|Name in Saurian|| Fuicaim (Fc)|
|Systematic name|| Untritrium (Utt)|
|Location on the periodic table|
|Previous element||Thomsonium (132To)|
|Next element||Arrhenium (134Ah)|
|Atomic mass||364.0163 u, 604.4633 yg|
|Atomic radius||162 pm, 1.62 Å|
|Van der Waals radius||192 pm, 1.92 Å|
|Nucleons||361 (133 p+, 228 n0)|
|Nuclear radius||8.51 fm|
|Electron configuration|| [Mc] 5g8 6f3 8s2 8p2|
2, 8, 18, 32, 40, 21, 8, 4
|Oxidation states|| +2, +3, +4, +5, +6|
(mildly basic oxide)
|First ionization energy||624.3 kJ/mol, 6.470 eV|
|Electron affinity||48.9 kJ/mol, 0.507 eV|
|Covalent radius||186 pm, 1.86 Å|
|Molar mass||364.016 g/mol|
|Molar volume||82.746 cm3/mol|
|Atomic number density||7.28 × 1021 cm−3|
|Average atomic separation||516 pm, 5.16 Å|
|Speed of sound||1956 m/s|
|Crystal structure||Body centered cubic|
|Melting point|| 832.56 K, 559.41°C|
|Boiling point|| 3099.89 K, 2826.74°C|
|Liquid range||2267.33 K/°C, 4081.20°F/°R|
|Triple point|| 832.56 K, 559.41°C|
@ 195.63 pPa, 1.4673 × 10−12 torr
|Critical point|| 6498.58 K, 6225.43°C|
@ 114.6951 MPa, 1131.956 atm
|Heat of fusion||8.674 kJ/mol|
|Heat of vaporization||312.929 kJ/mol|
|Heat capacity|| 0.06083 J/g/K, 0.10949 J/g/°R|
22.142 J/mol/K, 39.856 J/mol/°R
|Universe (by mass)|| Relative: 1.98 × 10−29|
Absolute: 6.62 × 1023 kg
Paulium is the fabricated name of a theoretical element with the symbol Pl and atomic number 133. Paulium was named in honor of Linus Pauling (1901–1994), who studied the nature of chemical bonds and the structures of molecules; also honoring Wolfgang Pauli (1900–1958), who proposed the spin theory with his exclusion principle. This element is known in scientific literature as untritrium (Utt), or simply element 133. Paulium is the thirteenth element of the lavoiside series and located in periodic table coordinate 5g13.
Unlike most metals, which are grayish white, paulium is a navy blue metal, due to outermost electrons oscillating only at blue region of the spectrum at low intensity instead of oscillating at ultraviolet wavelength as is the case for most metals. It has a density of 4.4 g/cm3, about 4⁄5 the mean density of Earth's. Like most metals, paulium is ductile and malleable, and lustrous. Paulium has a cubic crystal structure.
Its melting point is 833 K (1039°F), meaning it is solid on every planet in our solar system from the coldest planet (Neptune) to the hottest planet (Venus). Its liquid range is relatively wide as its boiling point is 3100 K (2827°C).
Paulium contains 133 protons and 228 neutrons that make up the nucleus, as well as 133 electrons surrounding the nucleus. Its mass number is 361, corresponding to the number of nucleons. But the real atomic mass is about 364 daltons to include electrons and both nucleons having masses slightly over one dalton.
It is assumed that there are 13 electrons in the 5g orbital since it is the thirteenth element of the g-block series, but due to smearing effects, there are only eight.
Like every other elements heavier than lead, paulium has no stable isotopes. The most stable isotope is 361Pl with a half-life of 12.5 hours. It undergoes spontaneous fission, splitting into two lighter nuclei plus neutrons like the following example.
All of the remaining isotopes have half-lives less than 40 minutes while majority of these have half-lives less than 3 seconds. Paulium has isomers, which are excited states of isotopes. The longest-lived isomer is 358m1Pl with a half-life of 88.1 hours, seven times longer than the most stable ground state isotope. The second longest-lived, 363m2Pl, has a half-life of just 19.8 seconds.
Paulium loses blue color and luster when exposed to air due to the formation of oxide PlO2, but in the powder form, it burns with brilliant orange flame when a spark or even a shock is applied to form the highest oxide PlO3. Due to its basic nature of metal, it forms a base when dissolved in water and neutralizes acids to form paulium salts.
PlO3 is a gray amorphous solid obtained when metal exposes to the air or burned in the presence of oxygen. Paulium reacting with halogens would most likely form pentahalides, such as PlCl5, which is a white crystalline solid. They compounds can be oxidized in water to form oxyhalides, such as PlOCl3 when PlCl5 is oxidized.
- PlCl5 + H2O → PlOCl3 + 2 HCl
Paulium(III) carbonate (Pl2(CO3)3) is a white chalky solid like limestone (CaCO3). Paulium(III) sulfide (Pl2S3) is a reddish purple crystalline solid, paulium(IV) sulfide (PlS2) is a pale green powder, and paulium(V) sulfide (Pl2S5) is a reddish purple crystalline solid. Paulium can form selenide with +2 oxidation state, PlSe, which is bright yellow amorphous solid. Paulium nitrides are PlN, Pl3N5, and PlN2.
4) are found in compounds such as yttrium paulate (Y2(PlO4)3) and zinc paulate (Zn2(PlO4)3).
Organopaulium are organometallic compounds of paulium. The three examples are paulium acetylide (Pl2C2), paulium pentacarbonyl (Pl(CO)5), and paulium methanide (Pl(CH2)2).
Occurrence and synthesis Edit
It is certain that paulium is virtually nonexistent on Earth, and is extremely rare in the universe. Since every element heavier than lithium were produced by stars, then paulium must be produced in stars, and then thrown out into space by exploding stars. But it is virtually 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 can only practically be made by advanced technological civilizations. An estimated abundance of paulium in the universe by mass is 1.98 × 10−29, which amounts to 6.62 × 1023 kilograms or about the mass of Mars worth of paulium.
To go along with other such civilizations, humans on Earth may eventually have the capability to synthesize paulium. To synthesize most stable isotopes of paulium, 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 361Pl.