These are the questions about the lab \"systhesis of trans-dichlorobis(ethylened

Question

These are the questions about the lab "systhesis of trans-dichlorobis(ethylenediamine)-cobalt(III) chloride and cis-dichlorobis(ethylenediamine)-cobalt(III) chloride".

1. Co^(3+) complexes are very stable and the ligands in such complexs are not labile. explain the relative inertness of Co^(3+) complexes.

2. Define the symmetry elements of the trans and cis isomers.

3. in place of oxygen as the oxidizing, hydrogen peroxide may be used in this reaction. Balance the following oxidation-reduction reaction using this reagent.

CO2+ + H++H2O2 -> Co3++ H2O. Which species is the reducing agent in this reaction?

4. In the absence of the ethylenediamine ligands, the hexaaquocobalt(III) ion reacts rapidly with water according to the following scheme.

[Co(H2O)6]3+ + H2O -> [Co(H2O)6]2+ + O2 + H+

Balance the equation and determine which species is the reducing agent.

Explanation / Answer

There are three factors which affect the labile/inert nature of complexes:

Size of the central metal ion: Smaller the size of the metal ion, greater will be the inertness because the ligands are held tightly by the metal ion.
Charge on the central metal ion: Greater the charge on the metal ion, greater will be the inertness of the complex.
d-electron configuration: If electrons are present in the antibonding eg* orbitals, complex will be labile because the ligands will be weakly bonded to the metal and hence can be substituted easily. If the complex contains empty t2g orbitals, then it will be labile because ligands can approach easily without much repulsion. In short, if the complex contains less than three d-electrons, it will be labile. Or, if one or more eg electrons are present, it will be labile.

In case of Co3+, the electronic configuration is d6 and t2g is filled. So Co3+ complexes are inert and not labile.

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