Organosulfur chemistry

Organosulfur chemistry is the study of the properties and synthesis of organosulfur compounds, which are organic compounds that contain sulfur. They are often associated with foul odors, but many of the sweetest compounds known are organosulfur derivatives, e.g., saccharin. Nature abounds with organosulfur compounds—sulfur is vital for life. Of the 20 common amino acids, two are organosulfur compounds, and the antibiotics penicillin and sulfa drugs both contain sulfur. While sulfur-containing antibiotics save many lives, sulfur mustard is a deadly chemical warfare agent. Fossil fuels, coal, petroleum, and natural gas, which are derived from ancient organisms, necessarily contain organosulfur compounds, the removal of which is a major focus of oil refineries.
Sulfur shares the chalcogen group with oxygen, selenium, and tellurium, and it is expected that organosulfur compounds have similarities with carbon–oxygen, carbon–selenium, and carbon–tellurium compounds.
A classical chemical test for the detection of sulfur compounds is the Carius halogen method.

Structural classes

Organosulfur compounds can be classified according to the sulfur-containing functional groups, which are listed in decreasing order of their occurrence.

Sulfides

Sulfides, formerly known as thioethers, are characterized by C−S−C bonds Relative to C−C bonds, C−S bonds are both longer, because sulfur atoms are larger than carbon atoms, and about 10% weaker. Representative bond lengths in sulfur compounds are 183 pm for the S−C single bond in methanethiol and 173 pm in thiophene. The C−S bond dissociation energy for thiomethane is 89 kcal/mol compared to methane's 100 kcal/mol and when hydrogen is replaced by a methyl group the energy decreases to 73 kcal/mol. The single carbon to oxygen bond is shorter than that of the C−C bond. The bond dissociation energies for dimethyl sulfide and dimethyl ether are respectively 73 and 77 kcal/mol.
Sulfides are typically prepared by alkylation of thiols. Alkylating agents include not only alkyl halides, but also epoxides, aziridines, and Michael acceptors.
They can also be prepared via the Pummerer rearrangement.
In the Ferrario reaction, phenyl ether is converted to phenoxathiin by action of elemental sulfur and aluminium chloride.
Thioacetals and thioketals feature C−S−C−S−C bond sequence. They represent a subclass of sulfides. The thioacetals are useful in "umpolung" of carbonyl groups. Thioacetals and thioketals can also be used to protect a carbonyl group in organic syntheses.
The above classes of sulfur compounds also exist in saturated and unsaturated heterocyclic structures, often in combination with other heteroatoms, as illustrated by thiiranes, thiirenes, thietanes, thietes, dithietanes, thiolanes, thianes, dithianes, thiepanes, thiepines, thiazoles, isothiazoles, and thiophenes, among others. The latter three compounds represent a special class of sulfur-containing heterocycles that are aromatic. The resonance stabilization of thiophene is 29 kcal/mol compared to 20 kcal/mol for the oxygen analogue furan. The reason for this difference is the higher electronegativity for oxygen [|drawing] away electrons to itself at the expense of the aromatic ring current. Yet as an aromatic substituent the thio group is less electron-releasing than the alkoxy group. Dibenzothiophenes, tricyclic heterocycles consisting of two benzene rings fused to a central thiophene ring, occurs widely in heavier fractions of petroleum.

Thiols, disulfides, polysulfides

groups contain the functionality R−SH. Thiols are structurally similar to the alcohol group, but these functionalities are very different in their chemical properties. Thiols are more nucleophilic, more acidic, and more readily oxidized. This acidity can differ by 5 pK_a units.
The difference in electronegativity between sulfur and hydrogen is small and therefore hydrogen bonding in thiols is not prominent. Aliphatic thiols form monolayers on gold, which are topical in nanotechnology.
Certain aromatic thiols can be accessed through a Herz reaction.
Removal of the hydrogen atom gives a thiyl radical, an unstable reaction intermediate.
Disulfides R−S−S−R with a covalent sulfur to sulfur bond are important for crosslinking: in biochemistry for the folding and stability of some proteins and in polymer chemistry for the crosslinking of rubber.
Longer sulfur chains are also known, such as in the natural product varacin which contains an unusual pentathiepin ring.

Inorganic thioesters

Esters of thiols with inorganic acids generally have properties deducible from those of thiols and the corresponding acid. Some are, however, of biological interest.
Thiophosphate esters see extensive use in pharmacology and agriculture, as the moiety tends to stall enzymes that hydrolyze phosphates.
S-Nitrosothiols, also known as thionitrites, attach a nitroso group to a thiol, e.g. R−S−N=O. They have received considerable attention in biochemistry because they serve as donors of the nitrosonium ion, NO⁺, and nitric oxide, NO, which may serve as signaling molecules in living systems, especially related to vasodilation.

