| Discovery date | 1949 |
| Discovered by | Stanley Thompson, Albert Ghiorso, and Glenn Seaborg |
| Origin of the name | Berkelium was named after the town Berkeley, California, where it was first made. |
| Allotropes |
|
Bk
Berkelium
97
[247]
| Group | Actinides | Melting point | 986°C, 1807°F, 1259 K |
| Period | 7 | Boiling point | Unknown |
| Block | f | Density (g cm−3) | 14.78 |
| Atomic number | 97 | Relative atomic mass | [247] |
| State at 20°C | Solid | Key isotopes | 247Bk, 249Bk |
| Electron configuration | [Rn] 5f97s2 | CAS number | 7440-40-6 |
| ChemSpider ID | 22409 | ChemSpider is a free chemical structure database | |
Image explanation
An abstract metal symbol is against a background of vibrant colours representing the creation of the element in nuclear reactors.
Appearance
Berkelium is a radioactive, silvery metal.
Uses
Because it is so rare, berkelium has no commercial or technological use at present.
Biological role
Berkelium has no known biological role. It is toxic due to its radioactivity.
Natural abundance
Less than a gram of berkelium is made each year. It is made in nuclear reactors by the neutron bombardment of plutonium-239.
Berkelium was first produced in December 1949, at the University of California at Berkeley, and was made by Stanley Thompson, Albert Ghiorso, and Glenn Seaborg. They took americium-241, which had first been made in 1944, and bombarded it with helium nuclei (alpha particles) for several hours in the 60-inch cyclotron. The americium itself had been produced by bombarding plutonium with neutrons.
The Berkeley team dissolved the target in acid and used ion exchange to separate the new elements that had been created. This was the isotope berkelium-243 which has a half-life of about 5 hours. It took a further nine years before enough berkelium had been made to see with the naked eye, and even this was only a few micrograms. The first chemical compound, berkelium dioxide, BkO2, was made in 1962.
| Atomic radius, non-bonded (Å) | 2.44 | Covalent radius (Å) | 1.68 |
| Electron affinity (kJ mol−1) | Unknown |
Electronegativity (Pauling scale) |
Unknown |
|
Ionisation energies (kJ mol−1) |
1st
598.007
2nd
-
3rd
-
4th
-
5th
-
6th
-
7th
-
8th
-
|
||
| Common oxidation states | 4, 3 | ||||
| Isotopes | Isotope | Atomic mass | Natural abundance (%) | Half life | Mode of decay |
| 247Bk | 247.070 | - | 1.43 x 103 y | α | |
| 249Bk | 249.075 | - | 320 d | β | |
|
|
α | ||||
| 1.8 x 109 y | sf | ||||
|
Specific heat capacity (J kg−1 K−1) |
Unknown | Young's modulus (GPa) | Unknown | |||||||||||
| Shear modulus (GPa) | Unknown | Bulk modulus (GPa) | Unknown | |||||||||||
| Vapour pressure | ||||||||||||||
| Temperature (K) |
|
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| Pressure (Pa) |
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| Listen to Berkelium Podcast |
|
Transcript :
Chemistry in its element: berkelium(Promo) You're listening to Chemistry in its element brought to you by Chemistry World, the magazine of the Royal Society of Chemistry. (End promo) Meera Senthilingam This week, no prizes for guessing where this element's name comes from. Eric Scerri. Eric Scerri Element 97 in the periodic table is one of only two elements named after a university, namely the University of California at Berkeley. The other such element is number 110 called darmstadtium after the University of Darmstadt in Germany. The university and the city of Berkeley were in turn named after the Anglo-Irish philosopher, Bishop George 'Barkeley'. The pronunciation changed from Barkeley to Berkeley when the name crossed the Atlantic ocean in 1869, the year that the city and university were both founded. Incidentally this was the same year in which Dimitri Mendeleev published the first mature periodic system and began to predict the existence of new elements. But let me get back to berkelium. It was the fifth element in the periodic table after the last naturally occurring element, uranium, to be artificially synthesised. Berkelium was first made some 60 years ago by Stan Thomson, Al Ghiroso and Glen Seaborg by bombarding the isotope americium-241 with alpha particles. The half-life of the first isotope of berkelium to be produced in this way was a healthy 4.5 hours. Subsequently discovered isotopes have included berkelium-249 with a half-life of as much as 314 days. One of the discoverers, Glen Seaborg, was a member of various teams that synthesised a total of 10 elements over a period of many years. His success led to a proposal that he should have an element named after him. But the official governing body, the International Union of Pure and Applied Chemistry, refused to accept this, on the basis that no living scientist had ever been honoured in this way, although actually the element fermium was proposed when the Italian physicist Enrico Fermi was still living and was indeed accepted. Finally after much campaigning by chemists around the world, IUPAC relented and element 106 was duly named seaborgium while he was still alive. This led to an amusing situation whereby people could try to send letters or postcards to Seaborg by using nothing but a sequence of symbols of various elements in the following order. First of all one could write Sg for element 106 or Seaborg's name. The second line consisted of Bk for this week's element 97 or the University at which Seaborg worked. The third line was Cf for element 98, or californium, or the state in which the university stands. Finally, if writing from abroad, the correspondent could add Am for element 95, or americium, or the country of America to complete the address. To the credit of several postal systems around the world a handful of people did indeed succeed in getting letters and messages of congratulations to Seaborg in this cryptic fashion. Many compounds of element 97, berkelium, have been prepared. Unlike the extremely short half-lives possessed by the superheavy