Where can you find information on color absorption? Please post the information here or site. Thank you!?
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Again, learn to use wikipedia. \n\nThe first link is slightly harder to understand - added another wiki page you can access from the first, in case you didnt see it.
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concentration of the chromophore and wavelength of light that it absorbs. the different wavelengths give the solution (chromophore) different colours.
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I'm not sure exactly what you're asking, but if you put a few drops of food coloring in the water with a white flower (like a carnation), it will absorb the dye and the color.
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http://www.desertusa.com/colorado/coloriv/du_coloriv.html
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do a yahoo search on    "black absorption and radiation"
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Solutions of some chemicals are coloured because the molecules in the solution selectively absorb certain colours from the light passing through. For example, if the chemical absorbed red light then the solution would appear blue-green. In the case of potassium permanganate almost all colours are absorbed, leaving only the blue/indigo/violet range (to use the popular names for the rainbow colours) to get through and cause the purple colour.\n\nNot sure by "band" whether you mean absorption band or transmittance band but the mechanism to produce one would be almost the same. An absorption band is caused by a strong removal of a certain colour (or range of wavelengths) in the area of the band and a transmittance band by the strong removal of colours on each side of the band.\n\nColours are absorbed because the energy the photons having that particular wavelength contain is exactly enough to excite an electron within a molecule. This excitation raises the electron to a higher energy level and the photon is absorbed. Somewhat later, the energy is returned to the system as the electron returns to its former energy level (often via other intermediate levels). The energy is not usually returned as light again however, but more often as a form of heat (a vibration of the crystal lattice, actually). In those cases where the energy does reappear as light the phenomenon is called luminescence, or in some circumstances laser action.\n\nElectrons associated with atoms in molecules and/or complex crystal lattices can have their energy levels changed by the close association with other atoms and so make it more likely they will absorb visible light. This is one of the reasons there are many more coloured compounds than elements. In particular, certain minerals can develop intensely absorbing locations within their structure called "colour centres" which is what produces the deep colours of precious stones. Diamond, on the other hand, is transparent because its highly ordered and stable structure means that a photon would need to have quite a high energy for it to be absorbed and so all visible light passes through unchanged.\n\nHope this is what you were after.
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Below are some links with some cool diagrams.  I'm not sure if it's specifically what you wanted though.  The second link has some really cool information about spectral transitions in a LASER.
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http://illusionsetc.blogspot.com/\n\nhttp://www.panoptikum.net/optischetaeuschungen/opticalillusions.htm\n\nhttp://images.search.yahoo.com/search/images?p=optical%20illusions&fr=FP-tab-web-t&toggle=1&cop=&ei=UTF-8\n\nhttp://search.yahoo.com/search?p=optical+illusions&fr=FP-tab-web-t&toggle=1&cop=&ei=UTF-8
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I'm not sure maybe the link will help.\n\nhttp://www.chemicalforums.com/
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dunnerzplant pretty much has it right.  To give a more basic explanation, the retina has an array of "rods and cones" laid out like pixels on a tv screen, and they are all connected to the visual cortex that has a similar array of perceptive neurons that can piece all fo the signals together as a picture.\n\nDifferent cells in the retina have different chemicals that are sensitive to different colors, or wavelengths of light.  When light of that color strike that cell, the chemical does a slight shape-shift that ignites a mechanism to change the cell's output of neuroreceptors, liek a switch.  Once the light disappears, the photochemical shifts back to its latent state, and the perception of that color also ceases.\n\nIt's pretty cool stuff, really.  Any good Molecular and Cellular Biology textbook will give a good description of how the whole thing works.  I think even a basic college Biology text will give a rudimentary treatment of the subject.
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Uh, I'm not smart on this, so I'm guessing here, but...\nSince different frequencies and wavelengths are what determines what color is being reflected, there has to be some way to quantify the amount of each in different hues of different colors.  Does that even make sense?  I don't know...
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I did find 0.47 for the refraction index "http://www.robinwood.com/Catalog/Technical/Gen3DTuts/Gen3DPages/RefractionIndexList.html" but I I do not know at what wave lenght that I am not seeing probably for green or blue. I found another values has well following:\nhttp://engr.smu.edu/ee/smuphotonics/Modeig/pages/MISC/RNCRIM.DOC\nn=0.18+i*5.72 for 900nm (near infrared)\nn=0.08+i*4.98 for 827nm (red)\n\nI do think it changes a lot with the wavelenght that you input\n\nI do not now if you know what the i means but is the imaginary part of the refraction index it reflects the absorption that light will suffer in the metal. Gold has a metal behaves to the the light much has it behaves  the plasma ones it has free electrons. This explines 2 things the imaginary part and second the value that is minus then 1. the imaginary part is due to the current that are induced when the light incidates in the metals it creates a current that consequently creates an energy lost. (ohm`s theorem) second the efect that is minus then one reflects that the phase velocity seams to propagate at a velocity larger then the velocity of light in vacuum ( its a rouder normal stuff in plasmas if you want to know more tell me I can inform you). Atention this does not mean that the energy travels faster then c it just means the phase does. \n\nif you want me to tell you why is it faster then light it is a litle bit more complicated but if you insist tell me
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Actually, this is a really hard one: color arises from light having different frequencies, and the different colors are reflected with varying efficiency from various substances: so a red color arises from a substance that reflects well low frequencies (red) and absorbs higher ones (blue and yellow).\n\nNow what determines in which way a given substance reflects light at different frequencies? That varies a lot: for starters, some atoms *are* in fact colored, that is, they reflect one frequency more  than another: chlorine gas is an example. This is also frequently the case for molecules (dyes). On the other hand, it is also often caused by some effect that cannot be traced back to the individual parts that make up the whole: think of a sand heap: clearly, none of the grains is a heap, nor is there any specific grain which gives the heap its peculiar properties. What makes a sand heap is just the large number of grains, all acting mutually one upon the other. A crowd, similarly, often does things you cannot really explain in terms of the individuals that make it up. Similarly, for example, a large number of copper atoms find a weird way of reflecting certain frequencies much more than others: it is a property of the whole substance that cannot be reduced to the individual copper atoms. Color, by the way, is not at all the only such property.
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If there are Colours Join the Colors same to the same... Like I mean join the same colors... together...\n\nok.. i actually have no idea..\n\nMaybe it would help..
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Any substance appears coloured because it absorbs all other wavelengths of the visible spectrum other than the wavelength of its colour.i.e if a substance is blue in colour then it absorbs all other wavelenths of the visible spectrum  including red,orange yellow, green  except those pertaining to the blue region of the spectrum. Hence when these wavelenths strike the retina of the eye ,we perceive it as a blue coloured substance.\n   Now though it absorbs all other wavelenths ,it absorbs maximally those of  a coloured region complementary to its physical colour.Thus for blue the complementary colour is orange(oppt ends of the spectrum),for violet  eg KMnO4 it is red etc.So if you have to study the absorption power of a blue solution you have to use  an orange filter in the colorimeter and for an orange coloured solution eg K2Cr2O7  you will use a blue filter.
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A little bit ambiguous...You want to write a "color picker"? Then API is your only way...:D... Beware also at the color "depth" conversion...
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If the colored solid is highly conjugated with at least 9 or more conjugated double bonds, then it is probably that color.\n\nAlso if it absorbs light at the frequency of the color complementary to green than there is no dye.\n\n\nMy recommendations: Filter-vac the solid over a buchner funnel and try various washes with different solvents both organic and inorganic.