Thionyl chloride

Thionyl chloride

Names
IUPAC name Sulfurous dichloride
Other names Thionyl dichloride Sulfurous oxychloride Sulfinyl chloride sulfinyl dichloride Dichlorosulfoxide Sulfur oxide dichloride Sulfur monoxide dichloride Sulfuryl(IV) chloride
Identifiers
CAS Number	7719-09-7
3D model (Jmol)	Interactive image
ChEBI	CHEBI:29290
ChemSpider	22797
ECHA InfoCard	100.028.863
EC Number	231-748-8
PubChem	24386
RTECS number	XM5150000
UNII	4A8YJA13N4
UN number	1836
InChI InChI=1S/Cl2OS/c1-4(2)3 Key: FYSNRJHAOHDILO-UHFFFAOYSA-N InChI=1/Cl2OS/c1-4(2)3 Key: FYSNRJHAOHDILO-UHFFFAOYAN
SMILES ClS(Cl)=O
Properties
Chemical formula	SOCl2
Molar mass	118.97 g/mol
Appearance	clear, colourless liquid (yellows on ageing)
Odor	pungent and unpleasant
Density	1.638 g/cm^3, liquid
Melting point	−104.5 °C (−156.1 °F; 168.7 K)
Boiling point	74.6 °C (166.3 °F; 347.8 K)
Solubility in water	reacts
Solubility	soluble in most aprotic solvents: toluene, chloroform, diethyl ether. Reacts with protic solvents: MeOH etc
Vapor pressure	384 Pa (-40 °C) 4.7 kPa (0 °C) 15.7 kPa (25 °C)[1]
Refractive index (nD)	1.517 (20 °C)[2]
Viscosity	0.6 cP
Structure
Molecular shape	pyramidal
Dipole moment	1.44 D
Thermochemistry
Specific heat capacity (C)	121.0 kJ/mol (liquid)[3]
Std molar entropy (S^o298)	309.8 kJ/mol (gas)[3]
Std enthalpy of formation (ΔfH^o298)	-245.6 kJ/mol (liquid)[3]
Hazards
Main hazards	Toxic Reacts violently with water to release toxic gas
GHS pictograms
GHS signal word	Danger
GHS hazard statements	H302, H314, H331
GHS precautionary statements	P261, P280, P305+351+338, P310
R-phrases	R14, R20/22, R29, R35
S-phrases	(S1/2), S26, S30, S36/37/39, S45
NFPA 704	0 4 2 W
Flash point	Non-flammable
US health exposure limits (NIOSH):
PEL (Permissible)	none[4]
REL (Recommended)	C 1 ppm (5 mg/m^3)[4]
IDLH (Immediate danger)	N.D.[4]
Related compounds
Related thionyl halides	Thionyl fluoride Thionyl bromide Thionyl iodide
Related compounds	Sulfuryl chloride Selenium oxydichloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Thionyl chloride is an inorganic compound with the chemical formula SOCl₂. It is a moderately volatile colourless liquid with an unpleasant acrid odour. Thionyl chloride is primarily used as a chlorinating reagent, with approximately 45,000 tons per year being produced during the early 1990s.^[5] It is toxic and will react violently with water to produce toxic gases, it is also listed as a Schedule 3 compound as it may be used for the production of chemical weapons.

Thionyl chloride is sometimes confused with sulfuryl chloride, SO₂Cl₂, but the properties of these compounds differ significantly. Sulfuryl chloride is a source of chlorine whereas thionyl chloride is a source of chloride ions.

Production

The major industrial synthesis involves the reaction of sulfur trioxide and sulfur dichloride:^[6]

SO₃ + SCl₂ → SOCl₂ + SO₂

Other methods include syntheses from phosphorus pentachloride, chlorine and sulfur dichloride, or phosgene:

SO₂ + PCl₅ → SOCl₂ + POCl₃

SO₂ + Cl₂ + SCl₂ → 2 SOCl₂

SO₃ + Cl₂ + 2 SCl₂ → 3 SOCl₂

SO₂ + COCl₂ → SOCl₂ + CO₂

The first of the above four reactions also affords phosphorus oxychloride (phosphoryl chloride), which resembles thionyl chloride in many of its reactions.

