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{{Expand German|Uran(VI)-fluorid|date=November 2012}} |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid [{{fullurl:Uranium_hexafluoride|oldid=472671585}} 472671585] of page [[Uranium_hexafluoride]] with values updated to verified values.}} |
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{{Chembox |
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|Watchedfields = changed |
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| verifiedrevid = 470619869 |
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|verifiedrevid = 476998888 |
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| Name = Uranium Hexafluoride |
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|Name = Uranium hexafluoride |
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|ImageFile = Uranium-hexafluoride-2D-V2.svg |
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|ImageSize = 144px |
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|ImageFile1 = Uranium-hexafluoride-3D-vdW.png |
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|ImageSize1 = 150px |
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| Section1 = {{Chembox Identifiers |
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|ImageFile2 = Uranium-hexafluoride-crystal-3D-vdW.png |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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|ImageSize2 = 150px |
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| ChemSpiderID = 22966 |
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|IUPACName = Uranium hexafluoride<br>Uranium(VI) fluoride |
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| PubChem = 24560 |
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|Section1={{Chembox Identifiers |
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| InChI = 1/6FH.U/h6*1H;/q;;;;;;+6/p-6/rF6U/c1-7(2,3,4,5)6 |
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|Abbreviations = hex |
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| InChIKey = SANRKQGLYCLAFE-IIYYNVFAAT |
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| |
|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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|ChemSpiderID = 22966 |
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| ChEBI = 30235 |
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|PubChem = 24560 |
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| SMILES = F[U](F)(F)(F)(F)F |
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|InChI = 1/6FH.U/h6*1H;/q;;;;;;+6/p-6/rF6U/c1-7(2,3,4,5)6 |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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|InChIKey = SANRKQGLYCLAFE-IIYYNVFAAT |
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| StdInChI = 1S/6FH.U/h6*1H;/q;;;;;;+6/p-6 |
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| |
|ChEBI_Ref = {{ebicite|correct|EBI}} |
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|ChEBI = 30235 |
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| StdInChIKey = SANRKQGLYCLAFE-UHFFFAOYSA-H |
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|EINECS = 232-028-6 |
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|Gmelin = 2923 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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|SMILES = F[U](F)(F)(F)(F)F |
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| RTECS = YR4720000 |
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|StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| UNNumber = 2978 (<1% <sup>235</sup>U)<br/>2977 (>1% <sup>235</sup>U) |
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|StdInChI = 1S/6FH.U/h6*1H;/q;;;;;;+6/p-6 |
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}} |
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|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| Section2 = {{Chembox Properties |
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|StdInChIKey = SANRKQGLYCLAFE-UHFFFAOYSA-H |
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| Formula = UF<sub>6</sub> |
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|CASNo = 7783-81-5 |
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| MolarMass = 352.02 g/mol |
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|CASNo_Ref = {{cascite|correct|CAS}} |
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| Appearance = colorless solid |
