Copper(I) sulfide: Difference between revisions

|Watchedfields = changed

|verifiedrevid = 443542677

|ImageFile = Kristallstruktur Chalkosin.png

|IUPACName = Copper(I) sulfide

|OtherNames = Cuprous sulfide<br/>[[Chalcocite]]<br/>Copper glance

|Section1={{Chembox Identifiers

|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

|ChemSpiderID = 8305611

|InChI = 1/2Cu.S/q2*+1;-2

|ChEBI_Ref = {{ebicite|correct|EBI}}

|ChEBI = 51114

|SMILES = [Cu+].[Cu+].[S-2]

|InChIKey = AQMRBJNRFUQADD-UHFFFAOYAN

|StdInChI_Ref = {{stdinchicite|correct|chemspider}}

|StdInChI = 1S/2Cu.S/q2*+1;-2

|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

|StdInChIKey = AQMRBJNRFUQADD-UHFFFAOYSA-N

|CASNo = 22205-45-4

|CASNo_Ref = {{cascite|correct|CAS}}

|UNII_Ref = {{fdacite|correct|FDA}}

|UNII = 349M3C1RS1

|PubChem = 62755

|RTECS = GL8910000

}}

|Section2={{Chembox Properties

|Formula = Cu₂S

|MolarMass = 159.16 g/mol

|Density = 5.6 g/cm³ <ref>Patnaik, Pradyot (2002). ''Handbook of Inorganic Chemicals''. McGraw-Hill, {{ISBN|0-07-049439-8}}</ref>

|MeltingPtC = 1130

|MeltingPt_ref = <ref name ="Greenwood">{{Greenwood&Earnshaw1st|page=1373}}</ref>

|Solubility = insoluble

|SolubleOther = slightly soluble in [[hydrochloric acid|HCl]]; soluble in [[ammonium hydroxide|NH₄OH]]; dissolves in [[potassium cyanide|KCN]]; decomposes in [[nitric acid|HNO₃]], [[sulfuric acid|H₂SO₄]]

}}

|Section3={{Chembox Hazards

|FlashPt = Nonflammable

|PEL = TWA 1 mg/m³ (as Cu)<ref name=PGCH>{{PGCH|0150}}</ref>

|REL = TWA 1 mg/m³ (as Cu)<ref name=PGCH/>

|IDLH = TWA 100 mg/m³ (as Cu)<ref name=PGCH/>

}}

|Section4={{Chembox Related

|OtherAnions = [[Copper(I) oxide]]<br/>[[Copper(I) selenide]]

|OtherCations = [[Nickel(II) sulfide]]<br/>[[Copper(II) sulfide]]<br/>[[Zinc sulfide]]

}}

'''Copper(I) sulfide''' is a [[copper sulfide]], a chemical compound of [[copper]] and [[sulfur]]. It has the chemical compound Cu₂S. It is found in nature as the mineral [[chalcocite]]. It has a narrow range of stoichiometry ranging from Cu_1.997S to Cu_2.000S.<ref>{{cite journal|title=An electrochemical investigation of the system copper-sulfur|author=Potter, R. W. |journal=Economic Geology|year=1977|volume=72 |issue=8|pages= 1524–1542|doi=10.2113/gsecongeo.72.8.1524|bibcode=1977EcGeo..72.1524P }}</ref> Samples are typically black.

==Preparation and reactions==

Cu₂S can be prepared by treating copper with sulfur or H₂S.<ref name ="Greenwood"/> The rate depends on the particle size and temperature.<ref>{{cite journal|title=The formation of Cu₂S from the elements I. Copper used in form of powders|author= Blachnik R., Müller A.|doi=10.1016/S0040-6031(00)00545-1|year=2000|journal=Thermochimica Acta|volume=361|pages=31}}</ref>

Cu₂S reacts with oxygen to form SO₂:<ref name = "Wiberg&Holleman">Wiberg, Egon and Holleman, Arnold Frederick (2001) ''Inorganic Chemistry'', Elsevier {{ISBN|0-12-352651-5}}</ref>

:{{chem2|2 Cu2S + 3 O2 -> 2 Cu2O + 2 SO2}}

The production of copper from chalcocite is a typical process in extracting the metal from ores. Usually, the conversion involves roasting, to give Cu₂O and sulfur dioxide:<ref name = "Wiberg&Holleman"/>

:{{chem2|Cu2S + O2 -> 2 Cu + SO2}}

Cuprous oxide readily converts to copper metal upon heating.

[[File:Chalcocite-139819.jpg|thumb|left|Crystals of chalcocite (mineral form of Cu₂S).]]

=== Stoichiometric ===

Two forms ([[Polymorphism (materials science)|a dimorphism]]) of Cu₂S are known. The so-called low temperature [[Monoclinic crystal system|monoclinic form]] ("low-chalcocite") has a complex structure with 96 copper atoms in the unit cell.<ref name=evans>{{cite journal|doi=10.1126/science.203.4378.356|title=Djurleite (Cu_1.94S) and Low Chalcocite (Cu₂S): New Crystal Structure Studies|year=1979|last1=Evans|first1=H. T.|journal=Science|volume=203|issue=4378|pages=356–8|pmid=17772445|bibcode=1979Sci...203..356E |s2cid=6132717 }}</ref> The hexagonal form, stable above 104&nbsp;°C,<ref name = "Wells">Wells A.F. (1984) ''Structural Inorganic Chemistry'', 5th ed., Oxford Science Publications, {{ISBN|0-19-855370-6}}</ref> has 24 crystallographically distinct Cu atoms. Its structure has been described as approximating to a [[hexagonal close packed]] array of sulfur atoms with Cu atoms in planar 3 coordination. This structure was initially assigned an orthorhombic cell due to the twinning of the sample crystal.

=== Non-stoichiometric ===

As illustrated by the mineral [[djurleite]], a cuprous sulfide is also known. With the approximate formula Cu_1.96S, this material is [[non-stoichiometric]] (range Cu_1.934S-Cu_1.965S) and has a monoclinic structure with 248 copper and 128 sulfur atoms in the unit cell.<ref name=evans/> Cu₂S and Cu_1.96S are similar in appearance and hard to distinguish one from another.<ref>{{cite journal|url=http://www.minsocam.org/ammin/AM66/AM66_807.pdf|title=Copper coordination in low chalcocite and djurleite and other copper-rich sulfides|author= Evans H.T.|journal=American Mineralogist|year=1981|volume= 66|issue= 7–8|pages=807–818}}</ref>

== Phase transition ==

The [[electrical resistivity]] increases abruptly at the phase transition point around 104 °C, with the precise temperature depending on the stoichiometry.<ref>{{Cite journal |last=Garisto |first=Dan |date=2023-08-16 |title=LK-99 isn't a superconductor — how science sleuths solved the mystery |url=https://www.nature.com/articles/d41586-023-02585-7 |journal=Nature |volume=620 |issue=7975 |pages=705–706 |language=en |doi=10.1038/d41586-023-02585-7|pmid=37587284 |bibcode=2023Natur.620..705G |s2cid=260955242 }}</ref><ref>Jain, Prashant K. "[[arxiv:2308.05222|Phase transition of copper (I) sulfide and its implication for purported superconductivity of LK-99]]." ''arXiv preprint arXiv:2308.05222'' (2023).</ref>

*[[Copper sulfide]] for an overview of all copper sulfide phases

*[[Copper monosulfide]], CuS

*[[LK-99]] - compound evaluated in 2023 for possible superconductivity

{{Sulfides}}

[[Category:Copper(I) compounds]]

[[tr:Bakır(I) sülfür]]