6th edition 1.15

[CaminaB_1D]

I am having trouble figuring this out:

1.15 says "In the ultraviolet spectrum of atomic hydrogen, a line is observed at 102.6 nm. Determine the values of n for the initial and final energy levels of the electron during the emission of energy that leads to this spectral line."

I understand we are given the wavelength, but I am not sure where to start or what equation to use. I calculated the change in energy needed to emit that wavelength, not sure if that is in the right direction.

[Chem_Mod]

That is a good direction, now you can use the Rydberg formula, and the energy you calculated will be E.

[ryanhon2H]

The way I did it was using the Rydberg equation, which is

1/wavelength (in meters) = R(1/n₁² - 1/n₂²)

The wavelength is given, and R is the Rydberg constant. Since this is in the ultraviolet spectrum of hydrogen, it is the Lyman series, where n₁ is 1. Now all you need to do is plug in and solve for n₂.