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{{Redirect|PbS|other uses|PBS (disambiguation)}}
{{chembox {{chembox
| Verifiedfields = changed
| verifiedrevid = 447377289
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| ImageFile1 = Galena-unit-cell-3D-ionic.png
| verifiedrevid = 450727917
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| ImageFile1 = Galena-unit-cell-3D-ionic.png
| ImageFile2 = Sulfid olovnatý.PNG
| ImageFile2 = Sulfid olovnatý.PNG
| ImageSize2 = 244
| ImageSize2 = 244
| ImageName = Lead(II) sulfide
| ImageName = Lead(II) sulfide
| IUPACName =
| IUPACName =
| OtherNames = Plumbous sulfide<br />]
| OtherNames = Plumbous sulfide<br />], Sulphuret of lead
| Section1 = {{Chembox Identifiers
| Section1 = {{Chembox Identifiers
| CASNo = 1314-87-0
| Abbreviations =
| CASNo_Ref = {{cascite}}
| CASNo = 1314-87-0
| CASNo_Comment =
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNoOther =
| PubChem = 14819
| ChemSpiderID = 14135
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID_Comment =
| EC_number = 215-246-6
| RTECS = OG4550000
| UNNumber = 3077
| UNII = 2425D15SYM
| UNII_Ref = {{fdacite|correct|FDA}}
| DrugBank =
| KEGG =
| KEGG_Ref = {{keggcite|correct|kegg}}
| MeSHName =
| ChEBI =
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEMBL =
| ChEMBL_Ref = {{ebicite|correct|EBI}}
| SMILES = =S
| InChI =
| StdInChI = 1S/Pb.S
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| StdInChIKey = XCAUINMIESBTBL-UHFFFAOYSA-N
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| Beilstein =
| Gmelin =
| 3DMet =
}} }}
| Section2 = {{Chembox Properties | Section2 = {{Chembox Properties
| Formula = PbS | Formula = PbS
| MolarMass = 239.30 g/mol | MolarMass = 239.30{{nbsp}}g/mol
| Appearance = Black
| Density = 7.60 g/cm<sup>3</sup><ref>{{cite book | last =Patnaik | first =Pradyot | year = 2003 | title =Handbook of Inorganic Chemical Compounds | publisher = McGraw-Hill | page = | isbn =0070494398 | url= http://books.google.com/?id=Xqj-TTzkvTEC&pg=PA119 | accessdate = 2009-06-06}}</ref>
| Density = 7.60{{nbsp}}g/cm<sup>3</sup><ref name=crc>Haynes, p. 4.69</ref>
| Solubility = 2.6{{e|-11}} kg/kg (calculated, at pH=7)<ref>{{cite book|author=W. Linke|title=Solubilities. Inorganic and Metal-Organic Compounds|volume=2|page=1318|publisher= American Chemical Society|location= Washington, D.C.|year= 1965}}</ref> 8.6{{e|-7}}</sup> kg/kg<ref>{{cite book|url=http://books.google.com/?id=cl1Kry_k6ZUC&pg=PA206|title= Handbook of Chemical Risk Assessment|author=Ronald Eisler|publisher=CRC Press|year= 2000|isbn=1566705061}}</ref>
| Solubility = 2.6{{e|-11}}{{nbsp}}kg/kg (calculated, at pH=7)<ref>{{cite book|author=Linke, W. |title=Solubilities. Inorganic and Metal-Organic Compounds|volume=2|page=1318|publisher= American Chemical Society|location= Washington, D.C.|year= 1965}}</ref> 8.6{{e|-7}} kg/kg<ref>{{cite book|url=https://books.google.com/books?id=cl1Kry_k6ZUC&pg=PA206|title= Handbook of Chemical Risk Assessment|author=Ronald Eisler|publisher=CRC Press|year= 2000|isbn=978-1-56670-506-6}}</ref>
| SolubilityProduct = 9.04{{e|-29}}
| SolubilityProduct =
| MeltingPtC = 1118
| MeltingPtC = 1113<ref name=crc/>
| BoilingPtC = 1281
| RefractIndex = 3.91 | MeltingPt_ref =
| BoilingPtC = 1281
| RefractIndex = 3.91<ref>Haynes, p. 4.135</ref>
| MagSus = −83.6·10<sup>−6</sup>{{nbsp}}cm<sup>3</sup>/mol<ref>Haynes, p. 4.128</ref>
}} }}
| Section3 = {{Chembox Structure | Section3 = {{Chembox Structure
| CrystalStruct = ] (cubic), ] | CrystalStruct = ] (cubic), ]
| SpaceGroup = Fm{{overline|3}}m, No. 225 | SpaceGroup = Fm{{overline|3}}m, No. 225
| Coordination = Octahedral (Pb<sup>2+</sup>)<br />Octahedral (S<sup>2−</sup>) | Coordination = Octahedral (Pb<sup>2+</sup>)<br />Octahedral (S<sup>2−</sup>)
| LattConst_a = | LattConst_a = 5.936{{nbsp}}Å
| UnitCellFormulas = 4
|Structure_ref= <ref>Haynes, p. 4.141</ref>
|Dipole = 3.59 D<ref>Haynes, p. 9.63</ref>
}} }}
| Section4 = {{Chembox Thermochemistry | Section4 = {{Chembox Thermochemistry
|Thermochemistry_ref= <ref>Haynes, p. 5.25</ref>
| DeltaHf = –1.00{{e|2}} kJ/mol
| Entropy = –98.7 kJ/mol | DeltaHf = −100.4{{nbsp}}kJ/mol
| DeltaGf = −98.7{{nbsp}}kJ/mol
| HeatCapacity = 46.02 J/degree mol
| Entropy = 91.2{{nbsp}}J/mol
| HeatCapacity = 49.5{{nbsp}}J/mol⋅K
}} }}
| Section7 = {{Chembox Hazards | Section7 = {{Chembox Hazards
| ExternalMSDS = | ExternalSDS =
| GHSPictograms = {{GHS07}}{{GHS08}}{{GHS09}}
| EUIndex = 082-001-00-6
| GHSSignalWord = Danger
| EUClass = Repr. Cat. 1/3<br />Harmful ('''Xn''')<br />Dangerous for the environment ('''N''')
| HPhrases = {{H-phrases|302|332|360|373|410}}
| RPhrases = {{R61}}, {{R20/22}}, {{R33}}, {{R62}}, {{R50/53}}
| PPhrases = {{P-phrases|201|202|260|261|264|270|271|273|281|301+312|304+312|304+340|308+313|312|314|330|391|405|501}}
| SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}}
| NFPA-H = 2 | NFPA-H = 2
| NFPA-F = 0 | NFPA-F = 0
| NFPA-R = 0 | NFPA-R = 0
| NFPA-O = | NFPA-S =
| FlashPt = Non-flammable | FlashPt = Non-flammable
}} }}
| Section8 = {{Chembox Related | Section8 = {{Chembox Related
| OtherAnions = ]<br />]<br />] | OtherAnions = ]<br />]<br />]
| OtherCations = ]<br />]<br />]<br />] | OtherCations = ]<br />]<br />]<br />]
| OtherCpds = ]<br />]<br />] | OtherCompounds = ]<br />]<br />]
}} }}
}} }}


