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Revision as of 11:31, 13 October 2011 editCheMoBot (talk | contribs)Bots141,565 edits Updating {{chembox}} (no changed fields - added verified revid - updated 'ChemSpiderID_Ref', 'DrugBank_Ref', 'UNII_Ref', 'ChEMBL_Ref', 'StdInChI_Ref', 'StdInChIKey_Ref') per Chem/Drugbox validation (report [[Wikipedia_talk:WikiPro...← Previous edit		Latest revision as of 15:20, 5 November 2024 edit undoRodw (talk | contribs)Autopatrolled, Event coordinators, Extended confirmed users, New page reviewers, Pending changes reviewers, Rollbackers765,085 editsm Disambiguating links to Pseudomorphosis (link changed to Pseudomorph) using DisamAssist.
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	{{chembox		{{chembox
			| Verifiedfields = changed
	| verifiedrevid = 445938307
			| Watchedfields = changed
	| ImageFile = Sulfid stříbrný.PNG
			| verifiedrevid = 455355846
	| ImageSize =
			| Name =
	| ImageName = Silver sulfide
			| ImageFile = Ag2S-bas.png
	| IUPACName = Silver sulfide
			| ImageSize = 160px
	| SystematicName =
			| ImageName = Ball-and-stick model of silver sulfide
	| OtherNames =
			| ImageFile1 = Sulfid stříbrný.PNG
	| Section1 = {{Chembox Identifiers
			| ImageSize1 =
			| ImageName1 = Sample of silver sulfide
			| IUPACName = Silver(I) sulfide
			| OtherNames = Silver sulfide <br/> Argentous sulfide
			| SystematicName =
			| Section1 = {{Chembox Identifiers
	| Abbreviations =		| Abbreviations =
	| CASNo = 21548-73-2		| CASNo = 21548-73-2
	| CASNo_Ref = {{cascite}}		| CASNo_Ref = {{cascite|correct|CAS}}
			| EC_number = 244-438-2
	| EINECS =
			| PubChem = 166738
	| EINECSCASNO =
	| PubChem =
	| SMILES =
	| InChI =
	| RTECS =		| RTECS =
			| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
	| MeSHName =
			| ChemSpiderID = 145878
	| ChEBI_Ref = {{ebicite|correct|EBI}}
			| UNII = 9ZB10YHC1C
	| ChEBI =
	| KEGG_Ref = {{keggcite|correct|kegg}}		| UNII_Ref = {{fdacite|changed|FDA}}
	| KEGG =		| SMILES = S(Ag)Ag
			| StdInChI = 1S/2Ag.S/q2*+1;-2
	| ATCCode_prefix =
			| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
	| ATCCode_suffix =
			| StdInChIKey = XUARKZBEFFVFRG-UHFFFAOYSA-N
	| ATC_Supplemental =}}
			| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
	| Section2 = {{Chembox Properties
			}}
	| Formula = Ag<sub>2</sub>S
			| Section2 = {{Chembox Properties
	| MolarMass = 247.8 g/mol
			| Ag=2 | S=1
	| Appearance = Black cubic crystal
			| Appearance = Grayish-blackish crystal
	| Density = 7.23 g/cm<sup>3</sup>
			| Odor = Odorless
	| MeltingPt = 1098 ] (825 ])
			| Density = 7.234 g/cm<sup>3</sup> (25&nbsp;°C)<ref name=crc /><ref name="sigma" /><br> 7.12 g/cm<sup>3</sup> (117&nbsp;°C)<ref name=hpp />
	| Melting_notes = 825 °C
	| BoilingPt =		| MeltingPtC = 836
			| MeltingPt_ref = <ref name=crc>{{CRC90}}</ref>
	| Boiling_notes =
	| Solubility = 8.5<sup>-12</sup> mg/L		| Solubility = 6.21·10<sup>−15</sup> g/L (25&nbsp;°C)
			| SolubleOther = Soluble in aq. ], aq. ] with ]<br> Insoluble in ]s, ]es, aqueous ]s<ref name=doc00>{{cite book|page = |title = A Dictionary of Chemical Solubilities: Inorganic|url = https://archive.org/details/in.ernet.dli.2015.171090|edition = 2nd|first1 = Arthur Messinger|last1 = Comey|first2 = Dorothy A.|last2 = Hahn|place = New York|publisher = The MacMillan Company|date = February 1921}}</ref>
