![]() | |
Names | |
---|---|
IUPAC name
Sulfur(IV) chloride | |
Identifiers | |
3D model (JSmol) |
|
ECHA InfoCard | 100.149.178 ![]() |
PubChem CID |
|
CompTox Dashboard (EPA) |
|
| |
| |
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: | |
![]() ![]() | |
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).
|
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.
It is obtained by treating sulfur dichloride with chlorine at 193 K:
(1) |
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 noncoordinating anions.[2][3] In contrast to this tetrachloride, SF4 is a neutral molecule.[4]
It decomposes above −30 °C (242 K) to sulfur dichloride and chlorine.
(2) |
It hydrolyzes readily:
(3) |
Sulfur tetrachloride reacts with water, producing hydrogen chloride and sulfur dioxide through the hydrolysis process. Thionyl chloride is an implied intermediate.[5]
(4) |
(5) |
| |||||
---|---|---|---|---|---|
Sulfides and disulfides |
| ||||
Sulfur halides |
| ||||
Sulfur oxides and oxyhalides |
| ||||
Thiocyanates |
| ||||
Organic compounds |
|
![]() | This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |