Question

the following values are the only energy levels of a hypothetical one electron atom:
E6= -2x10^-19J, E4= -11x10^-19J, E2= -17x10^-19J, E5= -7x10^-19L, E3= -15x10^-19J, E1= -20x10^-1J
a: if the electon were in the n = 3 level, what would be the highest frequency and minimum wavelength of radiation that could be emitted?
b: what is the ionization energy in kJ/mol of the atom in its ground state?
c: if the electron were in the n = 4 level, what would be the shortest wavelength in nm of radiation that could be absorbed without causing ionization?

Answer 1

I think you must have made at least one typo (for E1 I suspect that is -20 x 10^-19 J).
a.
delta E = E3 - E1 = hc/wavelength
Substitute and solve for wavelength, convert to frequency by c = freq x wavelength.

b.
(0-E1) = ?

c.
delta E = E6-E4 = hc/wavelength and convert to nm.