|Name in Saurian|| Fcudsbaim (Fb)|
|Systematic name|| Unbiseptium (Ubs)|
|Location on the periodic table|
|Previous element||Maxwellium (126Mw)|
|Next element||Boylium (128By)|
|Atomic mass||343.8481 u, 570.9731 yg|
|Atomic radius||181 pm, 1.81 Å|
|Van der Waals radius||201 pm, 2.01 Å|
|Nucleons||341 (127 p+, 214 n0)|
|Nuclear radius||8.35 fm|
|Electron configuration|| [Mc] 5g3 6f2 8s2 8p2|
2, 8, 18, 32, 35, 20, 8, 4
|Oxidation states|| +5, +7, +8, +9|
(strongly basic oxide)
|First ionization energy||483.6 kJ/mol, 5.012 eV|
|Electron affinity||17.2 kJ/mol, 0.179 eV|
|Covalent radius||175 pm, 1.75 Å|
|Molar mass||343.848 g/mol|
|Molar volume||28.688 cm3/mol|
|Atomic number density||2.10 × 1022 cm−3|
|Average atomic separation||363 pm, 3.63 Å|
|Speed of sound||786 m/s|
|Crystal structure||Centered tetragonal|
|Melting point|| 601.25 K, 328.10°C|
|Boiling point|| 1647.50 K, 1374.35°C|
|Liquid range||1046.25 K/°C, 1883.24°F/°R|
|Triple point|| 601.24 K, 328.09°C|
@ 49.751 μPa, 3.7317 × 10−7 torr
|Critical point|| 3866.42 K, 3593.27°C|
@ 85.6933 MPa, 845.730 atm
|Heat of fusion||5.968 kJ/mol|
|Heat of vaporization||158.013 kJ/mol|
|Heat capacity|| 0.07711 J/g/K, 0.13879 J/g/°R|
26.513 J/mol/K, 47.723 J/mol/°R
|Universe (by mass)|| Relative: 2.88 × 10−22|
Absolute: 9.66 × 1030 kg
Planckium is the fabricated name of a theoretical element with the symbol Pk and atomic number 127. Planckium was named in honor of Max Planck (1858–1947), who founded quantum theory, Planck's law of black body radiation, Planck's constant, and Planck postulate. This element is known in scientific literature as unbiseptium (Ubs), or simply element 127. Planckium is the seventh element of the lavoiside series and located in periodic table coordinate 5g7.
Planckium is a soft, brittle, greenish gray metal. Its molar mass is 360 g/mol and density of 12 g/cm3, dividing molar mass by density yields a molar volume of 29 cm3/mol. The atoms together form centered tetragonal lattices with atoms arranging to form tetragon, plus one in the center. Each lattice contains nine atoms, separated by an average of 363 pm. Upon heating, however, lattices reshape to face centered cubic at 266°C.
The melting point is low for a metal, it melts at 328°C to a dull green liquid. It boils more than 1000°C higher than its melting point, at 1374°C. Like all other materials, melting and boiling points are not the same at every conditions. Planckium would have different melting and boiling points at different pressures. Changing pressures affect boiling point, but it has tiny effect on melting point. The triple point of planckium is 328°C and at a pressure of 50 micropascals, the point where all three states of matter: solid, liquid, and gas, coexist. The critical point is 3593°C and 86 MPa; above that in both temperature and pressure, planckium exists as a supercritical fluid, whose property resemble both a liquid and gas. The molar heat capacity is 26.51 J/mol/°C, meaning the amount of energy needed to heat one mole of planckium by 1°C is 26.51 joules.
Plancium's atom comprises of 468 particles, with 73% of these are nucleons, particles that make up the nucleus at the atom's center. Nucleons are category of particles that includes protons and neutrons. There are 341 nucleons, 127 of these are positively charged protons that determines its atomic number, while the remaining 214 are neutrons which carry no charge. The remaining 27% of all subatomic particles are electrons found in 23 orbitals in 8 shells. Due to spin-orbit coupling, this element has added an electron in the 8p orbital. This leaves g-orbital with less electrons than is expected from the periodic table. In fact, there are two electrons in the 6f orbital, meaning there are three less electrons in the g-orbital than the periodic table would expect.
Like every other elements heavier than lead, planckium has no stable isotopes. The most stable isotope is 341Pk with a half-life of 963,620 years, alpha decaying to 337Dt. 355Pk has a half-life of 4,760 years, 342Pk has a half-life of 196 years, and 340Pk has a half-life of 2.60 years. All the remaining isotopes have half-lives less than a month and majority of these have half-lives less than 40 minutes. 334Pk (t½ = 17.7 minutes) is a beta decay product of its most stable maxwellium isotope 334Mw. There are also several metastable isomers, the most stable being 341m2Pk, whose half-life is 4.6 minutes (280 seconds). Other examples of isomers are 343mPk (30 seconds), 344m1Pk (286 milliseconds), and 339mPk (103 milliseconds).
Planckium has chemical properties similar to some other lavoisoids due to electrons filling in the deeply buried g-orbital. It commonly loses as many as seven or nine electrons due to low binding energy of electrons. The first ionization energy is 5.01 eV, which is the amount of energy required to remove an electron during ionization. The second ionization energy is only slightly higher than first, with the amount of energy needed to lose seven or nine electrons is only about 50–60% higher than energy needed to lose one electron. This would make planckium quite reactive and forms compounds easily. For example, pure planckium would tarnish rapidly in the air to form an oxide coating which protects the metal inside from further oxidation. In the powder form, it burns with a brilliant pink flame. The metal gets eaten by mineral acids, most rapidly in hydrochloric acid.
Pk7+, the most common ion, forms black solution, while Pk9+ forms dark brown solution and Pk5+ forms colorless. Due to its high oxistates, planckium can form exotic organic compounds called organoplanckium.
The most common oxide of planckium is planckium(VII) oxide (Pk2O7), which is a black solid. Planckium(VII) chloride (PkCl7) can be created when planckium reacts with hydrochloric acid or chlorides of higher electronegative metals. PkCl7 is a clear liquid or colorless gas with the boiling point of 24.78°C, right about the room temperature. Planckium nonafluoride (PkF9) is a gas with the condensation point of −98°C. Planckium(VII) sulfide (Pk2S7) is a pale yellow solid which can be made when this element reacts with hydrogen sulfide or carbonyl sulfide. Planckium(VIII) carbonate (Pk(CO3)4) is a white powder.
Planckium carry mainly +5 and +7 oxistates in salts. Planckium(V) sulfate (Pk2(SO4)5) and planckium(VII) nitrate (Pk(NO3)7) are the examples. Planckium can form organometallic compounds, known as organoplanckium. Such examples are pentaethylplanckium ((C2H5)5Pk) and pentachloromethylplanckium ((CH2Cl)5Pk).
Occurrence and synthesis Edit
It is certain that planckium is virtually nonexistent on Earth, and is extremely rare in the universe. Since every element heavier than lithium were produced by stars, then ium 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, however planckium can naturally be made as beta decay product of maxwellium. An estimated abundance of planckium in the universe by mass is 2.88 × 10−22, which amounts to 9.66 × 1030 kilograms or about five solar masses worth of planckium.
To go along with other such civilizations, humans on Earth may eventually have the capability to synthesize planckium. To synthesize most stable isotopes of planckium, nuclei of a couple lighter elements must be fused together, and right amount of neutrons must be seeded. This operation would be very difficult since it requires a great deal of energy. Here's couple of example equations in the production of the most stable isotope 341Pk.
There had been an attempt to synthesize planckium without enriching it with neutrons. In the near future, planckium shall successfully be made here on Earth.