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{{Chembox
| ImageFile = Sulfur tetrachloride.svg
| ImageSize = 200px
| IUPACName = Sulfur(IV) chloride
| OtherNames = 
| Section1 = {{Chembox Identifiers
|  CASNo = 13451-08-6
|  PubChem = 
|  ChemSpiderID = 
|  SMILES = ClS(Cl)(Cl)Cl
|  InChI = 1/Cl4S/c1-5(2,3)4
  }}
| Section2 = {{Chembox Properties
|  Formula = SCl<sub>4</sub>
|  MolarMass = 173.87
|  Appearance = White powder
|  Density = 
|  MeltingPt = -31°C
|  BoilingPt = -20°C (decomposes)
|  Solubility = soluble in water
  }}
| Section3 = {{Chembox Hazards
|   RPhrases = {{R14}}, {{R34}}, {{R50}}
|   SPhrases = {{S1/2}}, {{S26}}, {{S45}}, {{S61}}
|  MainHazards = 
|  FlashPt = 
|  Autoignition =
  }}
}}
'''Sulfur tetrachloride''' is an [[inorganic compound]] with [[chemical formula]] SCl<sub>4</sub>. It is an unstable pale yellow solid, decomposing to [[sulfur dichloride]] and chlorine at temperatures above 242K. It is obtained by treating [[sulfur dichloride]]s with [[chlorine]] at 193K:
:<math>\rm \ SCl_2 + Cl_2 \xrightarrow{193K} SCl_4</math>

Its solid structure is uncertain. It is probably the salt SCl<sub>3</sub><sup>+</sup>Cl<sup>-</sup>, since related salts are known.<ref>{{Greenwood&Earnshaw2nd}}</ref>

==Characteristics==
Sulfur tetrachloride is stable in solid state below -30 °C, and it decomposes to [[chlorine]] and [[sulfur]] when temperature rises. In solid state, there is a white, finely powdered substance. It melts with simultaneous decomposition if higher than -20 °C.<ref name="brauer">Georg Brauer: ''Handbuch der Präparativen Anorganischen Chemie''. {{de icon}}</ref> Sulfur tetrachloride reacts with water, producing [[hydrogen chloride]] and [[sulfur dioxide]] through the [[hydrolysis]] process.<ref>Holleman-Wiberg, Lehrbuch der Anorganischen Chemie, 101. Auflage, de Gruyter Verlag 1995 ISBN 3-11-012641-9 {{de icon}}</ref>

Gas phase SCl<sub>4</sub> has a [[seesaw molecular geometry]] as evidenced from [[microwave spectroscopy]] and [[electron diffraction]].<ref name=Goettel>Goettel, J. T., Kostiuk, N. and Gerken, M. (2013), ''The Solid-State Structure of SF4: The Final Piece of the Puzzle'' . Angew. Chem. Int. Ed., 52: 8037–8040. {{doi|10.1002/anie.201302917}}</ref> The liquid has a [[fluxional]] [[trigonal bipyramidal geometry]] with rapid exchange of the axial and equatorial fluorine atoms on the NMR timescale at room temperature.<ref name=Goettel /> For the solid state a structure has been reported consisting of a SCl<sub>4</sub> seesaw geometry <ref name=Goettel /> linked in a three-dimensional network by weak S-F interactions, two per per molecule.

==Reactions==
* Decomposition:
:<math>\mathrm{SCl_4 \ \xrightarrow{-15^oC}\ SCl_2 + Cl_2 }</math>

* Reacting with water in air:
:<math>\mathrm{SCl_4 + H_2O \ \xrightarrow{}\ SOCl_2 + 2HCl }</math>

* Treated with water:
:<math>\mathrm{SCl_4 + 2H_2O \ \xrightarrow{}\ SO_2 + 4HCl }</math>

* Oxidized by [[nitric acid]]:
:<math>\mathrm{SCl_4 + 2HNO_3 + 2H_2O \ \xrightarrow{}\ H_2SO_4 + 2NO_2\uparrow + 4HCl }</math>

* Reacting with [[sodium hydroxide]]:
:<math>\mathrm{SCl_4 + 6NaOH \ \xrightarrow{}\ Na_2SO_3 + 4NaCl + 3H_2O }</math><ref>Справочник химика / Редкол.: Никольский Б.П. и др.. — 3-е изд., испр. — Л.: Химия, 1971. — Т. 2. — 1168 с. {{ru icon}}</ref><ref>Химическая энциклопедия / Редкол.: Кнунянц И.Л. и др.. — М.: Советская энциклопедия, 1995. — Т. 4. — 639 с. — ISBN 5-82270-092-4 {{ru icon}}</ref><ref>Лидин Р.А. и др. Химические свойства неорганических веществ: Учеб. пособие для вузов. — 3-е изд., испр. — М.: Химия, 2000. — 480 с. — ISBN 5-7245-1163-0 {{ru icon}}</ref>

== References ==
{{reflist}}

[[Category:Sulfur compounds]]
[[Category:Chlorides]]
[[Category:Sulfur chlorides]]


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