Asked by Jodine
Why do electrons in hydrogen atoms emit infrared light when they make transitions to the n=3 energy level and uv light when they make transitions to the n=1 level?
Does this have to do with wavelengths?
Does this have to do with wavelengths?
Answers
Answered by
Damon
yes
The larger the energy loss in the transition, the higher the energy of the photon emitted.
The energy of a photon is proportional to its frequency.
therefore a transition from a higher level to n=1 will have a higher frequency (shorter wavelength) than a transition to the n=3 level
UV is higher frequency (shorter wave), infrared is lower frequency (longer wave)
The larger the energy loss in the transition, the higher the energy of the photon emitted.
The energy of a photon is proportional to its frequency.
therefore a transition from a higher level to n=1 will have a higher frequency (shorter wavelength) than a transition to the n=3 level
UV is higher frequency (shorter wave), infrared is lower frequency (longer wave)
Answered by
Jodine
Wow, Thanks, that helped a lot!
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