How do you calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level? Recall that for hydrogen #E_n# =#-2.18x10^-18# #J(1/n^2)#?
1 Answer
You can do it like this:
Explanation:
The energy of the electron is given by:
Where
We find the difference between the electrons energy in the
The difference in energy is given by:
To find the frequency of this emission line use the Planck Expression:
This transition is part of The Paschen Series of lines which occurs in the infra - red region of the electromagnetic spectrum.
This corresponds to a wavelength of 1094 nm.