|Roentgenium in the periodic table|
|Name, symbol, number||roentgenium, Rg, 111|
but probably a transition metal
|Group, period, block||11, 7, d|
|Standard atomic weight|||
|Electron configuration||[Rn] 5f14 6d9 7s2
2, 8, 18, 32, 32, 17, 2
|Density (near r.t.)||28.7 (predicted) g·cm−3|
|Oxidation states||5, 3, 1, −1 (predicted)|
|1st: 1022.7 (estimated) kJ·mol−1|
|2nd: 2074.4 (estimated) kJ·mol−1|
|3rd: 3077.9 (estimated) kJ·mol−1|
|Atomic radius||138 (predicted) pm|
|Covalent radius||121 (estimated) pm|
|Crystal structure||body-centered cubic (predicted)|
|CAS registry number||54386-24-2|
|Naming||after Wilhelm Röntgen|
|Discovery||Gesellschaft für Schwerionenforschung (1994)|
|Most stable isotopes|
|Main article: Isotopes of roentgenium|
Roentgenium is a chemical element with the symbol Rg and atomic number 111. It is an extremely radioactive synthetic element (an element that can be created in a laboratory but is not found in nature); the most stable known isotope, roentgenium-281, has a half-life of 26 seconds. Roentgenium was first created in 1994 by the GSI Helmholtz Centre for Heavy Ion Research near Darmstadt, Germany. It is named after the physicist Wilhelm Röntgen (also spelled Roentgen).
In the periodic table, it is a d-block transactinide element. It is a member of the 7th period and is placed in the group 11 elements, although no chemical experiments have been carried out to confirm that it behaves as the heavier homologue to gold in group 11. Roentgenium is calculated to have similar properties to its lighter homologues, copper, silver, and gold, although it may show some differences from them.
Roentgenium was first synthesized by an international team led by Sigurd Hofmann at the Gesellschaft für Schwerionenforschung (GSI) in Darmstadt, Germany, on December 8, 1994. The team bombarded a target of bismuth-209 with accelerated nuclei of nickel-64 and detected a single atom of the isotope roentgenium-272:
In 2001, the IUPAC/IUPAP Joint Working Party (JWP) concluded that there was insufficient evidence for the discovery at that time. The GSI team repeated their experiment in 2002 and detected three more atoms. In their 2003 report, the JWP decided that the GSI team should be acknowledged for the discovery of this element.
The name roentgenium (Rg) was suggested by the GSI team in 2004, to honor the German physicist Wilhelm Conrad Röntgen, the discoverer of X-rays. This name was accepted by IUPAC on November 1, 2004.
|272Rg||3.8 ms ?||α||1994||209Bi(64Ni,n)|
|273Rg||5? ms||α ?||unknown||—|
|275Rg||10? ms||α ?||unknown||—|
|276Rg||100? ms||α, SF ?||unknown||—|
|277Rg||1? s||α, SF ?||unknown||—|
|281Rg||26 s||α, SF||2009||293Uus(—,3α)|
|283Rg||10? min||α, SF ?||unknown||—|
Roentgenium has no stable or naturally-occurring isotopes. Several radioactive isotopes have been synthesized in the laboratory, either by fusion of the nuclei of lighter elements or as intermediate decay products of heavier elements. Seven different isotopes of roentgenium have been reported with atomic masses 272, 274, and 278–282, two of which, roentgenium-272 and roentgenium-274, have known but unconfirmed metastable states. All of these decay through alpha decay except roentgenium-281, which undergoes spontaneous fission.
Stability and half-lives
All roentgenium isotopes are extremely unstable and radioactive; in general, the heavier isotopes are more stable than the lighter. The most stable known roentgenium isotope, 281Rg, is also the second-heaviest known roentgenium isotope; it has a half-life of 26 seconds. The isotope 280Rg has been reported to also have a half-life of over a second. The isotopes 282Rg and 279Rg have half-lives of 0.5 and 0.17 seconds respectively. The remaining four isotopes have half-lives between 1 and 10 milliseconds. The undiscovered isotope 287Rg has been predicted to be the most stable towards beta decay; however, no known roentgenium isotope has been observed to undergo beta decay. The unknown isotopes 277Rg and 283Rg are also expected to have long half-lives of 1 second and 10 minutes respectively. Before their discovery, the isotopes 278Rg, 281Rg, and 282Rg were predicted to have long half-lives of 1 second, 1 minute, and 4 minutes respectively; however, they were discovered to have shorter half-lives of 4.2 milliseconds, 26 seconds, and 0.5 seconds respectively.
Roentgenium is the ninth member of the 6d series of transition metals. Since copernicium (element 112) has been shown to be a transition metal, it is expected that all the elements from 104 to 112 would form a fourth transition metal series. Calculations on its ionization potentials and atomic and ionic radii are similar to that of its lighter homologue gold, thus implying that roentgenium's basic properties will resemble those of the other group 11 elements, copper, silver, and gold; however, it is also predicted to show several differences from its lighter homologues.
