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{{Category see also|Sulfur compounds}}
'''Sulfur compounds''' are [[chemical compound]]s formed the element [[sulfur]] (S). Common [[oxidation state]]s of sulfur range from −2 to +6. Sulfur forms stable compounds with all elements except the [[noble gas]]es.

== Hydrogen sulfide ==

{{Main article|Hydrogen sulfide}}

Treatment of sulfur with hydrogen gives [[hydrogen sulfide]]. When dissolved in water, hydrogen sulfide is mildly acidic:<ref name="Greenwd">Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.), Oxford:Butterworth-Heinemann. {{ISBN|0-7506-3365-4}}.</ref>
:H<sub>2</sub>S {{eqm}} HS<sup>−</sup> + H<sup>+</sup>

Hydrogen sulfide gas and the hydrosulfide anion are extremely toxic to mammals, due to their inhibition of the oxygen-carrying capacity of hemoglobin and certain [[cytochrome]]s in a manner analogous to [[cyanide]] and [[azide]].

== Oxides ==
The two principal sulfur oxides are obtained by burning sulfur:
:S + O<sub>2</sub> → SO<sub>2</sub> ([[sulfur dioxide]])
:2 SO<sub>2</sub> + O<sub>2</sub> → 2 SO<sub>3</sub> ([[sulfur trioxide]])
Many other sulfur oxides are observed including the [[lower sulfur oxides|sulfur-rich oxides]] include sulfur monoxide, disulfur monoxide, disulfur dioxides, and [[higher sulfur oxides|higher oxides]] containing peroxo groups.

== Halides ==
Sulfur reacts with fluorine to give the highly reactive [[sulfur tetrafluoride]] and the highly inert [[Sulfur hexafluoride]].<ref>{{OrgSynth|last=Hasek|first=W. R.|title=1,1,1-Trifluoroheptane|volume=41|page=104|year=1961|doi=10.1002/0471264180.os041.28}}</ref> Whereas fluorine gives S(IV) and S(VI) compounds, chlorine gives S(II) and S(I) derivatives.  Thus, [[sulfur dichloride]], [[disulfur dichloride]], and higher chlorosulfanes arise from the chlorination of sulfur.   [[Sulfuryl chloride]] and [[chlorosulfuric acid]] are derivatives of sulfuric acid; [[thionyl chloride]] (SOCl<sub>2</sub>) is a common reagent in [[organic synthesis]].<ref>{{OrgSynth|last1=Rutenberg|first1=M. W.|last2=Horning|first2=E. C.|title= 1-Methyl-3-ethyloxindole|volume=30|page=62|year=1950|doi=10.15227/orgsyn.030.0062}}</ref>

=== Pseudohalides ===
Sulfur oxidizes [[cyanide]] and [[sulfite]] to give [[thiocyanate]] and [[thiosulfate]], respectively.

== Metal sulfides ==
Sulfur reacts with many metals. Electropositive metals give polysulfide salts. [[Copper]], [[zinc]] and [[silver]] are [[tarnished]] by slfur. Although many [[sulfide mineral|metal sulfides]] are known, most are prepared by high temperature reactions of the elements.<ref>{{Cite book |last=Vaughan |first=David J. |title=Mineral chemistry of metal sulfides |last2=Craig |first2=James R. |date=1978 |publisher=Cambridge university press |isbn=978-0-521-21489-6 |series=Cambridge earth science series |location=Cambridge London New york [etc.]}}</ref> Sulfide minerals contain the [[sulfide]] (S<sup>2-</sup>) or [[disulfide]] (S<sub>2</sub><sup>2-</sup>) anions. Typical examples are:

*[[Acanthite]] {{chem2|Ag2S}}
*[[Chalcocite]] {{chem2|Cu2S}}
*[[Galena]] {{chem2|PbS}}
*[[Sphalerite]] {{chem2|ZnS}}
*[[Chalcopyrite]] {{chem2|CuFeS2}}
*[[Millerite]] {{chem2|NiS}}
*[[Cinnabar]] {{chem2|HgS}}
*[[Stibnite]] {{chem2|Sb2S3}}
*[[Pyrite]] {{chem2|FeS2}}
*[[Molybdenite]] {{chem2|MoS2}}

