العربية
中国
Français
Deutsch
Ελληνική
हिन्दी
Italiano
日本語
Português
Русский
EspañolATOMIC PHYSICS
'Atomic physics' (or 'atom physics') is the field of physics that studies atoms as isolated systems comprised of electrons and an atomic nucleus. It is primarily concerned with the arrangement of electrons around the nucleus and
the processes by which these arrangements change. This clearly includes ions as well as neutral atoms and, unless otherwise stated, for the purposes of this discussion it should be assumed that the term ''atom'' includes ions.
The term ''atomic physics'' is often associated with nuclear power and nuclear bombs, due to the synonymous use of ''atomic'' and ''nuclear'' in standard English. However, physicists distinguish between atomic physics - which deals with the atom as
a system of electron(s) and a nucleus - and nuclear physics - which considers atomic nuclei alone.
As with many scientific fields, strict delineation can be highly contrived and atomic physics is often considered in the wider context of ''atomic, molecular, and optical physics''. Physics research groups are usually so classified.
Atomic physics always considers atoms in ''isolation'' - i.e. a model will consist of a single nucleus which may be surrounded by one or more bound electrons. It is 'not' concerned with the formation of molecules (although much of the physics is identical) nor does it examine atoms in a solid state as condensed matter. It 'is' concerned with processes such as
ionization and excitation by photons or collisions with atomic particles.
While modelling atoms in isolation may not seem realistic, if one considers atoms
in a gas or plasma then the time-scales for
atom-atom interactions are huge in comparison to the atomic processes that we are concerned with.
This means that the individual atoms can be treated as if each were in isolation because
for the vast majority of the time they are. By this consideration atomic physics provides the underlying theory in plasma physics and atmospheric physics
even though both deal with huge numbers of atoms.
Additionally, the properties of an atom in isolation is different from that of individual atoms in relatively close proximity to each other. This is because medium and long range forces come into play with proximity.
Electrons form notional shells around the nucleus. These are naturally in a ground state but can be excited
by the absorption of energy from light (photons), magnetic fields, or interaction with a colliding particle (typically other electrons). The excited electron may still be bound to the nucleus
and should, after a certain period of time, decay back to the original ground state. The energy is released as a photon. There
are strict selection rules as to the electronic configurations that can be reached by excitation by light - however there are no such rules for excitation by collision processes.
An electron may be sufficiently excited so that it breaks free of the nucleus and is no longer part of the atom. The remaining system is an ion and the atom is said to have been ionized having been left in a charged state.
The majority of fields in physics can be divided between theoretical work and experimental work
and atomic physics is no exception. It is usually the case, but not always, that progress goes
in alternate cycles from an experimental observation, through to a theoretical explanation
followed by some predictions which may or may not be confirmed by experiment, and so on. Of course, the current state of technology at any given time can put limitations on what can be achieved experimentally and theoretically so it may take considerable time for theory to be refined.
Clearly the earliest steps towards atomic physics was the recognition that matter was composed
of ''atoms'', in the modern sense of the basic unit of a chemical element. This theory was developed by the British chemist and physicist John Dalton in the 18th century. At this stage, it wasn't clear what atoms were although they could be described and classified by their properties (in bulk) in a periodic table.
The true beginning of atomic physics is marked by the discovery of spectral lines and attempts to describe the phenomenon, most notably by Joseph von Fraunhofer. The study of these lines led to the Bohr atom model and to the birth of quantum mechanics itself. In seeking to explain atomic spectra an entirely new mathematical model of matter was revealed. As far as atoms and their electron shells were concerned, not only did this yield a better overall description, i.e. the atomic orbital model, but it also provided a new theoretical basis for chemistry
(quantum chemistry) and spectroscopy.
Since the Second World War, both theoretical and experimental fields have advanced at a great pace. This can be attributed to progress in computing technology which has allowed bigger and more sophisticated models of atomic structure and associated collision processes. Similar technological advances in accelerators, detectors, magnetic field generation and lasers have greatly assisted experimental work.
; Pre quantum mechanics
★ John Dalton
★ Joseph von Fraunhofer
★ Johannes Rydberg
★ J.J. Thomson
; Post quantum mechanics
★ David Bates
★ Niels Bohr
★ Max Born
★ Clinton Joseph Davisson
★ Charlotte Froese Fischer
★ Vladimir Fock
★ Douglas Hartree
★ Harrie S. Massey
★ Nevill Mott
★ Mike Seaton
★ John C. Slater
★ George Paget Thomson
★ Energy level
★ Wavefunction
★ Atomic orbital
★ Electron configuration
★ SI units
★ Electron volt
★ Hartree
★ Rydberg
★ wavenumber
★ Plasma physics
★ Stellar atmosphere
★ Atmospheric physics
★ Atomic clock
★ Quantum optics
★ Molecular physics
★ Physics of Atoms and Molecules, Bransden, BH, , , Prentice Hall, 2002, ISBN 0-582-35692-X
★ Atomic Physics, Foot, CJ, , , Oxford University Press, 2004, ISBN 0-19-850696-1
★ Atomic Physics on the Internet
★ Atomic Physics Links
★ JILA (Atomic Physics)
the processes by which these arrangements change. This clearly includes ions as well as neutral atoms and, unless otherwise stated, for the purposes of this discussion it should be assumed that the term ''atom'' includes ions.
