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11. $[NiCl {]_{4}}^{2 -}$ is paramagnetic while $[Ni (CO)_{4}]$ is diamagnetic though both are tetrahedral. Why?

In Ni(CO)₄, Ni is the zero oxidation state whereas in NiCl₄^2–, it is in +2 oxidation state. In the presence of CO ligand, which is strong ligand can paired all electron in Ni(CO), Hence it is a diamagentic in nature. But Cl^– being a weak ligand is unable to pair up the unpaired electrons. Hence NiCl₄^2- is paramagnetic in nature.

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12.

[Fe (H_{2} O)_{6}]^{3 +}

is strongly paramagnetic whereas

[Fe (CN)_{6}]^{3 -}

is weakly paramagnetic. Explain.

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13. Explain

{[Co ({NH}_{3})_{6}]}^{3 +}

is an inner orbital complex whereas

{[Ni ({NH}_{3})_{6}]}^{2 +}

is an outer orbital complex.

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14.

Predict the number of unpaired electrons in the square planar [Pt(CN)₄,]^2– ion.

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15.

The hexaquo manganese(II) ion contains five unpaired electrons, while the hexacynoion contains only one unpaired electron. Explain using crystal field theory.

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16. Calculate the overall complex dissociation equilibrium constant for the Cu(NH₃)₄²⁺ion, given β₄ for this complex is 2.1 x 10¹³.

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17.

Identify the ligands from the following coordination compounds:
(a)    [Co(en)₂Cl(NO₂)₂]
(b)    K[Co(CN)(CO₂)(NO)]
(c)    K₃[Al(OH)₆]
(d)    [Co(H₂O)₂(NH₃)₄](OH)₃

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18. Write IUPAC name of the following complexes:
(a) [Fe(H₂O)₆]SO₄
(b) [Cu(en)₂(NO₃)₂

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19. Give IUPAC name of the following complexes:
(i) Na₂[Fe(CN)₅(NO)], (ii) K₂[Zn(CN)₄]

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20.

Provide systematic names to the following complexes:
(i) [Fe(H₂O)₅(NO)]SO₄,
(ii) [Cr(NH₃)₆]³⁺(iii) [Pt(NH₃)₂Cl₂],
(iv) [NiCl₄]^2–

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Coordination Compounds

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11. $[NiCl {]_{4}}^{2 -}$ is paramagnetic while $[Ni (CO)_{4}]$ is diamagnetic though both are tetrahedral. Why?

Previous Year Papers

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Short Answer Type

11. [NiCl]42- is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Why?

11. $[NiCl {]_{4}}^{2 -}$ is paramagnetic while $[Ni (CO)_{4}]$ is diamagnetic though both are tetrahedral. Why?