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Oganesson is a transactinide chemical element with symbol Og and atomic number 118. It was first synthesized in 2002 by a joint team of Russian and American scientists at the Joint Institute for Nuclear Research (JINR) in Dubna, Russia. In December 2015, it was recognized as one of four new elements by the Joint Working Party of international scientific bodies IUPAC and IUPAP. It was formally named on 28 November 2016.[12][13] The name is in line with the tradition of honoring a scientist and recognizes nuclear physicist Yuri Oganessian, who has played a leading role in the discovery of the heaviest elements in the periodic table. It is one of only two elements named after a living person at the time of naming, the other being seaborgium.[14]

Oganesson,  118Og
General properties
Pronunciation /ɒɡəˈnɛsɒn/
Mass number 294 (most stable isotope)
Oganesson in the periodic table
Hydrogen (diatomic nonmetal)
Helium (noble gas)
Lithium (alkali metal)
Beryllium (alkaline earth metal)
Boron (metalloid)
Carbon (polyatomic nonmetal)
Nitrogen (diatomic nonmetal)
Oxygen (diatomic nonmetal)
Fluorine (diatomic nonmetal)
Neon (noble gas)
Sodium (alkali metal)
Magnesium (alkaline earth metal)
Aluminium (post-transition metal)
Silicon (metalloid)
Phosphorus (polyatomic nonmetal)
Sulfur (polyatomic nonmetal)
Chlorine (diatomic nonmetal)
Argon (noble gas)
Potassium (alkali metal)
Calcium (alkaline earth metal)
Scandium (transition metal)
Titanium (transition metal)
Vanadium (transition metal)
Chromium (transition metal)
Manganese (transition metal)
Iron (transition metal)
Cobalt (transition metal)
Nickel (transition metal)
Copper (transition metal)
Zinc (post-transition metal)
Gallium (post-transition metal)
Germanium (metalloid)
Arsenic (metalloid)
Selenium (polyatomic nonmetal)
Bromine (diatomic nonmetal)
Krypton (noble gas)
Rubidium (alkali metal)
Strontium (alkaline earth metal)
Yttrium (transition metal)
Zirconium (transition metal)
Niobium (transition metal)
Molybdenum (transition metal)
Technetium (transition metal)
Ruthenium (transition metal)
Rhodium (transition metal)
Palladium (transition metal)
Silver (transition metal)
Cadmium (post-transition metal)
Indium (post-transition metal)
Tin (post-transition metal)
Antimony (metalloid)
Tellurium (metalloid)
Iodine (diatomic nonmetal)
Xenon (noble gas)
Caesium (alkali metal)
Barium (alkaline earth metal)
Lanthanum (lanthanide)
Cerium (lanthanide)
Praseodymium (lanthanide)
Neodymium (lanthanide)
Promethium (lanthanide)
Samarium (lanthanide)
Europium (lanthanide)
Gadolinium (lanthanide)
Terbium (lanthanide)
Dysprosium (lanthanide)
Holmium (lanthanide)
Erbium (lanthanide)
Thulium (lanthanide)
Ytterbium (lanthanide)
Lutetium (lanthanide)
Hafnium (transition metal)
Tantalum (transition metal)
Tungsten (transition metal)
Rhenium (transition metal)
Osmium (transition metal)
Iridium (transition metal)
Platinum (transition metal)
Gold (transition metal)
Mercury (post-transition metal)
Thallium (post-transition metal)
Lead (post-transition metal)
Bismuth (post-transition metal)
Polonium (post-transition metal)
Astatine (metalloid)
Radon (noble gas)
Francium (alkali metal)
Radium (alkaline earth metal)
Actinium (actinide)
Thorium (actinide)
Protactinium (actinide)
Uranium (actinide)
Neptunium (actinide)
Plutonium (actinide)
Americium (actinide)
Curium (actinide)
Berkelium (actinide)
Californium (actinide)
Einsteinium (actinide)
Fermium (actinide)
Mendelevium (actinide)
Nobelium (actinide)
Lawrencium (actinide)
Rutherfordium (transition metal)
Dubnium (transition metal)
Seaborgium (transition metal)
Bohrium (transition metal)
Hassium (transition metal)
Meitnerium (unknown chemical properties)
Darmstadtium (unknown chemical properties)
Roentgenium (unknown chemical properties)
Copernicium (post-transition metal)
Nihonium (unknown chemical properties)
Flerovium (unknown chemical properties)
Moscovium (unknown chemical properties)
Livermorium (unknown chemical properties)
Tennessine (unknown chemical properties)
Oganesson (unknown chemical properties)


