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a short-lived radioactive metallic element formed from uranium and disintegrating into actinium and then into lead (同)protoactinium, Pa, atomic number 91

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プロトアクチニウム(放射性金属元素;化学記号は『Pa』)
protactiniumの化学記号

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出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2016/05/09 06:49:39」(JST)

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Protactinium or protoactinium (former name) is a chemical element with symbol Pa and atomic number 91. It is a dense, silvery-gray metal which readily reacts with oxygen, water vapor and inorganic acids. It forms various chemical compounds where protactinium is usually present in the oxidation state +5, but can also assume +4 and even +2 or +3 states. The average concentrations of protactinium in the Earth's crust is typically on the order of a few parts per trillion, but may reach up to a few parts per million in some uraninite ore deposits. Because of its scarcity, high radioactivity and high toxicity, there are currently no uses for protactinium outside of scientific research, and for this purpose, protactinium is mostly extracted from spent nuclear fuel.

Protactinium was first identified in 1913 by Kasimir Fajans and Oswald Helmuth Göhring and named brevium because of the short half-life of the specific isotope studied, namely protactinium-234. A more stable isotope (²³¹Pa) of protactinium was discovered in 1917/18 by Otto Hahn and Lise Meitner, and they chose the name proto-actinium, but then the IUPAC named it finally protactinium in 1949 and confirmed Hahn and Meitner as discoverers. The new name meant "parent of actinium" and reflected the fact that actinium is a product of radioactive decay of protactinium. It is noted that John Arnold Cranston (working with Frederick Soddy and Ada Hitchins) is also credited with discovering the stable isotope in 1915 but delayed his announcement due to being called up for service in the First World War.^[5]

The longest-lived and most abundant (nearly 100%) naturally occurring isotope of protactinium, protactinium-231, has a half-life of 32,760 years and is a decay product of uranium-235. Much smaller trace amounts of the short-lived nuclear isomer protactinium-234m occur in the decay chain of uranium-238. Protactinium-233 results from the decay of thorium-233 as part of the chain of events used to produce uranium-233 by neutron irradiation of thorium-232. It is an undesired intermediate product in thorium-based nuclear reactors and is therefore removed from the active zone of the reactor during the breeding process. Analysis of the relative concentrations of various uranium, thorium and protactinium isotopes in water and minerals is used in radiometric dating of sediments which are up to 175,000 years old and in modeling of various geological processes.

1 History
2 Isotopes
3 Occurrence
- 3.1 In nuclear reactors
4 Preparation
5 Physical and chemical properties
6 Chemical compounds
- 6.1 Oxides and oxygen-containing salts
- 6.2 Halides
- 6.3 Other inorganic compounds
- 6.4 Organometallic compounds
7 Applications
8 Precautions
9 See also
10 References
11 Bibliography
12 External links

History

In 1871, Dmitri Mendeleev predicted the existence of an element between thorium and uranium.^[6] The actinide element group was unknown at the time. Therefore, uranium was positioned below tungsten, and thorium below zirconium, leaving the space below tantalum empty and, until the 1950s, periodic tables were published with this structure.^[7] For a long time chemists searched for eka-tantalum as an element with similar chemical properties to tantalum, making a discovery of protactinium nearly impossible. Tantalum's heavier analogue was later found to be the transuranic element dubnium.

In 1900, William Crookes isolated protactinium as an intensely radioactive material from uranium; however, he could not characterize it as a new chemical element and thus named it uranium-X (UX).^[6]^[8]^[9] Crookes dissolved uranium nitrate in ether, the residual aqueous phase contains most of the 234
90Th and 234
91Pa. His method was still used in the 1950s to isolate 234
90Th and 234
91Pa from uranium compounds.^[10] Protactinium was first identified in 1913, when Kasimir Fajans and Oswald Helmuth Göhring encountered the isotope ²³⁴Pa during their studies of the decay chains of uranium-238: 238
92U → 234
90Th → 234
91Pa → 234
92U. They named the new element brevium (from the Latin word, brevis, meaning brief or short) because of its short half-life, 6.7 hours for 234
91Pa.^[11]^[12]^[13]^[14] In 1917/18, two groups of scientists, Otto Hahn and Lise Meitner of Germany and Frederick Soddy and John Cranston of Great Britain, independently discovered another isotope of protactinium, ²³¹Pa having much longer half-life of about 32,000 years. Thus the name brevium was changed to protoactinium as the new element was part of the decay chain of uranium-235 before the actinium (from Greek: πρῶτος = protos meaning first, before). For ease of pronunciation, the name was shortened to protactinium by the IUPAC in 1949.^[15]^[16] The discovery of protactinium completed one of the last gaps in the early versions of the periodic table, proposed by Mendeleev in 1869, and it brought to fame the involved scientists.^[17]

Aristid von Grosse produced 2 milligrams of Pa₂O₅ in 1927,^[18] and in 1934 first isolated elemental protactinium from 0.1 milligrams of Pa₂O₅.^[19] He used two different procedures: in the first one, protactinium oxide was irradiated by 35 keV electrons in vacuum. In another method, called the van Arkel–de Boer process, the oxide was chemically converted to a halide (chloride, bromide or iodide) and then reduced in a vacuum with an electrically heated metallic filament:^[15]^[20]

