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On the basis of VB theory explain the nature of bonding in [Co(C_(2)O_(4))_(3)]^(3-). |
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Answer» Solution :In the complex entity `[Co(C_(2)O_(4))_(3)]^(3-)`, the `Co` is in `+3` oxidation state . The outer electronic configuration of `Co^(3+)` is `3d^(6)` . The oxalato ligand is FAIRLY strong FIELD ligand. So it faces the `3d` electrons in `Co^(3+)` to pair up and make two of the `3d` orbitals available for bonding. As a result, `Co3^(+)` shows `d^(2)sp^(2)` hybridisation. Electronic configuration of `Co` atom Electronic configuration of `Co^(3+)` ion Hybridisation and FORMATION of `[Co(C_(2)O_(4))_(3)]^(-3)` There is no unpaired electron in `[Co(C_(2)O_(4))_(3)]^(3-)`. Thus `[Co(C_(2)O_(4))_(3)]^(3-)` is diamagnetic in nature. During the formation of `[Co(C_(2)O_(4))_(3)]^(3-)`, two of the `3d`-orbitals are used in bonding. Therefore it is an inner ORBITAL (low SPIN)complex. The `[Co(C_(2)O_(4))_(3)]^(3-)` has the octahedral geometry. 
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