Antimony trisulfide

Names
IUPAC names

Antimony(III) sulfide
Diantimony trisulfide

Other names

* Antimonous sulfide
* Antimony sesquisulfide
* Antimony sulfide
* Antimony vermilion
* Black antimony
* Sulphuret of antimony

Identifiers

CAS Number

* 1345-04-6 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 17621613

PubChem CID

* 16689752

UNII |

* F79059A38U Y

InChI

* InChI=1S/3O.2Sb

Key: IHBMMJGTJFPEQY-UHFFFAOYSA-N

SMILES

* S=[Sb]S[Sb]=S

Properties

Chemical formula

| Sb

Molar mass | 339.70 g·mol−1
Appearance  | Grey or black orthorhombic crystals (stibnite)
Density | 4.562g cm−3 (stibnite)[1]
Melting point |  550 °C (1,022 °F; 823 K) (stibnite)[1]
Boiling point |  1,150 °C (2,100 °F; 1,420 K)

Solubility in water

| 0.00017 g/(100 mL) (18 °C)

Magnetic susceptibility (χ)

| −86.0·10−6 cm3/mol

Refractive index (nD)

| 4.046
Thermochemistry

Heat capacity (C)

| 123.32 J/(mol·K)

Std enthalpy of
formation (ΔfH⦵298)

| −157.8 kJ/mol
Hazards
NFPA 704 (fire diamond)  |

Lethal dose or concentration (LD, LC):

LD50 (median dose)

| > 2000 mg/kg (rat, oral)
NIOSH (US health exposure limits):

PEL (Permissible)

| TWA 0.5 mg/m3 (as Sb)[2]

REL (Recommended)

| TWA 0.5 mg/m3 (as Sb)[2]
Related compounds

Other anions

* Antimony trioxide
* Antimony triselenide
* Antimony telluride

Other cations

| Arsenic trisulfide
Bismuth(III) sulfide

Related compounds

| Antimony pentasulfide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Infobox references

Antimony trisulfide (Sb

3) is found in nature as the crystalline mineral stibnite and the amorphous red mineral (actually a mineraloid)[3] 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] In 1817, the dye and fabric chemist, John Mercer discovered the non-stoichiometric compound Antimony Orange (approximate formula Sb

3 * Sb

3), the first good orange pigment available for cotton fabric printing.[7]

Antimony trisulfide was also used as the image sensitive photoconductor in vidicon camera tubes. It is a semiconductor with a direct band gap of 1.8–2.5 eV.[citation needed] With suitable doping, p and n type materials can be produced.[8]

## Preparation and reactions

3 can be prepared from the elements at temperature 500–900 °C:[5]

2 Sb + 3 S → Sb

3 is precipitated when H
2S is passed through an acidified solution of Sb(III).[9] This reaction has been used as a gravimetric method for determining antimony, bubbling H
2S through a solution of Sb(III) compound in hot HCl deposits an orange form of Sb

3 which turns black under the reaction conditions.[10]

3 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 Sb

3 and chlorates may explode.[11]

In the extraction of antimony from antimony ores the alkaline sulfide process is employed where Sb

3 reacts to form thioantimonate(III) salts (also called thioantimonite):[12]

3 Na
2S + Sb

3 → 2 Na
3SbS

A number of salts containing different thioantimonate(III) ions can be prepared from Sb

3. These include:[13]

[SbS
3]3−, [SbS
2]−
, [Sb

5]4−, [Sb

9]6−, [Sb

7]2− and [Sb

17]10−

Schlippe's salt, Na
3SbS
4 * 9H2O, a thioantimonate(V) salt is formed when Sb

3 is boiled with sulfur and sodium hydroxide. The reaction can be represented as:[9]

3 \+ 3 S2− \+ 2 S → 2 [SbS
4]3−

## Structure

The structure of the black needle-like form of Sb

3, stibnite, consists of linked ribbons in which antimony atoms are in two different coordination environments, trigonal pyramidal and square pyramidal.[9] Similar ribbons occur in Bi

3 and Sb
2Se
3.[14] The red form, metastibnite, is amorphous. Recent work suggests that there are a number of closely related temperature dependent structures of stibnite which have been termed stibnite (I) the high temperature form, identified previously, stibnite (II) and stibnite (III).[15] Other paper shows that the actual coordination polyhedra of antimony are in fact SbS
7, with (3+4) coordination at the M1 site and (5+2) at the M2 site.[clarification needed] These coordinations consider the presence of secondary bonds. Some of the secondary bonds impart cohesion and are connected with packing.[16]

