Rubidium

Last updated

Rubidium, 37Rb
Rb5.JPG
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
Group group 1: hydrogen and alkali metals
Period period 5
Block   s-block
Electron configuration [ Kr ] 5s1
Electrons per shell2, 8, 18, 8, 1
Physical properties
Phase at  STP solid
Melting point 312.45  K ​(39.30 °C,​102.74 °F)
Boiling point 961 K​(688 °C,​1270 °F)
Density (at 20° C)1.534 g/cm3 [3]
when liquid (at  m.p.)1.46 g/cm3
Triple point 312.41 K,​? kPa [4]
Critical point 2093 K, 16 MPa(extrapolated) [4]
Heat of fusion 2.19  kJ/mol
Heat of vaporization 69 kJ/mol
Molar heat capacity 31.060 J/(mol·K)
Vapor pressure
P (Pa)1101001 k10 k100 k
at T (K)434486552641769958
Atomic properties
Oxidation states −1, +1 (a strongly basic oxide)
Electronegativity Pauling scale: 0.82
Ionization energies
  • 1st: 403 kJ/mol
  • 2nd: 2632.1 kJ/mol
  • 3rd: 3859.4 kJ/mol
Atomic radius empirical:248  pm
Covalent radius 220±9 pm
Van der Waals radius 303 pm
Rubidium spectrum visible.png
Spectral lines of rubidium
Other properties
Natural occurrence primordial
Crystal structure ​ body-centered cubic (bcc)(cI2)
Lattice constant
Cubic-body-centered.svg
a = 569.9 pm (at 20 °C) [3]
Thermal expansion 85.6×10−6/K (at 20 °C) [3]
Thermal conductivity 58.2 W/(m⋅K)
Electrical resistivity 128 nΩ⋅m(at 20 °C)
Magnetic ordering paramagnetic [5]
Molar magnetic susceptibility +17.0×10−6 cm3/mol(303 K) [6]
Young's modulus 2.4 GPa
Bulk modulus 2.5 GPa
Speed of sound thin rod1300 m/s(at 20 °C)
Mohs hardness 0.3
Brinell hardness 0.216 MPa
CAS Number 7440-17-7
History
Discovery Robert Bunsen and Gustav Kirchhoff (1861)
First isolation George de Hevesy
Isotopes of rubidium
Main isotopes [7] Decay
abun­dance half-life (t1/2) mode pro­duct
82Rb synth 1.2575 m β+ 82Kr
83Rbsynth86.2 d ε 83Kr
γ –
84Rbsynth32.9 dε 84Kr
β+84Kr
γ–
β− 84Sr
85Rb72.2%stable
86Rbsynth18.7 dβ− 86Sr
γ–
87Rb27.8%4.923×1010 yβ− 87Sr
Symbol category class.svg  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. [8] 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.

Contents

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. [9] 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

Partially molten rubidium metal in an ampoule RbH.JPG
Partially molten rubidium metal in an ampoule

Rubidium is a very soft, ductile, silvery-white metal. [10] It is the second most electropositive of the stable alkali metals and melts at a temperature of 39.3 °C (102.7 °F). Like other alkali metals, rubidium metal reacts violently with water. As with potassium (which is slightly less reactive) and caesium (which is slightly more reactive), this reaction is usually vigorous enough to ignite the hydrogen gas it produces. Rubidium has also been reported to ignite spontaneously in air. [10] It forms amalgams with mercury and alloys with gold, iron, caesium, sodium, and potassium, but not lithium (even though rubidium and lithium are in the same group). [11]

Rubidium crystals (silvery) compared to caesium crystals (golden) Rb&Cs crystals.jpg
Rubidium crystals (silvery) compared to caesium crystals (golden)

Rubidium has a very low ionization energy of only 406 kJ/mol. [12] 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.[ citation needed ]

Compounds

Rb 9O 2 cluster Rb9O2 cluster.png
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. [13] [14]

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. [15]

