Difference between revisions of "Sulfur oxoacids"

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The '''sulfur [[oxoacid]]s''' are chemical compounds that contain [[sulfur]], [[oxygen]] and [[hydrogen]]. The best known and most important industrially is [[sulfuric acid]]. Sulfur has a number of oxo acids; however, some of these are known only from their salts (these are shown in italics in the table below). The acids that have been characterised contain a variety of structural features, for example:  
+
The '''sulfur [[oxoacid]]s''' are chemical compounds that contain [[sulfur]], [[oxygen]] and [[hydrogen]]. The best known and most important industrially is [[sulfuric acid]]. Sulfur has a number of oxoacids; however, some of these are known only from their salts (these are shown in italics in the table below).<ref>{{Greenwood&Earnshaw1st|pages=834–54}}.</ref> The acids that have been characterised contain a variety of structural features, for example:  
 
*tetrahedral sulfur when  coordinated to oxygen
 
*tetrahedral sulfur when  coordinated to oxygen
 
*terminal and bridging oxygen atoms
 
*terminal and bridging oxygen atoms
 
*terminal and bridging peroxo groups
 
*terminal and bridging peroxo groups
 
*terminal S=S
 
*terminal S=S
−
*chains of (-S-)<sub>n</sub>
+
*chains of (–S–)<sub>n</sub>
  
 
{| class="wikitable"
 
{| class="wikitable"
 
|-
 
|-
−
| '''Acid'''
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! Acid
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| '''Formula'''
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! Formula
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| '''S oxdtn state'''
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! Sulfur oxidation state
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|'''Structure'''
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! Structure
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|'''Related anions'''
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! Related anions
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|'''Notes'''
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! Notes
 
|-
 
|-
−
|[[Sulfuric acid]]
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| [[Sulfuric acid]]
−
|H<sub>2</sub>SO<sub>4</sub>
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| H<sub>2</sub>SO<sub>4</sub>
 
| VI
 
| VI
−
|[[Image:Sulfuric-acid-2D.png|150px|sulfuric]]  
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| [[Image:Sulfuric-acid-2D.png|150px|sulfuric]]  
−
|[[Sulfate]], SO<sub>4</sub><sup>2<nowiki>&minus;</nowiki></sup> and hydrogen sulfate commonly known as [[bisulfate]]
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| [[Sulfate]], SO<sub>4</sub><sup>2−</sup> and hydrogen sulfate commonly known as [[bisulfate]]
−
|Best known and industrially significant
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| Best known and industrially significant
 
|-
 
|-
−
|[[Disulfuric acid]] or pyrosulfuric acid
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| [[Disulfuric acid]] or pyrosulfuric acid
−
|H<sub>2</sub>S<sub>2</sub>O<sub>7</sub>
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| H<sub>2</sub>S<sub>2</sub>O<sub>7</sub>
 
| VI
 
| VI
−
|[[Image:Disulfuric acid 2-D structure.png|150px|disulfuric]]
+
| [[Image:Disulfuric acid 2-D structure.png|150px|disulfuric]]
−
|Disulfate commonly known as [[pyrosulfate]], S<sub>2</sub>O<sub>7</sub><sup>2<nowiki>&minus;</nowiki></sup>
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| Disulfate commonly known as [[pyrosulfate]], S<sub>2</sub>O<sub>7</sub><sup>2−</sup>
−
|Pure form melts at 36°C. Present in fuming sulfuric acid, [[oleum]]
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| Pure form melts at 36&nbsp;°C. Present in fuming sulfuric acid, [[oleum]]
 
|-
 
|-
−
|[[Peroxymonosulfuric acid]]
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| [[Peroxymonosulfuric acid]]
−
|H<sub>2</sub>SO<sub>5</sub>
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| H<sub>2</sub>SO<sub>5</sub>
−
|VI
+
| VI
−
|[[Image:Peroxomonosulfuric acid 2-D structure.png|150px|peroxymonosulfuric]]
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| [[Image:Peroxomonosulfuric acid 2-D structure.png|150px|peroxymonosulfuric]]
−
|[[Peroxymonosulfate]], OOSO<sub>3</sub><sup>2<nowiki>&minus;</nowiki></sup>
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| [[Peroxymonosulfate]], OOSO<sub>3</sub><sup>2−</sup>
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|"Caro's acid", a solid melting at 45°C
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| "Caro's acid", a solid melting at 45&nbsp;°C
 
|-  
 
|-  
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|[[Peroxydisulfuric acid]]
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| [[Peroxydisulfuric acid]]
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|H<sub>2</sub>S<sub>2</sub>O<sub>8</sub>
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| H<sub>2</sub>S<sub>2</sub>O<sub>8</sub>
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|VI
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| VI
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|[[Image:Peroxodisulfuric_acid_2-D_structure.png|150px|peroxydisulfuric]]
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| [[Image:Peroxodisulfuric_acid_2-D_structure.png|150px|peroxydisulfuric]]
−
|[[Peroxydisulfate]], O<sub>3</sub>SOOSO<sub>3</sub><sup>2<nowiki>&minus;</nowiki></sup>
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| [[Peroxydisulfate]], O<sub>3</sub>SOOSO<sub>3</sub><sup>2−</sup>
−
|A solid melting at 65°C.
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| A solid melting at 65&nbsp;°C.
 
