2699-79-8

Usage

Chemical Properties

Different sources of media describe the Chemical Properties of 2699-79-8 differently. You can refer to the following data:
1. colourless odourless gas
2. Sulfuryl fluoride is a colorless, poisonous gas. Odorless.

Uses

Different sources of media describe the Uses of 2699-79-8 differently. You can refer to the following data:
1. Sulfuryl fluoride is another promising chemical, which is widely used for control of termites, and stored-product insects. This chemical shows considerable promise and is undergoing registration procedures as replacement for methyl bromide in several countries including the United States, Great Britain, Italy, and France. The fumigant has vapour pressure of about ten times higher (13,442 mm of Hg at 25oC) than that of methyl bromide and hence it is more penetrative into treated commodities which is a significant benefit in situations where insect infestations are located deep within cracks or machinery in premises such as flour mills . The fumigant has several other advantages as a replacement for methyl bromide; it is nonreactive with structural materials and components of electronic equipment, is non flammable and has not caused problems of taint following treatment of a wide range of materials. However the sulfuryl fluoride was found to be less effective in controlling the insect eggs.
2. Insect fumigant
3. Fumigant insecticide; termiticide.

General Description

A colorless odorless gas. Shipped as a liquefied gas under its own vapor pressure. Noncombustible. Heavier than air. Very toxic by inhalation. Contact with the unconfined liquid can cause frostbite. Prolonged exposure to heat can cause containers to rupture violently and rocket.

Air & Water Reactions

Reacts with moist air to give corrosive acid mists that are heavier than air. Decomposes with water forming hydrofluoric acid and sulfuric acid. Reacts violently with bases [Handling Chemicals Safely p. 881 1980].

Reactivity Profile

SULFURYL FLUORIDE is incompatible with water, strong oxidizing agents, alcohols, amines, and bases. May react vigorously or explosively if mixed with diisopropyl ether or other ethers in the presence of trace amounts of metal salts [J. Haz. Mat., 1981, 4, 291].

Hazard

Toxic by inhalation. Central nervous system impairment.

Agricultural Uses

Fumigant: Sulfuryl fluoride is used to fumigate closed structures and their contents such as domestic dwellings, garages, barns, storage buildings, commercial warehouses, ships in port, and railroad cars. It controls numerous insect pests including termites, powder post beetles, old house borers, bedbugs, carpet beetles, clothes moths and cockroaches, as well as rats and mice. It is also used in organic synthesis of drugs and dyes. Use pending in EU countries[ 115]. Registered for use in the U.S.

Trade name

TERMAFUME?; VIKANE?; VIKANE FUMIGANT?

Safety Profile

Poison by ingestion. Mildly toxic by inhalation. Accidental human exposure caused nausea, vomiting, cramps, itching. May be narcotic in high concentration. Experimental reproductive effects. Can react with water, steam. When heated to decomposition it emits very toxic fumes of Fand SOx. See also FLUORIDES.

Potential Exposure

Sulfuryl fluoride is used an insecticidal fumigant. It is also used in organic synthesis of drugs and dyes.

Shipping

UN2191 Sulfuryl fluoride, Hazard Class: 2.3; Labels: 2.3-Poisonous gas, Inhalation Hazard Zone D.

Incompatibilities

Reacts with water and steam; at temperatures ＞300℃, forms strong, highly corrosive acids. Incompatible with strong oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause fires or explosions. Keep away from metal hydroxides, alcohols, alkaline materials, amines, strong acids, strong bases. Fluorides form explosive gases on contact with strong acids or acid fumes.

Waste Disposal

Return refillable compressed gas cylinders to supplier. Addition of soda ash-slaked lime solution to form the corresponding sodium and calcium salt solution. This solution can be safely discharged after dilution. The precipitated calcium fluoride may be buried or added to a landfill. Small amounts could also be released directly to the atmosphere without serious harm.

