LabLynx Wiki

Posted on July 23, 2020 By Robert Payne

Edit links
Not to be confused with ruthenium.

Rubidium, 37Rb
Rubidium
Pronunciation/ruːˈbɪdiəm/ ​(roo-BID-ee-əm)
Appearancegrey white
Standard atomic weight Ar°(Rb)
Rubidium in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
K
↑
Rb
↓
Cs
krypton ← rubidium → strontium
Atomic number (Z)37
Groupgroup 1: hydrogen and alkali metals
Periodperiod 5
Block  s-block
Electron configuration[Kr] 5s1
Electrons per shell2, 8, 18, 8, 1
Physical properties
Phase at STPsolid
Melting point312.45 K ​(39.30 °C, ​102.74 °F)
Boiling point961 K ​(688 °C, ​1270 °F)
Density (at 20° C)1.534 g/cm3[3]
when liquid (at m.p.)1.46 g/cm3
Triple point312.41 K, ​? kPa[4]
Critical point2093 K, 16 MPa (extrapolated)[4]
Heat of fusion2.19 kJ/mol
Heat of vaporization69 kJ/mol
Molar heat capacity31.060 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 434 486 552 641 769 958
Atomic properties
Oxidation statescommon: +1
−1[5]
ElectronegativityPauling scale: 0.82
Ionization energies
  • 1st: 403 kJ/mol
  • 2nd: 2632.1 kJ/mol
  • 3rd: 3859.4 kJ/mol
Atomic radiusempirical: 248 pm
Covalent radius220±9 pm
Van der Waals radius303 pm
Color lines in a spectral range
Spectral lines of rubidium
Other properties
Natural occurrenceprimordial
Crystal structure ​body-centered cubic (bcc) (cI2)
Lattice constant
Body-centered cubic crystal structure for rubidium
a = 569.9 pm (at 20 °C)[3]
Thermal expansion85.6×10−6/K (at 20 °C)[3]
Thermal conductivity58.2 W/(m⋅K)
Electrical resistivity128 nΩ⋅m (at 20 °C)
Magnetic orderingparamagnetic[6]
Molar magnetic susceptibility+17.0×10−6 cm3/mol (303 K)[7]
Young's modulus2.4 GPa
Bulk modulus2.5 GPa
Speed of sound thin rod1300 m/s (at 20 °C)
Mohs hardness0.3
Brinell hardness0.216 MPa
CAS Number7440-17-7
History
DiscoveryRobert Bunsen and Gustav Kirchhoff (1861)
First isolationGeorge de Hevesy
Isotopes of rubidium
Main isotopes[8] Decay
abun­dance half-life (t1/2) mode pro­duct
82Rb synth 1.2575 m β+ 82Kr
83Rb synth 86.2 d ε 83Kr
γ –
84Rb synth 32.9 d ε 84Kr
β+ 84Kr
γ –
β− 84Sr
85Rb 72.2% stable
86Rb synth 18.7 d β− 86Sr
γ –
87Rb 27.8% 4.923×1010 y β− 87Sr
 Category: Rubidium
| references

Rubidium is a chemical element; it has symbol Rb and atomic number 37. It is a very soft, whitish-grey solid in the alkali metal group, similar to potassium and caesium.[9] Rubidium is the first alkali metal in the group to have a density higher than water. On Earth, natural rubidium comprises two isotopes: 72% is a stable isotope 85Rb, and 28% is slightly radioactive 87Rb, with a half-life of 48.8 billion years – more than three times as long as the estimated age of the universe.

German chemists Robert Bunsen and Gustav Kirchhoff discovered rubidium in 1861 by the newly developed technique, flame spectroscopy. The name comes from the Latin word rubidus, meaning deep red, the color of its emission spectrum. Rubidium's compounds have various chemical and electronic applications. Rubidium metal is easily vaporized and has a convenient spectral absorption range, making it a frequent target for laser manipulation of atoms.[10] Rubidium is not a known nutrient for any living organisms. However, rubidium ions have similar properties and the same charge as potassium ions, and are actively taken up and treated by animal cells in similar ways.

