Subjective Type

Explain the following: $$Co^{2+}$$ is easily oxidised to $$Co^{3+}$$ in the presence of a strong ligand.

Solution

With the electronic configuration $$3d^2 4s^0, Co^{2+}$$ has three unpaired electrons. $$H_2O$$ being a weak ligand, the unpaired electrons present in $$3d$$ orbital of $$Co\ (II)$$ do not pair up. In the presence of strong ligands, two unpaired electrons in $$3d$$ orbitals pair up and the third unpaired $$e^-$$ shifts to higher energy orbital from where it can be easily lost and hence show an oxidation state of $$III$$.

SIMILAR QUESTIONS

Coordination Compounds

Which of the following is diamagnetic?

Coordination Compounds

A $$[Cr(H_2O)_6]^{3-}$$ complex typically absorbs at around $$574 \ nm$$. It is allowed to react with ammonia to form a new complex $$[Cr(NH_3)_6]^{3+}$$ that should have absorption at :

Coordination Compounds

What is the correct electronic configuration of the central atom is $$K_4(Fe(CN)_6]$$ on crystal field theory?

Coordination Compounds

$$[Fe(H_2O)_5NO]^{2+}$$ is a complex formed during the brown ring test for $$NO^-_3$$ ion. In this complex :

Coordination Compounds

The stability constants of the complexes formed by a metal ion $$(M^{2+})$$ with $$NH_3,CN^-,H_2O$$ and $$en$$ are of the order $$10^{11},10^{27},10^{15}$$ and $$10^8$$ respectively. Then:

Coordination Compounds

$$\Delta_o$$ increases in the order of $$[CrCl_6]^{3-} < [Cr(CN)_6]^{3-} < [Cr(C_2O_4)_3]^{3-}$$.

Coordination Compounds

The value of the 'spin only' magnetic moment for one of the following configurations is $$2.84$$ BM. The correct one is?

Coordination Compounds

Among the ligands $$NH_3, en, CN^-$$ and $$CO$$, the correct order of their increasing field strength is?

Coordination Compounds

Given complexes are low spin complexes, [V(CN)6]4− [Cr(NH3)6]2+ [Ru(NH3)6]3+ [Fe(CN)6]4− then order of magnetic moment (μ) for V2+,Fe2+,Cr+3,Ru3+ is:

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