View source for Barium sulfide

{{Short description|Chemical compound}}
{{distinguish|Barium sulfate}}
{{chembox
| Watchedfields  = changed
| verifiedrevid  = 443414470
| ImageFile      = NaCl polyhedra.png
| ImageSize      = 
| IUPACName      = 
| OtherNames     = 
| Section1       = {{Chembox Identifiers
| InChI = 1/Ba.S/q+2;-2
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 32590
| SMILES = [Ba+2].[S-2]
| InChIKey = CJDPJFRMHVXWPT-UHFFFAOYAO
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/Ba.S/q+2;-2
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = CJDPJFRMHVXWPT-UHFFFAOYSA-N
| CASNo = 21109-95-5
| CASNo_Ref = {{cascite|correct|CAS}}
| PubChem = 6857597
| EINECS = 244-214-4
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID =5256933
| UNII = TV3U2GEW4H
| Gmelin = 13627
  }}
| Section2       = {{Chembox Properties
| Formula = 
| Ba=1 | S=1
| MolarMass = 169.39 g/mol
| Appearance = white solid
| Density = 4.25 g/cm<sup>3</sup> <ref>{{RubberBible87th}}</ref>
| MeltingPtC = 2235<ref name=Stinn2017>Stinn, C., Nose, K., Okabe, T. et al. Metall and Materi Trans B (2017) 48: 2922. https://doi.org/10.1007/s11663-017-1107-5 {{Webarchive|url=https://web.archive.org/web/20240101061122/https://link.springer.com/article/10.1007/s11663-017-1107-5 |date=2024-01-01 }}</ref>
| MeltingPt_notes = 
| BoilingPt = decomposes
| Solubility = 2.88 g/100 mL (0 °C) <br> 7.68 g/100 mL (20 °C) <br> 60.3 g/100 mL (100 °C) (reacts)
| SolubleOther = insoluble in alcohol
| RefractIndex = 2.155
  }}
| Section3       = {{Chembox Structure
| CrystalStruct = [[Halite]] (cubic), [[Pearson symbol|cF8]]
| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225
| Coordination = Octahedral (Ba<sup>2+</sup>); octahedral (S<sup>2−</sup>)
| LattConst_a = 
  }}
| Section7       = {{Chembox Hazards
| GHSPictograms = {{GHS07}}{{GHS09}}
| GHSSignalWord = Warning
| HPhrases = {{H-phrases|315|319|335|400}}
| PPhrases = {{P-phrases|261|264|271|273|280|302+352|304+340|305+351+338|312|321|332+313|337+313|362|391|403+233|405|501}}
| LD50=226 mg/kg humans
| NFPA-H = 2
| NFPA-F = 3
| NFPA-R = 2
  }}
| Section8       = {{Chembox Related
| OtherAnions = [[Barium oxide]]<br/>[[Barium selenide]]<br/>[[Barium telluride]]<br/>[[Barium polonide]]
| OtherCations = [[Beryllium sulfide]]<br/>[[Magnesium sulfide]]<br/>[[Calcium sulfide]]<br/>[[Strontium sulfide]]<br>[[Radium sulfide]]
| OtherFunction = 
| OtherFunction_label = 
| OtherCompounds = 
 }}
}}

'''Barium sulfide''' is the [[inorganic compound]] with the formula [[Barium|Ba]][[Sulfide|S]].  BaS is the barium compound produced on the largest scale.<ref>{{Greenwood&Earnshaw2nd|paage=678}}</ref> It is an important precursor to other barium compounds including BaCO<sub>3</sub> and the pigment [[lithopone]], ZnS/BaSO<sub>4</sub>.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref> Like other [[chalcogenide]]s of the alkaline earth metals, BaS is a short [[wavelength]] emitter for [[electronic display]]s.<ref>{{cite conference|last1=Vij|first1=D. R.|last2=Singh|first2= N. |title=Optical and electrical properties of II-VI wide gap semiconducting barium sulfide|journal=[[Proceedings of SPIE]] |year=1992|volume=1523 |conference=Conf. Phys. Technol. Semicond. Devices Integr. Circuits, 1992|pages= 608–612|doi=10.1117/12.634082|bibcode=1992SPIE.1523..608V}}</ref>  It is colorless, although like many sulfides, it is commonly obtained in impure colored forms.