Atomic number (Z) 118
Group, period group 18, period 7
Block p-block
Element category   unknown chemical properties, but probably a noble gas
Electron configuration [Rn] 5f14 6d10 7s2 7p6 (predicted)[1][2]
Electrons per shell
2, 8, 18, 32, 32, 18, 8 (predicted)
Physical properties
Phase (at STP) solid (predicted)[1]
Boiling point 350±30 K ​(80±30 °C, ​170±50 °F) (extrapolated)[1]
Density when liquid (at m.p.) 4.9–5.1 g/cm3 (predicted)[3]
Critical point 439 K, 6.8 MPa (extrapolated)[4]
Heat of fusion 23.5 kJ/mol (extrapolated)[4]
Heat of vaporization 19.4 kJ/mol (extrapolated)[4]
Atomic properties
Oxidation states −1,[2] 0, +1,[5] +2,[6] +4,[6] +6[2](predicted)
Ionization energies
  • 1st: 839.4 kJ/mol (predicted)[2]
  • 2nd: 1563.1 kJ/mol (predicted)[7]
Covalent radius 157 pm (predicted)[8]
Crystal structure face-centered cubic (fcc)
Face-centered cubic crystal structure for oganesson

CAS Number 54144-19-3
Naming after Yuri Oganessian
Prediction Niels Bohr (1922)
Discovery Joint Institute for Nuclear Research and Lawrence Livermore National Laboratory (2006)
Main isotopes of oganesson
Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct
294Og[10] syn 0.7 ms[11] α 290Lv
| references | in Wikidata

Oganesson has the highest atomic number and highest atomic mass of all known elements. The radioactive oganesson atom is very unstable, and since 2005, only five (possibly six) atoms of the isotope 294Og have been detected.[15] Although this allowed very little experimental characterization of its properties and possible compounds, theoretical calculations have resulted in many predictions, including some surprising ones. For example, although oganesson is a member of group 18 – the first synthetic element to be so – it may be significantly reactive, unlike all the other elements of that group (the noble gases).[1] It was formerly thought to be a gas under normal conditions but is now predicted to be a solid due to relativistic effects.[1] On the periodic table of the elements it is a p-block element and the last one of the 7th period.



Early speculationEdit

The Danish physicist Niels Bohr was the first to seriously consider the possibility of an element with atomic number as high as 118, noting in 1922 that such an element would take its place in the periodic table below radon as the seventh noble gas.[16] Following this, Aristid von Grosse wrote an article in 1965 predicting the likely properties of element 118. These were remarkably early predictions, given that it was not yet known how to produce elements artificially in 1922, and that the existence of the island of stability had not yet been theorized in 1965. It took eighty years from Bohr's initial prediction before oganesson was first successfully synthesised, although its chemical properties have not yet been investigated to see if it really does behave as the heavier congener of radon.[7]

Unsuccessful synthesis attemptsEdit

In late 1998, Polish physicist Robert Smolańczuk published calculations on the fusion of atomic nuclei towards the synthesis of superheavy atoms, including oganesson.[17] His calculations suggested that it might be possible to make oganesson by fusing lead with krypton under carefully controlled conditions.[17]

In 1999, researchers at Lawrence Berkeley National Laboratory made use of these predictions and announced the discovery of livermorium and oganesson, in a paper published in Physical Review Letters,[18] and very soon after the results were reported in Science.[19] The researchers reported to have performed the reaction

