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anonymous
 one year ago
Consider an electron in the second excited state of a hydrogen atom. Which of the photon wavelengths can the atom absorb?
a. 7.29 x 10^8m
b. 1.88x10^6m
The answer is B, I don't know how it was derived. I tried doing Rydberg equation but it just doesn't show.
anonymous
 one year ago
Consider an electron in the second excited state of a hydrogen atom. Which of the photon wavelengths can the atom absorb? a. 7.29 x 10^8m b. 1.88x10^6m The answer is B, I don't know how it was derived. I tried doing Rydberg equation but it just doesn't show.

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JFraser
 one year ago
Best ResponseYou've already chosen the best response.0You'd need to know what level it is transitioning to, in order to use rydberg

Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.2Using Bohr's levels, and the conservation of energy, we get this expression: \[\Large \lambda = \frac{{8\pi }}{3}\frac{{\hbar c}}{{{E_0}}}\] where E0=13.6 eV nevertheless, I get this final result: \[\Large \lambda = 1.21 \cdot {10^{  7}}meters\]
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