posted by Vea on .
The following values are the only allowable energy levels of a hypothetical one-electron atom:
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
A) If the electron 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?
*I'm not sure where to start... does this have anything to do with the Rydberg equations? and if so, what do i plug in for n^2 final and initial?
a. N1=3 N2=infinity
b. N1=1 N2=infinity
short wavelength = highest frequency=highest energy
N1=4 N2 = infinity
N1, N2 final and initial