+ 208

The following year, they published a retraction after researchers at other laboratories were unable to duplicate the results and the Berkeley lab could not duplicate them either.[20] In June 2002, the director of the lab announced that the original claim of the discovery of these two elements had been based on data fabricated by principal author Victor Ninov.[21][22]

Discovery reportsEdit

The first decay of atoms of oganesson was observed in 2002 at the Joint Institute for Nuclear Research (JINR) in Dubna, Russia, by a joint team of Russian and American scientists. Headed by Russian nuclear physicist Yuri Oganessian, the team included American scientists of the Lawrence Livermore National Laboratory, California.[23] On 9 October 2006, the researchers announced[10] that they had indirectly detected a total of three (possibly four) nuclei of oganesson-294 (one or two in 2002[24] and two more in 2005) produced via collisions of californium-249 atoms and calcium-48 ions.[25][26][27][28][29]

+ 48
+ 3
Radioactive decay pathway of the isotope oganesson-294.[10] The decay energy and average half-life is given for the parent isotope and each daughter isotope. The fraction of atoms undergoing spontaneous fission (SF) is given in green.

In 2011, IUPAC evaluated the 2006 results of the Dubna–Livermore collaboration and concluded: "The three events reported for the Z = 118 isotope have very good internal redundancy but with no anchor to known nuclei do not satisfy the criteria for discovery".[30]

Because of the very small fusion reaction probability (the fusion cross section is ~0.3–0.6 pb or (3–6)×10−41 m2) the experiment took four months and involved a beam dose of 2.5×1019 calcium ions that had to be shot at the californium target to produce the first recorded event believed to be the synthesis of oganesson.[31] Nevertheless, researchers were highly confident that the results were not a false positive, since the chance that the detections were random events was estimated to be less than one part in 100000.[32]

In the experiments, the alpha-decay of three atoms of oganesson was observed. A fourth decay by direct spontaneous fission was also proposed. A half-life of 0.89 ms was calculated: 294
decays into 290
by alpha decay. Since there were only three nuclei, the half-life derived from observed lifetimes has a large uncertainty: 0.89+1.07

+ 4

The identification of the 294
nuclei was verified by separately creating the putative daughter nucleus 290
directly by means of a bombardment of 245
with 48

+ 48
+ 3

and checking that the 290
decay matched the decay chain of the 294
nuclei.[10] The daughter nucleus 290
is very unstable, decaying with a lifetime of 14 milliseconds into 286
, which may experience either spontaneous fission or alpha decay into 282
, which will undergo spontaneous fission.[10]

In a quantum-tunneling model, the alpha decay half-life of 294
was predicted to be 0.66+0.23
[33] with the experimental Q-value published in 2004.[34] Calculation with theoretical Q-values from the macroscopic-microscopic model of Muntian–Hofman–Patyk–Sobiczewski gives somewhat lower but comparable results.[35]


In December 2015, the Joint Working Party of international scientific bodies International Union of Pure and Applied Chemistry (IUPAC) and International Union of Pure and Applied Physics (IUPAP) recognized the element's discovery and assigned the priority of the discovery to the Dubna–Livermore collaboration.[36] This was on account of two 2009 and 2010 confirmations of the properties of the granddaughter of 294Og, 286Fl, at the Lawrence Berkeley National Laboratory, as well as the observation of another consistent decay chain of 294Og by the Dubna group in 2012. The goal of that experiment had been the synthesis of 294Ts via the reaction 249Bk(48Ca,3n), but the short half-life of 249Bk resulted in a significant quantity of the target having decayed to 249Cf, resulting in the synthesis of oganesson instead of tennessine.[37]

From 1 October 2015 to 6 April 2016, the Dubna team performed a similar experiment with 48Ca projectiles aimed at a mixed-isotope californium target containing 249Cf, 250Cf, and 251Cf. Two beam energies at 252 MeV and 258 MeV were used. Only one atom was seen at the lower beam energies, whose decay chain fitted the previously known one of 294Og, and none were seen at the higher beam energy. The experiment was then halted, as the glue from the sector frames covered the target and blocked evaporation residues from escaping to the detectors. The Dubna team plans to repeat this experiment in 2017.[38]


Element 118 was named after Yuri Oganessian, a pioneer in the discovery of synthetic elements, with the name oganesson (Og).

