It is an extremely strong oxidant and decomposes into oxygen and fluorine even at −160 °C (113 K) at a rate of 4% per day: its lifetime at room temperature is thus extremely short. It reacted instantaneously with solid ethyl alcohol, producing a blue flame and an explosion. idlewords on Feb 25, 2010 Neither of those chemicals is particularly dense, and as a bonus HS is incredibly poisonous. No comments. Dioxygen difluoride can be obtained by subjecting a 1:1 mixture of gaseous fluorine and oxygen at low pressure (7–17 mmHg (0.9–2.3 kPa) is optimal) to an electric discharge of 25–30 mA at 2.1–2.4 kV. Viewing. Acronym Definition; FOOF: Dioxygen Difluoride (chemical compound): FOOF: Friends of the Oakland Fox (est. German manufacturers “Huettinger” demonstrate non-contact heating with a cube of ice in this video. It is an extremely strong oxidant and decomposes into oxygen and fluorine even at −160 °C (113 K) at a rate of 4% per day: its lifetime at room temperature is thus extremely short. Full Record; Other Related Research; Authors: Streng, L.V. And, and before you get any funny ideas, yes . [4] All of these methods involve synthesis according to the equation, It also arises from the thermal decomposition of ozone difluoride:[5]. noun. The crazy bastard that did said experiment also applied Dioxygen Difloride with the above Chlorine Trifloride, something the writer for the article could only respond with " say what ?" This geometry conforms with the predictions of VSEPR theory. • Some compounds are so unpleasant it would be better if they had names like ‘reconsideric acid’ or ‘notworthite’. FOOF Chemical/Physical Characteristics A.G. Steng of Temp University Hey! Rev., 1963, 63, p. 610]. Structural aspects of the fluorides of xenon: Structure of XeF 2: Logged Halleyscomet. Publication Date: Tue Feb 01 00:00:00 EST 1966 Research Org. Neptunium dioxide and tetrafluoride are converted in essentially quantitative yield to volatile neptunium hexafluoride by dioxygen difluoride (O 2 F 2), both in gas–solid reactions at ambient temperatures and in liquid anhydrous hydrogen fluoride at −78°C.Neptunium dioxydifluoride was identified by Raman spectroscopy as a dominant reaction intermediate in the neptunium dioxide … Mixtures with carbon monoxide, with hydrogen, or with methane explode on sparking [Streng, A. G., Chem. PHOTOCHEMICAL FORMATION OF KRYPTON DIFLUORIDE FROM KRYPTON AND FLUORINE OR OXYGEN DIFLUORIDE. Some of the compounds that produced violent reactions with O2F2 include ethyl alcohol, methane, ammonia, and even water ice. [9] Several experiments with the compound resulted in a series of fires and explosions. Dioxygen Difluoride » Videos. Another way to prevent getting this page in the future is to use Privacy Pass. Vote count: 0. FOOF Chemical/Physical Characteristics A.G. Steng of Temp University Hey! However, in the presence of UV radiation the products are sulfuryl fluoride, SO 2 F 2, and pyrosulfuryl fluoride, S 2 O 5 F 2: OF 2 + 2 SO 2 → S 2 O 5 F 2 When a drop of liquid 02F2 was added to liquid methane, cooled at 90°K., a white flame was produced instantaneously, which turned green upon … Full Record; Other Related Research; Authors: Streng, L V; Streng, A G Publication Date: Tue Feb 01 00:00:00 EST 1966 Research Org. Travel Videos; Drawing Videos; Menu The compound readily decomposes into oxygen and fluorine. Preparation. [7], The 19F NMR chemical shift of dioxygen difluoride is 865 ppm, which is by far the highest chemical shift recorded for a fluorine nucleus, thus underlining the extraordinary electronic properties of this compound. idlewords on Feb 25, 2010 Neither of those chemicals is particularly dense, and as a bonus HS is incredibly poisonous. [1] It is a strong oxidant and decomposes into OF 2 and oxygen even at −160 °C (4% per day) - it thus can not exist at room temperature. Not only did Streng prepare multiple batches of dioxygen difluoride and keep it around, he was apparently charged with … Submit Rating . Birb Aug 11, 2017 @ 8:23pm it is pretty good. Textbook solution for Chemistry & Chemical Reactivity 9th Edition John C. Kotz Chapter 2.8 Problem 1RC. I don't know how effective this chemical would be for your stated purpose, however, it is nasty enough that I want to mention it and you deserve to know about it. If you are on a personal connection, like at home, you can run an anti-virus scan on your device to make sure it is not infected with malware. It is an extremely strong oxidant and decomposes into oxygen and fluorine even at −160 °C (113 K) at a rate of 4% per day: its lifetime at room temperature is thus extremely short. [11], Except where otherwise noted, data are given for materials in their, covalent bonding in the fluorine molecule, Zeitschrift für anorganische und allgemeine Chemie, "Direct synthesis of liquid-phase dioxygen difluoride", "Thermodynamic Properties of Dioxygen Difluoride (O, "Things I Won't Work With: Dioxygen Difluoride", https://en.wikipedia.org/w/index.php?title=Dioxygen_difluoride&oldid=994067573, Pages using collapsible list with both background and text-align in titlestyle, Articles containing unverified chemical infoboxes, Creative Commons Attribution-ShareAlike License, This page was last edited on 13 December 2020, at 23:12. It is also nicknamed as FOOF as it is formed by the mixture of 1:1 fluorine and oxygen at low pressure. You may need to download version 2.0 now from the Chrome Web Store. * Do not eat, smoke, or drink where Oxygen Difluoride is handled, processed, or stored, since the chemical can be Dioxygen difluoride, O 2 F 2, is a yellow-orange solid melting at −163 °C.It is prepared by the reaction of O 2 and F 2 mixtures under glow discharge at −180 to −190 °C. This, folks, is the bracingly direct route to preparing dioxygen difluoride, often referred to in the literature by its evocative formula of FOOF. Dioxygen difluoride can be obtained by subjecting a 1:1 mixture of gaseous fluorine and oxygen at low pressure (7-17 mmgHg is optimal) [citation needed] to an electric discharge of 25-30 mA at 2.1-2.4 kV.This is basically the reaction used for the first synthesis by Otto Ruff in 1933. [3] Another synthesis involves mixing O2 and F2 in a stainless steel vessel cooled to −196 °C (77.1 K), followed by exposing the elements to 3 MeV bremsstrahlung for several hours. … Dioxygen difluoride is a compound of fluorine and oxygen with the molecular formula O2F2. The binary compound of oxygen and fluorine OF; it is explosive. Oxygen fluoride and more now FROM the Chrome web Store Univ., … OSTI.GOV Journal:. Similar method was used for the long and weak covalent bonding in sense! A cube of ice in this video. [ 8 ] FOOF as it is explosive funny,! Even at temperatures close to its melting point in bond FORMATION, as well as the ones that not.: FOOF: Friends of the containers to high heat may result in violent! And vapors 11:26pm @ Phoenix Thanks ru ; DE ; FR ; ES ; Remember this site dioxygen,. Collectively known as valence electrons a third method requires heating a mi… dioxygen difluoride Hydrogen... 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