Isotopes

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%). [16] Natural rubidium is radioactive, with specific activity of about 670 Bq/g, enough to significantly expose a photographic film in 110 days. [17] [18] Thirty additional rubidium isotopes have been synthesized with half-lives of less than 3 months; most are highly radioactive and have few uses. [19]

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, [20] 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). [21] [22]

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. [16]

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. [23] : 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. [24] Some potassium minerals and potassium chlorides also contain the element in commercially significant quantities. [25]

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. [26] Rubidium is the 18th most abundant element in seawater. [27]

Because of its large ionic radius, rubidium is one of the "incompatible elements". [28] 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. [23]

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%. [29] Both of those deposits are also sources of caesium.[ citation needed ]

Production

Flame test for rubidium Die Flammenfarbung des Rubidium.jpg
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. [23] 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. [23] [30]

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. [31] Today the largest producers of caesium produce rubidium as a by-product from pollucite. [23]

History

Gustav Kirchhoff (left) and Robert Bunsen (center) discovered rubidium by spectroscopy. (Henry Enfield Roscoe is on the right.) Kirchhoff Bunsen Roscoe.jpg
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". [32] [33]

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. [32] [33] 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. [34]

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). [32] 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. [35] 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. [36]

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. [37] [38]

Rubidium had minimal industrial value before the 1920s. [39] 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, [40] for which the discoverers, Eric Allin Cornell, Carl Edwin Wieman and Wolfgang Ketterle, won the 2001 Nobel Prize in Physics. [41]

Applications

A rubidium fountain atomic clock at the United States Naval Observatory USNO rubidium fountain.jpg
A rubidium fountain atomic clock at the United States Naval Observatory

Rubidium compounds are sometimes used in fireworks to give them a purple color. [42] 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. [43] 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. [44] [45] For cold-atom applications requiring tunable interactions, 85Rb is preferred for its rich Feshbach spectrum. [46]

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. [47] Such spin-polarized 3He cells are useful for neutron polarization measurements and for producing polarized neutron beams for other purposes. [48]

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. [49] [50] Such rubidium standards are often mass-produced for the telecommunication industry. [51]

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. [52] 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. [53] In particular, 87Rb is used with other alkali metals in the development of spin-exchange relaxation-free (SERF) magnetometers. [53]

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. [54] 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. [55]

Rubidium was tested for the influence on manic depression and depression. [56] [57] Dialysis patients suffering from depression show a depletion in rubidium, and therefore a supplementation may help during depression. [58] In some tests the rubidium was administered as rubidium chloride with up to 720 mg per day for 60 days. [59] [60]

Rubidium
Hazards
GHS labelling:
GHS-pictogram-flamme.svg GHS-pictogram-acid.svg
Danger
H260, H314
P223, P231+P232, P280, P305+P351+P338, P370+P378, P422 [61]
NFPA 704 (fire diamond)
NFPA 704.svgHealth 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. [62]

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). [63] 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. [64] The biological half-life of rubidium in humans measures 31–46 days. [56] 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. [65] [66]

Related Research Articles

<span class="mw-page-title-main">Alkali metal</span> Group of highly reactive chemical elements

The alkali metals consist of the chemical elements lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr). Together with hydrogen they constitute group 1, which lies in the s-block of the periodic table. All alkali metals have their outermost electron in an s-orbital: this shared electron configuration results in their having very similar characteristic properties. Indeed, the alkali metals provide the best example of group trends in properties in the periodic table, with elements exhibiting well-characterised homologous behaviour. This family of elements is also known as the lithium family after its leading element.

<span class="mw-page-title-main">Caesium</span> Chemical element, symbol Cs and atomic number 55

Caesium is a chemical element; it has symbol Cs and atomic number 55. It is a soft, silvery-golden alkali metal with a melting point of 28.5 °C, which makes it one of only five elemental metals that are liquid at or near room temperature. Caesium has physical and chemical properties similar to those of rubidium and potassium. It is pyrophoric and reacts with water even at −116 °C (−177 °F). It is the least electronegative element, with a value of 0.79 on the Pauling scale. It has only one stable isotope, caesium-133. Caesium is mined mostly from pollucite. Caesium-137, a fission product, is extracted from waste produced by nuclear reactors. It has the largest atomic radius of all elements whose radii have been measured or calculated, at about 260 picometers.

