Sulfur tetrachloride
Names | |
---|---|
IUPAC name Sulfur(IV) chloride | |
Identifiers | |
CAS Number |
|
3D model (JSmol) |
|
ECHA InfoCard | 100.149.178 |
PubChem CID |
|
CompTox Dashboard (EPA) |
|
InChI
| |
| |
Properties | |
Chemical formula | 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) |
Solubility in water | soluble in water |
Hazards | |
GHS labelling: | |
Pictograms | |
Danger | |
Hazard statements | H314, H400 |
Precautionary statements | 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). Infobox references |
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:
- (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]
Reactions
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)
- Oxidized by nitric acid:
- (5)
References
- ^ Georg Brauer: Handbuch der Präparativen Anorganischen Chemie. (in German)
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ Christian, Beverly H.; Collins, Michael J.; Gillespie, Ronald J.; Sawyer, Jeffery F. "Preparations, Raman spectra, and crystal structures of (SCl3)(SbCl6), (SeCl3)(SbCl6), (SBr1.2Cl1.8)(SbCl6), (TeCl3)(AlCl4) (triclinic modification), (TeCl3)(SbF6), (TeCl3)(AsF6), and (TeF3)2(SO4)" Inorganic Chemistry 1986, volume 25, 777-88. doi:10.1021/ic00226a012
- ^ 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
- ^ Holleman-Wiberg, Lehrbuch der Anorganischen Chemie, 101. Auflage, de Gruyter Verlag 1995 ISBN 3-11-012641-9 (in German)
- v
- t
- e
disulfides
- Al2S3
- As2S2
- As2S3
- As2S5
- As4S4
- Au2S
- Au2S3
- B2S3
- BaS
- BeS
- Bi2S3
- CS2
- C3S2
- C6S6
- CaS
- CdS
- CeS
- CoS
- Cr2S3
- CSSe
- CSTe
- CuFeS2
- CuS
- D2S
- Dy2S3
- Er2S3
- EuS
- FeS2
- GaS
- H2S
- HfS2
- HgS
- In2S3
- K2S
- LaS
- LiS
- MgS
- MoS2
- MoS3
- NaHS
- Na2S
- NH4HS
- NiS
- P4Sx
- PbS
- PbS2
- PSCl3
- PSI3
- PtS
- ReS2
- Re2S7
- SiS
- SrS
- TlS
- VS
- SeS2
- S2U
- WS2
- WS3
- Sb2S3
- Sb2S5
- Sb4S3O3
- Sm2S3
- Y2S3
- ZrS2
- La
2O
2S - Gd
2O
2S
- S2Br2
- SBr2
- S2Cl2
- SCl2
- SCl4
- SF2
- SF4
- S2F10
- SF6
- S2I2
and oxyhalides
- SO2
- SO3
- SOBr2
- SOCl2
- SOF2
- SOF4
- H2S3O6
- H2SO3
- H2SO4
- H2S2O7
- H2SO5
Sulfites |
|
---|---|
Sulfates |
|
- C2H4S
- C2H6S3
- C4H4S
- C32H66S2
- CHCl3S
- C2H3SN