'''Lead(II) sulfide''' (also spelled ]) is an ] with the ] ]{{Sulfur}}. It finds limited use in electronic devices. PbS, also known as ], is the principal ore and most important compound of lead. '''Lead(II) sulfide''' (also spelled '']'') is an ] with the ] ]]. ] is the principal ore and the most important compound of ]. It is a semiconducting material with niche uses.


==Formation, basic properties, related materials== ==Formation, basic properties, related materials==
Addition of hydrogen sulfide or sulfide salts to a solution of lead ions gives a poorly soluble black product consisting of PbS: Addition of ] or sulfide salts to a solution containing a lead salt, such as PbCl<sub>2</sub>, gives a black precipitate of lead sulfide.
:Pb<sup>2+</sup> + H<sub>2</sub>S → PbS + 2 H<sup>+</sup> : Pb<sup>2+</sup> + H<sub>2</sub>S → PbS↓ + 2 H<sup>+</sup>
The equilibrium constant for this reaction is 3{{e|6}} M.<ref>{{RubberBible86th}}
</ref>
This reaction, which entails a dramatic color change from colourless or white to black, was once used in ]. The presence of hydrogen sulfide or sulfide ions is still routinely tested using "lead acetate paper."


This reaction is used in ]. The presence of hydrogen sulfide or sulfide ions may be tested using "lead acetate paper."
Like the related materials ] and ], PbS is a ].<ref>{{cite book|author=Vaughan, D. J.; Craig, J. R. |title=Mineral Chemistry of Metal Sulfides|publisher= Cambridge University Press|location= Cambridge|year= 1978|isbn=0521214890}};</ref> In fact, lead sulfide was one of the earliest materials to be used as a semiconductor.<ref>C.Michael Hogan. 2011. </ref> Lead sulfide crystallizes in the ] motif, unlike many other ]s.

Like the related materials ] and ], PbS is a ].<ref>{{cite book|author1=Vaughan, D. J. |author2=Craig, J. R. |title=Mineral Chemistry of Metal Sulfides|publisher= Cambridge University Press|location= Cambridge|year= 1978|isbn=978-0-521-21489-6}};</ref> In fact, lead sulfide was one of the earliest materials to be used as a semiconductor.<ref>Hogan, C. Michael (2011). . in ''Encyclopedia of Earth'', eds. A. Jorgensen and C.J. Cleveland, National Council for Science and the environment, Washington DC. {{webarchive|url=https://web.archive.org/web/20121028080550/http://www.eoearth.org/article/Sulfur?topic=49557 |date=2012-10-28 }}</ref> Lead sulfide crystallizes in the ] motif, unlike many other ]s.

Since PbS is the main ore of lead, much effort has focused on its conversion. A major process involves ] of PbS followed by reduction of the resulting ]. Idealized equations for these two steps are:<ref>{{cite book|author1=Sutherland, Charles A. |author2=Milner, Edward F. |author3=Kerby, Robert C. |author4=Teindl, Herbert |author5=Melin, Albert |author6=Bolt, Hermann M. |chapter=Lead|title= Ullmann's Encyclopedia of Industrial Chemistry|year= 2005 |publisher=Wiley-VCH|location= Weinheim|doi=10.1002/14356007.a15_193.pub2|isbn=978-3527306732 }}</ref>
: 2 PbS + 3 O<sub>2</sub> → 2 ] + 2 SO<sub>2</sub>
: PbO + C → Pb + CO


Since PbS is the main ore of lead, much effort has focused on its conversion. A major process involves ] of PbS followed by reduction of the resulting ]. Idealized equations for these two steps are:<ref>{{cite book|author=Charles A. Sutherland, Edward F. Milner, Robert C. Kerby, Herbert Teindl, Albert Melin, Hermann M. Bolt |title=Lead. in Ullmann's Encyclopedia of Industrial Chemistry|year= 2005 |publisher=Wiley-VCH|location= Weinheim|doi=10.1002/14356007.a15_193.pub2}}</ref>
:2 PbS + 3 O<sub>2</sub> → 2 PbO + 2 SO<sub>2</sub>
:PbO + C → Pb + CO
The ] is converted to ]. The ] is converted to ].