	| SolubleOther = soluble in ] and ]
			| SolubilityProduct = 6.31·10<sup>−50</sup>
	| Solvent =
			}}
	| LogP =
			| Section3 = {{Chembox Structure
	| VaporPressure =
			| CrystalStruct = ], cI8 (α-form) <br> ], ] (β-form)<br> Cubic, cF12 (γ-form)<ref name=hpp>{{cite book|url = https://books.google.com/books?id=uo8wVw9Gq7wC&pg=PA13|title = High Pressure Phase Transformations: A Handbook|volume = 1|first = E. Yu|last = Tonkov|publisher = Gordon and Breach Science Publishers|year = 1992|isbn = 978-2-88124-761-3|page = 13}}</ref><ref name=spring />
	| HenryConstant =
			| SpaceGroup = Im{{overline|3}}m, No. 229 (α-form)<ref name=spring /><br> P2<sub>1</sub>/n, No. 14 (β-form)<br> Fm{{overline|3}}m, No. 225 (γ-form)<ref name=hpp />
	| AtmosphericOHRateConstant =
			| PointGroup = 2/m (α-form)<ref name=spring /><br> 4/m {{overline|3}} 2/m (β-form, γ-form)<ref name=hpp />
	| pKa =
			| LattConst_a = 4.23&nbsp;Å
	| pKb = }}
			| LattConst_b = 6.91&nbsp;Å
	| Section3 = {{Chembox Structure
			| LattConst_c = 7.87&nbsp;Å (α-form)<ref name=spring />
	| CrystalStruct = orthogonal
			| LattConst_beta = 99.583
	| Coordination =
	| MolShape = }}		| Coordination =
			}}
	| Section4 = {{Chembox Thermochemistry
			| Section4 = {{Chembox Thermochemistry
	| DeltaHf = -32.6 kJ/mol
			| DeltaHf = −32.59 kJ/mol<ref name=pphoic>{{cite book|last = Pradyot|first = Patnaik|year = 2003|title = Handbook of Inorganic Chemicals|publisher = The McGraw-Hill Companies, Inc.|isbn = 978-0-07-049439-8|page = 845}}</ref>
	| DeltaHc =
	| Entropy = 144.0 J/mol·K		| DeltaGf = −40.71 kJ/mol<ref name=pphoic />
			| Entropy = 143.93 J/mol·K<ref name=pphoic />
	| HeatCapacity = }}
			| HeatCapacity = 76.57 J/mol·K<ref name=pphoic />
	| Section5 = {{Chembox Pharmacology
			}}
	| AdminRoutes =
	| Bioavail =		| Section5 =
	| Metabolism =		| Section6 =
			| Section7 = {{Chembox Hazards
	| HalfLife =
	| ProteinBound =
	| Excretion =
	| Legal_status =
	| Legal_US =
	| Legal_UK =
	| Legal_AU =
	| Legal_CA =
	| PregCat =
	| PregCat_AU =
	| PregCat_US = }}
	| Section6 = {{Chembox Explosive
	| ShockSens =
	| FrictionSens =
	| ExplosiveV =
	| REFactor = }}
	| Section7 = {{Chembox Hazards
	| EUClass =
	| EUIndex =
	| MainHazards = May cause irritation		| MainHazards = May cause irritation
			| GHSPictograms = {{GHS07}}<ref name="sigma">{{Sigma-Aldrich| id=241474 |name=Silver sulfide|accessdate=2014-07-13}}</ref>
	| NFPA-H =
			| GHSSignalWord = Warning
	| NFPA-F =
			| HPhrases = {{H-phrases|315|319|335}}<ref name="sigma" />
	| NFPA-R =
			| PPhrases = {{P-phrases|261|305+351+338}}<ref name="sigma" />
	| NFPA-O =
	| RPhrases =		| NFPA-H = 0
	| SPhrases =		| NFPA-F = 0
	| RSPhrases =		| NFPA-R = 0
			| NFPA_ref = <ref name=slm2>{{cite web|url = http://www.saltlakemetals.com/MSDS_Silver_Sulfide.htm|title = MSDS of Silver Sulfide|website = saltlakemetals.com|publisher = Salt Lake Metals|access-date = 2014-07-13|place = Utah, USA|archive-date = 2014-08-10|archive-url = https://web.archive.org/web/20140810063028/http://www.saltlakemetals.com/MSDS_Silver_Sulfide.htm|url-status = dead}}</ref>
	| FlashPt =
	| Autoignition =		| LD50 =
			}}
	| ExploLimits =
	| LD50 =
	| PEL = }}
	| Section8 = {{Chembox Related
	| OtherAnions =
	| OtherCations =
	| OtherFunctn =
	| Function =
	| OtherCpds = }}
	}}		}}
