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This article is about the chemical element. For other uses, see Californium (disambiguation).

Californium, 98Cf
A very small disc of silvery metal, magnified to show its metallic texture
Californium
Pronunciation/ˌkæləˈfɔːrniəm/ ​(KAL-ə-FOR-nee-əm)
Appearancesilvery
Mass number[251]
Californium 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
Dy
↑
Cf
↓
—
berkelium ← californium → einsteinium
Atomic number (Z)98
Groupf-block groups (no number)
Periodperiod 7
Block  f-block
Electron configuration[Rn] 5f10 7s2[1]
Electrons per shell2, 8, 18, 32, 28, 8, 2
Physical properties
Phase at STPsolid
Melting point1173 K ​(900 °C, ​1652 °F)[2]
Boiling point1743 K ​(1470 °C, ​2678 °F) (estimation)[3]
Density (near r.t.)15.1 g/cm3[2]
Atomic properties
Oxidation statescommon: +3
+2,[4] +4,[4] +5[5][6]
ElectronegativityPauling scale: 1.3[7]
Ionization energies
  • 1st: 608 kJ/mol[8]
Color lines in a spectral range
Spectral lines of californium
Other properties
Natural occurrencesynthetic
Crystal structure ​double hexagonal close-packed (dhcp)
Double hexagonal close packed crystal structure for californium
Mohs hardness3–4[9]
CAS Number7440-71-3[2]
History
Namingafter California, where it was discovered
DiscoveryLawrence Berkeley National Laboratory (1950)
Isotopes of californium
Main isotopes[10][11] Decay
abun­dance half-life (t1/2) mode pro­duct
248Cf synth 333.5 d α100% 244Cm
SF<0.01% –
249Cf synth 351 y α100% 245Cm
SF≪0.01% –
250Cf synth 13.08 y α99.9% 246Cm
SF0.08% –
251Cf synth 898 y α 247Cm
252Cf synth 2.645 y α96.9% 248Cm
SF3.09% –
253Cf synth 17.81 d β−99.7% 253Es
α0.31% 249Cm
254Cf synth 60.5 d SF99.7% –
α0.31% 250Cm
 Category: Californium
| references

Californium is a synthetic chemical element; it has symbol Cf and atomic number 98. It was first synthesized in 1950 at Lawrence Berkeley National Laboratory (then the University of California Radiation Laboratory) by bombarding curium with alpha particles (helium-4 ions). It is an actinide element, the sixth transuranium element to be synthesized, and has the second-highest atomic mass of all elements that have been produced in amounts large enough to see with the naked eye (after einsteinium). It was named after the university and the U.S. state of California.

Two crystalline forms exist at normal pressure: one above and one below 900 °C (1,650 °F). A third form exists at high pressure. Californium slowly tarnishes in air at room temperature. Californium compounds are dominated by the +3 oxidation state. The most stable of californium's twenty known isotopes is californium-251, with a half-life of 898 years. This short half-life means the element is not found in significant quantities in the Earth's crust.[a] 252Cf, with a half-life of about 2.645 years, is the most common isotope used and is produced at Oak Ridge National Laboratory (ORNL) in the United States and Research Institute of Atomic Reactors in Russia.

Californium is one of the few transuranium elements with practical uses. Most of these applications exploit the fact that certain isotopes of californium emit neutrons. For example, californium can be used to help start up nuclear reactors, and it is used as a source of neutrons when studying materials using neutron diffraction and neutron spectroscopy. It can also be used in nuclear synthesis of higher mass elements; oganesson (element 118) was synthesized by bombarding californium-249 atoms with calcium-48 ions. Users of californium must take into account radiological concerns and the element's ability to disrupt the formation of red blood cells by bioaccumulating in skeletal tissue.

Characteristics

[edit]

Physical properties

[edit]

Californium is a silvery-white actinide metal[12] with a melting point of 900 ± 30 °C (1,650 ± 50 °F) and an estimated boiling point of 1,743 K (1,470 °C; 2,680 °F).[13] The pure metal is malleable and is easily cut with a knife. Californium metal starts to vaporize above 300 °C (570 °F) when exposed to a vacuum.[14] Below 51 K (−222 °C; −368 °F) californium metal is either ferromagnetic or ferrimagnetic (it acts like a magnet), between 48 and 66 K it is antiferromagnetic (an intermediate state), and above 160 K (−113 °C; −172 °F) it is paramagnetic (external magnetic fields can make it magnetic).[15] It forms alloys with lanthanide metals but little is known about the resulting materials.[14]

