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Silver oxide





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This article is about silver(I) oxide. For the mixed-valence oxide, see Silver(I,III) oxide.

Silver oxide is the chemical compound with the formulaAg2O. It is a fine black or dark brown powder that is used to prepare other silver compounds.

Silver oxide
Silver(I) oxide structure in unit cell

Unit cell


Crystal packing

Silver(I) oxide powder
Names
IUPAC name

Silver(I) oxide

Other names

Silver rust, Argentous oxide, Silver monoxide

Identifiers

CAS Number

3D model (JSmol)
ChemSpider
ECHA InfoCard 100.039.946 Edit this at Wikidata
EC Number
  • 243-957-1
MeSH silver+oxide

PubChem CID
RTECS number
  • VW4900000
UNII

CompTox Dashboard (EPA)

  • 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

Chemical formula

 Ag2O
Molar mass 231.735 g·mol−1
Appearance Black/ brown cubic crystals
Odor Odorless[1]
Density 7.14 g/cm3
Melting point 300 °C (572 °F; 573 K) decomposes from ≥200 °C[3][5]

Solubility in water

 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)
Solubility Soluble in acid, alkali
Insoluble in ethanol[2]
Acidity (pKa) 12.1 (estimated)[4]

Magnetic susceptibility (χ)

 −134.0·10−6cm3/mol
Structure

Crystal structure

 Cubic

Space group

 Pn3m, 224
Thermochemistry

Heat capacity (C)

 65.9 J/mol·K[2]

Std molar
entropy (S⦵298)

 122 J/mol·K[6]

Std enthalpy of
formation (ΔfH⦵298)

 −31 kJ/mol[6]

Gibbs free energy (ΔfG⦵)

 −11.3 kJ/mol[5]
Hazards
GHS labelling:

Pictograms

 GHS03: OxidizingGHS07: Exclamation mark[7]

Signal word

 Danger

Hazard statements

 H272, H315, H319, H335[7]

Precautionary statements

 P220, P261, P305+P351+P338[7]
NFPA 704 (fire diamond)
[1]
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
2
0
1
Lethal dose or concentration (LD, LC):

LD50 (median dose)

 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 their standard state (at 25 °C [77 °F], 100 kPa).

☒N verify (what is checkY☒N ?)

Infobox references

Preparation

edit
 
Silver(I) oxide produced by reacting lithium hydroxide with a very dilute silver nitrate solution

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

  (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 is isostructural with Cu2O. It "dissolves" in solvents that degrade it. It is slightly soluble in water due to the formation of the ion Ag(OH)−2 and possibly related hydrolysis products.[13] It is soluble in ammonia solution, producing active compound of Tollens' reagent. A slurry of Ag2O is readily attacked by acids:

 

where HX = HF, HCl, HBr, HI, or CF3COOH. It will also react with solutions of alkali chlorides to precipitate silver 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 in silver-oxide batteries. [17]In organic chemistry, silver oxide is used as a mild oxidizing agent. [18] For example, it oxidizes aldehydestocarboxylic acids.[19]

References

edit
  1. ^ a b c "Silver Oxide MSDS". SaltLakeMetals.com. Salt Lake Metals. Retrieved 2014-06-08.
  • ^ a b c Lide, David R. (1998). Handbook of Chemistry and Physics (81 ed.). Boca Raton, FL: CRC Press. pp. 4–83. ISBN 0-8493-0594-2.
  • ^ a b Perry, Dale L. (1995). Handbook of Inorganic Compounds (illustrated ed.). CRC Press. p. 354. ISBN 0849386713.
  • ^ 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.
  • ^ a b "Silver oxide".
  • ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
  • ^ a b c Sigma-Aldrich Co., Silver(I) oxide. Retrieved on 2014-06-07.
  • ^ 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.
  • ^ 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.
  • ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  • ^ 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.
  • ^ US 20050050990A1, Harigae, Kenichi & Shoji, Yoshiyuki, "Fine-grain silver oxide powder", published 2005-03-10 
  • ^ a b Cotton, F. Albert; Wilkinson, Geoffrey (1966). Advanced Inorganic Chemistry (2nd Ed.). New York:Interscience. p. 1042.
  • ^ General Chemistry by Linus Pauling, 1970 Dover ed. p703-704
  • ^ 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.
  • ^ Merck Index of Chemicals and Drugs Archived 2009-02-01 at the Wayback Machine, 14th ed. monograph 8521
  • ^ "Duracell PROCELL: The Chemistries: Silver Oxide". web.archive.org. 2009-12-20. Retrieved 2024-05-12.
  • ^ 裴, 坚 (2017). 基础有机化学 [Basic Organic Chemistry] (in Chinese) (4th ed.). p. 1064.
  • ^ 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.
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    Last edited on 23 June 2024, at 17:46  





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