Homework problem 1.11 asks:
In the spectrum of atomic hydrogen, several lines are
generally classified together as belonging to a series (for
example, Balmer series, Lyman series, Paschen series), as shown
in Figs. 1.10 and 2.1. What is common to the lines within a
series that makes grouping them together logical?
I answered, as we heard in lecture, that the lines in the Lyman series have in common that they all correspond to wavelengths in the UV region, whereas lines in the Balmer series correspond to wavelengths in the visible region. The answer, according to the solutions manual, is the following:
In each of these series, the principal quantum number of for the lower energy level involved is the same for each absorption line, Thus, for the Lyman series, the lower energy level is n=1; for the Balmer series, n=2; for the Paschen series, n=3; and for the Brackett series, n=4.
If this is the case, then why is it that in lecture we were taught that the Balmer and Lyman series' were distinguished by the type of radiation emitted or absorbed by hydrogen atoms? Why was there no mention of the lower energy level involved? Did I miss something in lecture?
Homework Problem 1.11 Issue
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Re: Homework Problem 1.11 Issue
Postby ginnyyao1L » Wed Oct 05, 2016 12:10 am
When the electron is excited and then falls down to its original energy level/ground state, the energy released is what the lines on the spectrum are; therefore, for groups that have around the same lowest energy level, the lines would be grouped together.
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