Properties and structure

Crystal structure of SOCl₂

SOCl₂ adopts a pyramidal molecular geometry with C_s molecular symmetry. This geometry is attributed to the effects of the lone pairs on the sulfur(IV) centre.

In the solid state SOCl₂ forms monoclinic crystals with the space group P2₁/c.^[7]

Stability

Thionyl chloride has a long shelf life, however "aged" samples develop a yellow hue, possibly due to the formation of disulfur dichloride. It slowly decomposes to S₂Cl₂, SO₂ and Cl₂ at just above the boiling point.^[6][8] Thionyl chloride is susceptible to photolysis, which primarily proceeds via a radical mechanism.^[9] Samples showing signs of ageing can be purified by distillation under reduced pressure, to give a clear colourless liquid.^[10]

Reactions

Thionyl chloride is mainly used in the industrial production of organochlorine compounds, which are often intermediates in pharmaceuticals and agrichemicals. It usually is preferred over other reagents, such as phosphorus pentachloride, as its by-products (HCl and SO₂) are gaseous, which simplifies purification of the product.

Many of the products of thionyl chloride are themselves highly reactive and as such it is involved in a wide range of reactions.

With oxygen species

Thionyl chloride reacts with water to form sulfur dioxide and hydrochloric acid. This process is highly exothermic.

SOCl₂ + H₂O → 2 HCl + SO₂

Classically, it converts carboxylic acids to acyl chlorides.^[11][12][13]

SOCl₂ + RCO₂H → RC(O)Cl + SO₂ + HCl

By a similar process it also converts alcohols to alkyl chlorides. If the alcohol is chiral the reaction generally proceeds via an SNi mechanism with retention of stereochemistry;^[14] however, depending on the exact conditions employed, stereo-inversion can also be achieved. Historically the use of SOCl₂ in combination with a tertiary amine such as pyridine was called the Darzens halogenation however this name is rarely used by modern chemists.

Reactions with an excess of alcohol produce sulfite esters, which can be powerful methylation, alkylation and hydroxyalkylation reagents.^[15]

SOCl₂ + 2 ROH → (RO)₂SO + 2 HCl

For example, the addition of SOCl₂ to amino acids in methanol selectively yields the corresponding methyl esters.^[16]

With nitrogen species

With primary amines, thionyl chloride gives the sulfinylamine derivatives (RNSO), one example being N-sulfinylaniline. Thionyl chloride reacts with primary formamides to form isocyanides^[17] and with secondary formamides to give chloroiminium ions; as such a reaction with dimethylformamide will form the Vilsmeier reagent.^[18] By an analogous process primary amides will react with thionyl chloride to form imidoyl chlorides, with secondary amides also giving chloroiminium ions. These species are highly reactive and can be used to catalyse the conversion of carboxylic acids to acyl chlorides, they are also exploited in the Bischler–Napieralski reaction as a means of forming isoquinolines.

Primary amides will continue on to form nitriles if heated (Von Braun amide degradation).^[19] Thionyl chloride has also been used to promote the Beckmann rearrangement of oximes.

With sulphur species

• Thionyl chloride will transform sulfinic acids into sulfinyl chlorides^[20][21]
• Sulfonic acids react with thionyl chloride to produce sulfonyl chlorides.^[22][23] Sulfonyl chlorides have also been prepared from the direct reaction of the corresponding diazonium salt with thionyl chloride.^[24]
• Thionyl chloride can be used in variations of the Pummerer rearrangement.

With phosphorus species

Thionyl chloride converts phosphonic acids and phosphonates into phosphoryl chlorides. It is for this type of reaction that thionyl chloride is listed as a Schedule 3 compound, as it can be used in the "di-di" method of producing G-series nerve agents. For example, thionyl chloride converts dimethyl methylphosphonate into methylphosphonic acid dichloride, which can be used in the production of sarin and soman.

