1. The problem statement, all variables and given/known data Calculate the shortest wavelength photon that is emitted in the hydrogen atom. Energy when n = 1 = -13.6 eV 2. Relevant equations E = hc/λ λ = hc/E 3. The attempt at a solution Well as far as I understand, when the electron is in the n = 1 energy level it has it's lowest energy, which is -13.6 eV. I believe this is where the shortest wavelength will be... λ = hc/E = (4.14 x 10^-15 eV*s)(3.00 x 10^8 m/s) / -13.6 eV = approx 9.13 x 10^-8 m Was my method correct? I would really just like a second opinion. Thank you!