A metal ion `M^(n+)` having `d^(4)` valence electrode configuration combines with three ligands to form a complex compound. Assuming `Delta_(0)gtP`.
i) Draw the diagram assuming d-orbital splitting during the complex formation.
ii) Write the electronic configuration of valence electrons of the metal `M^(n+)` ion in terms `t_(2g)` and `e_(g)`.
iii) What type of of hybrisation will `M^(n+)` ion have?
iv) Name the type of isomerism exhibited by the complex.

Explanation

i) N/A
ii) When `Delta_(0) gt P`, the electrons get paired up in the lower `t_(2g)` orbitals. The electronic configuration of `d^(4)` ion is: `t_(2g)^(2)e_(g)^(0)`.
iii) The complex is octahedral since the didenate ligands are attached to the `M^(n+)` ion which is `d^(2)sp^(3)` hybridised.
iv) The complex will exhibit optical isomerism.