Oxygen difluoride

Base Information

• Chemical Name: Oxygen difluoride
• CAS No.: 7783-41-7
• Molecular Formula: F2O
• Molecular Weight: 53.9962
• European Community (EC) Number: 231-996-7
• ICSC Number: 0818
• UN Number: 2190
• UNII: 7BCS2CW398
• DSSTox Substance ID: DTXSID20894009
• Nikkaji Number: J65.723I
• Wikipedia: Oxygen difluoride
• Wikidata: Q411301
• Mol file: 7783-41-7.mol

Synonyms:fluorine monoxide;oxyfluoride

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Chemical Property of Oxygen difluoride

Chemical Property:

• Melting Point: -223.8oC
• Boiling Point: °Cat760mmHg
• Flash Point: °C
• PSA: 9.23000
• Density: 1.179g/cm³
• LogP: 0.77200
• Water Solubility.: 6.8mL gas/100mL H2O (0°C) [MER06]
• XLogP3: 1.2
• Hydrogen Bond Donor Count: 0
• Hydrogen Bond Acceptor Count: 3
• Rotatable Bond Count: 0
• Exact Mass: 53.99172094
• Heavy Atom Count: 3
• Complexity: 2.8
• Transport DOT Label: Poison Gas Oxidizer Corrosive

Purity/Quality:

Safty Information:

• Pictogram(s): Explodes on contact with water, air, and reducing agents. Corrosive to tissue. TLV: ceiling 0.05 ppm.
• Hazard Codes: Explodes on contact with water, air, and reducing agents. Corrosive to tissue. TLV: ceiling 0.05 ppm.

MSDS Files:

SDS file from LookChem

Total 1 MSDS from other Authors

Useful:

• Chemical Classes: Toxic Gases & Vapors -> Oxidizers
• Canonical SMILES: O(F)F
• Inhalation Risk: A harmful concentration of this gas in the air will be reached very quickly on loss of containment.
• Effects of Short Term Exposure: Lachrymation. The substance is irritating to the respiratory tract. Inhalation of this gas may cause lung oedema. Exposure slightly above the OEL could cause death.
• Physical properties: Colorless gas with a characteristic odor; unstable in the presence of moisture, otherwise stable up to 250°C; gas density 2.21g/L at 25°C; liquefies to a yellowish-brown liquid at -144.8°C; density of the liquid 1.90g/ml at -223.8°C; solidifies at -223.8°C; slightly soluble in water, decomposing very slowly; solubility 68ml gas per liter of water at 0°C; slightly soluble in acids and alkali.
• Uses: Commercial applications of oxygen difluoride are limited. It is used in organic synthesis to prepare fluoropropylenes and acylfluorides. It is used as an oxidizing and fluorinating agent in many preparative reactions and as a monomer in diolefin copolymerization. Oxidant in missile propellant systems

Technology Process of Oxygen difluoride

There total 45 articles about Oxygen difluoride which guide to synthetic route it. The literature collected by LookChem mainly comes from the sharing of users and the free literature resources found by Internet computing technology. We keep the original model of the professional version of literature to make it easier and faster for users to retrieve and use. At the same time, we analyze and calculate the most feasible synthesis route with the highest yield for your reference as below:

synthetic route:

Reference yield: 58.0%

perchloric acid (7601-90-3) + fluorine (7782-41-4) → difluoroether (7783-41-7)

Guidance literature:

In neat (no solvent); byproducts: O2; dropwise addn. of a concd. soln. of HClO4 to a column filled with graphite under countercurrent of F2;;

DOI:10.1021/ja01195a063

Reference yield: 45.0%

fluorine (7782-41-4) + sodium hydroxide (1310-73-2) → difluoroether (7783-41-7)

Guidance literature:

In sodium hydroxide; byproducts: O2; aq. NaOH; F2 is passed through a Pt-tube in a 2% aq. NaOH (1-2 l/h);; washing with H2O; condensation by liq. O2; fractional distn.; 98.5% purity (one time distn.);;

Reference yield: 45.0%

fluorine (7782-41-4) + sodium hydroxide (1310-73-2) → difluoroether (7783-41-7) + sodium fluoride (7681-49-4)

Guidance literature:

In sodium hydroxide; byproducts: H2O; F2 is passed through tube of Pt into a 2% aq. soln. of NaOH;; washing with water; condensation with liq. air; fractional distn.;;

upstream raw materials:

fluorine

water

hydrogen fluoride

sodium hydroxide

Downstream raw materials:

nitrogen

cesium fluoride

dinitrogen monoxide

fluorosulfonyl fluoride

Refernces

Reaction of oxygen difluoride with sulfur dioxide, sulfur trioxide, and peroxydisulfuryl difluoride

10.1021/ic50016a044

The main content of the study revolves around the chemical reactions involving various nitrides and oxygen difluoride (O2F2). The research explores the fluorination of different types of nitrides, such as lithium nitride (Li3N), beryllium nitride (Be3N2), magnesium nitride (Mg3N2), boron nitride (BN), silicon nitride (Si3N4), titanium nitride (TiN), vanadium nitride (VN), and copper(I) nitride, using elementary fluorine. The aim is to establish if there is a relationship between the structure of a nitride and the formation of nitrogen trifluoride (NF3) as a product of its direct fluorination. Additionally, the study investigates the reaction of oxygen difluoride with sulfur dioxide, sulfur trioxide, and peroxydisulfuryl difluoride, focusing on the photochemical decomposition and the role of 0-F radical species as reaction intermediates. The experiments involve irradiating gaseous mixtures with ultraviolet light to observe the reactions and identify the products, which include peroxysulfuryl difluoride, pyrosulfuryl fluoride, sulfuryl fluoride, and fluorine fluorosulfonate, among others. The study employs various analytical techniques such as infrared and F19 n.m.r. spectroscopy to characterize the compounds formed.