The element has two crystalline forms at standard atmospheric pressure: a double-hexagonal close-packed form dubbed alpha (α) and a face-centered cubic form designated beta (β).[b] The α form exists below 600–800°C with a density of 15.10 g/cm3 and the β form exists above 600–800°C with a density of 8.74 g/cm3.[17] At 48 GPa of pressure the β form changes into an orthorhombic crystal system due to delocalization of the atom's 5f electrons, which frees them to bond.[18][c]

The bulk modulus of a material is a measure of its resistance to uniform pressure. Californium's bulk modulus is 50±5 GPa, which is similar to trivalent lanthanide metals but smaller than more familiar metals, such as aluminium (70 GPa).[18]

Chemical properties and compounds

[edit]
Further information: Californium compounds
Representative californium compounds[12][d]
state compound formula color
+2 californium(II) bromide CfBr2 yellow
+2 californium(II) iodide CfI2 dark violet
+3 californium(III) oxide Cf2O3 yellow-green
+3 californium(III) fluoride CfF3 bright green
+3 californium(III) chloride CfCl3 emerald green
+3 californium(III) bromide CfBr3 yellowish green
+3 californium(III) iodide CfI3 lemon yellow
+3 californium(III) polyborate Cf[B6O8(OH)5] pale green
+4 californium(IV) oxide CfO2 black brown
+4 californium(IV) fluoride CfF4 green

Californium exhibits oxidation states of 4, 3, or 2. It typically forms eight or nine bonds to surrounding atoms or ions. Its chemical properties are predicted to be similar to other primarily 3+ valence actinide elements[20] and the element dysprosium, which is the lanthanide above californium in the periodic table.[21] Compounds in the +4 oxidation state are strong oxidizing agents and those in the +2 state are strong reducing agents.[12]

The element slowly tarnishes in air at room temperature, with the rate increasing when moisture is added.[17] Californium reacts when heated with hydrogen, nitrogen, or a chalcogen (oxygen family element); reactions with dry hydrogen and aqueous mineral acids are rapid.[17]

Californium is only water-soluble as the californium(III) cation. Attempts to reduce or oxidize the +3 ion in solution have failed.[21] The element forms a water-soluble chloride, nitrate, perchlorate, and sulfate and is precipitated as a fluoride, oxalate, or hydroxide.[20] Californium is the heaviest actinide to exhibit covalent properties, as is observed in the californium borate.[22]

Isotopes

[edit]
Main article: Isotopes of californium

Twenty isotopes of californium are known (mass number ranging from 237 to 256[11]); the most stable are 251Cf with half-life 898 years, 249Cf with half-life 351 years, 250Cf at 13.08 years, and 252Cf at 2.645 years.[11] All other isotopes have half-life shorter than a year, and most of these have half-lives less than 20 minutes.[11]

249Cf is formed by beta decay of berkelium-249, and most other californium isotopes are made by subjecting berkelium to intense neutron radiation in a nuclear reactor.[21] Though californium-251 has the longest half-life, its production yield is only 10% due to its tendency to collect neutrons (high neutron capture) and its tendency to interact with other particles (high neutron cross section).[23]

252Cf is a very strong neutron emitter, which makes it extremely radioactive and harmful.[24][25][26] 252Cf, 96.9% of the time, alpha decays to curium-248; the other 3.1% of decays are spontaneous fission.[11] One microgram (μg) of 252Cf emits 2.3 million neutrons per second, an average of 3.7 neutrons per spontaneous fission.[27] Most other isotopes of californium, alpha decay to curium (atomic number 96).[11]

History

[edit]
Large pieces of equipment with a man standing nearby.
The 60-inch-diameter (1.52 m) cyclotron used to first synthesize californium

Californium was first made at University of California Radiation Laboratory, Berkeley, by physics researchers Stanley Gerald Thompson, Kenneth Street Jr., Albert Ghiorso, and Glenn T. Seaborg, about February 9, 1950.[28] It was the sixth transuranium element to be discovered; the team announced its discovery on March 17, 1950.[29][30]

To produce californium, a microgram-size target of curium-242 (242
96Cm
) was bombarded with 35 MeV alpha particles (4
2He
) in the 60-inch-diameter (1.52 m) cyclotron at Berkeley, which produced californium-245 (245
98Cf
) plus one free neutron (
n
).[28][29]

242
96Cm
 + 4
2He
 → 245
98Cf
 + 1
0
n

To identify and separate out the element, ion exchange and adsorsion methods were undertaken.[29][31] Only about 5,000 atoms of californium were produced in this experiment,[32] and these atoms had a half-life of 44 minutes.[28]

