Q. Show the electromagnetic radiation in spectrochemical series?

The spectrochemical series can sometimes be helpful in making certain prediction about the complex. For instance, if we know that a particular metal ion gives a low spin complex with ammonia ligands, then it is certain that its analogus compound with CN^- ligands would also be low spin, since CN^- creates much stronger crystal field than NH₃. However these predictions are pure qualitative in nature and many a times the order may be reversed for adjacent ligands in the spectrochemical series.

Once again let us consider one fine consequence of the splitting of d-orbital energy levels.  Except for d^l0 configuration all other configurations in an octahedral field would have _eg set of orbital incompletely filled. Under the circumstances electrons from d-orbitals can  jump toes orbitals, if the correct amount of energy is supplied to the complex. In the case of transition metal complexes the energy required for the electronic transition from ground state to the excited state generally falls in the visible part of the electromagnetic radiation. A plot of absorbance versus the wavelength of light for the compound is known as absorption spectrum of the complex. If the complex absorbs the red portion of the white light, the blue part will pass through the compound and the compound will appear blue to our eyes. As an example we take [Ti (H₂0)₆]³⁺ where in the ground state one electron of Ti³⁺ ion is present in   t_eg set of orbitals.