| Revision as of 14:04, 18 July 2011 edit218.215.25.57 (talk) →Structure and properties← Previous edit |
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{{distinguish|Silver(I,III) oxide}} |
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{{about|silver(I) oxide|the ] oxide|Silver(I,III) oxide}} |
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| ImageFile = Silver oxide.jpg |
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| ImageFile = Silver(I)-oxide-unit-cell-3D-bs-17.png |
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| ImageSize = |
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| IUPACName = Silver(I) oxide |
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| ImageCaption = ] |
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| OtherNames = Silver rust, Argentous oxide |
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| ImageName = Silver(I) oxide structure in unit cell |
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| Section1 = {{Chembox Identifiers |
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| ImageFile1 = Silver(I)-oxide-xtal-3x3x3-3D-bs-17.png |
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| ImageCaption1 = ] |
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| ImageFile2 = Silver oxide.jpg |
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| ImageName2 = Silver(I) oxide powder |
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| IUPACName = Silver(I) oxide |
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| OtherNames = Silver rust, Argentous oxide, Silver monoxide |
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| Section1 = {{Chembox Identifiers |
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| Abbreviations = |
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| Abbreviations = |
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| CASNo = 20667-12-3 |
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| CASNo = 20667-12-3 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| EINECS = |
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| PubChem = |
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| UNII = 897WUN6G6T |
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| SMILES = |
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| RTECS = VW4900000 |
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| InChI = |
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| PubChem = 9794626 |
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| ChemSpiderID = 7970393 |
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| RTECS = |
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| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} |
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| MeSHName = |
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| EINECS = 243-957-1 |
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| ChEBI = |
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| MeSHName = silver+oxide |
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| KEGG_Ref = {{keggcite|correct|kegg}} |
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| SMILES = .. |
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| KEGG = |
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| StdInChI = 1S/2Ag.O/q2*+1;-2 |
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| ATCCode_prefix = |
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| StdInChI_Ref = {{stdinchicite|changed|chemspider}} |
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| ATCCode_suffix = |
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| InChI = 1S/2Ag.O/q2*+1;-2 |
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| ATC_Supplemental =}} |
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| StdInChIKey = NDVLTYZPCACLMA-UHFFFAOYSA-N |
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| Section2 = {{Chembox Properties |
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| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} |
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| Formula = Ag<sub>2</sub>O |
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| InChIKey = NDVLTYZPCACLMA-UHFFFAOYSA-N |
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| MolarMass = 231.735 g/mol |
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| Appearance = black/brown ] crystals |
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}} |
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| Section2 = {{Chembox Properties |
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| Ag=2 | O=1 |
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| Appearance = Black/ brown ] crystals |
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| Odor = Odorless<ref name=slm>{{cite web |url=http://www.saltlakemetals.com/MSDS_Silver_Oxide.htm |title=Silver Oxide MSDS |website=SaltLakeMetals.com |publisher=Salt Lake Metals |access-date=2014-06-08}}</ref> |
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| Density = 7.14 g/cm<sup>3</sup> |
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| Density = 7.14 g/cm<sup>3</sup> |
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| MeltingPt = 280 °C |
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| MeltingPtC = 300 |
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| MeltingPt_notes = decomposes from ≥200 °C<ref name=crc2 /><ref name=chemister /> |
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| Melting_notes = decomposition |
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| BoilingPt = |
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| BoilingPtC = |
