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Phosphorus sesquisulfide
Names
	IUPAC names Tetraphosphorus trisulfide; or 3,5,7-trithia-1,2,4,6-tetraphosphatricyclo[2.2.1.02,6]heptane
	Other names phosphorus trisulfide, phosphorus sesquisulfide, phosphorus sulfide
Identifiers
CAS Number	1314-85-8 ;
3D model (JSmol)	Interactive image;
ChemSpider	14134 ;
ECHA InfoCard	100.013.860
PubChem CID	14818;
RTECS number	TH4330000;
UNII	8V5Q0M194Y ;
CompTox Dashboard (EPA)	DTXSID4074562 ;
	InChI InChI=1S/P4S3/c5-1-2-3(1)7-4(5)6-2 Key: RWQFRHVDPXXRQN-UHFFFAOYSA-N ; InChI=1/P4S3/c5-1-2-3(1)7-4(5)6-2 Key: RWQFRHVDPXXRQN-UHFFFAOYAM;
	SMILES S1P2P3SP1SP23;
Properties
Chemical formula	P4S3
Molar mass	220.093 g/mol
Appearance	Yellow, yellow-green or gray solid
Density	2.08 g.cm3, solid
Melting point	172.5 °C (342.5 °F; 445.6 K)
Boiling point	408 °C (766 °F; 681 K)
Structure
Crystal structure	orthorhombic, Schönflies notation D2h
Space group	Pmnb
Point group	C3v
Related compounds
Related compounds	P4S10; P4O6
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	Irritant
	GHS labelling:
Pictograms
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Phosphorus sesquisulfide is the inorganic compound with the formula P₄S₃. It was developed by Henri Sevene and Emile David Cahen in 1898 as part of their invention of friction matches that did not pose the health hazards of white phosphorus.^[2]^[3] This yellow solid is one of two commercially produced phosphorus sulfides. It is a component of "strike anywhere" matches.

Depending on purity, samples can appear yellow-green to grey. The compound was discovered by G. Lemoine and first produced safely in commercial quantities in 1898 by Albright and Wilson. It dissolves in an equal weight of carbon disulfide (CS₂), and in a 1:50 weight ratio of benzene. Unlike some other phosphorus sulfides, P₄S₃ is slow to hydrolyze and has a well-defined melting point.

Structure and synthesis

The molecule has C_3v symmetry. It is a derivative of the tetrahedral (P₄) unit from insertion of sulfur into three P-P bonds. The P-S and P-P distances are 2.090 and 2.235 Å, respectively. P₄Se₃ and P₄S₃ adopt the same structures.^[1] These compounds can be melted together and form mixed crystals of one dissolved in the other.^[4] Under higher temperatures, mixed chalcogenide molecules P₄S₂Se and P₄SSe₂ will form.^[5]

P₄S₃ is produced by the reaction of red or white phosphorus with sulfur. Excess sulfur gives phosphorus pentasulfide (P₄S₁₀). It is estimated that 150 ton/y were produced in 1989.^[6]

Applications

P₄S₃ and potassium chlorate, together with other materials, composes the heads of "strike-anywhere matches".^[7]

Safety

Its flash point is about 100 °C.^[8]

Health effects

Exposure to "strike anywhere" matches containing phosphorus sesquisulfide can cause contact dermatitis, usually in the pocket area but also on the face.^[9] Exposure over a long period of time to burning match tips (containing phosphorus sesquisulfide) can result in a recurring severe primary dermatitis about the eyes and face. Loosening of the teeth has also been reported which may have been due to phosphorus poisoning.^[10]

References

^ ^a ^b Leung, Y. C.; Waser, J.; van Houten, S.; Vos, A.; Wiegers, G. A.; Wiebenga, E. H. (1957). "The Crystal Structure of P₄S₃". Acta Crystallographica. 10 (9): 574–582. doi:10.1107/S0365110X57002042.
^ US patent 614350, Seyene, H.; Cahen, E. D., "Match Composition", issued 1898-11-15
^ US 614350
^ Burns, Gary R.; Sarfati, Jonathan D. (1988). "Raman spectra of tetraphosphorus triselenide doped in tetraphosphorus trisulphide". Solid State Communications. 66 (4): 347–349. Bibcode:1988SSCom..66..347B. doi:10.1016/0038-1098(88)90854-X.
^ Burns, Gary R.; Rollo, Joanne R.; Sarfati, Jonathan D. (1989). "Raman spectra of the tetraphosphorus trichalcogenide cage molecules P₄S₂Se and P₄SSe₂". Inorganica Chimica Acta. 161: 35–38. doi:10.1016/S0020-1693(00)90111-7.
^ Bettermann, G.; Krause, W.; Riess, G.; Hofmann, T. "Phosphorus Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_527. ISBN 978-3527306732.
^ Corbridge, D. E. C. (1995). Phosphorus: An Outline of its Chemistry, Biochemistry, and Technology (5th ed.). Amsterdam: Elsevier. pp. 115–116. ISBN 0-444-89307-5.
^ Lewis, R.J. Sr (2007). Hawley's Condensed Chemical Dictionary (15th ed.). New York, NY: John Wiley & Sons, Inc. p. 987.
^ Burgess, J. F.; Forsey, R. Roy (1951). "Contact Dermatitis of the Face Due to Matches". AMA Arch Dermatol Syphilol. 64 (5). American Medical Association: 636–637. doi:10.1001/archderm.1951.01570110106016.
^ Burgess, J. Frederick (December 1951). "Phosphorus Sesquisulphide Poisoning". Can Med Assoc J. 65 (6). Canadian Medical Association: 567–568. PMC 1822299. PMID 14886853.