| Discovery date | 1994 |
| Discovered by |
Sigurd Hofmann, Peter Armbruster and Gottfried Münzenberg
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| Origin of the name | Darmstadtium is named after Darmstadt, Germany, where the element was first produced. |
| Allotropes |
|
Ds
Darmstadtium
110
[281]
| Group | 10 | Melting point | Unknown |
| Period | 7 | Boiling point | Unknown |
| Block | d | Density (g cm−3) | Unknown |
| Atomic number | 110 | Relative atomic mass | [281] |
| State at 20°C | Solid | Key isotopes | 281Ds |
| Electron configuration | [Rn] 5f146d97s1 | CAS number | 54083-77-1 |
| ChemSpider ID | - | ChemSpider is a free chemical structure database | |
Image explanation
Darmstadtium is highly radioactive, so the image is based on an abstracted atomic model and trails of sub-atomic particles.
Appearance
A highly radioactive metal, of which only a few atoms have ever been made.
Uses
At present, it is only used in research.
Biological role
Darmstadtium has no known biological role.
Natural abundance
A man-made element of which only a few atoms have ever been created. It that is formed by fusing nickel and lead atoms in a heavy ion accelerator.
There are 15 known isotopes of darmstadtium, isotopes 267-281, and the heaviest is the longest-lived, with a half-life of 4 minutes.
There were several attempts to make element 110 at the Joint Institute for Nuclear Research (JINR) at Dubna in Russia, and at the German Geselleschaft für Schwerionenforschung (GSI) at Darmstadt, but all were unsuccessful. Then Albert Ghiorso and his team at the Lawrence Berkeley National Laboratory (LBNL), California, obtained isotope 267 by bombarding bismuth with cobalt, but they could not confirm their findings.
In 1994, a team headed by Yuri Oganessian and Vladimir Utyonkov at the JINR made isotope-273 by bombarding plutonium with sulfur. The same year, a team headed by Peter Armbruster and Gottfried Munzenberg at the GSI bombarded lead with nickel and synthesised isotope 269. The latter group’s evidence was deemed more reliable and confirmed by others around the world, so they were allowed to name element 110.
| Atomic radius, non-bonded (Å) | Unknown | Covalent radius (Å) | 1.28 |
| Electron affinity (kJ mol−1) | Unknown |
Electronegativity (Pauling scale) |
Unknown |
|
Ionisation energies (kJ mol−1) |
1st
-
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 |
| 281Ds | 281.165 | - | 13 s | 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 Darmstadtium Podcast |
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Transcript :
Chemistry in its element: darmstadtium(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, an element that brings fleeting moments of wonder. Here's Brian Clegg. Brian Clegg I've a coffee cup on my desk, a Christmas present from my niece, inscribed with the periodic table. There, at element 110 beneath platinum, is the clumsy and practically unpronounceable ununnilium - just a fancy way of saying 'one one oh - ium'. A range of artificial elements were originally given placeholder names like this back in 1979 by the International Union of Pure and Applied Chemistry, the body that controls the naming of chemical elements. Often this was because there was a dispute over just who had discovered the element and got the honour of naming it, but now, I'm glad to say, element 110 has a more manageable name, darmstadtium and my mug is out of date. This is one of the transfermium elements, the discontinuous block above element 100 that takes in a couple of the actinides and the row that continues after the actinides with lawrencium. If there is one thing that typifies darmstadtium it's that it is an element of speed. The first isotope discovered, darmstadtium 269, has a minuscule half life of just 270 microseconds. Before you can cry out in triumph 'We've made darmstadtium!' it is long gone. This brevity contributed to the disputes over who first made element 110. It was claimed by both the Joint Institute for Nuclear Research in Dubna, Russia in 1987 and by the Lawrence Berkeley Laboratory in 1991, but there was considerable doubt about both claims. Darmstadtium was to get its name after the location of the Gesellschaft für Schwerionenforschung, roughly translating as the 'centre for heavy ion research'. Usually contracted to the more easily pronounced GSI, and part of the impressively named German government group of establishments the Hermann von Helmholtz-Gemeinschaft Deutscher Forschungszentren, the GSI is located at Darmstadt in Germany. The alternative name of wixhausium was briefly considered for the element, after Wixhausen, the part of Darmstadt where the institute is located, but darmstadtium was considered to have a better ring to it. In 1994, at the GSI, an international team slammed high energy nickel ions into a lead target. The group, led by Sigurd Hofmann, included German physicists Peter Armbruster and Gottfried Münzenberg, a pair who between them have brought six of the transfermium elements into existence. Despite throwing in 3 trillion ions per second, just 3 atoms of darmstadtium 269 were produced, decaying to hassium, seaborgium and rutherfordium in the blink of an eye. To date, a handful of other isotopes have been made, all blinking out of existence before there's a chance to investigate their properties. There is some dispute over just what the half-lives are, but the longest is probably darmstadtium 281 at 11 seconds. The expectation, if we could study a piece of darmstadtium is that this would be a silvery metal, not unlike platinum in behaviour - but short of slowing down time, no one is going to get a chance to see. It's worth taking a closer look at just how darmstadtium was brought into being. Like all the elements heavier than uranium, it does not exist at all in nature. Up to around the element 100 mark, the heavier elements can be produced by pumping in neutrons, which undergo beta decay, giving off an electron, to add extra protons to the nucleus. But for heavier atoms still, like darmstadtium, it is necessary to slam particles like the nickel ions used here into a nucleus at velocities around 10 per cent of the speed of light, giving them enough energy to overcome the powerful electromagnetic repulsion of the nucleus, and allowing fusion to take place. The nickel ions were accelerated by UNILAC, short for 'universal linear accelerator' a 120 metre long straight acceleration chamber at the GSI where a series of powerful electromagnets blast charged particles along at higher and higher speeds. The vast majority of collisions fail, but just occasionally the nuclei fuse, typically losing a small number of neutrons and settle down to a short-lived new element. In the case of darmstadtium, the nucleus soon emits alpha particles - helium nuclei consisting of two protons and two neutrons bound together - which transforms the darmstadtium into its longer-lived decay products. With so many trillions of particles being shot down the accelerator, it is a difficult task to separate the very few products where fusion has taken place. This is the job of a second piece of technology called SHIP, the Separator for Heavy Ion reactor Products. SHIP acts as a filter - by balancing electric and magnetic fields very precisely, only the particular heavy reaction products, in our case, darmstadtium, that are selected for get through without being deflected out of the way. Rather confusingly, despite its short-lived nature, you may find yourself taking a visit to Darmstadtium or even holding a meeting there. This is because the town of Darmstadt took the name from the element for its science and meetings building - in essence a convention centre - opened in 2008. If elements were insects, darmstadtium would be the mayfly of the chemical world. It exists for the most fleeting time before it transforms to something else. Darmstadium is never going to have a practical use - but its sheer brevity of existence gives it a wistful fascination. Meera Senthilingam So its lack of application is made up for by the wistful wonder of its chemistry. That was science writer, Brian Clegg, with the fast paced chemistry of darmstadium. Now next week, we get minty fresh. Lars Ohrstrom If you chew gum, you will most likely encounter another result of rhodium catalysis, menthol. Originally extracted from different species of mint plants, the demand for this substance, with its characteristic minty scent, far exceeds the natural sources and it is now produced in several thousand tonnes a year in the process devised by Japanese Nobel Prize winner Ryoji Noyori. Meera Senthilingam And for other uses of the rare element, rhodium, join Lars Ohrstrom in next weeks Chemistry in its element and 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.
