13709-32-5

Basic information

• Product Name: PEROXYDISULFURYL DIFLUORIDE
• CAS NO: 13709-32-5
• Molecular Formula: F₂O₆S₂
• Molecular Weight: 198.125
• Mol File: 13709-32-5.mol
• Article Data: 10

Chemical Properties

• CAS DataBase Reference: PEROXYDISULFURYL DIFLUORIDE (CAS DataBase Reference)
• NIST Chemistry Reference: PEROXYDISULFURYL DIFLUORIDE (13709-32-5)
• EPA Substance Registry System: PEROXYDISULFURYL DIFLUORIDE (13709-32-5)

Safety Data

• Safety Statements: A powerful irritant and corrosive to skin, eyes, and mucous membranes. A very powerful oxidizer. A dangerous fire hazard. Ignites organic materials immediately on contact. Explosive reaction with carbon monoxide; dichloromethane. Violent reaction with boron nitride. When heated to decomposition it emits very toxic fumes of Fsup xmlns="">−/sup> and SOsub xmlns="">x/sub>. See also a target="_blank" href="lom/card_sa.tes?href=content/sax0021/sdp20097.xml&view=print">PEROXIDES, INORGANIC/a>; a target="_blank" href="lom/card_sa.tes?href=content/sax0021/sdp20098.xml&view=print">PEROXIDES, ORGANIC/a> and a target="_blank" href="lom/card_sa.tes?href=content/sax0013/sdp12465.xml&view=print">FLUORIDES/a>.
• Hazardous Substances Data: 13709-32-5(Hazardous Substances Data)

Usage

General Description

PEROXYDISULFURYL DIFLUORIDE is a chemical compound with the formula S2O6F2. It is a colorless, gas with a pungent odor and is highly reactive. It is primarily used as a fluorinating agent in organic synthesis, as well as a strong oxidizing and chlorinating agent. PEROXYDISULFURYL DIFLUORIDE is also used as a reagent in the preparation of various compounds, and as a source of fluorine in various chemical reactions. However, due to its highly reactive and hazardous nature, it requires careful handling and storage, and can pose significant health and environmental risks if not properly managed.

Upstream product

• 13536-85-1 fluorosulfuryl hypofluorite 
• 7446-09-5 sulfur dioxide 
• 7783-44-0 dioxygen difluoride 
• 7446-11-9 sulfur trioxide 
• 14884-42-5 chromium pentafluoride 
• 7783-81-5 uranium hexafluoride 
• 7782-41-4 fluorine 
• 13455-22-6 potassium fluorosulfonate 
• 7783-42-8 thionyl fluoride 
• 13709-36-9 xenon difluoride 
• 7446-11-9 sulfur trioxide 
• 7789-21-1 fluorosulphonic acid 
• 13771-24-9 O9S3, γ 

Downstream Products

• 13709-33-6 trisulfuryl fluoride 
• 65776-46-7 VO(SO₃F)3 
• 7782-50-5 chlorine 
• 14546-48-6 manganese(III) ion 
• 7446-08-4 selenium(IV) oxide 
• 13036-75-4 fluorosulfonyl anhydride 
• 27791-56-6 Se₈⁽²⁺⁾ 
• 44125-19-1 SeO₃F^(1-) 
• 372-64-5 Bis(trifluoromethyl)disulfid 
• 7446-09-5 sulfur dioxide 
• 7704-34-9 sulfur 
• 21690-87-9 bis(trifluorothioacetyl) disulfide 
• 5762-53-8 trifluoroacetyl fluosulfate 
• 7789-21-1 fluorosulphonic acid 

Relevant articles and documents

Synthesis and characterization of uranium(V) fluoride fluorosulfates and uranium(V) oxyfluorosulfate: UF3(SO3F)2, UF(SO3F)4, and UO(SO3F)3

The new uranium(V) fluoride fluorosulfate compounds UF3(SO3F)2 and UF(SO3F)4 and uranium(V) oxyfluorosulfate UO(SO3F)3 have been synthesized. UF3(SO3F)2, a pale green solid, resulted from the reaction of UF5 and S2O6F2 in CFCl3 at 40°C for 20 days; under these conditions the solvent also reacted and was partly transformed into CFCl2OSO2F and CF2Cl2. The beige solid UF(SO3F)4 was prepared by mixing UF6 and SO3 in CFCl3 at low temperature (3F)3, a tetragonal gray-beige solid. These three compounds were characterized by chemical analysis. Their thermal stabilities and vibrational and electronic spectra are also reported. The +5 oxidation state of uranium was confirmed by magnetic susceptibility measurements. Despite several attempts under different conditions, no uranium(VI) fluorosulfate or fluoride fluorosulfate was obtained.

