Help - energy of a photon :-/

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SUMMARY

The discussion focuses on calculating the energy of the highest energy photon produced in the hydrogen spectral series: Lyman, Balmer, Paschen, and Brackett. Participants confirm that after determining the shortest wavelength for each series, the next step is to compute the frequency using the formula \( c = \lambda \nu \). Subsequently, the energy can be calculated using the equation \( E = h\nu \), and converted to electron volts using the conversion factor \( 1 \text{ eV} = 1.602 \times 10^{-19} \text{ J} \).

PREREQUISITES
  • Understanding of the electromagnetic spectrum
  • Familiarity with the equations \( c = \lambda \nu \) and \( E = h\nu \)
  • Knowledge of the hydrogen spectral series
  • Basic understanding of energy conversion to electron volts
NEXT STEPS
  • Research the hydrogen spectral series in detail
  • Learn about the Planck constant and its application in photon energy calculations
  • Explore the relationship between wavelength, frequency, and energy in quantum mechanics
  • Study practical applications of spectral analysis in astrophysics
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Students in physics, educators teaching quantum mechanics, and anyone interested in the properties of light and atomic spectra.

Yael
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Hi,
i have a question...

compute the shortest wavelength in each of these hydrogen spectral series: Lyman, Balmer, Paschen, and Brackett. (which i managed...)

my problem is with the second part of the question : compute the energy in electron volts of the highest energy photon produced in each series.

any suggestions? :-/

Thanks !
 
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You have the wavelength, then you can calculate the frequency. After that you calculate the energy of the photons of each series. Then "translate" the energy into electron volts.
 
1 eV = 1.602x10^-19 J , i think this will help u to conver
 

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