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(b) Crystal field splitting in tetrahedral coordination entities In tetrahedral coordination entity formation, the d orbital splitting (Fig. 5.9) is inverted and is smaller as compared to the octahedral field splitting. For the same metal, the same ligands and metal-ligand distances, it can be shown that D = t4/9) D . Co0sequently, the orbital splitting energies are not sufficiently large for forcing pairing and, therefore, low spin configurations are rarely observed. The ‘g’ subscript is used for the octahedral and square planar complexes Fig.5.9: d orbital splitting in a tetrahedral which have centre of symmetry. Since crystal field. tetrahedral complexes lack symmetry, ‘g’ subscript is not used with energy levels. 5.5.5 Colour in In the previous Unit, we learnt that one of the most distinctive Coordination properties of transition metal complexes is their wide range of colours. Compounds This means that some of the visible spectrum is being removed from white light as it passes through the sample, so the light that emerges is no longer white. The colour of the complex is complementary to that which is absorbed. The complementary colour is the colour generated from the wavelength left over; if green light is absorbed by the complex, it appears red. Table 5.3 gives the relationship of the different wavelength absorbed and the colour observed. Table 5.3:Relationship between the Wavelength of Light absorbed and the Colour observed in some Coordination Entities Coordinaton Wavelength of light Colour of light Colour of coordination entity absorbed (nm) absorbed entity [CoCl(NH 3 52+ 535 Yellow Violet 3+ [Co(NH 3 5H2O)] 500 Blue Green Red [Co(NH ) ]+ 475 Blue Yellow Orange 3 6 Not in visible [Co(CN)6]3– 310 Ultraviolet region Pale Yellow 2+ [Cu(H2O)4] 600 Red Blue [Ti(H O) ]+ 498 Blue Green Violet 2 6 The colour in the coordination compounds can be readily explained in terms of the crystal field theory. Consider, for example, the complex [Ti(H O) ] , which is violet in colour. This is an octahedral complex 2 6 3+ 1 where the single electron (Ti is a 3d system) in the metal d orbital is in the t level in the ground state of the complex. The next higher state 2g available for the electron is the empty e gevel. If light corresponding to the energy of blue-green region is absorbed by the complex, it would 1 0 0 1 excite the electron from t 2g level to the e gevel (t 2geg ﬁ t 2g eg). Consequently, the complex appears violet in colour (Fig. 5.10). The crystal field theory attributes the colour of the coordination compounds to d-d transition of the electron. 133 Coordination Compounds Reprint 2026-27