Jump to content

Silver oxide: Difference between revisions

Browse history interactively
Page 1
Page 2
← Previous edit
Content deleted Content added
VisualWikitext
WP:WPCHECK Ordinal number found inside <sup> tags
 
(129 intermediate revisions by 96 users not shown)
Line 1: Line 1:
{{distinguish|Silver(I,III) oxide}}
{{about|silver(I) oxide|the [[Mixed-valence complex|mixed-valence]] oxide|Silver(I,III) oxide}}
{{chembox
{{chembox
| Watchedfields = changed
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 414434401
| verifiedrevid = 440120975
| ImageSize =
| ImageFile = Silver oxide.jpg
| ImageFile = Silver(I)-oxide-unit-cell-3D-bs-17.png
| ImageSize =
| IUPACName = Silver(I) oxide
| ImageCaption = [[Unit cell]]
| OtherNames = Silver rust, Argentous oxide
| ImageName = Silver(I) oxide structure in unit cell
| Section1 = {{Chembox Identifiers
| 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 =
| Abbreviations =
| CASNo = 20667-12-3
| CASNo = 20667-12-3
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo_Ref = {{cascite|correct|CAS}}
| UNII_Ref = {{fdacite|correct|FDA}}
| EINECS =
| PubChem =
| UNII = 897WUN6G6T
| SMILES =
| RTECS = VW4900000
| InChI =
| PubChem = 9794626
| ChemSpiderID = 7970393
| RTECS =
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| MeSHName =
| EINECS = 243-957-1
| ChEBI =
| MeSHName = silver+oxide
| KEGG_Ref = {{keggcite|correct|kegg}}
| SMILES = [O-2].[Ag+].[Ag+]
| KEGG =
| StdInChI = 1S/2Ag.O/q2*+1;-2
| ATCCode_prefix =
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| ATCCode_suffix =
| InChI = 1S/2Ag.O/q2*+1;-2
| ATC_Supplemental =}}
| StdInChIKey = NDVLTYZPCACLMA-UHFFFAOYSA-N
| Section2 = {{Chembox Properties
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| Formula = Ag<sub>2</sub>O
| InChIKey = NDVLTYZPCACLMA-UHFFFAOYSA-N
| MolarMass = 231.735 g/mol