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|UNII_Ref = {{fdacite|correct|FDA}} |
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| Density = 5.09 g/cm<sup>3</sup>, solid |
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|UNII = N06GJ1D94J |
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| Solubility = reacts |
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|RTECS = YR4720000 |
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| SolubleOther = soluble in [[chloroform]], [[carbon tetrachloride|CCl<sub>4</sub>]], liquid [[chlorine]] and [[bromine]] <br> dissolves in [[nitrobenzene]] |
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|UNNumber = 2978 (<1% {{chem2|^{235}U}})<br>2977 (>1% {{chem2|^{235}U}}) |
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| MeltingPt = 64.05 °C (triple point) |
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| BoilingPt = 56.5 °C (sublimes) |
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}} |
}} |
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| |
|Section2={{Chembox Properties |
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|Formula = {{chem2|UF6}} |
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| CrystalStruct = [[Orthorhombic]], [[Pearson symbol|oP28]] |
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|MolarMass = {{nowrap|352.02 g/mol}} |
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| SpaceGroup = Pnma, No. 62 |
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|Appearance = Colorless solid |
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| Coordination = octahedral (''O<sub>h</sub>'') |
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|Density = 5.09{{nbsp}}g/cm<sup>3</sup>, solid |
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| Dipole = 0 |
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|Solubility = Hydrolyzes |
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}} |
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|SolubleOther = {{ubl|Soluble in [[chloroform]], [[carbon tetrachloride|{{chem2|CCl4}}]], liquid [[chlorine]], and [[bromine]]|Dissolves in [[nitrobenzene]]; |
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| Section4 = {{Chembox Thermochemistry |
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151{{nbsp}}kPa<ref>{{cite web |url=http://www.ibilabs.com/Uranium%20Hexafluoride.htm |title=Uranium Hexafluoride |access-date=2013-08-08 |url-status=dead |archive-url=https://web.archive.org/web/20130916221434/http://ibilabs.com/Uranium%20Hexafluoride.htm |archive-date=2013-09-16}}</ref>}} |
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| DeltaHf = – solid: −(2197,7 ± 1,8) [[Joule|kJ]]·mol<sup>−1</sup><ref name="Enthalpie">Gerald K. Johnson: "The Enthalpy of Formation of Uranium Hexafluoride", ''[[The Journal of Chemical Thermodynamics]]'', '''1979''', ''11 (5)'', p. 483–490; {{DOI|10.1016/0021-9614(79)90126-5}}.</ref> |
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|BoilingPtC = 56.5 |
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– gaseous: −(2148,1 ± 1,8) kJ·mol<sup>−1</sup><ref name="Enthalpie"/> |
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|BoilingPt_notes = (sublimes, at atmospheric pressure)}} |
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| Entropy = – solid: −430,4 ± 1,5 J·K<sup>−1</sup>·mol<sup>−1</sup><ref name="Enthalpie"/> |
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|Section3={{Chembox Structure |
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– gaseous: −280,4 ± 1,5 J·K<sup>−1</sup>·mol<sup>−1</sup><ref name="Enthalpie"/> |
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|CrystalStruct = [[Orthorhombic]], [[Pearson symbol|oP28]] |
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}} |
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|SpaceGroup = Pnma, No. 62 |
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| Section7 = {{Chembox Hazards |
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|Coordination = Octahedral (''O<sub>h</sub>'') |
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| ExternalMSDS = [http://www.inchem.org/documents/icsc/icsc/eics1250.htm ICSC 1250] |
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|Dipole = 0}} |
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| EUIndex = 092-002-00-3 |
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|Section4={{Chembox Thermochemistry |
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| EUClass = Very toxic ('''T+''')<br/>Dangerous for the environment ('''N''') |
