Jump to content

Persulfate: Difference between revisions

From Wikipedia, the free encyclopedia
Browse history interactively
← Previous edit
Content deleted Content added
VisualWikitext
m →top: task, replaced: Journal of The Electrochemical Society → Journal of the Electrochemical Society
→Example salts: invalid link. removed.
 
(17 intermediate revisions by 13 users not shown)
Line 1: Line 1:
{{Short description|Class of chemical compounds}}
The term '''persulfate''' (sometimes known as peroxysulfate or peroxodisulfate)<ref>{{Cite journal|last=Shafiee|first=Saiful Arifin|last2=Aarons|first2=Jolyon|last3=Hamzah|first3=Hairul Hisham|date=|year=2018|title=Electroreduction of Peroxodisulfate: A Review of a Complicated Reaction|url=http://m.jes.ecsdl.org/content/165/13/H785.abstract?sid=3ddef67b-7f3b-49fa-93a7-c6eee812bfe4|journal=Journal of the Electrochemical Society|publisher=ECS|volume=165|issue=13|pages=H785-H798|doi=10.1149/2.1161811jes|via=}}</ref> refers to ions or compounds containing the anions {{chem|SO|5|2−}} or {{chem|S|2|O|8|2−}}.<ref name = Ullmann>{{Ullmann | title = Peroxo Compounds, Inorganic | author = Harald Jakob, Stefan Leininger, Thomas Lehmann, Sylvia Jacobi, Sven Gutewort | doi = 10.1002/14356007.a19_177.pub2}}</ref> The anion {{chem|SO|5|2−}} contains one peroxide group per sulfur center, whereas in {{chem|S|2|O|8|2−}}, the peroxide group bridges the sulfur atoms. In both cases, sulfur adopts the normal tetrahedral geometry typical for the S(VI) oxidation state. These salts are strong oxidizers.<ref>{{cite web|url=http://geocleanse.com/persulfate.asp |title=Geo-Cleanse International |publisher=Geocleanse.com |date= |accessdate=2012-06-13}}</ref><ref>{{cite web|url=https://www.sciencedirect.com/science/article/pii/S1385894717312718 |author = Wacławek, S., Lutze, H. V., Grübel, K., Padil, V.V.T., Černík, M., Dionysiou, D.D. (2017) |title=Chemistry of persulfates in water and wastewater treatment: A review. |doi = 10.1016/j.cej.2017.07.132}}</ref>
A '''persulfate''' (sometimes known as peroxysulfate or peroxodisulfate)<ref>{{Cite journal|last1=Shafiee|first1=Saiful Arifin|last2=Aarons|first2=Jolyon|last3=Hamzah|first3=Hairul Hisham|year=2018|title=Electroreduction of Peroxodisulfate: A Review of a Complicated Reaction|url=http://m.jes.ecsdl.org/content/165/13/H785.abstract?sid=3ddef67b-7f3b-49fa-93a7-c6eee812bfe4|journal=Journal of the Electrochemical Society|volume=165|issue=13|pages=H785–H798|doi=10.1149/2.1161811jes|s2cid=106396614 |doi-access=free}}</ref> is a compound containing the [[anion]]s {{chem|SO|5|2−}} or {{chem|S|2|O|8|2−}}.<ref name = Ullmann>{{Ullmann | title = Peroxo Compounds, Inorganic | author = Harald Jakob, Stefan Leininger, Thomas Lehmann, Sylvia Jacobi, Sven Gutewort | doi = 10.1002/14356007.a19_177.pub2}}</ref> The anion {{chem|SO|5|2−}} contains one [[peroxide]] group per sulfur center, whereas in {{chem|S|2|O|8|2−}}, the peroxide group bridges the sulfur atoms. In both cases, sulfur adopts the normal tetrahedral geometry typical for the S(VI) oxidation state. These salts are strong oxidizers.<ref>{{cite web|url=http://geocleanse.com/persulfate.asp |title=Geo-Cleanse International |publisher=Geocleanse.com |access-date=2012-06-13}}</ref><ref>{{cite journal|author = Wacławek, S., Lutze, H. V., Grübel, K., Padil, V.V.T., Černík, M., Dionysiou, D.D. (2017) |title=Chemistry of persulfates in water and wastewater treatment: A review. |journal = Chemical Engineering Journal |volume = 330 |pages = 44–62 |doi = 10.1016/j.cej.2017.07.132|date = 2017-12-15 }}</ref>


==Ions==
==Ions==
Line 19: Line 20:
{{reflist}}
{{reflist}}


[[Category:Persulfates|*]]
{{Persulfates}}

⚫
[[Category:Sulfur oxoanions]]
{{Authority control}}

[[Category:Persulfates| ]]
⚫
[[Category:Sulfur oxyanions]]
[[Category:Preservatives]]
[[Category:Preservatives]]


{{Inorganic-compound-stub}}

Latest revision as of 05:24, 21 October 2024

A persulfate (sometimes known as peroxysulfate or peroxodisulfate)[1] is a compound containing the anions SO2−
5 or S
2O2−
8.[2] The anion SO2−
5 contains one peroxide group per sulfur center, whereas in S
2O2−
8, the peroxide group bridges the sulfur atoms. In both cases, sulfur adopts the normal tetrahedral geometry typical for the S(VI) oxidation state. These salts are strong oxidizers.[3][4]

Ions

[edit]

Acids

[edit]

Example salts

[edit]

References

[edit]
  1. ^ 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.
  2. ^ 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)
  3. ^ "Geo-Cleanse International". Geocleanse.com. Retrieved 2012-06-13.
  4. ^ Wacławek, S., Lutze, H. V., Grübel, K., Padil, V.V.T., Černík, M., Dionysiou, D.D. (2017) (2017-12-15). "Chemistry of persulfates in water and wastewater treatment: A review". Chemical Engineering Journal. 330: 44–62. doi:10.1016/j.cej.2017.07.132.{{cite journal}}: CS1 maint: multiple names: authors list (link) CS1 maint: numeric names: authors list (link)


Stub icon

This inorganic compound–related article is a stub. You can help Wikipedia by expanding it.

Retrieved from "https://en.wikipedia.org/enwiki/w/index.php?title=Persulfate&oldid=1252401874"