The frequency of electromagnetic radiation associated with a quantum transition between atomic states.The transition frequency is the specific frequency of electromagnetic radiation that is emitted or absorbed when an atom or molecule makes a quantum jump between two discrete energy levels. This frequency is directly proportional to the energy difference between the two states, as described by the Planck-Einstein relation (E = hν). Because these energy levels are uniquely determined by the laws of quantum mechanics, the transition frequency acts as a precise fingerprint for each element and isotope, enabling highly accurate measurements and controls of atomic systems.
The concept originates from Niels Bohr's 1913 model of the hydrogen atom, which first quantized electron orbits and predicted specific spectral lines. The precise measurement of transition frequencies has since become a cornerstone of atomic physics, with the development of lasers in the 1960s enabling unprecedented accuracy.
When an atom absorbs a photon with an energy exactly matching the gap between two of its energy levels, an electron can transition to the higher-energy state. Conversely, when an electron spontaneously drops to a lower state, it emits a photon with that same characteristic frequency. The exact value of the frequency is influenced by the fine structure of the atom, including effects like electron spin and nuclear properties, which can be probed with extreme precision using techniques like laser spectroscopy.
Transition frequencies are the basis for atomic clocks, which use the microwave or optical transitions of atoms like cesium or strontium to define the second, and are also used in quantum computing to manipulate qubits and in GPS satellites for precise timekeeping.
The transition frequency of the hydrogen atom's 1S-2S transition is known to an accuracy of about 1 part in 10^15, making it one of the most precisely measured quantities in all of physics.




