Chemical Formula For Oxygen Difluoride
Oxygen fluorides are compounds of elements oxygen and fluorine with the general formula O n F2 , where n = 1 to half-dozen. Many different oxygen fluorides are known:
- oxygen difluoride (OF2 )
- dioxygen difluoride (O2Ftwo )
- trioxygen difluoride or ozone difluoride (O3Fii )[1] [2]
- tetraoxygen difluoride (O4F2 )[3]
- pentaoxygen difluoride (O5F2 )
- hexaoxygen difluoride (O6Ftwo )[4]
- dioxygen monofluoride or fluoroperoxyl (O2F)
Oxygen fluorides are strong oxidizing agents with high energy and can release their energy either instantaneously or at a controlled rate. Thus, these compounds attracted much attention as potential fuels in jet propulsion systems.[5]
Synthesis [edit]
Here are some synthesis methods and reactions of the three virtually common oxygen fluorides – oxygen difluoride (OFii ), dioxygen difluoride (OiiFtwo ) and ozone difluoride (O3F2 ).
Oxygen difluoride (OF2 ) [edit]
A common preparative method involves fluorination of sodium hydroxide:
- 2 Fii + 2 NaOH → OF2 + 2 NaF + H2O
OF2 is a colorless gas at room temperature and a yellow liquid below 128 1000. Oxygen difluoride has an irritating odor and is poisonous.[three] Information technology reacts quantitatively with aqueous haloacids to requite free halogens:
- OFtwo + 4 HCl → ii Cl2 + 2 HF + two H2O
It tin can too readapt halogens from their salts.[3] It is both an constructive fluorinating agent and a strong oxidizing agent. When reacted with unsaturated nitrogen fluorides with electrical discharge, it results in the formation of nitrogen trifluoride, oxide fluorides and other oxides.[6] [7]
Dioxygen difluoride (O2F2 ) [edit]
O2F2 precipitates equally a dark-brown solid upon the UV irradiation of a mixture of liquid O2 and F2 at −196 °C.[viii] It also only appears to be stable below −160 °C.[9] The general method of preparation of many oxygen fluorides is a gas-phase electric discharge in cold containers including OiiF2 .[ten]
- O2 + Fii → O2Ftwo (electric discharge, 183 °C)
Information technology is typically an orange-yellow solid which rapidly decomposes to Oii and F2 close to its normal boiling signal of nigh 216 K.[3]
O2F2 reacts violently with cerise phosphorus, even at −196 °C. Explosions can too occur if Freon-xiii is used to moderate the reaction.[nine]
Trioxygen difluoride or ozone difluoride (OthreeFii ) [edit]
O3F2 is a sticky, blood-ruby-red liquid. Information technology remains liquid at 90 One thousand and then can be differentiated from O2F2 which has a melting point of about 109 K.[11] [3]
Like the other oxygen fluorides, OiiiFii is endothermic and decomposes at about 115 K with the evolution of heat, which is given by the following reaction:
- 2 O3Ftwo → O2 + two OiiFii
OiiiFii is safer to work with than ozone, and can be evaporated, or thermally decomposed, or exposed to electric sparks, without any explosions. But on contact with organic matter or oxidizable compounds, information technology can detonate or explode. Thus, the improver of even 1 drop of ozone difluoride to solid anhydrous ammonia will result in a balmy explosion, when they are both at xc Grand each.[3]
Fluoroperoxyl [edit]
Fluoroperoxyl is a molecule such as O–O–F, whose chemic formula is O2F and is stable only at low temperature. It has been reported to be produced from atomic fluorine and dioxygen.[12]
- O2 + F → OiiF
General preparation of polyoxygen difluorides [edit]
| Reaction equation [6] | O2 :Ftwo by volume | Current | Temperature of bathroom (°C) |
|---|---|---|---|
| Otwo + F2 ⇌ O2F2 | 1:i | 10 – 50 mA | ~ -196° |
| 3 Oii + 2 F2 ⇌ 2 OthreeF2 | iii:two | 25 – 30 mA | ~ -196° |
| 2 O2 + F2 ⇌ O4Fii | 2:1 | iv – 5 mA | ~ -205° |
Effects on ozone [edit]
Oxygen- and fluorine-containing radicals similar O2F and OF occur in the temper. These forth with other element of group vii radicals have been implicated in the destruction of ozone in the atmosphere. However, the oxygen monofluoride radicals are assumed to not play as large a office in the ozone depletion considering gratis fluorine atoms in the atmosphere are believed to react with marsh gas to produce hydrofluoric acid which precipitates in pelting. This decreases the availability of gratis fluorine atoms for oxygen atoms to react with and destroy ozone molecules.[13]
- O3 + F → O2 + OF
- O + OF → O2 + F
Cyberspace reaction:
- Oiii + O → ii Otwo
Hypergolic propellant [edit]
Despite the depression solubility of O3Ftwo in liquid oxygen, it has been shown to be hypergolic with about rocket propellant fuels. The machinery involves the humid off oxygen from the solution containing OthreeFii , making information technology more reactive to have a spontaneous reaction with the rocket fuel. The degree of reactivity is besides dependent on the type of fuel used.[3]
Meet also [edit]
- Bromine oxide
- Chlorine oxide
- Iodine oxide
- Ozone
References [edit]
- ^ Solomon, I. J. et al. (1968). "Boosted Studies Concerning the Beingness of OiiiFtwo". Journal of the American Chemical Guild. ninety (20): 5408–5411. doi:x.1021/ja01022a014.
