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thenewmans
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Is there any paper on the quantization of color? Maybe not since it’s obvious. I always thought that color was on a continuum. But now I realize that electrons jump between a limited set of orbits.
thenewmans said:Is there any paper on the quantization of color? Maybe not since it’s obvious. I always thought that color was on a continuum. But now I realize that electrons jump between a limited set of orbits.
Well, you're talking about blending colours though. Seems the poster would want to understand pure, single-frequency colours.ZapperZ said:This is wrong. "Color" implies a particular frequency. You can generate ANY range of EM frequency, in principle! Atomic transition isn't the only way to generate light. Do you think your incandescent light bulb generate light because of some atomic transition? Try passing that light through a diffraction grating and see how that differs from, say, a discharge tube.
Zz.
DaveC426913 said:Well, you're talking about blending colours though. Seems the poster would want to understand pure, single-frequency colours.
Quantization of color is the phenomenon where electrons in an atom can only exist in specific energy levels, or orbits, around the nucleus. These energy levels are quantized, meaning that they can only have certain discrete values and cannot exist in between these values.
Electrons can jump between orbits when they absorb or emit energy. When an electron absorbs energy, it moves to a higher energy level, or orbit. When it emits energy, it moves to a lower energy level. This movement of electrons between orbits is what gives atoms their unique colors.
Electrons have specific energy levels due to the laws of quantum mechanics. These laws dictate that particles, such as electrons, can only exist in certain discrete energy levels and cannot exist in between these levels.
The higher an electron's energy, the further away it is from the nucleus and the larger its orbit. The lower its energy, the closer it is to the nucleus and the smaller its orbit. This relationship is known as the energy-quantization relationship.
No, according to the laws of quantum mechanics, electrons cannot exist in between energy levels. They can only exist in specific, quantized energy levels. This is why we see distinct colors when atoms absorb or emit energy, as the electrons can only jump between these specific energy levels.