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All the metal ions contains `t_(2g).^(6)eg^(0)` configuration which of the following complex will not be paramagnetic :A. `[FeCl(CN)_(4)(O_(2))]^(4-)`B. `[Co(CN)_(5)(O_(2))]^(-4)`C. `K_(4)[Fe(CN)_(6)]`D. `[Fe(CN)_(5)(O_(2))]^(5-)` |
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Answer» Correct Answer - B::C::D All the metal ion contains `t_(2g).^(6)eg^(0)` configuration so Fe should be in +2 oxidation state and Co in +3 oxidation state but oxygen having tendency to shown different type of oxidation state. [x = oxidation state of `O_(2)]` (A) `[FeCl(CN)_(4)(O_(2))]^(-4)` +2-1-4+x=-4 x=-1 due to the presence of unpatied `e^(-)" in "O_(2)^(-)`, it is an paramagnetic complex. (B) `[Co(CN)_(5)(O_(2))]^(-4)` +3-5+x=-4 x=-2 `O_(2)^(-2)` (diamagnetic) in nature. (C) `Fe^(+2)=t_(2g).^(6)eg^(0)` (diamagnetic) (D) `[Fe(CN)_(5)(O_(2))]^(5-)` +2-5+x=-5,x=-2 `O_(2)^(-2)` (peroxide) is diamagnetic in nature. |
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