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206.83.67.100: Remove redundancy

2015-01-05T22:18:26Z

Remove redundancy

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	An '''electron acceptor''' is a chemical entity that accepts [[electron]]s transferred to it from another compound. It is an [[oxidizing agent]] that, by virtue of its accepting electrons, is itself [[redox\|reduced]] in the process.<ref>http://toxics.usgs.gov/definitions/electron_acceptor.html</ref>		Hello and welcome. My name is Figures Wunder. Puerto Rico is where he's been living for many years and he will never move. Body developing is 1 of the things I adore most. Hiring is my profession.<br><br>Feel free to surf to my blog post; [http://Www.Streaming.Iwarrior.net/user/WMcneil streaming.iwarrior.net]

	~~Typical oxidizing agents undergo permanent chemical alteration through covalent or ionic reaction chemistry, resulting in the complete~~ and ~~irreversible transfer of one or more electrons~~. ~~In many chemical circumstances, however, the transfer of electronic charge from an [[electron donor]] may be only fractional, meaning an electron~~ is ~~not completely transferred, but results in an electron resonance between the donor and acceptor~~. ~~This leads to the formation of [[charge transfer complex]]es in which the components largely retain their chemical identities.~~

	~~The electron accepting power of an acceptor molecule is measured by its [[electron affinity]] which is the energy released when filling the lowest unoccupied [[molecular orbital]] (LUMO).~~

	~~The overall energy balance (ΔE), i.e., energy gained or lost, in an electron donor-acceptor transfer~~ is ~~determined by the difference between the acceptor~~'s ~~electron affinity (A)~~ and ~~the [[ionization potential]] (I)~~ of the ~~electron donor:~~
	~~:<math>{\Delta}E=A-~~I~~\,</math>~~.

	~~In [[chemistry]], a class of electron acceptors that acquire not just one, but a set of two paired electrons that form a [[covalent bond]] with an electron donor molecule,~~ is ~~known as a [[Lewis acid]]. This phenomenon gives rise to the wide field of [[Lewis acids and bases\|Lewis acid-base]] chemistry~~.<~~ref~~>~~{{cite book \|title=The Lewis acid-base concepts : an overview \|last=Jensen \|first=W.B.\|year=1980 \|publisher=Wiley \|location=New York \|isbn=0-471-03902-0 }}~~<~~/ref~~> The driving forces for electron donor and acceptor behavior in chemistry is based on the concepts of [[electropositivity]] (for donors) and [[electronegativity]] (for acceptors) of atomic or molecular entities.

	~~==Examples==~~
	Examples of electron acceptors include [[oxygen]], [[nitrate]], [[iron]] (III), [[manganese]] (IV), [[sulfate]], [[carbon dioxide]], or in some [[microorganisms]] the [[chlorinated]] solvents such as [[tetrachloroethylene]] (PCE), [[trichloroethylene]] (TCE), [[dichloroethene]] (DCE), and [[vinyl chloride]] (VC). These reactions are of interest not only because they allow organisms to obtain energy, but also because they are involved in the natural [[biodegradation]] of organic contaminants. When clean-up professionals use monitored natural attenuation to ~~clean up contaminated sites, biodegradation is one of the major contributing processes.{{Citation needed\|date=March 2008}}~~

	In [[biology]], a ''terminal electron acceptor'' is a compound that receives or accepts an electron during [[cellular respiration]] or [[photosynthesis]]. All organisms obtain energy by transferring electrons from an electron donor to ~~an electron acceptor. During this process ([[electron transport chain]]) the electron acceptor is reduced and the electron donor is [[oxidized]].~~

	~~==See also==~~
	*[[redox\|Redox reactions]]
	*[[Semiconductor]]
	*[[Acceptor (semiconductors)]]

	~~==References==~~
	~~{{Reflist}}~~

	~~==External links==~~
	*[http://~~toxics~~.~~usgs~~.~~gov/definitions/electron_acceptor~~.~~html Electron acceptor definition at United States Geological Survey website]~~
	*[http://~~www.epa~~.~~gov/OUST/cat/tumgloss~~.~~htm Environmental Protection Agency]~~

