Energy Level Diagram Homework: Get Started!

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SUMMARY

The discussion focuses on the energy level transitions of a monatomic gas when illuminated by visible light at a wavelength of 400nm. The initial energy state of the atoms is -5.0 eV, and upon absorption of the 400nm light, they emit radiation at both 400nm and 600nm. The energy of the excited state can be calculated using the photon energy equation E=hv, where v is the frequency derived from the wavelength. Additionally, the emitted radiation includes wavelengths outside the visible spectrum, which can be determined through further calculations.

PREREQUISITES
  • Understanding of photon energy calculations using E=hv
  • Knowledge of wavelength and frequency relationships (c=f*lambda)
  • Familiarity with atomic energy levels and transitions
  • Basic concepts of ionization energy in monatomic gases
NEXT STEPS
  • Research the calculation of photon energy using E=hv for different wavelengths
  • Learn about atomic spectra and the emission of photons during electron transitions
  • Study the concept of ionization energy and its implications in atomic physics
  • Explore resources on energy level diagrams and their applications in physics
USEFUL FOR

Students studying AP Physics, particularly those focusing on atomic structure and light interactions, as well as educators seeking to clarify concepts related to energy levels and photon emissions.

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Homework Statement


A monatomic gas is illuminated with visible light of wavelength 400nm. The gas is observed to absorb some of the light and subsequently emit visible light of both 400nm and 600nm. The initial state is -5.0 eV and the ionized atom (continuous energy levels) is 0 eV.
a) Draw the situation.
b) If the inital state of the atoms has energy -5 eV, what is the energy of the state to which the atoms were excited by the 400nm light?
c) At which other wavelength(s) outside the human visible range do these atoms emit radiation after they are excited by the 400nm light?

Homework Equations





The Attempt at a Solution


I wasn't in class when my teacher covered the material, and it's not in the book.
Can someone at least just get me started, explaining the drawing and what equations I should use?
 
Physics news on Phys.org
Anyone? Anyone?
 
try a post on the chemistry board.
 
But it's physics, AP physics actually. I've asked a few chem buds and they don't get it.
 
well you can calculate the energy of the photon from e=hv where v=frequency and of course c=f*lambda, different frequencies will be absorbed, the highest being that required to strip the electron (ionize) away= 5eV; alternatively, radiation is emitted in the form of a photon when an electron changes to a lower energy orbital. there should be scads of material online covering this as well as the calculations of these. here's one of hundreds: http://zebu.uoregon.edu/~soper/Light/atomspectra.html
 
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