|Name, symbol||copernicium, Cn|
|Copernicium in the periodic table|
|Atomic number (Z)||112|
|Group, block||group 12, d-block|
|Element category||transition metal|
|Standard atomic weight (Ar)|||
|Electron configuration||[Rn] 5f14 6d10 7s2 (predicted)|
|2, 8, 18, 32, 32, 18, 2 (predicted)|
−108 K (84+112
−108 °C, 183+202
|Density near r.t.||23.7 g/cm3 (predicted)|
|Oxidation states||4, 2, 1, 0 (predicted)|
|Ionization energies||1st: 1154.9 kJ/mol
2nd: 2170.0 kJ/mol
3rd: 3164.7 kJ/mol
(more) (all estimated)
|Atomic radius||empirical: 147 pm (predicted)|
|Covalent radius||122 pm (predicted)|
|Crystal structure||hexagonal close-packed (hcp)
|Naming||after Nicolaus Copernicus|
|Discovery||Gesellschaft für Schwerionenforschung (1996)|
|Most stable isotopes of copernicium|
Copernicium is a chemical element with symbol Cn and atomic number 112. It is an extremely radioactive synthetic element that can only be created in a laboratory. The most stable known isotope, copernicium-285, has a half-life of approximately 29 seconds. Copernicium was first created in 1996 by the GSI Helmholtz Centre for Heavy Ion Research near Darmstadt, Germany. It is named after the astronomer Nicolaus Copernicus.
In the periodic table of the elements, it is a d-block transactinide element. During reactions with gold, it has been shown to be an extremely volatile metal and a group 12 element, so much so that it is probably a gas at standard temperature and pressure. Copernicium is calculated to have several properties that differ between it and its lighter homologues, zinc, cadmium and mercury; the most notable of them is withdrawing two 6d-electrons before 7s ones due to relativistic effects, which confirm copernicium as an undisputed transition metal. Copernicium is also calculated to show a predominance of the oxidation state +4, while mercury shows it in only one compound at extreme conditions and zinc and cadmium do not show it at all. It has also been predicted to be more difficult to oxidise copernicium from its neutral state than the other group 12 elements.
Copernicium was first created on February 9, 1996, at the Gesellschaft für Schwerionenforschung (GSI) in Darmstadt, Germany, by Sigurd Hofmann, Victor Ninov et al. This element was created by firing accelerated zinc-70 nuclei at a target made of lead-208 nuclei in a heavy ion accelerator. A single atom (the second was subsequently dismissed) of copernicium was produced with a mass number of 277.
82Pb + 70
30Zn → 278
112Cn* → 277
112Cn + 1
In May 2000, the GSI successfully repeated the experiment to synthesize a further atom of copernicium-277. This reaction was repeated at RIKEN using the Search for a Super-Heavy Element Using a Gas-Filled Recoil Separator set-up in 2004 and 2013 to synthesize three further atoms and confirm the decay data reported by the GSI team.
The IUPAC/IUPAP Joint Working Party (JWP) assessed the claim of discovery by the GSI team in 2001 and 2003. In both cases, they found that there was insufficient evidence to support their claim. This was primarily related to the contradicting decay data for the known nuclide rutherfordium-261. However, between 2001 and 2005, the GSI team studied the reaction 248Cm(26Mg,5n)269Hs, and were able to confirm the decay data for hassium-269 and rutherfordium-261. It was found that the existing data on rutherfordium-261 was for an isomer, now designated rutherfordium-261m.
In May 2009, the JWP reported on the claims of discovery of element 112 again and officially recognized the GSI team as the discoverers of element 112. This decision was based on the confirmation of the decay properties of daughter nuclei as well as the confirmatory experiments at RIKEN.
Using Mendeleev's nomenclature for unnamed and undiscovered elements, copernicium should be known as eka-mercury. In 1979, IUPAC published recommendations according to which the element was to be called ununbium (with the corresponding symbol of Uub), a systematic element name as a placeholder, until the element was discovered (and the discovery then confirmed) and a permanent name was decided on. Although widely used in the chemical community on all levels, from chemistry classrooms to advanced textbooks, the recommendations were mostly ignored among scientists in the field, who either called it "element 112", with the symbol of (112) or even simply 112.