2 PaI₅ → 2 Pa + 5 I₂

In 1961, the United Kingdom Atomic Energy Authority (UKAEA) produced 125 grams of 99.9% pure protactinium by processing 60 tonnes of waste material in a 12-stage process, at a cost of about 500,000 USD.^[15] For many years, this was the world's only significant supply of protactinium, which was provided to various laboratories for scientific studies.^[6] Oak Ridge National Laboratory in the US provided protactinium at a cost of about 280 USD/gram.^[21]

Mendeleev's 1871 periodic table with a gap for protactinium on the bottom row of the chart, between thorium and uranium

Isotopes

Twenty-nine radioisotopes of protactinium have been discovered, the most stable being ²³¹Pa with a half-life of 32,760 years, ²³³Pa with a half-life of 27 days, and ²³⁰Pa with a half-life of 17.4 days. All of the remaining isotopes have half-lives shorter than 1.6 days, and the majority of these have half-lives less than 1.8 seconds. Protactinium also has two nuclear isomers, ^217mPa (half-life 1.2 milliseconds) and ^234mPa (half-life 1.17 minutes).^[22]

The primary decay mode for isotopes of protactinium lighter than (and including) the most stable isotope ²³¹Pa (i.e., ²¹²Pa to ²³¹Pa) is alpha decay and the primary mode for the heavier isotopes (i.e., ²³²Pa to ²⁴⁰Pa) is beta decay. The primary decay products of isotopes of protactinium lighter than (and including) ²³¹Pa are actinium isotopes and the primary decay products for the heavier isotopes of protactinium are uranium isotopes.^[22]

Occurrence

Protactinium is one of the rarest and most expensive naturally occurring elements. It is found in the form of two isotopes – ²³¹Pa and ²³⁴Pa, with the isotope ²³⁴Pa occurring in two different energy states. Nearly all natural protactinium is protactinium-231. It is an alpha emitter and is formed by the decay of uranium-235, whereas the beta radiating protactinium-234 is produced as a result of uranium-238 decay. Nearly all uranium-238 (99.8%) decays first to the ^234mPa isomer.^[23]

Protactinium occurs in uraninite (pitchblende) at concentrations of about 0.3-3 parts ²³¹Pa per million parts (ppm) of ore.^[6] Whereas the usual content is closer to 0.3 ppm^[24] (e.g. in Jáchymov, Czech Republic^[25]), some ores from the Democratic Republic of the Congo have about 3 ppm.^[15] Protactinium is homogeneously dispersed in most natural materials and in water, but at much lower concentrations on the order of one part per trillion, that corresponds to the radioactivity of 0.1 picocuries (pCi)/g. There is about 500 times more protactinium in sandy soil particles than in water, even the water present in the same sample of soil. Much higher ratios of 2,000 and above are measured in loam soils and clays, such as bentonite.^[23]^[26]

In nuclear reactors

Two major protactinium isotopes, ²³¹Pa and ²³³Pa, are produced from thorium in nuclear reactors; both are undesirable and are usually removed, thereby adding complexity to the reactor design and operation. In particular, ²³²Th via (n,2n) reactions produces ²³¹Th which quickly (half-life 25.5 hours) decays to ²³¹Pa. The last isotope, while not a transuranic waste, has a long half-life of 32,760 years and is a major contributor to the long term radiotoxicity of spent nuclear fuel.^[27]

Protactinium-233 is formed upon neutron capture by ²³²Th. It further either decays to uranium-233 or captures another neutron and converts into the non-fissile uranium-234.^[28] ²³³Pa has a relatively long half-life of 27 days and high cross section for neutron capture (the so-called "neutron poison"). Thus instead of rapidly decaying to the useful ²³³U, a significant fraction of ²³³Pa converts to non-fissile isotopes and consumes neutrons, degrading the reactor efficiency. To avoid this, ²³³Pa is extracted from the active zone of thorium molten salt reactors, during their operation, so that it only decays to ²³³U. This is achieved using several meters tall columns of molten bismuth with lithium dissolved in it. In a simplified scenario, lithium selectively reduces protactinium salts to protactinium metal which is then extracted from the molten-salt cycle, and bismuth is merely a carrier. It is chosen because of its low melting point (271 °C), low vapor pressure, good solubility for lithium and actinides, and immiscibility with molten halides.^[27]

Preparation

Protactinium occurs in uraninite ores.

Before the advent of nuclear reactors, protactinium was separated for scientific experiments from uranium ores. Nowadays, it is mostly produced as an intermediate product of nuclear fission in thorium high-temperature reactors:

The times are half-lives.