| Appearance = black/brown [[cubic crystal system|cubic]] crystals
}}
| Section2 = {{Chembox Properties
| Ag=2 | O=1
| Appearance = Black/ brown [[cubic crystal system|cubic]] crystals
| 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>
| Density = 7.14 g/cm<sup>3</sup>
| Density = 7.14 g/cm<sup>3</sup>
| MeltingPt = 280 °C
| MeltingPtC = 300
| MeltingPt_notes = decomposes from ≥200&nbsp;°C<ref name=crc2 /><ref name=chemister />
| Melting_notes = decomposition
| BoilingPt =
| BoilingPtC =
| Boiling_notes =
| BoilingPt_notes =
| Solubility = 0.013 g/L (20&nbsp;°C)<br /> 0.025 g/L (25&nbsp;°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&nbsp;°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>
| Solubility = 0.025 g/L<ref name="hand">
| SolubilityProduct = 1.52·10<sup>−8</sup> (20&nbsp;°C)
{{Cite book
| last = Lide
| first = David R.
| year = 1998
| title = Handbook of Chemistry and Physics
| edition = 87
| publication-place = Boca Raton, FL
| publisher = CRC Press
| isbn = 0-8493-0594-2
| pages = 4–83
}}</ref>
| SolubilityProduct = 1.52×10<sup>−8</sup> (20 °C)
| SolubilityProductAs = AgOH
| SolubilityProductAs = AgOH
| SolubleOther = soluble in [[acid]], [[alkali]] <br> insoluble in [[alcohol]], [[ethanol]]<ref name="hand"/>
| SolubleOther = Soluble in [[acid]], [[alkali]]<br /> Insoluble in [[ethanol]]<ref name="hand" />
| pKa = 12.1 (estimated)<ref name=P82db>{{cite book|title=Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution|editor-first=D.&nbsp;D.|editor-last=Perrin|edition=2nd|series=[[IUPAC]] 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&nbsp;210}}</ref>
| Solvent =
| MagSus = &minus;134.0·10<sup>−6</sup> cm<sup>3</sup>/mol }}
| pKa =
| Section3 = {{Chembox Structure
| pKb =
| CrystalStruct = [[Cubic crystal system|Cubic]]
| IsoelectricPt =
| SpaceGroup = Pn{{overline|3}}m, 224
| LambdaMax =
| Absorbance =
| SpecRotation =
| RefractIndex =
| Viscosity =
| Dipole = }}
| Section3 = {{Chembox Structure
| CrystalStruct = [[Cubic crystal system|cubic]]
| Coordination =
| Coordination =
| MolShape =
| MolShape =
| Dipole = }}
| Dipole =
| Section4 = {{Chembox Thermochemistry
| DeltaHf = -31.1 [[kJ/mol|kJ·mol<sup>−1</sup>]]
| DeltaHc =
| Entropy = 121.3 J·mol<sup>−1</sup>·K<sup>−1</sup>
| HeatCapacity = 65.9 J·mol<sup>−1</sup>·K<sup>−1</sup><ref name="hand2">
{{Cite book
| last = Lide
| first = David R.
| year = 1998
| title = Handbook of Chemistry and Physics
| edition = 87
| publication-place = Boca Raton, FL
| publisher = CRC Press
| isbn = 0-8493-0594-2
| pages = 5–5}}</ref>
}}
}}
| Section5 = {{Chembox Pharmacology
| Section4 = {{Chembox Thermochemistry
| 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>
| AdminRoutes =
| Entropy = 122 J/mol·K<ref name=b1/>
| Bioavail =
| HeatCapacity = 65.9 J/mol·K<ref name="hand"/>
| Metabolism =
| 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>
| HalfLife =
}}
| ProteinBound =
| Section7 = {{Chembox Hazards
| Excretion =
| Legal_status =
| ExternalSDS =
| GHSPictograms = {{GHS03}}{{GHS07}}<ref name="sigma">{{Sigma-Aldrich|id=226831|name=Silver(I) oxide|accessdate=2014-06-07}}</ref>
| Legal_US =
| GHSSignalWord = Danger
| Legal_UK =
| HPhrases = {{H-phrases|272|315|319|335}}<ref name="sigma" />
| Legal_AU =
| PPhrases = {{P-phrases|220|261|305+351+338}}<ref name="sigma" />
| Legal_CA =
| PregCat =
| PregCat_AU =
| PregCat_US = }}
| Section6 = {{Chembox Explosive
| ShockSens =
| FrictionSens =
| ExplosiveV =
| REFactor = }}
| Section7 = {{Chembox Hazards
| ExternalMSDS = [http://physchem.ox.ac.uk/MSDS/SI/silver_oxide.html Material Safety Data Sheet]
| EUClass =
| EUIndex =
| MainHazards =
| MainHazards =
| NFPA-H =
| NFPA-H = 2
| NFPA-F =
| NFPA-F = 0
| NFPA-R =
| NFPA-R = 1
| NFPA_ref = <ref name=slm />
| NFPA-O =
| LD50 = 2.82 g/kg (rats, oral)<ref name=slm />
| RPhrases =
}}
| SPhrases =
| Section8 = {{Chembox Related
| RSPhrases =
| FlashPt =
| Autoignition =
| ExploLimits =
| PEL = }}
| Section8 = {{Chembox Related
| OtherAnions =
| OtherAnions =
| OtherCations =
| OtherCations =
| OtherFunctn =
| OtherFunction =
| Function =
| OtherFunction_label =
| OtherCpds = [[silver(I,III) oxide|silver(I,III) oxide, AgO]] }}
| OtherCompounds = [[Silver(I,III) oxide]]
}}
}}
}}
'''Silver(I) oxide''' is the [[chemical compound]] with the [[chemical formula|formula]] Ag<sub>2</sub>O. It is a fine black or dark brown powder that is used to prepare other silver compounds.
'''Silver oxide''' is the [[chemical compound]] with the [[chemical formula|formula]] Ag<sub>2</sub>O. It is a fine black or dark brown powder that is used to prepare other [[silver]] compounds.


==Preparation==
==Preparation==
[[File:Silver(I) oxide.JPG|160px|thumbnail|left|Silver(I) oxide produced by reacting [[lithium hydroxide]] with a very dilute silver nitrate solution]]
Silver oxide is commercially available. It can be easily prepared by combining aqueous solutions of [[silver nitrate]] and an [[alkali hydroxide]].<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>
Silver oxide can be prepared by combining aqueous solutions of [[silver nitrate]] and an [[alkali hydroxide]].<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>
:2 AgOH → Ag<sub>2</sub>O + H<sub>2</sub>O ([[equilibrium constant|''p''K]] = 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>)
:<chem>2 AgOH -> Ag2O + H2O</chem> ([[equilibrium constant|p''K'']] = 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>)
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>


