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November 21, 2014

November 21, 2014

Posted by **Vea** on Sunday, January 24, 2010 at 5:22pm.

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?

- Physics -
**bobpursley**, Sunday, January 24, 2010 at 5:28pma. N1=3 N2=infinity

b. N1=1 N2=infinity

short wavelength = highest frequency=highest energy

N1=4 N2 = infinity

N1, N2 final and initial

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