Multiple Choice
Which electron transition in a hydrogen atom, starting from n = 10, will produce light of wavelength 3040 nm?
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9. Quantum Mechanics
Bohr Equation
Multiple Choice
What is the wavelength of light absorbed when an electron is promoted from the n=1 level to the n=2 level in a hydrogen atom, according to the Bohr model?
A
656 nm
B
486 nm
C
121 nm
D
434 nm
Verified step by step guidance1
Start by understanding the Bohr model, which describes the hydrogen atom's electron transitions between quantized energy levels. The energy difference between these levels can be calculated using the formula: , where is the Rydberg constant.
Calculate the energy difference between the n=1 and n=2 levels using the formula: . Substitute the values for and using the Bohr model formula.
Convert the energy difference to wavelength using the equation: , where is Planck's constant and is the speed of light.
Substitute the values for Planck's constant and the speed of light into the wavelength formula to find the wavelength of light absorbed.
Verify the calculated wavelength against the given options (656 nm, 486 nm, 121 nm, 434 nm) to ensure it matches the correct answer, which is 121 nm.
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