00:01
This question is mostly associated with the crystal field theory.
00:05
This question describes that there's a certain first -order transition metal that forms different colored solutions.
00:12
Four coordination compounds with this metal have the same coordination number, and when dissolved in water, form red, yellow, green, and blue solutions.
00:21
Further experiments reveal that two of the complex ions are paramagnetic, with four unpaired electrons and two are diamagnetic.
00:30
So what can we deduce about the four different coordination compounds that are created? well, according to the crystal field theory, building upon an octahedral complex, we can have energies of the de -orbital as being split, where three of them are lower in energy, and two of them are higher.
00:56
If the higher energy deorbital is significantly higher, it can force all of the electrons into the lower energy state.
01:06
When this occurs, we have all paired electrons and we have a diamagnetic species.
01:13
So this must be occurring for two of the coordination compounds.
01:21
This often occurs when we have negatively charged ligands forcing this greater energy difference.
01:29
With a greater energy difference than higher energy photons are absorbed in order to transition an electron from a lower energy state up to a higher energy state...
