The Bohr Model of the Hydrogen Atom

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A hydrogen atom in an excited state absorbs a photon with a wavelength of 434 nm, resulting in an energy difference of 2.825 eV between its initial and final states. The energy levels in the Bohr model are expressed as En = -E0/n^2. Participants suggest using a trial and error method to find transitions by calculating the energies of various levels and subtracting them. There is a discussion about the difficulty of finding a more algebraic solution for the quantum number "n." The conversation emphasizes the practical approach of plugging in values for "n" to identify the correct energy levels.
Shackleford
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A hydrogen atom in an excited state absorbs a photon of wavelength 434 nm. What were the initial and final states of the hydrogen atom?

E = hf = Eu - El = 2.825 eV

That's the difference in energy between the initial and final states.
 
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What's the expression for the energy levels in the Bohr model?
 
Doc Al said:
What's the expression for the energy levels in the Bohr model?

En = (- E0) / n^2
 
Shackleford said:
En = (- E0) / n^2
Good. Now start cranking out a few transitions and see if you can find a match. (The trial and error approach.)

Hint: List the energies of the first few levels and then you can just subtract.
 
Doc Al said:
Good. Now start cranking out a few transitions and see if you can find a match. (The trial and error approach.)

Seriously? That's all I have to do? Isn't there usually a fancy way to manipulate the equations algebraically and find the "n"s? I tried to find a fancy way to solve for the "n"s but couldn't. Okay. I'll start plugging in values for n.
 
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