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Sulfur dichloride
Structure and dimensions of the sulfur dichloride molecule
Ball-and-stick model of sulfur dichloride
Ball-and-stick model of sulfur dichloride
Space-filling model of sulfur dichloride
Space-filling model of sulfur dichloride
IUPAC name
  • Dichlorosulfane
  • Sulfur dichloride
  • Sulfur(II) chloride
Other names
  • Chloro thiohypobromite
  • Dichloro sulfide
  • Sulphur chloride

CAS Number

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  • 10545-99-0 check

3D model (JSmol)

  • Interactive image
  • 23682
ECHA InfoCard 100.031.014 Edit this at Wikidata
EC Number
  • 234-129-0

PubChem CID

  • 25353
RTECS number
  • WS4500000
  • 8Q6684WQ9H check
UN number 1828

CompTox Dashboard (EPA)

  • DTXSID4051538 Edit this at Wikidata


  • InChI=1S/Cl2S/c1-3-2


  • InChI=1/Cl2S/c1-3-2



  • ClSCl


Chemical formula

Molar mass 102.96 g·mol−1
Appearance Cherry-red liquid
Odor Pungent
Density 1.621 g/cm3
Melting point −121.0 °C (−185.8 °F; 152.2 K)
Boiling point 59 °C (138 °F; 332 K) (decomposes)

Solubility in water

Insoluble, reacts slowly

Magnetic susceptibility (χ)

−49.4·10−6 cm3/mol

Refractive index (nD)


Coordination geometry


Molecular shape

GHS labelling:


GHS05: CorrosiveGHS07: Exclamation markGHS09: Environmental hazard

Signal word

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Hazard statements

H314, H335, H400

Precautionary statements

P260, P261, P264, P271, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P312, P321, P363, P391, P403+P233, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code





234 °C (453 °F; 507 K)
Safety data sheet (SDS) ICSC 1661
Related compounds


  • Disulfur dichloride
  • Thionyl chloride
  • Sulfuryl chloride

Related compounds

  • Sulfur difluoride
  • Sulfur tetrafluoride
  • Sulfur hexafluoride
  • Disulfur dibromide

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

Sulfur dichloride is the chemical compound with the formula SCl2. This cherry-red liquid is the simplest sulfur chloride and one of the most common, and it is used as a precursor to tướng organosulfur compounds. It is a highly corrosive and toxic substance, and it reacts on liên hệ with water to tướng size chlorine-containing acids.

Chlorination of sulfur[edit]

SCl2 is produced by the chlorination of either elemental sulfur or disulfur dichloride.[1] The process occurs in a series of steps, some of which are:

S8 + 4 Cl2 → 4 S2Cl2; ΔH = −58.2 kJ/mol
S2Cl2 + Cl2 ↔ 2 SCl2; ΔH = −40.6 kJ/mol

The addition of Cl2 to tướng S2Cl2 has been proposed to tướng proceed via a mixed valence intermediate Cl3S−SCl. SCl2 undergoes even further chlorination to tướng give SCl4, but this species is unstable at near room temperature. It is likely that several SnCl2 exist where n > 2.

Disulfur dichloride, S2Cl2, is the most common impurity in SCl2. Separation of SCl2 from S2Cl2 is possible via distillation with PCl3 to tướng size an azeotrope of 99% purity, however sulfur dichloride loses chlorine slowly at room temperature and reverts to tướng disulfur dichloride. Pure samples may be stored in sealed glass ampules which develop a slight positive pressure of chlorine, halting the decomposition.

Use of SCl2 in chemical synthesis[edit]

SCl2 is used in organic synthesis. It adds to tướng alkenes to tướng give chloride-substituted thioethers. Illustrative is its addition to tướng 1,5-cyclooctadiene to tướng give a bicyclic thioether[2] A well tested method for the production of the mustard gas bis(2-chloroethyl)sulfide, is the addition of ethylene to tướng sulfur dichloride:[3]

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SCl2 + 2 C2H4 → (ClC2H4)2S

SCl2 is also a precursor to tướng several inorganic sulfur compounds. Treatment with fluoride salts gives SF4 via the decomposition of the intermediate sulfur difluoride. With H2S, SCl2 reacts to tướng give "lower" sulfanes such as S3H2.

Reaction with ammonia affords sulfur nitrides related to tướng S4N4. Treatment of SCl2 with primary amines gives sulfur diimides. One example is di-t-butylsulfurdiimide.[4]

Safety considerations[edit]

SCl2 hydrolyzes with release of HCl. Old samples contain Cl2.[citation needed]


  1. ^ F. Fehér "Dichloromonosulfane" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 370.
  2. ^ Bishop, Roger (1992). "9-Thiabicyclo[3.3.1]nonane-2,6-dione". Organic Syntheses. 70: 120.; Collective Volume, vol. 9, p. 692
  3. ^ R. J. Cremlyn “An Introduction to tướng Organosulfur Chemistry” John Wiley and Sons: Chichester (1996). ISBN 0-471-95512-4.
  4. ^ Kresze, G.; Wucherpfennig, W. (1967). "New Methods of Preparative Organic Chemistry V: Organic Syntheses with Imides of Sulfur Dioxide". Angewandte Chemie International Edition in English. 6 (2): 149–167. doi:10.1002/anie.196701491. PMID 4962859.