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Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:

    \[\left( i \right)\text{ }{{[Co{{({{C}_{2}}{{O}_{4}})}_{3}}]}^{3}}\]

    \[\left( ii \right)\text{ }{{[Co{{F}_{6}}]}^{3-}}\]

CBSE | Chemistry | Class 12 | Coordination Compounds | NCERT
Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory:

    \[\left( i \right)\text{ }{{[Co{{({{C}_{2}}{{O}_{4}})}_{3}}]}^{3}}\]

    \[\left( ii \right)\text{ }{{[Co{{F}_{6}}]}^{3-}}\]

(i) Here, the oxidation state of cobalt is +3.
Orbitals of Co 3+ ion :

Oxalate is a field ligand with a low affinity. As a result, the electrons in the 3d orbital will not pair.
Because there are six ligands, hybridization must be either sp3d2or d2sp3.
Co3+ sp3d2 hybridization:

The 6 electron pairs from the 3 oxalate ions (oxalate anion is a bidentate ligand) occupy these sp3d 2 orbitals :

Therefore, the complex shows octahedral geometry.

(iv) In this complex, Cobalt has an oxidation state of +3.
Orbitals of Co3+ ion:

The 3d electrons will not pair because the fluoride ion is a weak field ligand. As a result, the Co3+ ion will undergo sp3d2 hybridization.

sp3d2 hybridized orbitals of Co3+ ion are :

Therefore, the complex has a geometric configuration of an octahedral and it is paramagnetic.

i

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