The emission of light by electrons occurs through a process called "electromagnetic radiation" or "electromission." When an electron undergoes a transition from a higher energy state to a lower energy state within an atom or a molecule, it releases energy in the form of electromagnetic radiation, which includes visible light.
Electrons within atoms or molecules occupy specific energy levels or orbitals. These energy levels are quantized, meaning they exist at distinct, well-defined energy values. The energy levels of electrons are determined by the specific characteristics of the atom or molecule, such as its atomic structure and the arrangement of electrons within it.
When an electron absorbs energy, it can move to a higher energy level or be excited to an excited state. This absorption of energy can occur through various processes, such as thermal excitation, electrical excitation, or the absorption of photons from external sources. Once the electron is in an excited state, it is considered to be in an unstable configuration.
To return to a lower energy state and stabilize itself, the excited electron releases the excess energy it gained during excitation. This energy is emitted as electromagnetic radiation, which can include visible light if the energy transition corresponds to the visible spectrum. The emitted light carries the energy difference between the higher and lower energy levels of the electron.
The specific color (wavelength) of the emitted light depends on the energy difference between the initial and final energy levels of the electron. Different atoms and molecules have characteristic energy level structures, resulting in specific patterns of emitted light. This phenomenon is the basis for spectroscopy, where scientists analyze the emitted or absorbed light to gain information about the atomic or molecular structure of a substance.
It's important to note that the emission of light by electrons is a quantum mechanical process. It is governed by the principles of quantum mechanics, which describe the behavior of particles on a microscopic scale, including the wave-particle duality of electrons and the quantized nature of their energy levels.