Neptunium(VI) fluoride

Neptunium(VI) fluoride^[1]
Names
	IUPAC name Neptunium(VI) fluoride
	Other names Neptunium hexafluoride
Identifiers
CAS Number	14521-05-2 ;
3D model (JSmol)	Interactive image;
PubChem CID	19695135;
	InChI InChI=1S/6FH.Np/h6*1H;/q;;;;;;+6/p-6 ;
	SMILES F[Np](F)(F)(F)(F)F;
Properties
Chemical formula	F6Np
Molar mass	351 g·mol−1
Appearance	orange crystals
Melting point	54.4 °C (129.9 °F; 327.5 K)
Boiling point	55.18 °C (131.32 °F; 328.33 K)
Structure
Crystal structure	Orthorhombic, oP28
Space group	Pnma, No. 62
Coordination geometry	octahedral (Oh)
Dipole moment	0 D
Thermochemistry
Std molar; entropy (S⦵298)	229.1 ± 0.5 J·K−1·mol−1
Related compounds
Related fluoroNeptuniums	Neptunium trifluoride; Neptunium tetrafluoride
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). (what is ?) Infobox references

Neptunium(VI) fluoride (NpF₆) is the highest fluoride of neptunium, it is also one of seventeen known binary hexafluorides. It is a volatile orange crystalline solid.^[1] It is relatively hard to handle, being very corrosive, volatile and radioactive. Neptunium hexafluoride is stable in dry air but reacts vigorously with water.

At normal pressure, it melts at 54.4 °C and boils at 55.18 °C. It is the only neptunium compound that boils at a low temperature. Due to these properties, it is possible to easily separate neptunium from spent fuel.

Preparation

Neptunium hexafluoride was first prepared in 1943 by American chemist Alan E. Florin, who heated a sample of neptunium(III) fluoride on a nickel filament in a stream of fluorine and condensed the product in a glass capillary tube.^[3]^[4] Methods of preparation from both neptunium(III) fluoride and neptunium(IV) fluoride were later patented by Glenn T. Seaborg and Harrison S. Brown.^[5]

Standard method

The usual method of preparation is by fluorination of neptunium(IV) fluoride (NpF₄) by elemental fluorine (F₂) at 500 °C.^[6]

NpF
₄ + F
₂ → NpF
₆

In comparison, uranium hexafluoride (UF₆) is formed relatively rapidly from uranium tetrafluoride (UF₄) and F₂ at 300 °C, while plutonium hexafluoride (PuF₆) only begins forming from plutonium tetrafluoride (PuF₄) and F₂ at 750 °C.^[6] This difference allows uranium, neptunium and plutonium to be effectively separated.

Other methods

Using a different starting material

Neptunium hexafluoride can also be obtained by fluorination of neptunium(III) fluoride or neptunium(IV) oxide.^[7]

2 NpF
₃ + 3 F
₂ → 2 NpF
₆

NpO
₂ + 3 F
₂ → NpF
₆ + O
₂

Using a different fluorine source

The preparation can also be done with the help of stronger fluorinating reagents like bromine trifluoride (BrF₃) or bromine pentafluoride (BrF₅). These reactions can be used to separate plutonium, since PuF₄ does not undergo a similar reaction.^[8]^[9]

Neptunium dioxide and neptunium tetrafluoride are practically completely converted to volatile neptunium hexafluoride by dioxygen difluoride (O₂F₂). This works as a gas-solid reaction at moderate temperatures, as well as in anhydrous liquid hydrogen fluoride at −78 °C.^[10]

NpO
₂ + 3 O
₂F
₂ → NpF
₆ + 4 O
₂

NpF
₄ + O
₂F
₂ → NpF
₆ + O
₂

These reaction temperatures are markedly different from the high temperatures of over 200 °C previously required to synthesize neptunium hexafluoride with elemental fluorine or halogen fluorides.^[10] Neptunyl fluoride (NpO₂F₂) has been detected by Raman spectroscopy as a dominant intermediate in the reaction with NpO₂. Direct reaction of NpF₄ with liquid O₂F₂ led instead to vigorous decomposition of the O₂F₂ with no NpF₆ generation.

Properties

Physical properties

Neptunium hexafluoride forms orange orthorhombic crystals that melt at 54.4 °C and boil at 55.18 °C under standard pressure. The triple point is 55.10 °C and 1010 hPa (758 Torr).^[11]

The volatility of NpF₆ is similar to those of UF₆ and PuF₆, all three being actinide hexafluorides. The standard molar entropy is 229.1 ± 0.5 J·K⁻¹·mol⁻¹. Solid NpF₆ is paramagnetic, with a magnetic susceptibility of 165·10⁻⁶ cm³·mol⁻¹.^[12]^[13]

Chemical properties

Neptunium hexafluoride is stable in dry air. However, it reacts vigorously with water, including atmospheric moisture, to form the water-soluble neptunyl fluoride (NpO₂F₂) and hydrofluoric acid (HF).

NpF
₆ + 2 H
₂O → NpO
₂F
₂ + 4 HF

It can be stored at room temperature in a quartz or pyrex glass ampoule, provided that there are no traces of moisture or gas inclusions in the glass and any remaining HF has been removed.^[6] NpF₆ is light-sensitive, decomposing to NpF₄ and fluorine.^[6]

NpF₆ forms complexes with alkali metal fluorides: with caesium fluoride (CsF) it forms CsNpF₆ at 25 °C,^[14] and with sodium fluoride it reacts reversibly to form Na₃NpF₈.^[15] In either case, the neptunium is reduced to Np(V).

