Why V and Mn has E° value more than E° value of Cr?
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42.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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43.Transition metals tend to be less reactive. Explain
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44.
Compare qualitatively the first and second ionisation potentials of copper and zinc. Explain the above observation.
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45.
What does the E° value of M3+/M2+ show for Mn3+ and Co3+ (+ 1.57 and 1.97 V respectively)?
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46.Ti2+, V2+ and Cr2+are strong reducing agents. Why?
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47.Give a reaction to show that Cr2+ acts as a reducing agent.
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48.Why is the E° value for Mn3+/Mn2+ higher than that of Cr3+/ Cr2+ (or Fe3+/Fe2+)?
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49.How would you account for the increasing oxidising power in the series VO2+< Cr2O72– < MnO4–?
50.The ionisation enthalpies of Cr and Cu are larger than their neighbours. Why?
Electronic configuration of Cr is 4s1 3d5 and the electronic configuration of Cu is 3d10 4s1. Since both are stable due to having half filled or fully filled orbital thus Cr and Cu show higher ionisation enthalpies than their neighbours.
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