Americium compounds are compounds containing the element americium (Am). These compounds can form in the +2, +3, and +4, although the +3 oxidation state is the most common. The +5, +6 and +7 oxidation states have also been reported.

Oxides

Three americium oxides are known, with the oxidation states +2 (AmO), +3 (Am2O3), and +4 (AmO2). Americium(II) oxide was prepared in minute amounts and has not been characterized in detail.[1] Americium(III) oxide is a red-brown solid with a melting point of 2205 °C.[2] Americium(IV) oxide is the main form of solid americium which is used in nearly all its applications. Like most other actinide dioxides, it is a black solid with a cubic (fluorite) crystal structure.[3]

The oxalate of americium(III), vacuum dried at room temperature, has the chemical formula Am2(C2O4)3·7H2O. Upon heating in vacuum, it loses water at 240 °C and starts decomposing into AmO2 at 300 °C, the decomposition completes at about 470 °C.[4] The initial oxalate dissolves in nitric acid with the maximum solubility of 0.25 g/L.[5]

Halides

Halides of americium are known for the oxidation states +2, +3, and +4,[6] where the +3 is most stable, especially in solutions.[7]

Oxidation state F Cl Br I
+4 Americium(IV) fluoride
AmF4
pale pink
+3 Americium(III) fluoride
AmF3
pink		 Americium(III) chloride
AmCl3
pink		 Americium(III) bromide
AmBr3
light yellow		 Americium(III) iodide
AmI3
light yellow
+2 Americium(II) chloride
AmCl2
black		 Americium(II) bromide
AmBr2
black		 Americium(II) iodide
AmI2
black

Reduction of Am(III) compounds with sodium amalgam yields Am(II) salts – the black halides AmCl2, AmBr2, and AmI2. They are very sensitive to oxygen and oxidize in water, releasing hydrogen and converting back to the Am(III) state. Specific lattice constants are:

  • Orthorhombic AmCl2: a = 896.3±0.8 pm, b = 757.3±0.8 pm and c = 453.2±0.6 pm
  • Tetragonal AmBr2: a = 1159.2±0.4 pm and c = 712.1±0.3 pm.[8] They can also be prepared by reacting metallic americium with an appropriate mercury halide HgX2, where X = Cl, Br, or I:[9]
Am + HgX2 (mercury halide) → AmX2 + Hg (at 400–500 °C)

Americium(III) fluoride (AmF3) is poorly soluble and precipitates upon reaction of Am+3 and fluoride ions in weak acidic solutions:

Am+3 + 3F− → AmF3↓

The tetravalent americium(IV) fluoride (AmF4) is obtained by reacting solid americium(III) fluoride with molecular fluorine:[10][11]

2AmF3 + F2 → 2AmF4

Another known form of solid tetravalent americium fluoride is KAmF5.[10][12] Tetravalent americium has also been observed in the aqueous phase. For this purpose, black Am(OH)4 was dissolved in 15-M NH4F with the americium concentration of 0.01 M. The resulting reddish solution had a characteristic optical absorption spectrum which is similar to that of AmF4 but differed from other oxidation states of americium. Heating the Am(IV) solution to 90 °C did not result in its disproportionation or reduction, however a slow reduction was observed to Am(III) and assigned to self-irradiation of americium by alpha particles.[13]

Most americium(III) halides form hexagonal crystals with slight variation of the color and exact structure between the halogens. So, chloride (AmCl3) is reddish and has a structure isotypic to uranium(III) chloride (space group P63/m) and the melting point of 715 °C.[6] The fluoride is isotypic to LaF3 (space group P63/mmc) and the iodide to BiI3 (space group R3). The bromide is an exception with the orthorhombic PuBr3-type structure and space group Cmcm.[7] Crystals of americium chloride hexahydrate (AmCl3·6H2O) can be prepared by dissolving americium dioxide in hydrochloric acid and evaporating the liquid. Those crystals are hygroscopic and have yellow-reddish color and a monoclinic crystal structure.[14]

Oxyhalides of americium in the form AmVIO2X2, AmVO2X, AmIVOX2, and AmIIIOX can be obtained by reacting the corresponding americium halide with oxygen or Sb2O3, and AmOCl can also be produced by vapor phase hydrolysis:[9]