InChI:InChI=1/F2O2S/c1-5(2,3)4

Upstream product

• 7791-25-5 sulfuryl dichloride 
• 102-82-9 tributyl-amine 
• 76-05-1 trifluoroacetic acid 
• 717-45-3 4-fluoro-1,3-dibenzenedisulfonyl chloride 
• 7783-41-7 difluoroether 
• 7446-09-5 sulfur dioxide 
• 7446-11-9 sulfur trioxide 
• 13709-36-9 xenon difluoride 
• 7664-39-3 hydrogen fluoride 
• 7783-54-2 nitrogen trifluoride 
• 7783-60-0 sulfur tetrafluoride 
• 7783-70-2 antimony pentafluoride 
• 2551-62-4 sulfur(VI) hexafluoride 
• 7783-39-3 mercury(II) fluoride 

Downstream Products

• 382-97-8 N,N-Diethylamidosulfonyl fluoride 
• 25479-04-3 diethylamine monohydrofluoride 
• 55589-62-3 potassium acesulfame 
• 14984-73-7 bis(fluorosulfonyl)amide 
• 775-27-9 4-methoxyphenyl sulfurofluoridate 
• 51451-34-4 4-nitrophenyl sulfurofluoridate 
• 42158-97-4 1,4-phenylene bis(sulfurofluoridate) 
• 133042-64-5 1-<(Fluorosulfonyl)oxy>naphthalene 
• 14930-22-4 bis(perfluoroethyl)sulfone 
• 335-05-7 Trifluoromethanesulfonyl fluoride 
• 14856-91-8 perfluoroisopropylsulfonyl fluoride 
• 7732-18-5 water 
• 16984-48-8 fluoride 
• 14808-79-8 Sulfate 

Relevant academic research and scientific papers

Chemoselective Hydro(Chloro)pentafluorosulfanylation of Diazo Compounds with Pentafluorosulfanyl Chloride

Pentafluorosulfanyl chloride (SF5Cl) is the most prevalent reagent for the incorporation of SF5 group into organic compounds. However, the preparation of SF5Cl often relies on hazardous reagents and specialized apparatus. Herein, we described a safe and practical synthesis of a bench-stable and easy-to-handle solution of SF5Cl in n-hexane under gas-reagent-free conditions. The synthetic application of SF5Cl was demonstrated through the unprecedented reaction with diazo compounds. The chemoselective hydro- and chloropentafluorosulfanylations of α-diazo carbonyl compounds were developed in the presence of K3PO4 or copper catalyst, respectively. These reactions provide a direct and efficient access to various α-pentafluorosulfanyl carbonyl compounds of high value for potential applications.

Reductive photo-chemical separation of the hexafluorides of uranium and molybdenum

Two new techniques are described for the separation of molybdenum hexafluoride (MoF6) from uranium hexafluoride (UF6). Both separation techniques utilize the differences displayed by the hexafluorides in their ability to absorb light in the near UV region. Because UF6 absorbs light in the near UV region and MoF6 does not, this observation was used to selectively reduce UF6 to uranium pentafluoride (UF5) through irradiation with 395 nm light in the presence of a suitable reducing agent. Two reducing agents were chosen for this study: gaseous, liquid, or super-critical carbon monoxide (CO) and liquid sulfur dioxide (SO2). Since MoF6 is not reduced under the reaction conditions described here, it may be removed via distillation from the uranium-containing sample after complete reduction of UF6 to solid UF5. The molybdenum- and uranium-containing samples were measured for purity through elemental analysis using microwave plasma atomic emission spectroscopy (MP-AES). Elemental analysis showed more than 98.8 % of the Mo had been removed from the U-containing samples. Further analyses of the samples were performed by X-ray powder diffraction and IR spectroscopy.

One-pot fluorosulfurylation of Grignard reagents using sulfuryl fluoride

Herein, we report a new method for the one-pot syntheses of sulfonyl fluorides. Addition of an alkyl, aryl, or heteroaryl Grignard to a solution of sulfuryl fluoride at ambient temperature affords the desired sulfonyl fluorides in 18-78% yield. Furthermore, this method is applicable for in situ sequential reactions, whereby the Grignard reagent can be converted to the corresponding diarylsulfone, sulfonate ester, or sulfonamide in a one-pot process.

Fluorine-containing sulfonyl compound as well as intermediate, preparation method and application thereof

The invention discloses a fluorine-containing sulfonyl compound as well as an intermediate, a preparation method and application thereof. The fluorine-containing sulfonyl compound disclosed by the invention comprises positive ions and negative ions, wherein the positive ions are shown as the formula I. The fluorine-containing sulfonyl compound can react with substrates to effectively synthetize the fluorine-containing sulfonyl compound; the toxicity is low; the preparation is simple; the use is convenient; the fluorine-containing sulfonyl compound is in a solid stable state at normal temperature. In addition, the substrate applicability of the compound is extremely wide, and a phenol compound and an amine compound can be included; the fluorine-containing sulfonyl compound is a unique solidformation reagent capable of realizing the chemical conversion at present, so that important academic and application values are realized. The formula I is shown in the description.

