Question

why CO2+ is easily oxidized to CO3+ in presence of a strong ligand???

Answer 1

CO2+ ions can be easily oxidised to CO3+ ions because the crystal field stabilisation energy of Ci3+ ions with a d6 configuration is higher than d7 configuration.

In presence of ligand the d- orbitals of metal gets splits up into two set of orbitals that is t2g and eg. The half filled or fully filled t2g is more stable than other configuration. This is because it gives maximum amount of low energy of t29 orbital. Lower the energy more is the stabilisation.

Hope it will help you..

Answer 2

Answer:

Oxidized- combined with or containing experienced a chemical reaction with oxygen.

Explanation:

The electronic configuration $3 \mathrm{~d}^{2} 4 \mathrm{~s}^{0}, \mathrm{Co}^{2+}$ has three unpaired electrons.

$\mathrm{H}_{2} \mathrm{O}$ existing a weak ligand, the unpaired electrons present in $3 \mathrm{~d}$ the orbital of $\mathrm{Co}$ (II) do not pair up.  In the existence of strong ligands, two unpaired electrons in $3 \mathrm{~d}$ orbitals pair up and the third unpaired $e^{-}$ changes to a more increased energy orbital from where it can be readily failed and thus exhibit an oxidation state of III.

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