Multiple Choice
The electron in a hydrogen atom absorbs a photon, causing the electron to jump from the state n = 2 to the state n = 6. What is the frequency of the absorbed photon in x 10^14 Hz?
9. Quantum Mechanics
Bohr Model
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The electron in a hydrogen atom absorbs a photon, causing the electron to jump from the state n = 3 to the state n = 5. The frequency of the absorbed photon was __________ × 10^14 Hz.
A
3.29
B
6.17
C
4.57
D
2.45
Verified step by step guidance1
Identify the initial and final energy levels of the electron in the hydrogen atom: n_initial = 3 and n_final = 5.
Use the Rydberg formula to calculate the change in energy (ΔE) when an electron transitions between two energy levels: ΔE = R_H * (1/n_initial^2 - 1/n_final^2), where R_H is the Rydberg constant (2.18 × 10^-18 J).
Calculate the energy difference (ΔE) using the given energy levels: ΔE = 2.18 × 10^-18 J * (1/3^2 - 1/5^2).
Convert the energy difference (ΔE) to frequency (ν) using the equation: ν = ΔE/h, where h is Planck's constant (6.626 × 10^-34 J·s).
Calculate the frequency (ν) of the absorbed photon and express it in the form of ν × 10^14 Hz.
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