1.

What may be the stable oxidation state of the transition element with the following d-electron configuration in the ground state of their atoms: 3d^(3), 3d^(5), 3d^(8) and 3d^(4)?

Answer»

SOLUTION :(i) `3d^(3)`: Stable oxidation STATE will be `(+5)` DUE to outer electronic configuration `3d^(3) 4S^(2) (+2, +3,+4,+5)`.
(ii) `3d^(5)`: The outer electronic configuration is `3d^(5) 4s^(2)`, so stable. Oxidation state will be (+2) to (+7) i.e., `(+2), (+3),(+4),(+6),(+7)`
(iii) `3d^(8)`: Stable oxidation state will be (+2) as outer electronic configuration is `3d^(8) 4s^(2) ["(+2)", (+3),(+4)]`
(iv) `3d^(4)`: There is no `d^(4)` configuration in the ground state. The ground state configuration becomes `3d^(5) 4s^(1)`. The stable oxidation state will be `(+3) and (+6)`.


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