why don't d-orbitals split themselves because of themselves without the presence of ligands? Electrons are indistinguishable. Why wouldn't it be more correct that protons from a ligand split the d-orbitals rather than the lone-pairs cause d-orbital splitting energy?
Deepa Subramanian
On our Earth there are certain thermodynamic conditions under which a person can exist with the temperature parameters of 36-41 0C. Substances formed from d-elements and ligands, under conditions on Earth P=1atm and T=25 0C, like other substances during their formation, tend to a minimum decrease in Gibbs energy. For this, free energy levels must be formed, where non-covalent electrons of ligands will go. It is energetically unfavorable for the d-element itself to split energy levels.
Its because of the orientation of the d-orbitals i.e., geometry. The electrons in the d-orbitals are degenerate (similar energy) irrespective of the d-orbital geometry at first. And as the ligand approach this degenerate orbitals tend to vary in their energy . For example, if the ligand approach from xz-direction the d-orbital oriented to that position will have change in energy which ultimately cause splitting and Crystal field stabilization energy comes into play. The splitting of d-orbitals may occur if we are able to selectively apply energy in the particular direction of that d-orbital oriented to that direction.
The protons is a positively charged species and the electrons in the d-orbitals are negatively charged .
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