Chemical Formula For Chlorite Ion
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| IUPAC name Chlorite | |
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| ECHA InfoCard | 100.123.477 |
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| Chemical formula | ClO − 2 |
| Molar mass | 67.452 |
| Cohabit acid | Chlorous acrid |
| Except where otherwise noted, information are given for materials in their standard country (at 25 °C [77 °F], 100 kPa). Infobox references | |
The chlorite ion, or chlorine dioxide anion, is the halite with the chemical formula of ClO −
ii . A chlorite (compound) is a chemical compound that contains this group, with chlorine in the oxidation state of +three. Chlorites are also known as salts of chlorous acrid.
Compounds [edit]
The free acid, chlorous acrid HClO2, is the least stable oxoacid of chlorine and has only been observed as an aqueous solution at low concentrations. Since it cannot be concentrated, it is not a commercial product. The alkali metal and alkaline earth metal compounds are all colorless or pale xanthous, with sodium chlorite (NaClO2) being the merely commercially of import chlorite. Heavy metallic chlorites (Ag+, Hg+, Tl+, Lead2+, and also Cu2+ and NH +
4 ) are unstable and decompose explosively with estrus or daze.[1]
Sodium chlorite is derived indirectly from sodium chlorate, NaClOthree. First, the explosively unstable gas chlorine dioxide, ClOii is produced past reducing sodium chlorate with a suitable reducing agent such as methanol, hydrogen peroxide, hydrochloric acid or sulfur dioxide.
Structure and properties [edit]
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 bail angle of 111° and Cl–O bond lengths of 156 pm.[ane] Chlorite is the strongest oxidiser of the chlorine oxyanions on the basis of standard half cell potentials.[2]
| Ion | Acidic reaction | East° (Five) | Neutral/bones reaction | Eastward° (5) |
|---|---|---|---|---|
| Hypochlorite | H+ + HOCl + e− → one⁄ii Cl2(thou) + HtwoO | 1.63 | ClO− + HtwoO + 2 e− → Cl− + 2 OH− | 0.89 |
| Chlorite | iii H+ + HOClO + 3 e− → 1⁄2 Clii(g) + ii H2O | 1.64 | ClO − two + two HtwoO + 4 due east− → Cl− + 4 OH− | 0.78 |
| Chlorate | 6 H+ + ClO − 3 + five due east− → 1⁄2 Cl2(thou) + 3 HtwoO | 1.47 | ClO − three + 3 HtwoO + 6 east− → Cl− + half dozen OH− | 0.63 |
| Perchlorate | eight H+ + ClO − 4 + 7 e− → one⁄2 Cl2(g) + 4 H2O | one.42 | ClO − 4 + four HiiO + 8 east− → Cl− + 8 OH− | 0.56 |
Uses [edit]
The most of import chlorite is sodium chlorite (NaClO2); this is used in the bleaching of textiles, pulp, and paper, however despite its strongly oxidizing nature information technology is frequently not used straight being instead used to generate the neutral species chlorine dioxide (ClO2), ordinarily via a reaction with HCl:
- 5 NaClO2 + iv HCl → 5 NaCl + 4 ClO2 + two H2O
Other oxyanions [edit]
Several oxyanions of chlorine exist, in which it tin can assume oxidation states of −1, +one, +iii, +five, or +7 within the corresponding anions Cl−, ClO−, ClO −
2 , ClO −
three , 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 | +ane | +3 | +5 | +7 |
|---|---|---|---|---|---|
| anion named | chloride | hypochlorite | chlorite | chlorate | perchlorate |
| formula | Cl− | ClO− | ClO − 2 | ClO − 3 | ClO − iv |
| structure |  |  |  |  |  |
Run across also [edit]
- Tetrachlorodecaoxide, a chlorite-based drug
- Chloryl, ClO +
2
References [edit]
- ^ a b Greenwood, North.Northward.; Earnshaw, A. (2006). Chemical science of the elements (2nd ed.). Oxford: Butterworth-Heinemann. p. 861. ISBN0750633654.
- ^ Cotton, F. Albert; Wilkinson, Geoffrey (1988), Advanced Inorganic Chemistry (5th ed.), New York: Wiley-Interscience, p. 564, ISBN0-471-84997-9
- Kirk-Othmer Concise Encyclopedia of Chemical science, Martin Grayson, Editor, John Wiley & Sons, Inc., 1985
Chemical Formula For Chlorite Ion,
Source: https://en.wikipedia.org/wiki/Chlorite
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