Atomic Spectra Module Question 39

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Kevin Pilcher 3J
Posts: 94
Joined: Wed Sep 30, 2020 9:40 pm

Atomic Spectra Module Question 39

Postby Kevin Pilcher 3J » Fri Oct 16, 2020 3:09 pm

Calculate the wavelength of the radiation emitted by a hydrogen atom when an electron makes a transition from n = 4 to n = 2.

How would we do the proper conversions to get the wavelength considering we already know the energy per photon from the previous question?

Rose_Malki_3G
Posts: 123
Joined: Wed Sep 30, 2020 10:02 pm

Re: Atomic Spectra Module Question 39

Postby Rose_Malki_3G » Fri Oct 16, 2020 3:51 pm

You use the change in n values to find the frequency of the light emitted (using the V = -R((1/n^2)-(1/n^2)) equation). And then once you get the frequency, you use the equation c = (frequency)(wavelength) to solve for the wavelength

Jenny Lee 2L
Posts: 94
Joined: Thu Oct 08, 2020 12:15 am

Re: Atomic Spectra Module Question 39

Postby Jenny Lee 2L » Fri Oct 16, 2020 6:07 pm

I believe that after you have the energy for both energy level n=4 and n=2, you subtract n=4 energy from n=2 energy to get the difference in energy. The positive difference in energy is the energy of the light emitted as well. Thus using E=hv you can find the frequency, the use c=(lambda)(frequency) to find lambda the wavelength.


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