Answer :

The Oxidation state of Co in both the complexes is +3


F- is a weak field ligand, the cation Co3+ does not allow to pair electron in its excited state hence there is no pairing takes place, so it is paramagnetic, high spin complex, outer orbital complex with sp3d2 hybridisation.

[Co(C2O4)3]3-As the oxalate have -2 charge and is a strong field ligand, it allows to pair electron of Co in its exited state hence there is pairing of electrons which makes it more stable, so it is diamagnetic, low spin complex, inner orbital complex with d2sp3 hybridisation.

Therefore, from the above information, we can conclude

(i) Diamagnetic complex= [Co(C2O4)3]3-

(ii) More stable complex= [Co(C2O4)3]3-

(iii) Outer orbital complex= [CoF6]3-

(iv) Low spin complex= [Co(C2O4)3]3-

Rate this question :

How useful is this solution?
We strive to provide quality solutions. Please rate us to serve you better.
Try our Mini CourseMaster Important Topics in 7 DaysLearn from IITians, NITians, Doctors & Academic Experts
Dedicated counsellor for each student
24X7 Doubt Resolution
Daily Report Card
Detailed Performance Evaluation
view all courses

<span lang="EN-USChemistry - Exemplar

<span lang="EN-USChemistry - Exemplar

When 0.1 mol CoClChemistry - Exemplar

Arrange the folloChemistry - Exemplar

<span lang="EN-USChemistry - Exemplar

When 1 mol CrCl<sChemistry - Exemplar

A coordination coChemistry - Exemplar

Arrange the folloChemistry - Exemplar