Protactinium metal can be prepared by reduction of its fluoride with calcium fluoride,^[29] lithium or barium at a temperature of 1300–1400 °C.^[30]^[31]

Physical and chemical properties

Protactinium is an actinide which is positioned in the periodic table to the left of uranium and to the right of thorium, and many of its physical properties are intermediate between those two actinides. So, protactinium is more dense and rigid than thorium but is lighter than uranium, and its melting point is lower than that of thorium and higher than that of uranium. The thermal expansion, electrical and thermal conductivities of these three elements are comparable and are typical of post-transition metals. The estimated shear modulus of protactinium is similar to that of titanium.^[32] Protactinium is a metal with silvery-gray luster that is preserved for some time in air.^[15]^[33] Protactinium easily reacts with oxygen, water vapor and acids, but not with alkalis.^[6]

At room temperature, protactinium crystallizes in body-centered tetragonal structure which can be regarded as distorted body-centered cubic lattice; this structure does not change upon compression up to 53 GPa. The structure changes to face-centered cubic (fcc) upon cooling from high temperature, at about 1200 °C.^[29]^[34] The thermal expansion coefficient of the tetragonal phase between room temperature and 700 °C is 9.9×10⁻⁶/°C.^[29]

Protactinium is paramagnetic and no magnetic transitions are known for it at any temperature.^[35] It becomes superconductive at temperatures below 1.4 K.^[6]^[30] Protactinium tetrachloride is paramagnetic at room temperature but turns ferromagnetic upon cooling to 182 K.^[36]

Protactinium exists in two major oxidation states, +4 and +5, both in solids and solutions, and the +3 and +2 states were observed in some solid phases. As the electron configuration of the neutral atom is [Rn]5f²6d¹7s², the +5 oxidation state corresponds to the low-energy (and thus favored) 5f⁰ configuration. Both +4 and +5 states easily form hydroxides in water with the predominant ions being Pa(OH)³⁺, Pa(OH)2+
2, Pa(OH)+
3 and Pa(OH)₄, all colorless.^[37] Other known protactinium ions include PaCl2+
2, PaSO2+
4, PaF³⁺, PaF2+
2, PaF−
6, PaF2−
7 and PaF3−
8.^[38]^[39]

Chemical compounds

Formula	color	symmetry	space group	No	Pearson symbol	a (pm)	b (pm)	c (pm)	Z	density, g/cm³
Pa	silvery-gray	tetragonal^[2]	I4/mmm	139	tI2	392.5	392.5	323.8	2	15.37
PaO		rocksalt^[31]	Fm3m	225	cF8	496.1			4	13.44
PaO₂	black	fcc^[31]	Fm3m	225	cF12	550.5			4	10.47
Pa₂O₅	white		Fm3m^[31]	225	cF16	547.6	547.6	547.6	4	10.96
Pa₂O₅	white		orthorhombic^[31]			692	402	418
PaH₃	black	cubic^[31]	Pm3n	223	cP32	664.8	664.8	664.8	8	10.58
PaF₄	brown-red	monoclinic^[31]	C2/c	15	mS60				2
PaCl₄	green-yellow	tetragonal^[40]	I4₁/amd	141	tI20	837.7	837.7	748.1	4	4.72
PaBr₄	brown	tetragonal^[41]^[42]	I4₁/amd	141	tI20	882.4	882.4	795.7
PaCl₅	yellow	monoclinic^[43]	C2/c	15	mS24	797	1135	836	4	3.74
PaBr₅	red	monoclinic^[42]^[44]	P2₁/c	14	mP24	838.5	1120.5	1214.6	4	4.98
PaOBr₃		monoclinic^[42]	C2			1691.1	387.1	933.4
Pa(PO₃)₄		orthorhombic^[45]				696.9	895.9	1500.9
Pa₂P₂O₇		cubic^[45]	Pa3			865	865	865
Pa(C₈H₈)₂	golden-yellow	monoclinic^[46]				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

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.^[47] Its crystal structure is cubic, and the chemical composition is often non-stoichiometric, described as PaO_2.25. Another phase of this oxide with orthorhombic symmetry has also been reported.^[31]^[48] 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.^[31] The dioxide can be converted back to pentoxide by heating in oxygen-containing atmosphere to 1100 °C.^[48] The monoxide PaO has only been observed as a thin coating on protactinium metal, but not in an isolated bulk form.^[31]

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 for a hexagonal close-packed lattice. In all these materials, protactinium ions are octahedrally coordinated.^[49]^[50] The pentoxide Pa₂O₅ combines with rare-earth metal oxides R₂O₃ to form various nonstoichiometric mixed-oxides, also of perovskite structure.^[51]

Protactinium oxides are basic; they easily convert to hydroxides and can form various salts, such as sulfates, phosphates, nitrates, etc. The 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.^[52] 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 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 C_2v symmetry. Heating PaP₂O₇ in air to 1400 °C decomposes it into the pentoxides of phosphorus and protactinium.^[45]

Halides

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.^[53]

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.^[54] 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.^[31]

Protactinium(V) chloride is prepared by reacting protactinium oxide with carbon tetrachloride at temperature of 200–300 °C.^[31] The by-products (such as PaOCl₃) are removed by fractional sublimation.^[43] 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.^[31]

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.^[31] 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.^[42]^[44]

Protactinium iodides result from the oxides and aluminium iodide or ammonium iodide heated to 600 °C.^[31] Protactinium(III) iodide was obtained by heating protactinium(V) iodide in vacuum.^[54] 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.^[38]

More complex protactinium fluorides are also known such as Pa₂F₉^[54] 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).^[39]

Other inorganic compounds

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.^[42] 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.^[31]

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.^[31] 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.^[55]

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

Organometallic compounds

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.^[56] 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.^[46]

Applications

Although protactinium is located in the periodic table between uranium and thorium, which both have numerous applications, owing to its scarcity, high radioactivity and high toxicity, there are currently no uses for protactinium outside of scientific research.^[23]

