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How would you account for the increasing...

How would you account for the increasing oxidising power in the Example series `VO_(2)^(+) lt Cr_(2)O_(7)^(2–)lt MnO_(4) ^(-)`

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This is due to increasing stability of the lower species to which they are reduced.
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How would you account for the increasing oxidising power in the series VO_2^(o+)ltCr_2O_7^(2-)< MnO_4^(ɵ) ?

(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+) .

(a) What happens when (i) Manganate ions (MnO_(4)^(2-)) undergoes disproportionation reaction in acidic medium ? (ii) Lanthanum is heated with Sulphur? (b) Explain the following trends in the properties of the members of the First series of transition elements: (i) E^(@) (M^(2+)//M) value for copper is positive (+ 0.34 V) in contrast to the other members of the series. (ii) Cr^(2+) is reducing while Mn^(3+) is oxidising, though both have d^(4) configuration. (iii) The oxidising power in the series increases in the order VO_(2)^(+) lt Cr_(2)O_(7)^(2-) lt MnO_94)^(-) .

K_(2)Cr_(2)O_(7)+NaoH to CrO_(4)^(2-)

K_(2)Cr_(2)O_(7)+NaoH to CrO_(4)^(2-)

How would you account for the following? The oxidising power of the following three oxo ions in the series follows the order : VO_(2)^(+)ltCr_(2)O_(7)^(2-)ltMnO_(4)^(-)

Which of the following increasing order of oxidising power is correct for the following species? VO_(2)^(+),MnO_(4)^(-),Cr_(2)O_(7)^(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

MnO_(2)+2KOH+(1)/(2)O_(2) to K_(2)MnO_(4)+H(2)O

Na_(2)CrO_(4)+HCl to H_(2)Cr_(2)O_(7)+Na_(2)SO_(4)