The movement of an electron between energy states or molecules, often triggered by energy exchange.An electron transition is the movement of an electron from one energy level to another within an atom, molecule, or solid. This process is fundamental to all of chemistry and physics: it underlies the absorption and emission of light, chemical bonding, electrical conductivity, and many biological processes like photosynthesis. When an electron jumps to a higher energy level, energy is absorbed; when it falls to a lower level, energy is released, often as a photon. The specific energies involved are unique to each substance, providing a fingerprint for identifying materials.
The concept emerged from Niels Bohr's 1913 model of the hydrogen atom, which proposed discrete electron orbits and explained spectral lines as transitions between them. Later, quantum mechanics refined this into the modern understanding of electron wavefunctions and energy levels.
Electrons occupy discrete energy levels determined by quantum mechanics. A transition occurs when the electron gains or loses exactly the energy difference between two levels. This energy can come from absorbing a photon, colliding with another particle, or interacting with an electric field. The probability of a transition depends on quantum selection rules, which dictate which jumps are allowed. In molecules, transitions can also involve vibrational and rotational states, producing complex spectra. In solids, transitions between bands of energy levels govern whether a material conducts electricity or is an insulator.
Electron transitions are exploited in lasers, LEDs, solar cells, fluorescent lighting, and spectroscopy — a technique used in astronomy, medicine, and materials science to identify substances by their spectral signatures.
The green color of auroras is caused by a specific electron transition in oxygen atoms at high altitudes, where an electron drops from a metastable state and emits a 557.7 nm photon.






