The spectral lines observed for hydrogen arise from transitions from excited states back to the n=2 principle quantum level. Calculate the wavelengths associated with the spectral transitions of the hydrogen atom from the n=6,5,4 and 3 to the n=2 level.

These transitions to the n = 2 level are referred to as the Balmer Series of lines in the spectrum. Because the differences between energy levels are limited in number, so are the energies of the emitted photons.

Therefore only certain wavelengths (or frequencies) are observed for the spectral lines, thus discrete lines.

Wavelengths:

656 nm n = 3

486 nm n = 4

434 nm n = 5

410 nm n = 6

397 nm n = 7