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|DeltaHf = {{ubl |
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| RPhrases = {{R26/28}}, {{R33}}, {{R51/53}} |
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|Solid, −2197.7±1.8{{nbsp}}[[Joule|kJ]]·mol<sup>−1</sup><ref name="Enthalpie">{{cite journal |last1=Johnson |first1=Gerald K. |year=1979 |title=The Enthalpy of Formation of Uranium Hexafluoride |journal=[[The Journal of Chemical Thermodynamics]] |volume=11 |issue=5 |pages=483–490 |doi=10.1016/0021-9614(79)90126-5}}</ref> |
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| SPhrases = {{S1/2}}, {{S20/21}}, {{S45}}, {{S61}} |
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|Gaseous, −2148.1±1.8{{nbsp}}kJ·mol<sup>−1</sup><ref name="Enthalpie"/> |
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| FlashPt = Non-flammable |
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}} |
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| Section8 = {{Chembox Related |
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| OtherAnions = [[Uranium hexachloride]] |
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| OtherCations = [[Neptunium hexafluoride]]<br/>[[Plutonium hexafluoride]] |
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| OtherFunctn = [[Uranium(III) fluoride]]<br/>[[Uranium(IV) fluoride]]<br/>[[Uranium(V) fluoride]] |
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| Function = uranium fluorides |
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}} |
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}} |
}} |
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|Entropy = {{ubl |
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|Solid, 227.8±1.3{{nbsp}}J·K<sup>−1</sup>·mol<sup>−1</sup><ref name="Enthalpie"/> |
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|Gaseous, 377.8±1.3{{nbsp}}J·K<sup>−1</sup>·mol<sup>−1</sup><ref name="Enthalpie"/> |
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}}}} |
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|Section7={{Chembox Hazards |
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|MainHazards = Toxic, corrosive, radioactive<ref>Uranium(VI) fluoride</ref> |
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|ExternalSDS = [https://www.inchem.org/documents/icsc/icsc/eics1250.htm ICSC 1250] |
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|GHSPictograms = {{GHS skull and crossbones}}{{GHS health hazard}}{{GHS environment}} |
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|GHSSignalWord = Danger |
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|HPhrases = {{H-phrases|300|330|373|411}} |
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|PPhrases = {{P-phrases|}} |
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|NFPA-H = 4 |
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|NFPA-F = 0 |
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|NFPA-R = 2 |
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|NFPA-S = W+OX |
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|FlashPt = Non-flammable |
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}} |
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|Section9={{Chembox Related |
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|OtherAnions = [[Uranium hexachloride]] |
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|OtherCations = {{ubl|[[Neptunium hexafluoride]]|[[Plutonium hexafluoride]]|[[Americium hexafluoride]]|[[Curium hexafluoride]]|[[Tungsten hexafluoride]]}} |
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|OtherFunction = {{ubl|[[Uranium(III) fluoride]]|[[Uranium(IV) fluoride]]|[[Uranium(V) fluoride]]}} |
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|OtherFunction_label = uranium fluorides |
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}} |
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}} |
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'''Uranium hexafluoride''', sometimes called '''hex''', is an [[inorganic compound]] with the formula {{chem2|UF6|auto=1}}. Uranium hexafluoride is a volatile and toxic white solid that [[hydrolysis|reacts with water]], releasing corrosive [[hydrofluoric acid]]. The compound reacts mildly with [[aluminium]], forming a thin surface layer of [[aluminium fluoride|{{chem2|AlF3}}]] that resists any further reaction from the compound. {{chem2|UF6}} is used in the process of [[enriched uranium|enriching uranium]], which produces fuel for [[nuclear reactor]]s and [[nuclear weapon]]s. |
