I think this is when white light is used that you get an Absorption Spectra. Emission can occur at any frequency at which absorption can occur, and this allows the absorption lines to be determined from an emission spectrum. Many people can tell the difference between fluorescent lights, incandescent lights, and natural sunlight based on subtle differences in the quality (i.e. All the colors of the Absorption Spectra do make it kind of confusing. Reflectance spectra are typically a lot more complicated than emission and absorption spectra, and can be quite difficult to interpret. According to Bohrs model, an electron would absorb energy in the form of photons to get excited to a higher energy level as long as the photons energy was equal to the energy difference between the initial and final energy levels. And these are being absorbed (with emphasis on blue). Bohr could now precisely describe the processes of absorption and emission in terms of electronic structure. Actually, if you just burned hydrogen and looked at its spectra, you would get the Emission Spectra and not the Absorption Spectra, and this Emission Spectra would only show the bunch of blue lines, one purple line, and one red line. All the other colors shown are just part of the natural light being shown down on the element. The reason for this difference is that, in order for an atom to emit light, it must first be excited, meaning that its electrons must be raised to a. This is the color that will be the opposite of the flame color on the color wheel. The difference between the two is that emission spectra contain all the colors of the visible spectrum, while absorption spectra have dark lines corresponding to the colors that are absorbed. Remember, always look at the color area on the rainbow that is blacked out the most. So if blue is being absorbed, the opposite color would be transmitted and this color is orange. However, there are MORE dark lines in the blue region. If you look at the lines for hydrogen blue, purple, and red are being absorbed. Therefore, all the other colors would be absorbed. (This would be orange.) The element hydrogen turns orange when being burned and this color is transmitted to us. Absorption and Emission Spectrum Emission spectrum uses emitted energy to create the spectrum whereas an absorption spectrum uses absorbed energy. This means that if there is a big dark band where blue would be, then the opposite color to blue on the color wheel is being transmitted. The main difference between emission and absorption spectra is that an emission spectrum has different colored lines in the spectrum, whereas an absorption. You are supposed to look at the dark areas of the absorption spectra and those dark areas indicate that the color which would be there is being absorbed. I think both the absorption and emission lines are showing which colors are being absorbed.
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