Using Mendeleev's nomenclature for unnamed and undiscovered elements, oganesson is sometimes known as eka-radon (until the 1960s as eka-emanation, emanation being the old name for radon).[9] In 1979, IUPAC assigned the systematic placeholder name ununoctium to the undiscovered element, with the corresponding symbol of Uuo,[39] and recommended it to be used until after confirmed discovery of the element.[40] 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 called it "element 118", with the symbol of E118, (118), or even simply 118.[2]

Before the retraction in 2002, the researchers from Berkeley had intended to name the element ghiorsium (Gh), after Albert Ghiorso (a leading member of the research team).[41]

The Russian discoverers reported their synthesis in 2006. According to IUPAC recommendations, the discoverers of a new element have the right to suggest a name.[42] In 2007, the head of the Russian institute stated the team were considering two names for the new element: flyorium, in honor of Georgy Flyorov, the founder of the research laboratory in Dubna; and moskovium, in recognition of the Moscow Oblast where Dubna is located.[43] He also stated that although the element was discovered as an American collaboration, who provided the californium target, the element should rightly be named in honor of Russia since the Flerov Laboratory of Nuclear Reactions at JINR was the only facility in the world which could achieve this result.[44] These names were later proposed for element 114 (flerovium) and element 116 (moscovium).[45] However, the final name proposed for element 116 was instead livermorium,[46] and the name moscovium was later proposed and accepted for element 115 instead.[14]

Traditionally, the names of all noble gases end in "-on", with the exception of helium, which was not known to be a noble gas when discovered. The IUPAC guidelines valid at the moment of the discovery approval however required all new elements be named with the ending "-ium", even if they turned out to be halogens (traditionally ending in "-ine") or noble gases (traditionally ending in "-on").[47] While the provisional name ununoctium followed this convention, a new IUPAC recommendation published in 2016 recommended using the "-on" ending for new group 18 elements, regardless of whether they turn out to have the chemical properties of a noble gas.[48]

In June 2016 IUPAC announced that the discoverers planned to give the element the name oganesson (symbol: Og), in honour of the Russian nuclear physicist Yuri Oganessian, a pioneer in superheavy element research for sixty years reaching back to the field's foundation: his team and his proposed techniques had led directly to the synthesis of elements 106 to 113 in cold fusion reactions with lead-208 and bismuth-209 targets, as well as elements 112 through 118 through hot fusion reactions with calcium-48 projectiles.[49] The name became official on 28 November 2016.[14] Oganessian later commented on the naming:[50]

For me, it is an honour. The discovery of element 118 was by scientists at the Joint Institute for Nuclear Research in Russia and at the Lawrence Livermore National Laboratory in the US, and it was my colleagues who proposed the name oganesson. My children and grandchildren have been living in the US for decades, but my daughter wrote to me to say that she did not sleep the night she heard because she was crying.[50]

— Yuri Oganessian


Nuclear stability and isotopesEdit

Oganesson (row 118) is slightly above the "island of stability" (white circle) and thus its nuclei are slightly more stable than otherwise predicted.

The stability of nuclei decreases greatly with the increase in atomic number after plutonium, the heaviest primordial element, so that all known isotopes with an atomic number above 101 decay radioactively with a half-life under a day, with the sole exception of dubnium-268. No elements with atomic numbers above 82 (after lead) have stable isotopes.[51] Nevertheless, for reasons not very well understood yet, there is a slightly increased nuclear stability around atomic numbers 110114, which leads to the appearance of what is known in nuclear physics as the "island of stability". This concept, proposed by University of California professor Glenn Seaborg, hypothesizes why superheavy elements last longer than predicted.[52] Oganesson is radioactive and has a half-life that appears to be less than a millisecond. Nonetheless, this is still longer than some predicted values,[33][53] thus giving further support to the idea of this "island of stability".[54]