The discoverers named the new element after the university and the state. This was a break from the convention used for elements 95 to 97, which drew inspiration from how the elements directly above them in the periodic table were named.[33][e] However, the element directly above element 98 in the periodic table, dysprosium, has a name that means "hard to get at", so the researchers decided to set aside the informal naming convention.[35] They added that "the best we can do is to point out [that] ... searchers a century ago found it difficult to get to California".[34]

Weighable amounts of californium were first produced by the irradiation of plutonium targets at Materials Testing Reactor at National Reactor Testing Station, eastern Idaho; these findings were reported in 1954.[36] The high spontaneous fission rate of californium-252 was observed in these samples. The first experiment with californium in concentrated form occurred in 1958.[28] The isotopes 249Cf to 252Cf were isolated that same year from a sample of plutonium-239 that had been irradiated with neutrons in a nuclear reactor for five years.[12] Two years later, in 1960, Burris Cunningham and James Wallman of Lawrence Radiation Laboratory of the University of California created the first californium compounds—californium trichloride, californium(III) oxychloride, and californium oxide—by treating californium with steam and hydrochloric acid.[37]

The High Flux Isotope Reactor (HFIR) at ORNL in Oak Ridge, Tennessee, started producing small batches of californium in the 1960s.[38] By 1995, HFIR nominally produced 500 milligrams (0.018 oz) of californium annually.[39] Plutonium supplied by the United Kingdom to the United States under the 1958 US–UK Mutual Defence Agreement was used for making californium.[40]

The Atomic Energy Commission sold 252Cf to industrial and academic customers in the early 1970s for $10/microgram,[27] and an average of 150 mg (0.0053 oz) of 252Cf were shipped each year from 1970 to 1990.[41][f] Californium metal was first prepared in 1974 by Haire and Baybarz, who reduced californium(III) oxide with lanthanum metal to obtain microgram amounts of sub-micrometer thick films.[42][43][g]

Occurrence

[edit]

Traces of californium can be found near facilities that use the element in mineral prospecting and in medical treatments.[45] The element is fairly insoluble in water, but it adheres well to ordinary soil; and concentrations of it in the soil can be 500 times higher than in the water surrounding the soil particles.[46]

Nuclear fallout from atmospheric nuclear weapons testing prior to 1980 contributed a small amount of californium to the environment.[46] Californium-249, -252, -253, and -254 have been observed in the radioactive dust collected from the air after a nuclear explosion.[47] Californium is not a major radionuclide at United States Department of Energy legacy sites since it was not produced in large quantities.[46]

Californium was once believed to be produced in supernovas, as their decay matches the 60-day half-life of 254Cf.[48] However, subsequent studies failed to demonstrate any californium spectra,[49] and supernova light curves are now thought to follow the decay of nickel-56.[50]

The transuranic elements americium to fermium, including californium, occurred naturally in the natural nuclear fission reactor at Oklo, but no longer do so.[51]

Spectral lines of californium, along with those of several other non-primordial elements, were detected in Przybylski's Star in 2008.[52]

Production

[edit]
See also: Nuclear fuel cycle

Californium is produced in nuclear reactors and particle accelerators.[53] Californium-250 is made by bombarding berkelium-249 (249Bk) with neutrons, forming berkelium-250 (250Bk) via neutron capture (n,γ) which, in turn, quickly beta decays (β−) to californium-250 (250Cf) in the following reaction:[54]

249
97Bk
(n,γ)250
97Bk
 → 250
98Cf
 + β−

Bombardment of 250Cf with neutrons produces 251Cf and 252Cf.[54]

Prolonged irradiation of americium, curium, and plutonium with neutrons produces milligram amounts of 252Cf and microgram amounts of 249Cf.[55] As of 2006, curium isotopes 244 to 248 are irradiated by neutrons in special reactors to produce mainly californium-252 with lesser amounts of isotopes 249 to 255.[56]

Microgram quantities of 252Cf are available for commercial use through the U.S. Nuclear Regulatory Commission.[53] Only two sites produce 252Cf: Oak Ridge National Laboratory in the U.S., and the Research Institute of Atomic Reactors in Dimitrovgrad, Russia. As of 2003, the two sites produce 0.25 grams and 0.025 grams of 252Cf per year, respectively.[57]

Three californium isotopes with significant half-lives are produced, requiring a total of 15 neutron captures by uranium-238 without nuclear fission or alpha decay occurring during the process.[57] 253Cf is at the end of a production chain that starts with uranium-238, and includes several isotopes of plutonium, americium, curium, and berkelium, and the californium isotopes 249 to 253 (see diagram).

