InterviewSolution
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InterviewSolution
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How would you account for the following :(i) `Cr^(2+)` is reducing in nature while with the same d-orbital configuration `(d^(4)),Mn^(2+)` is oxidising in nature. (ii) In the transition series of metals, the metal which exhibits the greatest number of oxidation states occurs in the middle of the series. |
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Answer» (i) `Cr^(2+)` has the configuration `d^(4)` and easily changes to `d^(3)` has filled orbitals and hence stable. Therefore, `Cr^(2+)` is reducing .On the other hand `Mn^(2+)` is more stable due to half filled `d^(5)` configuartion and `Mn^(3+)` easliy changes to `Mn^(2+)` and hence is oxiding . (ii) This is due to the large no.of unpaired in d-orbitals in the middle of the series. |
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