AmCl3 + H2O → AmOCl + 2HCl

Other inorganic compounds

Hydroxide

The only known hydroxide of americium is Am(OH)3, which is the first compound of americium, discovered in 1944 as part of the Manhattan project. Americium hydroxide is a pink solid[15] which is sparingly soluble in water.[16]

Due to self-irradiation, the crystal structure of 241Am(OH)3 decomposes within 4 to 6 months (241Am has a half-life of 432.2 years); for 244Cm(OH)3 the same process takes less than a day (244Cm has a half-life of 18.11 years).[15]

When ozone is bubbled through a slurry of americium(III) hydroxide in 0.03 M potassium bicarbonate at 92 °C, hexagonal KAmO2CO3 (potassium dioxoamericium(V) carbonate) can be obtained. Potassium carbonate can also be used. The resulting KAmO2CO3 reacts with dilute acids to produce americium dioxide:[17]

O3 + Am(OH)3 + KHCO3 + H2O → KAmO2CO3 + 3H2O + O2

Chalcogenides and pnictides

The known chalcogenides of americium include the sulfide AmS2,[18] selenides AmSe2 and Am3Se4,[18][19] and tellurides Am2Te3 and AmTe2.[20] The pnictides of americium (243Am) of the AmX type are known for the elements phosphorus, arsenic,[21] antimony, and bismuth. They crystallize in the rock-salt lattice.[19]

Silicides and borides

Americium monosilicide (AmSi) and "disilicide" (nominally AmSix, with 1.87 < x < 2.0) were obtained by reduction of americium(III) fluoride with elementary silicon in vacuum at 1050 °C (AmSi) and 1150−1200 °C (AmSix). AmSi is a black solid isomorphic with LaSi, it has an orthorhombic crystal symmetry. AmSix has a bright silvery lustre and a tetragonal crystal lattice (space group I41/amd), it is isomorphic with PuSi2 and ThSi2.[22] Borides of americium include AmB4 and AmB6. The tetraboride can be obtained by heating an oxide or halide of americium with magnesium diboride in vacuum or inert atmosphere.[23][24]

Organoamericium compounds

Predicted structure of amerocene, (η8-C8H8)2Am

Analogous to uranocene, americium forms the organometallic compound amerocene with two cyclooctatetraene ligands, with the chemical formula (η8-C8H8)2Am,[25] but it is still hypothetical up to date. An anionic complex KAm(COT)2 can be prepared by reacting K2COT and AmI3 in THF.[26] A cyclopentadienyl complex is also known that is likely to be stoichiometrically AmCp3.[27][28]

Formation of the complexes of the type Am(n−C3H7−BTP)3, where BTP stands for 2,6-di(1,2,4-triazin-3-yl)pyridine, in solutions containing n−C3H7−BTP− and Am+3 ions has been confirmed by EXAFS. Some of these BTP-type complexes selectively interact with americium and therefore are useful in its selective separation from lanthanides and another actinides.[29]

