Berkelium is a synthetic chemical element; it has symbol Bk and atomic number 97. It is a member of the actinide and transuranium element series. It is named after the city of Berkeley, California, the location of the Lawrence Berkeley National Laboratory (then the University of California Radiation Laboratory) where it was discovered in December 1949. Berkelium was the fifth transuranium element discovered after neptunium, plutonium, curium and americium.

Berkelium, 97Bk
  • /bərˈkliəm/
  • /ˈbɜːrkliəm/
Mass number[247]
Berkelium in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson


Atomic number (Z)97
Groupf-block groups (no number)
Periodperiod 7
Block  f-block
Electron configuration[Rn] 5f9 7s2
Electrons per shell2, 8, 18, 32, 27, 8, 2
Physical properties
Phase at STPsolid
Melting pointbeta: 1259 K ​(986 °C, ​1807 °F)
Boiling pointbeta: 2900 K ​(2627 °C, ​4760 °F)
Density (near r.t.)alpha: 14.78 g/cm3
beta: 13.25 g/cm3
Heat of fusion7.92 kJ/mol (calculated)
Atomic properties
Oxidation states+2, +3, +4, +5[1]
ElectronegativityPauling scale: 1.3
Ionization energies
  • 1st: 601 kJ/mol
Atomic radiusempirical: 170 pm
Color lines in a spectral range
Spectral lines of berkelium
Other properties
Natural occurrencesynthetic
Crystal structuredouble hexagonal close-packed (dhcp)
Double hexagonal close packed crystal structure for berkelium
Thermal conductivity10 W/(m⋅K)
Magnetic orderingparamagnetic
CAS Number7440-40-6
Namingafter Berkeley, California, where it was discovered
DiscoveryLawrence Berkeley National Laboratory (1949)
Isotopes of berkelium
Main isotopes[2] Decay
abun­dance half-life (t1/2) mode pro­duct
245Bk synth 4.94 d ε 245Cm
α 241Am
246Bk synth 1.8 d α 242Am
β+ 246Cm
247Bk synth 1380 y α 243Am
248Bk synth >300 y[3] α 244Am
249Bk synth 330 d β 249Cf
α 245Am
 Category: Berkelium
| references

The major isotope of berkelium, 249Bk, is synthesized in minute quantities in dedicated high-flux nuclear reactors, mainly at the Oak Ridge National Laboratory in Tennessee, United States, and at the Research Institute of Atomic Reactors in Dimitrovgrad, Russia. The longest-lived and second-most important isotope, 247Bk, can be synthesized via irradiation of 244Cm with high-energy alpha particles.

Just over one gram of berkelium has been produced in the United States since 1967. There is no practical application of berkelium outside scientific research which is mostly directed at the synthesis of heavier transuranium elements and superheavy elements. A 22-milligram batch of berkelium-249 was prepared during a 250-day irradiation period and then purified for a further 90 days at Oak Ridge in 2009. This sample was used to synthesize the new element tennessine for the first time in 2009 at the Joint Institute for Nuclear Research, Russia, after it was bombarded with calcium-48 ions for 150 days. This was the culmination of the Russia–US collaboration on the synthesis of the heaviest elements on the periodic table.

Berkelium is a soft, silvery-white, radioactive metal. The berkelium-249 isotope emits low-energy electrons and thus is relatively safe to handle. It decays with a half-life of 330 days to californium-249, which is a strong emitter of ionizing alpha particles. This gradual transformation is an important consideration when studying the properties of elemental berkelium and its chemical compounds, since the formation of californium brings not only chemical contamination, but also free-radical effects and self-heating from the emitted alpha particles.




Double-hexagonal close packing with the layer sequence ABAC in the crystal structure of α-berkelium (A: green, B: blue, C: red)

Berkelium is a soft, silvery-white, radioactive actinide metal. In the periodic table, it is located to the right of the actinide curium, to the left of the actinide californium and below the lanthanide terbium with which it shares many similarities in physical and chemical properties. Its density of 14.78 g/cm3 lies between those of curium (13.52 g/cm3) and californium (15.1 g/cm3), as does its melting point of 986 °C, below that of curium (1340 °C) but higher than that of californium (900 °C).[4] Berkelium is relatively soft and has one of the lowest bulk moduli among the actinides, at about 20 GPa (2×1010 Pa).[5]

Berkelium(III) ions shows two sharp fluorescence peaks at 652 nanometers (red light) and 742 nanometers (deep red – near-infrared) due to internal transitions at the f-electron shell. The relative intensity of these peaks depends on the excitation power and temperature of the sample. This emission can be observed, for example, after dispersing berkelium ions in a silicate glass, by melting the glass in presence of berkelium oxide or halide.[6][7]

Between 70 K and room temperature, berkelium behaves as a Curie–Weiss paramagnetic material with an effective magnetic moment of 9.69 Bohr magnetonsB) and a Curie temperature of 101 K. This magnetic moment is almost equal to the theoretical value of 9.72 μB calculated within the simple atomic L-S coupling model. Upon cooling to about 34 K, berkelium undergoes a transition to an antiferromagnetic state.[8] Enthalpy of dissolution in hydrochloric acid at standard conditions is −600 kJ/mol, from which the standard enthalpy of formationfH°) of aqueous Bk3+ ions is obtained as −601 kJ/mol. The standard electrode potential Bk3+/Bk is −2.01 V.[9] The ionization potential of a neutral berkelium atom is 6.23 eV.[10]



At ambient conditions, berkelium assumes its most stable α form which has a hexagonal symmetry, space group P63/mmc, lattice parameters of 341 pm and 1107 pm. The crystal has a double-hexagonal close packing structure with the layer sequence ABAC and so is isotypic (having a similar structure) with α-lanthanum and α-forms of actinides beyond curium.[11] This crystal structure changes with pressure and temperature. When compressed at room temperature to 7 GPa, α-berkelium transforms to the β modification, which has a face-centered cubic (fcc) symmetry and space group Fm3m. This transition occurs without change in volume, but the enthalpy increases by 3.66 kJ/mol.[12] Upon further compression to 25 GPa, berkelium transforms to an orthorhombic γ-berkelium structure similar to that of α-uranium. This transition is accompanied by a 12% volume decrease and delocalization of the electrons at the 5f electron shell.[13] No further phase transitions are observed up to 57 GPa.[5][14]

