Is Cus Soluble In Water
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| Names | |
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| IUPAC name Copper sulfide | |
| Other names Covellite | |
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| ECHA InfoCard | 100.013.884 |
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| Properties | |
| Chemic formula | CuS |
| Tooth mass | 95.611 g/mol |
| Appearance | black powder or lumps |
| Density | 4.76 thousand/cmthree |
| Melting bespeak | above 500 °C (932 °F; 773 K) (decomposes)[2] |
| Solubility in h2o | 0.000033 g/100 mL (18 °C) |
| Solubility product (Grand sp) | 6 x 10−37 [one] |
| Solubility | soluble in HNO3, NH4OH, KCN insoluble in HCl, H2And then4 |
| Magnetic susceptibility (χ) | -2.0·10−half-dozen cm3/mol |
| Refractive index (north D) | one.45 |
| Construction | |
| Crystal construction | hexagonal |
| Hazards | |
| GHS labelling: | |
| Pictograms |  |
| Take a chance statements | H413 |
| Precautionary statements | P273, P501 |
| NIOSH (US health exposure limits): | |
| PEL (Permissible) | TWA 1 mg/m3 (as Cu)[3] |
| REL (Recommended) | TWA ane mg/one thousandthree (as Cu)[iii] |
| IDLH (Immediate danger) | TWA 100 mg/m3 (as Cu)[3] |
| Related compounds | |
| Other anions | Copper(2) oxide |
| Other cations | zinc sulfide |
| Except where otherwise noted, data are given for materials in their standard country (at 25 °C [77 °F], 100 kPa). Infobox references | |
Copper monosulfide is a chemic compound of copper and sulfur. It was initially thought to occur in nature every bit the night indigo blue mineral covellite. Withal, it was later shown to be rather a cuprous compound, formula Cu+ iiiS(S2).[4] CuS is a moderate conductor of electricity.[5] A blackness colloidal precipitate of CuS is formed when hydrogen sulfide, H2S, is bubbled through solutions of Cu(II) salts.[half dozen] It is i of a number of binary compounds of copper and sulfur (come across copper sulfide for an overview of this subject), and has attracted interest because of its potential uses in catalysis[7] and photovoltaics.[8]
Manufacturing [edit]
Copper monosulfide can exist prepared past passing hydrogen sulfide gas into a solution of copper(II) salt.
Alternatively, it can be prepared by melting an excess of sulfur with copper(I) sulfide or by precipitation with hydrogen sulfide from a solution of anhydrous copper(Two) chloride in anhydrous ethanol.
The reaction of copper with molten sulfur followed by boiling sodium hydroxide and the reaction of sodium sulfide with aqueous copper sulfate will too produce copper sulfide.
CuS structure and bonding [edit]
Copper sulfide crystallizes in the hexagonal crystal system, and this is the class of the mineral covellite. In that location is besides an amorphous loftier force per unit area course[9] which on the basis of the Raman spectrum has been described as having a distorted covellite construction. An baggy room temperature semiconducting class produced by the reaction of a Cu(2) ethylenediamine complex with thiourea has been reported, which transforms to the crystalline covellite form at 30 °C.[ten]
The crystal structure of covellite has been reported several times,[11] [12] [xiii] and whilst these studies are in full general agreement on assigning the infinite group P63/mmc there are small discrepancies in bond lengths and angles between them. The construction was described as "extraordinary" past Wells[14] and is quite different from copper(II) oxide, only similar to CuSe (klockmannite). The covellite unit cell contains vi formula units (12 atoms) in which:
- 4 Cu atoms have tetrahedral coordination (see illustration).
- 2 Cu atoms have trigonal planar coordination (see illustration).
- 2 pairs of S atoms are simply 207.1 pm apart[xiii] indicating the beingness of an South-Southward bond (a disulfide unit).
- the 2 remaining S atoms form trigonal planar triangles around the copper atoms, and are surrounded past five Cu atoms in a pentagonal bipyramid (see analogy).
- The S atoms at each end of a disulfide unit of measurement are tetrahedrally coordinated to 3 tetrahedrally coordinated Cu atoms and the other S atom in the disulfide unit (see illustration).
The conception of copper sulfide equally CuIiS (i.e. containing no sulfur-sulfur bond) is clearly incompatible with the crystal construction, and too at variance with the observed diamagnetism[15] equally a Cu(Ii) chemical compound would have a d9 configuration and exist expected to be paramagnetic.[6]
Studies using XPS[xvi] [17] [xviii] [xix] indicate that all of the copper atoms have an oxidation state of +1. This contradicts a formulation based on the crystal construction and obeying the octet dominion that is plant in many textbooks (e.g.[6] [20]) describing CuS as containing both CuI and CuII i.e. (Cu+)2Cuii+(S2)2−South2−. An alternative formulation as (Cu+)3(S2−)(S2)− was proposed and supported past calculations.[21] The conception should not be interpreted equally containing radical anion, just rather that in that location is a delocalized valence "pigsty".[21] [22] Electron paramagnetic resonance studies on the precipitation of Cu(II) salts indicates that the reduction of Cu(2) to Cu(I) occurs in solution.[23]
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| brawl-and-stick model of part of the crystal structure of covellite | trigonal planar coordination of copper | tetrahedral coordination of copper | trigonal bipyramidal coordination of sulfur | tetrahedral coordination of sulfur-note disulfide unit |
See likewise [edit]
- Copper sulfide for an overview of all copper sulfide phases
- Copper(I) sulfide, Cu2S
- Covellite
References [edit]
- ^ Rollie J. Myers (1986). "The new depression value for the second dissociation constant for H2S: Its history, its best value, and its impact on the teaching of sulfide equilibria". J. Chem. Educ. 63 (8): 687. Bibcode:1986JChEd..63..687M. doi:10.1021/ed063p687.
