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They refer to the different special lines electron transition to. So for the lyman series means that electrons transition to the first energy level (n1), balmer series transition to the second energy level (n2), and paschen series transition to the third energy level (n3)
Recall that for the hydrogen emission/absorption spectrum, we see a spectral line when an electron moves from a higher to a lower energy level. The Lyman, Balmer, and Paschen series simply refer to specific groups of spectral lines. The Lyman series starts with energy level n=1, the Balmer series starts with energy level n=2, and the Paschen series starts with energy level n=3. The Lyman series is in the UV region regarding wavelength, whereas the Balmer and Paschen series are in infrared.
From what I understand by reading, the different series have idfferent principal or (like base level) enery levels. So for the Lyman seires, the lower energy level is n = 1 and for Balmer it would be n=2 and so on and so on.
These names refer to groupings of spectral lines. What any given group has in common is to which the energy level the electron relaxes. For example, the Lyman series means the electron goes from any higher energy to level to n=1. This could be 5-->1, 4-->1, etc. For Balmer, the electrons go to n=2, Paschen n=3.
Jessica Dharmawan 1G wrote:Do we have to memorize these for the test this week?
I think it would be a good idea to familiarize yourself with these series, since they might throw it in the test. Just remember Lyman series has an final state of n=1, Balmer is n=2, and Paschen is n=3.
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