Choose incorrect stability order :

(1) ${\left[\mathrm{Cu}({\mathrm{NH}}_3{)}_4\right]}^{2+}<{\left[\mathrm{Cu}(\mathrm{en}{)}_2\right]}^{2+}<{\left[\mathrm{Cu}\left(\mathrm{trien}\right)\right]}^{2+}$

(2) ${\left[\mathrm{Fe}({\mathrm{H}}_2\mathrm{O}{)}_6\right]}^{3+}<{\left[\mathrm{Fe}({\mathrm{NO}}_2{)}_6\right]}^{3-}<{\left[\mathrm{Fe}({\mathrm{NH}}_3{)}_6\right]}^{3+}$

(3) ${\left[\mathrm{Co}({\mathrm{H}}_2\mathrm{O}{)}_6\right]}^{3+}<{\left[\mathrm{Rh}({\mathrm{H}}_2\mathrm{O}{)}_6\right]}^{3+}<{\left[\mathrm{Ir}({\mathrm{H}}_2\mathrm{O}{)}_6\right]}^{3+}$

(4) ${\left[\mathrm{Cr}({\mathrm{NH}}_3{)}_6\right]}^{1+}<{\left[\mathrm{Cr}({\mathrm{NH}}_3{)}_6\right]}^{2+}<{\left[\mathrm{Cr}({\mathrm{NH}}_3{)}_6\right]}^{3+}$

Aqueous solution of Ni²⁺ contains [Ni(H₂O)₆]²⁺ and its magnetic moment is 2.83 BM. When ammonia is added in it, the magnetic moment of solution:

1. Will remain the same.

2. Will increase from 2.83 BM.

3. Will decrease from 2.83 BM.

4. Cannot be predicted theoretically.

Which of the following is true about the complex $\left[{\mathrm{PtCl}}_2\right({\mathrm{H}}_2\mathrm{O}\left)\right({\mathrm{NH}}_3\left)\right]$ ?

(1) It exhibits geometrical isomerism

(2) It is a paramagnetic complex

(3) Its geometry is a tetrahedron 

(4) Platinum is ${\mathrm{sp}}^3$ hybridized 

Complex compound $\left[\mathrm{Cr}\right(\mathrm{NCS}\left)\right({\mathrm{NH}}_3{)}_5\left]\right[{\mathrm{ZnCl}}_4]$ will be:

(1) colourless and diamagnetic

(2) green coloured and diamagnetic

(3) green coloured and shows coordination isomerism

(4) diamagnetic and shows linkage isomerism

An aqueous solution of titanium chloride, when subjected to magnetic measurement, measured to zero magnetic moment. Assuming the octahedral complex in aqueous solution, the formula of the complex is :
1. \(\left[\mathrm{Ti}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right] \mathrm{Cl}_2 \)
2. \(\left[\mathrm{Ti}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right] \mathrm{Cl}_4 \)
3. \(\left[\mathrm{TiCl}_3\left(\mathrm{H}_2 \mathrm{O}\right)_3\right] \)
4. \(\left[\mathrm{TiCl}_2\left(\mathrm{H}_2 \mathrm{O}\right)_4\right]\)

Which of the following pairs of complexes are isomeric with each other but their aqueous solutions exhibit different molar conductivities?

(a) $\left[{\mathrm{PtCl}}_2\right({\mathrm{NH}}_3{)}_4]{\mathrm{Br}}_2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>[{\mathrm{PtBr}}_2\left({\mathrm{NH}}_3{)}_4\right]{\mathrm{Cl}}_2$ 

(b) $\left[{\mathrm{CoCl}}_2\right({\mathrm{NH}}_3{)}_4]{\mathrm{NO}}_2<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>[\mathrm{CoCl}\left({\mathrm{NO}}_2\right)\left({\mathrm{NH}}_3{)}_4\right]\mathrm{Cl}$

(c) $\left[\mathrm{Co}\right({\mathrm{NO}}_2\left)\right({\mathrm{NH}}_3{)}_5]{\mathrm{Cl}}_2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>[\mathrm{Co}\left(\mathrm{ONO}\right)\left({\mathrm{NH}}_3{)}_4\right]{\mathrm{Cl}}_2$

(d) $\left[\mathrm{CoBr}\right({\mathrm{NH}}_3{)}_5]{\mathrm{SO}}_4<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>[\mathrm{Co}\left({\mathrm{SO}}_4\right)\left({\mathrm{NH}}_3{)}_5\right]\mathrm{Br}$

The two compounds pentaamminesulphatocobalt (III) bromide and pentaamminesulphatocobalt (III) chloride represent :

(1) Linkage isomerism                   

(2) Ionization isomerism

(3) Coordination isomerism             

(4) No isomerism 

Select the correct code about complex $\left[\mathrm{Cr}\right({\mathrm{NO}}_2\left)\right({\mathrm{NH}}_3{)}_5\left]\right[{\mathrm{ZnCl}}_4]$ :

In the isoelectronic series of metal carbonyl, the CO bond strength is expected to increase in the order:

(1) $\left[\mathrm{Mn}\right(\mathrm{CO}{)}_6{]}^{+}<\left[\mathrm{Cr}\right(\mathrm{CO}{)}_6]<[\mathrm{V}(\mathrm{CO}{)}_6{]}^{-}$

(2) $\left[\mathrm{V}\right(\mathrm{CO}{)}_6{]}^{-}<\left[\mathrm{Cr}\right(\mathrm{CO}{)}_6]<[\mathrm{Mn}(\mathrm{CO}{)}_6{]}^{+}$

(3) $\left[\mathrm{V}\right(\mathrm{CO}{)}_6{]}^{-}<\left[\mathrm{Mn}\right(\mathrm{CO}{)}_6{]}^{+}<\left[\mathrm{Cr}\right(\mathrm{CO}{)}_6]$

(4) $\left[\mathrm{Cr}\right(\mathrm{CO}{)}_6]<[\mathrm{Mn}(\mathrm{CO}{)}_6{]}^{+}<[\mathrm{V}(\mathrm{CO}{)}_6{]}^{-}$

Which is not true about metal carbonyls?

1.  Here CO acts as a Lewis base as well as Lewis acid. 

2. Here metal acts as Lewis base as well as Lewis acid.

3. Here $\mathrm{d\pi }-\mathrm{p\pi }$ back bonding takes place.

4. Here $\mathrm{p\pi }-\mathrm{p\pi }$ back bonding takes place.