Upon heating, α-berkelium transforms into another phase with an fcc lattice (but slightly different from β-berkelium), space group Fm3m and the lattice constant of 500 pm; this fcc structure is equivalent to the closest packing with the sequence ABC. This phase is metastable and will gradually revert to the original α-berkelium phase at room temperature.[11] The temperature of the phase transition is believed to be quite close to the melting point.[15][16][17]



Like all actinides, berkelium dissolves in various aqueous inorganic acids, liberating gaseous hydrogen and converting into the berkelium(III) state. This trivalent oxidation state (+3) is the most stable, especially in aqueous solutions,[18][19] but tetravalent (+4),[20] pentavalent (+5),[21] and possibly divalent (+2) berkelium compounds are also known. The existence of divalent berkelium salts is uncertain and has only been reported in mixed lanthanum(III) chloride-strontium chloride melts.[22][23] A similar behavior is observed for the lanthanide analogue of berkelium, terbium.[24] Aqueous solutions of Bk3+ ions are green in most acids. The color of Bk4+ ions is yellow in hydrochloric acid and orange-yellow in sulfuric acid.[22][25][26] Berkelium does not react rapidly with oxygen at room temperature, possibly due to the formation of a protective oxide layer surface. However, it reacts with molten metals, hydrogen, halogens, chalcogens and pnictogens to form various binary compounds.[8][15]



Nineteen isotopes and six nuclear isomers (excited states of an isotope) of berkelium have been characterized, with mass numbers ranging from 233 to 253 (except 235 and 237).[27] All of them are radioactive. The longest half-lives are observed for 247Bk (1,380 years), 248Bk (over 300 years), and 249Bk (330 days); the half-lives of the other isotopes range from microseconds to several days. The isotope which is the easiest to synthesize is berkelium-249. This emits mostly soft β-particles which are inconvenient for detection. Its alpha radiation is rather weak (1.45×10−3%) with respect to the β-radiation, but is sometimes used to detect this isotope. The second important berkelium isotope, berkelium-247, is an alpha-emitter, as are most actinide isotopes.[27][28]



All berkelium isotopes have a half-life far too short to be primordial. Therefore, any primordial berkelium − that is, berkelium present on the Earth during its formation − has decayed by now.

On Earth, berkelium is mostly concentrated in certain areas, which were used for the atmospheric nuclear weapons tests between 1945 and 1980, as well as at the sites of nuclear incidents, such as the Chernobyl disaster, Three Mile Island accident and 1968 Thule Air Base B-52 crash. Analysis of the debris at the testing site of the first United States' first thermonuclear weapon, Ivy Mike, (1 November 1952, Enewetak Atoll), revealed high concentrations of various actinides, including berkelium. For reasons of military secrecy, this result was not published until 1956.[29]

Nuclear reactors produce mostly, among the berkelium isotopes, berkelium-249. During the storage and before the fuel disposal, most of it beta decays to californium-249. The latter has a half-life of 351 years, which is relatively long compared to the half-lives of other isotopes produced in the reactor,[30] and is therefore undesirable in the disposal products.

The transuranium elements from americium to fermium, including berkelium, occurred naturally in the natural nuclear fission reactor at Oklo, but no longer do so.[31]

Berkelium is also one of the elements that have theoretically been detected in Przybylski's Star.[32]


Glenn T. Seaborg
The 60-inch cyclotron at the Lawrence Radiation Laboratory, University of California, Berkeley, in August 1939
Berkelium is named after UC Berkeley.

Although very small amounts of berkelium were possibly produced in previous nuclear experiments, it was first intentionally synthesized, isolated and identified in December 1949 by Glenn T. Seaborg, Albert Ghiorso, Stanley Gerald Thompson, and Kenneth Street Jr. They used the 60-inch cyclotron at the University of California, Berkeley. Similar to the nearly simultaneous discovery of americium (element 95) and curium (element 96) in 1944, the new elements berkelium and californium (element 98) were both produced in 1949–1950.[24][33][34][35][36]

The name choice for element 97 followed the previous tradition of the Californian group to draw an analogy between the newly discovered actinide and the lanthanide element positioned above it in the periodic table. Previously, americium was named after a continent as its analogue europium, and curium honored scientists Marie and Pierre Curie as the lanthanide above it, gadolinium, was named after the explorer of the rare-earth elements Johan Gadolin. Thus the discovery report by the Berkeley group reads: "It is suggested that element 97 be given the name berkelium (symbol Bk) after the city of Berkeley in a manner similar to that used in naming its chemical homologue terbium (atomic number 65) whose name was derived from the town of Ytterby, Sweden, where the rare earth minerals were first found."[34] This tradition ended with berkelium, though, as the naming of the next discovered actinide, californium, was not related to its lanthanide analogue dysprosium, but after the discovery place.[37]

The most difficult steps in the synthesis of berkelium were its separation from the final products and the production of sufficient quantities of americium for the target material. First, americium (241Am) nitrate solution was coated on a platinum foil, the solution was evaporated and the residue converted by annealing to americium dioxide (AmO2). This target was irradiated with 35 MeV alpha particles for 6 hours in the 60-inch cyclotron at the Lawrence Radiation Laboratory, University of California, Berkeley. The (α,2n) reaction induced by the irradiation yielded the 243Bk isotope and two free neutrons:[34]

+ 4
+ 21

After the irradiation, the coating was dissolved with nitric acid and then precipitated as the hydroxide using concentrated aqueous ammonia solution. The product was centrifugated and re-dissolved in nitric acid. To separate berkelium from the unreacted americium, this solution was added to a mixture of ammonium and ammonium sulfate and heated to convert all the dissolved americium into the oxidation state +6. Unoxidized residual americium was precipitated by the addition of hydrofluoric acid as americium(III) fluoride (AmF3). This step yielded a mixture of the accompanying product curium and the expected element 97 in form of trifluorides. The mixture was converted to the corresponding hydroxides by treating it with potassium hydroxide, and after centrifugation, was dissolved in perchloric acid.[34]

Chromatographic elution curves revealing the similarity between the lanthanides terbium (Tb), gadolinium (Gd), and europium (Eu) (top graph) and their corresponding actinides berkelium (Bk), curium (Cm), and americium (Am) (bottom graph)[34]

