View source for Chromium(II) sulfide

{{Chembox
| ImageFile = CrS.png
| ImageSize = 150px
| ImageAlt = 
| PIN = 
| OtherNames = 
|Section1={{Chembox Identifiers
| index1_label = 
| index4_label = 
| CASNo = 12018-06-3
| ChemSpiderID = 10129648
|  EINECS = 
|  PubChem = 11955372
| StdInChI = 1S/Cr.S/q+2;-2
| StdInChIKey = LXEAUGDQDABWTN-UHFFFAOYSA-N
| SMILES = [S-2].[Cr+2]
 }}
|Section2={{Chembox Properties
| Formula =  CrS
| MolarMass = 84.061 g/mol
| Appearance = black crystals
| Density = 
| MeltingPtC = 1550
| BoilingPtC = 
| Solubility = insoluble
}}
|Section3={{Chembox Hazards
| MainHazards = 
| GHSPictograms = 
| GHSSignalWord = 
| HPhrases = 
| PPhrases = 
| FlashPtC = 
| AutoignitionPt = }}
|Section6={{Chembox Related
| OtherCompounds = [[Chromium(III) sulfide]]
}}
}}

'''Chromium(II) sulfide''' is an [[inorganic compound]] of [[chromium]] and [[sulfur]] with the chemical formula CrS.<ref>{{cite book |last1=Bretherick |first1=L. |title=Bretherick's Handbook of Reactive Chemical Hazards |date=27 October 2016 |publisher=[[Elsevier]] |isbn=978-1-4831-6250-8 |page=1074 |url=https://books.google.com/books?id=4_PJCgAAQBAJ&dq=Chromium+(II)+sulfide+CrS&pg=PA1074 |access-date=1 November 2021 |language=en}}</ref><ref>{{cite book |last1=Wiberg |first1=Egon |last2=Holleman |first2=A. F. |last3=Wiberg |first3=Nils |title=Inorganic Chemistry |date=2001 |publisher=[[Academic Press]] |isbn=978-0-12-352651-9 |page=1372 |url=https://books.google.com/books?id=Mtth5g59dEIC&dq=Chromium+(II)+sulfide+CrS&pg=PA1377 |access-date=1 November 2021 |language=en}}</ref><ref>{{cite book |last1=Sr |first1=Richard J. Lewis |title=Hazardous Chemicals Desk Reference |date=13 June 2008 |publisher=[[John Wiley & Sons]] |isbn=978-0-470-18024-2 |page=670 |url=https://books.google.com/books?id=WZeBDwAAQBAJ&dq=Chromium+(II)+sulfide&pg=PA670 |access-date=1 November 2021 |language=en}}</ref> The compound forms black hexagonal crystals, insoluble in water.<ref>{{cite book |last1=Lide |first1=David R. |title=1998 Freshman Achievement Award |date=26 June 2006 |publisher=[[CRC Press]] |isbn=978-0-8493-0594-8 |page=6-111 |url=https://books.google.com/books?id=lFjg0L-uOxoC&dq=Chromium+(II)+sulfide&pg=SA6-PA111 |access-date=1 November 2021 |language=en}}</ref>

==Synthesis==
Chromium(II) sulfide may be formed by reaction of chromium metal with sulfur or [[hydrogen sulfide]] at high temperature. It may also be formed by reacting [[chromium(III) chloride]] with H<sub>2</sub>S, reducing [[chromium(III) sulfide]] with [[hydrogen]], or by [[double replacement reaction]] of [[lithium sulfide]] with [[chromium(II) chloride]].<ref>{{Cite journal |last1=Wadhawan |first1=Amar R. |last2=Livi |first2=Kenneth J. |last3=Stone |first3=Alan T. |last4=Bouwer |first4=Edward J. |date=2015-03-17 |title=Influence of oxygenation on chromium redox reactions with manganese sulfide (MnS(s)) |journal=Environmental Science & Technology |volume=49 |issue=6 |pages=3523–3531 |doi=10.1021/es5057165 |issn=1520-5851 |pmid=25688449 }}</ref>
::<chem>Cr + S -> CrS</chem>
::<chem>Cr + H2S -> CrS + H2   </chem>
::<chem>2CrCl3 + 3H2S -> 2CrS + S + 6HCl </chem>
::<chem>Cr2S3 + H2 -> 2CrS + H2S</chem>
::<chem>Li2S + CrCl2 -> 2LiCl + CrS</chem>

==Physical properties==
Chromium(II) sulfide forms black paramagnetic crystals of two crystalline modifications:<ref>{{Cite journal |last=PubChem |title=Chromium sulfide (CrS) |url=https://pubchem.ncbi.nlm.nih.gov/compound/11955372 |url-status=live |archive-url=https://web.archive.org/web/20220904015205/https://pubchem.ncbi.nlm.nih.gov/compound/Chromium_II_-sulfide |archive-date=2022-09-04 |access-date=2022-09-04 |journal=[[PubChem]] |year=2002 |volume=40 |issue=1 |pages=24–26 |publisher=[[National Library of Medicine]] |language=en |pmid=11955372}}</ref>
*α-CrS, superstructured phase, hexagonal system, cell parameters a = 1.200 nm, c = 1.152 nm.
*β-CrS, monoclinic system, cell parameters a = 0.594 nm, b = 0.341 nm, c = 0.563 nm, β = 91.73°.

Chromium(II) sulfide is a semiconductor,<ref>{{cite book| first1=Erwin|last1= Riedel|first2=Christoph|last2= Janiak | title= Anorganische Chemie | publisher= Walter de Gruyter | isbn = 978-3-11-022566-2 |language=German| year= 2011 | page= 732 }}</ref><ref>{{cite book|first1= A. F.|last1=Holleman|first2=E.|last2=Wiberg|first3=N.|last3=Wiberg|title=Lehrbuch der Anorganischen Chemie. 101. Auflage.|language=German|publisher=[[Walter de Gruyter]]|year= 1995| isbn= 3-11-012641-9|page= 1451}}</ref> and is also used as a catalyst.<ref>{{cite book |last1=Macintyre |first1=Jane E. |title=Dictionary of Inorganic Compounds |date=23 July 1992 |publisher=[[CRC Press]] |isbn=978-0-412-30120-9 |page=3082 |url=https://books.google.com/books?id=9eJvoNCSCRMC&dq=Chromium+(II)+sulfide+CrS&pg=PA3082 |access-date=1 November 2021 |language=en}}</ref>

==Chemical properties==
Chromium(II) sulfide slowly oxidizes in air:{{cn|date=December 2021}}
::<chem>2CrS + 7O2 -> 2Cr2O3 + 4SO2</chem>

==References==
{{Reflist}}

{{Sulfides}}
{{Chromium compounds}}

[[Category:Chromium(II) compounds]]
[[Category:Monosulfides]]