Photon energies released during electron transitions have set values due to the electron moving from higher energy states to lower energy states (the states are quantized with discrete energy values). Interestingly, photons of similar energy values (quantized) can be absorbed to cause photons to move from lower energy states to higher energy states. An important consideration is the Bohr model established energies increasingly negative closest to the nucleus and an energy of zero for an electron dissociated from the atom. Problem#2. Determine the final principal energy level, nf, of an electron in the hydrogen atom when the atom with the electron in an excited state with n = 3 absorbs a photon of energy with wavelength of 8.225x102 nm (this photon is outside the visible spectrum ranging from 400nm (violet light) to 750nm (red light)) in the IR. What happened to electron? b) calculate the maximum wavelength, 1, of a photon (minimum energy) required to achieve the same result (recall the wavelength of light is inversely related to energy). What do we call the energy for this process