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Schrodium is the provisional non-systematic name of a theoretical element with the symbol So and atomic number 150. Schrodium was named in honor of Erwin Schrödinger (1887–1961), who developed his equation for quantum mechanics. This hypothetical element with atomic number 150 is known in the scientific literature as unpentnilium (Upn), eka-curium, or simply element 150. Schrodium is the eighth member of the dumaside series so it is found in the third row of the f-block (below gadolinium and curium); this hypothetical element is located in the periodic table coordinate 6f8.
Atomic properties[]
A schrodium atom is comprised of 569 subatomic particles, 419 of these make up the nucleus (protons and neutrons), while the remaining 150 are found surrounding the nucleus (electrons). Its atomic mass is 422.5 daltons, twice as heavy as an astatine atom; its radius is 129 picometers, similar in size to a copper atom.
The electron configuration is inconsistent with what the periodic table would tell, the f-orbital contains just seven electrons while one missing electron is in the d-orbital.
Isotopes[]
Like every other element heavier than lead, schrodium has no stable isotopes. The longest-lived isotope is 419So with a fission half-life of 5.7 milliseconds.
Schrodium has meta states, which are excited states of isotopes. The longest lived meta state has a half-life of 380 milliseconds for 420m1So, 66.6 times longer than the longest-lived ground-state isotope 419So.
Chemical properties and compounds[]
Schrodium is a lot less reactive than curium because electrons between 8s and 8p1/2 orbitals are bound, resulting in higher ionization energies, thus making it harder to form compounds. The common oxidation states for schrodium are +5 (pentavalent) and +6 (hexalent), compared to +3 (trivalent) for curium. In aqueous solutions, So6+ (dark blue) is more stable than So5+ (green).
Schrodium compounds are rare since it is so unreactive. Still, schrodium can form halides since halogens are the most reactive group of elements that can combine with metals. Examples of halides are schrodium heptafluoride (SoF7), schrodium hexafluoride (SoF6), hexachloride (SoCl6), and pentachloride (SoCl5). Schrodium can form other compounds, such as So2O7, SoO3, So2CO3, and So3PO4.
Schrodium can react with carbon, along with hydrogen, oxygen, and/or others to form organic compounds involving schrodium, called organoschrodium. One example is dimethylschrodium (So(CH3)2), a colorless liquid with a freezing point of 473°R (−10 °C) and boiling point of 826°R (186 °C).
Physical properties[]
Schrodium, even as a metal, is not gray, white, gold, reddish, nor bluish, but green. The metal appears green because electrons exchange energies at frequencies that would be at the green region of the electromagnetic spectrum at around 525 nanometers.
Its density is 9.56 g/cm3, which is about average for a metal. One mole of schrodium weighs 422.5 grams or about 15 ounces. The sound travels through a thin rod of this metal at 4582 m/s, a little above average for an element. Schrodium has a hexagonal crystal lattice, formed when atoms arrange together to form unique shapes. One cubic centimeter of schrodium contains 13.6 sextillion atoms, and separated by an average of 419 pm (4.19 Å) apart.
Schrodium's phase points are much lower than neighboring elements due to closed orbitals and split orbitals including 6f5/2 split orbital. It melts at 835°R (191 °C) and boils at 1652°R (645 °C). However, its melting and boiling points are not the same at every condition as pressure is the variable. The melting and boiling points given here are from Earth's standard atmospheric pressure at sea level, 101.325 kPa or 1 atm, which is the default pressure when determining phase points of elements, compounds, and mixtures. If we put schrodium in a low pressure environment, both phase points would be lower, but the boiling point would decrease far more rapidly with the same amount of decrease in pressure. Because of this, the boiling point would catch up to the melting point, and when both phase points are identical in temperature, it is called the triple point. For schrodium, the triple point is at a pressure of 2.24 kPa, 1⁄45 the Earth's sea level pressure. In conclusion, if we decrease pressure applied on schrodium 45 times, from default pressure to triple point pressure, boiling point would lower by 816.58°R (453.87 °C), but its melting point would lower by only 0.39°R (0.22 °C). If we increase the ambient pressure around schrodium from the default atmospheric pressure by 62260 times, it would exist as a supercritical fluid beyond its boiling point. At 62260 atmospheres (6309 megapascals), its boiling point would be 8810°R (4621 °C), while its melting point would be 838°R (192 °C). Its liquid range would be 7972°R (4429 °C) and its liquid ratio would be 10.51, compared to 817°R (454 °C) and 1.98, respectively at default pressure.
Occurrence[]
It is almost certain that schrodium doesn't exist on Earth at all, but it is believed to barely exist somewhere in the universe due to its brief lifetime. Every element heavier than iron can only naturally be produced by exploding stars. But it is likely impossible for even the most powerful supernovae or most violent neutron star collisions to produce this hypothetical element through r-process because there's not enough energy available or not enough neutrons, respectively, to produce this superheavy element. Instead, this hypothetical element can only be produced by advanced technological civilizations, virtually accounting for all of its abundance in the universe. An estimated abundance of schrodium in the universe by mass is 9.10 × 10−33, which amounts to 3.05 × 1020 kilograms or about a third the mass of dwarf planet Ceres worth of schrodium.
Synthesis[]
To synthesize most stable isotopes of schrodium, nuclei of a couple lighter elements must be fused together, and the right amount of neutrons must be seeded. This operation would be impossible using current technology since it requires a tremendous amount of energy, thus its cross section would be so low that it is beyond the technological limit. Even if synthesis succeeds, this resulting element would quickly undergo fission. Here's a couple of example equations in the synthesis of the most stable isotope, 419So.
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