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I'm not sure what your background is, but this is actually a very complicated question.

Short answer: It all has to do with the structure and symmetry of the molecule which is in question.

Long answer:

The degree to which substances absorb color depends on the way their chemical and physical properties interact with light. Because of this, this question is a quantum physics question. I'm not sure what your background is, but I can try and answer in generalized terms.

Certain chemicals can absorb light. Any dye does, such as Yellow-5, which is in Mountain Dew and myriad other foods. Dyes are able to absorb light because their structures are "conjugated". If you have had organic chemistry, this term should make sense. If you haven't, then this might sound foreign. Highly conjugated compounds have the ability to de-localize their electrons. Because of this, incident light is able to interact with it and be absorbed.

In a quantum physics sense, it depends on the size of the "box" which is created from the conjugation of the molecules. If you have any background with the "particle in a box" theory, which is taught in almost every undergraduate and graduate quantum physics course, then you can think of it that way. The greater the degree of conjugation, such as the length of a double bond system, affects the energies of the quantum levels, and thus the energies of light which can be absorbed.

So the ability for electrons to be promoted and de-localized is important when considering which wavelengths of light (and therefore colors) can be absorbed. This is based highly on molecular structure.

And always remember, symmetry is of paramount importance as well. An excited state must agree in symmetry with the electronic ground state.... (If you have had a molecular spectroscopy course or quantum mechanics, this should also make sense.)

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14y ago

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