An electronic transition is observed at 328.2 nm. Determine for this transition: the energy of a photon in Joules, the frequency in s-1, the wavenumber in cm-1, and the energy for one mole of these photons in Joules/mol. If this transition had corresponded to a spectral line of a He+ atom, what would have been the initial level for the emission of light at that wavelength? Remember that the equation of Rydberg is 1/ = ^2H { 1/nf^2  1/ni^2 } Determine the Rydberg constant if the difference between the wavelengths associated with the first emission line of the Balmer and Lyman series for He+ is equal to 297.3 nm.