3D model (JSmol)
CompTox Dashboard (EPA)
|Melting point||-121.0 °C (-185.8 °F; 152.2 K)|
|Boiling point||59 °C (138 °F; 332 K) (decomposes)|
Refractive index (nD)
|Safety data sheet||ICSC 1661|
|R-phrases (outdated)||R14, R34, R37, R50|
|S-phrases (outdated)||(S1/2), S26, S45, S61|
|NFPA 704 (fire diamond)|
|234 °C (453 °F; 507 K)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
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. It is used as a precursor to organosulfur compounds.
The addition of Cl2 to S2Cl2 has been proposed to proceed via a mixed valence intermediate Cl3S-SCl. SCl2 undergoes even further chlorination to give SCl4, but this species is unstable at near room temperature. It is likely that several SxCl2 exist where x > 2.
Disulfur dichloride, S2Cl2, is the most common impurity in SCl2. Separation of SCl2 from S2Cl2 is possible via distillation with PCl3 to form an azeotrope of 99% purity, however sulfur dichloride loses chlorine slowly at room temperature and reverts to disulfur dichloride. Pure samples may be stored in sealed glass ampules which develop a slight positive pressure of chlorine, halting the decomposition.
SCl2 is used In organic synthesis. It adds to alkenes to give chloride-substituted thioethers. Illustrative applications are its addition to 1,5-cyclooctadiene to give a bicyclic thioether and ethylene to give sulfur mustard S(CH2CH2Cl)2.
SCl2 is also a precursor to several inorganic sulfur compounds. Treatment with fluoride salts gives SF4 via the decomposition of the intermediate sulfur difluoride. With H2S, SCl2 reacts to give "lower" sulfanes such as S3H2.