- #36
sophiecentaur
Science Advisor
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Light doesn't have its wavelength changed upon reflection. What possible mechanism could account for that? For reflection to occur, there must be phase continuity at the boundary. A change in wavelength (and hence, frequency) would not satisfy this condition for the reflected wave.
Granted, you can get an effect where em waves of one frequency can be absorbed, excite an atom or molecule into high level and that energy can be re-emitted in two or more energy jumps. But that is not reflection, it is scattering (in all directions) and it non coherent.
For reflection to occur, the waves hitting a surface interact with the bulk material and there is a coherent reconstruction of the wavefront according to Snell's Law (this happens even for diffuse reflections from multiple small surfaces but on a small scale).
If broadband 'white' light hits a surface that absorbs some wavelengths (don't call it "colours" because colour is a perceptual thing) then the reflected light will consist of a selected range of wavelengths that the eye will interpret as a colour. This is the principle of 'subtractive' colour synthesis - as opposed to additive synthesis which is how this colour display works. If the incident light is not white (Say it consists of mostly energy at mid and longer wavelengths so it would 'look' yellowish from the greens and reds) then the pigment on a 'green' surface will still absorb the long wavelengths as it did with white light and just leave green light to be reflected. If the surface had a 'cyan' colour (under white light), it would reflect medium to short wavelengths but, if only medium / long wavelength light (yellowish) fell on it, there would only be mid wavelength colours reflected so it would look greenish. Note, I use "ish" to describe the apparent colours because this description is not quantitative.
You are right to say that the interaction involves electrons - but not individual electrons, necessarily. It will be with the whole of the structure and not like the dreaded Hydrogen Atom, which is used as a model by people to 'explain' everything. In solids (metals particularly) the electrons are not only in the field of just one atom but exist in the company of many surrounding nuclei and electrons; their energy level is due to all of their neighbours.
Granted, you can get an effect where em waves of one frequency can be absorbed, excite an atom or molecule into high level and that energy can be re-emitted in two or more energy jumps. But that is not reflection, it is scattering (in all directions) and it non coherent.
For reflection to occur, the waves hitting a surface interact with the bulk material and there is a coherent reconstruction of the wavefront according to Snell's Law (this happens even for diffuse reflections from multiple small surfaces but on a small scale).
If broadband 'white' light hits a surface that absorbs some wavelengths (don't call it "colours" because colour is a perceptual thing) then the reflected light will consist of a selected range of wavelengths that the eye will interpret as a colour. This is the principle of 'subtractive' colour synthesis - as opposed to additive synthesis which is how this colour display works. If the incident light is not white (Say it consists of mostly energy at mid and longer wavelengths so it would 'look' yellowish from the greens and reds) then the pigment on a 'green' surface will still absorb the long wavelengths as it did with white light and just leave green light to be reflected. If the surface had a 'cyan' colour (under white light), it would reflect medium to short wavelengths but, if only medium / long wavelength light (yellowish) fell on it, there would only be mid wavelength colours reflected so it would look greenish. Note, I use "ish" to describe the apparent colours because this description is not quantitative.
You are right to say that the interaction involves electrons - but not individual electrons, necessarily. It will be with the whole of the structure and not like the dreaded Hydrogen Atom, which is used as a model by people to 'explain' everything. In solids (metals particularly) the electrons are not only in the field of just one atom but exist in the company of many surrounding nuclei and electrons; their energy level is due to all of their neighbours.