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.
9. Quantum Mechanics
Bohr Equation
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple 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.
Related Videos
Related Practice