== Organic compounds ==

{{Main|Organosulfur compounds}}

<gallery caption="Illustrative organosulfur compounds">
File:Allicin skeletal.svg|[[Allicin]], a chemical compound in garlic
File:L-Cystein - L-Cysteine.svg |(''R'')-[[cysteine]], an [[amino acid]] containing a thiol group
File:Methionin - Methionine.svg|[[Methionine]], an [[amino acid]] containing a thioether
File:Diphenyl disulfide.svg|[[Diphenyl disulfide]], a representative disulfide
File:Perfluorooctanesulfonic acid structure.svg|[[Perfluorooctanesulfonic acid]], a surfactant
File:Dibenzothiophen - Dibenzothiophene.svg|[[Dibenzothiophene]], a component of crude oil
File:Penicillin core.svg|[[Penicillin]], an antibiotic where "R" is the variable group
</gallery>

Some of the main classes of sulfur-containing organic compounds include the following:<ref name="Cremlyn">{{cite book | author = Cremlyn R. J. | title = An Introduction to Organosulfur Chemistry | publisher = John Wiley and Sons | location = Chichester | date = 1996 | isbn = 0-471-95512-4 }}</ref>
* [[Thiol]]s or mercaptans (so called because they capture mercury as [[chelation|chelators]]) are the sulfur analogs of [[Alcohol (chemistry)|alcohol]]s; treatment of thiols with base gives [[thiolate]] ions.
* [[Thioether]]s are the sulfur analogs of [[ether]]s.
* [[Sulfonium]] ions have three groups attached to a cationic sulfur center. [[Dimethylsulfoniopropionate]] (DMSP) is one such compound, important in the marine organic [[sulfur cycle]].
* [[Sulfoxide]]s and [[sulfone]]s are thioethers with one and two oxygen atoms attached to the sulfur atom, respectively. The simplest sulfoxide, [[dimethyl sulfoxide]], is a common solvent; a common sulfone is [[sulfolane]].
* [[Sulfonic acid]]s are used in many detergents.

Compounds with carbon–sulfur multiple bonds are uncommon, an exception being [[carbon disulfide]], a volatile colorless liquid that is structurally similar to carbon dioxide. It is used as a reagent to make the polymer [[rayon]] and many organosulfur compounds. Unlike [[carbon monoxide]], [[carbon monosulfide]] is stable only as an extremely dilute gas, found between solar systems.<ref>{{cite journal|last1=Wilson|first1=R. W.|last2=Penzias|first2=A. A.|last3=Wannier|first3=P. G.|last4=Linke|first4=R. A.|author-link=Robert Woodrow Wilson|author-link2=Arno Allan Penzias|title=Isotopic abundances in interstellar carbon monosulfide|journal=Astrophysical Journal|date=15 March 1976|volume=204|pages=L135–L137|doi=10.1086/182072|bibcode=1976ApJ...204L.135W}}</ref>

Organosulfur compounds are responsible for some of the unpleasant odors of decaying organic matter. They are widely known as the [[odorizer|odorant]] in domestic natural gas, garlic odor, and skunk spray. Not all organic sulfur compounds smell unpleasant at all concentrations: the sulfur-containing [[terpene|monoterpenoid]] ([[grapefruit mercaptan]]) in small concentrations is the characteristic scent of grapefruit, but has a generic thiol odor at larger concentrations. [[Sulfur mustard]], a potent [[blister agent|vesicant]], was [[Chemical weapons in World War I|used in World War I]] as a disabling agent.<ref>{{cite book|last=Banoub|first=Joseph|title=Detection of Biological Agents for the Prevention of Bioterrorism|journal=Detection of Biological Agents for the Prevention of Bioterrorism|date=2011|isbn=978-90-481-9815-3|oclc=697506461|page=183|bibcode=2011dbap.book.....B|doi=10.1007/978-90-481-9815-3|series=NATO Science for Peace and Security Series A: Chemistry and Biology}}</ref>

Sulfur–sulfur bonds are a structural component used to stiffen rubber, similar to the disulfide bridges that rigidify proteins (see biological below). In the most common type of industrial "curing" or hardening and strengthening of natural [[rubber]], elemental sulfur is heated with the rubber to the point that chemical reactions form [[disulfide]] bridges between [[isoprene]] units of the polymer. This process, patented in 1843, made rubber a major industrial product, especially in automobile tires. Because of the heat and sulfur, the process was named [[sulfur vulcanization|vulcanization]], after the Roman god of the forge and [[volcanism]].

== See also ==

* [[:Category:Sulfur compounds]]
* [[Oxygen compounds]]
* [[Selenium compounds]]
* [[Phosphorus compounds]]
* [[Chlorine compounds]]

== References ==

{{reflist}}

{{Sulfur compounds}}