## 1.11 [ENDORSED]

$c=\lambda v$

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Hyein Cha 2I
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### 1.11

So the question is

"In the spectrum of atomic hydrogen, several lines are generally classified together as belonging to a series(for ex, Balmer, Lyman, Paschen series), as shown in figs 1.1 ans 2.1. What is common to the lines within a series that makes grouping them togehter logical?"

I was confused in general about what these series are, or what their purpose is. Can someone please explain?
Also, what does 'the principal quantum number for the lower energy lvl' mean?

Thanks!

McKenna disc 1C
Posts: 60
Joined: Fri Sep 29, 2017 7:04 am

### Re: 1.11

This refers to the value of n for the lower energy level. For the Lyman series n=1 at the lower energy level, for example. In all honesty I don't know what these lines mean/their importance, so I am wondering that as well?

Shawn Patel 1I
Posts: 54
Joined: Thu Jul 27, 2017 3:01 am

### Re: 1.11  [ENDORSED]

Hey,

The series consist of the lines that are grouped together based on their lower energy principal quantum level. Each series has the same principal quantum number associated with them, so the Lyman series has a lower energy level of n=1. The series are just a convenient way to associate the lines. The lines are the wavelengths of radiation that are emitted, like how in the Balmer series, there are lines that are colored which show the visible spectrum of radiation. Principal quantum energy level means are just the overall energy levels of the atom.

I hope this helps.

AtreyiMitra2L
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Joined: Fri Sep 29, 2017 7:03 am
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### Re: 1.11

The question is basically referring what lower energy level the electron will jump to. Everything in the Lyman series (ie n = 2,3,4,5,6...) should jump to n = 1. Everything in the Balmer series should jump to n = 2. This is the same for the other two series. These two series are in reference to Hydrogen specifically. The lines represent where the incident light is actually absorbed and the electrons jump to a higher energy state. The lines are spaced because energy is quantized. To jump to the next energy level, a specific quanta must be achieved. There will only be a jump to the next energy state if the photons energy level is equal to the energy difference between the final and initial levels. The distance between the lines just show this phenomenon occurring.

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