After acknowledging the GSI team's discovery, the IUPAC asked them to suggest a permanent name for element 112. On 14 July 2009, they proposed copernicium with the element symbol Cp, after Nicolaus Copernicus "to honor an outstanding scientist, who changed our view of the world".
During the standard six-month discussion period among the scientific community about the naming, it was pointed out that the symbol Cp was previously associated with the name cassiopeium (cassiopium), now known as lutetium (Lu). For this reason, the IUPAC disallowed the use of Cp as a future symbol, prompting the GSI team to put forward the symbol Cn as an alternative. On 19 February 2010, the 537th anniversary of Copernicus' birth, IUPAC officially accepted the proposed name and symbol.
|278Cn||10? ms||α, SF ?||unknown||—|
|279Cn||0.2? ms||α, SF ?||unknown||—|
|280Cn||0.5? ms||α, SF ?||unknown||—|
|283Cn||4 s||α, SF||2002||238U(48Ca,3n)|
Copernicium has no stable or naturally-occurring isotopes. Several radioactive isotopes have been synthesized in the laboratory, either by fusing two atoms or by observing the decay of heavier elements. Six different isotopes have been reported with atomic masses from 281 to 285, and 277. Most of these decay predominantly through alpha decay, but some undergo spontaneous fission.
All copernicium isotopes are extremely unstable and radioactive; in general, heavier isotopes are more stable than the lighter. The most stable isotope, 285Cn, has a half-life of 29 seconds. Other isotopes have half-lives shorter than 0.1 seconds. 281Cn and 284Cn both have half-lives of 97 ms, and the other two isotopes have half-lives slightly under one millisecond. It is predicted that the heavy isotopes 291Cn and 293Cn may have half-lives of around 1200 years, and may have been produced in the r-process and be detectable in cosmic rays, though they would be about 10−12 times as abundant as lead.
The lightest isotopes were synthesized by direct fusion between two lighter nuclei and as decay products (except for 277Cn, which is not known to be a decay product), while the heavier isotopes are only known to be produced by decay of heavier nuclei. The heaviest isotope produced by direct fusion is 283Cn; the two heavier isotopes, 284Cn and 285Cn have only been observed as decay products of elements with larger atomic numbers. In 1999, American scientists at the University of California, Berkeley, announced that they had succeeded in synthesizing three atoms of 293Uuo. These parent nuclei were reported to have successively emitted three alpha particles to form copernicium-281 nuclei, which were claimed to have undergone an alpha decay, emitting an alpha particle with decay energy of 10.68 MeV and half-life 0.90 ms, but their claim was retracted in 2001. The isotope, however, was produced in 2010 by the same team. The new data contradicted the previous (fabricated) data.
Copernicium is the last member of the 6d series of transition metals and the heaviest group 12 element in the periodic table, below zinc, cadmium and mercury. It is predicted to differ significantly from the lighter group 12 elements. Due to stabilization of 7s electronic orbitals and destabilization of 6d ones caused by relativistic effects, Cn2+ is likely to have a [Rn]5f146d87s2 electronic configuration, using the 6d orbitals before the 7s one, unlike its homologues. The fact that the 6d electrons participate readily in chemical bonding mean that copernicium should behave more like a transition metal than its lighter homologues, especially in the +4 oxidation state. In water solutions, copernicium is likely to form the +2 and +4 oxidation states, with the latter one being more stable. Among the lighter group 12 members, for which the +2 oxidation state is the most common, only mercury can show the +4 oxidation state, but it is highly uncommon, existing at only one compound (mercury(IV) fluoride, HgF4) at extreme conditions. The analogous compound for copernicium, copernicium(IV) fluoride (CnF4), is predicted to be more stable. The diatomic ion Hg2+
2, featuring mercury in the +1 oxidation state, is well-known, but the Cn2+
2 ion is predicted to be unstable or even non-existent. Oxidation of copernicium from its neutral state is also likely to be more difficult than those of previous group 12 members. Copernicium(II) fluoride, CnF2, should be more unstable than the analogous mercury compound, mercury(II) fluoride (HgF2), and may even decompose spontaneously into its constituent elements. In polar solvents, copernicium is predicted to preferentially form the CnF−
5 and CnF−
3 anions rather than the analogous neutral fluorides (CnF4 and CnF2, respectively), although the analogous bromide or iodide ions may be more stable towards hydrolysis in aqueous solution. The anions CnCl2−
4 and CnBr2−
4 should also be able to exist in aqueous solution.
