Question:

What is meant by 'disproportionation'? Give two examples of disproportionation reaction in aqueous solution.

 

Updated On: Sep 29, 2023
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Solution and Explanation

It is found that sometimes a relatively less stable oxidation state undergoes an oxidation - reduction reaction in which it is simultaneously oxidised and reduced. This is called disproportionation.
For example,
(i) \(3Cr^{3-}_4+8H^+ \rightarrow 2Cr^{2-}_4+Cr^{3+}+4H_2O\)
      Cr( V )                       Cr ( VI )          Cr ( III )
Cr(V) is oxidized to Cr(VI) and reduced to Cr(III)
(ii) \(3MnO^{2-}_4+4H+\rightarrow2MnO^-_4+MnO_2+2H_2O\)
       Mn( VI )                                Mn ( VII )       Mn( IV )
Mn (VI) is oxidized to Mn (VII) and reduced to Mn (IV).

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The d-block elements are placed in groups 3-12 and F-block elements with 4f and 5f orbital filled progressively. The general electronic configuration of d block elements and f- block elements are (n-1) d 1-10 ns 1-2 and (n-2) f 1-14 (n-1) d1 ns2 respectively. They are commonly known as transition elements because they exhibit multiple oxidation states because of the d-d transition which is possible by the availability of vacant d orbitals in these elements. 

They have variable Oxidation States as well as are good catalysts because they provide a large surface area for the absorption of reaction. They show variable oxidation states to form intermediate with reactants easily. They are mostly lanthanoids and show lanthanoid contraction. Since differentiating electrons enter in an anti-penultimate f subshell. Therefore, these elements are also called inner transition elements.

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