Characteristics

Physical properties

Partially molten rubidium metal in an ampoule

Rubidium is a very soft, ductile, silvery-white metal.[11] It has a melting point of 39.3 °C (102.7 °F) and a boiling point of 688 °C (1,270 °F).[12] It forms amalgams with mercury and alloys with gold, iron, caesium, sodium, and potassium, but not lithium (despite rubidium and lithium being in the same periodic group).[13] 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.[14]

Chemical properties

Rubidium crystals (silvery) compared to caesium crystals (golden)

Rubidium is the second most electropositive of the stable alkali metals and has a very low first ionization energy of only 403 kJ/mol.[12] It has an electron configuration of [Kr]5s1 and is photosensitive.[15]: 382  Due to its strong electropositive nature, rubidium reacts explosively with water[16] to produce rubidium hydroxide and hydrogen gas.[15]: 383  As with all the alkali metals, the reaction is usually vigorous enough to ignite metal or the hydrogen gas produced by the reaction, potentially causing an explosion.[17] Rubidium, being denser than potassium, sinks in water, reacting violently; caesium explodes on contact with water.[18] However, the reaction rates of all alkali metals depend upon surface area of metal in contact with water, with small metal droplets giving explosive rates.[19] Rubidium has also been reported to ignite spontaneously in air.[11]

Compounds

See also: Category:Rubidium compounds
The ball-and-stick diagram shows two regular octahedra which are connected to each other by one face. All nine vertices of the structure are purple spheres representing rubidium, and at the centre of each octahedron is a small red sphere representing oxygen.
Rb
9O
2 cluster

Rubidium chloride (RbCl) is probably the most used rubidium compound: among several other chlorides, it is used to induce living cells to take up DNA; it is also used as a biomarker, because in nature, it is found only in small quantities in living organisms and when present, replaces potassium. Other common rubidium compounds are the corrosive rubidium hydroxide (RbOH), the starting material for most rubidium-based chemical processes; rubidium carbonate (Rb2CO3), used in some optical glasses, and rubidium copper sulfate, Rb2SO4·CuSO4·6H2O. Rubidium silver iodide (RbAg4I5) has the highest room temperature conductivity of any known ionic crystal, a property exploited in thin film batteries and other applications.[20][21]

Rubidium forms a number of oxides when exposed to air, including rubidium monoxide (Rb2O), Rb6O, and Rb9O2; rubidium in excess oxygen gives the superoxide RbO2. Rubidium forms salts with halogens, producing rubidium fluoride, rubidium chloride, rubidium bromide, and rubidium iodide.[22]

Isotopes

Main article: Isotopes of rubidium

Although rubidium is monoisotopic, rubidium in the Earth's crust is composed of two isotopes: the stable 85Rb (72.2%) and the radioactive 87Rb (27.8%).[23] Natural rubidium is radioactive, with specific activity of about 670 Bq/g, enough to significantly expose a photographic film in 110 days.[24][25] Thirty additional rubidium isotopes have been synthesized with half-lives of less than 3 months; most are highly radioactive and have few uses.[26]

Rubidium-87 has a half-life of 48.8×109 years, which is more than three times the age of the universe of (13.799±0.021)×109 years,[27] making it a primordial nuclide. It readily substitutes for potassium in minerals, and is therefore fairly widespread. Rb has been used extensively in dating rocks; 87Rb beta decays to stable 87Sr. During fractional crystallization, Sr tends to concentrate in plagioclase, leaving Rb in the liquid phase. Hence, the Rb/Sr ratio in residual magma may increase over time, and the progressing differentiation results in rocks with elevated Rb/Sr ratios. The highest ratios (10 or more) occur in pegmatites. If the initial amount of Sr is known or can be extrapolated, then the age can be determined by measurement of the Rb and Sr concentrations and of the 87Sr/86Sr ratio. The dates indicate the true age of the minerals only if the rocks have not been subsequently altered (see rubidium–strontium dating).[28][29]

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. With a half-life of 76 seconds, rubidium-82 decays by positron emission to stable krypton-82.[23]

Occurrence

Rubidium is not abundant, being one of 56 elements that combined make up 0.05% of the Earth's crust; at roughly the 23rd most abundant element in the Earth's crust it is more abundant than zinc or copper.[30]: 4  It occurs naturally in the minerals leucite, pollucite, carnallite, and zinnwaldite, which contain as much as 1% rubidium oxide. Lepidolite contains between 0.3% and 3.5% rubidium, and is the commercial source of the element.[31] Some potassium minerals and potassium chlorides also contain the element in commercially significant quantities.[32]

