How can the existence of spectra help prove that energy levels in atoms exist?

<p>The existence of atomic spectra tells us that energy levels in atoms are quantised. When atoms absorb or emit light, they do so at specific wavelengths. They lead to line spectra instead of a continuous spectrum. Now, every line corresponds to an electron that transitions between fixed energy levels. This is to make the photon's energy equal to the difference between them. If energy levels were not discrete, the spectra would be continuous. So, the line spectra provide direct evidence that electrons in atoms occupy quantised energy states.</p>

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