How would you account for the increasing oxidising power in the series VO2+< Cr2O72– < MnO4–?
The oxidation state of V in VO2+ is +5 and oxidation state of Cr is +6, oxidation state of Mn is +7. Thus due to the increasing stability of the lower species to which they are reduced.
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What may be the stable oxidation state of the transition elements with the following d-electron configurations in the ground state of their atoms 3d3, 3d5, 3d8 and 3d4?
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The ionisation enthalpies of Cr and Cu are larger than their neighbours. Why?
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Compare qualitatively the first and second ionisation potentials of copper and zinc. Explain the above observation.
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Transition metals tend to be less reactive. Explain
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Ti2+, V2+ and Cr2+are strong reducing agents. Why?
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What does the E° value of M3+/M2+ show for Mn3+ and Co3+ (+ 1.57 and 1.97 V respectively)?
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Why V and Mn has E° value more than E° value of Cr?
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Why is the E° value for Mn3+/Mn2+ higher than that of Cr3+/ Cr2+ (or Fe3+/Fe2+)?
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Give a reaction to show that Cr2+ acts as a reducing agent.