|-
 
|-
−
|''[[Dithionic acid]]''
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| ''[[Dithionic acid]]''
 
| H<sub>2</sub>S<sub>2</sub>O<sub>6</sub>
 
| H<sub>2</sub>S<sub>2</sub>O<sub>6</sub>
−
|V
+
| V
−
|[[Image:Dithionic acid 2-D structure.png|150px|dithionic]]
+
| [[Image:Dithionic acid 2-D structure.png|150px|dithionic]]
−
|[[Dithionate]], O<sub>3</sub>SSO<sub>3</sub><sup>2<nowiki>&minus;</nowiki></sup>
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| [[Dithionate]], O<sub>3</sub>SSO<sub>3</sub><sup>2−</sup>
−
|Not obtained pure, only concentrated solutions
+
| Not obtained pure, only concentrated solutions
 
|-
 
|-
−
|[[Thiosulfuric acid]]
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| [[Thiosulfuric acid]]
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|H<sub>2</sub>S<sub>2</sub>O<sub>3</sub>
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| H<sub>2</sub>S<sub>2</sub>O<sub>3</sub>
 
| IV
 
| IV
−
|[[Image:Thiosulfuric acid 2-D structure.png|150px|thiosulfuric]]
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| [[Image:Thiosulfuric acid 2-D structure.png|150px|thiosulfuric]]
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|[[Thiosulfate]], S<sub>2</sub>O<sub>3</sub><sup>2<nowiki>&minus;</nowiki></sup><br />[[Hydrogenthiosulfate]]  HS<sub>2</sub>O<sub>3</sub><sup>&minus;</sup> (ammonium salt prepared in anhydrous methanol at -80 °C <ref>''Raman spectroscopic discovery of the hydrogenthiosulphate anion, HSSO<sub>3</sub><sup><nowiki>&minus;</nowiki></sup>, in solid NH<sub>4</sub>HS<sub>2</sub>O<sub>3</sub> Steudel Rr.; Prenzel A Zeitschrift für Naturforschung 1989,44, 12, 1499-1502</ref>)    
+
| [[Thiosulfate]], S<sub>2</sub>O<sub>3</sub><sup>2−</sup><br />[[Hydrogenthiosulfate]]  HS<sub>2</sub>O<sub>3</sub><sup>−</sup> (ammonium salt prepared in anhydrous methanol at −80&nbsp;°C)<ref>{{citation | title = Raman spectroscopic discovery of the hydrogenthiosulphate anion, HSSO<sub>3</sub><sup>−</sup>, in solid NH<sub>4</sub>HS<sub>2</sub>O<sub>3</sub> | last1 = Steudel | first1 = R. | last2 = Prenzel | first2 = A. | journal = Z. Naturforsch. | year = 1989 | volume = 44 | issue = 12 | pages = 1499–1502}}.</ref>   
−
|Aqueous solutions decompose.
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| Aqueous solutions decompose.
 
|-
 
|-
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|''[[Disulfurous acid]]''
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| ''[[Disulfurous acid]]''
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|H<sub>2</sub>S<sub>2</sub>O<sub>5</sub>
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| H<sub>2</sub>S<sub>2</sub>O<sub>5</sub>
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|IV
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| IV
−
|[[Image:Disulfurous acid 2-D structure.png|150px|disulfurous]]
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| [[Image:Disulfurous acid 2-D structure.png|150px|disulfurous]]
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|Disulfite commonly known as [[metabisulfite]], S<sub>2</sub>O<sub>5</sub><sup>2<nowiki>&minus;</nowiki></sup>
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| Disulfite commonly known as [[metabisulfite]], S<sub>2</sub>O<sub>5</sub><sup>2−</sup>
−
|Not known
+
| Not known
 
|-
 
|-
−
|''[[Sulfurous acid]]''
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| ''[[Sulfurous acid]]''
 
| H<sub>2</sub>SO<sub>3</sub>
 
| H<sub>2</sub>SO<sub>3</sub>
−
|IV
+
| IV
−
|[[Image:Sulfurous acid 2-D structure.png|150px|sulfurous]]
+
| [[Image:Sulfurous acid 2-D structure.png|150px|sulfurous]]
−
|[[Bisulfite]], HSO<sub>3</sub><sup><nowiki>&minus;</nowiki></sup> and [[sulfite]], SO<sub>3</sub><sup>2<nowiki>&minus;</nowiki></sup>
+
| [[Bisulfite]], HSO<sub>3</sub><sup>−</sup> and [[sulfite]], SO<sub>3</sub><sup>2−</sup>
−
|Not known.
+
| Not known
 
|-
 
|-
−
|''[[Dithionous acid]]''
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| ''[[Dithionous acid]]''
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|H<sub>2</sub>S<sub>2</sub>O<sub>4</sub>
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| H<sub>2</sub>S<sub>2</sub>O<sub>4</sub>
−
|III
+
| III
−
|[[Image:Dithionous acid 2-D structure.png|150px|dithionous]]
+
| [[Image:Dithionous acid 2-D structure.png|150px|dithionous]]
−
|[[Dithionite]], O<sub>2</sub>SSO<sub>2</sub><sup>2<nowiki>&minus;</nowiki></sup>
+
| [[Dithionite]], O<sub>2</sub>SSO<sub>2</sub><sup>2−</sup>
−
|Not known.
+
| Not known.
 
