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Given the wavelengths of emission lines: 463nm, 499.7nm, 660.6nm

I know how to use the equation but I don't

know how to find nf. Thank you!qa_attachment_1569941942093.jpg

qa_attachment_1569941942093.jpg

(a) You have previously determined (Section F) the wavelengths of the hydrogen
emission lines. Now determine the frequencies and energies of the light you
have observed from the hydrogen discharge tube.
/b) Determine exactly which electron transition (e.g., 2 - 1) corresponds to each
line in the spectrum you observed for hydrogen.
To do this, you will need to use the Rydberg equation regarding the energy differences
between the various allowed states for an electron in a hydrogen atom (given below).
At this point you should know all of the variables except for n;, the initial state of the
electron for each line observed. Hint: For emission of light, AE is negative since the
system is losing energy.
AE = Ry
2
n
n2
Ry = 2.18 X 10-18 Joules

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