|Name in Saurian|| Uhhxodaim (Ux)|
|Systematic name|| Untriquadium (Utq)|
|Location on the periodic table|
|Previous element||Paulium (133Ah)|
|Next element||Meyerium (135My)|
|Atomic mass||369.0588 u, 612.8365 yg|
|Atomic radius||159 pm, 1.59 Å|
|Van der Waals radius||184 pm, 1.84 Å|
|Nucleons||366 (134 p+, 232 n0)|
|Nuclear radius||8.55 fm|
|Electron configuration|| [Mc] 5g8 6f4 8s2 8p2|
2, 8, 18, 32, 40, 22, 8, 4
|Oxidation states|| +2, +4, +6|
(mildly basic oxide)
|First ionization energy||616.3 kJ/mol, 6.388 eV|
|Electron affinity||102.3 kJ/mol, 1.060 eV|
|Covalent radius||177 pm, 1.77 Å|
|Molar mass||369.059 g/mol|
|Molar volume||76.809 cm3/mol|
|Atomic number density|| 1.63 × 1021 g−1|
7.84 × 1021 cm−3
|Average atomic separation||503 pm, 5.03 Å|
|Speed of sound||2254 m/s|
|Crystal structure||Body centered cubic|
|Melting point|| 976.90 K, 1758.42°R|
|Boiling point|| 1600.52 K, 2880.94°R|
|Liquid range||623.62 K, 1122.52°R|
|Triple point|| 976.90 K, 1758.42°R|
@ 2.4676 Pa, 0.018509 torr
|Critical point|| 4103.30 K, 7385.94°R|
@ 156.8595 MPa, 1548.088 atm
|Heat of fusion||10.016 kJ/mol|
|Heat of vaporization||154.436 kJ/mol|
|Heat capacity|| 0.05949 J/(g•K), 0.10709 J/(g•°R)|
21.956 J/(mol•K), 39.521 J/(mol•°R)
|Universe (by mass)|| Relative: 4.33 × 10−28|
Absolute: 1.45 × 1025 kg
Arrhenium is the fabricated name of a theoretical element with the symbol Ah and atomic number 134. Arrhenium was named in honor of Svante Arrhenius (1859–1927), who founded physical chemistry, including Arrhenius equation and acid-base theory. This element is known in the scientific literature as untriquadium (Utq), or simply element 134. Arrhenium is the fourteenth element of the lavoiside series and located in the periodic table coordinate 5g14.
Like most metals, arrhenium is a shiny, silvery metal, but brittle, meaning the force can crumble it. It has a density of 4.8 g/cm3 and its speed of sound is 2254 m/s. The average separation between atoms is 5.03 Å and forms body centered cubic crystal structure.
Its liquification point is 1758°R, close to the minimum temperature of a charcoal fire. Arrhenium remains a liquid up to its vaporization point of 2881°R. The ratio between these two temperature values yields a liquid ratio of 1.64 and difference between it yields a liquid range of 1123°R.
Arrhenium contains 366 nucleons (134 protons, 232 neutrons, 1.73 neutrons per proton) that make up the nucleus and 134 electrons in 23 orbitals in 8 energy levels. Due to relativistic effectss, the 5g orbital that this element is filling is missing six electrons, instead of 14 electrons in the 5g orbital, there are just 8. Four of six missing 5g electrons are found in the next occupying orbital, 4f, while two make up the complete 8p1/2 split orbital.
Arrhenium atom weighs 369 daltons, three times heavier than iodine and two times heavier than tungsten. The atom sizes 1.29 Å from nucleus to outermost shell, but the real size based on atomic forces is 1.84 Å, roughly 10⁄7 of that between nucleus and outermost shell.
Like every other element heavier than lead, arrhenium has no stable isotopes. The most stable isotope is 366Ah with a half-life of 256 days, beta decaying to 366Pl. 368Ah has a half-life of 5.3 weeks. All of the remaining isotopes have half-lives less than 5 hours while majority of these have half-lives less than 45 seconds.
As with about 9 out of 10 elements on the periodic table, arrhenium isotopes can form excited state if energy is absorbed. Excited states are metastable because their lifetimes are often extremely short but still last at least a nanosecond. The longest-lived excited state is 371mAh with a very long half-life of 32 days; the second longest has a half-life of just 3 minutes for 369mAh.
Arrhenium, like other g-block elements, is reactive, meaning it tarnishes in the air quickly, reacts readily with water to form a base, and gets eaten by acids to form a solution. In the pure oxygen atmosphere under little pressure, it burns with a blue flame. Arrhenium reacts more violently with halogens to form ionic salts. Arrhenium(VI) dominates chemistry over arrhenium(II) and arrhenium(IV). However in aqueous solutions, arrhenium(VI) is rare.
When exposed to air, it forms AhO3 as well as AhN2 and Ah(CO3)3, all are black powder. Arrhenium hexafluoride (AhF6) can be synthesized when uranium hexafluoride give up all six fluorine atoms to arrhenium, since this element has higher electron affinity than uranium. Arrhenium trisulfide (AhS3) can be made when arrhenium reacts with powdered sulfur. During this same action, disulfide and monosulfide can also be produced albeit in smaller proportions than trisulfide. Trisulfide is a brown powder, disulfide is a pink powder, and monosulfide is a pale purple powder.
There are examples of soluble salts of arrhenium: Ah(CO3)2 (red), AhSO4 (blue), Ah(NO3)2 (yellow), and AhSiO4 (green). It can also form organic compounds of arrhenium, called organoarrhenium compounds, such as arrhenium sugars like C12H20O11Ah.
Occurrence and synthesis Edit
It is certain that arrhenium is virtually nonexistent on Earth, and is extremely rare in the universe. Since every element heavier than lithium were produced by stars, then arrhenium 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 hyperheavy element. Instead, this element can only practically be made by advanced technological civilizations. An estimated abundance of arrhenium in the universe by mass is 4.33 × 10−28, which amounts to 1.45 × 1025 kilograms or about one quarter Earth masses worth of arrhenium.
To go along with other such civilizations, humans on Earth may eventually have the capability to synthesize arrhenium. To synthesize most stable isotopes of arrhenium, 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 a vast amount of energy. Here's couple of example equations in the production of the most stable isotope, 366Ah.