|Name in Saurian|| Rikcohelaim (Ri)|
|Systematic name|| Unquadbium (Uqb)|
|Location on the periodic table|
|Above element||Thorium (90Th)|
|Previous element||Dumasium (141Du)|
|Next element||Abeggium (143Ab)|
|Atomic mass||388.2167 u, 644.6490 yg|
|Atomic radius||140 pm, 1.40 Å|
|Van der Waals radius||171 pm, 1.71 Å|
|Nucleons||385 (142 p+, 243 n0)|
|Nuclear radius||8.69 fm|
|Electron configuration|| [Mc] 5g16 6f2 7d2 8s2 8p2|
2, 8, 18, 32, 48, 20, 10, 4
|Oxidation states|| +1, +2, +3, +4|
(mildly basic oxide)
|First ionization energy||707.2 kJ/mol, 7.329 eV|
|Electron affinity||52.9 kJ/mol, 0.548 eV|
|Covalent radius||163 pm, 1.63 Å|
|Molar mass||388.217 g/mol|
|Molar volume||67.201 cm3/mol|
|Atomic number density||8.96 × 1021 cm−3|
|Average atomic separation||481 pm, 4.81 Å|
|Speed of sound||2427 m/s|
|Crystal structure||Face centered cubic|
|Melting point|| 1088.22 K, 815.07°C|
|Boiling point|| 2244.17 K, 1971.02°C|
|Liquid range||1155.96 K/°C, 2080.72°F/°R|
|Triple point|| 1088.20 K, 815.05°C|
@ 175.38 mPa, 1.3155 × 10−5 torr
|Critical point|| 4253.62 K, 3980.47°C|
@ 32.1621 MPa, 317.417 atm
|Heat of fusion||10.736 kJ/mol|
|Heat of vaporization||220.323 kJ/mol|
|Heat capacity|| 0.05656 J/g/K, 0.10181 J/g/°R|
21.959 J/mol/K, 39.526 J/mol/°R
|Universe (by mass)|| Relative: 4.65 × 10−31|
Absolute: 1.56 × 1022 kg
Butlerovium is the fabricated name of a hypothetical element with the symbol Bu and atomic number 142. Butlerovium was named in honor of Aleksandr Butlerov (1828–1886), who developed the theory of chemical structure. He also incorporated double bonds into structure formulae. This element is known in scientific literature as unquadbium (Uqb), eka-thorium, or simply element 142. Butlerovium is the second member of the dumaside series, found in the third row of f-block (below cerium and thorium); this element is located in periodic table coordinate 6f2.
Butlerovium is a brownish gray brittle solid metal at room temperature (77°F) that shows brown luster. The molar mass (same as atomic mass in value) is 388.22 g/mol, while its molar volume is 67.20 cm3/mol. Dividing molar mass by molar volume yields a density of 5.7 g/cm3, slightly denser than the densest planet in our solar system –– Earth. The average separation between butlerovium atoms is 481 pm (4.81 Å) and there are nine sextillion atoms in one cubic centimeter of metal.
Its liquid state ranges from 1499°F (1088 K) to 3580°F (2244 K). The amounts of energy absorbed causing phase transitions is related to its phase points. Its heat of fusion is 10.7 kJ/mol while its heat of vaporization is 220.3 kJ/mol, meaning that it requires 22 times more energy for boiling to convert from liquid to gas than converting from solid to liquid. It releases exactly the same amount of energy upon reversing phase transitions.
Butlerovium has 142 protons, 255 neutrons, and 142 electrons in atoms, with protons and neutrons making up the nucleus at its center while electrons revolve around the nucleus. Butlerovium has two electrons occupying in the f-orbital, consistent with being the second element of the dumaside series in f-block. However, the g-orbital is not completed as it needs two more to complete the orbital. Due to spin-orbit coupling due to relativistic effect, there are two electrons in the d-orbital and two in the outermost p-orbital. The electron configuration according to Dirac-Fock calculation is [Mc] 5g16 6f2 7d2 8s2 8p2 and the electron notation is 142-8-24.
Like every other elements heavier than lead, butlerovium has no stable isotopes. The most stable isotope is 385Bu with a half-life of 23.75 hours, just 15 minutes shy of a day. It cluster decays to 337Mw by emitting two oxygen-16 nuclei plus 32 neutrons. Two other isotopes have half-lives of at least an hour: 387Bu (4.24 hours) and 382Bu (2.49 hours). Like most other elements, butlerovium has metastable isomers, the most stable is 387m1Bu (t½ = 4.57 min).
Despite butlerovium is right below thorium, it doesn't have very similar chemical properties due to electrons in the g- and p-orbitals. Butlerovium's electronegativity is 40 points higher than thorium's, 1.68 vs. 1.28. Butlerovium has oxidation states ranging from +1 to +4, all are common states except for +3.
There are oxides of butlerovium: Bu2O, BuO or BuO2, formed when metal exposes to the air rich in oxygen. Butlerovium can react readily with halogens and acids. The examples of halides are Bu2Cl, BuF2, BuBr, and BuI. Butlerovium can form aqueous solutions such as sulfate (BuSO4) and nitrate (BuNO3). Other compounds include BuS, BuP, and BuN.
Occurrence and synthesis Edit
It is almost certain that butlerovium doesn't exist on Earth at all, but it is believed to exist somewhere in the universe, at least in very tiny amounts. Since every element heavier than lithium were produced by stars, then butlerovium must be produced in stars, and then thrown out into space by exploding stars. But it is theoretically impossible for even the most powerful supernovae or most violent neutron star collisions to produce this element through r-process because there's not enough energy available or not enough neutrons, respectively, to produce this heavy element. Instead, this element virtually can only be made by advanced technological civilizations. An estimated abundance of butlerovium in the universe by mass is 4.65 × 10−31, which amounts to 1.56 × 1022 kilograms or about 5⁄4 Pluto masses worth of butlerovium.
To go along with other such civilizations, humans on Earth may eventually have the capability to synthesize butlerovium. To synthesize most stable isotopes of butlerovium, nuclei of a couple lighter elements must be fused together, and right amount of neutrons must be seeded. This operation would be extremely difficult since it requires vast amounts of energy. Here's couple of example equations in the production of the most stable isotope 385Bu.