With metals

As SOCl₂ reacts vigorously with water it can be used to dehydrate various metal chloride hydrates, for example MgCl₂⋅6H₂O, AlCl₃⋅6H₂O, FeCl₃⋅6H₂O etc.^[6] This conversion involves treatment with refluxing thionyl chloride and follows the following general equation:^[25]

MCl_n·xH₂O + x SOCl₂ → MCl_n + x SO₂ + 2x HCl

Other reactions

• Thionyl chloride can engage in a range of electrophilic addition reactions. It adds to alkenes in the presence of AlCl₃ to form an aluminium complex which can be hydrolysed to form a sulfinic acid. Both aryl sulfinyl chlorides and diaryl sulfoxides can be prepared from arenes through reaction with thionyl chloride in triflic acid^[26] or the presence of catalysts such as BiCl₃, Bi(OTf)₃, LiClO₄ or NaClO₄.^[27][28]
• In the laboratory, a reaction between thionyl chloride and an excess of anhydrous alcohol can be used to produce anhydrous alcoholic solutions of HCl.
• Thionyl chloride undergoes halogen exchange reactions to give compounds such as thionyl bromide and thionyl fluoride

3 SOCl₂ + 2 SbF₃ → 3 SOF₂ + 2 SbCl₃

SOCl₂ + 2HBr → SOBr₂ + 2 HCl

Batteries

A selection of Lithium/Thionyl chloride batteries

Thionyl chloride is a component of lithium-thionyl chloride batteries, where it acts as the positive electrode (cathode) with lithium forming the negative electrode (anode); the electrolyte is typically lithium tetrachloroaluminate. The overall discharge reaction is as follows:

4Li + 2 SOCl₂ → 4 LiCl + S + SO₂

These non rechargeable batteries have many advantages over other forms of lithium battery such as a high energy density, a wide operational temperature range and long storage and operational lifespans. However, their high cost and safety concerns have limited their use. The contents of the batteries are highly toxic and require special disposal procedures, additionally they may explode if shorted.

Safety

SOCl₂ is a reactive compound that can violently and/or explosively release dangerous gases upon contact with water and other reagents. Thionyl chloride is controlled under the Chemical Weapons Convention, where it is listed in Schedule 3. Thionyl chloride is used in the "di-di" method of producing G-series nerve agents.

See also

• Oxalyl chloride
• Phosphorus pentachloride
• Phosgene
• Sulfur dichloride
• Thionyl bromide

