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Protactinium compounds

Protactinium compounds are compounds containing the element protactinium (symbol: Pa). These compounds usually have protactinium in the +5 oxidation state, although these compounds can also exist in the +2, +3 and +4 oxidation states.

Properties of protactinium compounds

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Formula color symmetry space group No Pearson symbol a (pm) b (pm) c (pm) Z density (g/cm3)
Pa silvery-gray tetragonal[1] I4/mmm 139 tI2 392.5 392.5 323.8 2 15.37
PaO rocksalt[2] Fm3m 225 cF8 496.1 4 13.44
PaO2 black fcc[2] Fm3m 225 cF12 550.5 4 10.47
Pa2O5 white Fm3m[2] 225 cF16 547.6 547.6 547.6 4 10.96
Pa2O5 white orthorhombic[2] 692 402 418
PaH3 black cubic[2] Pm3n 223 cP32 664.8 664.8 664.8 8 10.58
PaF4 brown-red monoclinic[2] C2/c 15 mS60 2
PaCl4 green-yellow tetragonal[3] I41/amd 141 tI20 837.7 837.7 748.1 4 4.72
PaBr4 brown tetragonal[4][5] I41/amd 141 tI20 882.4 882.4 795.7
PaCl5 yellow monoclinic[6] C2/c 15 mS24 797 1135 836 4 3.74
PaBr5 red monoclinic[5][7] P21/c 14 mP24 838.5 1120.5 1214.6 4 4.98
PaOBr3 monoclinic[5] C2 1691.1 387.1 933.4
Pa(PO3)4 orthorhombic[8] 696.9 895.9 1500.9
Pa2P2O7 cubic[8] Pa3 865 865 865
Pa(C8H8)2 golden-yellow monoclinic[9] 709 875 1062

Here a, b and c are lattice constants in picometers, No is space group number and Z is the number of formula units per unit cell; fcc stands for the face-centered cubic symmetry. Density was not measured directly but calculated from the lattice parameters.

Oxides and oxygen-containing salts

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Protactinium oxides are known for the metal oxidation states +2, +4 and +5. The most stable is white pentoxide Pa2O5, which can be produced by igniting protactinium(V) hydroxide in air at a temperature of 500 °C.[10] Its crystal structure is cubic, and the chemical composition is often non-stoichiometric, described as PaO2.25. Another phase of this oxide with orthorhombic symmetry has also been reported.[2][11] The black dioxide PaO2 is obtained from the pentoxide by reducing it at 1550 °C with hydrogen. It is not readily soluble in either dilute or concentrated nitric, hydrochloric or sulfuric acids, but easily dissolves in hydrofluoric acid.[2] The dioxide can be converted back to pentoxide by heating in oxygen-containing atmosphere to 1100 °C.[11] The monoxide PaO has only been observed as a thin coating on protactinium metal, but not in an isolated bulk form.[2]

Protactinium forms mixed binary oxides with various metals. With alkali metals A, the crystals have a chemical formula APaO3 and perovskite structure, or A3PaO4 and distorted rock-salt structure, or A7PaO6 where oxygen atoms form a hexagonal close-packed lattice. In all these materials, protactinium ions are octahedrally coordinated.[12][13] The pentoxide Pa2O5 combines with rare-earth metal oxides R2O3 to form various nonstoichiometric mixed-oxides, also of perovskite structure.[14]

Protactinium oxides are basic; they easily convert to hydroxides and can form various salts, such as sulfates, phosphates, nitrates, etc. Protactinyl nitrate is usually white but can be brown due to radiolytic decomposition. Heating the nitrate in air at 400 °C converts it to the white protactinium pentoxide.[15] The polytrioxophosphate Pa(PO3)4 can be produced by reacting difluoride sulfate PaF2SO4 with phosphoric acid (H3PO4) under inert gas atmosphere. Heating the product to about 900 °C eliminates the reaction by-products such as hydrofluoric acid, sulfur trioxide and phosphoric anhydride. Heating it to higher temperatures in an inert atmosphere decomposes Pa(PO3)4 into the diphosphate PaP2O7, which is analogous to diphosphates of other actinides. In the diphosphate, the PO3 groups form pyramids of C2v symmetry. Heating PaP2O7 in air to 1400 °C decomposes it into the pentoxides of phosphorus and protactinium.[8]

Halides

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Protactinium(V) fluoride forms white crystals where protactinium ions are arranged in pentagonal bipyramids and coordinated by 7 other ions. The coordination is the same in protactinium(V) chloride, but the color is yellow. The coordination changes to octahedral in the brown protactinium(V) bromide and is unknown for protactinium(V) iodide. The protactinium coordination in all its tetrahalides is 8, but the arrangement is square antiprismatic in protactinium(IV) fluoride and dodecahedral in the chloride and bromide. Brown-colored protactinium(III) iodide has been reported where protactinium ions are 8-coordinated in a bicapped trigonal prismatic arrangement.[16]

 
Coordination of protactinium (solid circles) and halogen atoms (open circles) in protactinium(V) fluoride or chloride.