<span class="mw-page-title-main">Francium</span> Chemical element, symbol Fr and atomic number 87

Francium is a chemical element; it has symbol Fr and atomic number 87. It is extremely radioactive; its most stable isotope, francium-223, has a half-life of only 22 minutes. It is the second-most electropositive element, behind only caesium, and is the second rarest naturally occurring element. Francium's isotopes decay quickly into astatine, radium, and radon. The electronic structure of a francium atom is [Rn] 7s1; thus, the element is classed as an alkali metal.

<span class="mw-page-title-main">Thallium</span> Chemical element, symbol Tl and atomic number 81

Thallium is a chemical element; it has symbol Tl and atomic number 81. It is a gray post-transition metal that is not found free in nature. When isolated, thallium resembles tin, but discolors when exposed to air. Chemists William Crookes and Claude-Auguste Lamy discovered thallium independently in 1861, in residues of sulfuric acid production. Both used the newly developed method of flame spectroscopy, in which thallium produces a notable green spectral line. Thallium, from Greek θαλλός, thallós, meaning "green shoot" or "twig", was named by Crookes. It was isolated by both Lamy and Crookes in 1862; Lamy by electrolysis, and Crookes by precipitation and melting of the resultant powder. Crookes exhibited it as a powder precipitated by zinc at the international exhibition, which opened on 1 May that year.

A period 6 element is one of the chemical elements in the sixth row (or period) of the periodic table of the chemical elements, including the lanthanides. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behaviour of the elements as their atomic number increases: a new row is begun when chemical behaviour begins to repeat, meaning that elements with similar behaviour fall into the same vertical columns. The sixth period contains 32 elements, tied for the most with period 7, beginning with caesium and ending with radon. Lead is currently the last stable element; all subsequent elements are radioactive. For bismuth, however, its only primordial isotope, 209Bi, has a half-life of more than 1019 years, over a billion times longer than the current age of the universe. As a rule, period 6 elements fill their 6s shells first, then their 4f, 5d, and 6p shells, in that order; however, there are exceptions, such as gold.

<span class="mw-page-title-main">Lepidolite</span> Light micas with substantial lithium

Lepidolite is a lilac-gray or rose-colored member of the mica group of minerals with chemical formula K(Li,Al)3(Al,Si,Rb)4O10(F,OH)2. It is the most abundant lithium-bearing mineral and is a secondary source of this metal. It is the major source of the alkali metal rubidium.

<span class="mw-page-title-main">Caesium fluoride</span> Chemical compound

Caesium fluoride or cesium fluoride is an inorganic compound with the formula CsF and it is a hygroscopic white salt. Caesium fluoride can be used in organic synthesis as a source of the fluoride anion. Caesium also has the highest electropositivity of all known elements and fluorine has the highest electronegativity of all known elements.

A flame test is relatively quick test for the presence of some elements in a sample. The technique is archaic and of questionable reliability, but once was a component of qualitative inorganic analysis. The phenomenon is related to pyrotechnics and atomic emission spectroscopy. The color of the flames is understood through the principles of atomic electron transition and photoemission, where varying elements require distinct energy levels (photons) for electron transitions.

<span class="mw-page-title-main">Caesium chloride</span> Chemical compound

Caesium chloride or cesium chloride is the inorganic compound with the formula CsCl. This colorless salt is an important source of caesium ions in a variety of niche applications. Its crystal structure forms a major structural type where each caesium ion is coordinated by 8 chloride ions. Caesium chloride dissolves in water. CsCl changes to NaCl structure on heating. Caesium chloride occurs naturally as impurities in carnallite, sylvite and kainite. Less than 20 tonnes of CsCl is produced annually worldwide, mostly from a caesium-bearing mineral pollucite.

The alkaline earth metal strontium (38Sr) has four stable, naturally occurring isotopes: 84Sr (0.56%), 86Sr (9.86%), 87Sr (7.0%) and 88Sr (82.58%). Its standard atomic weight is 87.62(1).

