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For Test 2, should we memorize what series correspond to different spectra? For ex, in problem 1.15, the question states "In the ultraviolet spectrum of atomic hydrogen, a line is observed at 102.6 nm. Determine the values of n for the initial and final energy levels of the electron during the emission of energy that leads to this spectral line." Should we know automatically that ultraviolet light has an initial n value of 1 (basically, should we know that it's the Lyman series)?
I think that we need to know the values that correspond to the Atomic spectrum so that we can Identify how different wavelengths result in different position on the spectrum like the series that you mention your question. So I think that we do need to memorize it.
It would help to know what energy levels are associated with what part of the EM spectrum. So in the problem you mentioned, recognizing a wavelength of 102.6 nm as being ultraviolet light, and knowing that ultraviolet light is associated with the n=1 energy level (Lyman series) would be really helpful. However, knowing the actual names of these various series I do not think is necessary.
Elana Weingord 1C wrote:Yes we need to know the different energy levels for the balmer (n=2) and lyman (n=1) series. I think that it is also important to know that there are only 7 different energy levels.
What do you mean by what you said that there are only 7 different energy levels? I thought the number of energy levels could approach infinity since nothing is really limiting the number of energy levels there could be, like in the equation for the H-atom: E(n)=-hR/n².
Pretty sure all we have to know regarding the Balmer/Lyman series in general (not just for test 2) is that they correspond to the visible light spectrum/ultraviolet spectrum and the numbering for atomic spectra (n=2 vs n=2 )
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