A complex flow diagram showing various isotopes.
Scheme of the production of californium-252 from uranium-238 by neutron irradiation

Applications

[edit]
Large conical structure on a pulley with a man on top and two near the base.
Fifty-ton shipping cask built at ORNL which can transport up to 1 gram of 252Cf.[58] Large and heavily shielded transport containers are needed to prevent the release of highly radioactive material in case of normal and hypothetical accidents.[59]

Californium-252 has a number of specialized uses as a strong neutron emitter; it produces 139 million neutrons per microgram per minute.[27] This property makes it useful as a startup neutron source for some nuclear reactors[17] and as a portable (non-reactor based) neutron source for neutron activation analysis to detect trace amounts of elements in samples.[60][h] Neutrons from californium are used as a treatment of certain cervical and brain cancers where other radiation therapy is ineffective.[17] It has been used in educational applications since 1969 when Georgia Institute of Technology got a loan of 119 μg of 252Cf from the Savannah River Site.[62] It is also used with online elemental coal analyzers and bulk material analyzers in the coal and cement industries.

Neutron penetration into materials makes californium useful in detection instruments such as fuel rod scanners;[17] neutron radiography of aircraft and weapons components to detect corrosion, bad welds, cracks and trapped moisture;[63] and in portable metal detectors.[64] Neutron moisture gauges use 252Cf to find water and petroleum layers in oil wells, as a portable neutron source for gold and silver prospecting for on-the-spot analysis,[21] and to detect ground water movement.[65] The main uses of 252Cf in 1982 were, reactor start-up (48.3%), fuel rod scanning (25.3%), and activation analysis (19.4%).[66] By 1994, most 252Cf was used in neutron radiography (77.4%), with fuel rod scanning (12.1%) and reactor start-up (6.9%) as important but secondary uses.[66] In 2021, fast neutrons from 252Cf were used for wireless data transmission.[67]

251Cf has a very small calculated critical mass of about 5 kg (11 lb),[68] high lethality, and a relatively short period of toxic environmental irradiation. The low critical mass of californium led to some exaggerated claims about possible uses for the element.[i]

In October 2006, researchers announced that three atoms of oganesson (element 118) had been identified at Joint Institute for Nuclear Research in Dubna, Russia, from bombarding 249Cf with calcium-48, making it the heaviest element ever made. The target contained about 10 mg of 249Cf deposited on a titanium foil of 32 cm2 area.[70][71][72] Californium has also been used to produce other transuranic elements; for example, lawrencium was first synthesized in 1961 by bombarding californium with boron nuclei.[73]

Precautions

[edit]

Californium that bioaccumulates in skeletal tissue releases radiation that disrupts the body's ability to form red blood cells.[74] The element plays no natural biological role in any organism due to its intense radioactivity and low concentration in the environment.[45]

Californium can enter the body from ingesting contaminated food or drinks or by breathing air with suspended particles of the element. Once in the body, only 0.05% of the californium will reach the bloodstream. About 65% of that californium will be deposited in the skeleton, 25% in the liver, and the rest in other organs, or excreted, mainly in urine. Half of the californium deposited in the skeleton and liver are gone in 50 and 20 years, respectively. Californium in the skeleton adheres to bone surfaces before slowly migrating throughout the bone.[46]

The element is most dangerous if taken into the body. In addition, californium-249 and californium-251 can cause tissue damage externally, through gamma ray emission. Ionizing radiation emitted by californium on bone and in the liver can cause cancer.[46]

Notes

[edit]
  1. ^ The Earth formed 4.5 billion years ago, and the extent of natural neutron emission within it that could produce californium from more stable elements is extremely limited.
  2. ^ A double hexagonal close-packed (dhcp) unit cell consists of two hexagonal close-packed structures that share a common hexagonal plane, giving dhcp an ABACABAC sequence.[16]
  3. ^ The three lower-mass transplutonium elements—americium, curium, and berkelium—require much less pressure to delocalize their 5f electrons.[18]
  4. ^ Other +3 oxidation states include the sulfide and metallocene.[19]
  5. ^ Europium, in the sixth period directly above element 95, was named for the continent it was discovered on, so element 95 was named americium. Element 96 was named curium for Marie Curie and Pierre Curie as an analog to the naming of gadolinium, which was named for the scientist and engineer Johan Gadolin. Terbium was named for the village it was discovered in, so element 97 was named berkelium.[34]
  6. ^ The Nuclear Regulatory Commission replaced the Atomic Energy Commission when the Energy Reorganization Act of 1974 was implemented. The price of californium-252 was increased by the NRC several times and was $60 per microgram by 1999; this price does not include the cost of encapsulation and transportation.[27]
  7. ^ In 1975, another paper stated that the californium metal prepared the year before was the hexagonal compound Cf2O2S and face-centered cubic compound CfS.[44] The 1974 work was confirmed in 1976 and work on californium metal continued.[42]
  8. ^ By 1990, californium-252 had replaced plutonium-beryllium neutron sources due to its smaller size and lower heat and gas generation.[61]
  9. ^ An article entitled "Facts and Fallacies of World War III" in the July 1961 edition of Popular Science magazine read "A californium atomic bomb need be no bigger than a pistol bullet. You could build a hand-held six-shooter to fire bullets that would explode on contact with the force of 10 tons of TNT."[69]

