Discrete allowed energies of a quantum system, such as an artificial atom or qubit.Energy levels are the discrete, quantized values of energy that a bound quantum system, such as an atom, molecule, or artificial atom, is allowed to possess. Unlike classical systems, where energy can vary continuously, quantum systems can only occupy specific energy states, with transitions between them occurring via absorption or emission of photons or other quanta. These levels are fundamental to understanding atomic spectra, chemical bonding, and the operation of devices like lasers and qubits.
The concept of discrete energy levels was introduced by Niels Bohr in 1913 to explain the hydrogen spectrum, and later formalized by Erwin Schrödinger's wave mechanics in 1926, which provided a general method for calculating energy levels from the system's Hamiltonian.
The discrete energy levels arise from the wave nature of quantum particles. When a particle is confined, for example by the electrostatic potential of a nucleus, its wavefunction must satisfy boundary conditions that allow only certain wavelengths, corresponding to specific energies. The lowest energy state is the ground state, and higher states are excited states. Transitions between levels occur when the system absorbs or emits a quantum of energy exactly equal to the difference between the levels, as described by the Bohr frequency condition.
Energy levels are exploited in lasers, where population inversion between levels enables stimulated emission, and in quantum computing, where the two lowest levels of an artificial atom define a qubit.
The energy levels of a hydrogen atom are so precisely known that their theoretical predictions match experimental measurements to better than one part in a trillion, making them one of the most accurate tests of quantum electrodynamics.