elements like 117 and 118 that have been in the news recently, experiments on berkelium are relatively easy to perform and its chemistry has been studied in some detail. The existence of weighable amounts of berkelium-249 have made it possible to determine some of its properties using macroscopic quantities. Although the pure element has not yet been isolated, it is predicted to be a silvery metal that would easily oxidise in air at high temperatures and would be soluble in dilute mineral acids. X-ray diffraction techniques have been used to identify various berkelium compounds such as berkelium dioxide (BkO2), berkelium fluoride (BkF3), berkelium oxychloride (BkOCl), and berkelium trioxide (BkO3). The oxidation states seen so far are +3 and +4 in accordance to its position below terbium in the periodic table. In 1962 visible amounts of berkelium chloride were isolated, weighing 3 billionth of a gram. This was the first time that visible amounts of a pure berkelium compound had been produced. Like other actinides, berkelium accumulates in skeletal tissue and is therefore highly toxic to humans. The element has not found any uses yet outside of basic research and plays no known biological role. Nevertheless its discovery was an important step towards the synthesis of the superheavy elements and has served to test theories of nuclear physics as well as showing that the predictions of the periodic table are fulfilled well beyond the elements for which it was originally devised. Meera Senthilingam Sp playing a pivotal role in fundamental chemistry and physics, while also testing the chemical knowledge of postal services worldwide. That was scientist and author Eric Scerri from UCLA with the discovery of Berkelium. Now next week, an element that requires a magic touch - as long as you don't get too close. Peter Wothers The next exciting thing about caesium, is that my love is not unrequited, it responds to my touch. Strictly speaking, it's the warmth from the hand that melts it, given that its melting point is only 28.4 °C. So just holding its container converts the crystalline solid into liquid gold. Liquid metals are always fascinating - everyone loves mercury; just imagine playing with liquid gold! But here's the snag that adds to my fascination with this metal - it has a rather fiery temper. In fact, you can't actually touch the metal itself since it spontaneously bursts into flames in the presence of air and reacts explosively with water. Awkward indeed. My caesium is sealed inside a glass tube under an atmosphere of the chemically inert gas argon. So to play with it, you have to hold the glass tube, knowing that if you accidentally crushed it, or dropped it, all hell would break loose. Meera Senthilingam And as well as a possible adrenalin rush, join Cambridge University's Peter Wothers for more exciting facts about the liquid gold element that is caesium in next week's Chemistry in its element. Until then thank you for listening, I'm Meera Senthilingam. (Promo) Chemistry in its element is brought to you by the Royal Society of Chemistry and produced by thenakedscientists.com. There's more information and other episodes of Chemistry in its element on our website at chemistryworld.org/elements. (End promo)
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Visual Elements images and videos
© Murray Robertson 1998-2017.
W. M. Haynes, ed., CRC Handbook of Chemistry and Physics, CRC Press/Taylor and Francis, Boca Raton, FL, 95th Edition, Internet Version 2015, accessed December 2014.
Tables of Physical & Chemical Constants, Kaye & Laby Online, 16th edition, 1995. Version 1.0 (2005), accessed December 2014.
J. S. Coursey, D. J. Schwab, J. J. Tsai, and R. A. Dragoset, Atomic Weights and Isotopic Compositions (version 4.1), 2015, National Institute of Standards and Technology, Gaithersburg, MD, accessed November 2016.
T. L. Cottrell, The Strengths of Chemical Bonds, Butterworth, London, 1954.
John Emsley, Nature’s Building Blocks: An A-Z Guide to the Elements, Oxford University Press, New York, 2nd Edition, 2011.
Thomas Jefferson National Accelerator Facility - Office of Science Education, It’s Elemental - The Periodic Table of Elements, accessed December 2014.
Periodic Table of Videos, accessed December 2014.
Derived in part from material provided by the British Geological Survey © NERC.
Elements 1-112, 114, 116 and 117 © John Emsley 2012. Elements 113, 115, 117 and 118 © Royal Society of Chemistry 2017.
Produced by The Naked Scientists.
Created by video journalist Brady Haran working with chemists at The University of Nottingham.
© Murray Robertson 1998-2017.
Data
W. M. Haynes, ed., CRC Handbook of Chemistry and Physics, CRC Press/Taylor and Francis, Boca Raton, FL, 95th Edition, Internet Version 2015, accessed December 2014.
Tables of Physical & Chemical Constants, Kaye & Laby Online, 16th edition, 1995. Version 1.0 (2005), accessed December 2014.
J. S. Coursey, D. J. Schwab, J. J. Tsai, and R. A. Dragoset, Atomic Weights and Isotopic Compositions (version 4.1), 2015, National Institute of Standards and Technology, Gaithersburg, MD, accessed November 2016.
T. L. Cottrell, The Strengths of Chemical Bonds, Butterworth, London, 1954.
Uses and properties
John Emsley, Nature’s Building Blocks: An A-Z Guide to the Elements, Oxford University Press, New York, 2nd Edition, 2011.
Thomas Jefferson National Accelerator Facility - Office of Science Education, It’s Elemental - The Periodic Table of Elements, accessed December 2014.
Periodic Table of Videos, accessed December 2014.
Supply risk data
Derived in part from material provided by the British Geological Survey © NERC.
History text
Elements 1-112, 114, 116 and 117 © John Emsley 2012. Elements 113, 115, 117 and 118 © Royal Society of Chemistry 2017.
Podcasts
Produced by The Naked Scientists.
Periodic Table of Videos
Created by video journalist Brady Haran working with chemists at The University of Nottingham.
