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| 1. |
Why are Mn^(2+)compounds more stable than Fe^(2+) towards oxidation to their +3 state? |
| Answer» Solution :The electronic configuration of `Mn^(2+) " is " 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3P^(6) 3D^(5)`. To oxidize to `Mn^(3+)`, the one electron has to be REMOVED from STATE `d^(5)` orbital which is half filled and requires high ionization energy. In `Fe^(2+)` ion, the third electron is taken from `3d^(6)` configuration that results in more STABLE `3d^(5)` configuration. | |