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.[33] Rubidium is the 18th most abundant element in seawater.[15]: 371 

Because of its large ionic radius, rubidium is one of the "incompatible elements".[34] During magma crystallization, rubidium is concentrated together with its heavier analogue caesium in the liquid phase and crystallizes last. Therefore, the largest deposits of rubidium and caesium are zone pegmatite ore bodies formed by this enrichment process. Because rubidium substitutes for potassium in the crystallization of magma, the enrichment is far less effective than that of caesium. Zone pegmatite ore bodies containing mineable quantities of caesium as pollucite or the lithium minerals lepidolite are also a source for rubidium as a by-product.[30]

Two notable sources of rubidium are the rich deposits of pollucite at Bernic Lake, Manitoba, Canada, and the rubicline ((Rb,K)AlSi3O8) found as impurities in pollucite on the Italian island of Elba, with a rubidium content of 17.5%.[35] Both of those deposits are also sources of caesium.[36]

Production

Flame test for rubidium

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.[30] Several methods are available for separating potassium, rubidium, and caesium. The fractional crystallization of a rubidium and caesium alum (Cs,Rb)Al(SO4)2·12H2O yields after 30 subsequent steps pure rubidium alum. Two other methods are reported, the chlorostannate process and the ferrocyanide process.[30][37]

For several years in the 1950s and 1960s, a by-product of potassium production called Alkarb was a main source for rubidium. Alkarb contained 21% rubidium, with the rest being potassium and a small amount of caesium.[38] Today the largest producers of caesium produce rubidium as a by-product from pollucite.[30]

History

Three middle-aged men, with the one in the middle sitting down. All wear long jackets, and the shorter man on the left has a beard.
Gustav Kirchhoff (left) and Robert Bunsen (center) discovered rubidium by spectroscopy. (Henry Enfield Roscoe is on the right.)

Rubidium was discovered in 1861 by Robert Bunsen and Gustav Kirchhoff, in Heidelberg, Germany, in the mineral lepidolite through flame spectroscopy. Because of the bright red lines in its emission spectrum, they chose a name derived from the Latin word rubidus, meaning "deep red".[39][40]

Rubidium is a minor component in lepidolite. Kirchhoff and Bunsen processed 150 kg of a lepidolite containing only 0.24% rubidium monoxide (Rb2O). Both potassium and rubidium form insoluble salts with chloroplatinic acid, but those salts show a slight difference in solubility in hot water. Therefore, the less soluble rubidium hexachloroplatinate (Rb2PtCl6) could be obtained by fractional crystallization. After reduction of the hexachloroplatinate with hydrogen, the process yielded 0.51 grams of rubidium chloride (RbCl) for further studies. Bunsen and Kirchhoff began their first large-scale isolation of caesium and rubidium compounds with 44,000 litres (12,000 US gal) of mineral water, which yielded 7.3 grams of caesium chloride and 9.2 grams of rubidium chloride.[39][40] Rubidium was the second element, shortly after caesium, to be discovered by spectroscopy, just one year after the invention of the spectroscope by Bunsen and Kirchhoff.[41]

The two scientists used the rubidium chloride to estimate that the atomic weight of the new element was 85.36 (the currently accepted value is 85.47).[39] They tried to generate elemental rubidium by electrolysis of molten rubidium chloride, but instead of a metal, they obtained a blue homogeneous substance, which "neither under the naked eye nor under the microscope showed the slightest trace of metallic substance". They presumed that it was a subchloride (Rb
2Cl); however, the product was probably a colloidal mixture of the metal and rubidium chloride.[42] In a second attempt to produce metallic rubidium, Bunsen was able to reduce rubidium by heating charred rubidium tartrate. Although the distilled rubidium was pyrophoric, they were able to determine the density and the melting point. The quality of this research in the 1860s can be appraised by the fact that their determined density differs by less than 0.1 g/cm3 and the melting point by less than 1 °C from the presently accepted values.[43]

The slight radioactivity of rubidium was discovered in 1908, but that was before the theory of isotopes was established in 1910, and the low level of activity (half-life greater than 1010 years) made interpretation complicated. The now proven decay of 87Rb to stable 87Sr through beta decay was still under discussion in the late 1940s.[44][45]