Further separation was carried out in the presence of a citric acid/ammonium buffer solution in a weakly acidic medium (pH≈3.5), using ion exchange at elevated temperature. The chromatographic separation behavior was unknown for the element 97 at the time, but was anticipated by analogy with terbium. The first results were disappointing because no alpha-particle emission signature could be detected from the elution product. With further analysis, searching for characteristic X-rays and conversion electron signals, a berkelium isotope was eventually detected. Its mass number was uncertain between 243 and 244 in the initial report,[24] but was later established as 243.[34]

Synthesis and extraction


Preparation of isotopes


Berkelium is produced by bombarding lighter actinides uranium (238U) or plutonium (239Pu) with neutrons in a nuclear reactor. In a more common case of uranium fuel, plutonium is produced first by neutron capture (the so-called (n,γ) reaction or neutron fusion) followed by beta-decay:[38]

  (the times are half-lives)

Plutonium-239 is further irradiated by a source that has a high neutron flux, several times higher than a conventional nuclear reactor, such as the 85-megawatt High Flux Isotope Reactor (HFIR) at the Oak Ridge National Laboratory in Tennessee, US. The higher flux promotes fusion reactions involving not one but several neutrons, converting 239Pu to 244Cm and then to 249Cm:


Curium-249 has a short half-life of 64 minutes, and thus its further conversion to 250Cm has a low probability. Instead, it transforms by beta-decay into 249Bk:[27]


The thus-produced 249Bk has a long half-life of 330 days and thus can capture another neutron. However, the product, 250Bk, again has a relatively short half-life of 3.212 hours and thus does not yield any heavier berkelium isotopes. It instead decays to the californium isotope 250Cf:[39][40]


Although 247Bk is the most stable isotope of berkelium, its production in nuclear reactors is very difficult because its potential progenitor 247Cm has never been observed to undergo beta decay.[41] Thus, 249Bk is the most accessible isotope of berkelium, which still is available only in small quantities (only 0.66 grams have been produced in the US over the period 1967–1983[42]) at a high price of the order 185 USD per microgram.[4] It is the only berkelium isotope available in bulk quantities, and thus the only berkelium isotope whose properties can be extensively studied.[43]

The isotope 248Bk was first obtained in 1956 by bombarding a mixture of curium isotopes with 25 MeV α-particles. Although its direct detection was hindered by strong signal interference with 245Bk, the existence of a new isotope was proven by the growth of the decay product 248Cf which had been previously characterized. The half-life of 248Bk was estimated as 23±5 hours,[44] though later 1965 work gave a half-life in excess of 300 years (which may be due to an isomeric state).[45] Berkelium-247 was produced during the same year by irradiating 244Cm with alpha-particles:[46]


Berkelium-242 was synthesized in 1979 by bombarding 235U with 11B, 238U with 10B, 232Th with 14N or 232Th with 15N. It converts by electron capture to 242Cm with a half-life of 7.0±1.3 minutes. A search for an initially suspected isotope 241Bk was then unsuccessful;[47] 241Bk has since been synthesized.[48]




The fact that berkelium readily assumes oxidation state +4 in solids, and is relatively stable in this state in liquids greatly assists separation of berkelium away from many other actinides. These are inevitably produced in relatively large amounts during the nuclear synthesis and often favor the +3 state. This fact was not yet known in the initial experiments, which used a more complex separation procedure. Various inorganic oxidation agents can be applied to the berkelium(III) solutions to convert it to the +4 state, such as bromates (BrO3), bismuthates (BiO3), chromates (CrO2−4 and Cr2O2−7), silver(I) thiolate (Ag2S2O8), lead(IV) oxide (PbO2), ozone (O3), or photochemical oxidation procedures. More recently, it has been discovered that some organic and bio-inspired molecules, such as the chelator called 3,4,3-LI(1,2-HOPO), can also oxidize Bk(III) and stabilize Bk(IV) under mild conditions.[20] Berkelium(IV) is then extracted with ion exchange, extraction chromatography or liquid-liquid extraction using HDEHP (bis-(2-ethylhexyl) phosphoric acid), amines, tributyl phosphate or various other reagents. These procedures separate berkelium from most trivalent actinides and lanthanides, except for the lanthanide cerium (lanthanides are absent in the irradiation target but are created in various nuclear fission decay chains).[49]

A more detailed procedure adopted at the Oak Ridge National Laboratory was as follows: the initial mixture of actinides is processed with ion exchange using lithium chloride reagent, then precipitated as hydroxides, filtered and dissolved in nitric acid. It is then treated with high-pressure elution from cation exchange resins, and the berkelium phase is oxidized and extracted using one of the procedures described above.[49] Reduction of the thus-obtained berkelium(IV) to the +3 oxidation state yields a solution, which is nearly free from other actinides (but contains cerium). Berkelium and cerium are then separated with another round of ion-exchange treatment.[50]

Bulk metal preparation


In order to characterize chemical and physical properties of solid berkelium and its compounds, a program was initiated in 1952 at the Material Testing Reactor, Arco, Idaho, US. It resulted in preparation of an eight-gram plutonium-239 target and in the first production of macroscopic quantities (0.6 micrograms) of berkelium by Burris B. Cunningham and Stanley Gerald Thompson in 1958, after a continuous reactor irradiation of this target for six years.[42][51] This irradiation method was and still is the only way of producing weighable amounts of the element, and most solid-state studies of berkelium have been conducted on microgram or submicrogram-sized samples.[15][52]

The world's major irradiation sources are the 85-megawatt High Flux Isotope Reactor at the Oak Ridge National Laboratory in Tennessee, USA,[53] and the SM-2 loop reactor at the Research Institute of Atomic Reactors (NIIAR) in Dimitrovgrad, Russia,[54] which are both dedicated to the production of transcurium elements (atomic number greater than 96). These facilities have similar power and flux levels, and are expected to have comparable production capacities for transcurium elements,[55] although the quantities produced at NIIAR are not publicly reported. In a "typical processing campaign" at Oak Ridge, tens of grams of curium are irradiated to produce decigram quantities of californium, milligram quantities of berkelium-249 and einsteinium, and picogram quantities of fermium.[56][57] In total, just over one gram of berkelium-249 has been produced at Oak Ridge since 1967.[15]