- ^ Blachnik, R.; Müller, A. (2000). "The formation of Cu2S from the elements I. Copper used in form of powders". Thermochimica Acta. 361 (one–2): 31–52. doi:10.1016/S0040-6031(00)00545-ane.
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Plant for Occupational Safety and Health (NIOSH).
- ^ Liang, Due west., Whangbo, Thou.H. (1993) Conductivity anisotropy and structural stage transition in Covellite CuS Solid State Communications, 85(v), 405-408
- ^ Wells A.F. (1962) Structural Inorganic Chemistry 3d edition Oxford Academy Press
- ^ a b c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemical science of the Elements (second ed.). Butterworth-Heinemann. ISBN978-0-08-037941-viii.
- ^ Kuchmii, S.Y.; Korzhak A.V.; Raevskaya A.E.; Kryukov A.I. (2001). "Catalysis of the Sodium Sulfide Reduction of Methylviologene by CuS Nanoparticles". Theoretical and Experimental Chemistry. New York: Springer. 37 (1): 36–41. doi:10.1023/A:1010465823376. S2CID 91893521.
- ^ Mane, R.South.; Lokhande C.D. (June 2000). "Chemic deposition method for metal chalcogenide sparse films". Materials Chemistry and Physics. 65 (1): 1–31. doi:10.1016/S0254-0584(00)00217-0.
- ^ Peiris, Thou; Sweeney, J.S.; Campbell, A.J.; Heinz D. L. (1996). "Pressure-induced amorphization of covellite, CuS". J. Chem. Phys. 104 (ane): 11–16. Bibcode:1996JChPh.104...11P. doi:10.1063/ane.470870.
- ^ Grijalva, H.; Inoue, M.; Boggavarapu, S.; Calvert, P. (1996). "Amorphous and crystalline copper sulfides, CuS". J. Mater. Chem. 6 (7): 1157–1160. doi:ten.1039/JM9960601157.
- ^ Oftedal, I. (1932). "Dice Kristallstruktur des Covellins (CuS)". Z. Kristallogr. 83 (ane–six): 9–25. doi:x.1524/zkri.1932.83.1.ix. S2CID 101164006.
- ^ Drupe, L. G. (1954). "The crystal structure of covellite CuS and klockmannite CuSe". American Mineralogist. 39: 504.
- ^ a b Evans, H.T. Jr.; Konnert J. (1976). "Crystal structure refinement of covellite". American Mineralogist. 61: 996–m.
- ^ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-vi
- ^ Magnetic susceptibility of the elements and inorganic compounds Archived 2012-01-12 at the Wayback Machine
- ^ Nakai, I.; Sugitani, Y.; Nagashima, Yard.; Niwa, Y. (1978). "Ten-ray photoelectron spectroscopic study of copper minerals". Periodical of Inorganic and Nuclear Chemistry. 40 (5): 789–791. doi:10.1016/0022-1902(78)80152-three.
- ^ Folmer, J.C.W.; Jellinek F. (1980). "The valence of copper in sulfides and selenides: An X-ray photoelectron spectroscopy study". Journal of the Less Mutual Metals. 76 (ane–ii): 789–791. doi:10.1016/0022-5088(80)90019-iii.
- ^ Folmer, J.C.W.; Jellinek F.; Calis G.H.M (1988). "The electronic structure of pyrites, particularly CuS2 and Fe1−10 Cu10Se 2 : An XPS and Mössbauer study". Journal of Solid State Chemistry. 72 (1): 137–144. Bibcode:1988JSSCh..72..137F. doi:ten.1016/0022-4596(88)90017-5.
- ^ Goh, S.W.; Buckley A.N.; Lamb R.N. (Feb 2006). "Copper(II) sulfide?". Minerals Technology. nineteen (2): 204–208. doi:10.1016/j.mineng.2005.09.003.
- ^ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN0-471-19957-5
- ^ a b Liang, W.; Whangbo Yard, -H (February 1993). "Electrical conductivity anisotropy and structural phase transition in Covellite CuS". Solid State Communications. 85 (5): 405–408. Bibcode:1993SSCom..85..405L. doi:10.1016/0038-1098(93)90689-Thousand.
- ^ Nozaki, H; Shibata, Chiliad; Ohhashi,N. (April 1991). "Metallic hole conduction in CuS". Periodical of Solid Country Chemistry. 91 (2): 306–311. Bibcode:1991JSSCh..91..306N. doi:x.1016/0022-4596(91)90085-5.
- ^ Luther, GW; Theberge SM; Rozan TF; Rickard D; Rowlands CC; Oldroyd A. (February 2002). "Aqueous copper sulfide clusters as intermediates during copper sulfide germination". Environ. Sci. Technol. 36 (3): 394–402. Bibcode:2002EnST...36..394L. doi:10.1021/es010906k. PMID 11871554.
Is Cus Soluble In Water,
Source: https://en.wikipedia.org/wiki/Copper_monosulfide
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