Question

According to the Bohr model, what determines the shortest wavelength in a given series of wavelengths emitted by the atom?

• A. The quantum number $n_i$ that identifies the higher energy level from which the electron falls into a lower energy level.
• B. The quantum number $n_f$ that identifies the lower energy level into which the electron falls from a higher energy level.
• C. The ratio $n_f/n_i$ , where $n_f$ is the quantum number that identifies the lower energy level into which the electron falls and $n_i$ is the quantum number that identifies the higher level from which the electron falls.
• D. The sum $n_f+n_i$ of two quantum numbers, where $n_f$ identifies the lower energy level into which the electron falls and $n_i$ identifies the higher level from which the electron falls.

Answer 1

Answer: (B)

The shortest wavelength ${\lambda }_{\text{shortest}}$ in a given series can be calculated $\frac{1}{{\lambda }_{\text{shortest}}}=\frac{{\text{RZ}}^2}{{\text{n}}_{\text{f}}^2}$ , where $R$ is the Rydberg constant and $Z$ is the number of protons in the nucleus.