Peroxide: Difference between revisions
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{{Short description|Chemical compounds with the structure R–O–O–R'}} | {{Short description|Chemical compounds with the structure R–O–O–R'}} | ||
{{Other uses}} | {{Other uses}} | ||
{{about|the molecule|the ion|inorganic peroxide}} | |||
'''Peroxides''' are a group of [[molecules]] with the structure {{chem2|R\sO\sO\sR}}, where each R represents a radical (a portion of a complete molecule; not a [[free radical]]<ref>{{Cite web |title=Illustrated Glossary of Organic Chemistry |url=http://www.chem.ucla.edu/~harding/IGOC/R/r_group.html |access-date=June 19, 2024 |website=UCLA}}</ref>) and the O's are single [[oxygen]] atoms.<ref>{{Greenwood&Earnshaw2nd}}</ref>{{page missing|date=November 2025}}<ref>{{March6th}}</ref>{{page missing|date=November 2025}} Oxygen atoms are joined to each other and to adjacent elements through [[Single bond|single covalent bonds]], denoted by dashes or lines. The {{chem2|O\sO}} group in a peroxide is often called the '''peroxide group''', though some nomenclature discrepancies exist. This linkage is recognized as a common [[polyatomic ion]], and exists in many molecules. | |||
== General structure == | == General structure == | ||
The characteristic structure of any regular peroxide is the oxygen–oxygen covalent single bond, which connects the two main atoms together. Each oxygen atom has a oxidation state of negative one, as 5 of its [[Valence electron|valence electrons]] remain in the outermost [[Atomic orbital|orbital shell]] whilst one is occupied in the [[covalent bond]]. Because of the nature of the covalent bond, this arrangement results in each atom having the equivalent of 7 valence electrons, [[Redox|reducing]] the oxygens and giving them a negative charge. This charge is affected by the addition of other elements, with the properties and structure changing depending on the added group(s).{{Citation needed|date=November 2025}} | |||
The characteristic structure of any regular peroxide is the oxygen–oxygen covalent single bond, which connects the two main atoms together | |||
== Common forms == | == Common forms == | ||
[[File:Peroxide_group_v.2.png|left|thumb|324x324px|Types of peroxides, from top to bottom: peroxide ion, [[organic peroxide]], | [[File:Peroxide_group_v.2.png|left|thumb|324x324px|Types of peroxides, from top to bottom: [[peroxide ion]], [[organic peroxide]], [[hydroperoxide]], [[peracid]]. The peroxide group is marked in '''blue'''. R, R<sup>1</sup> and R<sup>2</sup> mark hydrocarbon [[Moiety (chemistry)|moieties]].]] | ||
The most common peroxide is [[hydrogen peroxide]] ({{chem2|H2O2}}), colloquially known simply as "peroxide". | The most common peroxide is [[hydrogen peroxide]] ({{chem2|H2O2}}), colloquially known simply as "peroxide".<ref>{{Cite web |title=Hydrogen Peroxide {{!}} Hydrite.com |url=https://www.hydrite.com/Product/industrial/Hydrogen-Peroxide.htm |access-date=2025-11-12 |website=www.hydrite.com}}</ref> Many organic peroxides are known as well. | ||
In addition to hydrogen peroxide, some other major classes of peroxides are: | In addition to hydrogen peroxide, some other major classes of peroxides are: | ||
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* [[Metal peroxide|Metal peroxides]], examples being [[barium peroxide]] ({{chem2|BaO2}}), [[sodium peroxide]] ({{chem2|Na2O2}}) and [[zinc peroxide]] ({{chem2|ZnO2}}). | * [[Metal peroxide|Metal peroxides]], examples being [[barium peroxide]] ({{chem2|BaO2}}), [[sodium peroxide]] ({{chem2|Na2O2}}) and [[zinc peroxide]] ({{chem2|ZnO2}}). | ||
* [[Organic peroxide|Organic peroxides]], compounds with the linkage {{chem2|C\sO\sO\sC}} or {{chem2|C\sO\sO\sH}}. One example is [[Tert-Butyl hydroperoxide|''tert''-butylhydroperoxide]]. | * [[Organic peroxide|Organic peroxides]], compounds with the linkage {{chem2|C\sO\sO\sC}} or {{chem2|C\sO\sO\sH}}. One example is [[Tert-Butyl hydroperoxide|''tert''-butylhydroperoxide]]. | ||
== Nomenclature == | == Nomenclature == | ||
Latest revision as of 03:32, 12 November 2025
Template:Short description Script error: No such module "other uses". Script error: No such module "about". Peroxides are a group of molecules with the structure Template:Chem2, where each R represents a radical (a portion of a complete molecule; not a free radical[1]) and the O's are single oxygen atoms.[2]Template:Page missing[3]Template:Page missing Oxygen atoms are joined to each other and to adjacent elements through single covalent bonds, denoted by dashes or lines. The Template:Chem2 group in a peroxide is often called the peroxide group, though some nomenclature discrepancies exist. This linkage is recognized as a common polyatomic ion, and exists in many molecules.
General structure
The characteristic structure of any regular peroxide is the oxygen–oxygen covalent single bond, which connects the two main atoms together. Each oxygen atom has a oxidation state of negative one, as 5 of its valence electrons remain in the outermost orbital shell whilst one is occupied in the covalent bond. Because of the nature of the covalent bond, this arrangement results in each atom having the equivalent of 7 valence electrons, reducing the oxygens and giving them a negative charge. This charge is affected by the addition of other elements, with the properties and structure changing depending on the added group(s).Script error: No such module "Unsubst".
Common forms
The most common peroxide is hydrogen peroxide (Template:Chem2), colloquially known simply as "peroxide".[4] Many organic peroxides are known as well.
In addition to hydrogen peroxide, some other major classes of peroxides are:
- Peroxy acids, the peroxy derivatives of many familiar acids, examples being peroxymonosulfuric acid and peracetic acid, and their salts, one example of which is potassium peroxydisulfate.
- Main group peroxides, compounds with the linkage Template:Chem2 (E = main group element).Template:Multiple image
- Metal peroxides, examples being barium peroxide (Template:Chem2), sodium peroxide (Template:Chem2) and zinc peroxide (Template:Chem2).
- Organic peroxides, compounds with the linkage Template:Chem2 or Template:Chem2. One example is tert-butylhydroperoxide.
Nomenclature
The linkage between the oxygen molecules is known as a peroxy group (sometimes called peroxo group, peroxyl group, of peroxy linkage). The nomenclature of the peroxy group is somewhat variable,[5] and exists as an exception to the rules of naming polyatomic ions. This is because, when it was discovered, it was believed to be monatomic.[6] The term was introduced by Thomas Thomson in 1804 for a compound combined with as much oxygen as possible,[7] or the oxide with the greatest quantity of oxygen.[8]
References
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