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| Boiling_notes = |
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| BoilingPt_notes = |
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| Solubility = 0.013 g/L (20 °C)<br /> 0.025 g/L (25 °C)<ref name="hand">{{cite book|last = Lide|first = David R.|year = 1998|title = Handbook of Chemistry and Physics|edition = 81|location = Boca Raton, FL|publisher = CRC Press|isbn = 0-8493-0594-2|pages = 4–83}}</ref><br /> 0.053 g/L (80 °C)<ref name=crc2>{{cite book|last = Perry|first = Dale L.|year = 1995|title = Handbook of Inorganic Compounds|edition = illustrated|publisher = CRC Press|isbn = 0849386713|pages = 354}}</ref> |
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| Solubility = 0.025 g/L<ref name="hand"> |
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| SolubilityProduct = 1.52·10<sup>−8</sup> (20 °C) |
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{{Cite book |
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| last = Lide |
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| first = David R. |
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| year = 1998 |
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| title = Handbook of Chemistry and Physics |
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| edition = 87 |
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| publication-place = Boca Raton, FL |
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| publisher = CRC Press |
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| isbn = 0-8493-0594-2 |
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| pages = 4–83 |
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}}</ref> |
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| SolubilityProduct = 1.52×10<sup>−8</sup> (20 °C) |
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| SolubilityProductAs = AgOH |
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| SolubilityProductAs = AgOH |
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| SolubleOther = soluble in ], ] <br> insoluble in ], ]<ref name="hand"/> |
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| SolubleOther = Soluble in ], ]<br /> Insoluble in ]<ref name="hand" /> |
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| pKa = 12.1 (estimated)<ref name=P82db>{{cite book|title=Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution|editor-first=D. D.|editor-last=Perrin|edition=2nd|series=] Chemical Data|issue=29|publisher=Pergamon|location=Oxford|year=1982|publication-date=1984|orig-date=1969|lccn=82-16524|isbn=0-08-029214-3|at=Entry 210}}</ref> |
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| Solvent = |
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| MagSus = −134.0·10<sup>−6</sup> cm<sup>3</sup>/mol }} |
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| pKa = |
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| Section3 = {{Chembox Structure |
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| pKb = |
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| CrystalStruct = ] |
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| IsoelectricPt = |
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| SpaceGroup = Pn{{overline|3}}m, 224 |
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| LambdaMax = |
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| Absorbance = |
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| Dipole = }} |
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| Section3 = {{Chembox Structure |
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| CrystalStruct = ] |
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| Coordination = |
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| Coordination = |
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| Dipole = }} |
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| Dipole = |
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| Section4 = {{Chembox Thermochemistry |
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| DeltaHf = -31.1 ] |
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| DeltaHc = |
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| Entropy = 121.3 J·mol<sup>−1</sup>·K<sup>−1</sup> |
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| HeatCapacity = 65.9 J·mol<sup>−1</sup>·K<sup>−1</sup><ref name="hand2"> |
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{{Cite book |
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| last = Lide |
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| first = David R. |
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| year = 1998 |
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| title = Handbook of Chemistry and Physics |
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| edition = 87 |
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| publication-place = Boca Raton, FL |
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| publisher = CRC Press |
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| isbn = 0-8493-0594-2 |
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| pages = 5–5}}</ref> |
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}} |
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}} |
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| Section5 = {{Chembox Pharmacology |
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| Section4 = {{Chembox Thermochemistry |
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| DeltaHf = −31 kJ/mol<ref name=b1>{{cite book|author = Zumdahl, Steven S.|title = Chemical Principles 6th Ed.|publisher = Houghton Mifflin Company|year = 2009|isbn = 978-0-618-94690-7|page = A23}}</ref> |
