I.
INTRODUCTION
A peroxide is a compound containing an oxygen–oxygen single bond or the peroxide anion. The group is called the peroxide the peroxide group or peroxo peroxo group. In contrast tooxide ions, the oxygen atoms in the peroxide ion have an oxidation state of −1. The simplest stable peroxide is hydrogen peroxide. Peroxide compounds can be roughly classified into organic and inorganic. hereas the inorganic peroxides have an ionic, salt!li"e character, the organic peroxides are dominated by the covalent b onds. The oxygen! oxygen chemical bond of peroxide is unstable and easily split into reactive radicals. #or this reason, peroxides are found in nature only in small $uantities, in %ater, atmosphere, plants, and animals. Peroxide ion formation has recently been highlighted as one of the main mechanisms by %hich oxides accommodate excess oxygen in ionic crystals and may have a large impact on a range of industrial applications including solid oxide fuel cells. &everal organic and inorganic peroxides are useful as bleach ing agents, as initiators of polymeri'ation reactions, and in the preparation ofhydrogen peroxide and other oxygen compounds. The negatively charged peroxide ion ()**!+ is present in inorganic compounds that may be regarded as salts of the very %ea"acid hydrogen peroxide examples are sodium peroxide (-a*)*+, a bleaching agent, andbarium peroxide (a)*+, formerly used as a source of hydrogen peroxide. Peroxides have a bleaching a bleaching effect on organic substances and therefore are added to some detergents and hair colorants. )ther large!scale applications include medicine andchemical industry, %here peroxides are used in various synthesis reactions or occur as intermediate products. ith ith an annual production of over * million tonnes, hydrogen peroxide is the most economically important peroxide. /any peroxides are unstable and ha'ardous substances they cannot be stored and therefore are synthesi'ed in situ and used immediately. /any inorganic peroxides are used for bleaching textiles and paper and as a bleaching additive to detergents and cleaning products. The increasing environmental concerns resulted in the preference of peroxides over chlorine!based compounds and a sharp increase in the peroxide production. The past use of perborates as additives to detergents and cleaning products has been largely replaced bypercarbonates in order to decrease the emission of boron to the environment. &odium percarbonate is used in such products as )xi0lean and Tide laundry detergent. hen dissolved in %ater, it releases hydrogen peroxide and soda ash (sodium carbonate+. &ome peroxide salts release oxygen upon reaction %ith carbon dioxide. This reaction is used in generation of oxygen from exhaled carbon dioxide on submarines and spaceships.
&odium or lithium peroxides are preferred in space applications because of their lo%er molar mass and therefore higher oxygen yield per unit %eight. Inorganic peroxides are used as oxidi'ing agents for digestion of organic samples and in the synthesis of organic peroxides. They react violently %ith reducing agents and %ith several classes of organic compounds to generate organic peroxide and hydroperoxide products. 2ry 0aro3s reagent (monopersulfuric acid 4 5*)* 6 con. 7*&)+ reacts readily %ith carbonyl compounds (in the synthesis of organic peroxides+ and can react explosively %ith aldehydes and alcohols.
II.
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/ost al"ali metal peroxides can be synthesi'ed directly by oxygenation of the elements. >ithium peroxide is form upon treating lithium hydroxide %ith hydrogen peroxide? 2 LiOH + H 2O2 → Li2O2 + 2 H2O
7istorically, barium peroxide is prepared by oxygenation of barium oxide at elevated temperature and pressure. 2 BaO + O2 → 2 BaO 2
arium peroxide %as once used to produce pure oxygen from air. This process relies on the temperature!dependent chemical balance bet%een barium oxide and peroxide? the reaction of barium oxide %ith air at @ B0 results in barium peroxide, %hich upon heating to above C B0 in oxygen decomposes bac" to barium oxide releasing pure oxygen.
III.
9&;& A-2 APP>I0ATI)-& A. Inorganic Peroxy 0ompounds
/any inorganic peroxides are used for bleaching textiles and paper and as a bleaching additive to detergents and cleaning products. The increasing environmental concerns resulted in the preference of peroxides over chlorine!based compounds and a sharp increase in the peroxide production. The past use of perborates as additives to detergents and cleaning products has been largely replaced bypercarbonates in order to decrease the emission of boron to the environment. &odium percarbonate is used in such products as )xi0lean and Tide laundry detergent. hen dissolved in %ater, it releases hydrogen peroxide and soda ash (sodium carbonate+. The use of peroxide compounds in detergents is often reflected in their trade names for example, Persil is a combination of the %ords per borate and sil icate.