Calculations using a quantum-tunneling model predict the existence of several neutron-rich isotopes of oganesson with alpha-decay half-lives close to 1 ms.[55][56]

Theoretical calculations done on the synthetic pathways for, and the half-life of, other isotopes have shown that some could be slightly more stable than the synthesized isotope 294Og, most likely 293Og, 295Og, 296Og, 297Og, 298Og, 300Og and 302Og.[33][57] Of these, 297Og might provide the best chances for obtaining longer-lived nuclei,[33][57] and thus might become the focus of future work with this element. Some isotopes with many more neutrons, such as some located around 313Og, could also provide longer-lived nuclei.[58] Since these heavier isotopes greatly facilitate future chemical studies of oganesson, due to their expected longer half-lives, the Dubna team plans to conduct an experiment through the second half of 2017 with a heavier target containing a mix of the isotopes 249Cf, 250Cf, and 251Cf with 48Ca projectiles, aimed at the synthesis of the new isotopes 295Og and 296Og; a repeat of this reaction in 2020 at the JINR is planned to produce 297Og. The production of 293Og and its daughter 289Lv in this reaction is also possible. The isotopes 295Og and 296Og may also be produced in the fusion of 248Cm with 50Ti projectiles, a reaction planned at the JINR and at RIKEN in 2017–2018.[38][59][60]

Calculated atomic and physical propertiesEdit

Oganesson is a member of group 18, the zero-valence elements. The members of this group are usually inert to most common chemical reactions (for example, combustion) because the outer valence shell is completely filled with eight electrons. This produces a stable, minimum energy configuration in which the outer electrons are tightly bound.[61] It is thought that similarly, oganesson has a closed outer valence shell in which its valence electrons are arranged in a 7s27p6 configuration.[1]

Consequently, some expect oganesson to have similar physical and chemical properties to other members of its group, most closely resembling the noble gas above it in the periodic table, radon.[62] Following the periodic trend, oganesson would be expected to be slightly more reactive than radon. However, theoretical calculations have shown that it could be significantly more reactive.[6] In addition to being far more reactive than radon, oganesson may be even more reactive than the elements flerovium and copernicium, which are heavier homologs of the more chemically active elements lead and mercury respectively.[1] The reason for the possible enhancement of the chemical activity of oganesson relative to radon is an energetic destabilization and a radial expansion of the last occupied 7p-subshell.[1][a] More precisely, considerable spin–orbit interactions between the 7p electrons and the inert 7s2 electrons effectively lead to a second valence shell closing at flerovium, and a significant decrease in stabilization of the closed shell of oganesson.[1] It has also been calculated that oganesson, unlike the other noble gases, binds an electron with release of energy—or in other words, it exhibits positive electron affinity,[63][64][b] due to the relativistically stabilized 8s energy level and the destabilized 7p3/2 level.[65]

Oganesson is expected to have by far the broadest polarizability of all elements before it in the periodic table, almost double that of radon.[1] By extrapolating from the other noble gases, it is expected that oganesson has a boiling point between 320 and 380 K.[1] This is very different from the previously estimated values of 263 K[66] or 247 K.[67] Even given the large uncertainties of the calculations, it seems highly unlikely that oganesson would be a gas under standard conditions,[1] and as the liquid range of the other gases is very narrow, between 2 and 9 kelvins, this element should be solid at standard conditions. If oganesson forms a gas under standard conditions nevertheless, it would be one of the densest gaseous substances at standard conditions, even if it is monatomic like the other noble gases.

Because of its tremendous polarizability, oganesson is expected to have an anomalously low ionization energy (similar to that of lead which is 70% of that of radon[5] and significantly smaller than that of flerovium[68]) and a standard state condensed phase.[1]

Predicted compoundsEdit

has a square planar configuration.
is predicted to have a tetrahedral configuration.