Roentgenium is predicted to be a noble metal. Based on the most stable oxidation states of the lighter group 11 elements, roentgenium is predicted to show stable +5, +3, and −1 oxidation states, with a less stable +1 state. The +3 state is predicted to be the most stable. Roentgenium(III) is expected to be of comparable reactivity to gold(III), but should be more stable and form a larger variety of compounds. Gold also forms a somewhat stable −1 state due to relativistic effects, and roentgenium may do so as well: however, the electron affinity of roentgenium is expected to be around 1.6 eV, significantly lower than gold's value of 2.3 eV, so roentgenides may not be stable or even possible. The 6d orbitals are destabilized by relativistic effects and spin–orbit interactions near the end of the fourth transition metal series, thus making higher oxidation states like roentgenium(V) and copernicium(IV) more stable than their lighter homologues gold(V) and mercury(IV) (each of which are known only in one compound) as the 6d electrons participate in bonding to a greater extent. The spin-orbit interactions stabilize molecular roentgenium compounds with more bonding 6d electrons; for example, RgF−
6 is expected to be more stable than RgF−
4, which is expected to be more stable than RgF−
2. Roentgenium(I) is expected to be difficult to obtain.
The probable chemistry of roentgenium has received more interest than that of the two previous elements, meitnerium and darmstadtium, as the valence s-subshells of the group 11 elements are expected to be relativistically contracted most strongly at roentgenium. Calculations on the molecular compound RgH show that relativistic effects double the strength of the roentgenium–hydrogen bond, even though spin–orbit interactions also weaken it by 0.7 eV. The compounds AuX and RgX, where X = F, Cl, Br, O, Au, or Rg, were also studied. Rg+ should be the softest base among the metal ions, even softer than Au+.
Physical and atomic
Roentgenium is expected to be a solid under normal conditions and to crystallize in the body-centered cubic structure, unlike its lighter congeners which crystallize in the face-centered cubic structure, due to its being expected to have different electron charge densities from them. It should be a very heavy metal with a density of around 28.7 g/cm3; in comparison, the densest known element that has had its density measured, osmium, has a density of only 22.61 g/cm3. This results from roentgenium's high atomic weight, the lanthanide and actinide contractions, and relativistic effects, although production of enough roentgenium to measure this quantity would be impractical, and the sample would quickly decay.
The stable group 11 elements, copper, silver, and gold, all have an outer electron configuration nd10(n+1)s1. For each of these elements, the first excited state of their atoms has a configuration nd9(n+1)s2. Due to spin-orbit coupling between the d electrons, this state is split into a pair of energy levels. For copper, the difference in energy between the ground state and lowest excited state causes the metal to appear reddish. For silver, the energy gap widens and it becomes silvery. However, as the atomic number increases, the excited levels are stabilized by relativistic effects and in gold the energy gap decreases again and it appears gold. For roentgenium, calculations indicate that the 6d97s2 level is stabilized to such an extent that it becomes the ground state and the 6d107s1 level becomes the first excited state. The resulting energy difference between the new ground state and the first excited state is similar to that of silver and roentgenium is expected to be silvery in appearance. The atomic radius of roentgenium is expected to be around 138 pm.
Unambiguous determination of the chemical characteristics of roentgenium has yet to have been established due to the low yields of reactions that produce roentgenium isotopes. For chemical studies to be carried out on a transactinide, at least four atoms must be produced, the half-life of the isotope used must be at least 1 second, and the rate of production must be at least one atom per week. Even though the half-life of 281Rg, the most stable known roentgenium isotope, is 26 seconds, long enough to perform chemical studies, another obstacle is the need to increase the rate of production of roentgenium isotopes and allow experiments to carry on for weeks or months so that statistically significant results can be obtained. Separation and detection must be carried out continuously to separate out the roentgenium isotopes and automated systems can then experiment on the gas-phase and solution chemistry of roentgenium as the yields for heavier elements are predicted to be smaller than those for lighter elements. However, the experimental chemistry of roentgenium has not received as much attention as that of the heavier elements copernicium and flerovium.
- Turler, A. (2004). "Gas Phase Chemistry of Superheavy Elements". Journal of Nuclear and Radiochemical Sciences 5 (2): R19–R25.
- Haire, Richard G. (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.
- Östlin, A.; Vitos, L. (2011). "First-principles calculation of the structural stability of 6d transition metals". Physical Review B 84 (11). Bibcode:2011PhRvB..84k3104O. doi:10.1103/PhysRevB.84.113104.
- 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. Roentgenium - Rg, Royal Chemical Society
- Oganessian, Y. T.; Abdullin, F. S.; Alexander, C. et al. (2013). "Experimental studies of the 249Bk + 48Ca reaction including decay properties and excitation function for isotopes of element 117, and discovery of the new isotope 277Mt". Physical Review C 87 (5). Bibcode:2013PhRvC..87e4621O. doi:10.1103/PhysRevC.87.054621.
- Hofmann, S.; Ninov, V.; Heßberger, F. P.; Armbruster, P.; Folger, H.; Münzenberg, G.; Schött, H. J.; Popeko, A. G.; Yeremin, A. V.; Andreyev, A. N.; Saro, S.; Janik, R.; Leino, M. (1995). "The new element 111". Zeitschrift für Physik A 350 (4): 281. Bibcode:1995ZPhyA.350..281H. doi:10.1007/BF01291182.