Rubidium had minimal industrial value before the 1920s.[30] Since then, the most important use of rubidium is research and development, primarily in chemical and electronic applications. In 1995, rubidium-87 was used to produce a Bose–Einstein condensate,[46] for which the discoverers, Eric Allin Cornell, Carl Edwin Wieman and Wolfgang Ketterle, won the 2001 Nobel Prize in Physics.[47]

Applications

A rubidium fountain atomic clock at the United States Naval Observatory

Rubidium compounds are sometimes used in fireworks to give them a purple color.[48] Rubidium has also been considered for use in a thermoelectric generator using the magnetohydrodynamic principle, whereby hot rubidium ions are passed through a magnetic field.[49] These conduct electricity and act like an armature of a generator, thereby generating an electric current. Rubidium, particularly vaporized 87Rb, is one of the most commonly used atomic species employed for laser cooling and Bose–Einstein condensation. Its desirable features for this application include the ready availability of inexpensive diode laser light at the relevant wavelength and the moderate temperatures required to obtain substantial vapor pressures.[50][51] For cold-atom applications requiring tunable interactions, 85Rb is preferred for its rich Feshbach spectrum.[52]

Rubidium has been used for polarizing 3He, producing volumes of magnetized 3He gas, with the nuclear spins aligned rather than random. Rubidium vapor is optically pumped by a laser, and the polarized Rb polarizes 3He through the hyperfine interaction.[53] Such spin-polarized 3He cells are useful for neutron polarization measurements and for producing polarized neutron beams for other purposes.[54]

The resonant element in atomic clocks utilizes the hyperfine structure of rubidium's energy levels, and rubidium is useful for high-precision timing. It is used as the main component of secondary frequency references (rubidium oscillators) in cell site transmitters and other electronic transmitting, networking, and test equipment. These rubidium standards are often used with GNSS to produce a "primary frequency standard" that has greater accuracy and is less expensive than caesium standards.[55][56] Such rubidium standards are often mass-produced for the telecommunications industry.[57]

Other potential or current uses of rubidium include a working fluid in vapor turbines, as a getter in vacuum tubes, and as a photocell component.[58] 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.[59] In particular, 87Rb is used with other alkali metals in the development of spin-exchange relaxation-free (SERF) magnetometers.[59]

Rubidium-82 is used for positron emission tomography. Rubidium is very similar to potassium, and tissue with high potassium content will also accumulate the radioactive rubidium. One of the main uses is myocardial perfusion imaging. As a result of changes in the blood–brain barrier in brain tumors, rubidium collects more in brain tumors than normal brain tissue, allowing the use of radioisotope rubidium-82 in nuclear medicine to locate and image brain tumors.[60] Rubidium-82 has a very short half-life of 76 seconds, and the production from decay of strontium-82 must be done close to the patient.[61]

Rubidium was tested for the influence on manic depression and depression.[62][63] Dialysis patients suffering from depression show a depletion in rubidium, and therefore a supplementation may help during depression.[64] In some tests the rubidium was administered as rubidium chloride with up to 720 mg per day for 60 days.[65][66]

Rubidium
Hazards
GHS labelling:
GHS02: FlammableGHS05: Corrosive
Danger
H260, H314
P223, P231+P232, P280, P305+P351+P338, P370+P378, P422[67]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard W: Reacts with water in an unusual or dangerous manner. E.g. sodium, sulfuric acid
3
4
2
W

Precautions and biological effects

Rubidium reacts violently with water and can cause fires. To ensure safety and purity, this metal is usually kept under dry mineral oil or sealed in glass ampoules in an inert atmosphere. Rubidium forms peroxides on exposure even to a small amount of air diffused into the oil, and storage is subject to similar precautions as the storage of metallic potassium.[68]

Rubidium, like sodium and potassium, almost always has +1 oxidation state when dissolved in water, even in biological contexts. The human body tends to treat Rb+ ions as if they were potassium ions, and therefore concentrates rubidium in the body's intracellular fluid (i.e., inside cells).[69] 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.[70] The biological half-life of rubidium in humans measures 31–46 days.[62] Although a partial substitution of potassium by rubidium is possible, when more than 50% of the potassium in the muscle tissue of rats was replaced with rubidium, the rats died.[71][72]