==Structure and properties==
==Structure and properties==
Ag<sub>2</sub>O features linear, two-coordinate Ag centers linked by tetrahedral oxides. It is [[isostructural]] with [[copper (I) oxide|Cu<sub>2</sub>O]]. 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 [[ammonia]] solution, producing active compound of [[Tollens' reagent]]. A [[slurry]] of Ag<sub>2</sub>O is readily attacked by [[acid]]s:
[[File:Copper(I)-oxide-unit-cell-A-3D-balls.png|thumb|140px|left|Ag<sub>2</sub>O structure]]
:<chem>Ag2O + 2 HX -> 2 AgX + H2O</chem>
Like most binary [[oxide]]s, Ag<sub>2</sub>O is a three-dimensional polymer with [[covalent]] 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">[http://themerckindex.cambridgesoft.com/TheMerckIndex/default.asp?formgroup=basenp_form_group&dataaction=db&dbname=TheMerckIndex Merck Index of Chemicals and Drugs], 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=[[F. Albert Cotton|Cotton, F. Albert]]; [[Geoffrey Wilkinson|Wilkinson, Geoffrey]] | title=Advanced Inorganic Chemistry (2nd Ed.) | publisher=New York:Interscience |page=1042| year=1966}}</ref> It dissolves in [[ammonia]] solution to give soluble derivatives.
where HX = [[Hydrofluoric acid|HF]], [[hydrochloric acid|HCl]], [[hydrobromic acid|HBr]], [[hydroiodic acid|HI]], or [[Trifluoroacetic acid|CF<sub>3</sub>COOH]]. It will also react with solutions of alkali chlorides to precipitate [[silver chloride]], leaving a solution of the corresponding alkali hydroxide.<ref name="c_w"/><ref name="pauling">General Chemistry by [[Linus Pauling]], 1970 Dover ed. p703-704</ref>


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&nbsp;°C.<ref name="merck">[http://themerckindex.cambridgesoft.com/TheMerckIndex/default.asp?formgroup=basenp_form_group&dataaction=db&dbname=TheMerckIndex Merck Index of Chemicals and Drugs] {{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>
A slurry of Ag<sub>2</sub>O is readily attacked by [[acid]]s:
:Ag<sub>2</sub>O + 2 HX → 2 AgX + H<sub>2</sub>O
where HX = [[Hydrofluoric acid|HF]], [[hydrochloric acid|HCl]], [[hydrobromic acid|HBr]], or [[hydroiodic acid|HI]], [[Trifluoroacetic acid|HO<sub>2</sub>CCF<sub>3</sub>]]. It will also react with solutions of alkali chlorides to precipitate [[silver chloride]], leaving a solution of the corresponding alkali hydroxide.<ref name="pauling">General Chemistry by [[Linus Pauling]], 1970 Dover ed. p703-704</ref><ref name="c_w"/>

Like many silver compounds, silver oxide is photosensitive. It also decomposes at temperatures above 280 °C.<ref name="merck"/>


==Applications==
==Applications==
This oxide is used in [[silver-oxide battery|silver-oxide batteries]].<ref>{{Cite web |date=2009-12-20 |title=Duracell PROCELL: The Chemistries: Silver Oxide |url=https://web.archive.org/web/20091220201115/http://www.duracell.com/procell/chemistries/silver.asp |access-date=2024-05-12 |website=web.archive.org}}</ref> In organic chemistry, silver oxide is used as a mild [[oxidizing agent]].<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 [[aldehyde]]s to [[carboxylic acid]]s.<ref>{{Cite journal |last=Chakraborty |first=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>
Commercially, silver oxide is used in a [[silver-oxide battery]]. 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.


==References==
==References==
{{reflist}}
{{Reflist}}


==External links==
==External links==
{{Commons category|Silver(I) oxide}}
*[http://www.job-stiftung.de/index.php?id=31,163,0,0,1,0 Annealing of Silver Oxide] Demonstration experiment: Instruction and video
* [http://www.job-stiftung.de/index.php?id=31,163,0,0,1,0 Annealing of Silver Oxide] – Demonstration experiment: Instruction and video
*[http://www.saltlakemetals.com/Silver_Oxide.htm Silver Oxide, Ag2O]


{{Oxides}}
{{Silver compounds}}
{{Silver compounds}}


[[Category:Silver compounds]]
[[Category:Silver compounds]]
[[Category:Oxides]]
[[Category:Transition metal oxides]]

[[cs:Oxid stříbrný]]
[[de:Silber(I)-oxid]]
[[es:Óxido de plata]]
[[fr:Oxyde d'argent(I)]]
[[it:Ossido di argento]]
[[hu:Ezüst(I)-oxid]]
[[nl:Zilver(I)oxide]]
[[ja:酸化銀(I)]]
[[pl:Tlenek srebra(I)]]
[[pt:Óxido de prata]]
[[ru:Оксид серебра(I)]]
[[simple:Silver(I) oxide]]
[[fi:Hopeaoksidi]]
[[sv:Silveroxid]]
[[zh:氧化银]]
Retrieved from "https://en.wikipedia.org/wiki/Special:ComparePages"