Protactinium(V) fluoride and protactinium(V) chloride have a polymeric structure of monoclinic symmetry. There, within one polymeric chain, all the halide atoms lie in one graphite-like plane and form planar pentagons around the protactinium ions. The coordination 7 of protactinium originates from the 5 halide atoms and two bonds to protactinium atoms belonging to the nearby chains. These compounds easily hydrolyze in water.[17] The pentachloride melts at 300 °C and sublimates at even lower temperatures.

Protactinium(V) fluoride can be prepared by reacting protactinium oxide with either bromine pentafluoride or bromine trifluoride at about 600 °C, and protactinium(IV) fluoride is obtained from the oxide and a mixture of hydrogen and hydrogen fluoride at 600 °C; a large excess of hydrogen is required to remove atmospheric oxygen leaks into the reaction.[2]

Protactinium(V) chloride is prepared by reacting protactinium oxide with carbon tetrachloride at temperature of 200–300 °C.[2] The by-products (such as PaOCl3) are removed by fractional sublimation.[6] Reduction of protactinium(V) chloride with hydrogen at about 800 °C yields protactinium(IV) chloride – a yellow-green solid which sublimes in vacuum at 400 °C; it can also be obtained directly from protactinium dioxide by treating it with carbon tetrachloride at 400 °C.[2]

Protactinium bromides are produced by the action of aluminium bromide, hydrogen bromide, carbon tetrabromide or a mixture of hydrogen bromide and thionyl bromide on protactinium oxide. An alternative reaction is between protactinium pentachloride and hydrogen bromide or thionyl bromide.[2] Protactinium(V) bromide has two similar monoclinic forms, one is obtained by sublimation at 400–410 °C and another by sublimation at slightly lower temperature of 390–400 °C.[5][7]

Protactinium iodides result from the oxides and aluminium iodide or ammonium iodide heated to 600 °C.[2] Protactinium(III) iodide was obtained by heating protactinium(V) iodide in vacuum.[17] As with oxides, protactinium forms mixed halides with alkali metals. Among those, most remarkable is Na3PaF8 where protactinium ion is symmetrically surrounded by 8 F− ions which form a nearly perfect cube.[18]

More complex protactinium fluorides are also known such as Pa2F9[17] and ternary fluorides of the types MPaF6 (M = Li, Na, K, Rb, Cs or NH4), M2PaF7 (M = K, Rb, Cs or NH4) and M3PaF8 (M = Li, Na, Rb, Cs), all being white crystalline solids. The MPaF6 formula can be represented as a combination of MF and PaF5. These compounds can be obtained by evaporating a hydrofluoric acid solution containing these both complexes. For the small alkali cations like Na, the crystal structure is tetragonal, whereas it lowers to orthorphombic for larger cations K+, Rb+, Cs+ or NH4+. A similar variation was observed for the M2PaF7 fluorides, namely the crystal symmetry was dependent on the cation and differed for Cs2PaF7 and M2PaF7 (M = K, Rb or NH4).[19]

Other inorganic compounds

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Oxyhalides and oxysulfides of protactinium are known. PaOBr3 has a monoclinic structure composed of double-chain units where protactinium has coordination 7 and is arranged into pentagonal bipyramids. The chains are interconnected through oxygen and bromine atoms, and each oxygen atom is related to three protactinium atoms.[5] PaOS is a light-yellow non-volatile solid with a cubic crystal lattice isostructural to that of other actinide oxysulfides. It is obtained by reacting protactinium(V) chloride with a mixture of hydrogen sulfide and carbon disulfide at 900 °C.[2]

In hydrides and nitrides, protactinium has a low oxidation state of about +3. The hydride is obtained by direct action of hydrogen on the metal at 250 °C, and the nitride is a product of ammonia and protactinium tetrachloride or pentachloride. This bright yellow solid is stable to heating to 800 °C in vacuum. Protactinium carbide PaC is formed by reduction of protactinium tetrafluoride with barium in a carbon crucible at a temperature of about 1400 °C.[2] Protactinium forms borohydrides which include Pa(BH4)4. It has an unusual polymeric structure with helical chains where the protactinium atom has coordination number of 12 and is surrounded by six BH4− ions.[20]

Organometallic compounds

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The proposed structure of the protactinocene (Pa(C8H8)2) molecule

Protactinium(IV) forms a tetrahedral complex tetrakis(cyclopentadienyl)protactinium(IV) (or Pa(C5H5)4) with four cyclopentadienyl rings, which can be synthesized by reacting protactinium(IV) chloride with molten Be(C5H5)2. One ring can be substituted with a halide atom.[21] Another organometallic complex is golden-yellow bis(π-cyclooctatetraene) protactinium, or protactinocene, Pa(C8H8)2, which is analogous in structure to uranocene. There, the metal atom is sandwiched between two cyclooctatetraene ligands. Similar to uranocene, it can be prepared by reacting protactinium tetrachloride with dipotassium cyclooctatetraenide, K2C8H8, in tetrahydrofuran.[9]

