Electronic transition; Emission Spectra

AI Thread Summary
To determine the initial energy level (ni) of an electron transition in a hydrogen atom, the photon emitted has a wavelength of 486.2 nm, which corresponds to a specific energy calculated using the equation Energy = hc/wavelength. The energy can also be expressed using Rydberg's formula, relating the initial and final energy levels. The challenge arises from needing to solve for two variables simultaneously, leading to suggestions of using an iterative search or a computer program to find the solution. The discussion highlights the complexity of solving for initial energy levels in electronic transitions. Understanding these calculations is crucial for mastering concepts in quantum mechanics and atomic structure.
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Homework Statement



A photon emitted during an electronic transition in a hydrogen atom has a wavelength of 486.2
nm. From what initial energy level (ni) did the electron transition?

Homework Equations



Energy = hc/wavelength (h = Planck's constant; c is speed of light; and wavelength is 486.2 nm or 486.2 x 10^-9 meters).

Energy = Rydberg's constant(1/n-final^2 - 1/n-initial^2)

The Attempt at a Solution



I calculated the energy but I I can't solve for two variables at once in one equation. How am I supposed to find the initial energy level when I have the final energy level?
 
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An iterative search would soon find the levels ... a small computer program!
 

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