Disulfides

Sulfur is usually Reduced to a state with Oxidation Number −2 and forms a S²⁻ Ion , called a Sulfide ion, which has the electron configuration of a Noble Gas ( Argon ).

In some cases sulfur is only reduced to a state with oxidation number −1. Its configuration then resembles that of Chlorine and, like it, has the tendency to form a covalent bond with another S⁻ ion to form a disulfide (S₂)²⁻. Oxygen can also do this; e.g. in Peroxide s such as H₂O₂. In many cases, each of the two sulfur atoms in a disulfide group is covalently bonded to a carbon atom in an Organic Compound , forming a Disulfide Bond , sometimes called a ''disulfide linkage'' or a ''disulfide bridge''. Such organic compounds are often biologically occurring.

The tendency is a bit more elaborate in the case of sulfur, which can form Polysulfide s.

SOME EXAMPLES

An example of an Inorganic disulfide compound is Cadmium disulfide (CdS₂).

An inorganic example with covalent bonds is disulfur dichloride (S₂Cl₂) - a yellow liquid with a foul odor used in vulcanization of rubber.

Examples of organic compounds containing a disulfide bond or group are the biological amino acid Cystine and Alpha Lipoic Acid .

The compound Carbon Disulfide (CS₂) has a covalently bonded molecule similar to Carbon Dioxide except both Oxygen atoms are replaced by sulfur atoms.

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Disulfides