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 $\frac{1}{\lambda _{\text{shortest}}}=\frac{\textit{RZ}^{2}}{\textit{n}_{\text{f}}^{2}}$ , where $R$ is the Rydberg constant and $Z$ is the number of protons in the nucleus.