The Bhor Theory is a model proposed by Danish physicist Niels Bhor in the early 20th century to explain the behavior of electrons in an atom. It suggests that electrons orbit the nucleus of an atom at specific energy levels, and can only move between these levels by absorbing or emitting specific units of energy.
The Bhor Theory compares the energy levels of electrons in an atom to the angular momentum of their orbit. As an electron moves to a higher energy level, its angular momentum also increases. Conversely, when an electron moves to a lower energy level, its angular momentum decreases.
In the Bhor Theory, energy is measured in units of electron volts (eV), while angular momentum is measured in units of Planck's constant (h) divided by 2π. This unit is known as the reduced Planck's constant (ħ).
The Bhor Theory explains the spectral lines of elements by suggesting that when an electron moves from a higher energy level to a lower one, it emits a photon with a specific energy equal to the difference between the two levels. This energy corresponds to a specific wavelength of light, which creates the distinct spectral lines observed in the emission spectra of elements.
While the principles of the Bhor Theory have been incorporated into modern quantum mechanics, it is no longer considered a complete model of atomic behavior. It does not account for certain phenomena, such as electron spin, and has been replaced by more comprehensive models such as the Schrödinger equation.