Atomic Spectroscopy  [ENDORSED]

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Maria Roman 1A
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Atomic Spectroscopy

Postby Maria Roman 1A » Sun Apr 22, 2018 10:24 pm

How can you tell what spectroscopic series energy transition belongs to?

Bryan Jiang 1F
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Re: Atomic Spectroscopy  [ENDORSED]

Postby Bryan Jiang 1F » Sun Apr 22, 2018 10:49 pm

What spectroscopic series an energy transition belongs to depends on what energy level an electron jumps from when absorbing energy or what energy level an electron drops to when emitting energy. So for an H-atom, if an electron jumps from or drops to the n=1 energy level, these lines will be of the Lyman series (ultraviolet region). If an electron jumps from or drops to the n=2 energy level, the series will be the Balmer series (visible region). For the n=3 energy level, the Paschen series (infrared region). For the n=4 energy level, the Brackett series.

A way to view this can be to ask which is the lowest energy level that the electron either jumps from or drops to. If the lowest energy level is n=1, then you know it has something to do with the Lyman series, n=2 the Balmer series, n=3 the Paschen series, etc.

I do not believe we have to know the names of the series though, but have a grasp of what light is associated with each series.


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