Auger electron spectroscopy

related topics
{math, energy, light}
{acid, form, water}
{math, number, function}
{rate, high, increase}
{group, member, jewish}

Auger electron spectroscopy (AES; pronounced [oʒe] in French) is a common analytical technique used specifically in the study of surfaces and, more generally, in the area of materials science. Underlying the spectroscopic technique is the Auger effect, as it has come to be called, which is based on the analysis of energetic electrons emitted from an excited atom after a series of internal relaxation events. The Auger effect was discovered independently by both Lise Meitner and Pierre Auger in the 1920s. Though the discovery was made by Meitner and initially reported in the journal Zeitschrift für Physik in 1922, Auger is credited with the discovery in most of the scientific community.[1] Until the early 1950s Auger transitions were considered nuisance effects by spectroscopists, not containing much relevant material information, but studied so as to explain anomalies in x-ray spectroscopy data. Since 1953 however, AES has become a practical and straightforward characterization technique for probing chemical and compositional surface environments and has found applications in metallurgy, gas-phase chemistry, and throughout the microelectronics industry.[2][3][4][5]

Contents

Electron transitions and the Auger effect

The Auger effect is an electronic process at the heart of AES resulting from the inter- and intrastate transitions of electrons in an excited atom. When an atom is probed by an external mechanism, such as a photon or a beam of electrons with energies in the range of 2 keV to 50 keV, a core state electron can be removed leaving behind a hole. As this is an unstable state, the core hole can be filled by an outer shell electron, whereby the electron moving to the lower energy level loses an amount of energy equal to the difference in orbital energies. The transition energy can be coupled to a second outer shell electron which will be emitted from the atom if the transferred energy is greater than the orbital binding energy.[2][3][4][5][6][7] An emitted electron will have a kinetic energy of:

Full article ▸

related documents
Čerenkov radiation
Bremsstrahlung
Aperture
Comoving distance
Chandrasekhar limit
Luminosity
Superfluid
Shell model
Biot–Savart law
Crab Nebula
Star cluster
Electromagnetism
Pauli exclusion principle
Hall effect
Voyager 2
Ellipse
Apparent magnitude
Planetary science
Velocity
Geocentric model
Nucleon
Geographic coordinate system
Gaussian beam
Focal length
Alcubierre drive
Retrograde and direct motion
Map projection
Electrical impedance
Albedo
Galvanometer