All the following complex ions are found to be paramagnetic

$\mathrm{P} : {\left[{\mathrm{FeF}}_6\right]}^{3-}; \mathrm{Q} : {\left[{\mathrm{COF}}_6\right]}^{3-}; \mathrm{R} : {\left[\mathrm{V}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{3+}; \mathrm{S} : {\left[\mathrm{Ti}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{3+}$

The correct order of their paramagnetic moment (spin only) is

(1) P>Q>R>S                               

(2) P<Q<R<S

(3) P=Q=R=S                               

(4) P>R>Q>S

Among $\left[{\mathrm{NiCl}}_2{\left({\mathrm{PPh}}_3\right)}_2\right], \left[\mathrm{Ni}{\left(\mathrm{HDMG}\right)}_2\right] \mathrm{and} \left[\mathrm{Ni}{\left(\mathrm{CO}\right)}_4\right]$ complexes the hybridisation states of Ni atom are respectively.

(A) ${\mathrm{sp}}^3, {\mathrm{sp}}^3, {\mathrm{dsp}}^2$                                   

(B) ${\mathrm{sp}}^3, {\mathrm{dsp}}^2, {\mathrm{sp}}^3$

(C) ${\mathrm{dsp}}^2, {\mathrm{dsp}}^2, {\mathrm{sp}}^3$                               

(D) ${\mathrm{sp}}^3, {\mathrm{dsp}}^2, {\mathrm{dsp}}^2$

Amongst ${\left[\mathrm{Co}{\left(\mathrm{ox}\right)}_3\right]}^{3-}, {\left[{\mathrm{CoF}}_6\right]}^{3-} \mathrm{and} {\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_6\right]}^{3+}$ : 

1. ${\left[\mathrm{Co}{\left(\mathrm{ox}\right)}_3\right]}^{3-} \mathrm{and} {\left[{\mathrm{CoF}}_6\right]}^{3-}$ are paramagnetic $\mathrm{and} {\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_6\right]}^{3+}$ is diamagnetic.

2. ${\left[\mathrm{Co}{\left(\mathrm{ox}\right)}_3\right]}^{3-} \mathrm{and} {\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_6\right]}^{3+}$ are paramagnetic $\mathrm{and} {\left[{\mathrm{CoF}}_6\right]}^{3-}$ is diamagnetic.

3. ${\left[\mathrm{Co}{\left(\mathrm{ox}\right)}_3\right]}^{3-} \mathrm{and} {\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_6\right]}^{3+}$ are diamagnetic $\mathrm{and} {\left[{\mathrm{CoF}}_6\right]}^3$ is paramagnetic.

4. ${\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_6\right]}^{3+}$$\mathrm{and} {\left[{\mathrm{CoF}}_6\right]}^{3-}$ are paramagnetic $\mathrm{and} {\left[\mathrm{Co}{\left(\mathrm{ox}\right)}_3\right]}^{3+}$ is diamagnetic.

The 'brown ring' formed at the junction of two layers in the test of nitrate is due to the formation of a complex ion, ${\left[\mathrm{Fe}{\left({\mathrm{H}}_2\mathrm{O}\right)}_5\mathrm{NO}\right]}^{2+}.$ Which of the following statemens are correct for this complex [u=3.87 B.M.)

 (i) Oxidation state of Fe is +1 and NO exists as ${\mathrm{NO}}^{+}.$

 (ii) The complex ion is in octahedral geometry as attained by ${\mathrm{sp}}^3{\mathrm{d}}^2$ hybridisation.

(iii) The complex is paramagnetic and has three unpaired electrons due to transfer of electron from NO to ${\mathrm{Fe}}^{2+}.$

(iv) The complex is in octahedral geometry as attained by ${\mathrm{d}}^2{\mathrm{sp}}^3$ hybridisation.

 (v) The brown colour of the complex is attributed to d-d transition of electron.

(1) (i), (ii) and (v)                                       

(2) (iii), (iv) and (v)

(3) (i), (ii) and (iii)                                       

(4) (ii), (iii) and (v)

The incorrect statement among the following is:

1. $\mathrm{Ti}{\left({\mathrm{NO}}_3\right)}_4$ is a colourless compound.

2. ${\left[\mathrm{Cu}{\left({\mathrm{NCCH}}_3\right)}_4\right]}^{+}{\mathrm{BF}}_4^{-}$ is a colourless compound.

3. ${\left[\mathrm{Cr}{\left({\mathrm{NH}}_3\right)}_6\right]}^{3+}3{\mathrm{Cl}}^{‐}$ is a coloured compound..

4. ${\mathrm{K}}_3\left[{\mathrm{VF}}_6\right]$ is a colourless compound.

Identify the correct order of wavelength of light absorbed for the following complex ions.

${\left[\mathrm{Co}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{3+ ;}$          ${\left[\mathrm{Co}{\left(\mathrm{CN}\right)}_6\right]}^{3- ;}$             ${\left[\mathrm{Co}{\left(\mathrm{I}\right)}_6\right]}^{3- ;}$               ${\left[\mathrm{Co}{\left(\mathrm{en}\right)}_3\right]}^{3+}$

          I                                      II                                 III                                 IV

(1) III>I>IV>II                                 

(2) II>IV>I>III

(3) III>I>II>IV                                 

(4) I>III>IV>II

The possible geometrical isomers shown by ${\left[\mathrm{Co}\left(\mathrm{en}\right){\mathrm{Br}}_2{\mathrm{Cl}}_2\right]}^{-}$ is :

1. 2                                           

2. 3

3. 4                                           

4. 6

The total number of isomers of the complex, $\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_3{\left({\mathrm{NO}}_2\right)}_2\left({\mathrm{NO}}_3\right)\right]$ complex is :

1. 10                                       

2. 6

3. 4                                         

4. 12

Which one of the following complexes exhibit chirality ?

(1) ${\left[\mathrm{Cr}{\left(\mathrm{ox}\right)}_3\right]}^3$                             

(2) $\mathrm{cis}-\left[{\mathrm{PtCl}}_2\left(\mathrm{en}\right)\right]$

(3) $\mathrm{cis}-{\left[{\mathrm{RhCl}}_2{\left({\mathrm{NH}}_3\right)}_2\right]}^{‐}$             

(4) $\mathrm{mer}-\left[\mathrm{Co}{\left({\mathrm{NO}}_2\right)}_3\left(\mathrm{trine}\right)\right]$

Assertion : In complex $\left[\mathrm{Cr}{\left({\mathrm{NH}}_3\right)}_4 \mathrm{BrCl}\right]\mathrm{Cl},$ the 'spin only' magnetic moment is close to 1.73 B.M.

Reason : All known mononuclear complexes of chromium (III), irrespective of the strength of the

               ligand field, must have three unpaired electrons.