Antimon trisulfid

Antimon trisulfid
Antimon trisulfid
Nazivi
IUPAC naziv
diantimon trisulfid, antimon(III) sulfid
Drugi nazivi
antimon sulfid, antimonski sufid, antimon seskvisulfid, antimon vermilion, crni antimon, sulfuret antimona
Identifikacija
ECHA InfoCard 100.014.285
Svojstva
Sb2S3
Molarna masa 339,715
Agregatno stanje sivo / crni ortortombni kristali (stibnit)
Gustina 6,5g cm−3 (stibnit)[1]
Tačka topljenja 620 °C (1.148 °F; 893 K) (stibnit)[1]
Opasnosti
SAD zdravstvene granice izlaganja (NIOSH):
PEL (dozvoljivo)
TWA 0.5 mg/m3 (as Sb)
REL (preporučeno)
TWA 0.5 mg/m3 (as Sb)[2]
Ukoliko nije drugačije napomenuto, podaci se odnose na standardno stanje materijala (na 25 °C [77 °F], 100 kPa).
Reference infokutije

Antimon trisulfid Sb2S3 se nalazi u prirodi u obliku kristalnog minerala antimonita i amorfnog crvenog minerala meta-antimonita.[3] On se proizvodi radi upotrebe u bezbednim šibicama, vojnoj municiji, eksplozivima i materijalu za vatromet. On se isto tako koristi u proizvodnji stakla boje rubina i plastike otporne na plamen.[4] Istorijski antimonit je korišten kao sivi pigment u slikama iz 16-tog veka.[5] Ovaj materijal je poluprovodnik sa direktnim band otvorom od 1.8-2.5 eV. Uz odgovarajuću preradu p i n tipovi materijala se mogu proizvesti.[6]

Priprema i reakcije

Sb2S3 se može pripremiti iz elementa na temperaturi od 500-900 °C:[4]

2Sb + 3S → Sb2S3

Sb2S3 precipitira kad se H2S provodi kroz kiseli rastvor Sb(III).[7] Ova reakcija je korištena kao gravimetrijski metod za determinaciju antimona, provoženjem H2S kroz rastvor Sb(III) jedinjenja u toploj HCl dolazi do izdvajanja narandžaste forme Sb2S3, koja pocrni pod reakcionim uslovima.[8]

Sb2S3 se lako oksiduje. On energično reaguje sa oksidijućim agensima.[4] Ovaj materijal sagoreva na vazduhu u pravom plamenu. On reaguje sa kadmijumom, magnezijumom i cink hloratima. Smeše Sb2S3 i hlorata mogu da eksplodiraju.[9]

Pri ekstrakciji antimona iz ruda se koristi alkalni sulfidni proces, pri čemu Sb2S3 reaguje i formiraju se tioantimonat(III) sali (poznate i kao tioantimoniti):[10]

3Na2S + Sb2S3 → 2Na3SbS3

Brojne soli koje sadrže različite tioantimonat(III) jone se mogu pripremiti iz Sb2S3:[11]

[SbS3]3−, [SbS2], [Sb2S5]4−, [Sb4S9]6−, [Sb4S7]2− and [Sb8S17]10−

"Šlipeova so", Na3SbS4·9H2O, tioantimonat(V) so se formira kad se Sb2S3 zagreva do ključanja sa sumporom i natrijum hidroksidom. Reakcija se može napisati kao:[7]

Sb2S3 + 3S2− + 2S → 2[SbS4]3−

Reference

  1. ^ а б Lide David R., ур. (2006). CRC Handbook of Chemistry and Physics (87th изд.). Boca Raton, FL: CRC Press. ISBN 978-0-8493-0487-3. 
  2. ^ NIOSH Džepni vodič hemijskih hazarda 0036
  3. ^ SUPERGENE METASTIBNITE FROM MINA ALACRAN, PAMPA LARGA, COPIAPO,CHILE, Alan H Clark, THE AMERICAN MINERALOGIST. VOL.55.,I97O
  4. ^ а б в Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (II изд.). Oxford: Butterworth-Heinemann. стр. 581—582. ISBN 0080379419. 
  5. ^ Eastaugh, Nicholas (2004). Pigment Compendium: A Dictionary of Historical Pigments. Butterworth-Heinemann. стр. 359. ISBN 0-7506-5749-9. 
  6. ^ Electrochemistry of Metal Chalcogenides, Mirtat Bouroushian, Springer, 2010
  7. ^ а б Holleman A. F.; Wiberg E. (2001). Inorganic Chemistry (1st изд.). San Diego: Academic Press. стр. 765-766. ISBN 0-12-352651-5. 
  8. ^ A.I. Vogel, (1951), Quantitative Inorganic analysis, (2d edition), Longmans Green and Co
  9. ^ Hazardous Laboratory Chemicals Disposal Guide, Third Edition,CRC Press, 2003, Margaret-Ann Armour, ISBN 9781566705677
  10. ^ Anderson, Corby G. (2012). „The metallurgy of antimony”. Chemie der Erde - Geochemistry. 72: 3—8. ISSN 0009-2819. doi:10.1016/j.chemer.2012.04.001. 
  11. ^ 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 978-0-471-18658-8

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