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Symmetrical sulfides contain identical hydrocarbon groups bonded to the central sulfur atom, while asymmetrical sulfides have different groups attached to sulfur. Symmetrical sulfides form when 2 moles of alkyl halide react with 1 mole of sodium sulfide via SN2 mechanism. Asymmetrical sulfides are produced when a thiol reacts with an alkyl halide in the presence of a base, such as when benzenethiol reacts with methyl iodide and sodium hydroxide to yield methyl phenyl sulfide.

The base first deprotonates the thiol to produce a thiolate ion, which acts as a nucleophile. The thiolate ion then attacks the alpha carbon of the alkyl halide, displacing the halide ion and forming the sulfide through an SN2 reaction. This reaction is called the sulfur analog of Williamson ether synthesis and works best with methyl and primary alkyl halides, preferring these substrates over tertiary halides.

Sulfides readily oxidize at the sulfur atom to produce sulfoxides, which can further oxidize to sulfones. One equivalent of hydrogen peroxide at room temperature converts a sulfide to a sulfoxide. Further treatment with a peroxy acid oxidizes the sulfoxide to a sulfone. Alternatively, two equivalents of hydrogen peroxide directly converts the sulfide to a sulfone in a single step.

Cyclic sulfides form when dihalogenated compounds react with sodium sulfide under SN2 conditions. For example, 1,4-dichlorobutane produces a five-membered cyclic sulfide, while 1,5-dichloropentane yields a six-membered cyclic sulfide. The two halide groups are displaced sequentially by the sulfide nucleophile, forming the ring structure with sulfur as a ring atom.

Sulfoxides and sulfones are excellent dipolar aprotic solvents due to their chemical structure and polarity. Common examples include dimethyl sulfoxide (DMSO) and tetramethylene sulfone. These compounds can dissolve both polar and nonpolar substances effectively, making them valuable in organic synthesis, reactions, and laboratory applications where aprotic solvent properties are required.

Unlike ethers, which are non-oxidizable at the oxygen atom, sulfides can readily oxidize at the sulfur atom. This difference arises from sulfur's larger atomic size, lower electronegativity, and greater ability to expand its valence shell compared to oxygen. These properties make sulfur more susceptible to nucleophilic attack by oxidizing agents like hydrogen peroxide and peroxy acids.

Symmetrical sulfides form when 2 moles of alkyl halide react with 1 mole of sodium sulfide in an SN2 reaction without added base. Asymmetrical sulfides require a thiol starting material, an alkyl halide, and an external base like sodium hydroxide. The choice of starting material and reagents determines the sulfide structure, allowing chemists to selectively prepare either symmetrical or asymmetrical products.