Calculate Transition in Hydrogen for 600nm Wavelength

AI Thread Summary
To calculate the transition in hydrogen for a 600nm wavelength, the Rydberg formula is applied, leading to a frequency of approximately 5e14 Hz and an energy of 3.32e-19 J. The attempt to find the principal quantum number using the energy levels resulted in a negative value, indicating a misunderstanding of the transition process. The discussion highlights confusion around using the Rydberg constant and the correct application of energy equations for emission versus absorption. The user seeks clarification on their calculations and the proper interpretation of energy levels in hydrogen transitions. Overall, the thread emphasizes the complexities of quantum mechanics in relation to hydrogen's spectral lines.
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Homework Statement


use the RYDBERG formula to suggest a possible transition that would result in the observed wavelength


Homework Equations


Hydrogen - yellow wavelength about 600nm


The Attempt at a Solution


I used c= lambda x frequency(V) and found (V) to equal 5e14/second
I then used energy(E) = constant(h) x V and found E to equal 3.32e-19j
Last i used En = (-2.178e-18j)/n^2 to find the transition, I did 3.32e-19j = (-2.178e-18j)/n^2 and found n^2 to equal -6.57014 and I'm stuck there because it's a negative number...
 
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Rydberg formula contains two integers, not one.

What is Rydberg constant value?
 
I believe negative results infer emission rather than absorption.
 
That formula finds the principle energy level, not the energy emission or absorption
 
We haven't learned rydbergs constant yet, so I was assuming we used the one I posted
 
we haven'y learned that formula yet, he told us to use E(n) = (-2.178x10^-18)/n^2
 
ok well i did (change in energy) = E(f) - E(i)
delta(E) = 3.3e-19
E(f) = En when n=2
When n=2 E= -5.445e-19
so 3.3e-19 = -5.445e-19 - E(i)
E(i) = -8.745e-19
I then used E(i) = -2.178e-18/n2
i got n= 1.57815 which doesn't make sense, can anyone tell me what i did wrong?
 
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