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| AdminRoutes = |
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| Entropy = 122 J/mol·K<ref name=b1/> |
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| Bioavail = |
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| HeatCapacity = 65.9 J/mol·K<ref name="hand"/> |
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| Metabolism = |
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| DeltaGf = −11.3 kJ/mol<ref name=chemister>{{Cite web|url=http://chemister.ru/Database/properties-en.php?dbid=1&id=4098|title = Silver oxide}}</ref> |
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| HalfLife = |
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}} |
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| Section7 = {{Chembox Hazards |
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| GHSPictograms = {{GHS03}}{{GHS07}}<ref name="sigma">{{Sigma-Aldrich|id=226831|name=Silver(I) oxide|accessdate=2014-06-07}}</ref> |
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| GHSSignalWord = Danger |
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| HPhrases = {{H-phrases|272|315|319|335}}<ref name="sigma" /> |
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| PPhrases = {{P-phrases|220|261|305+351+338}}<ref name="sigma" /> |
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| Section6 = {{Chembox Explosive |
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| Section7 = {{Chembox Hazards |
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| MainHazards = |
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| NFPA-H = |
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| NFPA-H = 2 |
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| NFPA-F = |
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| NFPA-F = 0 |
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| NFPA-R = |
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| NFPA-R = 1 |
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| NFPA_ref = <ref name=slm /> |
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| NFPA-O = |
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| LD50 = 2.82 g/kg (rats, oral)<ref name=slm /> |
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| Section8 = {{Chembox Related |
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| OtherCpds = ] }} |
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'''Silver(I) oxide''' is the ] with the ] Ag<sub>2</sub>O. It is a fine black or dark brown powder that is used to prepare other silver compounds. |
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'''Silver oxide''' is the ] with the ] ]<sub>2</sub>]. It is a fine black or dark brown powder that is used to prepare other ] compounds. |
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==Preparation== |
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==Preparation== |
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] with a very dilute silver nitrate solution]] |
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Silver oxide is commercially available. It can be easily prepared by combining aqueous solutions of ] and an ].<ref>{{OrgSynth | title = 4-Iodoveratrole | author = Janssen, D. E.; Wilson, C. V. | collvol = 4 | collvolpages = 547 | year = 1963 | prep = CV4P0547}}</ref> Noteworthy is the fact that this reaction does not afford appreciable amounts of silver hydroxide due to the favorable energetics for the following reaction:<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref> |
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Silver oxide can be prepared by combining aqueous solutions of ] and an ].<ref>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.</ref><ref>{{OrgSynth | title = 4-Iodoveratrole | author = Janssen, D. E.; Wilson, C. V. | collvol = 4 | collvolpages = 547 | year = 1963 | prep = CV4P0547}}</ref> This reaction does not afford appreciable amounts of silver hydroxide due to the favorable energetics for the following reaction:<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref> |
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:2 AgOH → Ag<sub>2</sub>O + H<sub>2</sub>O (] = 2.875<ref>{{cite journal | doi = 10.3891/acta.chem.scand.14-0717 | author = Biedermann, George; Sillén, Lars Gunnar | title = Studies on the Hydrolysis of Metal Ions. Part 30. A Critical Survey of the Solubility Equilibria of Ag<sub>2</sub>O | year = 1960 | journal = Acta Chemica Scandinavica | volume = 14 | pages = 717}}</ref>) |
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:<chem>2 AgOH -> Ag2O + H2O</chem> (] = 2.875<ref>{{cite journal | doi = 10.3891/acta.chem.scand.14-0717 |author1=Biedermann, George |author2=Sillén, Lars Gunnar | title = Studies on the Hydrolysis of Metal Ions. Part 30. A Critical Survey of the Solubility Equilibria of Ag<sub>2</sub>O | year = 1960 | journal = Acta Chemica Scandinavica | volume = 13 | pages = 717–725| doi-access = free }}</ref>) |
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With suitably controlled conditions, this reaction can be used to prepare Ag<sub>2</sub>O powder with properties suitable for several uses including as a fine grained conductive paste filler.<ref>{{Cite patent|country=US|number=20050050990A1|title=Fine-grain silver oxide powder|status=|pubdate=2005-03-10|invent1=Harigae|invent2=Shoji|inventor1-first=Kenichi|inventor2-first=Yoshiyuki}}</ref> |
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==Structure and properties== |