Protactinium-231 arises from the decay of uranium-235 formed in nuclear reactors, and by the reaction ²³²Th + n → ²³¹Th + 2n and subsequent beta decay. It was once thought to be able to support a nuclear chain reaction, which could in principle be used to build nuclear weapons: the physicist Walter Seifritz (de) once estimated the associated critical mass as 7002750000000000000♠750±180 kg.^[57] However, the possibility of criticality of ²³¹Pa has been ruled out since then.^[58]

With the advent of highly sensitive mass spectrometers, an application of ²³¹Pa as a tracer in geology and paleoceanography has become possible. So, the ratio of protactinium-231 to thorium-230 is used for radiometric dating of sediments which are up to 175,000 years old and in modeling of the formation of minerals.^[24] In particular, its evaluation in oceanic sediments allowed to reconstruct the movements of North Atlantic water bodies during the last melting of Ice Age glaciers.^[59] Some of the protactinium-related dating variations rely on the analysis of the relative concentrations for several long-living members of the uranium decay chain – uranium, thorium and protactinium, for example. These elements have 6, 5 and 4 f-electrons in the outer shell and thus favor +6, +5 and +4 oxidation states, respectively, and show different physical and chemical properties. So, thorium and protactinium, but not uranium compounds are poorly soluble in aqueous solutions, and precipitate into sediments; the precipitation rate is faster for thorium than for protactinium. Besides, the concentration analysis for both protactinium-231 (half-life 32,760 years) and thorium-230 (half-life 75,380 years) allows to improve the accuracy compared to when only one isotope is measured; this double-isotope method is also weakly sensitive to inhomogeneities in the spatial distribution of the isotopes and to variations in their precipitation rate.^[24]^[60]

Precautions

Protactinium is both toxic and highly radioactive and thus all manipulations with it are performed in a sealed glove box. Its major isotope ²³¹Pa has a specific activity of 0.048 curies (1.8 GBq) per gram and primarily emits alpha-particles with an energy of 5 MeV, which can be stopped by a thin layer of any material. However, it slowly decays, with a half-life of 32,760 years, into ²²⁷Ac, which has a specific activity of 74 curies (2,700 GBq) per gram, emits both alpha and beta radiation, and has a much shorter half-life of 22 years. ²²⁷Ac, in turn, decays into lighter isotopes with even shorter half-lives and much greater specific activities (SA), as summarized in the table below showing the decay chain of protactinium-231.^[23]

Isotope	²³¹Pa	²²⁷Ac	²²⁷Th	²²³Ra	²¹⁹Rn	²¹⁵Po	²¹¹Pb	²¹¹Bi	²⁰⁷Tl
SA (Ci/g)	0.048	73	3.1×10⁴	5.2×10⁴	1.3×10¹⁰	3×10¹³	2.5×10⁷	4.2×10⁸	1.9×10⁸
Decay	α	α, β	α	α	α	α	β	α, β	β
Half-life	33 ka	22 a	19 days	11 days	4 s	1.8 ms	36 min	2.1 min	4.8 min

As protactinium is present in small amounts in most natural products and materials, it is ingested with food or water and inhaled with air. Only about 0.05% of ingested protactinium is absorbed into the blood and the remainder is excreted. From the blood, about 40% of the protactinium deposits in the bones, about 15% goes to the liver, 2% to the kidneys, and the rest leaves the body. The biological half-life of protactinium is about 50 years in the bones, whereas in other organs the kinetics has a fast and slow component. So in the liver 70% of protactinium have a half-life of 10 days and 30% remain for 60 days. The corresponding values for kidneys are 20% (10 days) and 80% (60 days). In all these organs, protactinium promotes cancer via its radioactivity.^[23]^[52] The maximum safe dose of Pa in the human body is 0.03 µCi (1.1 kBq), which corresponds to 0.5 micrograms of ²³¹Pa. This isotope is 2.5×10⁸ times more toxic than hydrocyanic acid.^[61] The maximum allowed concentrations of ²³¹Pa in the air in Germany is 6996300000000000000♠3×10⁻⁴ Bq/m³.^[52]

