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The emission spectra in Bohr's experiments served to illustrate that electrons could shift positions between the various orbital structures surrounding the atom's nucleus. When the electrons did this, they released small packets of energy, called photons. These photons were the emission spectra that showed up as clear divisive lines between the different spectrum lines. That indicated the emissions were of varying frequency, that they were not all the same. The Bohr model of the atom differed greatly with that of it's predecessors, the Rutherford model, the Thomson model, and the plum-pudding model. Electrons could now be shown to exist at different energy levels, and also possess the capability to jump, or shift, between those energy levels. This new development served to further expand knowledge in the area of atomic theory.
Niels Bohr carried out this experiment and found that instead seeing a continous spectrum, he saw a series of narrow lines. His experimental works involved measuring the wavelengths of each line in the emission line spectrum of hydrogen using a spectrometer. Bohr found out that wavelengths of light in the emission spectrumof hydrogen atom, calculating using his theory, were exactly the same values as those measured experimentally
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