Multiple Choice
According to the Bohr model, which of the following statements is true about the energy levels of a hydrogen atom?
9. Quantum Mechanics
Bohr Model
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
According to the Bohr model, what is the wavelength of light emitted when an electron transitions from the n=2 to the n=1 energy level in a hydrogen atom?
A
656.3 nm
B
121.6 nm
C
434.0 nm
D
486.1 nm
Verified step by step guidance1
Identify the initial and final energy levels for the electron transition: n=2 (initial) and n=1 (final).
Use the Rydberg formula to calculate the wavelength of light emitted during the transition: \( \frac{1}{\lambda} = R_H \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right) \), where \( R_H \) is the Rydberg constant (1.097 x 10^7 m^-1), \( n_1 \) is the final energy level, and \( n_2 \) is the initial energy level.
Substitute the values for \( n_1 = 1 \) and \( n_2 = 2 \) into the Rydberg formula: \( \frac{1}{\lambda} = 1.097 \times 10^7 \left( \frac{1}{1^2} - \frac{1}{2^2} \right) \).
Calculate the difference in the terms inside the parentheses: \( \frac{1}{1^2} - \frac{1}{2^2} = 1 - \frac{1}{4} = \frac{3}{4} \).
Solve for \( \lambda \) by taking the reciprocal of the product: \( \lambda = \frac{1}{1.097 \times 10^7 \times \frac{3}{4}} \).
2:43mWatch next
Master Bohr Model of the Atom with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
