The visible region of the hydrogen spectrum results from relaxation of electrons
ID: 556303 • Letter: T
Question
The visible region of the hydrogen spectrum results from relaxation of electrons from excited states to energy level 2. Use the Rydberg equation and your measured wavelengths to determine the energy transitions associated with each of your observed wavelengths for hydrogen. In other words, calculate the excited state energy level (n2) for each of your observed wavelengths for hydrogen. n has integer values; so, calculate it first with appropriate significant digits, then round it to an integer.
2. Energy Level from which the electron relaxed Observed Wavelengths from Hydrogen in nm: 485.10 nm 654.80 nm 1. Energy of a photon in J: 4.09E-19 3.04E-19 Correct ncorrei CorrectExplanation / Answer
A) Given that wavelength = 485.1 nm , Energy of photon = 4.09 x 10-19J , n1 = 2 , n2 = ?
1/ = R [1/n1^2 - 1/n2^2]
1/485.1 nm = 1.09678 x 10-2 nm-1 [1/2^2 - 1/n2^2] [ R = 1.09678 x 10-2 nm-1 ]
On simplification, n2 = 4
Therefore,
Energy level from which electron relaxed = 4
B) Given that wavelength = 654.8 nm , Energy of photon = 3.04 x 10-19J , n1 = 2 , n2 = ?
1/ = R [1/n1^2 - 1/n2^2]
1/654.8 nm = 1.09678 x 10-2 nm-1 [1/2^2 - 1/n2^2] [ R = 1.09678 x 10-2 nm-1 ]
On simplification, n2 = 3
Therefore,
Energy level from which electron relaxed = 3
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