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Oxygen difluoride. A common preparative method involves fluorination of sodium hydroxide: 2 F 2 + 2 NaOH → OF 2 + 2 NaF + H 2 O. OF 2 is a colorless gas at room temperature and a yellow liquid below 128 K. Oxygen difluoride has an irritating odor and is poisonous. [3] It reacts quantitatively with aqueous haloacids to give free halogens:
Oxygen difluoride was first reported in 1929; it was obtained by the electrolysis of molten potassium fluoride and hydrofluoric acid containing small quantities of water. [7] [8] The modern preparation entails the reaction of fluorine with a dilute aqueous solution of sodium hydroxide, with sodium fluoride as a side-product:
Compounds containing oxygen in other oxidation states are very uncommon: − 1 ⁄ 2 (superoxides), − 1 ⁄ 3 , 0 (elemental, hypofluorous acid), + 1 ⁄ 2 , +1 (dioxygen difluoride), and +2 (oxygen difluoride). Oxygen is reactive and will form oxides with all other elements except the noble gases helium, neon, argon and krypton. [1]
In 1935, professor George H. Cady was first to synthesize fluorine nitrate and has since maintained a long and controversial history. In 1937, American chemist and biochemist Linus Pauling and one of his first graduate students, Lawrence O. Brockway, utilized electron diffraction intensities to determine the structure of the oxygen and fluorine bond perpendicular to the NO2 plane to be a non ...
The bond energy is significantly weaker than those of Cl 2 or Br 2 molecules and similar to the easily cleaved oxygen–oxygen bonds of peroxides or nitrogen–nitrogen bonds of hydrazines. [8] The covalent radius of fluorine of about 71 picometers found in F 2 molecules is significantly larger than that in other compounds because of this weak ...
The oxygen (0) atom is the root of hypofluorous acid's strength as an oxidizer, in contrast to the halogen (+1) atom in other hypohalic acids. This alters the acid's chemistry. Where reduction of a general hypohalous acid reduces the halogen atom and yields the corresponding elemental halogen gas, 2 HOX + 2 H + + 2 e − → 2 H 2 O + X 2
Dioxygenyl hexafluoroplatinate can be synthesized from the elements by the action of a mixture of oxygen and fluorine gas on platinum sponge at 450 °C. [1] It can also be prepared by the reaction of oxygen difluoride (OF 2) with platinum sponge. At 350 °C, platinum tetrafluoride is produced; above 400 °C, dioxygenyl hexafluoroplatinate is ...
The Birkeland–Eyde process was one of the competing industrial processes in the beginning of nitrogen-based fertilizer production. It is a multi-step nitrogen fixation reaction that uses electrical arcs to react atmospheric nitrogen (N 2) with oxygen (O 2), ultimately producing nitric acid (HNO 3) with water. [1]