Multiple Choice
The electron in a hydrogen atom absorbs a photon, causing the electron to jump from the state n = 3 to the state n = 6. The frequency of the absorbed photon was __________ x 10^14 Hz.
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9. Quantum Mechanics
Bohr Model
Multiple Choice
An electron in the n=6 level emits a photon with a wavelength of 410.2 nm. To what energy level does the electron move according to the Bohr Model?
A
n=5
B
n=3
C
n=2
D
n=4
Verified step by step guidance1
First, understand that the Bohr Model describes the electron transitions between energy levels in an atom, where the energy difference between levels is emitted or absorbed as a photon.
Use the Rydberg formula to calculate the wavelength of the emitted photon during the transition: , where is the Rydberg constant, is the wavelength, and and are the initial and final energy levels.
Substitute the given wavelength (410.2 nm) into the Rydberg formula and solve for the final energy level . Remember to convert the wavelength from nanometers to meters by multiplying by .
Rearrange the equation to solve for : . Calculate the value of using the known values.
Compare the calculated value of with the given options (n=5, n=3, n=2) to determine the correct energy level transition. The correct answer is n=4, which is not listed among the options, indicating a potential error in the problem statement.
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