# Why do transition metals make colored compounds despite the remaining d orbitals being hybridized? [closed]

I know that transition metals make colored compounds when they forms a bond with a ligand, as the ligand increases the energy level of $\ce{d_{x^2-y^2}}$ and $\ce{d_{z^2}}$ orbital by repelling these orbitals with the lone pair electrons of the ligand. So, the electrons move to the lower energy orbitals and when they absorb energy, they again move to the higher orbitals and that absorbed energy creates color.

Now my question is, $\ce{d_{x^2-y^2}}$ and $\ce{d_{z^2}}$ orbital become hybridized while forming a bond with the ligands and those orbitals get filled up with the lone pair electrons of ligands. Then, how are the electrons excited from lower energy orbitals into the higher energy orbital where there is no place left for them?

## closed as off-topic by Mithoron, airhuff, M.A.R., Jan, TyberiusFeb 20 '18 at 17:04

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• There are many theories in coordination compounds. VBT, CFT, LFT, <more that I probably don't know of>. Which one are you using? – Gaurang Tandon Feb 19 '18 at 14:59
• @GaurangTandon Seems you're rather overoptimistic here. I'm afraid not one sentence here is correct. – Mithoron Feb 19 '18 at 16:47
• I am talking about CFT(Crystal Field Theory). – Abtahee Salekeen Feb 20 '18 at 4:03
• I agree with Mithoron here. Not one single sentence is correct from its first capital letter to its final full stop. However, some contain correct fragments in-between. Many of OP’s misconceptions may clear up once they go back to their books and fully understand what is written there. – Jan Feb 20 '18 at 9:09