Synthesis and characterization of the difluorotris(fluorosulfate) of uranium(V): UF2(SO3F)3

A new U(V) compound, UF2(SO3F)3, has been synthesized by the reaction of UF6 and SO3 in both the gaseous phase and CFCl3 solution. This leads to a blue-green solid, the x-ray powder diffraction pattern of which has been recorded. Its oxidation state has been deduced from chemical analysis, the electronic absorption spectrum, and magnetic measurements. The environment around uranium is discussed from Raman and infrared spectra recorded at ambient and liquid nitrogen temperatures.

METHODS OF MAKING HALOGENATED FLUORINATED ETHER-CONTAINING COMPOUNDS

Described herein are three methods for making halogenated fluorinated ether-containing compounds using a fluorinated olefin or hexafluoropropylene oxide.

Cationic carbonyl complexes of rhodium(I) and rhodium(III): Syntheses, vibrational spectra, NMR studies, and molecular structures of tetrakis(carbonyl)rhodium(I) heptachlorodialuminate and -gallate, [Rh(CO)4][Al2Cl7] and [Rh(CO)4][Ga2Cl7]

Dimeric rhodium(I) bis(carbonyl) chloride, [Rh(CO)2(μ-Cl)]2, is found to be a useful and convenient starting material for the syntheses of new cationic carbonyl complexes of both rhodium(I) and rhodium(III). Its reaction with the Lewis acids AlCl3 or GaCl3 produces in a CO atmosphere at room temperature the salts [Rh(CO)4][M2Cl7] (M = Al, Ga), which are characterized by Raman spectroscopy and single-crystal X-ray diffraction. Crystal data for [Rh(CO)4][Al2Cl7]: triclinic, space group P1 (No. 2); a = 9.705(3), b = 9.800(2), c = 10.268(2) A; α = 76.52(2), β = 76.05(2), γ = 66.15(2)°; V = 856.7(5) A3; Z = 2; T = 293 K; R1 [I > 2σ(I)] = 0.0524, wR2 = 0.1586. Crystal data for [Rh(CO)4][Ga2Cl7]: triclinic, space group P1 (No. 2); a = 9.649(1), b = 9.624(1), c = 10.133(1) A; α = 77.38(1), β = 76.13(1), γ = 65.61(1)°; V = 824.4(2) A3; Z = 2; T = 143 K; R1 [I > 2σ(I)] = 0.0358, wR2 = 0.0792. Structural parameters for the square planar cation [Rh(CO)4]+ are compared to those of isoelectronic [Pd(CO)4]2+ and of [Pt(CO)4]2+. Dissolution of [Rh(CO)2Cl]2 in HSO3F in a CO atmosphere allows formation of [Rh(CO)4]+(solv). Oxidation of [Rh(CO)2Cl]2 by S2O6F2 in HSO3F results in the formation of ClOSO2F and two seemingly oligomeric RH(III) carbonyl fluorosulfato intermediates, which are easily reduced by CO addition to [Rh(CO)4]+(solv). Controlled oxidation of this solution with S2O6F2 produces fac-Rh(CO)3(SO3F)3 in about 95% yield. This RH(III) complex can be reduced by CO at 25 °C in anhydrous HF to give [Rh(CO)4]+(solv); addition of SbF5 at -40 °C to the resulting solution allows isolation of [Rh(CO)4][Sb2F11]2, which is found to have a highly symmetrical (D4h) [Sb2F11]- anion. Oxidation of [Rh(CO)2Cl]2 in anhydrous HF by F2, followed in a second step by carbonylation in the presence of SbF5, is found to be a simple, straightforward route to pure [Rh(CO)5Cl][Sb2F11]2, which has previously been structurally characterized by us. All new complexes are characterized by vibrational and NMR spectroscopy. Assignment of the vibrational spectra and interpretation of the structural data are supported by DFT calculations.