NpF
₆ + CsF → CsNpF
₆ + 1/2 F
₂

NpF
₆ + 3 NaF → Na
₃NpF
₈ + 1/2 F
₂

In the presence of chlorine trifluoride (ClF₃) as solvent and at low temperatures, there is some evidence of the formation of an unstable Np(IV) complex.^[14]

Neptunium hexafluoride reacts with carbon monoxide (CO) and light to form a white powder, presumably containing neptunium pentafluoride (NpF₅) and an unidentified substance.^[2]^: 732

Uses

The irradiation of nuclear fuel inside nuclear reactors generates both fission products and transuranic elements, including neptunium and plutonium. The separation of these three elements is an essential component of nuclear reprocessing. Neptunium hexafluoride plays a role in the separation of neptunium from both uranium and plutonium.

In order to separate the uranium (95% of the mass) from spent nuclear fuel, it is first powdered and reacted with elemental fluorine ("direct fluorination"). The resulting volatile fluorides (mainly UF₆, small amounts of NpF₆) are easily extracted from the non-volatile fluorides of other actinides, like plutonium(IV) fluoride (PuF₄), americium(III) fluoride (AmF₃), and curium(III) fluoride (CmF₃).^[16]

The mixture of UF₆ and NpF₆ is then selectively reduced by pelleted cobalt(II) fluoride, which converts the neptunium hexafluoride to the tetrafluoride but does not react with the uranium hexafluoride, using temperatures in the range of 93 to 204 °C.^[17] Another method is using magnesium fluoride, on which the neptunium fluoride is sorbed at 60-70% but not the uranium fluoride.^[18]

References

^ ^a ^b Gmelins Handbuch der anorganischen Chemie, System Nr. 71, Transurane, Teil C, p. 108–114.
^ ^a ^b Yoshida, Zenko; Johnson, Stephen G.; Kimura, Takaumi; Krsul, John R. Neptunium.
^ Florin, Alan E. (1943) Report MUC-GTS-2165
^ Fried, Sherman; Davidson, Norman (1948). "The Preparation of Solid Neptunium Compounds". J. Am. Chem. Soc. 70 (11): 3539–3547. doi:10.1021/ja01191a003. PMID 18102891.
^ US patent 2982604, Seaborg, Glenn T. & Brown, Harrison S., "Preparation of Neptunium Hexafluoride", published 1961-05-02, issued 1961-04-25
^ ^a ^b ^c ^d Malm, John G.; Weinstock, Bernard; Weaver, E. Eugene (1958). "The Preparation and Properties of NpF₆; a Comparison with PuF₆". J. Phys. Chem. 62 (12): 1506–1508. doi:10.1021/j150570a009..
^ Fried, Sherman; Davidson, Norman (1948). "The Preparation of Solid Neptunium Compounds". J. Am. Chem. Soc. 70 (11): 3539–3547. doi:10.1021/ja01191a003. PMID 18102891.
^ Trevorrow, L. E.; Gerding, T. J.; Steindler, M. J. (1968) Laboratory Investigations in Support of Fluid-bed Fluoride Volatility Processes, Part XVII, The Fluorination of Neptunium(IV) fluoride and Neptunium(IV) oxide (Argonne National Laboratory Report ANL-7385) 1 January 1968. doi:10.2172/4492135
^ Trevorrow, L. E.; Gerding, T. J.; Steindler, M. J. (1968). "The Fluorination of Neptunium(IV) Fluoride and Neptunium(IV) Oxide". J. Inorg. Nucl. Chem. 30 (10): 2671–2677. doi:10.1016/0022-1902(68)80394-X.
^ ^a ^b Eller, P. Gary; Asprey, Larned B.; Kinkead, Scott A.; Swanson, Basil I.; Kissane, Richard J. (1998). "Reactions of Dioxygen Difluoride with Neptunium Oxides and Fluorides". J. Alloys Compd. 269 (1–2): 63–66. doi:10.1016/S0925-8388(98)00005-X.
^ Keller C. (1969) Die Chemie des Neptuniums. In: Anorganische Chemie. Fortschritte der Chemischen Forschung, vol 13/1. Springer, Berlin, Heidelberg. doi:10.1007/BFb0051170
^ Hutchison, Clyde A.; Weinstock, Bernard (1960). "Paramagnetic Resonance Absorption in Neptunium Hexafluoride". J. Chem. Phys. 32 (1): 56. Bibcode:1960JChPh..32...56H. doi:10.1063/1.1700947.
^ Hutchison, Clyde A.; Tsang, Tung; Weinstock, Bernard (1962). "Magnetic Susceptibility of Neptunium Hexafluoride in Uranium Hexafluoride". J. Chem. Phys. 37 (3): 555. Bibcode:1962JChPh..37..555H. doi:10.1063/1.1701373.
^ ^a ^b Peacock, R. D. (1976). "Some Reactions of Neptunium Hexafluoride". J. Inorg. Nucl. Chem. 38 (4): 771–773. doi:10.1016/0022-1902(76)80353-3.
^ Trevorrow, LeVerne E.; T. J., Gerding; Steindler, Martin J. (1968). "Reaction of Neptunium Hexafluoride". Inorg. Chem. 7 (11): 2226–2229. doi:10.1021/ic50069a010.
^ Uhlíř, Jan; Mareček, Martin (2009). "Fluoride Volatility Method for Reprocessing of LWR and FR Fuels". Journal of Fluorine Chemistry. 130 (1): 89–93. doi:10.1016/j.jfluchem.2008.07.002.
^ US patent 3615267, Golliher, Waldo R.; Harris, Robert L. & Ledoux, Reynold A., "Separation of Neptunium from Uranium Hexafluoride Containing the Same", published 1971-10-26, issued 1971-10-26
^ Nakajima, Tsuyoshi; Groult, Henri, eds. (2005). Fluorinated Materials for Energy Conversion. Elsevier. p. 559. ISBN 9780080444727.