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UF 6 reacts with water, releasing hydrofluoric acid. The compound reacts with aluminium, forming a surface layer of AlF 3 that resists any further reaction from the compound. Uranium hexafluoride is a mild oxidant. [10] It is a Lewis acid as evidenced by its binding to form heptafluorouranate(VI), [UF 7] −. [11]
All uranium chlorides react with water and air. Bromides and iodides of uranium are formed by direct reaction of, respectively, bromine and iodine with uranium or by adding UH 3 to those element's acids. [6] Known examples include: UBr 3, UBr 4, UI 3, and UI 4. UI 5 has never been prepared. Uranium oxyhalides are water-soluble and include UO 2 ...
Uranium tetrafluoride is the inorganic compound with the formula UF 4. It is a green solid with an insignificant vapor pressure and low solubility in water . Uranium in its tetravalent ( uranous ) state is important in various technological processes.
Uranium hexafluoride is used in the uranium enrichment process to produce fuel for nuclear reactors. Fluoride volatility can also be exploited for nuclear fuel reprocessing . Tungsten hexafluoride is used in the production of semiconductors through the process of chemical vapor deposition .
The noble metals ruthenium, rhodium, palladium, platinum, and gold react least readily, requiring pure fluorine gas at 300–450 °C (575–850 °F). [14] Fluorine reacts explosively with hydrogen in a manner similar to that of alkali metals. [15] The halogens react readily with fluorine gas [16] as does the heavy noble gas radon. [17]
It is an oxidant [10] and a Lewis acid which is able to bind to fluoride, for instance the reaction of copper(II) fluoride with uranium hexafluoride in acetonitrile is reported to form copper(II) heptafluorouranate(VI), Cu(UF 7) 2. [11] It reacts with water to form a solid compound, and is very difficult to handle on an industrial scale. [6]
In nuclear physics, a nuclear chain reaction occurs when one single nuclear reaction causes an average of one or more subsequent nuclear reactions, thus leading to the possibility of a self-propagating series or "positive feedback loop" of these reactions. The specific nuclear reaction may be the fission of heavy isotopes (e.g., uranium-235 ...
The usual method of preparation is by fluorination of neptunium(IV) fluoride (NpF 4) by elemental fluorine (F 2) at 500 °C. [6]NpF 4 + F 2 → NpF 6. In comparison, uranium hexafluoride (UF 6) is formed relatively rapidly from uranium tetrafluoride (UF 4) and F 2 at 300 °C, while plutonium hexafluoride (PuF 6) only begins forming from plutonium tetrafluoride (PuF 4) and F 2 at 750 °C. [6]