What is this problem asking me, and how would i solve it?

Question

A student determined that one of the lines in the hydrogen atom spectrum had a wavelength for which the calculated photon energy was 4.1 x 10-19 joules. To what electronic transition in the hydrogen atom should this line be assigned?

a. 7 - 2
b. 6 - 2
c. 5 - 2
d. 4 - 2
e. 3 - 2

I am not even sure what it is asking me to do?

Answer 1

Use the equation E = RH(1/nf^2 – 1/ni^2) where RH is the Rydberg constant = 2.180x10-18J; nf is the final energy level; and ni is the initial energy level.

For your question, you are looking for a value of E/RH = 4.1x10-19 / 2.180x10-18 = 1.88x10-1 = (1/nf^2 – 1/ni^2) Which of the possible answers will give 0.188?

a) 1/2^2 – 1/7^2 = 0.230
b) 1/2^2 – 1/6^2 = 0.222
c) 1/2^2 – 1/5^2 = 0.210
d) 1/2^2 – 1/4^2 = 0.188
e) 1/2^2 – 1/3^2 = 0.139

The answer is “d”, the transition from energy level 4 to energy level 2.

Answer 2

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Answer 3

They are asking you which orbital jump is made to produce that specific amount of energy. Think Principle Quantum Numbers...