Exercises

9.8 List various types of isomerism possible for coordination compounds, giving an example of each.

9.9 How many geometrical isomers are possible in the following coordination entities?

(i) [Cr(C2O4)3]3–                      (ii) [Co(NH3)3Cl3]

9.10 Draw the structures of optical isomers of:

(i) [Cr(C2O4)3]3–           (ii) [PtCl2(en)2]2+              

 (iii) [Cr(NH3)2Cl2(en)]+

9.11 Draw all the isomers (geometrical and optical) of:

(i) [CoCl2(en)2]+           (ii) [Co(NH3)Cl(en)2]2+      

(iii) [Co(NH3)2Cl2(en)]+

9.12 Write all the geometrical isomers of [Pt(NH3)(Br)(Cl)(py)] and how many of these will exhibit optical isomers?

9.13 Aqueous copper sulphate solution (blue in colour) gives:

(i) a green precipitate with aqueous potassium fluoride and

(ii) a bright green solution with aqueous potassium chloride. Explain these experimental results.

9.14 What is the coordination entity formed when excess of aqueous KCN is added to an aqueous solution of copper sulphate? Why is it that no precipitate of copper sulphide is obtained when H2S(g) is passed through this solution?

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

(i) [Fe(CN)6]4–        (ii) [FeF6]3–         

(iii) [Co(C2O4)3]3–            (iv) [CoF6]3–

9.16 Draw figure to show the splitting of d orbitals in an octahedral crystal field.

9.17 What is spectrochemical series? Explain the difference between a weak field ligand and a strong field ligand.

9.18 What is crystal field splitting energy? How does the magnitude of ∆o decide the actual configuration of d orbitals in a coordination entity?