References

  1. ^ "Standard Atomic Weights: Rubidium". CIAAW. 1969.
  2. ^ Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (2022-05-04). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN 1365-3075.
  3. ^ a b c Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN 978-1-62708-155-9.
  4. ^ a b Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, Florida: CRC Press. p. 4.122. ISBN 1-4398-5511-0.
  5. ^ Rb(–1) is known in rubidides; see John E. Ellis (2006). "Adventures with Substances Containing Metals in Negative Oxidation States". Inorganic Chemistry. 45 (8). doi:10.1021/ic052110i.
  6. ^ Lide, D. R., ed. (2005). "Magnetic susceptibility of the elements and inorganic compounds". CRC Handbook of Chemistry and Physics (PDF) (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
  7. ^ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
  8. ^ Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  9. ^ Lenk, Winfried; Prinz, Horst; Steinmetz, Anja (2010). "Rubidium and Rubidium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a23_473.pub2. ISBN 978-3527306732.
  10. ^ "Rubidium (Rb)". American Elements (americanelements.com). Retrieved 2024-03-27.
  11. ^ a b Ohly, Julius (1910). "Rubidium". Analysis, detection and commercial value of the rare metals. Mining Science Pub. Co. – via Google books.
  12. ^ a b "Rubidium". Element information, properties and uses. www.rsc.org. Periodic Table. Retrieved 2024-09-09.
  13. ^ Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (1985). "Vergleichende Übersicht über die Gruppe der Alkalimetalle" [Brief overview of the Alkalai metal group]. Lehrbuch der Anorganischen Chemie [Textbook of Inorganic Chemistry] (in German) (91–100 ed.). Walter de Gruyter. pp. 953–955. ISBN 978-3-11-007511-3.
  14. ^ Ahrens, L.H.; Pinson, W.H.; Kearns, Makgaret M. (1952-01-01). "Association of rubidium and potassium and their abundance in common igneous rocks and meteorites". Geochimica et Cosmochimica Acta. 2 (4): 229–242. Bibcode:1952GeCoA...2..229A. doi:10.1016/0016-7037(52)90017-3. ISSN 0016-7037.
  15. ^ a b c Hart, William A.; Beumel Jr., O.F .; Whaley, Thomas P. (1973). The Chemistry of Lithium, Sodium, Potassium, Rubidium, Cesium and Francium. Pergamon. doi:10.1016/c2013-0-05695-2. ISBN 978-0-08-018799-0.
  16. ^ Cotton, F. Albert; Wilkinson, Geoffrey (1972). Advanced inorganic chemistry: a comprehensive text (3d ed., completely rev ed.). New York: Interscience Publishers. p. 190. ISBN 978-0-471-17560-5.
  17. ^ Stanford University. "Information on Alkali Metals – Stanford Environmental Health & Safety". Retrieved 2024-09-12.
  18. ^ Jim Clark. "Reactions of the Group 1 elements with water". www.chemguide.co.uk. Retrieved 2024-09-12.
  19. ^ Maustellar, J. W, F Tepper, and S. J. (Sheridan Joseph) Rodgers. "Alkali Metal Handling and Systems Operating Techniques" Prepared under the Direction of the American Nuclear Society for the United States Atomic Energy Commission. New York: Gordon and Breach, 1968.
  20. ^ Smart, Lesley; Moore, Elaine (1995). "RbAg4I5". Solid state chemistry: an introduction. CRC Press. pp. 176–177. ISBN 978-0-7487-4068-0.
  21. ^ Bradley, J. N.; Greene, P. D. (1967). "Relationship of structure and ionic mobility in solid MAg4I5". Trans. Faraday Soc. 63: 2516. doi:10.1039/TF9676302516.
