Plutonium tetrafluoride

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

CAS Number

* 13709-56-3 N

3D model (JSmol)

* Interactive image

ChemSpider |

* 123078

PubChem CID

* 139558

InChI

* InChI=1S/4FH.Pu/h4*1H;/q;;;;+4/p-4

Key: USCBBUFEOOSGAJ-UHFFFAOYSA-J

SMILES

* F[Pu](F)(F)F

Properties

Chemical formula

| 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

Crystal structure

| Monoclinic, mS60

Space group

| C12/c1, No. 15

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

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". https://osf.io/5md4c/.
3. ↑ 3.0 3.1 3.2 United States Department of Energy (1997). Linking Legacies: Connecting the Cold War Nuclear Weapons Production Processes to Their Environmental Consequences. Washington D.C.: United States Department of Energy. pp. 184; passim. https://www.energy.gov/sites/prod/files/2014/03/f8/Linking_Legacies.pdf.
4. ↑ 4.0 4.1 Baldwin, Charles E.; Navratil, James D. (1983-05-19). "Plutonium Process Chemistry at Rocky Flats". in Carnall, William T.; Choppin, Gregory R. (in en). Plutonium Chemistry. ACS Symposium Series. 216. AMERICAN CHEMICAL SOCIETY. pp. 369–380. doi:10.1021/bk-1983-0216.ch024. ISBN 9780841207721.
5. ↑ 5.0 5.1 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. (in en). Plutonium Chemistry. ACS Symposium Series. 216. AMERICAN CHEMICAL SOCIETY. pp. 349–368. doi:10.1021/bk-1983-0216.ch023. ISBN 9780841207721.
6. ↑ Gmelins Handbuch der anorganischen Chemie, System Nr. 71, Transurane, Teil C, pp. 104–107.
7. ↑ , Sherman W. & George M. Campbell"Photochemical preparation of plutonium pentafluoride"  patent 4670239, 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". https://osf.io/27xzs/.

* v
* t
* e

Plutonium compounds

Plutonium(II)|

* PuH2
* PuB2

Plutonium(III)|

* PuH3
* PuB
* PuCl3
* PuF3

Plutonium(IV)|

* PuC
* PuF4
* PuO2
* Pu(C8H8)2

Plutonium(VI)|

* PuF6

* v
* t
* e

Salts and covalent derivatives of the fluoride ion

HF |  |  |  | He

|
|
|
|

LiF | BeF2 | BF
BF3
B2F4 | CF4
other compounds | NF3
FN3
N2F2
N2F4
NF5§  | F2O
F2O2
other compounds | F2 | Ne
NaF | MgF2 | AlF
AlF3 | SiF4 | P2F4
PF3
PF5 | S2F2
SF2
SF4
SF6 | ClF
ClF3
ClF5 | Ar
KF | CaF
CaF2 | ScF3 | TiF2
TiF3
TiF4 | VF2
VF3
VF4
VF5 | CrF2
CrF3
CrF4
CrF5
CrF6§  | MnF2 | FeF2
FeF3 | CoF2
CoF3 | NiF2 | CuF
CuF2 | ZnF2 | GaF2
GaF3 | GeF2
GeF4 | AsF3
AsF5 | Se2F2
SeF4
SeF6 | BrF
BrF3
BrF5 | KrF2
RbF | SrF
SrF2 | YF3 | ZrF3
ZrF4 | NbF4
NbF5 | MoF2
MoF3
MoF4
MoF5
MoF6 | TcF4
TcF6 | RuF3
RuF5
RuF6 | RhF3
RhF5
RhF6 | PdF2 | AgF | CdF2 | InF
InF2
InF3 | SnF2
SnF4 | SbF3
SbF5 | Te3F2
TeF4
TeF6 | IF
IF3</br>IF5</br>IF7 | XeF2
XeF4
XeF6
CsF | BaF2 |  | HfF4 | TaF5 | WF2
WF3
WF4
WF5
WF6 | Re3F9
ReF4
ReF5
ReF6
ReF7 | OsF4
OsF5
OsF6 | IrF2
IrF3
IrF4
IrF5
IrF6 | PtF2
PtF4
PtF5
PtF6 | AuF
AuF3
Au2F10
AuF5•F2 | Hg2F2
HgF2
HgF4 | TlF | PbF2
PbF4 | BiF3
BiF5 | PoF2
PoF4
PoF6 | AtF  | RnF2
FrF | RaF2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaF3 | CeF3
CeF4 | PrF3 | NdF2,
NdF3 | PmF3 | SmF2,
SmF3 | EuF2,
EuF3 | GdF3 | TbF3 | DyF2,
DyF3 | HoF3 | ErF3 | TmF2
TmF3 | YbF2
YbF3 | LuF3
AcF3 | ThF4 | PaF5 | UF3
UF4
UF5
UF6 | NpF4
NpF6 | PuF3
PuF6 | AmF2
AmF3 | CmF3 | BkF3 | CfF3 | EsF3 | Fm  | Md  | No  | LrF3

§ means the substance has not been made.

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