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Silver oxide
	; Unit cell
	; Crystal packing
Names
	IUPAC name Silver(I) oxide
	Other names Silver rust, Argentous oxide, Silver monoxide
Identifiers
CAS Number	20667-12-3 ;
3D model (JSmol)	Interactive image;
ChemSpider	7970393 ;
ECHA InfoCard	100.039.946
EC Number	243-957-1;
MeSH	silver+oxide
PubChem CID	9794626;
RTECS number	VW4900000;
UNII	897WUN6G6T ;
CompTox Dashboard (EPA)	DTXSID40893897 ;
	InChI InChI=1S/2Ag.O/q2+1;-2 Key: NDVLTYZPCACLMA-UHFFFAOYSA-N ; InChI=1S/2Ag.O/q2+1;-2 Key: NDVLTYZPCACLMA-UHFFFAOYSA-N;
	SMILES [O-2].[Ag+].[Ag+];
Properties
Chemical formula	Ag2O
Molar mass	231.735 g·mol−1
Appearance	Black/ brown cubic crystals
Odor	Odorless
Density	7.14 g/cm3
Melting point	300 °C (572 °F; 573 K) decomposes from ≥200 °C
Solubility in water	0.013 g/L (20 °C); 0.025 g/L (25 °C); 0.053 g/L (80 °C)
Solubility product (Ksp) of AgOH	1.52·10−8 (20 °C)
Solubility	Soluble in acid, alkali; Insoluble in ethanol
Acidity (pKa)	12.1 (estimated)
Magnetic susceptibility (χ)	−134.0·10−6 cm3/mol
Structure
Crystal structure	Cubic
Space group	Pn3m, 224
Thermochemistry
Heat capacity (C)	65.9 J/mol·K
Std molar; entropy (S⦵298)	122 J/mol·K
Std enthalpy of; formation (ΔfH⦵298)	−31 kJ/mol
Gibbs free energy (ΔfG⦵)	−11.3 kJ/mol
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H272, H315, H319, H335
Precautionary statements	P220, P261, P305+P351+P338
NFPA 704 (fire diamond)	2 0 1
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	2.82 g/kg (rats, oral)
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). verify (what is ?) Infobox references

Silver oxide is the chemical compound with the formula Ag₂O. It is a fine black or dark brown powder that is used to prepare other silver compounds.

Preparation

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]

{\ce {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

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:

{\ce {Ag2O + 2 HX -> 2 AgX + H2O}}

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

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 aldehydes to carboxylic acids.^[19]

References

^ ^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". 2009-12-20. Archived from the original on 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.