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Plutonium tetrafluoride

In today's world, Plutonium tetrafluoride has become a topic of great relevance and interest to a wide variety of people. Its impact and scope are so significant that they do not go unnoticed in any area. From the academic field, through the work world, to the personal sphere, Plutonium tetrafluoride arouses great interest and debate. As we delve into this topic, we will realize the importance it has in today's society and how its influence has been growing over time. In addition, we will explore its implications, challenges and potential solutions, with the aim of thoroughly understanding this phenomenon and its consequences in our daily lives.

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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(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 , 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 gives 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. doi:10.1016/C2009-0-30414-6. 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.
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