| 词条 | Antimony trisulfide |
| 释义 |
| ImageAlt = | IUPACName = diantimony trisulfide antimony(III) sulfide | OtherNames = antimony sulfide, antimonous sufide, antimony sesquisulfide, antimony vermilion, black antimony, sulphuret of antimony | ImageFile = Sulfid antimonitý.JPG | ImageSize = |Section1={{Chembox Identifiers | PubChem = 16689752 | CASNo = 1345-04-6 | RTECS = | EINECS = | ChemSpiderID = 17621613 | SMILES = S=[Sb]S[Sb]=S | InChI = 1S/3O.2Sb | InChIKey = IHBMMJGTJFPEQY-UHFFFAOYSA-N }} |Section2={{Chembox Properties | Formula = Sb2S3 | MolarMass = 339.715 | Appearance = grey / black orthorhombic crystal (stibnite) | Density = 4.562g cm−3 (stibnite)[1] | MeltingPtC = 550 | MeltingPt_notes = (stibnite)[2] | BoilingPtC = 1150 | Solubility = 0.00017 g/100 mL (18 °C) | RefractIndex = 4.046 | MagSus = -86.0·10−6 cm3/mol}} |Section3={{Chembox Thermochemistry | HeatCapacity = 123.32 J/K mol | DeltaHf = -157.8 kJ/mol }} |Section7={{Chembox Hazards | MainHazards = | NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 0 | FlashPt = | AutoignitionPt = | REL = TWA 0.5 mg/m3 (as Sb)[3] | PEL = TWA 0.5 mg/m3 (as Sb)[3] | LD50 = > 2000 mg/kg (rat, oral) }}Antimony trisulfide (Sb2S3) is found in nature as the crystalline mineral stibnite and the amorphous red mineral metastibnite.[4] It is manufactured for use in safety matches, military ammunition, explosives and fireworks. It also is used in the production of ruby-colored glass and in plastics as a flame retardant.[5] Historically the stibnite form was used as a grey pigment in paintings produced in the 16th century.[6] It is a semiconductor with a direct band gap of 1.8-2.5 eV.{{Citation needed|date=March 2017}} With suitable doping, p and n type materials can be produced.[7] Preparation and reactionsSb2S3 can be prepared from the elements at temperature 500-900 °C:[5] 2Sb + 3S → Sb2S3 Sb2S3 is precipitated when H2S is passed through an acidified solution of Sb(III).[8] This reaction has been used as a gravimetric method for determining antimony, bubbling H2S through a solution of Sb(III) compound in hot HCl deposits an orange form of Sb2S3 which turns black under the reaction conditions.[9] Sb2S3 is readily oxidised, reacting vigorously with oxidising agents.[5] It burns in air with a blue flame. It reacts with incandescence with cadmium, magnesium and zinc chlorates. Mixtures of Sb2S3 and chlorates may explode.[10] In the extraction of antimony from antimony ores the alkaline sulfide process is employed where Sb2S3 reacts to form thioantimonate(III) salts (also called thioantimonite):[11] 3Na2S + Sb2S3 → 2Na3SbS3 A number of salts containing different thioantimonate(III) ions can be prepared from Sb2S3 these include:[12] [SbS3]3−, [SbS2]−, [Sb2S5]4−, [Sb4S9]6−, [Sb4S7]2− and [Sb8S17]10− "Schlippe's salt", Na3SbS4·9H2O, a thioantimonate(V) salt is formed when Sb2S3 is boiled with sulfur and sodium hydroxide. The reaction can be represented as:[8] Sb2S3 + 3S2− + 2S → 2[SbS4]3− StructureThe structure of the black needle-like form of Sb2S3, stibnite, consists of linked ribbons in which antimony atoms are in two different coordination environments, trigonal pyramidal and square pyramidal.[8] Similar ribbons occur in Bi2S3 and Sb2Se3.[13] The red form, metastibnite, is amorphous. Recent work suggests that there are a number of closely related temperature dependant structures of stibnite which have been termed stibnite(I) the high temperature form, identified previously, stibnite(II) and stibnite(III).[14] Other paper shows that the actual coordination polyhedra of antimony are in fact SbS7, with (3+4) coordination at the M1 site and (5+2) at the M2 site. These coordinations consider the presence of secondary bonds. Some of the secondary bonds impart cohesion and are connected with packing.[15] References1. ^{{cite book |editor1-last=Haynes |editor1-first=W. M. |title=CRC Handbook of Chemistry and Physics |date=2014 |publisher=CRC Press |location=Boca Raton, FL |isbn=978-1-4822-0867-2 |page=4–48 |edition=95th }} {{Antimony compounds}}{{Sulfides}}2. ^{{cite book |editor1-last=Haynes |editor1-first=W. M. |title=CRC Handbook of Chemistry and Physics |date=2014 |publisher=CRC Press |location=Boca Raton, FL |isbn=978-1-4822-0867-2 |page=4–48 |edition=95th }} 3. ^1 {{PGCH|0036}} 4. ^SUPERGENE METASTIBNITE FROM MINA ALACRAN, PAMPA LARGA, COPIAPO,CHILE, Alan H Clark, THE AMERICAN MINERALOGIST. VOL.55.,I97O 5. ^1 2 {{Greenwood&Earnshaw2nd|pages=581–582}} 6. ^{{cite book | last = Eastaugh | first = Nicholas | authorlink = | title = Pigment Compendium: A Dictionary of Historical Pigments | publisher = Butterworth-Heinemann | year = 2004 | location = | page = 359 | url = | isbn = 978-0-7506-5749-5}} 7. ^Electrochemistry of Metal Chalcogenides, Mirtat Bouroushian, Springer, 2010 8. ^1 2 {{Holleman&Wiberg|page=765-766}} 9. ^A.I. Vogel, (1951), Quantitative Inorganic analysis, (2d edition), Longmans Green and Co 10. ^Hazardous Laboratory Chemicals Disposal Guide, Third Edition,CRC Press, 2003, Margaret-Ann Armour, {{ISBN|9781566705677}} 11. ^{{cite journal|last1=Anderson|first1=Corby G.|title=The metallurgy of antimony|journal=Chemie der Erde - Geochemistry|volume=72|year=2012|pages=3–8|issn=0009-2819|doi=10.1016/j.chemer.2012.04.001}} 12. ^Inorganic Reactions and Methods, The Formation of Bonds to Group VIB (O, S, Se, Te, Po) Elements (Part 1) (Volume 5) Ed. A.P, Hagen,1991, Wiley-VCH, {{ISBN|0-471-18658-9}} 13. ^Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications {{ISBN|0-19-855370-6}} 14. ^Kuze S., Du Boulay D., Ishizawa N., Saiki A, Pring A.; (2004), X ray diffraction evidence for a monoclinic form of stibnite, Sb2S3, below 290K; American Mineralogist, 9(89), 1022-1025. 15. ^{{cite journal | doi=10.1007/s00269-001-0227-1 | volume=29 | issue=4 | title=Low-temperature crystal structures of stibnite implying orbital overlap of Sb 5s 2 inert pair electrons | journal=Physics and Chemistry of Minerals | pages=254–260|year = 2002|last1 = Kyono|first1 = A.| last2=Kimata | first2=M. | last3=Matsuhisa | first3=M. | last4=Miyashita | first4=Y. | last5=Okamoto | first5=K. }} 2 : Antimony compounds|Sulfides |
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