See also

References

  1. ↑ Akimoto, Y. (1967). "A note on AmN and AmO". Journal of Inorganic and Nuclear Chemistry. 29 (10): 2650–2652. doi:10.1016/0022-1902(67)80191-X.
  2. ↑ Wiberg, p. 1972
  3. ↑ Greenwood, p. 1267
  4. ↑ Penneman, p. 4
  5. ↑ Penneman, p. 5
  6. 1 2 Wiberg, p. 1969
  7. 1 2 Asprey, L. B.; Keenan, T. K.; Kruse, F. H. (1965). "Crystal Structures of the Trifluorides, Trichlorides, Tribromides, and Triiodides of Americium and Curium". Inorganic Chemistry. 4 (7): 985. doi:10.1021/ic50029a013. S2CID 96551460.
  8. ↑ Baybarz, R. D. (1973). "The preparation and crystal structures of americium dichloride and dibromide". Journal of Inorganic and Nuclear Chemistry. 35 (2): 483. doi:10.1016/0022-1902(73)80560-3.
  9. 1 2 Greenwood, p. 1272
  10. 1 2 Asprey, L. B. (1954). "New Compounds of Quadrivalent Americium, AmF4, KAmF5". Journal of the American Chemical Society. 76 (7): 2019. doi:10.1021/ja01636a094.
  11. ↑ Greenwood, p. 1271
  12. ↑ Penneman, p. 6
  13. ↑ Asprey, L. B.; Penneman, R. A. (1961). "First Observation of Aqueous Tetravalent Americium1". Journal of the American Chemical Society. 83 (9): 2200. doi:10.1021/ja01470a040.
  14. ↑ Burns, John H.; Peterson, Joseph Richard (1971). "Crystal structures of americium trichloride hexahydrate and berkelium trichloride hexahydrate". Inorganic Chemistry. 10: 147. doi:10.1021/ic50095a029.
  15. 1 2 Krivovichev, Sergey; Burns, Peter; Tananaev, Ivan (2006). Structural Chemistry of Inorganic Actinide Compounds. Elsevier. p. 67. ISBN 978-0-08-046791-7.
  16. ↑ Runde, Wolfgang (2011), "Americium and Curium: Radionuclides", Encyclopedia of Inorganic and Bioinorganic Chemistry, American Cancer Society, doi:10.1002/9781119951438.eibc0438, ISBN 978-1-119-95143-8, retrieved 2020-03-21
  17. ↑ Penneman, R. A.; Keenan, T. K. (1960-01-01). The Radiochemistry of Americium and Curium (Technical report). doi:10.2172/4187189. OSTI 4187189.
  18. 1 2 Damien, D.; Jove, J. (1971). "Americium disulfide and diselenide". Inorganic and Nuclear Chemistry Letters. 7 (7): 685. doi:10.1016/0020-1650(71)80055-7.
  19. 1 2 Roddy, J. (1974). "Americium metallides: AmAs, AmSb, AmBi, Am3Se4, and AmSe2". Journal of Inorganic and Nuclear Chemistry. 36 (11): 2531. doi:10.1016/0022-1902(74)80466-5.
  20. ↑ Damien, D. (1972). "Americium tritelluride and ditelluride". Inorganic and Nuclear Chemistry Letters. 8 (5): 501. doi:10.1016/0020-1650(72)80262-9.
  21. ↑ Charvillat, J.; Damien, D. (1973). "Americium monoarsenide". Inorganic and Nuclear Chemistry Letters. 9 (5): 559. doi:10.1016/0020-1650(73)80191-6.
  22. ↑ Weigel, F.; Wittmann, F.; Marquart, R. (1977). "Americium monosilicide and "disilicide"". Journal of the Less Common Metals. 56: 47. doi:10.1016/0022-5088(77)90217-X.
  23. ↑ Lupinetti, A. J. et al. U.S. Patent 6,830,738 "Low-temperature synthesis of actinide tetraborides by solid-state metathesis reactions", Filed 4 Apr 2002, Issued 14 December 2004
  24. ↑ Eick, Harry A.; Mulford, R. N. R. (1969). "Americium and neptunium borides". Journal of Inorganic and Nuclear Chemistry. 31 (2): 371. doi:10.1016/0022-1902(69)80480-X.
  25. ↑ Elschenbroich, Christoph (2008). Organometallchemie. Vieweg+teubner Verlag. p. 589. ISBN 978-3-8351-0167-8.
  26. ↑ Mueller, Werner; Lindner, Roland. Potassium bis(cyclooctatetraenyl)americium(III). Transplutonium 1975, Proc. Int. Transplutionium Elem. Symp., 4th [Conference]. 1976. pp 131-137.
  27. ↑ Albrecht-Schmitt, Thomas E. (2008). Organometallic and Coordination Chemistry of the Actinides. Springer. p. 8. ISBN 978-3-540-77836-3.
  28. ↑ Dutkiewicz, Michał S.; Apostolidis, Christos; Walter, Olaf; Arnold, Polly L. (30 January 2017). "Reduction chemistry of neptunium cyclopentadienide complexes: from structure to understanding". Chemical Science. 2017 (8): 2553–61. doi:10.1039/C7SC00034K. PMC 5431675. PMID 28553487.
  29. ↑ Girnt, Denise; Roesky, Peter W.; Geist, Andreas; Ruff, Christian M.; Panak, Petra J.; Denecke, Melissa A. (2010). "6-(3,5-Dimethyl-1H-pyrazol-1-yl)-2,2'-bipyridine as Ligand for Actinide(III)/Lanthanide(III) Separation" (PDF). Inorganic Chemistry. 49 (20): 9627–35. doi:10.1021/ic101309j. PMID 20849125.
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.