The valence s-subshells of the group 12 elements and period 7 elements are expected to be relativistically contracted most strongly at copernicium. This and the closed-shell configuration of copernicium result in it probably being a very noble metal. Its metallic bonds should also be very weak, possibly making it extremely volatile, like the noble gases, and potentially making it gaseous at room temperature. However, it should be able to form metal–metal bonds with copper, palladium, platinum, silver, and gold; these bonds are predicted to be only about 15–20 kJ/mol weaker than the analogous bonds with mercury.
Physical and atomic
Copernicium should be a very heavy metal with a density of around 23.7 g/cm3 in the solid state; in comparison, the most dense known element that has had its density measured, osmium, has a density of only 22.61 g/cm3. This results from copernicium's high atomic weight, the lanthanide and actinide contractions, and relativistic effects, although production of enough copernicium to measure this quantity would be impractical, and the sample would quickly decay. However, some calculations predict copernicium to be a gas at room temperature, the first gaseous metal in the periodic table (the second being flerovium), due to the closed-shell electron configurations of copernicium and flerovium. The atomic radius of copernicium is expected to be around 147 pm. Due to the relativistic stabilization of the 7s orbital and destabilization of the 6d orbital, the Cn+ and Cn2+ ions are predicted to give up 6d electrons instead of 7s electrons, which is the opposite of the behavior of its lighter homologues.
In addition to the relativistic contraction and binding of the 7s subshell, the 6d5/2 orbital is expected to be destabilized due to spin-orbit coupling, making it behave similarly to the 7s orbital in terms of size, shape, and energy. Hence copernicium may not be a noble transition metal, but rather a semiconductor with a band gap of around 0.2 eV. Copernicium is expected to crystallize in the hexagonal close-packed crystal structure, with lattice parameters a = 332 pm and c = 540 pm. The c/a ratio of 1.63 is the ideal value, establishing a kinship between solid copernicium and the solid noble gases, though its cohesive energy (enthalpy of crystallization) should be on the order of that of mercury rather than be near the lower value of the noble gases.
Experimental atomic gas phase chemistry
Interest in copernicium's chemistry was sparked by predictions that it would have the largest relativistic effects in the whole of period 7 and group 12. Copernicium has the ground state electron configuration [Rn]5f146d107s2 and thus should belong to group 12 of the periodic table, according to the Aufbau principle. As such, it should behave as the heavier homologue of mercury and form strong binary compounds with noble metals like gold. Experiments probing the reactivity of copernicium have focused on the adsorption of atoms of element 112 onto a gold surface held at varying temperatures, in order to calculate an adsorption enthalpy. Owing to relativistic stabilization of the 7s electrons, copernicium shows radon-like properties. Experiments were performed with the simultaneous formation of mercury and radon radioisotopes, allowing a comparison of adsorption characteristics.
The first experiments were conducted using the 238U(48Ca,3n)283Cn reaction. Detection was by spontaneous fission of the claimed parent isotope with half-life of 5 minutes. Analysis of the data indicated that copernicium was more volatile than mercury and had noble gas properties. However, the confusion regarding the synthesis of copernicium-283 has cast some doubt on these experimental results. Given this uncertainty, between April–May 2006 at the JINR, a FLNR–PSI team conducted experiments probing the synthesis of this isotope as a daughter in the nuclear reaction 242Pu(48Ca,3n)287Fl. In this experiment, two atoms of copernicium-283 were unambiguously identified and the adsorption properties indicated that copernicium is a more volatile homologue of mercury, due to formation of a weak metal-metal bond with gold, placing it firmly in group 12.