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^ Shea, William R. (1983) Otto Hahn and the rise of nuclear physics, Springer, p. 213, ISBN 90-277-1584-X.
^ von Grosse, Aristid (1928). "Das Element 91; seine Eigenschaften und seine Gewinnung". Berichte der deutschen chemischen Gesellschaft 61 (1): 233–245. doi:10.1002/cber.19280610137.
^ Graue, G.; Käding, H. (1934). "Die technische Gewinnung des Protactiniums". Angewandte Chemie 47 (37): 650–653. doi:10.1002/ange.19340473706.
^ Grosse, A. V. (1934). "Metallic Element 91". Journal of the American Chemical Society 56 (10): 2200. doi:10.1021/ja01325a508.
^ Protactinium at the Wayback Machine (archived September 28, 2011) from Los Alamos National Laboratory.
^ ^a ^b Audi, G; Bersillon, O.; Blachot, J.; Wapstra, A.H. (2003). "The NUBASE evaluation of nuclear and decay properties" (PDF). Nuclear Physics A 729: 3. Bibcode:2003NuPhA.729....3A. doi:10.1016/j.nuclphysa.2003.11.001.
^ ^a ^b ^c ^d ^e Protactinium, Argonne National Laboratory, Human Health Fact Sheet, August 2005
^ ^a ^b ^c Articles "Protactinium" and "Protactinium-231 – thorium-230 dating" in Encyclopædia Britannica, 15th edition, 1995, p. 737
^ Grosse, A. V.; Agruss, M. S. (1934). "The Isolation of 0.1 Gram of the Oxide of Element 91 (Protactinium)". Journal of the American Chemical Society 56 (10): 2200. doi:10.1021/ja01325a507.
^ Cornelis, Rita (2005) Handbook of elemental speciation II: species in the environment, food, medicine & occupational health, Vol. 2, John Wiley and Sons, pp. 520–521, ISBN 0-470-85598-3.
^ ^a ^b Groult, Henri (2005) Fluorinated materials for energy conversion, Elsevier, pp. 562–565, ISBN 0-08-044472-5.
^ Hébert, Alain (July 2009). Applied Reactor Physics. Presses inter Polytechnique. pp. 265–. ISBN 978-2-553-01436-9.
^ ^a ^b ^c Marples, J. A. C. (1965). "On the thermal expansion of protactinium metal". Acta Crystallographica 18 (4): 815. doi:10.1107/S0365110X65001871.
^ ^a ^b Fowler, R. D.; Matthias, B.; Asprey, L.; Hill, H.; et al. (1965). "Superconductivity of Protactinium". Phys. Rev. Lett. 15 (22): 860. Bibcode:1965PhRvL..15..860F. doi:10.1103/PhysRevLett.15.860.
^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m ⁿ ^o ^p ^q 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.
^ Seitz, Frederick and Turnbull, David (1964) Solid state physics: advances in research and applications, Academic Press, pp. 289–291, ISBN 0-12-607716-9.
^ Myasoedov, B. F.; Kirby, H. W.; Tananaev, I. G. (2006). "Chapter 4: Protactinium". In Morss, L. R.; Edelstein, N. M.; Fuger, J. The Chemistry of the Actinide and Transactinide Elements (3rd ed.). Dordrecht, The Netherlands: Springer. ISBN 978-1-4020-3555-5.
^ Young, David A. (1991) Phase diagrams of the elements, University of California Press, p. 222, ISBN 0-520-07483-1.
^ Buschow, K. H. J. (2005) Concise encyclopedia of magnetic and superconducting materials, Elsevier, pp. 129–130, ISBN 0-08-044586-1.
^ Hendricks, M. E. (1971). "Magnetic Properties of Protactinium Tetrachloride". The Journal of Chemical Physics 55 (6): 2993. Bibcode:1971JChPh..55.2993H. doi:10.1063/1.1676528.
^ Greenwood, p. 1265
^ ^a ^b Greenwood, p. 1275
^ ^a ^b 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.
^ 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)". J. Chem. Soc., Dalton Trans (6): 686–691. doi:10.1039/DT9730000686.
^ 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. doi:10.1016/0022-5088(90)90436-N.
^ ^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.
^ ^a ^b Dodge, R. P.; Smith, G. S.; Johnson, Q.; Elson, R. E. (1967). "The crystal structure of protactinium pentachloride". Acta Crystallogr 22: 85–89. doi:10.1107/S0365110X67000155.
^ ^a ^b Brown, D.; Petcher, T. J.; Smith, A. J. (1969). "The crystal structure of β-protactinium pentabromide". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry 25 (2): 178. doi:10.1107/S0567740869007357.
^ ^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.
^ ^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.
^ Greenwood, p. 1268
^ ^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.
^ Greenwood, p. 1269
^ Iyer, P. N.; Smith, A. J. (1971). "Double oxides containing niobium, tantalum or protactinium. IV. Further systems involving alkali metals". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry 27 (4): 731. doi:10.1107/S056774087100284X.
^ 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. doi:10.1107/S0365110X67003639.
^ ^a ^b ^c Grossmann, R; Maier, H; Szerypo, J; Friebel, H (2008). "Preparation of 231Pa targets". Nuclear Instruments and Methods in Physics Research Section A: Accelerators, Spectrometers, Detectors and Associated Equipment 590: 122. Bibcode:2008NIMPA.590..122G. doi:10.1016/j.nima.2008.02.084.
^ Greenwood, p. 1270
^ ^a ^b ^c Greenwood, p. 1271
^ Greenwood, p. 1277
^ Greenwood, pp. 1278–1279
^ Seifritz, Walter (1984) Nukleare Sprengkörper – Bedrohung oder Energieversorgung für die Menschheit, Thiemig-Verlag, ISBN 3-521-06143-4.
^ Ganesan, S. (1999). "A Re-calculation of Criticality Property of ²³¹Pa Using New Nuclear Data" (PDF). Current Science 77 (5): 667–677.
^ McManus, J. F.; Francois, R.; Gherardi, J.-M.; Keigwin, L. D.; et al. (2004). "Collapse and rapid resumption of Atlantic meridional circulation linked to deglacial climate changes" (PDF). Nature 428 (6985): 834–837. Bibcode:2004Natur.428..834M. doi:10.1038/nature02494. PMID 15103371.
^ Cheng, H; Edwards, R.Lawrence; Murrell, M.T.; Benjamin, T.M. (1998). "Uranium-thorium-protactinium dating systematics". Geochimica et Cosmochimica Acta 62 (21–22): 3437. Bibcode:1998GeCoA..62.3437C. doi:10.1016/S0016-7037(98)00255-5.
^ Palshin, E.S.; et al. (1968). Analytical chemistry of protactinium. Moscow: Nauka.

