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Coordination Compounds

Question
CBSEENCH12007307
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[NiCl]42- is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Why?

Solution
In Ni(CO)4, Ni is the zero oxidation state whereas in NiCl42–, 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 NiCl42- is paramagnetic in nature.

Some More Questions From Coordination Compounds Chapter

Indicate the type of isomerism exhibited by the following complexes and draw structures for these isomers:
(i)    K[Cr(H2O)2(C2O4)2],                      (ii) [Co(en)3Cl3,
(iii) [Co(NH3)5(NO2)]|NO3]2,                 (iv) [Pt(NH3)(H2O)Cl2]

Explain on the basis of valence bond theory that [Ni(CN)4]2–  ion with square planar is diamagnetic and the [NiCl4]2– ion with tetrahedral geometry is paramagnetic.

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

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

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

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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