Sulfur dichloride

is produced by the chlorination of either elemental sulfur or disulfur dichloride. The process occurs in a series of steps, some of which are: :(ΔH = −58.2 kJ/mol) :(ΔH = −40.6 kJ/mol) The addition of chlorine| to has been proposed to proceed via a mixed valence intermediate . undergoes even further chlorination to give SCl4|, but this species is unstable at near room temperature. It is likely that several {{chem2|S_{n}Cl2}} exist where n > 2. Disulfur dichloride, , is a common impurity in . Separation of from is possible via distillation with Phosphorus trichloride| to form an azeotrope of 99% purity. Sulfur dichloride loses chlorine slowly at room temperature, converting to disulfur dichloride and eventually higher sulfanes. Pure samples may be stored in sealed glass ampules which develop a slight positive pressure of chlorine, halting the decomposition. ==Use of in chemical synthesis==

is used in organic synthesis. It adds to alkenes to give chloride-substituted thioethers. Illustrative is its addition to 1,5-cyclooctadiene to give a bicyclic thioether A well tested method for the production of the mustard gas bis(2-chloroethyl)sulfide, is the addition of ethylene to sulfur dichloride: : is also a precursor to several inorganic sulfur compounds. Treatment with fluoride salts gives Sulfur tetrafluoride| via the decomposition of the intermediate sulfur difluoride. With , reacts to give "lower" sulfanes such as . oxidizes to . Reaction with ammonia affords sulfur nitrides related to tetrasulfur tetranitride|. Treatment of with primary amines gives sulfur diimides. One example is di-t-butylsulfurdiimide. ==Safety considerations==

hydrolyzes with release of HCl. Old samples contain . ==References==