According to the Bohr model of the hydrogen atom, how is hydrogen's bright line spectrum produced?
When the one electron is moved from the orbit to far away.
The Bohr model of the hydrogen atom explains the production of hydrogen's bright line spectrum through the concept of electron energy levels and transitions.
In the Bohr model, electrons orbit the hydrogen nucleus in specific energy levels or shells. Each energy level corresponds to a specific amount of energy that an electron possesses. The lowest energy level, closest to the nucleus, is called the ground state.
When an electron absorbs energy, it moves to a higher energy level or excited state. This absorption of energy can occur through different processes, such as heating the hydrogen gas or exposing it to light or electricity.
However, electrons in the excited state are unstable and tend to return to their lower energy levels. When this happens, the excess energy is released in the form of electromagnetic radiation, which we see as light. The frequency or color of the emitted light depends on the energy difference between the excited state and the state the electron returns to.
Hydrogen's bright line spectrum consists of distinct lines of different colors or wavelengths. These lines represent the specific energy differences between the excited states and the ground state. Each line corresponds to a specific transition of an electron between energy levels.
The formula used to calculate the wavelength of these spectral lines is known as the Rydberg formula, which is given by:
1/λ = R_H[(1/n_f^2) - (1/n_i^2)]
Where:
- λ represents the wavelength of the emitted light.
- R_H is the Rydberg constant for hydrogen.
- n_f and n_i are the final and initial energy levels, respectively.
By using this formula, you can calculate the wavelengths of the spectral lines and determine the specific colors observed in hydrogen's bright line spectrum.