A hypothetical atom (not hydrogen) has four electron bound states, with energy levels given in the diagram below. The gray band at E > 0 indicates the continuum of positive energy states for which the electron is not bound to the atom.

E>0 0 ev E4 = -0.6 ev E3 = - 1.4 ev E2 = -2.1 ev E1 = -3.1 ev Suppose the electron is initially in its ground state. (a) [6 pts] Explain what happens to the photon and the electron when orange light of wavelength 620nm is incident on the system. (b) [7 pts] Likewise explain what happens when the wavelength of the incident light is changed to 496nm (blue). (c) [7 pts] What if the wavelength is 310nm (ultraviolet)