An energetically excited hydrogen atom has its electron in a 5f subshell. The electron drops down to the 3d subshell, releasing a photon in the process. What wavelength of light (in nm) is emitted by the process?

Answer 1

Use the same equation as in the previous problem.
1/wavelength in meters = R(1/n^2 - 1/n^2) where R is the Rydberg constant. You can look that up on the web for the EXACT number but it is about 1.097E7 but many more digits. The first n in the equation is nsubscript 1 and the second n is nsubscript 2. It works out as 1/wavelength = R(1/3^2 - 1/5^2) and I obtained about 1280 nm. By the way I found a spectral line calculator on the web. Here is the url. https://www.omnicalculator.com/physics/rydberg-equation
You shouldn't use this because it doesn't give you any practice on the math part that must be learned but it sure is nice to check your manual work. Post your work if you get stuck.