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{{about|silver(I) oxide|the mixed-valence oxide|Silver(I,III) oxide}}{{chembox| Verifiedfields = changed| Watchedfields = changed| verifiedrevid = 440120975| ImageFile = Silver(I)-oxide-unit-cell-3D-bs-17.png| ImageSize = | ImageCaption = Unit cell| ImageName = Silver(I) oxide structure in unit cell| ImageFile1 = Silver(I)-oxide-xtal-3x3x3-3D-bs-17.png| ImageCaption1 = Crystal packing| ImageFile2 = Silver oxide.jpg| ImageName2 = Silver(I) oxide powder| IUPACName = Silver(I) oxide| OtherNames = Silver rust, Argentous oxide, Silver monoxide| Section1 = {{Chembox Identifiers| Abbreviations = | CASNo = 20667-12-3

correct|CAS}}

correct|FDA}}| UNII = 897WUN6G6T| RTECS = VW4900000| PubChem = 9794626| ChemSpiderID = 7970393

changed|chemspider}}| EINECS = 243-957-1| MeSHName = silver+oxide| SMILES = [O-2].[Ag+].[Ag+]| StdInChI = 1S/2Ag.O/q2*+1;-2

changed|chemspider}}| InChI = 1S/2Ag.O/q2*+1;-2| StdInChIKey = NDVLTYZPCACLMA-UHFFFAOYSA-N

changed|chemspider}}| InChIKey = NDVLTYZPCACLMA-UHFFFAOYSA-N}}| Section2 = {{Chembox Properties

O=1

cubic crystal system>cubic crystals

WEBSITE=SALTLAKEMETALS.COM

ACCESS-DATE=2014-06-08, | Density = 7.14 g/cm3| MeltingPtC = 300| MeltingPt_notes = decomposes from ≥200 Â°C| BoilingPtC = | BoilingPt_notes =

YEAR = 1998

EDITION = 81

PUBLISHER = CRC PRESS

PAGES = 4–83, 0.053 g/L (80 Â°C)PERRY>FIRST = DALE L.

TITLE = HANDBOOK OF INORGANIC COMPOUNDS

PUBLISHER = CRC PRESS

PAGES = 354, | SolubilityProduct = 1.52·10−8 (20 Â°C)| SolubilityProductAs = AgOH| SolubleOther = Soluble in acid, alkali Insoluble in ethanol | Solvent = | pKa =| pKb = | IsoelectricPt = | LambdaMax =| Absorbance =| SpecRotation = | RefractIndex = | Viscosity = | Dipole =| MagSus = −134.0·10−6 cm3/mol }}| Section3 = {{Chembox Structure

Cubic crystal system>Cubic

3}}m, 224| Coordination = | MolShape = | Dipole = }}| Section4 = {{Chembox Thermochemistry

PUBLISHER = HOUGHTON MIFFLIN COMPANY

ISBN = 978-0-618-94690-7, A23, | Entropy = 122 J/mol·K| HeatCapacity = 65.9 J/mol·K

id=226831

accessdate=2014-06-07}}| GHSSignalWord = Danger

272

319|335}}

220

305+351+338}}| MainHazards = | NFPA-H = 2| NFPA-F = 0| NFPA-R = 1| NFPA_ref = | LD50 = 2.82 g/kg (rats, oral)}}| Section8 = {{Chembox Related| OtherAnions = | OtherCations = | OtherFunction = | OtherFunction_label = | OtherCompounds = Silver(I,III) oxide}}}}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 File:Silver(I) oxide.JPG|160px|thumbnail|left|Silver(I) oxide produced by reacting lithium hydroxidelithium hydroxideSilver oxide can be prepared by combining aqueous solutions of silver nitrate and an alkali hydroxide.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.{{OrgSynth | title = 4-Iodoveratrole | author = Janssen, D. E.; Wilson, C. V. | collvol = 4 | collvolpages = 547 | year = 1963 | prep = CV4P0547}} This reaction does not afford appreciable amounts of silver hydroxide due to the favorable energetics for the following reaction:Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}. 2 AgOH -> Ag2O + H2O (pK = 2.875JOURNAL, 10.3891/acta.chem.scand.14-0717, Biedermann, George, Sillén, Lars Gunnar, Studies on the Hydrolysis of Metal Ions. Part 30. A Critical Survey of the Solubility Equilibria of Ag2O, 1960, Acta Chemica Scandinavica, 13, 717–725, free, ) 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.PATENT, US, 20050050990A1, Fine-grain silver oxide powder, 2005-03-10, Harigae, Shoji, Kenichi, Yoshiyuki, 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 {{Chem2|Ag(OH)2-}} and possibly related hydrolysis products.BOOK, Cotton, F. Albert, Geoffrey Wilkinson, Wilkinson, Geoffrey, Advanced Inorganic Chemistry (2nd Ed.), New York:Interscience, 1042, 1966, F. Albert Cotton, It is soluble in ammonia solution, producing active compound of Tollens' reagent. A slurry of Ag2O is readily attacked by acids: 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.General Chemistry by Linus Pauling, 1970 Dover ed. p703-704Despite the photosensitivity of many silver compounds, silver oxide is not photosensitive,JOURNAL, Herley, P. J., Prout, E. G., 1960-04-01, The Thermal Decomposition of Silver Oxide,weblink Journal of the American Chemical Society, 82, 7, 1540–1543, 10.1021/ja01492a006, 0002-7863, although it readily decomposes at temperatures above 280 Â°C.Merck Index of Chemicals and Drugs {{webarchive|url=https://web.archive.org/web/20090201140752weblink |date=2009-02-01 }}, 14th ed. monograph 8521 Applications {{Unreferenced section|date=February 2024}}This oxide is used in silver-oxide batteries. WEB, 2009-12-20, Duracell PROCELL: The Chemistries: Silver Oxide,weblink" title="web.archive.org/web/20091220201115weblink">weblink 2024-05-12, web.archive.org, In organic chemistry, silver oxide is used as a mild oxidizing agent. BOOK, 裴, 坚, 基础有机化学, 4th, 2017, 1064, Chinese, Basic Organic Chemistry, For example, it oxidizes aldehydes to carboxylic acids. Such reactions often work best when the silver oxide is prepared in situ from silver nitrate and alkali hydroxide. References {{Reflist}} External links {{Commons category|Silver(I) oxide}} Annealing of Silver Oxide – Demonstration experiment: Instruction and video {{Oxides}}{{Silver compounds}}