  22. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  23. ^ a b Audi, Georges; Bersillon, Olivier; Blachot, Jean; Wapstra, Aaldert Hendrik (2003), "The NUBASE evaluation of nuclear and decay properties", Nuclear Physics A, 729: 3–128, Bibcode:2003NuPhA.729....3A, doi:10.1016/j.nuclphysa.2003.11.001
  24. ^ Strong, W. W. (1909). "On the Possible Radioactivity of Erbium, Potassium and Rubidium". Physical Review. Series I. 29 (2): 170–173. Bibcode:1909PhRvI..29..170S. doi:10.1103/PhysRevSeriesI.29.170.
  25. ^ Lide, David R; Frederikse, H. P. R (June 1995). CRC handbook of chemistry and physics: a ready-reference book of chemical and physical data. CRC-Press. pp. 4–25. ISBN 978-0-8493-0476-7.
  26. ^ "Universal Nuclide Chart". nucleonica. Archived from the original on 2017-02-19. Retrieved 2017-01-03.
  27. ^ Planck Collaboration (2016). "Planck 2015 results. XIII. Cosmological parameters (See Table 4 on page 31 of pfd)". Astronomy & Astrophysics. 594: A13. arXiv:1502.01589. Bibcode:2016A&A...594A..13P. doi:10.1051/0004-6361/201525830. S2CID 119262962.
  28. ^ Attendorn, H.-G.; Bowen, Robert (1988). "Rubidium-Strontium Dating". Isotopes in the Earth Sciences. Springer. pp. 162–165. ISBN 978-0-412-53710-3.
  29. ^ Walther, John Victor (2009) [1988]. "Rubidium-Strontium Systematics". Essentials of geochemistry. Jones & Bartlett Learning. pp. 383–385. ISBN 978-0-7637-5922-3.
  30. ^ a b c d e f Butterman, William C.; Brooks, William E.; Reese, Robert G. Jr. (2003). "Mineral Commodity Profile: Rubidium" (PDF). United States Geological Survey. Retrieved 2010-12-04.
  31. ^ Wise, M. A. (1995). "Trace element chemistry of lithium-rich micas from rare-element granitic pegmatites". Mineralogy and Petrology. 55 (13): 203–215. Bibcode:1995MinPe..55..203W. doi:10.1007/BF01162588. S2CID 140585007.
  32. ^ Norton, J. J. (1973). "Lithium, cesium, and rubidium—The rare alkali metals". In Brobst, D. A.; Pratt, W. P. (eds.). United States mineral resources. Vol. Paper 820. U.S. Geological Survey Professional. pp. 365–378. Archived from the original on 2010-07-21. Retrieved 2010-09-26.
  33. ^ Bolter, E.; Turekian, K.; Schutz, D. (1964). "The distribution of rubidium, cesium and barium in the oceans". Geochimica et Cosmochimica Acta. 28 (9): 1459. Bibcode:1964GeCoA..28.1459B. doi:10.1016/0016-7037(64)90161-9.
  34. ^ McSween Jr., Harry Y; Huss, Gary R (2010). Cosmochemistry. Cambridge University Press. p. 224. ISBN 978-0-521-87862-3.
  35. ^ Teertstra, David K.; Cerny, Petr; Hawthorne, Frank C.; Pier, Julie; Wang, Lu-Min; Ewing, Rodney C. (1998). "Rubicline, a new feldspar from San Piero in Campo, Elba, Italy". American Mineralogist. 83 (11–12 Part 1): 1335–1339. Bibcode:1998AmMin..83.1335T. doi:10.2138/am-1998-11-1223.
  36. ^ Enghag, Per (2004). "Rubidium and Caesium". Encyclopedia of the Elements (1 ed.). Wiley. doi:10.1002/9783527612338.ch13. ISBN 978-3-527-30666-4.
  37. ^ bulletin 585. United States. Bureau of Mines. 1995.
  38. ^ "Cesium and Rubidium Hit Market". Chemical & Engineering News. 37 (22): 50–56. 1959. doi:10.1021/cen-v037n022.p050.
  39. ^ a b c Kirchhoff, G.; Bunsen, R. (1861). "Chemische Analyse durch Spectralbeobachtungen" (PDF). Annalen der Physik und Chemie. 189 (7): 337–381. Bibcode:1861AnP...189..337K. doi:10.1002/andp.18611890702. hdl:2027/hvd.32044080591324.
  40. ^ a b Weeks, Mary Elvira (1932). "The discovery of the elements. XIII. Some spectroscopic discoveries". Journal of Chemical Education. 9 (8): 1413–1434. Bibcode:1932JChEd...9.1413W. doi:10.1021/ed009p1413.