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==Preparation== |
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Milled uranium ore—{{chem2|U3O8}} or "[[yellowcake]]"—is dissolved in [[nitric acid]], yielding a solution of [[uranyl nitrate]] {{chem2|UO2(NO3)2}}. Pure uranyl nitrate is obtained by [[solvent extraction]], then treated with [[ammonia]] to produce [[ammonium diuranate]] ("ADU", {{chem2|[NH4]2U2O7}}). Reduction with [[hydrogen]] gives {{chem2|UO2}}, which is converted with [[hydrofluoric acid]] (HF) to [[uranium tetrafluoride]], {{chem2|UF4}}. Oxidation with [[fluorine]] yields {{chem2|UF6}}. |
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The [[Honeywell Uranium Hexafluoride Processing Facility]] uses a different process. |
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During [[nuclear reprocessing#Fluoride volatility|nuclear reprocessing]], uranium is reacted with [[chlorine trifluoride]] to give {{chem2|UF6}}: |
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:{{chem2|U + 2 ClF3 → UF6 + Cl2}} |
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==Properties== |
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=== Physical properties === |
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At [[atmospheric pressure]], {{chem2|UF6}} [[sublimation (phase transition)|sublimes]] at 56.5 °C.<ref>{{cite journal |last1=Brickwedde |first1=Ferdinand G. |last2=Hoge |first2=Harold J. |last3=Scott |first3=Russell B. |year=1948 |title=The Low Temperature Heat Capacities, Enthalpies, and Entropies of UF<sub>4</sub> and UF<sub>6</sub> |journal=[[J. Chem. Phys.]] |volume=16 |issue=5 |pages=429–436 |doi=10.1063/1.1746914 |bibcode=1948JChPh..16..429B|doi-access=free}}</ref> |
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[[File:Uranium hexafluoride crystals sealed in an ampoule.jpg|thumb|center|upright=1.5|{{chem2|UF6}} in a glass [[ampoule]]]] |
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The solid-state structure was determined by [[neutron diffraction]] at 77 K and 293 K.<ref>{{cite journal |author1=J. H. Levy |author2=John C. Taylor |author3=Paul W. Wilson |title=Structure of Fluorides. Part XII. Single-Crystal Neutron Diffraction Study of Uranium Hexafluoride at 293 K |journal=J. Chem. Soc., Dalton Trans. |year=1976 |pages=219–224 |doi=10.1039/DT9760000219 |issue=3}}</ref><ref>{{cite journal |author=J. H. Levy, J. C. Taylor and A. B. Waugh |title=Neutron Powder Structural Studies of UF<sub>6</sub>, MoF<sub>6</sub> and WF<sub>6</sub> at 77 K |journal=Journal of Fluorine Chemistry |year=1983 |pages=29–36 |volume=23 |doi=10.1016/S0022-1139(00)81276-2}}</ref> |
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<gallery class="center" widths="180" heights="200"> |
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File:Uranium-hexafluoride-unit-cell-3D-balls.png|[[Ball-and-stick model]] of the unit cell of uranium hexafluoride<ref name="UF6_1973">J. C. Taylor, P. W. Wilson, J. W. Kelly: „The structures of fluorides. I. Deviations from ideal symmetry in the structure of crystalline UF<sub>6</sub>: a neutron diffraction analysis", ''[[Acta Crystallogr.]]'', '''1973''', ''B29'', p. 7–12; {{doi|10.1107/S0567740873001895}}.</ref> |
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File:Uranium hexafluoride dimensions.svg|Bond lengths and angles of gaseous uranium hexafluoride<ref name="UF6_1968">{{cite journal |last1=Kimura |first1=Masao |last2=Schomaker |first2=Werner |last3=Smith |first3=Darwin W. |last4=Bernard |year=1968 |title=Electron-Diffraction Investigation of the Hexafluorides of Tungsten, Osmium, Iridium, Uranium, Neptunium, and Plutonium |url=https://authors.library.caltech.edu/71173/ |journal=[[J. Chem. Phys.]] |volume=48 |issue=8 |pages=4001–4012 |doi=10.1063/1.1669727 |bibcode=1968JChPh..48.4001K |access-date=2020-10-10 |archive-date=2023-01-11 |archive-url=https://web.archive.org/web/20230111083844/https://authors.library.caltech.edu/71173/ |url-status=dead }}</ref> |
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</gallery> |
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===Chemical properties=== |