==Discovery==
BaS was prepared by the Italian alchemist Vincenzo Cascariolo (also known as Vincentius or Vincentinus Casciarolus or Casciorolus, 1571–1624) via the thermo-chemical reduction of [[barium sulfate|BaSO<sub>4</sub>]] (available as the mineral [[barite]]).<ref>F. Licetus, Litheosphorus, sive de lapide Bononiensi lucem in se conceptam ab ambiente claro mox in tenebris mire conservante, Utini, ex typ. N. Schiratti, 1640. See http://www.chem.leeds.ac.uk/delights/texts/Demonstration_21.htm {{Webarchive|url=https://web.archive.org/web/20110813075857/http://www1.chem.leeds.ac.uk/delights/texts/Demonstration_21.htm |date=2011-08-13 }}</ref> It is currently manufactured by an improved version of Cascariolo's process using [[coke (fuel)|coke]] in place of flour and [[charcoal]]. This kind of conversion is called a [[carbothermic reaction]]:

:{{chem2|BaSO4  +  2C  →  BaS  +  2CO2}}
and also:
:{{chem2|BaSO4  +  4C  →  BaS  +  4CO}}

The basic method remains in use today. BaS dissolves in water. These aqueous solutions, when treated with [[sodium carbonate]] or [[carbon dioxide]], give a white solid of [[barium carbonate]], a source material for many commercial barium compounds.<ref name=Ull>{{Ullmann |doi=10.1002/14356007.a03_325.pub2|title=Barium and Barium Compounds|year=2007|last1=Kresse|first1=Robert|last2=Baudis|first2=Ulrich|last3=Jäger|first3=Paul|last4=Riechers|first4=H. Hermann|last5=Wagner|first5=Heinz|last6=Winkler|first6=Jochen|last7=Wolf|first7=Hans Uwe|isbn=978-3527306732}}</ref>

According to Harvey (1957),<ref name="Harvey_1957">Harvey E. Newton (1957). A History of Luminescence: From the Earliest Times until 1900. Memoirs of the American Physical Society, Philadelphia, J. H. FURST Company, Baltimore, Maryland (USA), Vol. 44, Chapter 1, pp. 11-43.</ref> in 1603, Vincenzo Cascariolo used [[barite]], found at the bottom of Mount Paterno near [[Bologna]], in one of his non-fruitful attempts to produce [[gold]]. After grinding and heating the mineral with charcoal under reducing conditions, he obtained a persistent [[luminescence|luminescent]] material that soon came to be known as ''Lapis Boloniensis'', or Bolognian stone.<ref name="Smet_2010">{{cite journal|last1=Smet|first1=Philippe F.|last2=Moreels|first2=Iwan|last3=Hens|first3=Zeger|last4=Poelman|first4=Dirk|title=Luminescence in Sulfides: A Rich History and a Bright Future|journal=Materials|volume=3|issue=4|year=2010|pages=2834–2883|issn=1996-1944|doi=10.3390/ma3042834|bibcode=2010Mate....3.2834S|doi-access=free|hdl=1854/LU-1243707|hdl-access=free}}</ref><ref name="Hardev_2014">{{Cite web |title=History of Luminescence from Ancient to Modern Times |author=Hardev Singh Virk |work=ResearchGate |date=2014 |access-date=6 March 2021 |url= https://www.researchgate.net/publication/259713568}}</ref> The [[phosphorescence]] of the material obtained by Casciarolo made it a curiosity.<ref>{{cite web| url = http://www.zeno.org/Lemery-1721/A/Lapis+Boloniensis| title = Lapis Boloniensis| publisher = www.zeno.org| access-date = 2011-01-03| archive-date = 2012-10-23| archive-url = https://web.archive.org/web/20121023034505/http://www.zeno.org/Lemery-1721/A/Lapis+Boloniensis| url-status = live}}</ref><ref>{{cite book | url = https://books.google.com/books?id=K25AAAAAcAAJ&pg=PA458 | title  =Trait℗e universel des drogues simples | author1 = Lemery, Nicolas | year = 1714 }}</ref><ref>{{cite book | url = https://books.google.com/books?id=jAYAAAAAQAAJ&pg=PA411| title  =Recreations in mathematics and natural philosophy .. | author1 = Ozanam, Jacques | author2 = Montucla, Jean Etienne | author3 = Hutton, Charles | year = 1814 }}</ref>

==Preparation==
A modern procedure proceeds from barium carbonate:<ref name=Brauer>{{cite book|author1=P. Ehrlich|chapter=Alkaline Earth Metals|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY, NY|volume=2pages=937}}</ref>
:{{chem2|BaCO3  +  H2S  ->  BaS  +  H2O  +  CO2}}
BaS crystallizes with the [[NaCl structure]], featuring octahedral Ba<sup>2+</sup> and S<sup>2−</sup> centres.

The observed [[melting point]] of barium sulfide is highly sensitive to impurities.<ref name=Stinn2017 />

==Safety==
BaS is quite poisonous, as are related sulfides, such as CaS, which evolve toxic [[hydrogen sulfide]] upon contact with water.

==References==
<references/>

{{Barium compounds}}
{{Sulfides}}

[[Category:Barium compounds]]
[[Category:Monosulfides]]
[[Category:Cubic minerals]]
[[Category:Phosphors and scintillators]]
[[Category:Rock salt crystal structure]]