1. The problem statement, all variables and given/known data When an electron in a hydrogen atom makes a transiton between two levels with prinicipal quantum numbers n1 and n2, light is emitted with wavelength of 658.1 nm. If we assume that the energy levels of the atom are in agreement with the Bohr model, what are n1 and n2? 2. Relevant equations 3. The attempt at a solutionI tried to calculate: E = hc/λ = 3.022 * 10-19 which is the Energy for the wavelength. E = -hcR/n^2 n^2 = -hcR/E n^2 = -R/λ which result in negative value(?) Then I tried with λ = (n1^2 - n2^2)/R but then I always get two unknowns, and cant really come any further than that. Maybe Im looking in the wrong way or missing some theory.