Compare qualitatively the first and second ionisation potent
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    The d-And-f-Block Elements

    Multiple Choice QuestionsShort Answer Type

    41.

    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.

    Electronic configuration of copper is [Kr] 3d10 4s1 and electronic configuration of zinc is [Kr] 3d10 4s2 .
    On the basis of Cu and Zn. The first ionization potential of zinc is higehr than Cu.
    Because in the zinc electron is removed form 4s2 configuration (which is in stable state) while in copper it is removed form 4s1 configuration thus more energy is required for the removal of 4s2 electron than that of 4s1.

    While in second ionization potential of copper is higher than that of zinc because Cu+ has 3d10 configuration (stable) in comparsion of 3d10 4s1of Zn+.

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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–?
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    50. The ionisation enthalpies of Cr and Cu are larger than their neighbours. Why?
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