Multiple Choice
Which statement best describes how the Bohr model explains both the discrete line spectra of hydrogen and the stability of electrons in atoms?
67
views
9. Quantum Mechanics
Bohr Model
Multiple Choice
According to the Bohr model of atomic quantization, what is the energy of photons emitted during an electron transition?
A
The energy equals the energy of the final level only: E = E_f
B
The energy equals the sum of the initial and final energy levels: E = E_i + E_f
C
The energy equals the difference between the initial and final energy levels: E = E_i - E_f
D
The energy equals the product of the initial and final energy levels: E = E_i imes E_f
Verified step by step guidance1
Understand that in the Bohr model, electrons occupy discrete energy levels, each with a specific energy value denoted as \(E_i\) for the initial level and \(E_f\) for the final level.
Recognize that when an electron transitions from a higher energy level (\(E_i\)) to a lower energy level (\(E_f\)), it emits a photon whose energy corresponds to the difference between these two levels.
Express the energy of the emitted photon as the difference between the initial and final energy levels: \(E = E_i - E_f\).
Note that this energy difference corresponds to the photon's energy, which can also be related to its frequency (\(\nu\)) and wavelength (\(\lambda\)) through the equation \(E = h \nu = \frac{hc}{\lambda}\), where \(h\) is Planck's constant and \(c\) is the speed of light.
Conclude that the correct expression for the energy of the emitted photon during an electron transition in the Bohr model is the difference between the initial and final energy levels, not their sum, product, or just the final energy.
Related Videos
Related Practice
