max values is:

	(i)	[M(NCS)6](-6+n)
	(ii)	[MF6](-6+n)
	(iii)	[M(NH3)6]n+

Options:

Which of the following complexes is not expected to exhibit isomerism?

The d-electron configuration of [Ru(en)₃]Cl₂ and [Fe(H₂O)₆]Cl₂, respectively are :

1.  t_2g⁶ e_g⁰ and  t_2g⁴ e_g²
\(2.~ t_{2 g}^{4} e_{g}^{2}~ and ~t_{2 g}^{4} e_{g}^{2}\\ 3.~ t_{2 g}^{3} e_{g}^{3} ~and~ t_{2 g}^{4} e_{g}^{2}\\ 4.~ t_{2 g}^{4} e_{g}^{2} ~and~ t_{2 g}^{3} e_{g}^{3}\)

The values of the crystal field stabilization energies for a high spin d⁶ metal ion in octahedral and tetrahedral fields, respectively, are :

1. –0.4 ${∆}_0$ and –0.27 ${∆}_t$
2. –1.6 ${∆}_0$ and –0.4 ${∆}_t$
3. –0.4 ${∆}_0$ and –0.6 ${∆}_t$
4. –2.4 ${∆}_0$ and –0.6 ${∆}_t$

The stepwise formation of [Cu(NH₃)₄]²⁺ is given below

$\begin{array}{l}{\mathrm{Cu}}^{2+}+{\mathrm{NH}}_3\stackrel{{\mathrm{K}}_1}{\rightleftarrows }{\left[\mathrm{Cu}\left({\mathrm{NH}}_3\right)\right]}^{2+}\\ {\left[\mathrm{Cu}\left({\mathrm{NH}}_3\right)\right]}^{2+}+{\mathrm{NH}}_3\stackrel{{\mathrm{K}}_2}{\rightleftharpoons }{\left[\mathrm{Cu}{\left({\mathrm{NH}}_3\right)}_3\right]}^{2+}\\ {\left[\mathrm{Cu}{\left({\mathrm{NH}}_3\right)}_2\right]}^{2+}+{\mathrm{NH}}_3\stackrel{{\mathrm{K}}_3}{\rightleftharpoons }{\left[\mathrm{Cu}{\left({\mathrm{NH}}_3\right)}_3\right]}^{2+}\\ {\left[\mathrm{Cu}{\left({\mathrm{NH}}_3\right)}_3\right]}^{2+}+\mathrm{NH}\stackrel{{\mathrm{K}}_4}{{}_3\rightleftharpoons }{\left[\mathrm{Cu}{\left({\mathrm{NH}}_3\right)}_4\right]}^{2+}\end{array}$

The value of stability constants K₁, K₂, K₃ and K₄ $\text{\hspace{0.17em}are\hspace{0.17em}}{10}^4,1.58\times {10}^3,5\times {10}^2\text{\hspace{0.17em}and\hspace{0.17em}}{10}^2$ respectively. The overall equilibrium constants for the dissociation of $[\mathrm{Cu}{\left({\mathrm{NH}}_3\right)}_4]$²⁺ is x × 10^–12. The value of x is ________.

(Rounded off to the nearest integer)

1. 2

2. 4

3. 3

4. 1