Carbon disulfide (CS2)

Structure and properties

In CS2 the central carbon is formally in a +4 oxidation state while each sulfur is often treated as -2; the bonding can be represented by double bonds to sulfur and delocalized electron distributions. The molecule is relatively nonpolar, a good solvent for many organic substances and sulfur-containing compounds, and is practically immiscible with water. Its volatility and flammability are key physical characteristics.

Production and history

Historically CS2 was produced by heating carbon (such as coke) with sulfur; it also appears as a byproduct in some high-temperature industrial processes. Industrial manufacture evolved to larger-scale methods to supply its uses in the late 19th and 20th centuries. For elemental constituents consult constituent elements.

Uses and applications

• Organic solvent for phosphorus, sulfur, and rubber-processing chemicals.
• Intermediate in the manufacture of cellulose xanthate, which is converted into viscose rayon and cellophane films.
• Precursor to other sulfur-containing chemicals and occasionally used historically as a fumigant or pesticide (now restricted in many regions).

Health, safety and regulation

CS2 is highly flammable and its vapors can be toxic; acute exposure may depress the central nervous system, and chronic exposure has been associated with neurological and reproductive effects and liver damage. Handling requires engineering controls, monitoring and personal protective equipment. International and national agencies set occupational limits and control measures; see safety guidance for more information and oxidation states and hazard context.