The CFSE for  [CoCl₆]^4-  is 18000  cm^-1. The  ∆_t  for  [CoCl₄]^2- will be :

1. 18000 ${\mathrm{cm}}^{-1}$

2. 16000 ${\mathrm{cm}}^{-1}$

3. 8000 ${\mathrm{cm}}^{-1}$

4. 2000 ${\mathrm{cm}}^{-1}$

The correct order of energies of d-orbitals of metal ion in a square planar complex is-

1. ${\mathrm{d}}_{\mathrm{xy}}={\mathrm{d}}_{\mathrm{yz}}={\mathrm{d}}_{\mathrm{zx}}>{\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}={\mathrm{d}}_{{\mathrm{z}}^2}$

2. ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}={\mathrm{d}}_{{\mathrm{z}}^2}>{\mathrm{d}}_{\mathrm{xy}}={\mathrm{d}}_{\mathrm{yz}}={\mathrm{d}}_{\mathrm{zx}}$

3. ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}>{\mathrm{d}}_{{\mathrm{z}}^2}>{\mathrm{d}}_{\mathrm{xy}}>{\mathrm{d}}_{\mathrm{yz}}={\mathrm{d}}_{\mathrm{zx}}$

4. ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}>{\mathrm{d}}_{\mathrm{xy}}>{\mathrm{d}}_{{\mathrm{z}}^2}>{\mathrm{d}}_{\mathrm{zx}}={\mathrm{d}}_{\mathrm{yz}}$

${\left[{\mathrm{CoCl}}_2{\left({\mathrm{NH}}_3\right)}_4\right]}^{+}+C{l}^{-}\to \left[{\mathrm{CoCl}}_3{\left({\mathrm{NH}}_3\right)}_3\right]+{\mathrm{NH}}_3$

If in the above reaction only one isomer of the product is obtained, which is true for the initial
(reactant) complex

1. Compound is in cis form

2. Compound is in trans form

3. Compound is in both (cis and trans) forms

4. Can't be predicted

Aqueous solution of Ni²⁺ contains ${\left[\mathrm{Ni}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{2+}$ and its magnetic moment is 2.83 B.M.When ammonia is added in it, comment on the magnetic moment of solution

1. It will remain same

2. It increases from 2.83 B.M.

3. It decreases from 2.83 B.M.

4. It can not be predicted theoretically

Among the following, the $\mathrm{\pi }$-acid ligand is

1.  ${\mathrm{F}}^{-}$

2.  ${\mathrm{NH}}_3$

3.  ${\mathrm{CN}}^{-}$

4.  l

The Crystal Field Stabilization Energy (CFSE) and the spin-only magnetic moment in Bohr Magneton (BM) for the complex ${\mathrm{K}}_3\left[\mathrm{Fe}{\left(\mathrm{CN}\right)}_6\right]$ are, respectively,

1.  $0.0{∆}_0 \mathrm{and} \sqrt{35} \mathrm{BM}$

2.  $-2.0{∆}_0 \mathrm{and} \sqrt{3} \mathrm{BM}$

3.  $-0.4{∆}_0 \mathrm{and} \sqrt{24} \mathrm{BM}$

4.  $-2.4{∆}_0 \mathrm{and} \sqrt{0} \mathrm{BM}$

Among the following, the species that is both tetrahedral and diamagnetic is

1.  ${\left[{\mathrm{NiCl}}_4\right]}^{2-}$

2.  ${\left[\mathrm{Ni}{\left(\mathrm{CN}\right)}_4\right]}^{2-}$

3.  $\left[\mathrm{Ni}{\left(\mathrm{CO}\right)}_4\right]$

4.  ${\left[\mathrm{Ni}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{2+}$

In aqueous solution, ${\left[\mathrm{Co}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{2+}$ (X) reacts with molecular oxygen in the presence of excess liquor $N{H}_3$ to give a new complex Y. The number of unpaired electrons in X and Y are, respectively

1.  3,1

2.  3,0

3.  3,3

4.  7,0 

The energies of ${\mathrm{d}}_{\mathrm{xy}} \mathrm{and} {{\mathrm{d}}_{\mathrm{z}}}^2$ orbitals in octahedral and tetrahedral transition metal complexes are such that

1.  $\mathrm{E}\left({\mathrm{d}}_{\mathrm{xy}}\right) > \mathrm{E}\left({\mathrm{d}}_{{\mathrm{z}}^2}\right)$ in both tetrahedral and octahedral complexes

2.  $\mathrm{E}\left({\mathrm{d}}_{\mathrm{xy}}\right) < \mathrm{E}\left({\mathrm{d}}_{{\mathrm{z}}^2}\right)$ in both tetrahedral and octahedral complexes

3.  $\mathrm{E}\left({\mathrm{d}}_{\mathrm{xy}}\right) > \mathrm{E}\left({\mathrm{d}}_{{\mathrm{z}}^2}\right)$ in tetrahedral but $\mathrm{E}\left({\mathrm{d}}_{\mathrm{xy}}\right) < \mathrm{E}\left({\mathrm{d}}_{{\mathrm{z}}^2}\right)$ in octahedral complexes

4.   $\mathrm{E}\left({\mathrm{d}}_{\mathrm{xy}}\right) < \mathrm{E}\left({\mathrm{d}}_{{\mathrm{z}}^2}\right)$  in tetrahedral but $\mathrm{E}\left({\mathrm{d}}_{\mathrm{xy}}\right) > \mathrm{E}\left({\mathrm{d}}_{{\mathrm{z}}^2}\right)$ in octahedral complexes   

The number of geometrical isomers of $\left[{\mathrm{CrCl}}_2\left(\mathrm{en}\right){\left({\mathrm{NH}}_3\right)}_2\right]$, where en = ethylenediamine, is

1.  2

2.  3

3.  4

4.  1