The first berkelium metal sample weighing 1.7 micrograms was prepared in 1971 by the reduction of berkelium(III) fluoride with lithium vapor at 1000 °C; the fluoride was suspended on a tungsten wire above a tantalum crucible containing molten lithium. Later, metal samples weighing up to 0.5 milligrams were obtained with this method.[11][58]

BkF3 + 3 Li → Bk + 3 LiF

Similar results are obtained with berkelium(IV) fluoride.[13] Berkelium metal can also be produced by the reduction of berkelium(IV) oxide with thorium or lanthanum.[58][59]





Two oxides of berkelium are known, with the berkelium oxidation state of +3 (Bk2O3) and +4 (BkO2).[60] Berkelium(IV) oxide is a brown solid,[61] while berkelium(III) oxide is a yellow-green solid with a melting point of 1920 °C[62][61] and is formed from BkO2 by reduction with molecular hydrogen:

2 BkO2 + H2 → Bk2O3 + H2O

Upon heating to 1200 °C, the oxide Bk2O3 undergoes a phase change; it undergoes another phase change at 1750 °C. Such three-phase behavior is typical for the actinide sesquioxides. Berkelium(II) oxide, BkO, has been reported as a brittle gray solid but its exact chemical composition remains uncertain.[63]



In halides, berkelium assumes the oxidation states +3 and +4.[64] The +3 state is the most stable, especially in solutions, while the tetravalent halides BkF4 and Cs2BkCl6 are only known in the solid phase.[65] The coordination of berkelium atom in its trivalent fluoride and chloride is tricapped trigonal prismatic, with the coordination number of 9. In trivalent bromide, it is bicapped trigonal prismatic (coordination 8) or octahedral (coordination 6),[66] and in the iodide it is octahedral.[67]

F Cl Br I
+4 BkF4
+3 BkF3

Berkelium(IV) fluoride (BkF4) is a yellow-green ionic solid and is isotypic with uranium tetrafluoride or zirconium tetrafluoride.[68][70][71] Berkelium(III) fluoride (BkF3) is also a yellow-green solid, but it has two crystalline structures. The most stable phase at low temperatures is isotypic with yttrium(III) fluoride, while upon heating to between 350 and 600 °C, it transforms to the structure found in lanthanum trifluoride.[68][70][72]

Visible amounts of berkelium(III) chloride (BkCl3) were first isolated and characterized in 1962, and weighed only 3 billionths of a gram. It can be prepared by introducing hydrogen chloride vapors into an evacuated quartz tube containing berkelium oxide at a temperature about 500 °C.[73] This green solid has a melting point of 600 °C,[64] and is isotypic with uranium(III) chloride.[74][75] Upon heating to nearly melting point, BkCl3 converts into an orthorhombic phase.[76]

Two forms of berkelium(III) bromide are known: one with berkelium having coordination 6, and one with coordination 8.[52] The latter is less stable and transforms to the former phase upon heating to about 350 °C. An important phenomenon for radioactive solids has been studied on these two crystal forms: the structure of fresh and aged 249BkBr3 samples was probed by X-ray diffraction over a period longer than 3 years, so that various fractions of berkelium-249 had beta decayed to californium-249. No change in structure was observed upon the 249BkBr3249CfBr3 transformation. However, other differences were noted for 249BkBr3 and 249CfBr3. For example, the latter could be reduced with hydrogen to 249CfBr2, but the former could not – this result was reproduced on individual 249BkBr3 and 249CfBr3 samples, as well on the samples containing both bromides.[66] The intergrowth of californium in berkelium occurs at a rate of 0.22% per day and is an intrinsic obstacle in studying berkelium properties. Beside a chemical contamination, 249Cf, being an alpha emitter, brings undesirable self-damage of the crystal lattice and the resulting self-heating. The chemical effect however can be avoided by performing measurements as a function of time and extrapolating the obtained results.[65]

Other inorganic compounds


The pnictides of berkelium-249 of the type BkX are known for the elements nitrogen,[77] phosphorus, arsenic and antimony. They crystallize in the rock-salt structure and are prepared by the reaction of either berkelium(III) hydride (BkH3) or metallic berkelium with these elements at elevated temperature (about 600 °C) under high vacuum.[78]

Berkelium(III) sulfide, Bk2S3, is prepared by either treating berkelium oxide with a mixture of hydrogen sulfide and carbon disulfide vapors at 1130 °C, or by directly reacting metallic berkelium with elemental sulfur. These procedures yield brownish-black crystals.[79]

Berkelium(III) and berkelium(IV) hydroxides are both stable in 1 molar solutions of sodium hydroxide. Berkelium(III) phosphate (BkPO4) has been prepared as a solid, which shows strong fluorescence under excitation with a green light.[80] Berkelium hydrides are produced by reacting metal with hydrogen gas at temperatures about 250 °C.[77] They are non-stoichiometric with the nominal formula BkH
(0 < x < 1).[79] Several other salts of berkelium are known, including an oxysulfide (Bk2O2S), and hydrated nitrate (Bk(NO
), chloride (BkCl
), sulfate (Bk
) and oxalate (Bk
).[65] Thermal decomposition at about 600 °C in an argon atmosphere (to avoid oxidation to BkO2) of Bk
yields the crystals of berkelium(III) oxysulfate (Bk2O2SO4). This compound is thermally stable to at least 1000 °C in inert atmosphere.[81]

Organoberkelium compounds


Berkelium forms a trigonal (η5–C5H5)3Bk metallocene complex with three cyclopentadienyl rings, which can be synthesized by reacting berkelium(III) chloride with the molten beryllocene (Be(C5H5)2) at about 70 °C. It has an amber color and a density of 2.47 g/cm3. The complex is stable to heating to at least 250 °C, and sublimates without melting at about 350 °C. The high radioactivity of berkelium gradually destroys the compound (within a period of weeks).[73][82] One cyclopentadienyl ring in (η5–C5H5)3Bk can be substituted by chlorine to yield [Bk(C5H5)2Cl]2. The optical absorption spectra of this compound are very similar to those of (η5–C5H5)3Bk.[83]


22 milligrams of berkelium (as nitrate) prepared at HFIR in 2009 at a cost of approximately one million dollars, used for the synthesis of tennessine in JINR[84]

