Chromium(II) sulfide: Difference between revisions

Chromium(II) sulfide
Identifiers
CAS Number	12018-06-3;
3D model (JSmol)	Interactive image;
ChemSpider	10129648;
PubChem CID	11955372;
CompTox Dashboard (EPA)	DTXSID10923256 ;
	InChI InChI=1S/Cr.S/q+2;-2 Key: LXEAUGDQDABWTN-UHFFFAOYSA-N;
	SMILES [S-2].[Cr+2];
Properties
Chemical formula	CrS
Molar mass	84.061 g/mol
Appearance	black crystals
Melting point	1,550 °C (2,820 °F; 1,820 K)
Solubility in water	insoluble
Related compounds
Related compounds	Chromium(III) sulfide
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

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Chromium(II) sulfide is an inorganic compound of chromium and sulfur with the chemical formula CrS.^[1]^[2]^[3] The compound forms black hexagonal crystals, insoluble in water.^[4]

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 H₂S, reducing chromium(III) sulfide with hydrogen, or by double replacement reaction of lithium sulfide with chromium(II) chloride.^[5]

{\ce {Cr + S -> CrS}}

{\ce {Cr + H2S -> CrS + H2}}

{\ce {2CrCl3 + 3H2S -> 2CrS + S + 6HCl}}

{\ce {Cr2S3 + H2 -> 2CrS + H2S}}

{\ce {Li2S + CrCl2 -> 2LiCl + CrS}}

Physical properties

Chromium(II) sulfide forms black paramagnetic crystals of two crystalline modifications:^[6]

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,^[7]^[8] and is also used as a catalyst.^[9]

Chemical properties

Chromium(II) sulfide slowly oxidizes in air:^{[citation needed]}

{\ce {2CrS + 7O2 -> 2Cr2O3 + 4SO2}}

References

^ Bretherick, L. (27 October 2016). Bretherick's Handbook of Reactive Chemical Hazards. Elsevier. p. 1074. ISBN 978-1-4831-6250-8. Retrieved 1 November 2021.
^ Wiberg, Egon; Holleman, A. F.; Wiberg, Nils (2001). Inorganic Chemistry. Academic Press. p. 1372. ISBN 978-0-12-352651-9. Retrieved 1 November 2021.
^ Sr, Richard J. Lewis (13 June 2008). Hazardous Chemicals Desk Reference. John Wiley & Sons. p. 670. ISBN 978-0-470-18024-2. Retrieved 1 November 2021.
^ Lide, David R. (26 June 2006). 1998 Freshman Achievement Award. CRC Press. p. 6-111. ISBN 978-0-8493-0594-8. Retrieved 1 November 2021.
^ Wadhawan, Amar R.; Livi, Kenneth J.; Stone, Alan T.; Bouwer, Edward J. (2015-03-17). "Influence of oxygenation on chromium redox reactions with manganese sulfide (MnS(s))". Environmental Science & Technology. 49 (6): 3523–3531. doi:10.1021/es5057165. ISSN 1520-5851. PMID 25688449.
^ PubChem (2002). "Chromium sulfide (CrS)". PubChem. 40 (1). National Library of Medicine: 24–26. PMID 11955372. Archived from the original on 2022-09-04. Retrieved 2022-09-04.
^ Riedel, Erwin; Janiak, Christoph (2011). Anorganische Chemie (in German). Walter de Gruyter. p. 732. ISBN 978-3-11-022566-2.
^ Holleman, A. F.; Wiberg, E.; Wiberg, N. (1995). Lehrbuch der Anorganischen Chemie. 101. Auflage (in German). Walter de Gruyter. p. 1451. ISBN 3-11-012641-9.
^ Macintyre, Jane E. (23 July 1992). Dictionary of Inorganic Compounds. CRC Press. p. 3082. ISBN 978-0-412-30120-9. Retrieved 1 November 2021.

[1] Bretherick, L. (27 October 2016). Bretherick's Handbook of Reactive Chemical Hazards. Elsevier. p. 1074. ISBN 978-1-4831-6250-8. Retrieved 1 November 2021.

[2] Wiberg, Egon; Holleman, A. F.; Wiberg, Nils (2001). Inorganic Chemistry. Academic Press. p. 1372. ISBN 978-0-12-352651-9. Retrieved 1 November 2021.

[3] Sr, Richard J. Lewis (13 June 2008). Hazardous Chemicals Desk Reference. John Wiley & Sons. p. 670. ISBN 978-0-470-18024-2. Retrieved 1 November 2021.

[4] Lide, David R. (26 June 2006). 1998 Freshman Achievement Award. CRC Press. p. 6-111. ISBN 978-0-8493-0594-8. Retrieved 1 November 2021.

[5] Wadhawan, Amar R.; Livi, Kenneth J.; Stone, Alan T.; Bouwer, Edward J. (2015-03-17). "Influence of oxygenation on chromium redox reactions with manganese sulfide (MnS(s))". Environmental Science & Technology. 49 (6): 3523–3531. doi:10.1021/es5057165. ISSN 1520-5851. PMID 25688449.

