|Name, symbol||ununennium, Uue|
|Alternative names||element 119, eka-francium|
|Ununennium in the periodic table|
|Standard atomic weight (Ar)|| (predicted)|
|Element category||unknown, but probably an alkali metal|
|Group, block||group 1 (alkali metals), s-block|
|Electron configuration||[Uuo] 8s1 (predicted)|
|2, 8, 18, 32, 32, 18, 8, 1 (predicted)|
|Phase||unknown (could be solid or liquid)|
|Melting point||273–303 K (0–30 °C, 32–86 °F) (predicted)|
|Boiling point||903 K (630 °C, 1166 °F) (predicted)|
|Density near r.t.||3 g/cm3 (predicted)|
|Heat of fusion||2.01–2.05 kJ/mol (extrapolated)|
|Oxidation states||1, 3 (predicted)|
|Ionization energies||1st: 463.1 kJ/mol
2nd: 1698.1 kJ/mol (predicted)
|Atomic radius||empirical: 240 pm (predicted)|
|Covalent radius||263–281 pm (extrapolated)|
|CAS Registry Number||54846-86-5|
|Naming||IUPAC systematic element name|
|Most stable isotopes|
Ununennium, also known as eka-francium or simply element 119, is the hypothetical chemical element with atomic number 119 and symbol Uue. Ununennium and Uue are the temporary systematic IUPAC name and symbol, until a permanent name is decided upon. In the periodic table of the elements, it is expected to be an s-block element, an alkali metal, and the first element in the eighth period.
Ununennium is the element with the lowest atomic number that has not yet been synthesized. To date, all attempts to synthesize this element have been unsuccessful. Its position as the seventh alkali metal suggests that it would have similar properties to the alkali metals, lithium, sodium, potassium, rubidium, caesium, and francium; however, relativistic effects may cause some of its properties to differ from those expected from a straight application of periodic trends. For example, ununennium is expected to be less reactive than caesium and francium and be closer in behavior to potassium or rubidium, and while it should show the characteristic +1 oxidation state of the alkali metals, it is also predicted to show the +3 oxidation state unknown in any other alkali metal.
Ununennium and unbinilium are the lightest elements that have not yet been synthesized, and attempts to synthesize them would push the limits of current technology, due to the decreasing cross sections of the production reactions and their probably short half-lives. Previously, important help (characterized as "silver bullets") in the synthesis of superheavy elements came from the deformed nuclear shells around hassium-270 which increased the stability of surrounding nuclei, and the existence of the neutron-rich isotope calcium-48 which could thus be used as a projectile to produce more neutron-rich isotopes of superheavy elements. However, using calcium-48 to synthesize ununennium would require a target of einsteinium-253 or -254, which while not impossible to produce is very difficult. To more practically produce further superheavy elements, projectiles heavier than 48Ca are needed.
No atoms were identified, leading to a limiting yield of 300 nb. Later calculations suggest that the yield of the 3n reaction (which would result in 299Uue and three neutrons as products) would be 0.5 pb.
As of May 2012, plans were under way to attempt to synthesize the isotopes 295Uue and 296Uue by bombarding a target of berkelium with titanium at the GSI Helmholtz Centre for Heavy Ion Research in Darmstadt, Germany:
No atoms were identified, leading to a yielding limit of 70 fb.
The alpha-decay half-lives of 1700 nuclei with 100 ≤ Z ≤ 130 have been calculated in a quantum tunneling model with alpha-decay Q-values from different mass estimates. The alpha-decay half-lives predicted for 291–307Uue are of the order of micro-seconds. The highest value of the alpha-decay half-life predicted in the quantum tunneling model with the mass estimates from a macroscopic-microscopic model is ~485 microseconds for the isotope 294Uue. For 302Uue it is ~163 microseconds.
Being the first period 8 element, ununennium is predicted to be the next alkali metal after francium and behave much like their lighter congeners; however, it is also predicted to differ from the lighter alkali metals in some properties. Its chemistry is predicted to be closer to that of potassium or rubidium instead of caesium or francium. This is unusual as periodic trends, ignoring relativistic effects would predict ununennium to be even more reactive than caesium and francium. This lowered reactivity is due to the relativistic stabilisation of ununennium's valence electron, increasing ununennium's first ionisation energy and decreasing the metallic and ionic radii; this effect is already seen for francium. The relativistic stabilisation of the 8s orbital also increases ununennium's electron affinity far beyond that of caesium and francium; indeed, ununennium is expected to have an electron affinity higher than all the alkali metals lighter than it. Relativistic effects also cause a very large drop in the polarisability of ununennium. On the other hand, ununennium is predicted to continue the trend of melting points decreasing going down the group, being expected to have a melting point between 0 °C and 30 °C.
The stabilisation of ununennium's valence electron and thus the contraction of the 8s orbital cause its atomic radius to be lowered to 240 pm, very close to that of rubidium (247 pm), so that the chemistry of ununennium in the +1 oxidation state should be more similar to the chemistry of rubidium than to that of francium. On the other hand, the ionic radius of the Uue+ ion is predicted to be larger than that of Rb+, because the 7p orbitals are destabilised and are thus larger than the p-orbitals of the lower shells. Ununennium may also show the +3 oxidation state, which is not seen in any other alkali metal, in addition to the +1 oxidation state that is characteristic of the other alkali metals and is also the main oxidation state of all the known alkali metals: this is because of the destabilisation and expansion of the 7p3/2 spinor, causing its outermost electrons to have a lower ionisation energy than what would otherwise be expected. Indeed, many ununennium compounds are expected to have a large covalent character, due to the involvement of the 7p3/2 electrons in the bonding: this effect is also seen to a lesser extent in francium.
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|Extended periodic table (Large version)|