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How would you account for the increasing...

How would you account for the increasing oxidising power in the series `VO_2^(o+)ltCr_2O_7^(2-)< MnO_4^(ɵ)`?

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This is due to the increasing stability of the species with lower oxidation state of metal atom to which they are reduced , e.g., `overset(V) ( V) O_(2)^(+) rarr overset(IV)(V) O^(2+) , overset(VI) (Cr_(2))O_(7)^(2-) rarr overset(III)(Cr^(3+) )rarr overset(VII)(Mn) O_(4)^(-)rarr overset(II) (M) n^(2+) ` etc.
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(a) Complete the following chemical equations: (i) Cr_(2) O_(7)^(2-) (aq) + H_(2) S(g) + H^(+) (aq) to (ii) Cu^(2+)(aq) + I^(-) (aq) to (b) How would you account for the following : (i) The oxidising power of oxoanions are in the order VO_(2)^(+) lt Cr_(2)O_(7)^(2-) lt Mn O_(4)^(-) (ii) The third ionization enthalpy of manganess (Z = 25) is exceptionally high. (iii) Cr^(2+) is a stronger reducing agent than Fe^(2+) .

Following order is observed in oxidising power of certain ions : VO_2^(+) lt Cr_2O_7^(2-) lt MnO_4^(-) The reason for this increasing order of oxidising power is