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Do the spectral lines on an emission spectrum represent all the different combinations of electrons of a certain atom moving from a higher to a lower energy level? What does the absorption spectrum show, and what do the spectral lines show on that scale. Lastly, is there any significance in the frequency of the spectral lines in either the emission or absorption spectrum for a certain atom.
Spectral lines on the emission spectrum show the specific wavelengths of light that are absorbed or emitted from an electron in a transitory state between energy levels. So, you could use the different wavelengths to find the amount of energy given off or absorbed to attain different energy levels using the equation with the Rydberg constant, E=-hR/n^2. Since each element exhibits a unique set of spectral lines, they have practical usage in identifying different elements.
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