Sulfur tetrachloride
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| Names | |
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| IUPAC name
Sulfur(IV) chloride
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| Identifiers | |
3D model (
JSmol ) |
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ECHA InfoCard
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100.149.178 |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| SCl4 | |
| Molar mass | 173.87 |
| Appearance | White powder |
| Melting point | −31 °C (−24 °F; 242 K) |
| Boiling point | −20 °C (−4 °F; 253 K) (decomposes) |
| soluble in water | |
| Hazards | |
| GHS labelling: | |
 
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| Danger | |
| H314, H400 | |
| P260, P264, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P391, P405, P501 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Sulfur tetrachloride is an inorganic compound with chemical formula SCl4. It has only been obtained as an unstable pale yellow solid. The corresponding SF4 is a stable, useful reagent.
Preparation and structure
It is obtained by treating sulfur dichloride with chlorine at 193 K:
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(1)
![{\displaystyle {\begin{matrix}{}\\{\ce {{SCl2}+Cl2->[{\text{193 K}}]SCl4}}\\{}\end{matrix}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/a9def2efb84134526c63d5304a080329bfcf89b9)
It melts with simultaneous decomposition above −20 °C.[1]
Its solid structure is uncertain. It is probably the salt SCl3+Cl−, since related salts are known with
Reactions
It decomposes above −30 °C (242 K) to sulfur dichloride and chlorine.
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(2)
![{\displaystyle {\begin{matrix}{}\\{\ce {SCl4->[{\text{-15 }}^{\circ }{\ce {C}}]{SCl2}+Cl2}}\\{}\end{matrix}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/502e8c19766026db1f83a732e9e7a102a8ebc2c1)
It hydrolyzes readily:
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(3)
Sulfur tetrachloride reacts with water, producing hydrogen chloride and sulfur dioxide through the hydrolysis process. Thionyl chloride is an implied intermediate.[5]
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(4)
- Oxidized by nitric acid:
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(5)
References
- ^ Georg Brauer: Handbuch der Präparativen Anorganischen Chemie. (in German)
- ISBN 978-0-08-037941-8.
- ISBN 3-11-012641-9(in German)
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