In April 2007, this experiment was repeated and a further three atoms of copernicium-283 were positively identified. The adsorption property was confirmed and indicated that copernicium has adsorption properties completely in agreement with being the heaviest member of group 12. These experiments also allowed the first experimental estimation of copernicium's boiling point: 84+112
−108 °C, so that it may be a gas at standard conditions.
- Hoffman, Darleane C.; Lee, Diana M.; Pershina, Valeria (2006). "Transactinides and the future elements". In Morss; Edelstein, Norman M.; Fuger, Jean. The Chemistry of the Actinide and Transactinide Elements (3rd ed.). Dordrecht, The Netherlands: Springer Science+Business Media. ISBN 1-4020-3555-1.
- Soverna S 2004, 'Indication for a gaseous element 112,' in U Grundinger (ed.), GSI Scientific Report 2003, GSI Report 2004-1, p. 187, ISSN 0174-0814
- Eichler, R.; Aksenov, N. V.; Belozerov, A. V.; Bozhikov, G. A.; Chepigin, V. I.; Dmitriev, S. N.; Dressler, R.; Gäggeler, H. W.; et al. (2008). "Thermochemical and physical properties of element 112". Angewandte Chemie. 47 (17): 3262–6. doi:10.1002/anie.200705019. Retrieved 5 November 2013.
- H. W. Gäggeler (2007). "Gas Phase Chemistry of Superheavy Elements" (PDF). Paul Scherrer Institute. pp. 26–28.
- Fricke, Burkhard (1975). "Superheavy elements: a prediction of their chemical and physical properties". Recent Impact of Physics on Inorganic Chemistry. 21: 89–144. doi:10.1007/BFb0116498. Retrieved 4 October 2013.
- Chemical Data. Copernicium - Cn, Royal Chemical Society
- Gaston, Nicola; Opahle, Ingo; Gäggeler, Heinz W.; Schwerdtfeger, Peter (2007). "Is eka-mercury (element 112) a group 12 metal?". Angewandte Chemie. 46 (10): 1663–6. doi:10.1002/anie.200604262. Retrieved 5 November 2013.
- Chart of Nuclides. Brookhaven National Laboratory
- Eichler, R.; et al. (2007). "Chemical Characterization of Element 112". Nature. 447 (7140): 72–75. Bibcode:2007Natur.447...72E. doi:10.1038/nature05761. PMID 17476264.
- Hofmann, S.; et al. (1996). "The new element 112". Zeitschrift für Physik A. 354 (1): 229–230. doi:10.1007/BF02769517.
- Hofmann, S.; et al. (2002). "New Results on Element 111 and 112". European Physical Journal A. 14 (2): 147–57. doi:10.1140/epja/i2001-10119-x.
- Hofmann, S.; et al. (2000). "New Results on Element 111 and 112" (PDF). Gesellschaft für Schwerionenforschung.
- Morita, K. (2004). "Decay of an Isotope 277112 produced by 208Pb + 70Zn reaction". In Penionzhkevich, Yu. E.; Cherepanov, E. A. Exotic Nuclei: Proceedings of the International Symposium. World Scientific. pp. 188–191. doi:10.1142/9789812701749_0027.
- Karol, P. J.; Nakahara, H.; Petley, B. W.; Vogt, E. (2001). "On the Discovery of the Elements 110–112" (PDF). Pure and Applied Chemistry. 73 (6): 959–967. doi:10.1351/pac200173060959.
- Karol, P. J.; Nakahara, H.; Petley, B. W.; Vogt, E. (2003). "On the Claims for Discovery of Elements 110, 111, 112, 114, 116 and 118" (PDF). Pure and Applied Chemistry. 75 (10): 1061–1611. doi:10.1351/pac200375101601.
