A hypothetical one-electron atom has these energy levels:
E6 = -2 x 10-19 J
E5 = -7 x 10-19 J
E4 = -11 x 10-19 J
E3 = -15 x 10-19 J
E2 = -17 x 10-19 J
E1 = -20 x 10-19 J
(This is not an actual atom that exists.According to the Bohr model, energies should follow the expression discussed in section 6.2 of Silberberg.This exercise prepares you for calculations like Questions 6 and 7 of Problem Set 1.)
(a) If the electron is initially in the n = 4 level, what is the shortest wavelength of radiation that could be emitted?Provide your answer to one significant figure: _______x10-7 m.
(b) What is the ionization energy (in kJ/mol) of the atom in its third excited state?Provide your answer to two significant figures: ______ kJ/mol