See also

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References

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  1. ^ Donohue, J. (1959). "On the crystal structure of protactinium metal". Acta Crystallographica. 12 (9): 697–698. Bibcode:1959AcCry..12..697D. doi:10.1107/S0365110X59002031.
  2. ^ a b c d e f g h i j k l m n o p Sellers, Philip A.; Fried, Sherman; Elson, Robert E.; Zachariasen, W. H. (1954). "The Preparation of Some Protactinium Compounds and the Metal". Journal of the American Chemical Society. 76 (23): 5935. doi:10.1021/ja01652a011.
  3. ^ Brown D.; Hall T.L.; Moseley P.T (1973). "Structural parameters and unit cell dimensions for the tetragonal actinide tetrachlorides(Th, Pa, U, and Np) and tetrabromides (Th and Pa)". Journal of the Chemical Society, Dalton Transactions (6): 686–691. doi:10.1039/DT9730000686.
  4. ^ Tahri, Y.; Chermette, H.; El Khatib, N.; Krupa, J.; et al. (1990). "Electronic structures of thorium and protactinium halide clusters of [ThX8]4− type". Journal of the Less Common Metals. 158: 105–116. doi:10.1016/0022-5088(90)90436-N.
  5. ^ a b c d e Brown, D.; Petcher, T. J.; Smith, A. J. (1968). "Crystal Structures of some Protactinium Bromides". Nature. 217 (5130): 737. Bibcode:1968Natur.217..737B. doi:10.1038/217737a0. S2CID 4264482.
  6. ^ a b Dodge, R. P.; Smith, G. S.; Johnson, Q.; Elson, R. E. (1967). "The crystal structure of protactinium pentachloride". Acta Crystallographica. 22 (1): 85–89. Bibcode:1967AcCry..22...85D. doi:10.1107/S0365110X67000155.
  7. ^ a b Brown, D.; Petcher, T. J.; Smith, A. J. (1969). "The crystal structure of β-protactinium pentabromide". Acta Crystallographica B. 25 (2): 178. Bibcode:1969AcCrB..25..178B. doi:10.1107/S0567740869007357.
  8. ^ a b c Brandel, V.; Dacheux, N. (2004). "Chemistry of tetravalent actinide phosphates—Part I". Journal of Solid State Chemistry. 177 (12): 4743. Bibcode:2004JSSCh.177.4743B. doi:10.1016/j.jssc.2004.08.009.
  9. ^ a b Starks, David F.; Parsons, Thomas C.; Streitwieser, Andrew; Edelstein, Norman (1974). "Bis(π-cyclooctatetraene) protactinium". Inorganic Chemistry. 13 (6): 1307. doi:10.1021/ic50136a011.
  10. ^ Greenwood, p. 1268
  11. ^ a b Elson, R.; Fried, Sherman; Sellers, Philip; Zachariasen, W. H. (1950). "The tetravalent and pentavalent states of protactinium". Journal of the American Chemical Society. 72 (12): 5791. doi:10.1021/ja01168a547.
  12. ^ Greenwood, p. 1269
  13. ^ Iyer, P. N.; Smith, A. J. (1971). "Double oxides containing niobium, tantalum or protactinium. IV. Further systems involving alkali metals". Acta Crystallographica B. 27 (4): 731. Bibcode:1971AcCrB..27..731I. doi:10.1107/S056774087100284X.
  14. ^ Iyer, P. N.; Smith, A. J. (1967). "Double oxides containing niobium, tantalum, or protactinium. III. Systems involving the rare earths". Acta Crystallographica. 23 (5): 740. Bibcode:1967AcCry..23..740I. doi:10.1107/S0365110X67003639.
  15. ^ Grossmann, R.; Maier, H.; Szerypo, J.; Friebel, H. (2008). "Preparation of 231Pa targets". Nuclear Instruments and Methods in Physics Research A. 590 (1–3): 122. Bibcode:2008NIMPA.590..122G. doi:10.1016/j.nima.2008.02.084.
  16. ^ Greenwood, p. 1270
  17. ^ a b c Greenwood, p. 1271
  18. ^ Greenwood, p. 1275
  19. ^ Asprey, L. B.; Kruse, F. H.; Rosenzweig, A.; Penneman, R. A. (1966). "Synthesis and X-Ray Properties of Alkali Fluoride-Protactinium Pentafluoride Complexes". Inorganic Chemistry. 5 (4): 659. doi:10.1021/ic50038a034.
  20. ^ Greenwood, p. 1277
  21. ^ Greenwood, pp. 1278–1279
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