Two of the wavelengths emitted by a hydrogen atom are 102.6 nm and 1282 nm . I n

Question

Two of the wavelengths emitted by a hydrogen atom are 102.6 nm and 1282 nm . I need to know what n and m are for both wavelengths and if each is inferred, ultraviolet, or visible. Also, screenshot of my failed attempts:

I can confirm that this is not accepting n=1 as the answer.

Please help! Also, work would be helpful! I want to understand where I'm going wrong (because I can get three and one but nothing else). Thanks!

Part A What is the m value for the wavelength 102.6 nm? Express your answer as an integer. 2 m= Submit My Answers Give Up Incorrect; Try Again; 19 attempts remaining Part B What is the n value for the wavelength 102.6 nm? Express your answer as an integer. 2 L0487 n= Submit My Answers Give Up Incorrect; Try Again; 18 attempts remaining

Explanation / Answer

E = -Rh / n^2.

Rh = Rydberg's constant
= 13.6 eV
= 2.180 * 10^-18 J

Calculate the E for n = 1, n = 2, n = 3, n = 4, and n = 5. Then calculate the energy differences between two consecutive levels.

c = f
f = c/

E = hf
= hc/
= (6.626 * 10^-34 Js)(3.00 * 10^8 m/s) / (102.6 * 10^-9 m)
E 1.94 * 10^-18 J = 12.1 eV

This is more than the energy difference between n = 2 and n = 1.

so the transition is somwhere in between the states n = 1 and n = 2

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