Calculate the ni for the three strongest of the lines in the hydrogen spectrum.

Question

Calculate the n_i for the three strongest of the lines in the hydrogen spectrum.

1. The magnitude of ΔE_atom for the blue-violet wavelength 425nm?
2. n_i for the blue-violet wavelength
3. The magnitude of ΔE_atom for the blue-green wavelength 480nm?
4. n_i for the blue-green wavelength
5. The magnitude of ΔE_atom for the red wavelength 660nm?
6. n_i for the red wavelength

Answer 1

So Michael S.,

Badly phrased question! n(i) is not a single value here, you are making a transition between electron levels around a hydrogen atom. Take you Bohr equation for energy levels and start calculating whan transitions are possible that will give photons of those energies.

If you want to cheat a ittle, you could look up the hydrogen spectral series; they form named sets for particular end states for each related bunch of transitions. I think the first set is actually in the UV, if memory serves. That's one good reason why hydrogen flames are almost colorless in air. I wonder if a combustion front for H2 could be manipulated to lower its temperature and bring radiation from the flame into the second series (by dilution, or reaction with other oxidants than O2, etc.)?

-- Cheers, --mr. d.