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'''Klorit''', ClO<sub>2</sub><sup>−</sup> formülüyle göserilen bir kimyasal kök. Bileşiklerinde daima bir adet elektron alır.
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==Oxidation states==
Chlorine can assume oxidation states of −1, +1, +3, +5, or +7 corresponding to the anions Cl<sup>−</sup>, ClO<sup>−</sup>, ClO<sub>2</sub><sup>−</sup>, ClO<sub>3</sub><sup>−</sup>, or ClO<sub>4</sub><sup>−</sup>, respectively (known as chloride, hypochlorite, chlorite, chlorate, and perchlorate.)
{| border="1" cellspacing="0" cellpadding="2"
|-
! oxidation state
| −1
| +1
| +3
| +5
| +7
|-
! anion name
| [[chloride]]
| [[hypochlorite]]
| chlorite
| [[chlorate]]
| [[perchlorate]]
|-
! formula
| Cl<sup>−</sup>
| ClO<sup>−</sup>
| ClO<sub>2</sub><sup>−</sup>
| ClO<sub>3</sub><sup>−</sup>
| ClO<sub>4</sub><sup>−</sup>
|-
! structure
| [[Image:Chloride-ion-3D-vdW.png|50px|The chloride ion]]
| [[Image:Hypochlorite-3D-vdW.png|50px|The hypochlorite ion]]
| [[Image:Chlorite-3D-vdW.png|50px|The chlorite ion]]
| [[Image:Chlorate-3D-vdW.png|50px|The chlorate ion]]
| [[Image:Perchlorate-3D-vdW.png|50px|The perchlorate ion]]
|}
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==Örnekler==
* [[sodyum kloriti]], NaClO<sub>2</sub>
* [[magnezyum kloriti]], Mg(ClO<sub>2</sub>)<sub>2</sub>
==Klorun iyonları==
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==Manufacture==
{{Klor iyonları}}
The free acid, '''chlorous acid''', HClO<sub>2</sub>, is only stable at low concentrations. Since it cannot be concentrated, it is not a commercial product. However, the corresponding sodium salt, [[sodium chlorite]], NaClO<sub>2</sub> is stable and inexpensive enough to be commercially available. The corresponding salts of heavy metals (Ag<sup>+</sup>, Hg<sup>+</sup>, Tl<sup>+</sup>, Pb<sup>2+</sup>, and also Cu<sup>2+</sup> and NH<sub>4</sub><sup>+</sup>) decompose explosively with heat or shock.
[[Sodium chlorite]] is derived indirectly from [[sodium chlorate]], NaClO<sub>3</sub>. First, the explosively unstable gas [[chlorine dioxide]], ClO<sub>2</sub> 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). The [[chlorine dioxide]] is then absorbed into an alkaline solution and reduced with [[hydrogen peroxide]], H<sub>2</sub>O<sub>2</sub> yielding [[sodium chlorite]].
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==Kullanma==
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The main application of [[sodium chlorite]] is the generation of chlorine dioxide for bleaching and stripping of textiles, pulp, and paper. It is also used for disinfection in a few municipal water treatment plants after conversion to [[chlorine dioxide]]. An advantage in this application, as compared to the more commonly used chlorine, is that trihalomethanes are not produced from organic contaminants. [[Sodium chlorite]], NaClO<sub>2</sub> also finds application as a component of contact lens cleaning solution under the trade name purite.
==Kaynakça==
Sodium chlorite, like many oxidizers, should be protected from inadvertent contamination by organic materials to avoid the formation of an explosive mixture.
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==Referanslar==
*''Chemistry of the Elements'', N.N. Greenwood and A. Earnshaw, Pergamon Press, 1984.
*''Kirk-Othmer Concise Encyclopedia of Chemistry'', Martin Grayson, Editor, John Wiley & Sons, Inc., 1985
[[Kategori:Klor bileşikleri]]
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[[Category:Chlorites|Chlorites]]
[[Category:Oxoanions]]
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[[de:Chlorit (Chemie)]]
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