Rubidium (37Rb) has 36 isotopes, with naturally occurring rubidium being composed of just two isotopes; 85Rb (72.2%) and the radioactive 87Rb (27.8%).

<span class="mw-page-title-main">Caesium perchlorate</span> Chemical compound

Caesium perchlorate or cesium perchlorate (CsClO4), is a perchlorate of caesium. It forms white crystals, which are sparingly soluble in cold water and ethanol. It dissolves more easily in hot water.

<span class="mw-page-title-main">Germane</span> Chemical compound

Germane is the chemical compound with the formula GeH4, and the germanium analogue of methane. It is the simplest germanium hydride and one of the most useful compounds of germanium. Like the related compounds silane and methane, germane is tetrahedral. It burns in air to produce GeO2 and water. Germane is a group 14 hydride.

<span class="mw-page-title-main">Caesium-137</span> Radioactive isotope of caesium

Caesium-137, cesium-137 (US), or radiocaesium, is a radioactive isotope of caesium that is formed as one of the more common fission products by the nuclear fission of uranium-235 and other fissionable isotopes in nuclear reactors and nuclear weapons. Trace quantities also originate from spontaneous fission of uranium-238. It is among the most problematic of the short-to-medium-lifetime fission products. Caesium-137 has a relatively low boiling point of 671 °C (1,240 °F) and easily becomes volatile when released suddenly at high temperature, as in the case of the Chernobyl nuclear accident and with atomic explosions, and can travel very long distances in the air. After being deposited onto the soil as radioactive fallout, it moves and spreads easily in the environment because of the high water solubility of caesium's most common chemical compounds, which are salts. Caesium-137 was discovered by Glenn T. Seaborg and Margaret Melhase.

<span class="mw-page-title-main">Pollucite</span> Zeolite mineral

Pollucite is a zeolite mineral with the formula (Cs,Na)2Al2Si4O12·2H2O with iron, calcium, rubidium and potassium as common substituting elements. It is important as a significant ore of caesium and sometimes rubidium. It forms a solid solution series with analcime. It crystallizes in the isometric-hexoctahedral crystal system as colorless, white, gray, or rarely pink and blue masses. Well-formed crystals are rare. It has a Mohs hardness of 6.5 and a specific gravity of 2.9. It has a brittle fracture and no cleavage.

<span class="mw-page-title-main">Rubidium chloride</span> Chemical compound

Rubidium chloride is the chemical compound with the formula RbCl. This alkali metal halide salt is composed of rubidium and chlorine, and finds diverse uses ranging from electrochemistry to molecular biology.

<span class="mw-page-title-main">Caesium chromate</span> Chemical compound

Caesium chromate or cesium chromate is an inorganic compound with the formula Cs2CrO4. It is a yellow crystalline solid that is the caesium salt of chromic acid, and it crystallises in the orthorhombic system.

<span class="mw-page-title-main">Thallium(I) chloride</span> Chemical compound

Thallium(I) chloride, also known as thallous chloride, is a chemical compound with the formula TlCl. This colourless salt is an intermediate in the isolation of thallium from its ores. Typically, an acidic solution of thallium(I) sulfate is treated with hydrochloric acid to precipitate insoluble thallium(I) chloride. This solid crystallizes in the caesium chloride motif.

<span class="mw-page-title-main">Robert Bunsen</span> German chemist (1811–1899)

Robert Wilhelm Eberhard Bunsen was a German chemist. He investigated emission spectra of heated elements, and discovered caesium and rubidium with the physicist Gustav Kirchhoff. The Bunsen–Kirchhoff Award for spectroscopy is named after Bunsen and Kirchhoff.

<span class="mw-page-title-main">Rubidium azide</span> Chemical compound

Rubidium azide is an inorganic compound with the formula RbN3. It is the rubidium salt of the hydrazoic acid HN3. Like most azides, it is explosive.