- Karol et al.; Nakahara, H.; Petley, B. W.; Vogt, E. (2001). "On the discovery of the elements 110–112". Pure Appl. Chem. 73 (6): 959–967. doi:10.1351/pac200173060959.
- Hofmann, S.; Heßberger, F. P.; Ackermann, D.; Münzenberg, G.; Antalic, S.; Cagarda, P.; Kindler, B.; Kojouharova, J.; Leino, M.; Lommel, B.; Mann, R.; Popeko, A. G.; Reshitko, S.; Śaro, S.; Uusitalo, J.; Yeremin, A. V. (2002). "New results on elements 111 and 112". European Physical Journal A 14 (2): 147–157. doi:10.1140/epja/i2001-10119-x.
- Hofmann et al. "New results on element 111 and 112". GSI report 2000. Retrieved 2008-03-02.
- 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". Pure Appl. Chem. 75 (10): 1601–1611. doi:10.1351/pac200375101601.
- Corish, J. et al.; Rosenblatt, G. M. (2004). "Name and symbol of the element with atomic number 111". Pure Appl. Chem. 76 (12): 2101–2103. doi:10.1351/pac200476122101.
- Corish et al.; Rosenblatt, G. M. (2004). "Name and symbol of the element with atomic number 111". Pure Appl. Chem. 76 (12): 2101–2103. doi:10.1351/pac200476122101.
- Sonzogni, Alejandro. "Interactive Chart of Nuclides". National Nuclear Data Center: Brookhaven National Laboratory. Retrieved 2008-06-06.
- Morita, Kosuke; Morimoto, Kouji; Kaji, Daiya; Akiyama, Takahiro; Goto, Sin-ichi; Haba, Hiromitsu; Ideguchi, Eiji; Kanungo, Rituparna; Katori, Kenji; Koura, Hiroyuki; Kudo, Hisaaki; Ohnishi, Tetsuya; Ozawa, Akira; Suda, Toshimi; Sueki, Keisuke; Xu, HuShan; Yamaguchi, Takayuki; Yoneda, Akira; Yoshida, Atsushi; Zhao, YuLiang (2004). "Experiment on the Synthesis of Element 113 in the Reaction 209Bi(70Zn,n)278113". Journal of the Physical Society of Japan 73 (10): 2593–2596. Bibcode:2004JPSJ...73.2593M. doi:10.1143/JPSJ.73.2593.
- Oganessian, Yu. Ts.; Penionzhkevich, Yu. E.; Cherepanov, E. A. (2007). "Heaviest Nuclei Produced in 48Ca-induced Reactions (Synthesis and Decay Properties)". AIP Conference Proceedings 912. p. 235. doi:10.1063/1.2746600.
- Oganessian, Y. T.; Abdullin, F. S.; Bailey, P. D. et al. (2010). "Synthesis of a New Element with Atomic Number Z=117". Physical Review Letters 104 (14): 142502. Bibcode:2010PhRvL.104n2502O. doi:10.1103/PhysRevLett.104.142502. PMID 20481935.
- Nie, G. K. (2005). "Charge radii of β-stable nuclei". Modern Physics Letters A 21 (24): 1889. arXiv:nucl-th/0512023. Bibcode:2006MPLA...21.1889N. doi:10.1142/S0217732306020226.
- Griffith, W. P. (2008). "The Periodic Table and the Platinum Group Metals". Platinum Metals Review 52 (2): 114. doi:10.1595/147106708X297486.
- Seth, M.; Cooke, F.; Schwerdtfeger, P.; Heully, J.-L.; Pelissier, M. (1998). "The chemistry of the superheavy elements. II. The stability of high oxidation states in group 11 elements: Relativistic coupled cluster calculations for the di-, tetra- and hexafluoro metallates of Cu, Ag, Au, and element 111". J. Chem. Phys 109 (10): 3935–43. Bibcode:1998JChPh.109.3935S. doi:10.1063/1.476993.
- Seth, M.; Faegri, K.; Schwerdtfeger, P. (1998). "The Stability of the Oxidation State +4 in Group 14 Compounds from Carbon to Element 114". Angew. Chem. Int. Ed. Engl. 37 (18): 2493–6. doi:10.1002/(SICI)1521-3773(19981002)37:18<2493::AID-ANIE2493>3.0.CO;2-F.
- Liu, W.; van Wüllen, C. (1999). "Spectroscopic constants of gold and eka-gold (element 111) diatomic compounds: The importance of spin–orbit coupling". J. Chem. Phys 110 (8): 3730–5. Bibcode:1999JChPh.110.3730L. doi:10.1063/1.478237.
- Thayer, John S. (2010). Chemistry of heavier main group elements. p. 82. doi:10.1007/9781402099755_2.
- Düllmann, Christoph E. (2012). "Superheavy elements at GSI: a broad research program with element 114 in the focus of physics and chemistry". Radiochimica Acta 100 (2): 67–74. doi:10.1524/ract.2011.1842.
|Periodic table (Large version)|