There is currently no use for any isotope of berkelium outside basic scientific research.[15] Berkelium-249 is a common target nuclide to prepare still heavier transuranium elements and superheavy elements,[85] such as lawrencium, rutherfordium and bohrium.[15] It is also useful as a source of the isotope californium-249, which is used for studies on the chemistry of californium in preference to the more radioactive californium-252 that is produced in neutron bombardment facilities such as the HFIR.[15][86]

A 22 milligram batch of berkelium-249 was prepared in a 250-day irradiation and then purified for 90 days at Oak Ridge in 2009. This target yielded the first 6 atoms of tennessine at the Joint Institute for Nuclear Research (JINR), Dubna, Russia, after bombarding it with calcium ions in the U400 cyclotron for 150 days. This synthesis was a culmination of the Russia-US collaboration between JINR and Lawrence Livermore National Laboratory on the synthesis of elements 113 to 118 which was initiated in 1989.[87][88]

Nuclear fuel cycle


The nuclear fission properties of berkelium are different from those of the neighboring actinides curium and californium, and they suggest berkelium to perform poorly as a fuel in a nuclear reactor. Specifically, berkelium-249 has a moderately large neutron capture cross section of 710 barns for thermal neutrons, 1200 barns resonance integral, but very low fission cross section for thermal neutrons. In a thermal reactor, much of it will therefore be converted to berkelium-250 which quickly decays to californium-250.[89][90][91] In principle, berkelium-249 can sustain a nuclear chain reaction in a fast breeder reactor. Its critical mass is relatively high at 192 kg; it can be reduced with a water or steel reflector but would still exceed the world production of this isotope.[92]

Berkelium-247 can maintain chain reaction both in a thermal-neutron and in a fast-neutron reactor, however, its production is rather complex and thus the availability is much lower than its critical mass, which is about 75.7 kg for a bare sphere, 41.2 kg with a water reflector and 35.2 kg with a steel reflector (30 cm thickness).[92]

Health issues


Little is known about the effects of berkelium on human body, and analogies with other elements may not be drawn because of different radiation products (electrons for berkelium and alpha particles, neutrons, or both for most other actinides). The low energy of electrons emitted from berkelium-249 (less than 126 keV) hinders its detection, due to signal interference with other decay processes, but also makes this isotope relatively harmless to humans as compared to other actinides. However, berkelium-249 transforms with a half-life of only 330 days to the strong alpha-emitter californium-249, which is rather dangerous and has to be handled in a glovebox in a dedicated laboratory.[93]

Most available berkelium toxicity data originate from research on animals. Upon ingestion by rats, only about 0.01% of berkelium ends in the blood stream. From there, about 65% goes to the bones, where it remains for about 50 years, 25% to the lungs (biological half-life about 20 years), 0.035% to the testicles or 0.01% to the ovaries where berkelium stays indefinitely. The balance of about 10% is excreted.[94] In all these organs berkelium might promote cancer, and in the skeleton, its radiation can damage red blood cells. The maximum permissible amount of berkelium-249 in the human skeleton is 0.4 nanograms.[4][95]