[6] PubChem (2002). "Chromium sulfide (CrS)". PubChem. 40 (1). National Library of Medicine: 24–26. PMID 11955372. Archived from the original on 2022-09-04. Retrieved 2022-09-04.

[7] Riedel, Erwin; Janiak, Christoph (2011). Anorganische Chemie (in German). Walter de Gruyter. p. 732. ISBN 978-3-11-022566-2.

[8] Holleman, A. F.; Wiberg, E.; Wiberg, N. (1995). Lehrbuch der Anorganischen Chemie. 101. Auflage (in German). Walter de Gruyter. p. 1451. ISBN 3-11-012641-9.

[9] Macintyre, Jane E. (23 July 1992). Dictionary of Inorganic Compounds. CRC Press. p. 3082. ISBN 978-0-412-30120-9. Retrieved 1 November 2021.

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@@ Line 19: / Line 19: @@
 | Formula =  CrS
 | MolarMass = 84.061 g/mol
-| Appearance = Black crystals
+| Appearance = black crystals
 | Density =
 | MeltingPtC = 1550
 | BoilingPtC =
-| Solubility = Insoluble in water.
+| Solubility = insoluble
 }}
 |Section3={{Chembox Hazards
@@ Line 34: / Line 34: @@
 | AutoignitionPt = }}
 |Section6={{Chembox Related
-| OtherCompounds = [[Tungsten disulfide]]
+| OtherCompounds = [[Chromium(III) sulfide]]
 }}
 }}
-'''Chromium(II) sulfide''' is an [[inorganic compound]] of [[chromium]] and [[sulfur]] with the chemical formula CrS.<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://www.google.ru/books/edition/Inorganic_Chemistry/Mtth5g59dEIC?hl=en&gbpv=1&dq=Chromium+(II)+sulfide+CrS&pg=PA1377&printsec=frontcover |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://www.google.ru/books/edition/Hazardous_Chemicals_Desk_Reference/WZeBDwAAQBAJ?hl=en&gbpv=1&dq=Chromium+(II)+sulfide&pg=PA670&printsec=frontcover |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://www.google.ru/books/edition/1998_Freshman_Achievement_Award/lFjg0L-uOxoC?hl=en&gbpv=1&dq=Chromium+(II)+sulfide&pg=SA6-PA111&printsec=frontcover |access-date=1 November 2021 |language=en}}</ref>
+'''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>
-. Reaction of pure substances on heating:
-::<chem>Cr + S = CrS</chem>
+::<chem>Cr + S -> CrS</chem>
+::<chem>Cr + H2S -> CrS + H2   </chem>
+::<chem>2CrCl3 + 3H2S -> 2CrS + S + 6HCl </chem>
-. The effect of [[hydrogen sulfide]] when heated on powdered chromium:
-::<chem>Cr + H2S = CrS + H2   </chem>
+::<chem>Cr2S3 + H2 -> 2CrS + H2S</chem>
+::<chem>Li2S + CrCl2 -> 2LiCl + CrS</chem>
-. Effect of [[hydrogen sulfide]] on heating on [[chromium(III) chloride]]:
-::<chem>2CrCl3 + 3H2S = 2CrS + S + 6HCl </chem>
-. Reduction of chromium (III) sulfide with [[hydrogen]]:
-::<chem>Cr2S3 + H2 = 2CrS + H2S</chem>
-. Reaction of [[lithium sulfide]] with [[chromium(II) chloride]]
-::<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>
-Chromium (II) sulfide forms black paramagnetic crystals of two crystalline modifications:
 *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>
-Insoluble in water.
-Chromium (II) sulfide is a semiconductor.<ref>{{cite book| first=Erwin|last= Riedel|first2=Christoph|last2= Janiak | title= Anorganische Chemie | publisher= Walter de Gruyter | ISBN = 3-11-022566-2 |language=German| year= 2011 | page= 732 }}</ref><ref>{{cite book|first= A. F.|last=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> 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://www.google.ru/books/edition/Dictionary_of_Inorganic_Compounds/9eJvoNCSCRMC?hl=en&gbpv=1&dq=Chromium+(II)+sulfide+CrS&pg=PA3082&printsec=frontcover |access-date=1 November 2021 |language=en}}</ref>
 ==Chemical properties==
-Slowly oxidizes in air:
+Chromium(II) sulfide slowly oxidizes in air:{{cn|date=December 2021}}
+::<chem>2CrS + 7O2 -> 2Cr2O3 + 4SO2</chem>
-::<chem>2CrS + 7O2 = 2Cr2O3 + 4SO2</chem>
 ==References==
@@ Line 77: / Line 65: @@
 {{Chromium compounds}}
-[[Category:Chromium compounds]]
+[[Category:Chromium(II) compounds]]
-[[Category:Sulfides]]
+[[Category:Monosulfides]]