Bibliography

Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth–Heinemann. ISBN 0080379419.

External links

Protactinium at The Periodic Table of Videos (University of Nottingham)

English Journal

Elucidating Protactinium Hydrolysis: The Relative Stabilities of PaO2(H2O)(+) and PaO(OH)2(+).

Dau PD1, Wilson RE2, Gibson JK1.
Inorganic chemistry.Inorg Chem.2015 Aug 3;54(15):7474-80. doi: 10.1021/acs.inorgchem.5b01078. Epub 2015 Jul 23.
It is demonstrated that the gas-phase oxo-exchange of PaO2(+) with water is substantially faster than that of UO2(+), indicating that the Pa-O bonds are more susceptible to activation and formation of the bis-hydroxide intermediate, PaO(OH)2(+). To elucidate the nature of the water adduct of PaO2(+)
PMID 26203499

The strength of actinide-element bonds from the quantum theory of atoms-in-molecules.

Huang QR1, Kingham JR, Kaltsoyannis N.
Dalton transactions (Cambridge, England : 2003).Dalton Trans.2015 Feb 14;44(6):2554-66. doi: 10.1039/c4dt02323d.
[AnX(3)](2)(μ-η(2):η(2)-N(2)) (An = Th-Pu; X = F, Cl, Br, Me, H, OPh) have been studied using relativistic density functional theory. Geometric and vibrational data suggest that metal→N(2) charge transfer maximises at the protactinium systems, which feature the longest N-N bonds and the smalles
PMID 25307773

Production of medical isotopes from a thorium target irradiated by light charged particles up to 70 MeV.

Duchemin C1, Guertin A, Haddad F, Michel N, Métivier V.
Physics in medicine and biology.Phys Med Biol.2015 Feb 7;60(3):931-46. doi: 10.1088/0031-9155/60/3/931. Epub 2015 Jan 9.
The irradiation of a thorium target by light charged particles (protons and deuterons) leads to the production of several isotopes of medical interest. Direct nuclear reaction allows the production of Protactinium-230 which decays to Uranium-230 the mother nucleus of Thorium-226, a promising isotope
PMID 25574934

EXAFS study of the speciation of protactinium(V) in aqueous hydrofluoric acid solutions.

De Sio SM1, Wilson RE.
Inorganic chemistry.Inorg Chem.2014 Dec 1;53(23):12643-9. doi: 10.1021/ic502376m. Epub 2014 Nov 12.
The speciation of protactinium(V) in hydrofluoric acid (HF) solutions was studied using X-ray absorption spectroscopy. Extended X-ray absorption fine structure measurements were performed on an aqueous solution of 0.05 M protactinium(V) with various HF concentrations ranging from 0.5 to 27 M in orde
PMID 25389749

Japanese Journal

Emission Probabilities of Gamma Rays from the Decay of 233Pa and 238Np, and the Thermal Neutron Capture Cross Section of 237Np

Harada Hideo,Nakamura Shoji,Ohta Masayuki [他]
Journal of Nuclear Science and Technology 43(11), 1289-1297, 2006-11
NAID 40015163800

Solvent Extraction Study of ^<233>Pa(V) with 1-phenyl-3-methyl-4-benzoyl-5-pyrazolone

Ding Huajie,Niu Yanning,Yang Weifan [他],XU Yanbing,YUAN Shuanggui,QIN Zhi,ZHOU Xiaohong
Journal of nuclear science and technology 42(9), 839-841, 2005-09-25
NAID 10016124710

ウランガラスからのγ線スペクトル測定

鈴木章悟,永山明彦,大井昇
日本原子力学会和文論文誌 = Transactions of the Atomic Energy Society of Japan 4(1), 1-6, 2005-03-25
Uranium glass is yellowish green glass which is produced by adding a small amount of uranium as a coloring agent into ordinary glasses. The glass has a characteristic of emitting strong fluorescent li …
NAID 10014003968

Production of Pa-U Fuel with Proliferation Resistance by 14MeV Neutron for Long-life Core

Imamura Tomo,Saito Masaki,Yoshida Tadashi [他],ARTISYUK Vladimir
Journal of nuclear science and technology 41(6), 655-664, 2004-06-25
NAID 10012627027

「Pa」

Protactinium, ₉₁Pa
General properties
Name, symbol	protactinium, Pa
Appearance	bright, silvery metallic luster
Pronunciation	/ˌproʊtækˈtɪniəm/; PROH-tak-TIN-ee-əm
Protactinium in the periodic table
	thorium ← protactinium → uranium
Atomic number (Z)	91
Group, block	group n/a, f-block
Period	period 7
Element category	actinide
Standard atomic weight (±) (Ar)	231.03588(2)
Electron configuration	[Rn] 5f2 6d1 7s2
per shell	2, 8, 18, 32, 20, 9, 2
Physical properties
Phase	solid
Melting point	1841 K (1568 °C, 2854 °F)
Boiling point	4300 K (4027 °C, 7280 °F) (?)
Density near r.t.	15.37 g/cm3
Heat of fusion	12.34 kJ/mol
Heat of vaporization	481 kJ/mol
Atomic properties
Oxidation states	2, 3, 4, 5 (a weakly basic oxide)
Electronegativity	Pauling scale: 1.5
Ionization energies	1st: 568 kJ/mol
Atomic radius	empirical: 163 pm
Covalent radius	200 pm
Miscellanea
Crystal structure	tetragonal
Thermal expansion	~9.9 µm/(m·K) (at r.t.)
Thermal conductivity	47 W/(m·K)
Electrical resistivity	177 nΩ·m (at 0 °C)
Magnetic ordering	paramagnetic
CAS Number	7440-13-3
History
Prediction	Dmitri Mendeleev (1869)
Discovery and first isolation	William Crookes (1900)
Named by	Otto Hahn and Lise Meitner (1917–8)
Most stable isotopes of protactinium
	view; talk; edit; \| references