  1. ^ Kovács, Attila; Dau, Phuong D.; Marçalo, Joaquim; Gibson, John K. (2018). "Pentavalent Curium, Berkelium, and Californium in Nitrate Complexes: Extending Actinide Chemistry and Oxidation States". Inorg. Chem. 57 (15). American Chemical Society: 9453–9467. doi:10.1021/acs.inorgchem.8b01450. OSTI 1631597. PMID 30040397. S2CID 51717837.
  2. ^ Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  3. ^ Milsted, J.; Friedman, A. M.; Stevens, C. M. (1965). "The alpha half-life of berkelium-247; a new long-lived isomer of berkelium-248". Nuclear Physics. 71 (2): 299. doi:10.1016/0029-5582(65)90719-4.
  4. ^ a b c Hammond C. R. "The elements" in Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
  5. ^ a b Benedict, U. (1984). "Study of actinide metals and actinide compounds under high pressures". Journal of the Less Common Metals. 100: 153–170. doi:10.1016/0022-5088(84)90061-4.
  6. ^ Assefa, Z.; Haire, R. G.; Stump, N. A. (1998). "Emission profile of Bk(III) in a silicate matrix: anomalous dependence on excitation power". Journal of Alloys and Compounds. 271–273: 854–858. doi:10.1016/S0925-8388(98)00233-3.
  7. ^ Rita Cornelis, Joe Caruso, Helen Crews, Klaus Heumann Handbook of elemental speciation II: species in the environment, food, medicine & occupational health. Volume 2 of Handbook of Elemental Speciation, John Wiley and Sons, 2005, ISBN 0-470-85598-3 p. 553
  8. ^ a b Peterson & Hobart 1984, p. 45.
  9. ^ Fuger, J.; Haire, R. G.; Peterson, J. R. (1981). "A new determination of the enthalpy of solution of berkelium metal and the standard enthalpy of formation of Bk3+ (aq)". Journal of Inorganic and Nuclear Chemistry. 43 (12): 3209. doi:10.1016/0022-1902(81)80090-5.
  10. ^ Peterson & Hobart 1984, p. 34.
  11. ^ a b c Peterson, J. R.; Fahey, J. A.; Baybarz, R. D. (1971). "The crystal structures and lattice parameters of berkelium metal". J. Inorg. Nucl. Chem. 33 (10): 3345–51. doi:10.1016/0022-1902(71)80656-5.
  12. ^ Peterson & Hobart 1984, p. 44.
  13. ^ a b Itie, J. P.; Peterson, J. R.; Haire, R. G.; Dufour, C.; Benedict, U. (1985). "Delocalisation of 5f electrons in berkelium-californium alloys under pressure". Journal of Physics F: Metal Physics. 15 (9): L213. Bibcode:1985JPhF...15L.213I. doi:10.1088/0305-4608/15/9/001.
  14. ^ Young, David A. Phase diagrams of the elements, University of California Press, 1991, ISBN 0-520-07483-1 p. 228
  15. ^ a b c d e f g Hobart, David E.; Peterson, Joseph R. (2006). "Berkelium". In Morss, Lester R.; Edelstein, Norman M.; Fuger, Jean (eds.). The Chemistry of the Actinide and Transactinide Elements (PDF). Vol. 3 (3rd ed.). Dordrecht, the Netherlands: Springer. pp. 1444–98. doi:10.1007/1-4020-3598-5_10. ISBN 978-1-4020-3555-5. Archived from the original (PDF) on 17 July 2010. Retrieved 30 September 2010.
  16. ^ Fahey, J. A.; Peterson, J. R.; Baybarz, R. D. (1972). "Some properties of berkelium metal and the apparent trend toward divalent character in the transcurium actinide metals". Inorg. Nucl. Chem. Lett. 8 (1): 101–7. doi:10.1016/0020-1650(72)80092-8.
  17. ^ Ward, John W.; Kleinschmidt, Phillip D.; Haire, Richard G. (1982). "Vapor pressure and thermodynamics of Bk-249 metal". J. Chem. Phys. 77 (3): 1464–68. Bibcode:1982JChPh..77.1464W. doi:10.1063/1.443975.
  18. ^ Deblonde, Gauthier J.-P.; Kelley, Morgan P.; Su, Jing; Batista, Enrique R.; Yang, Ping; Booth, Corwin H.; Abergel, Rebecca J. (2018). "Spectroscopic and Computational Characterization of Diethylenetriaminepentaacetic Acid/Transplutonium Chelates: Evidencing Heterogeneity in the Heavy Actinide(III) Series". Angewandte Chemie International Edition. 57 (17): 4521–4526. doi:10.1002/anie.201709183. ISSN 1521-3773. PMID 29473263.
  19. ^ Kelley, Morgan P.; Deblonde, Gauthier J.-P.; Su, Jing; Booth, Corwin H.; Abergel, Rebecca J.; Batista, Enrique R.; Yang, Ping (7 May 2018). "Bond Covalency and Oxidation State of Actinide Ions Complexed with Therapeutic Chelating Agent 3,4,3-LI(1,2-HOPO)". Inorganic Chemistry. 57 (9): 5352–5363. doi:10.1021/acs.inorgchem.8b00345. ISSN 0020-1669. OSTI 1458511. PMID 29624372.
  20. ^ a b Deblonde, Gauthier; Sturzbecher-Hoehne, Manuel; Rupert, Peter; An, Dahlia; Illy, Marie-Claire; Ralston, Corie; brabec, Jiri; de Jong, Wibe; Strong, Roland; Abergel, Rebecca (2017). "Chelation and stabilization of berkelium in oxidation state +IV". Nature Chemistry. 9 (9): 843–849. Bibcode:2017NatCh...9..843D. doi:10.1038/nchem.2759. OSTI 1436161. PMID 28837177.
  21. ^ Attila Kovács; Phuong D. Dau; Joaquim Marçalo; John K. Gibson (2018). "Pentavalent Curium, Berkelium, and Californium in Nitrate Complexes: Extending Actinide Chemistry and Oxidation States" (PDF). Inorganic Chemistry. 57 (15). ACS Publications: 9453–9467. doi:10.1021/acs.inorgchem.8b01450. OSTI 1631597. PMID 30040397. S2CID 51717837.
  22. ^ a b Peterson & Hobart 1984, p. 55.
  23. ^ Sullivan, Jim C.; Schmidt, K. H.; Morss, L. R.; Pippin, C. G.; Williams, C. (1988). "Pulse radiolysis studies of berkelium(III): preparation and identification of berkelium(II) in aqueous perchlorate media". Inorganic Chemistry. 27 (4): 597. doi:10.1021/ic00277a005.
  24. ^ a b c Thompson, Stanley G.; Seaborg, Glenn T. (1950). "Chemical properties of berkelium". Lawrence Berkeley National Lab. doi:10.2172/932812. hdl:2027/mdp.39015086479683. OSTI 932812.
  25. ^ Holleman & Wiberg 2007, p. 1956.
  26. ^ Greenwood & Earnshaw 1997, p. 1265.
  27. ^ a b c Audi, G.; Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S. (2017). "The NUBASE2016 evaluation of nuclear properties" (PDF). Chinese Physics C. 41 (3): 030001. Bibcode:2017ChPhC..41c0001A. doi:10.1088/1674-1137/41/3/030001.
  28. ^ B. Myasoedov; et al. (1972). Analytical chemistry of transplutonium elements. Moscow: Nauka. ISBN 978-0-470-62715-0.
