In: Physics
You measure the emission spectrum of hydrogen gas, and see many discrete wavelengths in the emission, of which, one is 102.6nm. To what initial and final states can this wavelength be attributed?. (hint, use a little trial and error to get the intergers)
Some energy Levels and Transition Lines are shown in figure given below..
Corresponding energy equation of photon emmision is given by..
Ephoton = E0( | 1 | − | 1 | ) |
n12 | n22 |
Where,
E0 = -13.6 eV
Given, = 102.6 nm
So, Energy corresponding to emmision of photon with wavelength 102.6 nm is Ephoton.
where,
By substituting value of we got
Ephoton = 12.09 eV
1.) Let electron coming from state 2 to 1
From energy level diagram shown above we got,
E1 - E2= - 10.2 eV
Ephoton
Negative because electron is coming in lower energy state from higher one by releasing photon of equivalent energy.
So, energy released by H-atom in this case is 10.2 which isn't equal to Ephoton.
It's isn't state 2 to 1 jump.
2.) Let electron coming from state 3 to 1
E1 - E3= - 12.10 eV -
12.09 = Ephoton
Again, negative because electron is coming in lower energy state from higher one by releasing photon of equivalent energy
It's nearly equal to energy corresponding to a emmited photon with wavelength of 102.6 nm.
Hence for the given data and conditions, electron is undergoing jump from Energy state 3 to Energy state 1 .