|-
 
|-
−
|[[Polythionic acid]]
+
| [[Polythionic acid]]
−
|H<sub>2</sub>S<sub>x</sub>O<sub>6</sub>
+
| H<sub>2</sub>S<sub>''x''</sub>O<sub>6</sub>
 
|
 
|
−
|[[Image:Polythionic acid 2-D structure.png|150px|polythionic]]
+
| [[Image:Polythionic acid 2-D structure.png|150px|polythionic]]
−
|[[Polythionate]], O<sub>3</sub>S(S<sub>x-2</sub>)SO<sub>3</sub><sup>2<nowiki>&minus;</nowiki></sup>. Example [[tetrathionate]].
+
| [[Polythionate]], O<sub>3</sub>S(S<sub>''x''−2</sub>)SO<sub>3</sub><sup>2−</sup>. Example [[tetrathionate]].
−
|Examples known with x= 3, 4, 5, 6, 7, 8, 10, 12, 14.  
+
| Examples known with ''x''&nbsp;= 3, 4, 5, 6, 7, 8, 10, 12, 14.  
 
|}
 
|}
 +
 +
==References==
 +
{{reflist}}
  
 
==External links==
 
==External links==
 
* {{MeshName|Sulfur+Acids}} Sulfur oxoacids along with other acids containing sulfur
 
* {{MeshName|Sulfur+Acids}} Sulfur oxoacids along with other acids containing sulfur
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==Footnotes==
 
−
<references/>
 
−
{{Greenwood&Earnshaw}}
 
  
 
[[Category:Sulfur oxoacids|*]]
 
[[Category:Sulfur oxoacids|*]]
  
 
{{Imported from Wikipedia|name=Sulfur oxoacids|id=267814680}}
 
{{Imported from Wikipedia|name=Sulfur oxoacids|id=267814680}}

Revision as of 12:23, 20 August 2009

The sulfur oxoacids are chemical compounds that contain sulfur, oxygen and hydrogen. The best known and most important industrially is sulfuric acid. Sulfur has a number of oxoacids; however, some of these are known only from their salts (these are shown in italics in the table below).[1] The acids that have been characterised contain a variety of structural features, for example:

  • tetrahedral sulfur when coordinated to oxygen
  • terminal and bridging oxygen atoms
  • terminal and bridging peroxo groups
  • terminal S=S
  • chains of (–S–)n
Acid Formula Sulfur oxidation state Structure Related anions Notes
Sulfuric acid H2SO4 VI sulfuric Sulfate, SO42− and hydrogen sulfate commonly known as bisulfate Best known and industrially significant
Disulfuric acid or pyrosulfuric acid H2S2O7 VI disulfuric Disulfate commonly known as pyrosulfate, S2O72− Pure form melts at 36 °C. Present in fuming sulfuric acid, oleum
Peroxymonosulfuric acid H2SO5 VI peroxymonosulfuric Peroxymonosulfate, OOSO32− "Caro's acid", a solid melting at 45 °C
Peroxydisulfuric acid H2S2O8 VI peroxydisulfuric Peroxydisulfate, O3SOOSO32− A solid melting at 65 °C.
Dithionic acid H2S2O6 V dithionic Dithionate, O3SSO32− Not obtained pure, only concentrated solutions
Thiosulfuric acid H2S2O3 IV thiosulfuric Thiosulfate, S2O32−
Hydrogenthiosulfate HS2O3− (ammonium salt prepared in anhydrous methanol at −80 °C)[2] 		Aqueous solutions decompose.
Disulfurous acid H2S2O5 IV disulfurous Disulfite commonly known as metabisulfite, S2O52− Not known
Sulfurous acid H2SO3 IV sulfurous Bisulfite, HSO3− and sulfite, SO32− Not known
Dithionous acid H2S2O4 III dithionous Dithionite, O2SSO22− Not known.
Polythionic acid H2SxO6 polythionic Polythionate, O3S(Sx−2)SO32−. Example tetrathionate. Examples known with x = 3, 4, 5, 6, 7, 8, 10, 12, 14.

References

  1. ↑ Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; pp 834–54. ISBN 0-08-022057-6.
  2. ↑ Steudel, R.; Prenzel, A. Raman spectroscopic discovery of the hydrogenthiosulphate anion, HSSO3−, in solid NH4HS2O3. Z. Naturforsch. 1989, 44 (12), 1499–1502.

External links

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