1. The problem statement, all variables and given/known data Between which two orbits of the Bohr hydrogen atom must an electron fall to produce light of wavelength 954.8 nm ? 2. Relevant equations E = hv E = R(1/n1^2 - 1/n2^2) 3. The attempt at a solution I've got it down to the differences in the reciprocals of the squares of the energy levels = .09548. I don't know how to calculate each n though. I've tried randomly plugging in different n's to see if i get .09548, but that's not getting me anywhere.