Electronic Transition
First calculate the frequency of light needed to energize an electron from the orbital to the orbital in a hydrogen atom. Which type of EM radiation is the light?
This section requires Javascript.
You are seeing this because something didn't load right. We suggest you, (a) try
refreshing the page, (b) enabling javascript if it is disabled on your browser and,
finally, (c)
loading the
non-javascript version of this page
. We're sorry about the hassle.
1 solution
Firstly use the Rydberg Formula specifically for a hydrogen atom to calculate the wavelength of the electromagnetic radiation emitted in vacuum.
Where l a m b d a , is the wavelength and n 1 and n 2 are the principal quantum numbers of the orbitals and R is the Rydberg constant.
After calculating the wavelength, use the wave-speed equation to find the frequency of the wave.
where v is 3 . 0 × 1 0 8 m s − 1 for all electromagnetic waves.
Finally, cross-reference the calculated frequency with the frequency table of the electromagnetic spectrum to find the type of wave emitted, which is UV-radiation!