{{cite journal}}: CS1 maint: uses authors parameter (link) - ^ Misochko, Eugenii Ya, Alexander V. Akimov, Charles A. Wight (1999). "Infrared spectroscopic observation of the stabilized Intermediate circuitous FOthree formed by reaction of mobile Fluorine atoms with ozone molecules Trapped in an Argon Matrix". The Journal of Concrete Chemistry A. 103 (40): 7972–7977. Bibcode:1999JPCA..103.7972M. doi:10.1021/jp9921194.
{{cite journal}}: CS1 maint: uses authors parameter (link) - ^ a b c d e f g Streng, A. G. (1963). "The Oxygen Fluorides". Chemical Reviews. 63 (6): 607–624. doi:10.1021/cr60226a003.
- ^ Streng, A. G., A. V. Grosse (1966). "2 New Fluorides of Oxygen, O5F2 and OviF2". Journal of the American Chemical Society. 88: 169–170. doi:ten.1021/ja00953a035.
{{cite journal}}: CS1 maint: uses authors parameter (link) - ^ Jäger, Susanne et al. (1986). "Fluorine and Oxygen". Fluorine. Berlin, Heidelberg: Springer. pp. i–161.
{{cite book}}: CS1 maint: uses authors parameter (link) - ^ a b Nikitin, Igor Vasil'evich, and V. Ya Rosolovskii (1971). "Oxygen Fluorides and Dioxygenyl Compounds". Russian Chemical Reviews. 40 (11): 889–900. Bibcode:1971RuCRv..twoscore..889N. doi:10.1070/rc1971v040n11abeh001981. S2CID 250903149.
{{cite journal}}: CS1 maint: uses authors parameter (link) - ^ Lawless, Edward W., Ivan C. Smith (1968). Inorganic high-free energy oxidizers: synthesis, structure, and properties. One thousand. Dekker.
{{cite book}}: CS1 maint: uses authors parameter (link) - ^ Marx, Rupert, Konrad Seppelt (2015). "Structure investigations on oxygen fluorides". Dalton Transactions. 44 (45): 19659–19662. doi:10.1039/c5dt02247a. PMID 26351980.
{{cite journal}}: CS1 maint: uses authors parameter (link) - ^ a b Solomon, Irvine J. Research on Chemical science of O3F2 and O2F2 . No. IITRI-C227-six. IIT RESEARCH INST CHICAGO IL, 1964.
- ^ Goetschel, Charles T. et al. (1969). "Low-Temperature Radiation Chemistry. I. Training of Oxygen Fluorides and Dioxygenyl Tetrafluoroborate". Periodical of the American Chemic Social club. 91 (17): 4702–4707. doi:10.1021/ja01045a020.
{{cite journal}}: CS1 maint: uses authors parameter (link) - ^ De Marco, Ronald A., and Jean'ne M. Shreeve . "Fluorinated Peroxides." Advances in Inorganic Chemical science and Radiochemistry. Vol. 16. Bookish Press, 1974. 109-176.
- ^ J.Fifty.Lyman and R. Holland, J. Phys. Chem.,1988,92, 7232.
- ^ Francisco J. Due south. (1993). "An ab initio investigation of the significance of the HOOF intermediate in coupling reactions involving FOO x and HO x species". The Journal of Chemic Physics. 98 (iii): 2198–2207. Bibcode:1993JChPh..98.2198F. doi:10.1063/1.464199.
External links [edit]
- National Pollutant Inventory - Fluoride and compounds fact sheet
- Oxygen Fluoride PubChem
- Center for Disease Control and Prevention - Health Hazards of Oxygen Difluoride
Chemical Formula For Oxygen Difluoride,
Source: https://en.wikipedia.org/wiki/Oxygen_fluoride
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