Thioic acid derivatives

s and dithiocarboxylic acids are well known. They are structurally similar to carboxylic acids but more acidic.
Thioesters have general structure R−C−S−R. They are related to regular esters but are more susceptible to hydrolysis and related reactions. Thioesters formed from coenzyme A are prominent in biochemistry, especially in fatty acid synthesis.
Thioamides, with the formula R₁CNR₃ are more common than thioketones and thioaldehydes. They are typically prepared by the reaction of amides with Lawesson's reagent. Isothiocyanates, with formula R−N=C=S, are found naturally. Vegetable foods with characteristic flavors due to isothiocyanates include wasabi, horseradish, mustard, radish, Brussels sprouts, watercress, nasturtiums, and capers.
Few thioacyl chlorides are stable.
Thiocyanates, R−S−CN, are related to [|sulfenyl halides] and esters in terms of reactivity.

Other unsaturated C–S bonding

Compounds with double bonds between carbon and sulfur are relatively uncommon, but include the important compounds carbon disulfide, carbonyl sulfide, and thiophosgene. Thioketones are uncommon with alkyl substituents, but one example is thiobenzophenone. Thioaldehydes are rarer still, reflecting their lack of steric protection.
The S-oxides of thiocarbonyl compounds are known as thiocarbonyl S-oxides:. The thione S-oxides have also been known as sulfines, and while IUPAC considers this term obsolete, the name persists in the literature. These compounds are well known with extensive chemistry. Examples include syn-propanethial-S-oxide and sulfene.
Triple bonds between sulfur and carbon in sulfaalkynes are rare and can be found in carbon monosulfide and have been suggested for the compounds F₃CCSF₃ and F₅SCSF₃. The unbranched compound HCSOH is also represented as having a formal triple bond.

Sulfur halides

A wide range of organosulfur compounds are known which contain one or more halogen atom bonded to a single sulfur atom, e.g.: sulfenyl halides, RSX; sulfinyl halides, RSX; sulfonyl halides, RSO₂X; alkyl and arylsulfur trichlorides, RSCl₃ and trifluorides, RSF₃; and alkyl and arylsulfur pentafluorides, RSF₅. Less well known are dialkylsulfur tetrahalides, mainly represented by the tetrafluorides, e.g., R₂SF₄.

S-oxidized moieties

A sulfoxide, R−S−R, is the S-oxide of a sulfide ; a sulfone, R−S₂−R, is the S,''S-dioxide of a sulfide; a thiosulfinate, R−S−S−R, is the S''-oxide of a disulfide; and a thiosulfonate, R−S₂−S−R, is the S,''S''-dioxide of a disulfide. All of these compounds are well known with extensive chemistry, e.g., dimethyl sulfoxide, dimethyl sulfone, and allicin.
Sulfonic acids have functionality R−S₂−OH. They are strong acids that are typically soluble in organic solvents. Sulfonic acids like trifluoromethanesulfonic acid is a frequently used reagent in organic chemistry. Sulfinic acids have functionality R−S−OH while sulfenic acids have functionality R−S−OH. In the series sulfonic—sulfinic—sulfenic acids, both the acid strength and stability diminish in that order. Sulfonamides, sulfinamides and sulfenamides, with formulas R−SO₂N₂, R−SN₂, and R−SN₂, respectively, each have a rich chemistry. For example, sulfa drugs are sulfonamides derived from aromatic sulfonation. Chiral sulfinamides are used in asymmetric synthesis, while sulfenamides are used extensively in the vulcanization process to assist cross-linking.

S-oxidation with nitrogen

are sulfur–nitrogen compounds of structure R₂S⁺N⁻, the nitrogen analog of sulfoxides. They are of interest in part due to their pharmacological properties. When two different R groups are attached to sulfur, sulfimides are chiral. Sulfimides form stable α-carbanions.
Sulfinyl nitrenes, despite their formal resonance structure as R-S≡N, instead behave primarily as nitrenic sulfinamides.
Sulfoximides are tetracoordinate sulfur–nitrogen compounds, isoelectronic with sulfones, in which one oxygen atom of the sulfone is replaced by a substituted nitrogen atom, e.g., R₂S=N. When two different R groups are attached to sulfur, sulfoximides are chiral. Much of the interest in this class of compounds is derived from the discovery that methionine sulfoximide is an inhibitor of glutamine synthetase.
In Sulfonediimines, a nitrogen replaces both sulfone oxygen atoms, e.g., R₂S₂. They are of interest because of their biological activity and as building blocks for heterocycle synthesis.
Sulfinylamines are bicoordinate sulfur-oxygen-nitrogen compounds, roughly describable as RN=S⁺-O⁻.