Stationary state

It is very similar to the concept of atomic orbital and molecular orbital in chemistry, with some slight differences explained below.

A stationary state is called stationary because the system remains in the same state as time elapses, in every observable way.

For a single-particle Hamiltonian, this means that the particle has a constant probability distribution for its position, its velocity, its spin, etc.

[1] (This is true assuming the particle's environment is also static, i.e. the Hamiltonian is unchanging in time.)

The wavefunction itself is not stationary: It continually changes its overall complex phase factor, so as to form a standing wave.

The oscillation frequency of the standing wave, multiplied by the Planck constant, is the energy of the state according to the Planck–Einstein relation.

is a linear operator on a vector space,

is plugged into the time-dependent Schrödinger equation, the result is[2]

Therefore, a stationary state is a standing wave that oscillates with an overall complex phase factor, and its oscillation angular frequency is equal to its energy divided by

As shown above, a stationary state is not mathematically constant:

However, all observable properties of the state are in fact constant in time.

represents a simple one-dimensional single-particle wavefunction

which is independent of the time t. The Heisenberg picture is an alternative mathematical formulation of quantum mechanics where stationary states are truly mathematically constant in time.

As mentioned above, these equations assume that the Hamiltonian is time-independent.

Spontaneous decay complicates the question of stationary states.

For example, according to simple (nonrelativistic) quantum mechanics, the hydrogen atom has many stationary states: 1s, 2s, 2p, and so on, are all stationary states.

But in reality, only the ground state 1s is truly "stationary": An electron in a higher energy level will spontaneously emit one or more photons to decay into the ground state.

[3] This seems to contradict the idea that stationary states should have unchanging properties.

The explanation is that the Hamiltonian used in nonrelativistic quantum mechanics is only an approximation to the Hamiltonian from quantum field theory.

are stationary states according to the approximate Hamiltonian, but not stationary according to the true Hamiltonian, because of vacuum fluctuations.

An orbital is a stationary state (or approximation thereof) of a one-electron atom or molecule; more specifically, an atomic orbital for an electron in an atom, or a molecular orbital for an electron in a molecule.

[4] For a molecule that contains only a single electron (e.g. atomic hydrogen or H2+), an orbital is exactly the same as a total stationary state of the molecule.

However, for a many-electron molecule, an orbital is completely different from a total stationary state, which is a many-particle state requiring a more complicated description (such as a Slater determinant).

This concept of an orbital is only meaningful under the approximation that if we ignore the electron–electron instantaneous repulsion terms in the Hamiltonian as a simplifying assumption, we can decompose the total eigenvector of a many-electron molecule into separate contributions from individual electron stationary states (orbitals), each of which are obtained under the one-electron approximation.

(Luckily, chemists and physicists can often (but not always) use this "single-electron approximation".)

In this sense, in a many-electron system, an orbital can be considered as the stationary state of an individual electron in the system.

In chemistry, calculation of molecular orbitals typically also assume the Born–Oppenheimer approximation.

A harmonic oscillator in classical mechanics (A–B) and quantum mechanics (C–H). In (A–B), a ball, attached to a spring , oscillates back and forth. (C–H) are six solutions to the Schrödinger equation for this situation. The horizontal axis is position, the vertical axis is the real part (blue) or imaginary part (red) of the wavefunction . (C, D, E, F), but not (G, H), are **stationary states** , or standing waves . The standing-wave oscillation frequency, multiplied by the Planck constant , is the energy of the state.

Three wavefunction solutions to the time-dependent Schrödinger equation for a harmonic oscillator . Left: The real part (blue) and imaginary part (red) of the wavefunction. Right: The probability of finding the particle at a certain position. The top two rows are two stationary states, and the bottom is the superposition state ${\textstyle \psi _{N}\equiv (\psi _{0}+\psi _{1})/{\sqrt {2}}}$ , which is not a stationary state. The right column illustrates why stationary states are called "stationary".