References

[edit]
  1. ^ CRC 2006, p. 1.14.
  2. ^ a b c CRC 2006, p. 4.56.
  3. ^ Joseph Jacob Katz; Glenn Theodore Seaborg; Lester R. Morss (1986). The Chemistry of the actinide elements. Chapman and Hall. p. 1038. ISBN 9780412273704. Retrieved July 11, 2011.
  4. ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 28. ISBN 978-0-08-037941-8.
  5. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1265. ISBN 978-0-08-037941-8.
  6. ^ 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.
  7. ^ Emsley 1998, p. 50.
  8. ^ CRC 2006, p. 10.204.
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  10. ^ CRC 2006, p. 11.196.
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  14. ^ a b Haire 2006, p. 1526.
  15. ^ Haire 2006, p. 1525.
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  18. ^ a b c Haire 2006, p. 1522.
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  21. ^ a b c d CRC 2006, p. 4.8.
  22. ^ Polinski, Matthew J.; Iii, Edward B. Garner; Maurice, Rémi; Planas, Nora; Stritzinger, Jared T.; Parker, T. Gannon; Cross, Justin N.; Green, Thomas D.; Alekseev, Evgeny V. (May 1, 2014). "Unusual structure, bonding and properties in a californium borate". Nature Chemistry. 6 (5): 387–392. Bibcode:2014NatCh...6..387P. CiteSeerX 10.1.1.646.749. doi:10.1038/nchem.1896. ISSN 1755-4330. PMID 24755589. S2CID 104331283.
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  33. ^ Weeks & Leichester 1968, p. 849.
  34. ^ a b Weeks & Leichester 1968, p. 848.
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  39. ^ Osborne-Lee 1995, p. 11.
  40. ^ "Plutonium and Aldermaston – an Historical Account" (PDF). UK Ministry of Defence. September 4, 2001. p. 30. Archived from the original (PDF) on December 13, 2006. Retrieved March 15, 2007.
  41. ^ Osborne-Lee 1995, p. 6.
  42. ^ a b Haire 2006, p. 1519.
  43. ^ Haire, R. G.; Baybarz, R. D. (1974). "Crystal Structure and Melting Point of Californium Metal". Journal of Inorganic and Nuclear Chemistry. 36 (6): 1295. doi:10.1016/0022-1902(74)80067-9.
  44. ^ Zachariasen, W. (1975). "On Californium Metal". Journal of Inorganic and Nuclear Chemistry. 37 (6): 1441–1442. doi:10.1016/0022-1902(75)80787-1.
  45. ^ a b Emsley 2001, p. 90.
  46. ^ a b c d e "Human Health Fact Sheet: Californium" (PDF). Argonne National Laboratory. August 2005. Archived from the original (PDF) on July 21, 2011.
  47. ^ Fields, P. R.; Studier, M.; Diamond, H.; Mech, J.; Inghram, M.; Pyle, G.; Stevens, C.; Fried, S.; 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.
  48. ^ Baade, W.; Burbidge, G. R.; Hoyle, F.; Burbidge, E. M.; Christy, R. F.; Fowler, W. A. (August 1956). "Supernovae and Californium 254" (PDF). Publications of the Astronomical Society of the Pacific. 68 (403): 296–300. Bibcode:1956PASP...68..296B. doi:10.1086/126941. Archived (PDF) from the original on October 10, 2022. Retrieved September 26, 2012.
  49. ^ Conway, J. G.; Hulet, E.K.; Morrow, R.J. (February 1, 1962). "Emission Spectrum of Californium". Journal of the Optical Society of America. 52 (2): 222. Bibcode:1962JOSA...52..222C. doi:10.1364/josa.52.000222. OSTI 4806792. PMID 13881026.
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