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Peroxydisulfate

Summary

The peroxydisulfate ion, S
2O2−
8, is an oxyanion, the anion of peroxydisulfuric acid. It is commonly referred to as persulfate, but this term also refers to the peroxomonosulfate ion, SO2−
5. It is also called peroxodisulfate.[2] Approximately 500,000 tons of salts containing this anion are produced annually. Important salts include sodium persulfate (Na2S2O8), potassium persulfate (K2S2O8), and ammonium persulfate ((NH4)2S2O8). These salts are colourless, water-soluble solids that are strong oxidants.[3]

Peroxydisulfate
Names
Other names
  • Peroxodisulfate
  • Persulfate[1]
Identifiers
  • 15092-81-6
3D model (JSmol)
  • Interactive image
ChEBI
  • CHEBI:29267
ChemSpider
  • 97014
  • 107879
UNII
  • 1SQ1481FEQ
  • InChI=1S/H2O8S2/c1-9(2,3)7-8-10(4,5)6/h(H,1,2,3)(H,4,5,6)/p-2
    Key: JRKICGRDRMAZLK-UHFFFAOYSA-L
  • [O-]S(=O)(=O)OOS([O-])(=O)=O
Properties
O8S2−2
Molar mass 192.11 g·mol−1
Conjugate acid Peroxydisulfuric acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Applications edit

Salts of peroxydisulfate are mainly used to initiate the polymerization of various alkenes, including styrene, acrylonitrile, and fluoroalkenes. Polymerization is initiated by the homolysis of the peroxydisulfate:

[O3SO–OSO3]2− ⇌ 2 [SO4]•−

Moreover, sodium peroxydisulfate can be used for soil and groundwater remediation, water and wastewater treatment, and etching of copper on circuit boards.[4][2]

It has also been used to produce hair lighteners and bleaches, medical drugs, cellophane, rubber, soaps, detergents, adhesive papers, dyes for textiles, and in photography.[2]

In addition to its major commercial applications, peroxydisulfate participates in reactions of interest in the laboratory:

Structure edit

Peroxydisulfate is a centrosymmetric anion. The O-O distance is 1.48 Å. The sulfur centers are tetrahedral.[5]

References edit

  1. ^ Ambiguous—see persulfate
  2. ^ a b c Shafiee, Saiful Arifin; Aarons, Jolyon; Hamzah, Hairul Hisham (2018). "Electroreduction of Peroxodisulfate: A Review of a Complicated Reaction". Journal of the Electrochemical Society. 165 (13): H785–H798. doi:10.1149/2.1161811jes. S2CID 106396614.
  3. ^ Harald Jakob, Stefan Leininger, Thomas Lehmann, Sylvia Jacobi, Sven Gutewort. "Peroxo Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_177.pub2. ISBN 978-3527306732.{{cite encyclopedia}}: CS1 maint: multiple names: authors list (link)
  4. ^ Wacławek, Stanisław; Lutze, Holger V.; Grübel, Klaudiusz; Padil, Vinod V.T.; Černík, Miroslav; Dionysiou, Dionysios.D. (2017). "Chemistry of persulfates in water and wastewater treatment: A review". Chemical Engineering Journal. 330: 44–62. doi:10.1016/j.cej.2017.07.132.
  5. ^ Allan, David R. (2006). "Sodium Peroxodisulfate". Acta Crystallographica Section E. 62 (3): i44–i46. doi:10.1107/S1600536806004302.