rubidium oor Masedonies
rubidium
en
A metallic chemical element (symbol Rb) with an atomic number of 37.
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рубидиум
en
element with atomic number 37
Рубидиум
en
chemical element with the atomic number of 37
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Although the distilled rubidium was pyrophoric, they were able to determine the density and the melting point.
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Several methods are available for separating potassium, rubidium, and caesium.
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Therefore, the largest deposits of rubidium and caesium are zone pegmatite ore bodies formed by this enrichment process.
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Rubidium is also used as an ingredient in special types of glass, in the production of superoxide by burning in oxygen, in the study of potassium ion channels in biology, and as the vapor in atomic magnetometers.
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The resonant element in atomic clocks utilizes the hyperfine structure of rubidium's energy levels, and rubidium is useful for high-precision timing.
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Seawater contains an average of 125 μg/L of rubidium compared to the much higher value for potassium of 408 mg/L and the much lower value of 0.3 μg/L for caesium.
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Because of its large ionic radius, rubidium is one of the "incompatible elements."
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Although rubidium is more abundant in Earth's crust than caesium, the limited applications and the lack of a mineral rich in rubidium limits the production of rubidium compounds to 2 to 4 tonnes per year.
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Rubidium
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Rubidium was discovered in 1861 by Robert Bunsen and Gustav Kirchhoff, in Heidelberg, Germany, in the mineral lepidolite through flame spectroscopy.
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Rubidium has a very low ionization energy of only 406 kJ/mol.
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Rubidium compounds are sometimes used in fireworks to give them a purple color.
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Because rubidium substitutes for potassium in the crystallization of magma, the enrichment is far less effective than that of caesium.
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Rubidium and potassium show a very similar purple color in the flame test, and distinguishing the two elements requires more sophisticated analysis, such as spectroscopy.
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The ions are not particularly toxic; a 70 kg person contains on average 0.36 g of rubidium, and an increase in this value by 50 to 100 times did not show negative effects in test persons.
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Rubidium is not a known nutrient for any living organisms.
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Like other alkali metals, rubidium metal reacts violently with water.
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In some tests the rubidium was administered as rubidium chloride with up to 720 mg per day for 60 days.
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Rubidium-82, one of the element's non-natural isotopes, is produced by electron-capture decay of strontium-82 with a half-life of 25.36 days.
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In 1995, a gas of rubidium atoms cooled down to a temperature of 170 nK was used to experimentally realize the Bose–Einstein condensate, a novel state of matter originally predicted by S. N. Bose and Albert Einstein, wherein a large number of atoms occupy one quantum state.
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During a seminar at the UMCP Department of Chemistry and Biochemistry titled Coherent Atoms in Optical Lattices Phillips stated, "Rubidium is God's gift to Bose–Einstein condensates."
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Both potassium and rubidium form insoluble salts with chloroplatinic acid, but those salts show a slight difference in solubility in hot water.
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For example, rubidium-83 (37 protons, 46 neutrons) will decay to krypton-83 (36 protons, 47 neutrons) solely by electron capture (the energy difference, or decay energy, is about 0.9 MeV).
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However, rubidium ions have the same charge as potassium ions, and are actively taken up and treated by animal cells in similar ways.
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Of the unstable isotopes, the primary decay mode of the isotopes lighter than 85Sr is electron capture or positron emission to isotopes of rubidium, and that of the isotopes heavier than 88Sr is electron emission to isotopes of yttrium.
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86 sinne gevind in 4 ms. Hulle kom uit baie bronne en word nie nagegaan nie.