Electronic transition; Emission Spectra

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SUMMARY

The discussion focuses on calculating the initial energy level (ni) of an electron in a hydrogen atom based on a photon emitted during an electronic transition with a wavelength of 486.2 nm. The relevant equations include Energy = hc/wavelength and Energy = Rydberg's constant(1/n-final^2 - 1/n-initial^2). The user expressed difficulty in solving for two variables simultaneously, indicating a need for computational assistance to perform an iterative search for the energy levels.

PREREQUISITES
  • Understanding of electronic transitions in hydrogen atoms
  • Familiarity with Planck's constant and the speed of light
  • Knowledge of Rydberg's formula for energy levels
  • Basic programming skills for iterative calculations
NEXT STEPS
  • Learn to apply Rydberg's formula for different electronic transitions
  • Explore computational methods for solving simultaneous equations
  • Study the principles of photon emission and absorption in quantum mechanics
  • Investigate programming languages suitable for scientific calculations, such as Python or MATLAB
USEFUL FOR

Students studying quantum mechanics, physicists interested in atomic transitions, and educators teaching concepts related to electronic energy levels in hydrogen atoms.

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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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