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It has been shown that uranium hexafluoride is an [[oxidant]]<ref>{{cite journal |author1=G. H. Olah |author2=J. Welch |title=Synthetic methods and reactions. 46. Oxidation of organic compounds with uranium hexafluoride in haloalkane solutions |journal=[[J. Am. Chem. Soc.]] |year=1978 |pages=5396–5402 |volume=100 |issue=17 |doi=10.1021/ja00485a024}}</ref> and a [[Lewis acids and bases|Lewis acid]] that 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), {{chem2|Cu(2+)[UF7−]2}}.<ref>{{cite journal |author1=J. A. Berry |author2=R. T. Poole |author3=A. Prescott |author4=D. W. A. Sharp |author5=J. M. Winfield |title=The oxidising and fluoride ion acceptor properties of uranium hexafluoride in acetonitrile |journal=J. Chem. Soc., Dalton Trans. |year=1976 |pages=272–274 |doi=10.1039/DT9760000272 |issue=3}}</ref> |
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[[Polymer]]ic uranium(VI) fluorides containing organic cations have been isolated and characterized by X-ray diffraction.<ref>{{cite journal |author1=S. M. Walker |author2=P. S. Halasyamani |author3=S. Allen |author4=D. O'Hare |title=From Molecules to Frameworks: Variable Dimensionality in the UO<sub>2</sub>(CH<sub>3</sub>COO)<sub>2</sub>·2H<sub>2</sub>O/HF(aq)/Piperazine System. Syntheses, Structures, and Characterization of Zero-Dimensional (C<sub>4</sub>N<sub>2</sub>H<sub>12</sub>)UO<sub>2</sub>F<sub>4</sub>·3H<sub>2</sub>O, One-Dimensional (C<sub>4</sub>N<sub>2</sub>H<sub>12</sub>)<sub>2</sub>U<sub>2</sub>F<sub>12</sub>·H<sub>2</sub>O, Two-Dimensional (C<sub>4</sub>N<sub>2</sub>H<sub>12</sub>)<sub>2</sub>(U<sub>2</sub>O<sub>4</sub>F<sub>5</sub>)<sub>4</sub>·11H<sub>2</sub>O, and Three-Dimensional (C<sub>4</sub>N<sub>2</sub>H<sub>12</sub>)U<sub>2</sub>O<sub>4</sub>F<sub>6</sub> |journal=J. Am. Chem. Soc. |year=1999 |pages=10513–10521 |volume=121 |issue=45 |doi=10.1021/ja992145f}}</ref> |
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==Application in the fuel cycle== |
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[[File:Uranium hexafluoride phase diagram.gif|thumb|left|250px|[[Phase diagram]] of {{chem2|UF6}}]] |
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As one of the most [[volatility (chemistry)|volatile]] compounds of uranium, uranium hexafluoride is relatively convenient to process and is used in both of the main uranium [[nuclear enrichment|enrichment]] methods, namely [[gaseous diffusion]] and the [[gas centrifuge]] method. Since the [[triple point]] of {{chem2|UF6}}; 64 °C(147 °F; 337 K) and 152 kPa (22 psi; 1.5 atm);<ref>{{cite web |title=Uranium Hexafluoride: Source: Appendix A of the PEIS (DOE/EIS-0269): Physical Properties |url=https://web.evs.anl.gov/uranium/guide/ucompound/propertiesu/hexafluoride.cfm |access-date=2022-08-18 |website=web.evs.anl.gov}}</ref> is close to ambient conditions, phase transitions can be achieved with little [[work (thermodynamics)|thermodynamic work]]. |
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Fluorine has only a single naturally occurring stable isotope, so [[isotopologue]]s of {{chem2|UF6}} differ in their molecular weight based solely on the uranium [[isotope]] present.<ref>{{cite web |title=Uranium Enrichment and the Gaseous Diffusion Process |publisher=USEC Inc |url=http://www.usec.com/v2001_02/HTML/Aboutusec_enrichment.asp |access-date=2007-09-24 |url-status=dead |archive-url=https://web.archive.org/web/20071019081831/http://www.usec.com/v2001_02/HTML/Aboutusec_enrichment.asp |archive-date=2007-10-19}}</ref> This difference is the basis for the physical separation of isotopes in enrichment. |
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All the other uranium fluorides are nonvolatile solids that are [[coordination polymer]]s. |
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The conversion factor for the {{chem2|^{238}U}} isotopologue of {{chem2|UF6}} ("hex") to "U mass" is 0.676.<ref>{{cite web |
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|website=TranslatorsCafé |
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|date=1 February 2021 |
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|title=Unit converter molar mass calculator |
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|url=https://www.translatorscafe.com/unit-converter/en-US/molar-mass/?q=UF6 |
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|publisher=ANVICA Software Development |
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|location=Mississauga, Ontario, Canada |
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}}</ref> |
