I have read my text and have not been able to answer the following question. "Explain, using d orbitals, why Copper has so many colors?" The text has just confused me even further.
any and all help appreciated.
2006-11-29 16:31:29 · 2 answers · asked by roncho 4 in Science & Mathematics ➔ Chemistry
When a ligand binds to Cu, it splits the 5 d orbitals into two groups (off the top of my head I cant remember the names but I think they are t2g and eg). The color results from electrons transitioning between the two d orbital levels. Different ligands split the orbitals different amounts so you get different wavelengths of light emitted.
Also, since it is technically forbidden to have an electron transfer within an orbital level, the d-d transition peaks are much smaller than other electron transitions.
2006-11-29 17:11:33 · answer #1 · answered by anon 4 · 0⤊ 0⤋
The reason why is because electrons in the d orbitals can become excited and move to higher energy levels in the d orbital. When they move back down again they release energy in the form of light energy, the colour depends on how much energy was released.
2006-11-30 00:42:23 · answer #2 · answered by Em_butterfly 5 · 0⤊ 0⤋