  41. ^ Ritter, Stephen K. (2003). "C&EN: It's Elemental: The Periodic Table – Cesium". American Chemical Society. Retrieved 2010-02-25.
  42. ^ Zsigmondy, Richard (2007). Colloids and the Ultra Microscope. Read books. p. 69. ISBN 978-1-4067-5938-9. Retrieved 2010-09-26.
  43. ^ Bunsen, R. (1863). "Ueber die Darstellung und die Eigenschaften des Rubidiums". Annalen der Chemie und Pharmacie. 125 (3): 367–368. doi:10.1002/jlac.18631250314.
  44. ^ Lewis, G. M. (1952). "The natural radioactivity of rubidium". Philosophical Magazine. Series 7. 43 (345): 1070–1074. doi:10.1080/14786441008520248.
  45. ^ Campbell, N. R.; Wood, A. (1908). "The Radioactivity of Rubidium". Proceedings of the Cambridge Philosophical Society. 14: 15.
  46. ^ "The 2001 Nobel Prize in Physics". Nobel Institute nobelprize.org (Press release). 2001. Retrieved 2010-02-01.
  47. ^ Levi, Barbara Goss (2001). "Cornell, Ketterle, and Wieman share Nobel Prize for Bose-Einstein condensates". Physics Today. 54 (12): 14–16. Bibcode:2001PhT....54l..14L. doi:10.1063/1.1445529.
  48. ^ Koch, E.-C. (2002). "Special Materials in Pyrotechnics, Part II: Application of Caesium and Rubidium Compounds in Pyrotechnics". Journal Pyrotechnics. 15: 9–24. Archived from the original on 2011-07-13. Retrieved 2010-01-29.
  49. ^ Boikess, Robert S; Edelson, Edward (1981). Chemical principles. Harper & Row. p. 193. ISBN 978-0-06-040808-4.
  50. ^ Eric Cornell; et al. (1996). "Bose-Einstein condensation (all 20 articles)". Journal of Research of the National Institute of Standards and Technology. 101 (4): 419–618. doi:10.6028/jres.101.045. PMC 4907621. PMID 27805098. Archived from the original on 2011-10-14. Retrieved 2015-09-14.
  51. ^ Martin, J. L.; McKenzie, C. R.; Thomas, N. R.; Sharpe, J. C.; Warrington, D. M.; Manson, P. J.; Sandle, W. J.; Wilson, A. C. (1999). "Output coupling of a Bose-Einstein condensate formed in a TOP trap". Journal of Physics B: Atomic, Molecular and Optical Physics. 32 (12): 3065. arXiv:cond-mat/9904007. Bibcode:1999JPhB...32.3065M. doi:10.1088/0953-4075/32/12/322. S2CID 119359668.
  52. ^ Chin, Cheng; Grimm, Rudolf; Julienne, Paul; Tiesinga, Eite (2010-04-29). "Feshbach resonances in ultracold gases". Reviews of Modern Physics. 82 (2): 1225–1286. arXiv:0812.1496. Bibcode:2010RvMP...82.1225C. doi:10.1103/RevModPhys.82.1225. S2CID 118340314.
  53. ^ Gentile, T. R.; Chen, W. C.; Jones, G. L.; Babcock, E.; Walker, T. G. (2005). "Polarized 3He spin filters for slow neutron physics" (PDF). Journal of Research of the National Institute of Standards and Technology. 110 (3): 299–304. doi:10.6028/jres.110.043. PMC 4849589. PMID 27308140. Archived from the original (PDF) on 2016-12-21. Retrieved 2015-08-06.
  54. ^ "Neutron spin filters based on polarized helium-3". NIST Center for Neutron Research 2002 Annual Report. Retrieved 2008-01-11.
  55. ^ Eidson, John C (2006-04-11). "GPS". Measurement, control, and communication using IEEE 1588. Springer. p. 32. ISBN 978-1-84628-250-8.
  56. ^ King, Tim; Newson, Dave (1999-07-31). "Rubidium and crystal oscillators". Data network engineering. Springer. p. 300. ISBN 978-0-7923-8594-3.
  57. ^ Marton, L. (1977-01-01). "Rubidium Vapor Cell". Advances in electronics and electron physics. Academic Press. ISBN 978-0-12-014644-4.