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Gaseous diffusion requires about 60 times as much energy as the gas centrifuge process: gaseous diffusion-produced nuclear fuel produces 25 times more energy than is used in the diffusion process, while centrifuge-produced fuel produces 1,500 times more energy than is used in the centrifuge process. |
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In addition to its use in enrichment, uranium hexafluoride has been used in an advanced reprocessing method ([[fluoride volatility]]), which was developed in the [[Czech Republic]]. In this process, [[spent nuclear fuel]] is treated with fluorine gas to transform the oxides or elemental metals into a mixture of fluorides. This mixture is then distilled to separate the different classes of material. Some [[fission product]]s form nonvolatile fluorides which remain as solids and can then either be prepared for storage as nuclear waste or further processed either by [[solvation]]-based methods or [[electrochemistry|electrochemically]]. |
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Uranium enrichment produces large quantities of [[depleted uranium hexafluoride]] (D{{chem2|UF6}} or D-{{chem2|UF6}}) as a waste product. The long-term storage of D-{{chem2|UF6}} presents environmental, health, and safety risks because of its chemical instability. When {{chem2|UF6}} is exposed to moist air, it reacts with the water in the air to produce {{chem2|UO2F2}} ([[uranyl fluoride]]) and HF ([[hydrogen fluoride]]) both of which are highly corrosive and toxic. In 2005, 686,500 tonnes of D-{{chem2|UF6}} was housed in 57,122 storage cylinders located near [[Portsmouth, Ohio]]; [[Oak Ridge, Tennessee]]; and [[Paducah, Kentucky]].<ref>{{cite web |work=Depleted UF<sub>6</sub> FAQs |title=How much depleted uranium hexafluoride is stored in the United States? |url=https://web.evs.anl.gov/uranium/faq/mgmt/faq23.cfm |publisher=[[Argonne National Laboratory]]}}</ref><ref>{{cite web |title=Depleted UF<sub>6</sub> Management Program Documents |url=https://web.evs.anl.gov/uranium/documents/ |access-date=2006-05-17 |url-status=live |archive-url=https://web.archive.org/web/20080216013118/http://web.ead.anl.gov/uranium/documents/index.cfm |archive-date=2008-02-16}}</ref> Storage cylinders must be regularly inspected for signs of corrosion and leaks. The estimated lifetime of the steel cylinders is measured in decades.<ref>{{cite web |publisher=Institute for Energy and Environmental Research |date=2007-09-24 |title=What is DUF<sub>6</sub>? Is it dangerous and what should we do with it? |url=http://www.ieer.org/sdafiles/vol_5/5-2/deararj.html}}</ref> |
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== Accidents and disposal == |
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There have been several accidents involving uranium hexafluoride in the US, including a cylinder-filling accident and material release at the [[Sequoyah Fuels Corporation]] in 1986 where an estimated 29 500 pounds of gaseous {{chem2|UF6}} escaped.<ref>{{cite journal | pmc=1963288 | date=2007 | last1=Brugge | first1=D. | last2=Delemos | first2=J. L. | last3=Bui | first3=C. | title=The Sequoyah Corporation Fuels Release and the Church Rock Spill: Unpublicized Nuclear Releases in American Indian Communities | journal=American Journal of Public Health | volume=97 | issue=9 | pages=1595–1600 | doi=10.2105/AJPH.2006.103044 | pmid=17666688 }}</ref> <ref> |
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{{cite web |work=Depleted UF<sub>6</sub> FAQs |title=Have there been accidents involving uranium hexafluoride? |url=http://web.ead.anl.gov/uranium/faq/health/faq30.cfm |publisher=Argonne National Laboratory |archive-url=https://web.archive.org/web/20170609171651/http://web.ead.anl.gov/uranium/faq/health/faq30.cfm |archive-date=2017-06-09}}</ref> The U.S. government has been converting D{{chem2|UF6}} to solid [[uranium oxides]] for disposal.<ref>{{cite web |work=Depleted UF<sub>6</sub> FAQs |title=What is going to happen to the uranium hexafluoride stored in the United States? |url=https://web.evs.anl.gov/uranium/faq/storage/faq22.cfm |publisher=Argonne National Laboratory}}</ref> Such disposal of the entire D{{chem2|UF6}} stockpile could cost anywhere from $15 million to $450 million.<ref>{{cite web |work=Depleted UF<sub>6</sub> FAQs |title=Are there any currently-operating disposal facilities that can accept all of the depleted uranium oxide that would be generated from conversion of DOE's depleted UF<sub>6</sub> inventory? |url=http://web.evs.anl.gov/uranium/faq/mgmt/faq27.cfm |publisher=Argonne National Laboratory}}</ref> |