  29. ^ Fields, P. R.; Studier, M. H.; Diamond, H.; et al. (1956). "Transplutonium Elements in Thermonuclear Test Debris". Physical Review. 102 (1): 180–182. Bibcode:1956PhRv..102..180F. doi:10.1103/PhysRev.102.180.
  30. ^ Alejandro A. Sonzogni (Database Manager), ed. (2008). "Chart of Nuclides". Upton, New York: National Nuclear Data Center, Brookhaven National Laboratory. Archived from the original on 10 October 2018. Retrieved 1 March 2010.
  31. ^ Emsley, John (2011). Nature's Building Blocks: An A-Z Guide to the Elements (New ed.). New York, NY: Oxford University Press. ISBN 978-0-19-960563-7.
  32. ^ Gopka, V. F.; Yushchenko, A. V.; Yushchenko, V. A.; Panov, I. V.; Kim, Ch. (15 May 2008). "Identification of absorption lines of short half-life actinides in the spectrum of Przybylski's star (HD 101065)". Kinematics and Physics of Celestial Bodies. 24 (2): 89–98. Bibcode:2008KPCB...24...89G. doi:10.3103/S0884591308020049. S2CID 120526363.
  33. ^ Thompson, S.; Ghiorso, A.; Seaborg, G. (1950). "Element 97". Physical Review. 77 (6): 838. Bibcode:1950PhRv...77..838T. doi:10.1103/PhysRev.77.838.2.
  34. ^ a b c d e f Thompson, S.; Ghiorso, A.; Seaborg, G. (1950). "The New Element Berkelium (Atomic Number 97)" (PDF). Physical Review. 80 (5): 781. Bibcode:1950PhRv...80..781T. doi:10.1103/PhysRev.80.781. Archived (PDF) from the original on 9 October 2022. Abstract
  35. ^ Thompson, S. G.; Cunningham, B. B.; Seaborg, G. T. (1950). "Chemical Properties of Berkelium". Journal of the American Chemical Society. 72 (6): 2798. doi:10.1021/ja01162a538. hdl:2027/mdp.39015086479683.
  36. ^ "Comment". The New Yorker. April 1950. Retrieved 4 June 2017.
  37. ^ Heiserman, David L. (1992). "Element 98: Californium". Exploring Chemical Elements and their Compounds. TAB Books. p. 347. ISBN 978-0-8306-3018-9.
  38. ^ Thompson, S.; Ghiorso, A.; Harvey, B.; Choppin, G. (1954). "Transcurium Isotopes Produced in the Neutron Irradiation of Plutonium". Physical Review. 93 (4): 908. Bibcode:1954PhRv...93..908T. doi:10.1103/PhysRev.93.908.
  39. ^ Magnusson, L.; Studier, M.; Fields, P.; Stevens, C.; Mech, J.; Friedman, A.; Diamond, H.; Huizenga, J. (1954). "Berkelium and Californium Isotopes Produced in Neutron Irradiation of Plutonium". Physical Review. 96 (6): 1576. Bibcode:1954PhRv...96.1576M. doi:10.1103/PhysRev.96.1576.
  40. ^ Eastwood, T.; Butler, J.; Cabell, M.; Jackson, H.; Schuman, R.; Rourke, F.; Collins, T. (1957). "Isotopes of Berkelium and Californium Produced by Neutron Irradiation of Plutonium". Physical Review. 107 (6): 1635. Bibcode:1957PhRv..107.1635E. doi:10.1103/PhysRev.107.1635.
  41. ^ Audi, G.; Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S. (2017). "The NUBASE2016 evaluation of nuclear properties" (PDF). Chinese Physics C. 41 (3): 030001. Bibcode:2017ChPhC..41c0001A. doi:10.1088/1674-1137/41/3/030001.
  42. ^ a b Peterson & Hobart 1984, p. 30.
  43. ^ Trabesinger, A. (2017). "Peaceful berkelium". Nature Chemistry. 9 (9): 924. Bibcode:2017NatCh...9..924T. doi:10.1038/nchem.2845. PMID 28837169.
  44. ^ Hulet, E. (1956). "New Isotope of Berkelium". Physical Review. 102 (1): 182. Bibcode:1956PhRv..102..182H. doi:10.1103/PhysRev.102.182.
  45. ^ Milsted, J.; Friedman, A. M.; Stevens, C. M. (1965). "The alpha half-life of berkelium-247; a new long-lived isomer of berkelium-248". Nuclear Physics. 71 (2): 299. Bibcode:1965NucPh..71..299M. doi:10.1016/0029-5582(65)90719-4.
  46. ^ Milsted, J.; Friedman, A. M.; Stevens, C. M. (1965). "The alpha half-life of berkelium-247; a new long-lived isomer of berkelium-248". Nuclear Physics. 71 (2): 299. Bibcode:1965NucPh..71..299M. doi:10.1016/0029-5582(65)90719-4.
  47. ^ Williams, Kimberly; Seaborg, Glenn (1979). "New isotope 242Bk". Physical Review C. 19 (5): 1794. Bibcode:1979PhRvC..19.1794W. doi:10.1103/PhysRevC.19.1794.
  48. ^ Nucleonica (2007–2011). "Nucleonica: Universal Nuclide Chart". Nucleonica. Retrieved 22 July 2011.
  49. ^ a b Peterson & Hobart 1984, p. 32.
  50. ^ Peterson & Hobart 1984, pp. 33–34.
  51. ^ S. G. Thompson, BB Cunningham: "First Macroscopic Observations of the Chemical Properties of Berkelium and californium," supplement to Paper P/825 presented at the Second International Conference on Peaceful Uses of Atomic Energy, Geneva, 1958
  52. ^ a b Peterson & Hobart 1984, p. 38.
  53. ^ "High Flux Isotope Reactor". Oak Ridge National Laboratory. Retrieved 23 September 2010.
  54. ^ "Радионуклидные источники и препараты". Research Institute of Atomic Reactors. Retrieved 26 September 2010.
  55. ^ Haire, Richard G. (2006). "Einsteinium". In Morss, Lester R.; Edelstein, Norman M.; Fuger, Jean (eds.). The Chemistry of the Actinide and Transactinide Elements (PDF). Vol. 3 (3rd ed.). Dordrecht, the Netherlands: Springer. pp. 1577–1620. doi:10.1007/1-4020-3598-5_12. ISBN 978-1-4020-3555-5. Archived from the original (PDF) on 17 July 2010.
  56. ^ Greenwood & Earnshaw 1997, p. 1262.
  57. ^ Porter, C. E.; Riley, F. D. Jr.; Vandergrift, R. D.; Felker, L. K. (1997). "Fermium Purification Using Teva Resin Extraction Chromatography". Sep. Sci. Technol. 32 (1–4): 83–92. doi:10.1080/01496399708003188.
  58. ^ a b Peterson & Hobart 1984, p. 41.
  59. ^ Spirlet, J. C.; Peterson, J. R.; Asprey, L. B. (1987). Preparation and Purification of Actinide Metals. Advances in Inorganic Chemistry. Vol. 31. pp. 1–41. doi:10.1016/S0898-8838(08)60220-2. ISBN 9780120236312. {{cite book}}: |journal= ignored (help)
  60. ^ Peterson, J.; Cunningham, B. B. (1967). "Crystal structures and lattice parameters of the compounds of berkelium I. Berkelium dioxide and cubic berkelium sesquioxide". Inorganic and Nuclear Chemistry Letters. 3 (9): 327. doi:10.1016/0020-1650(67)80037-0.
