Q11 of 46 Page 1

(a) Using valence bond theory, write the hybridisation and magnetic character of the complex [Fe(CN)6]4-. (Atomic no. of Fe = 26)

(b) Write the electronic configuration of d6 on the basis of crystal field theory when


(i) Δo< P and


(ii) Δo > P


(a) Fe exists in +2 oxidation state in [Fe(CN)6]4-.


Electronic configuration of Fe+2 = 3d6


fe.png


As CN is a strong field ligand, there will be pairing of electrons in d orbital.



Hybridization and shape of [Fe(CN)6]4- is d2sp3 and octahedral respectively.


Since, there is no unpaired electron present therefore, the complex is diamagnetic in nature.


(b) (i) When Δo< P, the electronic configuration of d6 will be t2g3eg3.


(ii) When Δo > P, the electronic configuration of d6 will be t2g6eg0.


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