  58. ^ Mittal (2009). Introduction To Nuclear And Particle Physics. Prentice-Hall Of India Pvt. Limited. p. 274. ISBN 978-81-203-3610-0.
  59. ^ a b Li, Zhimin; Wakai, Ronald T.; Walker, Thad G. (2006). "Parametric modulation of an atomic magnetometer". Applied Physics Letters. 89 (13): 23575531–23575533. Bibcode:2006ApPhL..89m4105L. doi:10.1063/1.2357553. PMC 3431608. PMID 22942436.
  60. ^ Yen, C. K.; Yano, Y.; Budinger, T. F.; Friedland, R. P.; Derenzo, S. E.; Huesman, R. H.; O'Brien, H. A. (1982). "Brain tumor evaluation using Rb-82 and positron emission tomography". Journal of Nuclear Medicine. 23 (6): 532–7. PMID 6281406.
  61. ^ Jadvar, H.; Anthony Parker, J. (2005). "Rubidium-82". Clinical PET and PET/CT. Springer. p. 59. ISBN 978-1-85233-838-1.
  62. ^ a b Paschalis, C.; Jenner, F. A.; Lee, C. R. (1978). "Effects of rubidium chloride on the course of manic-depressive illness". J R Soc Med. 71 (9): 343–352. doi:10.1177/014107687807100507. PMC 1436619. PMID 349155.
  63. ^ Malekahmadi, P.; Williams, John A. (1984). "Rubidium in psychiatry: Research implications". Pharmacology Biochemistry and Behavior. 21: 49–50. doi:10.1016/0091-3057(84)90162-X. PMID 6522433. S2CID 2907703.
  64. ^ Canavese, Caterina; Decostanzi, Ester; Branciforte, Lino; Caropreso, Antonio; Nonnato, Antonello; Sabbioni, Enrico (2001). "Depression in dialysis patients: Rubidium supplementation before other drugs and encouragement?". Kidney International. 60 (3): 1201–2. doi:10.1046/j.1523-1755.2001.0600031201.x. PMID 11532118.
  65. ^ Lake, James A. (2006). Textbook of Integrative Mental Health Care. New York: Thieme Medical Publishers. pp. 164–165. ISBN 978-1-58890-299-3.
  66. ^ Torta, R.; Ala, G.; Borio, R.; Cicolin, A.; Costamagna, S.; Fiori, L.; Ravizza, L. (1993). "Rubidium chloride in the treatment of major depression". Minerva Psichiatrica. 34 (2): 101–110. PMID 8412574.
  67. ^ "Rubidium 276332". Sigma-Aldrich.
  68. ^ Martel, Bernard; Cassidy, Keith (2004-07-01). "Rubidium". Chemical risk analysis: a practical handbook. Butterworth-Heinemann. p. 215. ISBN 978-1-903996-65-2.
  69. ^ Relman, A. S. (1956). "The Physiological Behavior of Rubidium and Cesium in Relation to That of Potassium". The Yale Journal of Biology and Medicine. 29 (3): 248–62. PMC 2603856. PMID 13409924.
  70. ^ Fieve, Ronald R.; Meltzer, Herbert L.; Taylor, Reginald M. (1971). "Rubidium chloride ingestion by volunteer subjects: Initial experience". Psychopharmacologia. 20 (4): 307–14. doi:10.1007/BF00403562. PMID 5561654. S2CID 33738527.
  71. ^ Meltzer, H. L. (1991). "A pharmacokinetic analysis of long-term administration of rubidium chloride". Journal of Clinical Pharmacology. 31 (2): 179–84. doi:10.1002/j.1552-4604.1991.tb03704.x. PMID 2010564. S2CID 2574742. Archived from the original on 2012-07-09.
  72. ^ Follis, Richard H. Jr. (1943). "Histological effects in rats resulting from adding rubidium or cesium to a diet deficient in potassium". AJP: Legacy Content. 138 (2): 246–250. doi:10.1152/ajplegacy.1943.138.2.246.

Further reading

  • Meites, Louis (1963). Handbook of Analytical Chemistry (New York: McGraw-Hill Book Company, 1963)
  • Steck, Daniel A. "Rubidium-87 D Line Data" (PDF). Los Alamos National Laboratory (technical report LA-UR-03-8638). Archived from the original (PDF) on 2013-11-02. Retrieved 2008-02-09.
source: https://en.wikipedia.org/wiki/Rubidium

    by Robert Payne

    Follow me opinions Website

    Related Posts