  61. ^ a b Baybarz, R. D. (1968). "The berkelium oxide system". Journal of Inorganic and Nuclear Chemistry. 30 (7): 1769–1773. doi:10.1016/0022-1902(68)80352-5.
  62. ^ Holleman & Wiberg 2007, p. 1972.
  63. ^ a b Peterson & Hobart 1984, p. 51.
  64. ^ a b Holleman & Wiberg 2007, p. 1969.
  65. ^ a b c Peterson & Hobart 1984, p. 47.
  66. ^ a b c Young, J. P.; Haire, R. G.; Peterson, J. R.; Ensor, D. D.; Fellows, R. L. (1980). "Chemical consequences of radioactive decay. 1. Study of californium-249 ingrowth into crystalline berkelium-249 tribromide: a new crystalline phase of californium tribromide". Inorganic Chemistry. 19 (8): 2209. doi:10.1021/ic50210a003.
  67. ^ a b c d e f Greenwood & Earnshaw 1997, p. 1270.
  68. ^ a b c Peterson & Hobart 1984, p. 48.
  69. ^ Burns, J.; Peterson, J. R.; Stevenson, J. N. (1975). "Crystallographic studies of some transuranic trihalides: 239PuCl3, 244CmBr3, 249BkBr3 and 249CfBr3". Journal of Inorganic and Nuclear Chemistry. 37 (3): 743. doi:10.1016/0022-1902(75)80532-X.
  70. ^ a b Ensor, D.; Peterson, J. R.; Haire, R. G.; Young, J. P. (1981). "Absorption spectrophotometric study of berkelium(III) and (IV) fluorides in the solid state". Journal of Inorganic and Nuclear Chemistry. 43 (5): 1001. doi:10.1016/0022-1902(81)80164-9.
  71. ^ Keenan, Thomas K.; Asprey, Larned B. (1969). "Lattice constants of actinide tetrafluorides including berkelium". Inorganic Chemistry. 8 (2): 235. doi:10.1021/ic50072a011.
  72. ^ Peterson, J. R.; Cunningham, B. B. (1968). "Crystal structures and lattice parameters of the compounds of berkelium—IV berkelium trifluoride☆". Journal of Inorganic and Nuclear Chemistry. 30 (7): 1775. doi:10.1016/0022-1902(68)80353-7.
  73. ^ a b Laubereau, Peter G.; Burns, John H. (1970). "Microchemical preparation of tricyclopentadienyl compounds of berkelium, californium, and some lanthanide elements". Inorganic Chemistry. 9 (5): 1091. doi:10.1021/ic50087a018.
  74. ^ Peterson, J. R.; Cunningham, B. B. (1968). "Crystal structures and lattice parameters of the compounds of berkelium—IIBerkelium trichloride". Journal of Inorganic and Nuclear Chemistry. 30 (3): 823. doi:10.1016/0022-1902(68)80443-9.
  75. ^ Peterson, J. R.; Young, J. P.; Ensor, D. D.; Haire, R. G. (1986). "Absorption spectrophotometric and x-ray diffraction studies of the trichlorides of berkelium-249 and californium-249". Inorganic Chemistry. 25 (21): 3779. doi:10.1021/ic00241a015.
  76. ^ Peterson & Hobart 1984, p. 52.
  77. ^ a b Stevenson, J.; Peterson, J. (1979). "Preparation and structural studies of elemental curium-248 and the nitrides of curium-248 and berkelium-249". Journal of the Less Common Metals. 66 (2): 201. doi:10.1016/0022-5088(79)90229-7.
  78. ^ Damien, D.; Haire, R. G.; Peterson, J. R. (1980). "Preparation and lattice parameters of 249Bk monopnictides". Journal of Inorganic and Nuclear Chemistry. 42 (7): 995. doi:10.1016/0022-1902(80)80390-3.
  79. ^ a b Peterson & Hobart 1984, p. 53.
  80. ^ Peterson & Hobart 1984, pp. 39–40.
  81. ^ Peterson & Hobart 1984, p. 54.
  82. ^ Christoph Elschenbroich Organometallic Chemistry, 6th Edition, Wiesbaden 2008, ISBN 978-3-8351-0167-8, pp. 583–584
  83. ^ Peterson & Hobart 1984, pp. 41, 54.
  84. ^ Finally, Element 117 Is Here! Archived 30 October 2010 at the Wayback Machine, Science Now, 7 April 2010
  85. ^ Stwertka, Albert. A Guide to the Elements, Oxford University Press, 1996, p. 211. ISBN 0-19-508083-1
  86. ^ Haire, Richard G. (2006). "Californium". In Morss, Lester R.; Edelstein, Norman M.; Fuger, Jean (eds.). The Chemistry of the Actinide and Transactinide Elements (PDF). Vol. 3 (3rd ed.). Dordrecht, the Netherlands: Springer. pp. 1499–1576. doi:10.1007/1-4020-3598-5_11. ISBN 978-1-4020-3555-5. Archived from the original (PDF) on 17 July 2010.
  87. ^ Collaboration Expands the Periodic Table, One Element at a Time Archived 18 July 2011 at the Wayback Machine, Science and Technology Review, Lawrence Livermore National Laboratory, October/November 2010
  88. ^ Nuclear Missing Link Created at Last: Superheavy Element 117, Science daily, 7 April 2010
  89. ^ G. Pfennig, H. Klewe-Nebenius, W. Seelmann Eggebert (Eds.): Karlsruhe nuclide, 7 Edition, 2006
  90. ^ Chadwick, M. B.; Obložinský, P.; Herman, M.; et al. (2006). "ENDF/B-VII.0: Next Generation Evaluated Nuclear Data Library for Nuclear Science and Technology". Nuclear Data Sheets. 107 (12): 2931–3060. Bibcode:2006NDS...107.2931C. doi:10.1016/j.nds.2006.11.001.
  91. ^ Koning, A. J.; Avrigeanu, M.; Avrigeanu, V.; et al. (2007). "The JEFF evaluated nuclear data project". ND2007. Vol. ND2007. doi:10.1051/ndata:07476. {{cite book}}: |journal= ignored (help)
  92. ^ a b Institut de Radioprotection et de Sûreté Nucléaire: "Evaluation of nuclear criticality safety. data and limits for actinides in transport" Archived 19 May 2011 at the Wayback Machine, p. 16
  93. ^ Emeleus, H. J. Advances in inorganic chemistry, Academic Press, 1987, ISBN 0-12-023631-1 p. 32
  94. ^ International Commission on Radiological Protection Limits for intakes of radionuclides by workers, Part 4, Volume 19, Issue 4, Elsevier Health Sciences, ISBN, 0080368867 p. 14
  95. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals McGraw-Hill, 2002, ISBN 0-07-049439-8


  • Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  • Holleman, Arnold F.; Wiberg, Nils (2007). Textbook of Inorganic Chemistry (102nd ed.). Berlin: de Gruyter. ISBN 978-3-11-017770-1.
  • Peterson, J. R.; Hobart, D. E. (1984). "The Chemistry of Berkelium". In Emeléus, Harry Julius (ed.). Advances in inorganic chemistry and radiochemistry. Vol. 28. Academic Press. pp. 29–64. doi:10.1016/S0898-8838(08)60204-4. ISBN 978-0-12-023628-2.