Sulfur tetrafluoride
| |||
Names | |||
---|---|---|---|
IUPAC name
Sulfur(IV) fluoride
| |||
Other names
Sulfur tetrafluoride
| |||
Identifiers | |||
3D model (
JSmol ) |
|||
ChEBI | |||
ChemSpider | |||
ECHA InfoCard
|
100.029.103 | ||
PubChem CID
|
|||
RTECS number
|
| ||
UNII | |||
UN number | 2418 | ||
CompTox Dashboard (EPA)
|
|||
| |||
| |||
Properties | |||
SF4 | |||
Molar mass | 108.07 g/mol | ||
Appearance | colorless gas | ||
Density | 1.95 g/cm3, −78 °C | ||
Melting point | −121.0 °C | ||
Boiling point | −38 °C | ||
reacts | |||
Vapor pressure | 10.5 atm (22 °C)[1] | ||
Structure | |||
Seesaw (C2v) | |||
0.632 D[2] | |||
Hazards | |||
Occupational safety and health (OHS/OSH): | |||
Main hazards
|
highly toxic corrosive | ||
NFPA 704 (fire diamond) | |||
NIOSH (US health exposure limits): | |||
PEL (Permissible)
|
none[1] | ||
REL (Recommended)
|
C 0.1 ppm (0.4 mg/m3)[1] | ||
IDLH (Immediate danger) |
N.D.[1] | ||
Safety data sheet (SDS) | ICSC 1456 | ||
Related compounds | |||
Other anions
|
Sulfur dichloride Disulfur dibromide Sulfur trifluoride | ||
Other cations
|
Oxygen difluoride Selenium tetrafluoride Tellurium tetrafluoride | ||
Related sulfur fluorides
|
Disulfur difluoride Sulfur difluoride Disulfur decafluoride Sulfur hexafluoride | ||
Related compounds
|
Thionyl fluoride | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|
Sulfur tetrafluoride is a
Structure
Sulfur in SF4 is in the +4
The 19F NMR spectrum of SF4 reveals only one signal, which indicates that the axial and equatorial F atom positions rapidly interconvert via pseudorotation.[4]
Synthesis and manufacture
At the laboratory scale, sulfur tetrafluride is prepared from elemental sulfur and
- S + 4CoF3 → SF4 + 4CoF2
SF4 is industrially produced by the reaction of SCl2 and NaF with acetonitrile as a catalyst[6]
- 3 SCl2 + 4 NaF → SF4 + S2Cl2 + 4 NaCl
At higher temperatures (e.g. 225–450 °C), the solvent is superfluous. Moreover, sulfur dichloride may be replaced by elemental sulfur (S) and chlorine (Cl2).[7][8]
A low-temperature (e.g. 20–86 °C) alternative to the chlorinative process above uses liquid bromine (Br2) as oxidant and solvent:[9]
- S(s) + 2 Br2(l; excess) + 4KF(s) → SF4↑ + 4 KBr(brom)
Use in synthesis of organofluorine compounds
In organic synthesis, SF4 is used to convert COH and C=O groups into CF and CF2 groups, respectively.[10] The efficiency of these conversions are highly variable.
In the laboratory, the use of SF4 has been superseded by the safer and more easily handled diethylaminosulfur trifluoride, (C2H5)2NSF3, "DAST":[11] This reagent is prepared from SF4:[12]
- SF4 + (CH3)3SiN(C2H5)2 → (C2H5)2NSF3 + (CH3)3SiF
Other reactions
Sulfur chloride pentafluoride (SF
5Cl), a useful source of the SF5 group, is prepared from SF4.[13]
- SF4 + Cl2 + CsF → SF5Cl + CsCl
Hydrolysis of SF4 gives sulfur dioxide:[14]
- SF4 + 2 H2O → SO2 + 4 HF
This reaction proceeds via the intermediacy of thionyl fluoride, which usually does not interfere with the use of SF4 as a reagent.[6]
When amines are treated with SF4 and a base, aminosulfur difluorides result.[15]
Toxicity
SF
4 reacts inside the lungs with moisture, forming sulfur dioxide and hydrogen fluoride which forms highly toxic and corrosive hydrofluoric acid [16]
References
- ^ a b c d NIOSH Pocket Guide to Chemical Hazards. "#0580". National Institute for Occupational Safety and Health (NIOSH).
- .
- ISBN 9780471936237.
- ISBN 0-12-352651-5.
- LCCN 63-14307– via the Internet Archive.
- ^ ISBN 978-0-470-13166-4.
- .
- ^ US 2992073, Tullock, C.W., "Synthesis of Sulfur Tetrafluoride", issued 1961
- .
- ISBN 9780471936237..
- .
- ISBN 9780470132395.
- ISBN 978-0-08-037941-8.
- ISSN 0040-4039.
- ISBN 981-238-153-8.