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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]
3) while the higher chlorides of uranium are prepared by reaction with additional chlorine. [6] 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 ...
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]
Electrochemical fluorination ("electrofluorination") was announced, which Joseph H. Simons had developed in the 1930s to generate highly stable perfluorinated materials compatible with uranium hexafluoride. [15] These new methodologies allowed the synthesis of C-F bonds without using elemental fluorine and without relying on metathetical methods.
Uranyl nitrate can be prepared by reaction of uranium salts with nitric acid. It is soluble in water, ethanol, and acetone. As determined by neutron diffraction, the uranyl center is characteristically linear with short U=O distances. In the equatorial plane of the complex are six U-O bonds to bidentate nitrate and two water ligands.
It is most notable as a contaminant in the production of uranium tetrafluoride. [1] As shown by X-ray crystallography, the uranyl (UO 2 2+) centers are complemented by six fluoride ligands. [2] This salt is very soluble in water as well as hygroscopic. It is formed in the hydrolysis of uranium hexafluoride (UF 6): UF 6 + 2 H 2 O → UO 2 F 2 + 4 HF
Pentavalent uranyl complexes are obtained by the oxidation of U IV or other low-valent uranium compounds and these reactions are done under oxygen-free conditions in organic solvents. The oxidation of U III and U IV precursors under non-aqueous conditions or controlled hydrolysis conditions gives large polyoxo uranium clusters containing U V. [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.