References

1. Thionyl chloride in Linstrom, P.J.; Mallard, W.G. (eds.) NIST Chemistry WebBook, NIST Standard Reference Database Number 69. National Institute of Standards and Technology, Gaithersburg MD. http://webbook.nist.gov (retrieved 2014-05-11)
2. Patnaik, Pradyot (2003). Handbook of inorganic chemicals. New York, NY [u.a.]: McGraw-Hill. ISBN 0-07-049439-8.
3. Lide, ed.-in-chief David R. (1996). CRC handbook of chemistry and physics (76. ed.). Boca Raton, Fla.: CRC Press. pp. 5–10. ISBN 0-8493-0476-8.
4. "NIOSH Pocket Guide to Chemical Hazards #0611". National Institute for Occupational Safety and Health (NIOSH).
5. Hans-Dietrich Lauss, Wilfried Steffens “Sulfur Halides” in Ullmann's Encyclopedia of Industrial Chemistry Wiley-VCH, Weinheim, 2005.doi:10.1002/14356007.a25_623
6. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 694. ISBN 0-08-037941-9.
7. Mootz, D.; Merschenz-Quack, A. (15 May 1988). "Structures of thionyl halides: SOCl₂ and SOBr₂". Acta Crystallographica Section C. 44 (5): 926–927. doi:10.1107/S010827018800085X.
8. Riley, edited by Georg Brauer ; translated by Scripta Technica, Inc. Translation editor Reed F. (1963). Handbook of preparative inorganic chemistry. Volume 1 (2nd ed.). New York, N.Y.: Academic Press. p. 383. ISBN 978-0121266011.
9. Donovan, R. J.; Husain, D.; Jackson, P. T. (1969). "Spectroscopic and kinetic studies of the SO radical and the photolysis of thionyl chloride". Transactions of the Faraday Society. 65: 2930. doi:10.1039/TF9696502930.
10. Friedman, Lester; Wetter, William P. (1967). "Purification of thionyl chloride". Journal of the Chemical Society A: Inorganic, Physical, Theoretical: 36. doi:10.1039/J19670000036.
11. Clayden, Jonathan; Greeves, Nick; Warren, Stuart; Wothers, Peter (2001). Organic Chemistry (1st ed.). Oxford University Press. p. 295. ISBN 978-0-19-850346-0.
12. Allen, C. F. H.; Byers, Jr., J. R.; Humphlett, W. J. (1963). "Oleoyl chloride". Org. Synth.; Coll. Vol., 4, p. 739
13. Rutenberg, M. W.; Horning, E. C. (1963). "1-Methyl-3-ethyloxindole". Org. Synth.; Coll. Vol., 4, p. 620
14. Smith, Michael B.; March, Jerry (2007), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (6th ed.), New York: Wiley-Interscience, p. 469, ISBN 0-471-72091-7
15. van Woerden, H. F. (1963). "Organic Sulfites". Chemical Reviews. 63 (6): 557–571. doi:10.1021/cr60226a001.
16. Brenner, M.; Huber, W. (1953). "Herstellung von α-Aminosäureestern durch Alkoholyse der Methylester". Helvetica Chimica Acta (in German). 36 (5): 1109–1115. doi:10.1002/hlca.19530360522.
17. Niznik, G. E.; Morrison, III, W. H.; Walborsky, H. M. (1988). "1-d-Aldehydes from organometallic reagents: 2-methylbutanal-1-d". Org. Synth.; Coll. Vol., 6, p. 751
18. Arrieta, A; Aizpurua, J.M; Palomo, C (1984). "N,N-Dimethylchlorosulfitemethaniminium chloride (SOCl₂-DMF) a versatile dehydrating reagent". Tetrahedron Letters. 25 (31): 3365–3368. doi:10.1016/S0040-4039(01)81386-1.
19. Krynitsky, J. A.; Carhart, H. W. (1963). "2-Ethylhexanonitrile". Org. Synth.; Coll. Vol., 4, p. 436
20. Hulce, M.; Mallomo, J. P.; Frye, L. L.; Kogan, T. P.; Posner, G. H. (1990). "(S)-(+)-2-(p-toluenesulfinyl)-2-cyclopentenone: Precursor for enantioselective synthesis of 3-substituted cyclopentanones". Org. Synth.; Coll. Vol., 7, p. 495
21. Kurzer, F. (1963). "p-Toluenesulfinyl chloride". Org. Synth.; Coll. Vol., 4, p. 937
22. Weinreb, S. M.; Chase, C. E.; Wipf, P.; Venkatraman, S. (2004). "2-Trimethylsilylethanesulfonyl chloride (SES-Cl)". Org. Synth.; Coll. Vol., 10, p. 707
23. Hazen, G. G.; Bollinger, F. W.; Roberts, F. E.; Russ, W. K.; Seman, J. J.; Staskiewicz, S. (1998). "4-Dodecylbenzenesulfonyl azides". Org. Synth.; Coll. Vol., 9, p. 400
24. Philip J. Hogan & Brian G. Cox (2009). "Aqueous Process Chemistry: The Preparation of Aryl Sulfonyl Chlorides". Org. Process Res. Dev. 13 (5): 875–879. doi:10.1021/op9000862.
25. Alfred R. Pray, Richard F. Heitmiller, Stanley Strycker; Heitmiller; Strycker; Aftandilian; Muniyappan; Choudhury; Tamres (1990). "Anhydrous Metal Chlorides". Inorganic Syntheses. Inorganic Syntheses. 28: 321–323. doi:10.1002/9780470132593.ch80. ISBN 978-0-470-13259-3.
26. Smith, Michael B.; March, Jerry (2007), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (6th ed.), New York: Wiley-Interscience, p. 697, ISBN 0-471-72091-7
27. Peyronneau, Magali; Roques, Nicolas; Mazières, Stéphane; Le Roux, Christophe (2003). "Catalytic Lewis Acid Activationof Thionyl Chloride: Application to the Synthesis of ArylSulfinyl Chlorides Catalyzed by Bismuth(III) Salts". Synlett (5): 0631–0634. doi:10.1055/s-2003-38358.
28. Bandgar, B. P. & Makone, S. S. (2004). "Lithium/Sodium Perchlorate Catalyzed Synthesis of Symmetrical Diaryl Sulfoxides". Syn. Commun. 34 (4): 743–750. doi:10.1081/SCC-120027723.