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I’m confused about why we don’t see absorbed light. The way I understand it is if an atom absorbs a photon then the electrons move up to an energy level corresponding to the energy of the photon. The electrons move down and emit a photon with the same energy so the emitted light would be of the same or lower wavelength as the absorbed light? When hydrogen is excited the colour seen is a mixture of the emitted wavelengths which are the same as the wavelengths absorbed. So why is it that objects that absorb red light reflect blue light? Is red light still emitted but we don’t see it, or does this energy absorbed completely disappear with no emission? Is emission of photons from excited atoms different to how colour is seen from other objects? I’d really appreciate if someone could explain this to me

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However, standard LEDs exhibit radial emission patterns. Therefore, it is necessary to obtain parallel light by placing a collimate lens in the optical path.

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For salts and other ionic compounds, the absorption can be due on either transitions between electron bands or on localized absorption centers like impurities or defects levels. For example, the colour of rubies is due to impurities. A pure crystal of aluminum oxide is colorless. With chromium impurities is ruby red.

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The colour of solids is due to various processes. There is no unique explanation for all types of solids. For solid metals, light interacts with the free electrons in the conduction bands. This results in a very strong reflexion for all the frequencies in the visible band. So, most metals have no special colour. You could call them white or grey but due to the strong reflexion they look shiny or "metallic". There are a few exceptions, like copper or gold. They have free electrons too, as all metals, so they are shiny. But there is some absorption of light in the green-blue band so the reflected light is displaced towards red. This absorption is not due to free electrons but to the electrons in the ionic cores, electrons on the "d" levels who can be excited to the "s" levels which for these few metals are not fully occupied.

In the case of a circularly polarized wave, the tip of the electric field vector, at a given point in space, relates to the phase of the light as it travels ...

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For free atoms, you are correct. An atom will absorb on resonance light and reemit it after some time. This is resonance fluorescence.

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However, if you take a bunch of atoms, or molecules, and make a solid then some of the absorbed light will be converted to heat. The excited atoms are coupled to phonons of the material, so in this case the reemission doesn't happen.

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