　　[★]

「プロトアクチニウム」

　　[★]

英: protactinium、Pa
関: パスカル

[IUPAC-1] Standard Atomic Weights 2013. Commission on Isotopic Abundances and Atomic Weights

[str-2] Donohue, J. (1959). "On the crystal structure of protactinium metal". Acta Crystallographica 12 (9): 697. doi:10.1107/S0365110X59002031.

[3] Cverna, Fran, ed. (2002). "Chapter 2. Thermal Expansion". ASM Ready Reference: Thermal Properties of Metals (PDF). ASM International. p. 11. ISBN 0871707683.

[magnet-4] Lide, D. R., ed. (2005). "Magnetic susceptibility of the elements and inorganic compounds". CRC Handbook of Chemistry and Physics (PDF) (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.

[5] John Arnold Cranston. University of Glasgow

[Emsley-6] ^ ^a ^b ^c ^d ^e ^f Emsley, John (2003) [2001]. "Protactinium". Nature's Building Blocks: An A-Z Guide to the Elements. Oxford, England, UK: Oxford University Press. pp. 347–349. ISBN 0-19-850340-7.

[7] Laing, Michael (2005). "A Revised Periodic Table: With the Lanthanides Repositioned". Foundations of Chemistry 7 (3): 203. doi:10.1007/s10698-004-5959-9.

[google-8] National Research Council (U.S.). Conference on Glossary of Terms in Nuclear Science and Technology (1957). A Glossary of Terms in Nuclear Science and Technology. American Society of Mechanical Engineers. p. 180. Retrieved 25 July 2015.

[9] Crookes, W. (1899). "Radio-Activity of Uranium". Proceedings of the Royal Society of London 66: 409–423. doi:10.1098/rspl.1899.0120.

[10] Johansson, Sven (1954). "Decay of UX1, UX2, and UZ". Physical Review 96 (4): 1075. Bibcode:1954PhRv...96.1075J. doi:10.1103/PhysRev.96.1075.

[g1250-11] Greenwood, p. 1250

[g1254-12] Greenwood, p. 1254

[13] Fajans, K. & Gohring, O. (1913). "Über die komplexe Natur des Ur X". Naturwissenschaften 14 (14): 339. Bibcode:1913NW......1..339F. doi:10.1007/BF01495360.

[14] Fajans, K. & Gohring, O. (1913). "Über das Uran X₂-das neue Element der Uranreihe". Physikalische Zeitschrift 14: 877–84.

[CRC-15] Hammond, C. R. The Elements, in Handbook of Chemistry and Physics (81st ed.). CRC press. ISBN 0-8493-0485-7.

[g1251-16] Greenwood, p. 1251

[17] Shea, William R. (1983) Otto Hahn and the rise of nuclear physics, Springer, p. 213, ISBN 90-277-1584-X.

[18] von Grosse, Aristid (1928). "Das Element 91; seine Eigenschaften und seine Gewinnung". Berichte der deutschen chemischen Gesellschaft 61 (1): 233–245. doi:10.1002/cber.19280610137.

[19] Graue, G.; Käding, H. (1934). "Die technische Gewinnung des Protactiniums". Angewandte Chemie 47 (37): 650–653. doi:10.1002/ange.19340473706.

[20] Grosse, A. V. (1934). "Metallic Element 91". Journal of the American Chemical Society 56 (10): 2200. doi:10.1021/ja01325a508.

[21] Protactinium at the Wayback Machine (archived September 28, 2011) from Los Alamos National Laboratory.

[nubase-22] Audi, G; Bersillon, O.; Blachot, J.; Wapstra, A.H. (2003). "The NUBASE evaluation of nuclear and decay properties" (PDF). Nuclear Physics A 729: 3. Bibcode:2003NuPhA.729....3A. doi:10.1016/j.nuclphysa.2003.11.001.

[ANL-23] Protactinium, Argonne National Laboratory, Human Health Fact Sheet, August 2005

[brit-24] Articles "Protactinium" and "Protactinium-231 – thorium-230 dating" in Encyclopædia Britannica, 15th edition, 1995, p. 737

[25] Grosse, A. V.; Agruss, M. S. (1934). "The Isolation of 0.1 Gram of the Oxide of Element 91 (Protactinium)". Journal of the American Chemical Society 56 (10): 2200. doi:10.1021/ja01325a507.

[26] Cornelis, Rita (2005) Handbook of elemental speciation II: species in the environment, food, medicine & occupational health, Vol. 2, John Wiley and Sons, pp. 520–521, ISBN 0-470-85598-3.

