Incorrect match among the following is:

	IUPAC name of coordination compound	Representation
1.	Sodium (ethylenediamine tetraacetato) chromate (II)	\(\small{\mathrm{Na}_2\left[\mathrm{Cr}\left(\mathrm{CH}_3 \mathrm{COO}\right)_4(\mathrm{en})\right]}~~\)
2.	Dichloridobis (ethane-1, 2-diamine) cobalt (III) ion	\(\small{\left[\mathrm{Co}(\mathrm{Cl})_2(\mathrm{en})_2\right]^{+}}\)
3.	Tris (ethane-1,2-diamine) cobalt(III)  sulphate	\(\small{\left[\mathrm{Co}\left(\mathrm{H}_2 \mathrm{NCH}_2 \mathrm{CH}_2 \mathrm{NH}_2\right)_3\right]_2\left(\mathrm{SO}_4\right)_3}\)
4.	Ammineaquadi bromidocopper(II)	\(\small{\left[\mathrm{Cu}\left(\mathrm{NH}_3\right)\left(\mathrm{H}_2 \mathrm{O}\right) \mathrm{Br}_2\right]}\)

The EAN of metal atoms in $\left[\mathrm{Fe}{\left(\mathrm{CO}\right)}_2{\left({\mathrm{NO}}^{+}\right)}_2\right] \mathrm{and} {\left(\mathrm{Co}\right)}_2{{\left(\mathrm{CO}\right)}_8}_{}$ respectively are :

1. 34, 35 

2. 34, 36

3. 36, 36                                       

4. 36, 35

Match the complex ions listed in column-I with the characteristics listed in column-II using the codes given below.

Column-I                                                        Column-II

(a) ${\left[\mathrm{Ni}{\left({\mathrm{NH}}_3\right)}_6\right]}^{2+}$                                     (p) ${\mathrm{d}}^2{\mathrm{sp}}^3$ and diamagnetic

(b) ${\left[\mathrm{Cr}{\left({\mathrm{NH}}_3\right)}_6\right]}^{3+}$                                     (q) ${\mathrm{sp}}^3{\mathrm{d}}^2$ and diamagnetic

(c) ${\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_6\right]}^{3+}$                                     (r) ${\mathrm{sp}}^3{\mathrm{d}}^2$ and two unpaired electrons.

(d) ${\left[\mathrm{Zn}{\left({\mathrm{NH}}_3\right)}_6\right]}^{2+}$                                     (s) ${\mathrm{d}}^2{\mathrm{sp}}^3$ and three unpaired electrons.

$\mathrm{a} \mathrm{b} \mathrm{c} \mathrm{d}$
$\left(1\right) \mathrm{r} \mathrm{s} \mathrm{p} \mathrm{q}$
$\left(2\right) \mathrm{s} \mathrm{r} \mathrm{q} \mathrm{p}$
$\left(3\right) \mathrm{r} \mathrm{s} \mathrm{q} \mathrm{p}$
$\left(4\right) \mathrm{p} \mathrm{q} \mathrm{r} \mathrm{s}$

Which of the following statements is correct?

(A) ${\left[\mathrm{Cr}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{2+} \left(\mathrm{aq}\right) \mathrm{and} {\left[\mathrm{Cr}{\left(\mathrm{CN}\right)}_6^{}\right]}^{4-} \left(\mathrm{aq}\right)$ are high spin and low spin complexes respectively but

     both have same number of unpaired electrons.

(B) ${\left[\mathrm{V}{\left({\mathrm{NH}}_3\right)}_6\right]}^{3+}$ is inner orbital complex and paramagnetic with two unpaired electrons.

(C) ${\left[\mathrm{Co}\left({\mathrm{CN}}_6\right)\right]}^{4-}$ is outer orbital complex and paramagnetic with three unpaired electrons.

(D) $\left[\mathrm{Mn}{\left(\mathrm{NO}\right)}_3\left(\mathrm{CO}\right)\right]$ is square planar and diamagnetic.

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