Energy level

This article is about orbital (electron) energy levels. For compounds' energy levels, see chemical potential.

A quantum mechanical system can only be in certain states, so that only certain energy levels are possible. The term energy level is most commonly used in reference to the electron configuration in atoms or molecules. In other words, the energy spectrum can be quantized (see continuous spectrum for the more general case).

As with classical potentials, the potential energy is usually set to zero at infinity, leading to a negative potential energy for bound electron states.

Energy levels are said to be degenerate, if the same energy level is obtained by more than one quantum mechanical state. They are then called degenerate energy levels.

The following sections of this article gives an overview over the most important factors that determine the energy levels of atoms and molecules.

Atoms

Intrinsic energy levels

Orbital state energy level

Assume an electron in a given atomic orbital. The energy of its state is mainly determined by the electrostatic interaction of the (negative) electron with the (positive) nucleus. The energy levels of an electron around a nucleus are given by :

Failed to parse (Missing texvc executable; please see math/README to configure.): E_n = - h c R_{\infty} \frac{Z^2}{n^2} \

,

where Failed to parse (Missing texvc executable; please see math/README to configure.): R_{\infty} \

is the Rydberg constant (typically between 1 eV and 103 eV), Z is the charge of the atom's nucleus, Failed to parse (Missing texvc executable; please see math/README to configure.): n \ 
is the principal quantum number, e is the charge of the electron, Failed to parse (Missing texvc executable; please see math/README to configure.):  h 
is Planck's constant, and c is the speed of light.

The Rydberg levels depend only on the principal quantum number Failed to parse (Missing texvc executable; please see math/README to configure.): n \ .

Fine structure splitting

Fine structure arises from relativistic kinetic energy corrections, spin-orbit coupling (an electrodynamic interaction between the electron's spin and motion and the nucleus's electric field) and the Darwin term (contact term interaction of s-shell electrons inside the nucleus). Typical magnitude Failed to parse (Missing texvc executable; please see math/README to configure.): 10^{-3}

eV.

Hyperfine structure

Spin-nuclear-spin coupling (see hyperfine structure). Typical magnitude Failed to parse (Missing texvc executable; please see math/README to configure.): 10^{-4}

eV.

Electrostatic interaction of an electron with other electrons

If there is more than one electron around the atom, electron-electron-interactions raise the energy level. These interactions are often neglected if the spatial overlap of the electron wavefunctions is low.

Energy levels due to external fields

Zeeman effect

Main article: Zeeman effect

The interaction energy is: Failed to parse (Missing texvc executable; please see math/README to configure.): U = - \mu B

with Failed to parse (Missing texvc executable; please see math/README to configure.): \mu = q L / 2m

Zeeman effect taking spin into account

This takes both the magnetic dipole moment due to the orbital angular momentum and the magnetic momentum arising from the electron spin into account.

Due to relativistic effects (Dirac equation), the magnetic moment arising from the electron spin is Failed to parse (Missing texvc executable; please see math/README to configure.): \mu = - \mu_B g s

with Failed to parse (Missing texvc executable; please see math/README to configure.): g
the gyro-magnetic factor (about 2). 

Failed to parse (Missing texvc executable; please see math/README to configure.): \mu = \mu_l + g \mu_s

The interaction energy therefore gets Failed to parse (Missing texvc executable; please see math/README to configure.): U_B = - \mu B = \mu_B B (m_l + g m_s) .

Stark effect

Interaction with an external electric field (see Stark effect).

Paschen-Back effect

For strong magnetic fields, the quantum numbers Failed to parse (Missing texvc executable; please see math/README to configure.): l, s, j, m_j

are not "good" any more and the Zeeman splitting does not give a correct description of the energy levels. This is known as the Paschen-Back effect.

Molecules

Roughly speaking, a molecular energy state, i.e. an eigenstate of the molecular Hamiltonian, is the sum of an electronic, vibrational, rotational and translational component, such that:

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where Failed to parse (Missing texvc executable; please see math/README to configure.): E_\mathrm{electronic}

is an eigenvalue of the electronic molecular Hamiltonian (the value of the potential energy surface) at the equilibrium geometry of the molecule.  

The molecular energy levels are labelled by the molecular term symbols.

The specific energies of these components vary with the specific energy state and the substance.

In molecular physics and quantum chemistry, an energy level is a quantized energy of a bound quantum mechanical state.

Crystalline Materials

Crystalline materials are often characterized by a number of important energy levels. The most important ones are the top of the valence band, the bottom of the conduction band, the Fermi energy, the vacuum level, and the energy levels of any defect states in the crystals.

See also

• Atomic Orbital
• Electron configuration
• Perturbation theory (quantum mechanics)
• Computational chemistry
• Potential energy surface
• Molecular term symbol
• Spectroscopyar:مستوى طاقة

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