- Dressler, R.; Türler, A. (2001). "Evidence for Isomeric States in 261Rf" (PDF). Annual Report. Paul Scherrer Institute.
- "A New Chemical Element in the Periodic Table". Gesellschaft für Schwerionenforschung. 10 June 2009.
- Barber, R. C.; et al. (2009). "Discovery of the element with atomic number 112" (PDF). Pure and Applied Chemistry. 81 (7): 1331. doi:10.1351/PAC-REP-08-03-05.
- Chatt, J. (1979). "Recommendations for the naming of elements of atomic numbers greater than 100". Pure and Applied Chemistry. 51 (2): 381–384. doi:10.1351/pac197951020381.
- "New Chemical Element In The Periodic Table". Science Daily. 11 June 2009.
- "Element 112 shall be named "copernicium"". Gesellschaft für Schwerionenforschung. 14 July 2009.
- "New element named 'copernicium'". BBC News. 16 July 2009. Retrieved 2010-02-22.
- "Start of the Name Approval Process for the Element of Atomic Number 112". IUPAC. 20 July 2009.
- Meija, J. (2009). "The need for a fresh symbol to designate copernicium". Nature. 461 (7262): 341. Bibcode:2009Natur.461..341M. doi:10.1038/461341c. PMID 19759598.
- van der Krogt, P. "Lutetium". Elementymology & Elements Multidict. Retrieved 2010-02-22.
- "IUPAC Element 112 is Named Copernicium". IUPAC. 19 February 2010. Retrieved 2012-04-13.
- Holden, N. E. (2004). "Table of the Isotopes". In D. R. Lide. CRC Handbook of Chemistry and Physics (85th ed.). CRC Press. Section 11. ISBN 978-0-8493-0485-9.
- Dullman, C.E. Superheavy Element Research Superheavy Element - News from GSI and Mainz. University Mainz
- Barber, R. C.; et al. (2011). "Discovery of the elements with atomic numbers greater than or equal to 113" (PDF). Pure and Applied Chemistry. 83 (7): 5–7. doi:10.1351/PAC-REP-10-05-01.
- Zagrebaev, Valeriy; Karpov, Alexander; Greiner, Walter (2013). "Future of superheavy element research: Which nuclei could be synthesized within the next few years?" (PDF). Journal of Physics: Conference Series. IOP Science. pp. 1–15. Retrieved 20 August 2013.
- Ninov, V.; et al. (1999). "Observation of Superheavy Nuclei Produced in the Reaction of 86Kr with 208Pb". Physical Review Letters. 83 (6): 1104–1107. Bibcode:1999PhRvL..83.1104N. doi:10.1103/PhysRevLett.83.1104.
- Public Affairs Department (21 July 2001). "Results of element 118 experiment retracted". Berkeley Lab. Retrieved 2008-01-18.
- At Lawrence Berkeley, Physicists Say a Colleague Took Them for a Ride George Johnson, The New York Times, 15 October 2002
- Public Affairs Department (26 October 2010). "Six New Isotopes of the Superheavy Elements Discovered: Moving Closer to Understanding the Island of Stability". Berkeley Lab. Retrieved 2011-04-25.
- Wang, X.; Andrews, L.; Riedel, S.; Kaupp, M. (2007). "Mercury is a Transition Metal: The First Experimental Evidence for HgF4". Angewandte Chemie. 119 (44): 8523–8527. doi:10.1002/ange.200703710.
- "Chemistry on the islands of stability", New Scientist, 11 September 1975, p. 574, ISSN 1032-1233
- Kratz, Jens Volker. The Impact of Superheavy Elements on the Chemical and Physical Sciences. 4th International Conference on the Chemistry and Physics of the Transactinide Elements, 5 – 11 September 2011, Sochi, Russia
- Gäggeler, H. W. (2007). "Gas Phase Chemistry of Superheavy Elements" (PDF). Paul Scherrer Institute. pp. 26–28.
|Look up copernicium in Wiktionary, the free dictionary.|
|Wikimedia Commons has media related to copernicium.|
|Periodic table (Large cells)|