	~~[[Category:Electrochemistry]~~]

en>Jochen Burghardt: /* References */

2013-11-24T20:40:38Z

References

← Older revision		Revision as of 22:40, 24 November 2013
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	~~Hi there~~, ~~I am Andrew Berryhill~~. ~~Some time ago she chose~~ to ~~reside~~ in ~~Alaska and her parents reside close~~ by. ~~To play lacross~~ is ~~some thing~~ I ~~truly appreciate doing~~. ~~Since he was eighteen he's been working~~ as ~~an info officer but he ideas on changing it~~.<br><br>~~Feel free~~ to ~~surf~~ to my website~~; real psychic readings [~~[http://~~findyourflirt~~.~~net~~/~~index~~.~~php?m=member_profile&p=profile&id=117823 continue reading this~~]]		An '''electron acceptor''' is a chemical entity that accepts [[electron]]s transferred to it from another compound. It is an [[oxidizing agent]] that, by virtue of its accepting electrons, is itself [[redox\|reduced]] in the process.<ref>http://toxics.usgs.gov/definitions/electron_acceptor.html</ref>

			Typical oxidizing agents undergo permanent chemical alteration through covalent or ionic reaction chemistry, resulting in the complete and irreversible transfer of one or more electrons. In many chemical circumstances, however, the transfer of electronic charge from an [[electron donor]] may be only fractional, meaning an electron is not completely transferred, but results in an electron resonance between the donor and acceptor. This leads to the formation of [[charge transfer complex]]es in which the components largely retain their chemical identities.

			The electron accepting power of an acceptor molecule is measured by its [[electron affinity]] which is the energy released when filling the lowest unoccupied [[molecular orbital]] (LUMO).

			The overall energy balance (ΔE), i.e., energy gained or lost, in an electron donor-acceptor transfer is determined by the difference between the acceptor's electron affinity (A) and the [[ionization potential]] (I) of the electron donor:
			:<math>{\Delta}E=A-I\,</math>.

			In [[chemistry]], a class of electron acceptors that acquire not just one, but a set of two paired electrons that form a [[covalent bond]] with an electron donor molecule, is known as a [[Lewis acid]]. This phenomenon gives rise to the wide field of [[Lewis acids and bases\|Lewis acid-base]] chemistry.<ref>{{cite book \|title=The Lewis acid-base concepts : an overview \|last=Jensen \|first=W.B.\|year=1980 \|publisher=Wiley \|location=New York \|isbn=0-471-03902-0 }}</ref> The driving forces for electron donor and acceptor behavior in chemistry is based on the concepts of [[electropositivity]] (for donors) and [[electronegativity]] (for acceptors) of atomic or molecular entities.

			==Examples==
			Examples of electron acceptors include [[oxygen]], [[nitrate]], [[iron]] (III), [[manganese]] (IV), [[sulfate]], [[carbon dioxide]], or in some [[microorganisms]] the [[chlorinated]] solvents such as [[tetrachloroethylene]] (PCE), [[trichloroethylene]] (TCE), [[dichloroethene]] (DCE), and [[vinyl chloride]] (VC). These reactions are of interest not only because they allow organisms to obtain energy, but also because they are involved in the natural [[biodegradation]] of organic contaminants. When clean-up professionals use monitored natural attenuation to clean up contaminated sites, biodegradation is one of the major contributing processes.{{Citation needed\|date=March 2008}}

			In [[biology]], a ''terminal electron acceptor'' is a compound that receives or accepts an electron during [[cellular respiration]] or [[photosynthesis]]. All organisms obtain energy by transferring electrons from an electron donor to an electron acceptor. During this process ([[electron transport chain]]) the electron acceptor is reduced and the electron donor is [[oxidized]].

			==See also==
			*[[redox\|Redox reactions]]
			*[[Semiconductor]]
			*[[Acceptor (semiconductors)]]

			==References==
			{{Reflist}}

			==External links==
			*[http://toxics.usgs.gov/definitions/electron_acceptor.html Electron acceptor definition at United States Geological Survey website]
			*[http://www.epa.gov/OUST/cat/tumgloss.htm Environmental Protection Agency]

			[[Category:Electrochemistry]]

en>BenTels: /* External links */ Not really a stub.

2012-08-23T06:34:29Z

External links: Not really a stub.

New page

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