| Discovery date | 1964 |
| Discovered by | Georgy Flerov and colleagues and at Dubna, near Moscow, Russia, and independently by Albert Ghiorso and colleagues at Berkeley, California, USA |
| Origin of the name | Rutherfordium is named in honour of New Zealand Chemist Ernest Rutherford, one of the first to explain the structure of atoms. |
| Allotropes |
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Rf
Rutherfordium
104
[267]
| Group | 4 | Melting point | Unknown |
| Period | 7 | Boiling point | Unknown |
| Block | d | Density (g cm−3) | Unknown |
| Atomic number | 104 | Relative atomic mass | [267] |
| State at 20°C | Solid | Key isotopes | 265Rf |
| Electron configuration | [Rn] 5f146d27s2 | CAS number | 53850-36-5 |
| ChemSpider ID | 11201447 | ChemSpider is a free chemical structure database | |
Image explanation
The abstract metallic symbol and background are inspired by imagery from early and modern particle accelerators.
Appearance
A radioactive metal that does not occur naturally. Relatively few atoms have ever been made.
Uses
At present, it is only used in research.
Biological role
Rutherfordium has no known biological role.
Natural abundance
Rutherfordium is a transuranium element. It is created by bombarding californium-249 with carbon-12 nuclei.
In 1964, a team led by Georgy Flerov at the Russian Joint Institute for Nuclear Research (JINR) in Dubna, bombarded plutonium with neon and produced element 104, isotope 259. They confirmed their findings in 1966.
In 1969, a team led by Albert Ghiorso at the Californian Lawrence Berkeley Laboratory (LBL) made three successful attempts to produce element 104: by bombarding curium with oxygen to get isotope-260, californium with carbon to get isotope-257, and californium with carbon to get isotope-258.
A dispute over priority of discovery followed and eventually, in 1992, the International Unions of Pure and Applied Chemistry (IUPAC) concluded that both the Russian and American researchers had been justified in making their claims. IUPAC decided element 104 would be called rutherfordium.
| Atomic radius, non-bonded (Å) | Unknown | Covalent radius (Å) | 1.57 |
| Electron affinity (kJ mol−1) | Unknown |
Electronegativity (Pauling scale) |
Unknown |
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Ionisation energies (kJ mol−1) |
1st
579
2nd
-
3rd
-
4th
-
5th
-
6th
-
7th
-
8th
-
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| Common oxidation states | Unknown | ||||
| Isotopes | Isotope | Atomic mass | Natural abundance (%) | Half life | Mode of decay |
| 265Rf | 265.117 | - | ~ 2 m | α | |
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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 Rutherfordium Podcast |
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Transcript :
Chemistry in its element: rutherfordium(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 we find out how the elements beyond the actinides were discovered. Revealing the chemistry of the first transactinide rutherfordium, here's Simon Cotton. Simon Cotton When the last member of the actinide series, element 103 or lawrencium, was discovered, I was at school doing my A-levels, and I remember reading about it in the magazine Scientific American. The isotope found had a mass of 258 and it didn't hang about for long - having a half-life of just 3.8 seconds. This was not unexpected as half lives had been getting shorter right along the actinide series. This discovery prompted the scientific community to start asking, are there any elements waiting to be made beyond lawrencium? And if so, where would they fit in the periodic table? In those days, scientific competition between Russia and America was intense, and over the next few years both Russian and American nuclear scientists had a bash at element 104. Both of them used the nuclear equivalent of a shooting gallery. They fired nuclear bullets, the positive ions of light atoms at targets. The targets weren't moving ducks, but stationary targets of very heavy nuclei. What they had to do was to overcome the repulsion between the positive nucleus of the target atom and the positive projectile, so that the two nuclei fused together to make the new heavier atom. And both groups took different approaches. The Russians went first, firing neon-22 ions at a target of plutonium-242. The reaction products were immediately chlorinated, and the team claimed they had made a new element which had formed a volatile chloride, though they were not clear about which isotope they might have made, or even its half-life. Three years later, an American team bombarded californium-249 with carbon-12 ions, and were confident they had made rutherfordium-257, identifying its alpha-decay product, an isotope of nobelium. This was confirmed by a different American team in 1973. Subsequently rutherfordium was also made in 1985 by a German team at Darmstadt, who bombarded a lead-208 target with titanium-50 ions, in other words a lighter target but a heavier projectile. Since it wasn't clear who the true 'discoverer' was, both the Americans and the Russians suggested names for element 104. The Americans called it rutherfordium, after Ernest Rutherford, who pioneered the planetary model of the atom and discovered nuclear fission, whilst the Russians chose kurchatovium after Igor Vasilyevich Kurchatov, a pioneering Russian nuclear physicist who led the project to make the first Russian atom bomb. After much dispute, IUPAC, the institute who officially names new elements, selected the name Rutherfordium. Several isotopes of rutherfordium have half-lives in the order of seconds, making chemical experiments possible before the atoms decay. Rutherfordium-261 has a half-life of just over a minute; rutherfordium-263 has a half-life of 10 minutes and rutherfordium-267 may have a half life of over an hour, but so far the experiments have to be carried out with the lighter isotopes that are easier to make, like rutherfordium-261. Because it has been around for longer and its isotopes are better known, more is known about the chemistry of rutherfordium than of any succeeding element. Working with rutherfordium requires specialist methods and knowledge, as it involves working with tiny quantities of very short-lived, radioactive atoms. This means that as soon as a new atom has been made, it has to be whipped away from the action before it decays. So new atoms of rutherfordium have to be collected as soon as they recoil from the target, and then be transported by an aerosol before being chlorinated and chromatographed before passing to a detector. It has been found that in solution, rutherfordium behaves very similarly to zirconium and hafnium, but unlike the trivalent actinides, leading chemists to concluded that rutherfordium belongs in the same group as Zr and Hf, rather than being a kind of super-actinide. It also forms quite strong chloride complexes in solution, again resembling zirconium and hafnium rather than the actinides or Group I and II metals. Rutherfordium chloride is believed to be RfCl4. It condenses around 220°C, similar to zirconium chloride but more volatile than hafnium chloride and much more volatile than the actinide tetrachlorides. Similarly rutherfordium bromide is more volatile than hafnium bromide. So even though it is extremely unlikely that enough of any rutherfordium compound is going to be isolated in visible quantities, we do know enough to see which family rutherfordium belongs in. That's another triumph for our understanding of the periodic table. Meera Senthilingam Triumph indeed when the half lives of the isotopes involved are a matter of seconds. That was Uppingham School's Simon Cotton with the chemistry of the first transactinide rutherfordium. Now next week an element that some may unfairly consider useless when it certainly does have its uses. Brian Clegg For a long time thulium was a Cinderella substance. There was nothing you could do with thulium that couldn't be done better and cheaper with one of the other elements. It's notable that one science writer has said of thulium 'the most surprising thing about it is there's nothing surprising about it.' But that's a little unfair. Thulium 170 with a half life of 128 days, produced by bombarding thulium in a nuclear reactor, has proved a good portable source of X-rays. It was first suggested for this role in the 1950s and has frequently turned up since in small scale devices, such as those used in dentist's surgeries, but also find it cropping up in engineering, where the X-rays can be used to hunt for cracks in components. Meera Senthilingam And join Brian Clegg to find out how this rare earth element was discovered and why it's considered more valuable than platinum in next week's Chemistry in its element. Until then I'm Meera Senthilingam and thank you for listening. (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.