	'''Silver sulfide''', Ag<sub>2</sub>S, is the ] of ]. This dense black solid constitutes the ] that forms over time on silverware and other silver objects.<ref> Silver, Chemical Element </ref> Silver sulfide is ] in all solvents, but is degraded by strong acids. Silver sulfide features a ], as it is made up of silver (] of 1.98) and sulfur (electronegativity of 2.58). It is a component of classical ].<ref>{{Greenwood&Earnshaw2nd}}</ref> When formed on ]s operating in an atmosphere rich in hydrogen sulfide, long filaments known as ] can form.		'''Silver sulfide''' is an ] with the formula {{chem|Ag|2|S}}. A dense black solid, it is the only ] of ]. It is useful as a ] in ]. It constitutes the ] that forms over time on silverware and other silver objects. Silver sulfide is ] in most solvents, but is degraded by strong acids. Silver sulfide is a network solid made up of silver (electronegativity of 1.98) and sulfur (electronegativity of 2.58) where the bonds have low ionic character (approximately 10%).
	==Structure==		== Formation ==
			Silver sulfide naturally occurs as the tarnish on silverware. When combined with silver, ] gas creates a layer of black silver sulfide ] on the silver, protecting the inner silver from further conversion to silver sulfide.<ref>{{cite book|last1=Zumdahl|first1=Steven S.|url=https://books.google.com/books?id=hsuV9JTGaP8C&pg=PA505|title=Chemical Principles|last2=DeCoste|first2=Donald J.|year=2013|isbn=978-1-111-58065-0|edition=7th|page=505|publisher=Cengage Learning }}</ref> Silver ] can form when silver sulfide forms on the surface of silver electrical contacts operating in an atmosphere rich in hydrogen sulfide and high humidity.<ref>{{Cite web|date=2002|title=Degradation of Power Contacts in Industrial Atmosphere: Silver Corrosion and Whiskers|url=https://nepp.nasa.gov/whisker/reference/tech_papers/chudnovsky2002-paper-silver-corrosion-whiskers.pdf}}</ref> Such atmospheres can exist in ] and ]s.<ref>{{Cite journal|last1=Dutta|first1=Paritam K.|last2=Rabaey|first2=Korneel|last3=Yuan|first3=Zhiguo|last4=Rozendal|first4=René A.|last5=Keller|first5=Jürg|date=2010|title=Electrochemical sulfide removal and recovery from paper mill anaerobic treatment effluent|journal=Water Research|volume=44|issue=8|pages=2563–2571|doi=10.1016/j.watres.2010.01.008|issn=0043-1354|pmid=20163816|bibcode=2010WatRe..44.2563D }}</ref><ref>{{Cite web|title=Control of Hydrogen Sulfide Generation {{!}} Water & Wastes Digest|url=https://www.wwdmag.com/corrosion/control-hydrogen-sulfide-generation|access-date=2018-07-05|website=www.wwdmag.com|date=5 March 2012 |language=en}}</ref>
	Three ] are known: monoclinic ], stable below 500&nbsp;°C, body centered cubic so-called ], stable above 176&nbsp;°C, and a high temperature face-centred cubic form stable above 586&nbsp;°C.<ref name = "Wells"> Wells A.F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications ISBN 0-19-855370-6 </ref> The higher temperature forms are electrical conductors.<ref name = "Wells"/> It is found in nature as relatively low temperature mineral ]. The name argentite refers to a cubic form, which, due to instability in "normal" temperatures, is found in form of the pseudomorphosis of acanthite after argentite. Acanthite is an important ore of silver. Ag<sub>2</sub>S is used as a photosensitizer in photography.