No compounds of oganesson have been synthesized yet, but calculations on theoretical compounds have been performed since 1964.[9] It is expected that if the ionization energy of the element is high enough, it will be difficult to oxidize and therefore, the most common oxidation state will be 0 (as for other noble gases);[69] nevertheless, this appears not to be the case.[7]

Calculations on the diatomic molecule Og
showed a bonding interaction roughly equivalent to that calculated for Hg
, and a dissociation energy of 6 kJ/mol, roughly 4 times of that of Rn
.[1] But most strikingly, it was calculated to have a bond length shorter than in Rn
by 0.16 Å, which would be indicative of a significant bonding interaction.[1] On the other hand, the compound OgH+ exhibits a dissociation energy (in other words proton affinity of oganesson) that is smaller than that of RnH+.[1]

The bonding between oganesson and hydrogen in OgH is predicted to be very weak and can be regarded as a pure van der Waals interaction rather than a true chemical bond.[5] On the other hand, with highly electronegative elements, oganesson seems to form more stable compounds than for example copernicium or flerovium.[5] The stable oxidation states +2 and +4 have been predicted to exist in the fluorides OgF
and OgF
.[70] The +6 state would be less stable due to the strong binding of the 7p1/2 subshell.[7] This is a result of the same spin-orbit interactions that make oganesson unusually reactive. For example, it was shown that the reaction of oganesson with F
to form the compound OgF
would release an energy of 106 kcal/mol of which about 46 kcal/mol come from these interactions.[5] For comparison, the spin-orbit interaction for the similar molecule RnF
is about 10 kcal/mol out of a formation energy of 49 kcal/mol.[5] The same interaction stabilizes the tetrahedral Td configuration for OgF
, as distinct from the square planar D4h one of XeF
, which RnF
is also expected to have.[70] The Og–F bond will most probably be ionic rather than covalent, rendering the oganesson fluorides non-volatile.[6][71] OgF2 is predicted to be partially ionic due to oganesson's high electropositivity.[72] Unlike the other noble gases (except possibly xenon and radon),[73][74] oganesson is predicted to be sufficiently electropositive[72] to form an Og–Cl bond with chlorine.[6]

See alsoEdit


  1. ^ The actual quote is "The reason for the apparent enhancement of chemical activity of element 118 relative to radon is the energetic destabilization and radial expansion of its occupied 7p3/2 spinor shell."
  2. ^ Nevertheless, quantum electrodynamic corrections have been shown to be quite significant in reducing this affinity by decreasing the binding in the anion Og by 9%, thus confirming the importance of these corrections in superheavy elements. See Pyykkö.


