Plutonium tetrafluoride[1]

A sample of plutonium tetrafluoride produced at the Hanford Site during the Cold War[2][3]
Names
IUPAC name
Plutonium(IV) fluoride
Other names
Plutonium tetrafluoride
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/4FH.Pu/h4*1H;/q;;;;+4/p-4
    Key: USCBBUFEOOSGAJ-UHFFFAOYSA-J
  • F[Pu](F)(F)F
Properties
PuF4
Molar mass 320 g/mol
Appearance reddish-brown monoclinic crystals
Density 7.1 g/cm3
Melting point 1,027 °C (1,881 °F; 1,300 K)
Structure
Monoclinic, mS60
C12/c1, No. 15
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Plutonium(IV) fluoride is a chemical compound with the formula (PuF4). This salt is generally a brown solid but can appear a variety of colors depending on the grain size, purity, moisture content, lighting, and presence of contaminants.[4][5] Its primary use in the United States has been as an intermediary product in the production of plutonium metal for nuclear weapons usage.[3]

Formation

Plutonium(IV) fluoride is produced in the reaction between plutonium dioxide (PuO2) or plutonium(III) fluoride (PuF3) with hydrofluoric acid (HF) in a stream of oxygen (O2) at 450 to 600 °C. The main purpose of the oxygen stream is to avoid reduction of the product by hydrogen gas, small amounts of which are often found in HF.[6]

PuO2 + O2 + 4 HF → PuF4 + O2 + 2 H2O
4 PuF3 + O2 + 4 HF → 4 PuF4 + 2 H2O

Laser irradiation of plutonium hexafluoride (PuF6) at wavelengths under 520 nm causes it to decompose into plutonium pentafluoride (PuF5) and fluorine; if this is continued, plutonium(IV) fluoride is obtained.[7]

Properties

In terms of its structure, solid plutonium(IV) fluoride features 8-coordinate Pu centers interconnected by doubly bridging fluoride ligands.[8]

Reaction of plutonium tetrafluoride with barium, calcium, or lithium at 1200 °C give Pu metal:[4][5][3]

PuF4 + 2 Ba → 2 BaF2 + Pu
PuF4 + 2 Ca → 2 CaF2 + Pu
PuF4 + 4 Li → 4 LiF + Pu
Plutonium tetrafluoride sample with example of one color illustrated through reference to a color standard[9]

References

  1. ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, Florida: CRC Press, pp. 4–76, ISBN 0-8493-0594-2
  2. ^ Pfeiffer, Martin (March 3, 2019). "FOI 2019-00371.Loaded powder pan at RMC line". Pfeiffer Nuclear Weapon and National Security Archive. Retrieved May 23, 2019.
  3. ^ a b c United States Department of Energy (1997). Linking Legacies: Connecting the Cold War Nuclear Weapons Production Processes to Their Environmental Consequences (PDF). Washington D.C.: United States Department of Energy. pp. 184, passim.
  4. ^ a b Baldwin, Charles E.; Navratil, James D. (1983-05-19). "Plutonium Process Chemistry at Rocky Flats". In Carnall, William T.; Choppin, Gregory R. (eds.). Plutonium Chemistry. ACS Symposium Series. Vol. 216. AMERICAN CHEMICAL SOCIETY. pp. 369–380. doi:10.1021/bk-1983-0216.ch024. ISBN 9780841207721.
  5. ^ a b Christensen, Eldon L.; Grey, Leonard W.; Navratil, James D.; Schulz, Wallace W. (1983-05-19). "Present Status and Future Directions of Plutonium Process Chemistry". In Carnall, William T.; Choppin, Gregory R. (eds.). Plutonium Chemistry. ACS Symposium Series. Vol. 216. AMERICAN CHEMICAL SOCIETY. pp. 349–368. doi:10.1021/bk-1983-0216.ch023. ISBN 9780841207721. OSTI 6781635.
  6. ^ Gmelins Handbuch der anorganischen Chemie, System Nr. 71, Transurane, Teil C, pp. 104–107.
  7. ^ 4670239, Rabideau, Sherman W. & Campbell, George M., "Photochemical preparation of plutonium pentafluoride", issued 1987-06-02 
  8. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  9. ^ Pfeiffer, Martin (March 3, 2019). "PuF4 Pics ORO 2019 00475-FN Final Response 20190312_Page_07_Image_0001". Pfeiffer Nuclear Weapon and National Security Archive. Retrieved May 23, 2019.
source: http://en.wikipedia.org/wiki/Plutonium_tetrafluoride