Neptunium(VI) fluoride
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| Names | |
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| IUPAC name
Neptunium(VI) fluoride
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| Identifiers | |
3D model (JSmol)
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PubChem CID
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| Properties | |
| 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 | |
| Orthorhombic, oP28 | |
| Pnma, No. 62 | |
| octahedral (Oh) | |
| 0 D | |
| Thermochemistry[2]: 736 | |
Std molar
entropy (S⦵298) |
229.1 ± 0.5 J·K−1·mol−1 |
| Related compounds | |
Related fluoroNeptuniums
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Neptunium trifluoride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Neptunium hexafluoride (NpF6) is the highest fluoride of neptunium, it is also one of seventeen known binary hexafluorides. It is an orange volatile 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 is easily converted into the gas phase. Due to these properties, it is possible to separate neptunium from spent fuel. This quickly increased the interest in his presentation and in the exact examination of its properties.
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 and PuF6 are light-sensitive, decomposing to the corresponding tetrafluoride 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]
The hydrolysis of neptunium hexafluoride an almost anhydrous HF solution leads to the formation of NpOF4, which has a similar structure to UOF4. Attempts to oxidize the NpOF4 to the maximal possible oxidation state Np(VIII) using krypton difluoride were unsuccessful.
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
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.
- ^ 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.
- ^ 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: 56. 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: 555. doi:10.1063/1.170137.
- ^ 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.