Lead(II) sulfide: Difference between revisions

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			{{Redirect\|PbS\|other uses\|PBS (disambiguation)}}
	{{chembox		{{chembox
			\| Verifiedfields = changed
	\| verifiedrevid = 447377289
			\| Watchedfields = changed
	\| ImageFile1 = Galena-unit-cell-3D-ionic.png
			\| verifiedrevid = 450727917
	\| ImageSize1 = 200
			\| 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 pressurised or liquified gas 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 km (1.63 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 km (1.63 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>~~MSDS~~ http://www.espimetals.com/msds%27s/leadsulfide.pdf</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>Studies on the Toxicity of Various Lead Compounds Given Intravenously. Fritz ~~Bischoff~~, L. C. ~~Maxwell~~, Richard D. ~~Evens and~~ Franklin R. ~~Nuzum.~~ Journal of Pharmacology and Experimental Therapeutics~~, September~~ 1928 ~~vol.~~ 34 ~~no.~~ 1 ~~85-109~~ ~~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}}
	*		*
	*		*
	*		*

	{{Lead compounds}}		{{Lead compounds}}
			{{Sulfides}}

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

	]
	]
	]
	]
	]
	]
	]
	]

Latest revision as of 14:10, 14 April 2024

"PbS" redirects here. For other uses, see PBS (disambiguation).

Lead(II) sulfide
Names


Other names Plumbous sulfide Galena, Sulphuret of lead
Identifiers
CAS Number	1314-87-0
3D model (JSmol)	Interactive image
ChemSpider	14135
ECHA InfoCard	100.013.861
EC Number	215-246-6
PubChem CID	14819
RTECS number	OG4550000
UNII	2425D15SYM
UN number	3077
CompTox Dashboard (EPA)	DTXSID401352852 DTXSID0025498, DTXSID401352852
InChI InChI=1S/Pb.SKey: XCAUINMIESBTBL-UHFFFAOYSA-N
SMILES =S
Properties
Chemical formula	PbS
Molar mass	239.30 g/mol
Appearance	Black
Density	7.60 g/cm
Melting point	1,113 °C (2,035 °F; 1,386 K)
Boiling point	1,281 °C (2,338 °F; 1,554 K)
Solubility in water	2.6×10 kg/kg (calculated, at pH=7) 8.6×10 kg/kg
Magnetic susceptibility (χ)	−83.6·10 cm/mol
Refractive index (n_D)	3.91
Structure
Crystal structure	Halite (cubic), cF8
Space group	Fm3m, No. 225
Lattice constant	a = 5.936 Å
Formula units (Z)	4
Coordination geometry	Octahedral (Pb) Octahedral (S)
Dipole moment	3.59 D
Thermochemistry
Heat capacity (C)	49.5 J/mol⋅K
Std molar entropy (S₂₉₈)	91.2 J/mol
Std enthalpy of formation (Δ_fH₂₉₈)	−100.4 kJ/mol
Gibbs free energy (Δ_fG)	−98.7 kJ/mol
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H302, H332, H360, H373, H410
Precautionary statements	P201, P202, P260, P261, P264, P270, P271, P273, P281, P301+P312, P304+P312, P304+P340, P308+P313, P312, P314, P330, P391, P405, P501
NFPA 704 (fire diamond)	2 0 0
Flash point	Non-flammable
Safety data sheet (SDS)	External MSDS
Related compounds
Other anions	Lead(II) oxide Lead selenide Lead telluride
Other cations	Carbon monosulfide Silicon monosulfide Germanium(II) sulfide Tin(II) sulfide
Related compounds	Thallium sulfide Lead(IV) sulfide Bismuth sulfide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). N verify (what is ?) Infobox references

Chemical compound

Lead(II) sulfide (also spelled sulphide) is an inorganic compound with the formula Pb S. Galena is the principal ore and the most important compound of lead. It is a semiconducting material with niche uses.

Formation, basic properties, related materials

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

Pb + 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 PbSe and PbTe, PbS is a semiconductor. In fact, lead sulfide was one of the earliest materials to be used as a semiconductor. Lead sulfide crystallizes in the sodium chloride motif, unlike many other IV-VI semiconductors.

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:

2 PbS + 3 O₂ → 2 PbO + 2 SO₂

PbO + C → Pb + CO

The sulfur dioxide is converted to sulfuric acid.

Nanoparticles

Lead sulfide-containing nanoparticle and quantum dots have been well studied. Traditionally, such materials are produced by combining lead salts with a variety of sulfide sources. In 2009, PbS nanoparticles have been examined for use in solar cells.

Applications

Galena-based cat's-whisker detector used in the early 1900s

Photodetector

Planetary science

Elevations above 2.6 km (1.63 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 "snows" 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.

Safety

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. 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. A large safety risk occurs in the synthesis of PbS using lead carboxylates, as they are particularly soluble and can cause negative physiological conditions.

References

^ Haynes, p. 4.69
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Cited sources

Haynes, William M., ed. (2016). CRC Handbook of Chemistry and Physics (97th ed.). CRC Press. ISBN 9781498754293.

External links

v t e Lead compounds
Pb(II)	Pb(BiO₃)₂ PbBr₂ Pb(C₅H₅)₂ Pb(C₂H₃O₂)₂ PbC₂O₄ PbC₃₂H₁₆N₈ PbCl₂ Pb(ClO₄)₂ PbCO₃ PbCrO₄ PbF₂ PbHAsO₄ PbI₂ Pb(C ₁₁H ₂₃COO) ₂ Pb(NO₃)₂ Pb(N₃)₂ PbO Pb(OH)₂ PbPo PbP₇ Pb₃(PO₄)₂ PbS Pb(SCN)₂ PbSe PbSO₄ PbSeO₄ PbTe PbTiO₃ PbGeO₃ C ₃₆H ₇₀PbO ₄ PbO2−2 PbC₂ (hypothetical)
Pb(II,IV)	Pb₃O₄
Pb(IV)	Pb(C₂H₃O₂)₄ PbCl₄ PbF₄ PbH₄ PbO₂ PbS₂ plumbate Pb(OH)₄ (hypothetical)