Of the following complex ions, which is diamagnetic in nature?

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

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

3.  ${\left[{\mathrm{CoF}}_6\right]}^{3-}$

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

The complexes [Co(NH₃)₆][Cr(CN)₆] and [Cr(NH₃)₆][Co(CN)₆] show:

1. Ionisation isomerism

2. Co-ordination isomerism

3. Geometrical isomerism

4. Linkage isomerism

The number of geometrical isomers shown by $\left[\mathrm{Pt}\left(\mathrm{Py}\right)\left({\mathrm{NH}}_3\right)\mathrm{BrCl}\right]$ are:

The  complex ion that does not expected to absorb visible light is:

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

2. $\left[Cr\right(N{H}_3{)}_6{]}^{3+}$

3. $\left[Fe\right(H_{2}O{)}_6{]}^{2+}$

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

The existence of two different coloured complexes with the composition of [Co(NH₃)₄Cl₂]⁺is due to:

1. Linkage isomerism

2. Geometrical isomerism

3. Coordination isomerism

4. Ionisation isomerism

Which of the following ions doesn't exhibit optical isomerism?

(en = ethylenediamine)

1. [Co(en)₂Cl₂]⁺

2. [Co(NH₃)₃Cl₃]

3. [Co(en)Cl₂(NH₃)₂]⁺

4. [Co(en)₃]³⁺

A complex  ion among the following can absorb visible light is:
(At. no. Zn = 30, Sc = 21, Ti = 22, Cr = 24)

1. [Sc(H₂O)₃(NH₃)₃]³⁺

2. [Ti(en)₂ (NH₃)₂]⁴⁺

3. [Cr(NH₃)₆]³⁺

4. [Zn(NH₃)₆]²⁺

Out of ${\mathrm{TiF}}_6^{2-}$, ${\mathrm{CoF}}_6^{3-}$, Cu₂Cl₂ and ${\mathrm{NiCl}}_4^{2-}$(Z of Ti = 22, Co=27, Cu = 29, Ni= 28) the colourless species are:

1. $Ti{F}_6^{2-}$ $and$ $Co{F}_6^{3-}$

2. $C{u}_{2}C{l}_2$ $and$ $NiC{l}_4^{2-}$

3. $Ti{F}_6^{2-}$ $and$ $C{u}_{2}C{l}_2$

4. $Co{F}_6^{3-}$ $and$ $NiC{l}_4^{2-}$

Which of the following complexes has the highest paramagnetic behaviour?

(where gly = glycine, en = ethylenediamine, ox = oxalate ion and bpy = bipyridyl moieties )
(At no : Ti= 22, V = 23, Fe = 26, Co = 27)

1. [V(gly)₂(OH)₂(NH₃)₂]⁺

2. [Fe(en)(bpy)(NH₃)₂]²⁺

3.  [Co(ox)₂(OH)₂]^-

4. [Ti(NH₃)₆]³⁺

CFSE (in the octahedral field) will be maximum in:
(Atomic number Co = 27)

1. ${\left[\mathrm{Co}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{3+}$

2. ${\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_6\right]}^{3+}$

3. ${\left[\mathrm{Co}{\left(\mathrm{CN}\right)}_6\right]}^{3-}$

4. ${\left[\mathrm{Co}{\left({\mathrm{C}}_2{\mathrm{O}}_4\right)}_3\right]}^{3-}$