sulfinic acid

Sulfinic acids RSO₂H are typically more acidic than the corresponding carboxylic acid RCO₂H.{{cite journal|title=Carboxylic Acid (Bio)Isosteres in Drug Design|journal=ChemMedChem|volume=8|issue=3|pages=385-395|last1=Ballatore|first1=Carlo|last2=Huryn|first2=Donna M.|last3=Smith III|first3=Amos B.|year=2013|doi=10.1002/cmdc.201200585|pmc=3640829}}{{cite web|url=http://ccc.chem.pitt.edu/wipf/MechOMs/evans_pKa_table.pdf|title=Chem 206: pKa's of Inorganic and Oxo-Acids|access-date=22 January 2025|last1=Ripin|first1=D.H.|last2=Evans|first2=D.A.|website=University of Pittsburgh}} Sulfur is pyramidal, consequently sulfinic acids are chiral. The free acids are typically unstable, disproportionating to the sulfonic acid RSO₃H and thiosulfonate RSSO₂R.{{rp|679}} The formal anhydride of a sulfinic acid has not joining oxygen atom, but is instead a sulfinyl sulfone (R–S⁺(–O⁻)–S²⁺(–O⁻)₂–{{prime|R}}),{{cite journal|doi=10.1002/cber.19600931145|pages=2736–2742|first1=Hellmut|last1=Bredereck|first2=Adolf|last2=Wagner|first3=Heinz|last3=Beck|first4=Rainer-Joachim|last4=Klein|title=Die Struktur der Sulfinsäureanhydride|journal=Chemische Berichte |date=1960 |volume=93 |issue=11 |lang=de|trans-title=The structure of sulfinic acid anhydrides|orig-date=2 July 1960}} and disproportionation is believed to occur through the free-radical fission of this intermediate.{{Cite journal |last1=Kice |first1=John L. |last2=Guaraldi |first2=Giancarlo |last3=Venier |first3=Clifford G. |date=Nov 1966 |title=The Mechanism of the Disproportionation of Sulfinic Acids. Rate and Equilibrium Constants for the Sulfinic Acid-Sulfinyl Sulfone (Sulfinic Anhydride) Equilibrium |url=https://pubs.acs.org/doi/abs/10.1021/jo01349a021 |journal=The Journal of Organic Chemistry |language=en |volume=31 |issue=11 |pages=3561–3567 |doi=10.1021/jo01349a021 |issn=0022-3263}}

Alkylation of sulfinic acids can give either sulfones or sulfinate esters, depending on the solvent and reagent. Strongly polarized reactants (e.g. trimethyloxonium tetrafluoroborate) give esters, whereas relatively unpolarized reactants (e.g. an alkyl halide or enone) give sulfones.{{rp|682}} Sulfinates react with Grignard reagents to give sulfoxides, and undergo a variant of the Claisen condensation towards the same end.{{rp|p=686}}

Cobalt(III) salts can oxidize sulfinic acids to disulfones, although yields are only 30–50%.{{cite journal|doi=10.1021/jo01348a514|pages=3418–3419|title=The preparation of α-disulfones by cobalt(III) oxidation|first1=George C., Jr.|last1=Denzer|first2=Paul, Jr.|last2=Allen|first3=Patrick|last3=Conway|first4=James M.|last4=van der Veen|orig-date=17 March 1966|date=Oct 1966|journal=J. Org. Chem.|volume=31 |issue=10 }}

Sulfinic acids are often prepared in situ by acidification of the corresponding sulfinate salts, which are typically more robust than the acid. These salts are generated by reduction of sulfonyl chlorides with metals,{{cite journal| author = Whitmore, F. C. | author2 = Hamilton, F. H. | doi= 10.15227/orgsyn.002.0089| title = Sodium p-Toluenesulfinic Acid | volume= 2 | page= 89| year = 1922|journal=Organic Syntheses}} although thiolates also reduce sulfonate thioesters to a sulfinate and a disulfide.{{rp|681}}

An alternative route is the reaction of Grignard reagents with sulfur dioxide. Transition metal sulfinates are also generated by insertion of sulfur dioxide into metal alkyls, a reaction that may proceed via a metal sulfur dioxide complex.

Sulfones may eliminate in base, particularly if a strong nucleophile is present; thus for example sodium cyanide causes bis(2{{nbh}}butanone-4{{nbh}}yl) sulfone to split into levulinonitrile and 3{{nbh}}oxobutane 1{{nbh}}sulfinic acid:{{rp|681}}

:SO₂((CH₂)₂Ac)₂ + NaCN → NaSO₂(CH₂)₂Ac + NC(CH₂)₂Ac

The nitrile presumably forms through conjugate addition of cyanide to the corresponding enone.

Friedel-Crafts addition of thionyl chloride to an alkene gives an α{{nbh}}chloro sulfinyl chloride, typically complexed to a Lewis acid. Likewise a carbanion can attack thionyl chloride to give a sulfinyl chloride. Careful hydrolysis then gives a sulfinic acid.{{Rp|pp=682,684}} Sulfinyl chlorides attack sulfinates to give sulfinyl sulfones (sulfinic anhydrides).

Unsubstituted sulfinic acid, when R is the hydrogen atom, is a higher energy isomer of sulfoxylic acid, both of which are unstable.

{{Gallery|title=Sulfinic Acids and Derivatives|file:thiourea dioxide.svg|thiourea dioxide, a reducing agent used in textiles

|file:Hypotaurine.svg|hypotaurine, a biosynthetic intermediate|Rongalite.svg|Rongalite, a source of "SO₂²⁻" }}

An example of a simple, well-studied sulfinic acid is phenylsulfinic acid. A commercially important sulfinic acid is thiourea dioxide, which is prepared by the oxidation of thiourea with hydrogen peroxide.D. Schubart "Sulfinic Acids and Derivatives" in Ullmann's Encyclopedia of Industrial Chemistry 2012, Wiley-VCH, Weinheim. {{doi|10.1002/14356007.a25_461}}

:(NH₂)₂CS + 2H₂O₂ → (NH)(NH₂)CSO₂H + 2H₂O

Another commercially important sulfinic acid is hydroxymethyl sulfinic acid, which is usually employed as its sodium salt (HOCH₂SO₂Na). Called Rongalite, this anion is also commercially useful as a reducing agent.

The conjugate base of a sulfinic acid is a sulfinate anion. The enzyme cysteine dioxygenase converts cysteine into the corresponding sulfinate. One product of this catabolic reaction is the sulfinic acid hypotaurine. Sulfinite also describes esters of sulfinic acid. Cyclic sulfinite esters are called sultines.

{{reflist}}

• {{MeshName|Sulfinic+Acids}}
• [http://www.chem.ucalgary.ca/courses/351/Carey5th/Ch15/ch15-1-2.html Diagram at ucalgary.ca]
• [http://www.acdlabs.com/iupac/nomenclature/93/r93_505.htm Diagram at acdlabs.com]

{{Functional groups}}

{{DEFAULTSORT:Sulfinic Acid}}

Category:Functional groups