1.

All the metal ions contains t_(2g).^(6)eg^(0) configuration which of the following complex will not be paramagnetic :

Answer»

`[FeCl(CN)_(4)(O_(2))]^(4-)`
`[Co(CN)_(5)(O_(2))]^(-4)`
`K_(4)[Fe(CN)_(6)]`
`[Fe(CN)_(5)(O_(2))]^(5-)`

Solution :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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