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Silver oxide

From Wikipedia, the free encyclopedia
(Redirected fromSilver hydroxide)
This article is about silver(I) oxide. For themixed-valence oxide, seeSilver(I,III) oxide.
Silver oxide
Silver(I) oxide structure in unit cell
Silver(I) oxide structure in unit cell
Silver(I) oxide powder
Silver(I) oxide powder
Names
IUPAC name
Silver(I) oxide
Other names
Silver rust, Argentous oxide, Silver monoxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard100.039.946Edit this at Wikidata
EC Number
  • 243-957-1
MeSHsilver+oxide
RTECS number
  • VW4900000
UNII
  • InChI=1S/2Ag.O/q2*+1;-2 ☒N
    Key: NDVLTYZPCACLMA-UHFFFAOYSA-N ☒N
  • InChI=1S/2Ag.O/q2*+1;-2
    Key: NDVLTYZPCACLMA-UHFFFAOYSA-N
  • [O-2].[Ag+].[Ag+]
Properties
Ag2O
Molar mass231.735 g·mol−1
AppearanceBlack/ browncubic crystals
OdorOdorless[1]
Density7.14 g/cm3
Melting point300 °C (572 °F; 573 K) decomposes from ≥200 °C[3][5]
0.013 g/L (20 °C)
0.025 g/L (25 °C)[2]
0.053 g/L (80 °C)[3]
Solubility product (Ksp) of AgOH
1.52·10−8 (20 °C)
SolubilitySoluble inacid,alkali
Insoluble inethanol[2]
Acidity (pKa)12.1 (estimated)[4]
−134.0·10−6 cm3/mol
Structure
Cubic
Pn3m, 224
Thermochemistry
65.9 J/mol·K[2]
122 J/mol·K[6]
−31 kJ/mol[6]
−11.3 kJ/mol[5]
Hazards
GHS labelling:
GHS03: OxidizingGHS07: Exclamation mark[7]
Danger
H272,H315,H319,H335[7]
P220,P261,P305+P351+P338[7]
NFPA 704 (fire diamond)
Lethal dose or concentration (LD, LC):
2.82 g/kg (rats, oral)[1]
Related compounds
Related compounds
Silver(I,III) oxide
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa).
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Chemical compound

Silver oxide is thechemical compound with theformulaAg2O. It is a fine black or dark brown powder that is used to prepare othersilver compounds.

Preparation

[edit]
Silver(I) oxide produced by reactinglithium hydroxide with a very dilute silver nitrate solution

Silver oxide can be prepared by combining aqueous solutions ofsilver nitrate and analkali hydroxide.[8][9] This reaction does not afford appreciable amounts of silver hydroxide due to the favorable energetics for the following reaction:[10]

2 AgOH → Ag2O + H2O    (pK = 2.875[11])

With suitably controlled conditions, this reaction can be used to prepare Ag2O powder with properties suitable for several uses including as a fine grained conductive paste filler.[12]

Structure and properties

[edit]

Ag2O features linear, two-coordinate Ag centers linked by tetrahedral oxides. It isisostructural withCu2O. It "dissolves" in solvents that degrade it. It is slightly soluble in water due to the formation of the ionAg(OH)−2 and possibly related hydrolysis products.[13] It is soluble inammonia solution, producing active compound ofTollens' reagent. Aslurry of Ag2O is readily attacked byacids:

Ag2O + 2 HX → 2 AgX + H2

where HX =HF,HCl,HBr,HI, orCF3COOH. It will also react with solutions of alkali chlorides to precipitatesilver chloride, leaving a solution of the corresponding alkali hydroxide.[13][14]

Despite the photosensitivity of many silver compounds, silver oxide is not photosensitive,[15] although it readily decomposes at temperatures above 280 °C.[16]

Applications

[edit]

This oxide is used insilver-oxide batteries.[17] In organic chemistry, silver oxide is used as a mildoxidizing agent.[18] For example, it oxidizesaldehydes tocarboxylic acids.[19]

References

[edit]
  1. ^abc"Silver Oxide MSDS".SaltLakeMetals.com. Salt Lake Metals. Retrieved2014-06-08.
  2. ^abcLide, David R. (1998).Handbook of Chemistry and Physics (81 ed.). Boca Raton, FL: CRC Press. pp. 4–83.ISBN 0-8493-0594-2.
  3. ^abPerry, Dale L. (1995).Handbook of Inorganic Compounds (illustrated ed.). CRC Press. p. 354.ISBN 0849386713.
  4. ^Perrin, D. D., ed. (1982) [1969].Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution.IUPAC Chemical Data (2nd ed.). Oxford: Pergamon (published 1984). Entry 210.ISBN 0-08-029214-3.LCCN 82-16524.
  5. ^ab"Silver oxide".
  6. ^abZumdahl, Steven S. (2009).Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23.ISBN 978-0-618-94690-7.
  7. ^abcSigma-Aldrich Co.,Silver(I) oxide. Retrieved on 2014-06-07.
  8. ^O. Glemser and H. Sauer "Silver Oxide" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1037.
  9. ^Janssen, D. E.; Wilson, C. V. (1963)."4-Iodoveratrole".Organic Syntheses{{cite journal}}: CS1 maint: multiple names: authors list (link);Collected Volumes, vol. 4, p. 547.
  10. ^Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001.ISBN 0-12-352651-5.
  11. ^Biedermann, George; Sillén, Lars Gunnar (1960)."Studies on the Hydrolysis of Metal Ions. Part 30. A Critical Survey of the Solubility Equilibria of Ag2O".Acta Chemica Scandinavica.13:717–725.doi:10.3891/acta.chem.scand.14-0717.
  12. ^US 20050050990A1, Harigae, Kenichi & Shoji, Yoshiyuki, "Fine-grain silver oxide powder", published 2005-03-10 
  13. ^abCotton, F. Albert;Wilkinson, Geoffrey (1966).Advanced Inorganic Chemistry (2nd Ed.). New York:Interscience. p. 1042.
  14. ^General Chemistry byLinus Pauling, 1970 Dover ed. p703-704
  15. ^Herley, P. J.; Prout, E. G. (1960-04-01)."The Thermal Decomposition of Silver Oxide".Journal of the American Chemical Society.82 (7):1540–1543.doi:10.1021/ja01492a006.ISSN 0002-7863.
  16. ^Merck Index of Chemicals and DrugsArchived 2009-02-01 at theWayback Machine, 14th ed. monograph 8521
  17. ^"Duracell PROCELL: The Chemistries: Silver Oxide". 2009-12-20. Archived fromthe original on 2009-12-20. Retrieved2024-05-12.
  18. ^裴, 坚 (2017).基础有机化学 [Basic Organic Chemistry] (in Chinese) (4th ed.). p. 1064.
  19. ^Chakraborty, Debashis; Gowda, Ravikumar R.; Malik, Payal (2009)."Silver nitrate-catalyzed oxidation of aldehydes to carboxylic acids by H2O2".Tetrahedron Letters.50 (47):6553–6556.doi:10.1016/j.tetlet.2009.09.044.

External links

[edit]
Wikimedia Commons has media related toSilver(I) oxide.
Mixed oxidation states
+1 oxidation state
+2 oxidation state
+3 oxidation state
+4 oxidation state
+5 oxidation state
+6 oxidation state
+7 oxidation state
+8 oxidation state
Related
Oxides are sorted byoxidation state.Category:Oxides
Silver(0,I)
Silver(I)
Organosilver(I) compounds
Silver(II)
Silver(III)
Silver(I,III)
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