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{{Gallery |
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|width=250 |
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|height=180 |
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|File:UF6 cylinder rupture bw.png |
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|Ruptured 14-ton {{chem2|UF6}} shipping cylinder. 1 fatality, dozens injured. ~29500 lbs of material released. Sequoyah Fuels Corporation 1986. |
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|File:DUF6 storage yard far.jpg |
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|D{{chem2|UF6}} storage yard from afar |
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|File:Corroded DUF6 cylinder.jpg |
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|D{{chem2|UF6}} cylinders: painted (left) and corroded (right)<!-- (The left image is available on Commons; have to find the right image and then can make it look better as currently the images are not sized correctly.) --> |
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==References== |
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{{Reflist}} |
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==Further reading== |
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* ''[[Gmelins Handbuch der anorganischen Chemie]]'', System Nr. 55, Uran, Teil A, p. 121–123. |
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* ''Gmelins Handbuch der anorganischen Chemie'', System Nr. 55, Uran, Teil C 8, p. 71–163. |
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* R. DeWitt: ''Uranium hexafluoride: A survey of the physico-chemical properties'', Technical report, GAT-280; Goodyear Atomic Corp., Portsmouth, Ohio; 12. August 1960; {{doi|10.2172/4025868}}. |
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* Ingmar Grenthe, Janusz Drożdżynński, Takeo Fujino, Edgar C. Buck, [[Thomas E. Albrecht-Schmitt]], Stephen F. Wolf: [http://radchem.nevada.edu/classes/rdch710/files/Uranium.pdf Uranium] {{Webarchive|url=https://web.archive.org/web/20120118213655/http://radchem.nevada.edu/classes/rdch710/files/Uranium.pdf |date=2012-01-18}}, in: Lester R. Morss, Norman M. Edelstein, Jean Fuger (Hrsg.): ''The Chemistry of the Actinide and Transactinide Elements'', Springer, Dordrecht 2006; {{ISBN|1-4020-3555-1}}, p. 253–698; {{doi|10.1007/1-4020-3598-5_5}} (p. 530–531, 557–564). |
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* US-Patent 2535572: [https://www.freepatentsonline.com/2535572.html Preparation of UF<sub>6</sub>]; 26. December 1950. |
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* US-Patent 5723837: [https://www.freepatentsonline.com/5723837.html Uranium Hexafluoride Purification]; 3. March 1998. |
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==External links== |
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{{Commons category}} |
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* Simon Cotton (Uppingham School, Rutland, UK): [http://www.chm.bris.ac.uk/motm/uf6/uf6v.htm Uranium Hexafluoride]. |
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* [https://web.evs.anl.gov/uranium/guide/uf6/ Uranium Hexafluoride (UF<sub>6</sub>) – Physical and chemical properties of UF<sub>6</sub>, and its use in uranium processing – Uranium Hexafluoride and Its Properties] |
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* [https://www.webelements.com/compounds/uranium/uranium_hexafluoride.html Uranium Hexafluoride] at WebElements |
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* [http://ecoperestroika.ru/english/details-import-of-uranium-tails-2013-and-our-protests/ Import of Western depleted uranium hexafluoride (uranium tails) to Russia] [dead link 30 June 2017] |
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{{Hexafluorides}} |
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{{Uranium compounds}} |
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{{Fluorides}} |
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{{Actinide halides}} |
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[[Category:Actinide halides]] |
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[[Category:Hexafluorides]] |
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[[Category:Nuclear materials]] |
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[[Category:Octahedral compounds]] |
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[[Category:Uranium(VI) compounds]] |