Chemistry:Copper(I) sulfide
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| IUPAC name
Copper(I) sulfide
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| Other names | |
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3D model (JSmol)
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PubChem CID
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| Properties | |
| Cu2S | |
| Molar mass | 159.16 g/mol |
| Density | 5.6 g/cm3 [1] |
| Melting point | 1,130 °C (2,070 °F; 1,400 K)[2] |
| insoluble | |
| Solubility | slightly soluble in HCl; soluble in NH4OH; dissolves in KCN; decomposes in HNO3, H2SO4 |
| Hazards | |
| Flash point | Nonflammable |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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TWA 1 mg/m3 (as Cu)[3] |
REL (Recommended)
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TWA 1 mg/m3 (as Cu)[3] |
IDLH (Immediate danger)
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TWA 100 mg/m3 (as Cu)[3] |
| Related compounds | |
Other anions
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Copper(I) oxide Copper(I) selenide |
Other cations
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Nickel(II) sulfide Copper(II) sulfide Zinc sulfide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
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 Cu1.997S to Cu2.000S.[4] Samples are typically black.
Preparation and reactions
Cu2S can be prepared by treating copper with sulfur or H2S.[2] The rate depends on the particle size and temperature.[5] Cu2S reacts with oxygen to form SO2:[6]
- 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:[6]
- Cu
2S + O
2 → 2 Cu + SO
2
Cuprous oxide readily converts to copper metal upon heating.
Structure
Stoichiometric
Two forms (a dimorphism) of Cu2S are known. The so-called low temperature monoclinic form ("low-chalcocite") has a complex structure with 96 copper atoms in the unit cell.[7] The hexagonal form, stable above 104 °C,[8] 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 Cu1.96S, this material is non-stoichiometric (range Cu1.934S-Cu1.965S) and has a monoclinic structure with 248 copper and 128 sulfur atoms in the unit cell.[7] Cu2S and Cu1.96S are similar in appearance and hard to distinguish one from another.[9]
Phase transition
The electrical resistivity increases abruptly at the phase transition point around 104 °C, with the precise temperature depending on the stoichiometry.[10][11]
See also
- Copper sulfide for an overview of all copper sulfide phases
- Copper monosulfide, CuS
- Chalcocite
- Djurleite
- LK-99 - compound evaluated in 2023 for possible superconductivity
References
- ↑ Patnaik, Pradyot (2002). Handbook of Inorganic Chemicals. McGraw-Hill, ISBN:0-07-049439-8
- ↑ 2.0 2.1 Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 1373. ISBN 978-0-08-022057-4. https://books.google.com/books?id=OezvAAAAMAAJ&q=0-08-022057-6&dq=0-08-022057-6&source=bl&ots=m4tIRxdwSk&sig=XQTTjw5EN9n5z62JB3d0vaUEn0Y&hl=en&sa=X&ei=UoAWUN7-EM6ziQfyxIDoCQ&ved=0CD8Q6AEwBA.
- ↑ 3.0 3.1 3.2 NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0150.html.
- ↑ Potter, R. W. (1977). "An electrochemical investigation of the system copper-sulfur". Economic Geology 72 (8): 1524–1542. doi:10.2113/gsecongeo.72.8.1524.
- ↑ Blachnik R., Müller A. (2000). "The formation of Cu2S from the elements I. Copper used in form of powders". Thermochimica Acta 361: 31. doi:10.1016/S0040-6031(00)00545-1.
- ↑ 6.0 6.1 Wiberg, Egon and Holleman, Arnold Frederick (2001) Inorganic Chemistry, Elsevier ISBN:0-12-352651-5
- ↑ 7.0 7.1 Evans, H. T. (1979). "Djurleite (Cu1.94S) and Low Chalcocite (Cu2S): New Crystal Structure Studies". Science 203 (4378): 356–8. doi:10.1126/science.203.4378.356. PMID 17772445.
- ↑ Wells A.F. (1984) Structural Inorganic Chemistry, 5th ed., Oxford Science Publications, ISBN:0-19-855370-6
- ↑ Evans H.T. (1981). "Copper coordination in low chalcocite and djurleite and other copper-rich sulfides". American Mineralogist 66 (7–8): 807–818. http://www.minsocam.org/ammin/AM66/AM66_807.pdf.
- ↑ Garisto, Dan (2023-08-16). "LK-99 isn’t a superconductor — how science sleuths solved the mystery" (in en). Nature. doi:10.1038/d41586-023-02585-7. https://www.nature.com/articles/d41586-023-02585-7.
- ↑ Jain, Prashant K. "Phase transition of copper (I) sulfide and its implication for purported superconductivity of LK-99." arXiv preprint arXiv:2308.05222 (2023).
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