The electronic arrangement of an octahedral complex with a ${\mathrm{d}}^4$ configuration, if ∆₀ < pairing energy is:

1. ${\mathrm{t}}_{2\mathrm{g}}^4{\mathrm{e}}_{\mathrm{g}}^0$                       

2. ${\mathrm{e}}_{\mathrm{g}}^4{\mathrm{t}}_{2\mathrm{g}}^0$               

3. ${\mathrm{t}}_{2\mathrm{g}}^3{\mathrm{e}}_{\mathrm{g}}^1$           

4. ${\mathrm{e}}_{\mathrm{g}}^2{\mathrm{t}}_{2\mathrm{g}}^2$

Which among the following is incorrect?

The incorrect option among the following is:

The correct IUPAC name among the following is:

Correct IUPAC name for ${\mathrm{H}}_2\left[{\mathrm{PtCl}}_6\right]$ is:

1. Hydrogen hexachloroplatinate(IV)

2. Dihydrogen hexachloroplatinate(IV)

3. Hydrogen hexachloroplatinic(IV) acid

4. Hexachloroplatinic(IV) acid

[Fe(H₂O)₆]²⁺ and [Fe(CN)₆]^4-  differ in:

1. Geometry and magnetic moment.

2. Geometry and hybridization.

3. Magnetic moment and colour.                       

4. Hybridization and number of d-electrons.

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.

[Co(NH₃)₄(NO₂)₂]Cl can show:

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

1. [Co(H₂O)₆]³⁺

2. [Co(NH3)₆]³⁺

3. [Co(CN)₆]^3$-$

4. [Co(C₂O₄)₃]^3$-$

The complex that does not exhibit optical isomerism is:

(en-ethylenediamine)

1. [Co(en)₂Cl₂]⁺

2. [Co(NH₃)₃Cl₃]

3. [Co(en)Cl₂(NH₃)₂]⁺

4. [Co(en)₃]³⁺