=== Nanoparticles ===
Lead sulfide-containing ] and ]s have been well studied.<ref>{{Cite journal|title = The Quantum Mechanics of Larger Semiconductor Clusters ("Quantum Dots")|journal = Annual Review of Physical Chemistry|date = 1990-01-01|pages = 477–496|volume = 41|issue = 1|doi = 10.1146/annurev.pc.41.100190.002401|first3 = L. E.|last3 = Brus|bibcode = 1990ARPC...41..477B}}</ref> Traditionally, such materials are produced by combining lead salts with a variety of sulfide sources.<ref>{{Cite journal|title = Coated semiconductor nanoparticles; the cadmium sulfide/lead sulfide system's synthesis and properties|journal = The Journal of Physical Chemistry|date = 2002-05-01|pages = 895–901|volume = 97|issue = 4|doi = 10.1021/j100106a015|language = EN|first1 = H. S.|last1 = Zhou|first2 = I.|last2 = Honma|first3 = H.|last3 = Komiyama|first4 = Joseph W.|last4 = Haus}}</ref><ref>{{Cite journal|title = A novel and simple one-step solid-state reaction for the synthesis of PbS nanoparticles in the presence of a suitable surfactant|journal = Materials Research Bulletin|date = 2001-09-15|pages = 1977–1984|volume = 36|issue = 11|doi = 10.1016/S0025-5408(01)00678-X|first1 = Wenzhong|last1 = Wang|first2 = Yingkai|last2 = Liu|first3 = Yongjie|last3 = Zhan|first4 = Changlin|last4 = Zheng|first5 = Guanghou|last5 = Wang}}</ref> In 2009, PbS nanoparticles have been examined for use in solar cells.<ref>{{Cite journal|title = PbS and CdS Quantum Dot-Sensitized Solid-State Solar Cells: "Old Concepts, New Results"|journal = Advanced Functional Materials|date = 2009-09-09|issn = 1616-3028|pages = 2735–2742|volume = 19|issue = 17|doi = 10.1002/adfm.200900081|language = en|first1 = HyoJoong|last1 = Lee|first2 = Henry C.|last2 = Leventis|first3 = Soo-Jin|last3 = Moon|first4 = Peter|last4 = Chen|first5 = Seigo|last5 = Ito|first6 = Saif A.|last6 = Haque|first7 = Tomas|last7 = Torres|first8 = Frank|last8 = Nüesch|first9 = Thomas|last9 = Geiger| s2cid=98631978 |doi-access = free}}</ref>


==Applications== ==Applications==
] used in the early 1900s]]
PbS was once used as a black pigment, but current applications exploit its semiconductor properties, which have long been recognized.<ref>{{cite journal|doi=10.1088/0370-1301/64/7/110|title=Lead Sulphide – An Intrinsic Semiconductor|year=1951|author=Putley, E H|journal=Proceedings of the Physical Society Section B|volume=64|pages=616|last2=Arthur|first2=J B}}</ref> PbS is one of the oldest and most common detection element materials in various ]s. As an infrared detector, PbS functions as a photon detector, responding directly to the photons of radiation, as opposed to thermal detectors, which respond to a change in detector element temperature caused by the radiation.
]


=== Photodetector ===
A PbS element can be used to measure radiation in either of two ways: by measuring the tiny ] the photons cause when they hit the PbS material, or by measuring the change in the material's ] that the photons cause. Measuring the resistance change is the more commonly used method.
{{See also|Photoconductivity}}
PbS was one of the first materials used for electrical diodes that could detect electromagnetic radiation, including ].<ref>{{cite journal |doi=10.1088/0370-1301/64/7/110 |title=Lead Sulphide – An Intrinsic Semiconductor |year=1951 |author=Putley, E H |journal=Proceedings of the Physical Society | series = Series B | volume=64 |issue=7 |pages=616–618 |last2=Arthur |first2=J B|author-link=E. H. Putley }}</ref> As an infrared sensor, PbS directly detects light, as opposed to thermal detectors, which respond to a change in detector element temperature caused by the radiation. A PbS element can be used to measure radiation in either of two ways: by measuring the tiny ] the photons cause when they hit the PbS material, or by measuring the change in the material's ] that the photons cause. Measuring the resistance change is the more commonly used method. At ], PbS is sensitive to radiation at ]s between approximately 1 and 2.5 ]. This range corresponds to the shorter wavelengths in the infra-red portion of the ], the so-called short-wavelength infrared (SWIR). Only very hot objects emit radiation in these wavelengths.


Cooling the PbS elements, for example using liquid nitrogen or a ] system, shifts its sensitivity range to between approximately 2 and 4 ]. Objects that emit radiation in these wavelengths still have to be quite hot—several hundred degrees ]—but not as hot as those detectable by uncooled sensors. (Other compounds used for this purpose include ] (InSb) and ] (HgCdTe), which have somewhat better properties for detecting the longer IR wavelengths.) The high ] of PbS leads to relatively slow detectors (compared to ], ], InSb, or HgCdTe).
At ], PbS is sensitive to radiation at ]s between approximately 1 and 2.5 ]. This range corresponds to the shorter wavelengths in the infra-red portion of the ], the so-called short-wavelength infrared (SWIR). Only very hot objects emit radiation in these wavelengths.


