1. The problem statement, all variables and given/known data In a set of experiments on a hypothetical one-electron atm, you measure the wavelengths of photons emitted as electrons return to the ground state (n=1), as shown in the energy level diagram. You also observe that it takes 17.50 eV to ionise this atom. Diagram shows: n=5 --> n=1 ~ λ = 73.86nm n=4 --> n=1 ~ λ = 75.63nm n=3 --> n=1 ~ λ = 79.76nm n=2 --> n=1 ~ λ = 94.54nm (i) What is the energy of the atom in each of the levels n=1 to n=5 (ii) If an electron makes a transition from the n=4 to the n=2 level, what wavelength of light would it emit? 2. Relevant equations None provided 3. The attempt at a solution My attempt at A I think i use this equation: E = -hxR/n^2 where: h is Planck's constant 6.626 x 10^-34 R is Rydbergs constant 1.097 x 10^7 and n is the energy level at n=5 i get: -2.907 x 10^-28 at n=4 i get: -4.543 x 10^-28 at n=3 i get: -8.076 x 10^-28 at n=2 i get: -1.817 x 10^-27 at n=1 i get: -7.269 x 10^-27 I think i use balmers equation in part B? 1/λ = R(1/2^2 - 1/4^2) where R= 1.097 x 10^7 1/λ = 2056875 I have a feeling i'm doing this all wrong.