Novel synthetic route to perfluoroallyl cyanide (PFACN) reacting perfluoroallyl fluorosulfonate with cyanide

A novel synthetic method for the preparation of perfluoroallyl cyanide CF2[dbnd]CFCF2CN (PFACN) is presented. This includes the addition – elimination reaction of cyanide anion with perfluoroallyl fluorosulfate CF2[dbnd]CF

Merging [2+2] Cycloaddition with Radical 1,4-Addition: Metal-Free Access to Functionalized Cyclobuta[a]naphthalen-4-ols

A metal-free [2+2] cycloaddition and 1,4-addition sequence induced by S-centered radicals has been achieved by treating benzene-linked allene-ynes with aryldiazonium tetrafluoroborates and DABCO-bis(sulfur dioxide) in a one-pot procedure. The reaction provides a greener and more practical access to functionalized cyclobuta[a]naphthalen-4-ols with valuable applications. More than 50 examples are demonstrated with excellent diastereoselectivity and chemical yields. The reaction pathway is proposed to proceed by the following steps:[2+2] cycloaddition, insertion of SO2, 1,4-addition, diazotization, and tautomerization.

Ex situ generation of sulfuryl fluoride for the synthesis of aryl fluorosulfates

A convenient transformation of phenols into the corresponding aryl fluorosulfates is presented: the first protocol to completely circumvent direct handling of gaseous sulfuryl fluoride (SO2F2). The proposed method employs 1,1'-sulfonyldiimidazole as a precursor to generate near-stoichiometric amounts of SO2F2 gas using a two-chamber reactor. With NMR studies, it was shown that this ex situ gas evolution is extremely rapid, and a variety of phenols and hydroxylated heteroarenes were fluorosulfated in good to excellent yields.

Multidimensional SuFEx Click Chemistry: Sequential Sulfur(VI) Fluoride Exchange Connections of Diverse Modules Launched From An SOF4 Hub

Sulfur(VI) fluoride exchange (SuFEx) is a new family of click chemistry based transformations that enable the synthesis of covalently linked modules via SVI hubs. Here we report thionyl tetrafluoride (SOF4) as the first multidimensional SuFEx connector. SOF4 sits between the commercially mass-produced gases SF6 and SO2F2, and like them, is readily synthesized on scale. Under SuFEx catalysis conditions, SOF4 reliably seeks out primary amino groups [R-NH2] and becomes permanently anchored via a tetrahedral iminosulfur(VI) link: R?N=(O=)S(F)2. The pendant, prochiral difluoride groups R?N=(O=)SF2, in turn, offer two further SuFExable handles, which can be sequentially exchanged to create 3-dimensional covalent departure vectors from the tetrahedral sulfur(VI) hub.

Ion chemistry of sulfuryl fluoride: An experimental and theoretical study on gas-phase reactions involving neutral and ionized SO2F2

The gas phase ion chemistry of sulfuryl fluoride is studied by ion trap mass spectrometry and ab initio calculations. Reactions of ions of atmospheric relevance with neutral SO2F2 mainly result in SO 2F2 depletion by dissociative electron transfer. In few cases, a different reaction mechanism involving F-abstraction is invoked, since dissociative ion products are observed despite the electron transfer channel being endothermic. Ab initio calculations revealed a nearly perfect distonic structure for the molecular SO2F2+ ion, whose capability of activating strong HX bonds (X = C, N, O) is ascribable to the high spin density located on the oxygen atoms, in line with literature reports. Among the ions produced by electron ionization of SO2F2, the FSOx+ (x = 0-2) ions are capable of activating the HNH2 bond of ammonia. Theoretical investigation revealed that NH 3 activation by SF+ requires a triplet to singlet conversion along the reaction pathway. This conversion is expected to be fast, the conceivable reaction rate determining step being the subsequent intramolecular hydrogen migration.

Thermally persistent fluorosulfonyl nitrene and unexpected formation of the fluorosulfonyl radical

Thermally persistent triplet sulfonyl nitrene, FSO2N, was produced in the gas phase in high yields (up to 66%) by flash vacuum pyrolysis of FSO2N3. Surprisingly, no rearrangement of FSO 2N was observed, but the