==Planetary science==
Cooling the PbS elements, for example using liquid nitrogen or a ] system, shifts its sensitivity range to between approximately 2 and 4 ]. Objects that emit radiation in these wavelengths still have to be quite hot—several hundred degrees ]—but not as hot as those detectable by uncooled sensors. Other compounds used for this purpose include ] (InSb) and ] (HgCdTe), which have somewhat better properties for detecting the longer IR wavelengths. The high dielectric constant of PbS leads to relatively slow detectors (compared to ], ], InSb, or HgCdTe).
Elevations above 2.6&nbsp;km (1.63&nbsp;mi) on the ] ] are coated with a shiny substance. Though the composition of this coat is not entirely certain, one theory is that Venus "]s" crystallized lead sulfide much as ] snows frozen water. If this is the case, it would be the first time the substance was identified on a foreign planet. Other less likely candidates for Venus' "snow" are ] and ].<ref>{{cite news|url=http://news-info.wustl.edu/news/page/normal/633.html|access-date=2009-07-07|title='Heavy metal' snow on Venus is lead sulfide|publisher=]|archive-date=2008-04-15|archive-url=https://web.archive.org/web/20080415000214/http://news-info.wustl.edu/news/page/normal/633.html|url-status=live}}</ref>

==Astronomy==
Elevations above 2.6&nbsp;km (1.63&nbsp;mi) on the ] ] are coated with a shiny substance. Though the composition of this coat is not entirely certain, one theory is that Venus "]s" crystallized lead sulfide much as ] snows frozen water. If this is the case, it would be the first time the substance was identified on a foreign planet. Other less likely candidates for Venus' "snow" are ] and ].<ref>{{cite news|url=http://news-info.wustl.edu/news/page/normal/633.html|accessdate=2009-07-07|title='Heavy metal' snow on Venus is lead sulfide|publisher= Washington University in St. Louis}}</ref>


==Safety== ==Safety==
Lead(II) sulfide is toxic if the lead and sulfur are heated to decomposition and toxic compounds of lead and sulfur oxides are produced (such as in a fire).<ref></ref> Lead sulfide is insoluble and a stable compound in the pH of blood and so is probably one of the less toxic forms of lead.<ref>{{cite journal|title=Studies on the Toxicity of Various Lead Compounds Given Intravenously|author= Fritz Bischoff, L. C. Maxwell, Richard D. Evens and Franklin R. Nuzum|journal= Journal of Pharmacology and Experimental Therapeutics|year= 1928|volume=34 |issue=1 |pages=85–109|url= http://jpet.aspetjournals.org/content/34/1/85.abstract}}</ref> Lead(II) sulfide is so insoluble that it is almost nontoxic, but pyrolysis of the material, as in smelting, gives dangerous toxic fumes of lead and oxides of sulfur.<ref>{{Cite web |url=http://www.espimetals.com/msds%27s/leadsulfide.pdf |title=Lead sulfide MSDS |access-date=2009-11-20 |archive-url=https://web.archive.org/web/20061111080525/http://www.espimetals.com/msds's/leadsulfide.pdf |archive-date=2006-11-11 |url-status=dead }}</ref> Lead sulfide is insoluble and a stable compound in the pH of blood and so is probably one of the less toxic forms of lead.<ref>{{cite journal |url=https://jpet.aspetjournals.org/content/34/1/85|title=Studies on the Toxicity of Various Lead Compounds Given Intravenously |author1=Bischoff, Fritz |author2=Maxwell, L. C. |author3=Evens, Richard D. |author4=Nuzum, Franklin R. |journal=Journal of Pharmacology and Experimental Therapeutics |year=1928 |volume=34 |issue=1 |pages=85–109 }}</ref> A large safety risk occurs in the synthesis of PbS using lead carboxylates, as they are particularly soluble and can cause ]


==References== ==References==
{{reflist|30em}} {{reflist|30em}}

==Cited sources==
*{{cite book |ref=Haynes| editor= Haynes, William M. | date = 2016| title = ] | edition = 97th | publisher = ] | isbn = 9781498754293}}


==External links== ==External links==
{{Commons cat|Lead(II) sulfide}} {{Commons category|Lead(II) sulfide}}
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{{Lead compounds}} {{Lead compounds}}
{{Sulfides}}


{{DEFAULTSORT:Lead(Ii) Sulfide}} {{DEFAULTSORT:Lead(Ii) Sulfide}}
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