[b1-27] Groult, Henri (2005) Fluorinated materials for energy conversion, Elsevier, pp. 562–565, ISBN 0-08-044472-5.

[28] Hébert, Alain (July 2009). Applied Reactor Physics. Presses inter Polytechnique. pp. 265–. ISBN 978-2-553-01436-9.

[exp-29] Marples, J. A. C. (1965). "On the thermal expansion of protactinium metal". Acta Crystallographica 18 (4): 815. doi:10.1107/S0365110X65001871.

[super-30] Fowler, R. D.; Matthias, B.; Asprey, L.; Hill, H.; et al. (1965). "Superconductivity of Protactinium". Phys. Rev. Lett. 15 (22): 860. Bibcode:1965PhRvL..15..860F. doi:10.1103/PhysRevLett.15.860.

[pao2-31] ^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m ⁿ ^o ^p ^q 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.

[32] Seitz, Frederick and Turnbull, David (1964) Solid state physics: advances in research and applications, Academic Press, pp. 289–291, ISBN 0-12-607716-9.

[33] Myasoedov, B. F.; Kirby, H. W.; Tananaev, I. G. (2006). "Chapter 4: Protactinium". In Morss, L. R.; Edelstein, N. M.; Fuger, J. The Chemistry of the Actinide and Transactinide Elements (3rd ed.). Dordrecht, The Netherlands: Springer. ISBN 978-1-4020-3555-5.

[34] Young, David A. (1991) Phase diagrams of the elements, University of California Press, p. 222, ISBN 0-520-07483-1.

[35] Buschow, K. H. J. (2005) Concise encyclopedia of magnetic and superconducting materials, Elsevier, pp. 129–130, ISBN 0-08-044586-1.

[36] Hendricks, M. E. (1971). "Magnetic Properties of Protactinium Tetrachloride". The Journal of Chemical Physics 55 (6): 2993. Bibcode:1971JChPh..55.2993H. doi:10.1063/1.1676528.

[g1265-37] Greenwood, p. 1265

[g1275-38] Greenwood, p. 1275

[trif-39] 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.

[40] 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)". J. Chem. Soc., Dalton Trans (6): 686–691. doi:10.1039/DT9730000686.

[pabr4-41] 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. doi:10.1016/0022-5088(90)90436-N.

[pabr5b-42] 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.

[pacl5-43] Dodge, R. P.; Smith, G. S.; Johnson, Q.; Elson, R. E. (1967). "The crystal structure of protactinium pentachloride". Acta Crystallogr 22: 85–89. doi:10.1107/S0365110X67000155.

[pabr5-44] Brown, D.; Petcher, T. J.; Smith, A. J. (1969). "The crystal structure of β-protactinium pentabromide". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry 25 (2): 178. doi:10.1107/S0567740869007357.

[papo3-45] 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.

[cene-46] Starks, David F.; Parsons, Thomas C.; Streitwieser, Andrew; Edelstein, Norman (1974). "Bis(π-cyclooctatetraene) protactinium". Inorganic Chemistry 13 (6): 1307. doi:10.1021/ic50136a011.

[g1268-47] Greenwood, p. 1268

[pacl4b-48] 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.

[g1269-49] Greenwood, p. 1269

[50] Iyer, P. N.; Smith, A. J. (1971). "Double oxides containing niobium, tantalum or protactinium. IV. Further systems involving alkali metals". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry 27 (4): 731. doi:10.1107/S056774087100284X.

[51] 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. doi:10.1107/S0365110X67003639.

[target-52] Grossmann, R; Maier, H; Szerypo, J; Friebel, H (2008). "Preparation of 231Pa targets". Nuclear Instruments and Methods in Physics Research Section A: Accelerators, Spectrometers, Detectors and Associated Equipment 590: 122. Bibcode:2008NIMPA.590..122G. doi:10.1016/j.nima.2008.02.084.

[g1270-53] Greenwood, p. 1270

[g1271-54] Greenwood, p. 1271

[g1277-55] Greenwood, p. 1277

[g1278-56] Greenwood, pp. 1278–1279

[57] Seifritz, Walter (1984) Nukleare Sprengkörper – Bedrohung oder Energieversorgung für die Menschheit, Thiemig-Verlag, ISBN 3-521-06143-4.

[58] Ganesan, S. (1999). "A Re-calculation of Criticality Property of ²³¹Pa Using New Nuclear Data" (PDF). Current Science 77 (5): 667–677.

[59] McManus, J. F.; Francois, R.; Gherardi, J.-M.; Keigwin, L. D.; et al. (2004). "Collapse and rapid resumption of Atlantic meridional circulation linked to deglacial climate changes" (PDF). Nature 428 (6985): 834–837. Bibcode:2004Natur.428..834M. doi:10.1038/nature02494. PMID 15103371.

[60] Cheng, H; Edwards, R.Lawrence; Murrell, M.T.; Benjamin, T.M. (1998). "Uranium-thorium-protactinium dating systematics". Geochimica et Cosmochimica Acta 62 (21–22): 3437. Bibcode:1998GeCoA..62.3437C. doi:10.1016/S0016-7037(98)00255-5.

[61] Palshin, E.S.; et al. (1968). Analytical chemistry of protactinium. Moscow: Nauka.

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protactinium