. 7ydrogen Peroxide Industrial About DE of the %orldFs production of hydrogen peroxide is used for pulp! and paper!bleaching. The second maGor industrial application is the manufacture of sodium percarbonate and sodium perborate %hich are used as mild bleaches in laundry detergents. 7ydrogen peroxide is used in certain %aste!%ater treatment processes to remove organic impurities. This is achieved by advanced oxidation processes, such as the #enton reaction, %hich use it to generate highly reactive hydroxyl radicals (H)7+. These are able to destroy organic contaminates %hich are ordinarily difficult to remove, such as aromatic or halogenated compounds. It can also oxidi'e sulphur based compounds present in the %aste %hich is beneficial as it generally reduces their odour. /edical 2isinfectant ! 7ydrogen peroxide is seen as a n environmentally safe alternative to chlorine!based bleaches, as it degrades to form oxygen and %ater. It can be used for the disinfection of various surfaces. 7o%ever studies have found it to be ineffective in certain cases and hospitals and other medical institutions are no% being advised to use chlorine! based bleaches for disinfection. 0osmetics ! 7ydrogen Peroxide (bet%een 1.E and 1*E+ mixed %ith ammonium hydroxide is used to bleach human hair. The chemicalFs bleaching property lends its n ame to the phrase 6peroxide blonde6. 7ydrogen peroxide is also used for tooth %hitening and can be mixed %ith ba"ing soda and salt to ma"e a home!made toothpaste. Alternative ! Practitioners of alternative medicine have advocated the use of hydrogen peroxide for the treatment of various conditions, including emphysema, influen'a, AI2& and in particular cancer . oth the effectiveness and safety of hydrogen peroxide therapy is disputed by mainstream scientists. 7ydrogen peroxide is produced by the immune system but in a carefully controlled manner. Propellant 7igh concentration 7*)* is referred to as 7igh Test Peroxide (7TP+. It can be used either as a monopropellant (not mixed %ith fuel+ or as the oxidi'er componen t of a bipropellant roc"et. 9se as a monopropellant ta"es advantage of the decomposition of C–JKE concentration hydrogen peroxide into steam and oxygen.
;xplosives
7ydrogen peroxide has been used for creating organic peroxide based explosives, such as acetone peroxide, for improvised explosive devices. These explosives tend to degrade $uic"ly and hence are not used as commercial or military explosives.
)ther 9ses 7ydrogen peroxide has various domestic uses, primarily as a cleaning and disinfecting agent. a.+ :lo% stic"s 7ydrogen peroxide reacts %ith esters, such as cyalume and phenyl oxalate ester, to produce chemiluminescence this application is most commonly encountered in the form of glo% stic"s. b.+ 7orticulture &ome horticulturalists and users of hydroponics advocate the use of %ea" hydrogen peroxide solution in %atering solutions. Its spontaneous deco mposition releases oxygen that enhances a plantFs root development and helps to treat root rot (cellular root death due to lac" of oxygen+ and a variety of other pests.LDMLD1MLD*M c.+ #ish aeration >aboratory tests conducted by fish culturists in recent years have demonstrated that common household hydrogen peroxide can be used safely to provide oxygen for small fish. The hydrogen peroxide releases oxygen by decomposition %hen it is exposed to catalysts such as manganese dioxide.
IN.
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i"ipedia (*1@+. Peroxide. 8etrieved from http?OOen.%i"ipedia.orgO%i"iOPeroxide on #ebruary *1@. 0lar", 2onald ;. Peroxides and peroxide-forming compounds. 8etrieved from http?OOccc.chem.pitt.eduO%ipfOebO1D.pdf on #ebruary *1@ Taylor, Qanice. 34 Reasons Why You Need Hydrogen Peroxide In Your Home. 8etrieved from http?OO%%%.naturallivingideas.comOhydrogen!peroxide!usesO on @ #ebruary *1@ ;ncyclopedia ritannica (*1@+. Peroxide. 8etrieved from http?OO%%%.britannica.comO;chec"edOtopicO @*@Operoxide on @ #ebruary *1@ rin!ing Hydrogen Peroxide" 8etrieved from https?OOans%ers.yahoo.comO$uestionOindexR $idS*JCJ*1@DAA>I%DA on @ #ebruary *1@ i"ipedea (*1@+. #xidi$ing agent. 8etrieved from http?OOen.%i"ipedia.orgO %i"iO )xidi'ingagent on @ #ebruary *1@ i"ipedia (*1@+. Hydrogen Peroxide. 8etrieved from http?OOen.%i"ipedia.orgO%i"iO7ydrogenperoxide on @ #ebruary *1@ i"ipedia (*1@+. %ithium Peroxide. 8etrieved from http?OOen.%i"ipedia.org O%i"iO>ithiumperoxide on @ #ebruary *1@ i"ipedia (*1@+. &arium Peroxide. 8etrieved from http?OOen.%i"ipedia.org O%i"iOariumperoxide on @ #ebruary *1@