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==Structure and properties== |
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Ag<sub>2</sub>O features linear, two-coordinate Ag centers linked by tetrahedral oxides. It is ] with ]. 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.<ref name="c_w">{{cite book |author1=Cotton, F. Albert |author2-link=Geoffrey Wilkinson |author2=Wilkinson, Geoffrey | title=Advanced Inorganic Chemistry (2nd Ed.) | publisher=New York:Interscience |page=1042| year=1966|author1-link=F. Albert Cotton }}</ref> It is soluble in ] solution, producing active compound of ]. A ] of Ag<sub>2</sub>O is readily attacked by ]s: |
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:<chem>Ag2O + 2 HX -> 2 AgX + H2O</chem> |
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Like most binary ]s, Ag<sub>2</sub>O is a three-dimensional polymer with ] metal-oxygen bonding. It is isostructural with Cu<sub>2</sub>O. It is therefore expected that Ag<sub>2</sub>O is insoluble in all solvents,<ref name="merck">, 14th ed. monograph 8521</ref> except by reaction. It is also slightly soluble in aqueous solution due to the formation of the ion, Ag(OH)<sub>2</sub><sup>–</sup> and possibly related hydrolysis products.<ref name="c_w">{{cite book | author=]; ] | title=Advanced Inorganic Chemistry (2nd Ed.) | publisher=New York:Interscience |page=1042| year=1966}}</ref> It dissolves in ] solution to give soluble derivatives. |
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where HX = ], ], ], ], or ]. It will also react with solutions of alkali chlorides to precipitate ], leaving a solution of the corresponding alkali hydroxide.<ref name="c_w"/><ref name="pauling">General Chemistry by ], 1970 Dover ed. p703-704</ref> |
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Despite the photosensitivity of many silver compounds, silver oxide is not photosensitive,<ref>{{Cite journal|last1=Herley|first1=P. J.|last2=Prout|first2=E. G.|date=1960-04-01|title=The Thermal Decomposition of Silver Oxide|url=https://doi.org/10.1021/ja01492a006|journal=Journal of the American Chemical Society|volume=82|issue=7|pages=1540–1543|doi=10.1021/ja01492a006|issn=0002-7863}}</ref> although it readily decomposes at temperatures above 280 °C.<ref name="merck"> {{webarchive|url=https://web.archive.org/web/20090201140752/http://themerckindex.cambridgesoft.com/TheMerckIndex/default.asp?formgroup=basenp_form_group&dataaction=db&dbname=TheMerckIndex |date=2009-02-01 }}, 14th ed. monograph 8521</ref> |
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A slurry of Ag<sub>2</sub>O is readily attacked by ]s: |
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:Ag<sub>2</sub>O + 2 HX → 2 AgX + H<sub>2</sub>O |
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where HX = ], ], ], or ], ]. It will also react with solutions of alkali chlorides to precipitate ], leaving a solution of the corresponding alkali hydroxide.<ref name="pauling">General Chemistry by ], 1970 Dover ed. p703-704</ref><ref name="c_w"/> |
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Like many silver compounds, silver oxide is photosensitive. It also decomposes at temperatures above 280 °C.<ref name="merck"/> |
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==Applications== |
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==Applications== |
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This oxide is used in ].<ref>{{Cite web |date=2009-12-20 |title=Duracell PROCELL: The Chemistries: Silver Oxide |url=http://www.duracell.com/procell/chemistries/silver.asp |access-date=2024-05-12 |archive-url=https://web.archive.org/web/20091220201115/http://www.duracell.com/procell/chemistries/silver.asp |archive-date=2009-12-20 }}</ref> In organic chemistry, silver oxide is used as a mild ].<ref>{{Cite book |last=裴 |first=坚 |title=基础有机化学 |edition=4th |publication-date=2017 |pages=1064 |language=Chinese |trans-title=Basic Organic Chemistry}}</ref> For example, it oxidizes ]s to ]s.<ref>{{Cite journal |last1=Chakraborty |first1=Debashis |last2=Gowda |first2=Ravikumar R. |last3=Malik |first3=Payal |date=2009 |title=Silver nitrate-catalyzed oxidation of aldehydes to carboxylic acids by H2O2 |url=https://linkinghub.elsevier.com/retrieve/pii/S0040403909017663 |journal=Tetrahedron Letters |language=en |volume=50 |issue=47 |pages=6553–6556 |doi=10.1016/j.tetlet.2009.09.044}}</ref> |
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Commercially, silver oxide is used in a ]. In organic chemistry, silver oxide is used as a mild oxidizing agent. 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. |
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==References== |
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==References== |
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{{reflist}} |
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{{Reflist}} |
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==External links== |
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==External links== |
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{{Commons category|Silver(I) oxide}} |
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* Demonstration experiment: Instruction and video |
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* – Demonstration experiment: Instruction and video |
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{{Oxides}} |
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{{Silver compounds}} |
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{{Silver compounds}} |
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