The term ''atomic physics'' is often associated with nuclear power and nuclear bombs, due to the synonymous use of ''atomic'' and ''nuclear'' in standard English. However, physicists distinguish between atomic physics - which deals with the atom as
a system of electron(s) and a nucleus - and nuclear physics - which considers atomic nuclei alone.
As with many scientific fields, strict delineation can be highly contrived and atomic physics is often considered in the wider context of ''atomic, molecular, and optical physics''. Physics research groups are usually so classified.
| Contents |
| Isolated atoms |
| Electronic configuration |
| History and developments |
| Significant atomic physicists |
| See also |
| Fundamental atomic physics |
| Common units |
| Applications |
| Related fields |
| References |
| External links |
Isolated atoms
Atomic physics always considers atoms in ''isolation'' - i.e. a model will consist of a single nucleus which may be surrounded by one or more bound electrons. It is 'not' concerned with the formation of molecules (although much of the physics is identical) nor does it examine atoms in a solid state as condensed matter. It 'is' concerned with processes such as
ionization and excitation by photons or collisions with atomic particles.
While modelling atoms in isolation may not seem realistic, if one considers atoms
in a gas or plasma then the time-scales for
atom-atom interactions are huge in comparison to the atomic processes that we are concerned with.
This means that the individual atoms can be treated as if each were in isolation because
for the vast majority of the time they are. By this consideration atomic physics provides the underlying theory in plasma physics and atmospheric physics
even though both deal with huge numbers of atoms.
Additionally, the properties of an atom in isolation is different from that of individual atoms in relatively close proximity to each other. This is because medium and long range forces come into play with proximity.
Electronic configuration
Electrons form notional shells around the nucleus. These are naturally in a ground state but can be excited
by the absorption of energy from light (photons), magnetic fields, or interaction with a colliding particle (typically other electrons). The excited electron may still be bound to the nucleus
and should, after a certain period of time, decay back to the original ground state. The energy is released as a photon. There
are strict selection rules as to the electronic configurations that can be reached by excitation by light - however there are no such rules for excitation by collision processes.
An electron may be sufficiently excited so that it breaks free of the nucleus and is no longer part of the atom. The remaining system is an ion and the atom is said to have been ionized having been left in a charged state.
History and developments
The majority of fields in physics can be divided between theoretical work and experimental work
and atomic physics is no exception. It is usually the case, but not always, that progress goes
in alternate cycles from an experimental observation, through to a theoretical explanation
followed by some predictions which may or may not be confirmed by experiment, and so on. Of course, the current state of technology at any given time can put limitations on what can be achieved experimentally and theoretically so it may take considerable time for theory to be refined.
Clearly the earliest steps towards atomic physics was the recognition that matter was composed
of ''atoms'', in the modern sense of the basic unit of a chemical element. This theory was developed by the British chemist and physicist John Dalton in the 18th century. At this stage, it wasn't clear what atoms were although they could be described and classified by their properties (in bulk) in a periodic table.
The true beginning of atomic physics is marked by the discovery of spectral lines and attempts to describe the phenomenon, most notably by Joseph von Fraunhofer. The study of these lines led to the Bohr atom model and to the birth of quantum mechanics itself. In seeking to explain atomic spectra an entirely new mathematical model of matter was revealed. As far as atoms and their electron shells were concerned, not only did this yield a better overall description, i.e. the atomic orbital model, but it also provided a new theoretical basis for chemistry
(quantum chemistry) and spectroscopy.
Since the Second World War, both theoretical and experimental fields have advanced at a great pace. This can be attributed to progress in computing technology which has allowed bigger and more sophisticated models of atomic structure and associated collision processes. Similar technological advances in accelerators, detectors, magnetic field generation and lasers have greatly assisted experimental work.
Significant atomic physicists
; Pre quantum mechanics
★ John Dalton
★ Joseph von Fraunhofer
★ Johannes Rydberg
★ J.J. Thomson
; Post quantum mechanics
★ David Bates
★ Niels Bohr
★ Max Born
★ Clinton Joseph Davisson
★ Charlotte Froese Fischer
★ Vladimir Fock
★ Douglas Hartree
★ Harrie S. Massey
★ Nevill Mott
★ Mike Seaton
★ John C. Slater
★ George Paget Thomson
See also
Fundamental atomic physics
★ Energy level
★ Wavefunction
★ Atomic orbital
★ Electron configuration
Common units
★ SI units
★ Electron volt
★ Hartree
★ Rydberg
★ wavenumber
Applications
★ Plasma physics
★ Stellar atmosphere
★ Atmospheric physics
★ Atomic clock
Related fields
★ Quantum optics
★ Molecular physics
References
★ Physics of Atoms and Molecules, Bransden, BH, , , Prentice Hall, 2002, ISBN 0-582-35692-X
★ Atomic Physics, Foot, CJ, , , Oxford University Press, 2004, ISBN 0-19-850696-1
External links
★ Atomic Physics on the Internet
★ Atomic Physics Links
★ JILA (Atomic Physics)
This article provided by Wikipedia. To edit the contents of this article, click here for original source.
psst.. try this: add to faves
