Chlorite - wikipedia Chlorite For the mineral type, see chlorite group. For the neutral chemical compound, see chlorine dioxide. Chlorite Names IUPAC name Chlorite Identifiers CAS Number 14998 - 27 - 7 3D model ( JSmol ) Interactive image ChemSpider 170734 ECHA InfoCard 100.123. 477 EC Number 215 - 285 - 9 PubChem CID 197148 InChI InChI = 1S / ClHO2 / c2 - 1 - 3 / h ( H, 2, 3 ) / p - 1 Key : QBWCMBCROVPCKQ - UHFFFAOYSA - M SMILES ( O - ) Cl =O Properties Chemical formula ClO − Molar mass 67.452 Except where otherwise noted, data are given for materials in their standard state ( at 25 ° C ( 77 ° F ), 100 kPa ). Infobox references The chlorite ion, or chlorine dioxide anion, is ClO − 2. A chlorite ( compound ) is a compound that contains this group, with chlorine in oxidation state + 3. Chlorites are also known as salts of chlorous acid. Contents 1 Compounds 2 Structure and properties 3 Uses 4 Other oxyanions 5 See also 6 References Compounds See also : Category : Chlorites The free acid, chlorous acid HClO, is the least stable oxoacid of chlorine and has only been observed as an aqueous solution at low concentrations. Since it can not be concentrated, it is not a commercial product. The alkali metal and alkaline earth metal compounds are all colorless or pale yellow, with sodium chlorite ( NaClO ) being the only commercially important chlorite. Heavy metal chlorites ( Ag, Hg, Tl, Pb, and also Cu and NH + 4 ) are unstable and decompose explosively with heat or shock. Sodium chlorite is derived indirectly from sodium chlorate, NaClO. First, the explosively unstable gas chlorine dioxide, ClO is produced by reducing sodium chlorate in a strong acid solution with a suitable reducing agent ( for example, sodium chloride, sulfur dioxide, or hydrochloric acid ). Structure and properties The chlorite ion adopts a bent molecular geometry, due to the effects of the lone pairs on the chlorine atom, with an O -- Cl -- O bond angle of 111 ° and Cl -- O bond lengths of 156 pm. Chlorite is the strongest oxidiser of the chlorine oxyanions on the basis of standard half cell potentials. Ion Acidic reaction E ° ( V ) Neutral / basic reaction E ° ( V ) Hypochlorite H + HOCl + e → ⁄ Cl ( g ) + H O 1.63 ClO + H O + 2 e → Cl + 2 OH 0.89 Chlorite 3 H + HOClO + 3 e → ⁄ Cl ( g ) + 2 H O 1.64 ClO − 2 + 2 H O + 4 e → Cl + 4 OH 0.78 Chlorate 6 H + ClO − 3 + 5 e → ⁄ Cl ( g ) + 3 H O 1.47 ClO − 3 + 3 H O + 6 e → Cl + 6 OH 0.63 Perchlorate 8 H + ClO − 4 + 7 e → ⁄ Cl ( g ) + 4 H O 1.42 ClO − 4 + 4 H O + 8 e → Cl + 8 OH 0.56 Uses The most important chlorite is sodium chlorite ( NaClO ) ; this is used in the bleaching of textiles, pulp, and paper, however despite its strongly oxidizing nature it is often not used directly being instead used to generate the neutral species chlorine dioxide ( ClO ), normally via a reaction with HCl : 5 NaClO + 4 HCl → 5 NaCl + 4 ClO + 2 H O Other oxyanions Several oxyanions of chlorine exist, in which it can assume oxidation states of − 1, + 1, + 3, + 5, or + 7 within the corresponding anions Cl, ClO, ClO − 2, ClO − 3, or ClO − 4, known commonly and respectively as chloride, hypochlorite, chlorite, chlorate, and perchlorate. These are part of a greater family of other chlorine oxides. oxidation state − 1 + 1 + 3 + 5 + 7 anion named chloride hypochlorite chlorite chlorate perchlorate formula Cl ClO ClO − ClO − ClO − structure See also Tetrachlorodecaoxide, a chlorite based drug Chloryl, ClO References ^ Jump up to : Greenwood, N.N. ; Earnshaw, A. ( 2006 ). Chemistry of the elements ( 2nd ed. ). Oxford : Butterworth - Heinemann. p. 861. ISBN 0750633654. Jump up ^ Cotton, F. Albert ; Wilkinson, Geoffrey ( 1988 ), Advanced Inorganic Chemistry ( 5th ed. ), New York : Wiley - Interscience, p. 564, ISBN 0 - 471 - 84997 - 9 Kirk - Othmer Concise Encyclopedia of Chemistry, Martin Grayson, Editor, John Wiley & Sons, Inc., 1985 Retrieved from `` https://en.wikipedia.org/w/index.php?title=Chlorite&oldid=793577594 '' Categories : Chlorites Oxoanions Chlorine oxides Hidden categories : Articles without InChI source Articles without EBI source Articles without KEGG source Articles without UNII source ECHA InfoCard ID from Wikidata Articles containing unverified chemical infoboxes Talk Contents About Wikipedia Afrikaans Català Deutsch Español فارسی Français 한국어 Bahasa Indonesia Italiano Nederlands 日本 語 Norsk Русский Simple English Svenska Türkçe 中文 Edit links This page was last edited on 2 August 2017, at 16 : 51. Text is available under the Creative Commons Attribution - ShareAlike License ; additional terms may apply. By using this site, you agree to the Terms of Use and Privacy Policy. Wikipedia ® is a registered trademark of the Wikimedia Foundation, Inc., a non-profit organization. About Wikipedia

Question: give the name and formula for the acid derived from the following anion chlorite
Answer: chlorous acid