			==Structure and properties==
			Three ] are known: monoclinic ] (α-form), stable below 179&nbsp;°C, body centered cubic so-called ] (β-form), stable above 180&nbsp;°C, and a high temperature face-centred cubic (γ-form) stable above 586&nbsp;°C.<ref name="spring">{{cite book|doi = 10.1007/10681727_86|pages = 1–4|year = 1998|isbn = 978-3-540-31360-1|volume = 41C|publisher = Springer Berlin Heidelberg|chapter-url = https://link.springer.com/static-content/lookinside/996/chp%253A10.1007%252F10681727_86/000.png|title = Non-Tetrahedrally Bonded Elements and Binary Compounds I|series = Landolt-Börnstein - Group III Condensed Matter|chapter = Silver sulfide (Ag2S) crystal structure}}</ref> The higher temperature forms are electrical conductors. It is found in nature as relatively low temperature mineral ]. Acanthite is an important ore of silver. The acanthite, monoclinic, form features two kinds of silver centers, one with two and the other with three near neighbour sulfur atoms.<ref>Frueh, A. J. (1958). The crystallography of silver sulfide, Ag2S. Zeitschrift für Kristallographie-Crystalline Materials, 110(1-6), 136-144.</ref> Argentite refers to a cubic form, which, due to instability in "normal" temperatures, is found in form of the ] of acanthite after argentite.
			== Exceptional ductility of α-Ag<sub>2</sub>S ==
			Relative to most inorganic materials, α-Ag<sub>2</sub>S displays exceptional ductility at room temperature.<ref name=":1">{{Cite journal |last=Chen |first=Lidong |year=2018 |title=Room-temperature ductile inorganic semiconductor |url=https://www.nature.com/articles/s41563-018-0047-z |journal=Nature Materials |volume=17 |pages=421-426}}</ref><ref>{{Cite journal |last=Chen |first=Lidong |title=Flexible thermoelectrics based on ductile semiconductors |url=https://www.science.org/doi/full/10.1126/science.abq0682 |journal=Science |volume=377 |issue=6608 |pages=854-858}}</ref> This material can undergo extensive deformation, akin to metals, without fracturing. Such behavior is evident in various mechanical tests; for instance, α-Ag2S can be easily machined into cylindrical or bar shapes and can withstand substantial deformation under compression, three-point bending, and tensile stresses. The material sustains over 50% engineering strain in compression tests and up to 20% or more in bending tests.<ref name=":1" />
			The intrinsic ductility of alpha-phase silver sulfide (α-Ag<sub>2</sub>S) is underpinned by its unique structural and chemical bonding characteristics. At the atomic level, its monoclinic crystal structure, which remains stable up to 451 K, enables the movement of atoms and dislocations along well-defined crystallographic planes known as slip planes. Additionally, the dynamic bonding within the crystal structure supports both the sliding of atomic layers and the maintenance of material integrity during deformation. The interatomic forces within the slip planes are sufficiently strong to prevent the material from cleaving while still allowing for considerable flexibility.<ref name=":1" /> Further insights into α-Ag<sub>2</sub>S's ductility come from density functional theory calculations, which reveal that the primary slip planes align with the direction and slipping occurs along the direction. This arrangement permits atoms to glide over each other under stress through minute adjustments in the interlayer distances, which are energetically favorable as indicated by low slipping energy barriers (ΔE<sub>B</sub>) and high cleavage energies (ΔE<sub>C</sub>). These properties ensure significant deformation capability without fracture. Silver and sulfur atoms in α-Ag<sub>2</sub>S form transient, yet robust interactions that enable the material to retain its integrity while deforming. This behavior is akin to that of metals, where dislocations move with relative ease, providing α-Ag<sub>2</sub>S with a unique combination of flexibility and strength, making it exceptionally resistant to cracking under mechanical stress.<ref name=":1" />
			== History ==
			In 1833 ] noticed that the resistance of silver sulfide decreased dramatically as temperature increased. This constituted the first report of a semiconducting material.<ref name="CHM-semicon">{{cite web|title=1833 - First Semiconductor Effect is Recorded|url=http://www.computerhistory.org/semiconductor/timeline/1833-first.html|access-date=24 June 2014|website=Computer History Museum}}</ref>
			Silver sulfide is a component of classical ].<ref>{{Greenwood&Earnshaw2nd}}</ref>
	==References==		==References==
	{{reflist}}		{{reflist}}
			==External links==
			* V&A Conservation Journal
			* NASA
			{{Commons category|Silver sulfide}}
	{{Silver compounds}}		{{Silver compounds}}
			{{Sulfides}}
			{{Authority control}}
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