## References

1. ↑ 1.0 1.1 Haynes, W. M., ed (2014). CRC Handbook of Chemistry and Physics (95th ed.). Boca Raton, FL: CRC Press. pp. 4–48. ISBN 978-1-4822-0867-2.
2. ↑ 2.0 2.1 NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0036.html.
3. ↑ "Metastibnite". https://www.mindat.org/min-2686.html.
4. ↑ SUPERGENE METASTIBNITE FROM MINA ALACRAN, PAMPA LARGA, COPIAPO, CHILE, Alan H Clark, THE AMERICAN MINERALOGIST. VOL. 55., 1970
5. ↑ 5.0 5.1 5.2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 581–582. ISBN 978-0-08-037941-8.
6. ↑ Eastaugh, Nicholas (2004). Pigment Compendium: A Dictionary of Historical Pigments. Butterworth-Heinemann. p. 359. ISBN 978-0-7506-5749-5.
7. ↑ Parnell, Edward A (1886). The life and labours of John Mercer. London: Longmans, Green & Co.. pp. 23.
8. ↑ Electrochemistry of Metal Chalcogenides, Mirtat Bouroushian, Springer, 2010
9. ↑ 9.0 9.1 9.2 Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils, ed., Inorganic Chemistry, San Diego/Berlin: Academic Press/De Gruyter, p. 765-766, ISBN 0-12-352651-5
10. ↑ A.I. Vogel, (1951), Quantitative Inorganic analysis, (2d edition), Longmans Green and Co
11. ↑ Hazardous Laboratory Chemicals Disposal Guide, Third Edition, CRC Press, 2003, Margaret-Ann Armour, ISBN 9781566705677
12. ↑ Anderson, Corby G. (2012). "The metallurgy of antimony". Chemie der Erde - Geochemistry 72: 3–8. doi:10.1016/j.chemer.2012.04.001. ISSN 0009-2819. Bibcode: 2012ChEG...72....3A.
13. ↑ 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
14. ↑ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
15. ↑ 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.
16. ↑ Kyono, A.; Kimata, M.; Matsuhisa, M.; Miyashita, Y.; Okamoto, K. (2002). "Low-temperature crystal structures of stibnite implying orbital overlap of Sb 5s 2 inert pair electrons". Physics and Chemistry of Minerals 29 (4): 254–260. doi:10.1007/s00269-001-0227-1. Bibcode: 2002PCM....29..254K.

* v
* t
* e

Antimony compounds

* SbBr3
* Sb(C2H3O2)3
* SbCl3
* SbCl5
* SbF3
* SbF5
* SbH3
* SbI3
* Sb2O3
* Sb2O4
* Sb2O5
* Sb2S3
* Sb2S5
* Sb2(SO4)3
* Sb2Se3
* Sb2Te3

* v
* t
* e

Sulfides

| H2S
H2S2 |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  | He

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Li2S | BeS |  |  |  |  |  |  |  |  |  |  | B2S3 | CS2
COS | (NH4)SH | O | F | Ne
Na2S
Na2Sx | MgS |  |  |  |  |  |  |  |  |  |  | Al2S3 | SiS
SiS2 | PxSy | S | Cl | Ar
K2S | CaS | Sc2S3 | TiS2 | V | CrS
Cr2S3 | MnS
MnS2 | FeS
Fe3S4 | CoS | NiS | Cu2S
CuS | ZnS | GaS
Ga2S3 | GeS
GeS2 | As2S3
As4S3 | SeS2 | Br | Kr
Rb2S | SrS | Y2S3 | ZrS2 | NbS2 | MoS2 | Tc | Ru | Rh2S3 | PdS | Ag2S | CdS | In2S3 | SnS
SnS2 | Sb2S3
Sb2S5 | TeS2 | I | Xe
Cs2S | BaS | *  | HfS2 | TaS2 | WS2
WS3 | ReS2
Re2S7 | Os | Ir2S3
IrS2 | PtS
PtS2 | Au2S
Au2S3 | HgS | Tl2S | PbS
PbS2 | Bi2S3 | Po | At | Rn
Fr | Ra | **  | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og |  |  |  |  |  |  |  |
|  | ↓ |  |  |  |  |  |  |  |  |  |  |  |  |  |  |
| * | La2S3 | CeS
Ce2S3 | Pr2S3 | Nd2S3 | Pm2S3 | SmS
Sm2S3 | Eu2S3 | Gd2S3 | Tb2S3 | Dy2S3 | Ho2S3 | Er2S3 | Tm2S3 | Yb2S3 | Lu2S3 |
| ** | Ac | ThS2 | Pa | US2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr |

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