04-07-2018, 03:32 PM

I'm having trouble figuring this question out... I know that if I was dealing with hydrogen I would use the Rydberg constant and it would be smooth sailing, but I can't seem to find anyone online explaining how to solve this type of question when you are given energy differences between states and the atom is not hydrogen.

Any help is greatly appreciated.

The energy difference between n=2 and n=3 for an atom is 3.00x10-19 J and the energy difference between n=3 and n=4 is 2.00x10-19 J, if an electron makes a transition from n=4 to n=2 by emitting a photon, the wavelength of the emitted photon should be (express in nm)?

Any help is greatly appreciated.

The energy difference between n=2 and n=3 for an atom is 3.00x10-19 J and the energy difference between n=3 and n=4 is 2.00x10-19 J, if an electron makes a transition from n=4 to n=2 by emitting a photon, the wavelength of the emitted photon should be (express in nm)?