Multiple Choice
Using the Bohr equation, calculate the wavelength of light emitted when an electron in a hydrogen atom transitions from n=3 to n=1.
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9. Quantum Mechanics
Bohr Equation
Multiple Choice
Using the Bohr Equation, determine the energy change associated with the electron transition from n=2 to n=5 in the hydrogen atom.
A
0.850 eV
B
0.306 eV
C
-0.850 eV
D
-0.306 eV
Verified step by step guidance1
Identify the initial and final energy levels for the electron transition: n_initial = 2 and n_final = 5.
Recall the Bohr Equation for the energy change in a hydrogen atom: ΔE = -R_H * (1/n_final^2 - 1/n_initial^2), where R_H is the Rydberg constant (13.6 eV for hydrogen).
Substitute the given energy levels into the Bohr Equation: ΔE = -13.6 eV * (1/5^2 - 1/2^2).
Calculate the values inside the parentheses: 1/5^2 = 1/25 and 1/2^2 = 1/4.
Subtract the two fractions: (1/25 - 1/4), then multiply the result by -13.6 eV to find the energy change ΔE.
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