  1. ^ a b c d e f g h i j k l m n o p Nash, Clinton S. (2005). "Atomic and Molecular Properties of Elements 112, 114, and 118". Journal of Physical Chemistry A. 109 (15): 3493–3500. Bibcode:2005JPCA..109.3493N. PMID 16833687. doi:10.1021/jp050736o. 
  2. ^ a b c d e 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. 
  3. ^ Bonchev, Danail; Kamenska, Verginia (1981). "Predicting the Properties of the 113–120 Transactinide Elements". Journal of Physical Chemistry. American Chemical Society. 85 (9): 1177–1186. doi:10.1021/j150609a021. 
  4. ^ a b c Eichler, R.; Eichler, B., Thermochemical Properties of the Elements Rn, 112, 114, and 118 (PDF), Paul Scherrer Institut, retrieved 2010-10-23 
  5. ^ a b c d e f Han, Young-Kyu; Bae, Cheolbeom; Son, Sang-Kil; Lee, Yoon Sup (2000). "Spin–orbit effects on the transactinide p-block element monohydrides MH (M=element 113–118)". Journal of Chemical Physics. 112 (6): 2684. Bibcode:2000JChPh.112.2684H. doi:10.1063/1.480842. 
  6. ^ a b c d e Kaldor, Uzi; Wilson, Stephen (2003). Theoretical Chemistry and Physics of Heavy and Superheavy Elements. Springer. p. 105. ISBN 140201371X. Retrieved 2008-01-18. 
  7. ^ a b c d 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. 
  8. ^ Chemical Data. Ununoctium - Uuo, Royal Chemical Society
  9. ^ a b c Grosse, A. V. (1965). "Some physical and chemical properties of element 118 (Eka-Em) and element 86 (Em)". Journal of Inorganic and Nuclear Chemistry. Elsevier Science Ltd. 27 (3): 509–19. doi:10.1016/0022-1902(65)80255-X. 
  10. ^ a b c d e f Oganessian, Yu. Ts.; Utyonkov, V. K.; Lobanov, Yu. V.; Abdullin, F. Sh.; Polyakov, A. N.; Sagaidak, R. N.; Shirokovsky, I. V.; Tsyganov, Yu. S.; et al. (2006-10-09). "Synthesis of the isotopes of elements 118 and 116 in the 249Cf and 245Cm+48Ca fusion reactions". Physical Review C. 74 (4): 044602. Bibcode:2006PhRvC..74d4602O. doi:10.1103/PhysRevC.74.044602. Retrieved 2008-01-18. 
  11. ^ Oganessian, Yuri Ts.; Rykaczewski, Krzysztof P. (August 2015). "A beachhead on the island of stability". Physics Today. 68 (8): 32–38. Bibcode:2015PhT....68h..32O. doi:10.1063/PT.3.2880. Retrieved 2017-06-14. 
  12. ^ Staff (30 November 2016). "IUPAC Announces the Names of the Elements 113, 115, 117, and 118". IUPAC. Retrieved 1 December 2016. 
  13. ^ St. Fleur, Nicholas (1 December 2016). "Four New Names Officially Added to the Periodic Table of Elements". New York Times. Retrieved 1 December 2016. 
  14. ^ a b c "IUPAC Is Naming The Four New Elements Nihonium, Moscovium, Tennessine, And Oganesson". IUPAC. 2016-06-08. Retrieved 2016-06-08. 
  15. ^ "The Top 6 Physics Stories of 2006". Discover Magazine. 7 January 2007. Retrieved 18 January 2008. 
  16. ^ Leach, Mark R. "The INTERNET Database of Periodic Tables". Retrieved 8 July 2016. 
  17. ^ a b Smolanczuk, R. (1999). "Production mechanism of superheavy nuclei in cold fusion reactions". Physical Review C. 59 (5): 2634–2639. Bibcode:1999PhRvC..59.2634S. doi:10.1103/PhysRevC.59.2634. 
  18. ^ Ninov, Viktor (1999). "Observation of Superheavy Nuclei Produced in the Reaction of 86
    with 208
    ". Physical Review Letters. 83 (6): 1104–1107. Bibcode:1999PhRvL..83.1104N. doi:10.1103/PhysRevLett.83.1104.
  19. ^ Service, R. F. (1999). "Berkeley Crew Bags Element 118". Science. 284 (5421): 1751. doi:10.1126/science.284.5421.1751. 
  20. ^ Public Affairs Department (21 July 2001). "Results of element 118 experiment retracted". Berkeley Lab. Retrieved 18 January 2008. 
  21. ^ Dalton, R. (2002). "Misconduct: The stars who fell to Earth". Nature. 420 (6917): 728–729. Bibcode:2002Natur.420..728D. PMID 12490902. doi:10.1038/420728a. 
  22. ^ Element 118 disappears two years after it was discovered. Retrieved on 2 April 2012.
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    (PDF). JINR Communication. JINR, Dubna.
  24. ^ Oganessian, Yu. T.; et al. (2002). "Element 118: results from the first 249
    + 48
    . Communication of the Joint Institute for Nuclear Research. Archived from the original on 22 July 2011.
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  26. ^ Oganessian, Yu. T. (2006). "Synthesis and decay properties of superheavy elements". Pure Appl. Chem. 78 (5): 889–904. doi:10.1351/pac200678050889. 
  27. ^ Sanderson, K. (2006). "Heaviest element made – again". Nature News. Nature. doi:10.1038/news061016-4. 
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Further readingEdit

  • Scerri, Eric (2007). The Periodic Table, Its Story and Its Significance. New York: Oxford University Press. ISBN 978-0-19-530573-9. 

External linksEdit