Lead(II) sulfide: Difference between revisions

{{Redirect|PbS|other uses|PBS (disambiguation)}}

| Verifiedfields = changed

| Watchedfields = changed

| verifiedrevid = 450727917

| ImageFile1 = Galena-unit-cell-3D-ionic.png

| ImageFile2 = Sulfid olovnatý.PNG

| ImageSize2 = 244

| ImageName = Lead(II) sulfide

| IUPACName =

| OtherNames = Plumbous sulfide<br />[[Galena]], Sulphuret of lead

| Section1 = {{Chembox Identifiers

| Abbreviations =

| 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 = [Pb]=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

| Formula = PbS

| MolarMass = 239.30{{nbsp}}g/mol

| Appearance = Black

| Density = 7.60{{nbsp}}g/cm³<ref name=crc>Haynes, p. 4.69</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 =

| MeltingPtC = 1113<ref name=crc/>

| MeltingPt_ref =

| BoilingPtC = 1281

| RefractIndex = 3.91<ref>Haynes, p. 4.135</ref>

| MagSus = −83.6·10⁻⁶{{nbsp}}cm³/mol<ref>Haynes, p. 4.128</ref>

| Section3 = {{Chembox Structure

| CrystalStruct = [[Halite]] (cubic), [[Pearson symbol|cF8]]

| SpaceGroup = Fm{{overline|3}}m, No. 225

| Coordination = Octahedral (Pb²⁺)<br />Octahedral (S²⁻)

| 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

|Thermochemistry_ref= <ref>Haynes, p. 5.25</ref>

| DeltaHf = −100.4{{nbsp}}kJ/mol

| DeltaGf = −98.7{{nbsp}}kJ/mol

| Entropy = 91.2{{nbsp}}J/mol

| HeatCapacity = 49.5{{nbsp}}J/mol⋅K

| Section7 = {{Chembox Hazards

| ExternalSDS = [http://msds.chem.ox.ac.uk/LE/lead_sulfide.html External MSDS]

| GHSPictograms = {{GHS07}}{{GHS08}}{{GHS09}}

| GHSSignalWord = Danger

| HPhrases = {{H-phrases|302|332|360|373|410}}

| 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}}

| NFPA-H = 2

| NFPA-F = 0

| NFPA-R = 0

| NFPA-S =

| FlashPt = Non-flammable

| Section8 = {{Chembox Related

| OtherAnions = [[Lead(II) oxide]]<br />[[Lead selenide]]<br />[[Lead telluride]]

| OtherCations = [[Carbon monosulfide]]<br />[[Silicon monosulfide]]<br />[[Germanium(II) sulfide]]<br />[[Tin(II) sulfide]]

| OtherCompounds = [[Thallium sulfide]]<br />[[Lead(IV) sulfide]]<br />[[Bismuth sulfide]]

'''Lead(II) sulfide''' (also spelled ''[[Sulfur#Spelling and etymology|sulphide]]'') is an [[inorganic compound]] with the [[chemical formula|formula]] [[Lead|Pb]][[Sulfide|S]]. [[Galena]] is the principal ore and the most important compound of [[lead]]. It is a semiconducting material with niche uses.

Addition of [[hydrogen sulfide]] or sulfide salts to a solution containing a lead salt, such as PbCl₂, gives a black precipitate of lead sulfide.

: Pb²⁺ + H₂S → PbS↓ + 2 H⁺

This reaction is used in [[qualitative inorganic analysis]]. The presence of hydrogen sulfide or sulfide ions may be tested using "lead acetate paper."

Like the related materials [[lead selenide|PbSe]] and [[lead telluride|PbTe]], PbS is a [[semiconductor]].<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). [http://www.eoearth.org/article/Sulfur?topic=49557 "Sulfur"]. 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 [[sodium chloride]] motif, unlike many other [[List of semiconductor materials#Group IV-VI|IV-VI semiconductor]]s.

Since PbS is the main ore of lead, much effort has focused on its conversion. A major process involves [[smelting]] of PbS followed by reduction of the resulting [[oxide]]. 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 O₂ → 2 [[Lead(II) oxide|PbO]] + 2 SO₂

: PbO + C → Pb + CO

=== Nanoparticles ===

Lead sulfide-containing [[nanoparticle]] and [[quantum dot]]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>

[[File:CatWhisker.jpg|thumb|left|Galena-based [[cat's-whisker detector]] used in the early 1900s]]

[[File:German WWII PbS IR detector.jpg|thumb|left|World War II German PbS infrared detector]]

=== Photodetector ===

{{See also|Photoconductivity}}

PbS was one of the first materials used for electrical diodes that could detect electromagnetic radiation, including [[infrared light]].<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 [[photocurrent]] the photons cause when they hit the PbS material, or by measuring the change in the material's [[electrical resistance]] that the photons cause. Measuring the resistance change is the more commonly used method. At [[room temperature]], PbS is sensitive to radiation at [[wavelength]]s between approximately 1 and 2.5 [[micrometre|μm]]. This range corresponds to the shorter wavelengths in the infra-red portion of the [[electromagnetic spectrum|spectrum]], 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 [[Peltier element]] system, shifts its sensitivity range to between approximately 2 and 4 [[μm]]. Objects that emit radiation in these wavelengths still have to be quite hot—several hundred degrees [[Celsius]]—but not as hot as those detectable by uncooled sensors. (Other compounds used for this purpose include [[indium antimonide]] (InSb) and [[HgCdTe|mercury-cadmium telluride]] (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 [[silicon]], [[germanium]], InSb, or HgCdTe).

==Planetary science==

Elevations above 2.6&nbsp;km (1.63&nbsp;mi) on the [[planet]] [[Venus]] are coated with a shiny substance. Though the composition of this coat is not entirely certain, one theory is that Venus "[[Venus snow|snow]]s" crystallized lead sulfide much as [[Earth]] 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 [[bismuth sulfide]] and [[tellurium]].<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=[[Washington University in St. Louis]]|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>

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 [[Lead poisoning|negative physiological conditions.]]

==Cited sources==

*{{cite book |ref=Haynes| editor= Haynes, William M. | date = 2016| title = [[CRC Handbook of Chemistry and Physics]] | edition = 97th | publisher = [[CRC Press]] | isbn = 9781498754293}}

{{Commons category|Lead(II) sulfide}}

* [https://www.atsdr.cdc.gov/csem/csem.html Case Studies in Environmental Medicine (CSEM): Lead Toxicity]

* [https://www.atsdr.cdc.gov/toxfaqs/tfacts13.pdf ToxFAQs: Lead]

* [https://web.archive.org/web/20080111154608/http://www.npi.gov.au/database/substance-info/profiles/50.html National Pollutant Inventory – Lead and Lead Compounds Fact Sheet]

{{Sulfides}}

[[Category:Lead(II) compounds]]

[[Category:Monosulfides]]

[[Category:IV-VI semiconductors]]

[[Category:Rock salt crystal structure]]