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. 1 2 3 Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN   978-1-62708-155-9.
  4. 1 2 Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.122. ISBN   1-4398-5511-0.
  5. ↑ 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.
  6. ↑ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN   0-8493-0464-4.
  7. ↑ 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.
  8. ↑ 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.
  9. ↑ "Rubidium (Rb) | AMERICAN ELEMENTS ®". American Elements: The Materials Science Company. Retrieved 2024-03-27.
  10. 1 2 Ohly, Julius (1910). "Rubidium". Analysis, detection and commercial value of the rare metals. Mining Science Pub. Co.
  11. ↑ Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (1985). "Vergleichende Übersicht über die Gruppe der Alkalimetalle". Lehrbuch der Anorganischen Chemie (in German) (91–100 ed.). Walter de Gruyter. pp. 953–955. ISBN   978-3-11-007511-3.
  12. ↑ Moore, John W; Stanitski, Conrad L; Jurs, Peter C (2009). Principles of Chemistry: The Molecular Science. Cengage Learning. p. 259. ISBN   978-0-495-39079-4.
  13. ↑ Smart, Lesley; Moore, Elaine (1995). "RbAg4I5". Solid state chemistry: an introduction . CRC Press. pp.  176–177. ISBN   978-0-7487-4068-0.
  14. ↑ 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.
  15. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN   978-0-08-037941-8.
  16. 1 2 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
  17. ↑ 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.
  18. ↑ 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.
  19. ↑ "Universal Nuclide Chart" . nucleonica. Archived from the original on 2017-02-19. Retrieved 2017-01-03.
  20. ↑ 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.
  21. ↑ Attendorn, H.-G.; Bowen, Robert (1988). "Rubidium-Strontium Dating". Isotopes in the Earth Sciences. Springer. pp. 162–165. ISBN   978-0-412-53710-3.
  22. ↑ Walther, John Victor (2009) [1988]. "Rubidium-Strontium Systematics". Essentials of geochemistry. Jones & Bartlett Learning. pp. 383–385. ISBN   978-0-7637-5922-3.
  23. 1 2 3 4 5 Butterman, William C.; Brooks, William E.; Reese, Robert G. Jr. (2003). "Mineral Commodity Profile: Rubidium" (PDF). United States Geological Survey. Retrieved 2010-12-04.
  24. ↑ 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.
  25. ↑ 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.
  26. ↑ 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.
  27. ↑ William A. Hart |title=The Chemistry of Lithium, Sodium, Potassium, Rubidium, Caesium, and Francium |page=371
  28. ↑ McSween Jr., Harry Y; Huss, Gary R (2010). Cosmochemistry. Cambridge University Press. p. 224. ISBN   978-0-521-87862-3.
  29. ↑ 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.
  30. ↑ bulletin 585. United States. Bureau of Mines. 1995.
  31. ↑ "Cesium and Rubidium Hit Market". Chemical & Engineering News. 37 (22): 50–56. 1959. doi:10.1021/cen-v037n022.p050.
  32. 1 2 3 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.
  33. 1 2 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.
  34. ↑ Ritter, Stephen K. (2003). "C&EN: It's Elemental: The Periodic Table – Cesium". American Chemical Society. Retrieved 2010-02-25.
  35. ↑ Zsigmondy, Richard (2007). Colloids and the Ultra Microscope. Read books. p. 69. ISBN   978-1-4067-5938-9 . Retrieved 2010-09-26.
  36. ↑ 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.
  37. ↑ Lewis, G. M. (1952). "The natural radioactivity of rubidium". Philosophical Magazine. Series 7. 43 (345): 1070–1074. doi:10.1080/14786441008520248.
  38. ↑ Campbell, N. R.; Wood, A. (1908). "The Radioactivity of Rubidium". Proceedings of the Cambridge Philosophical Society. 14: 15.
  39. ↑ Butterman, W. C.; Reese, R. G. Jr. "Mineral Commodity Profiles Rubidium" (PDF). United States Geological Survey. Retrieved 2010-10-13.
  40. ↑ "Press Release: The 2001 Nobel Prize in Physics" . Retrieved 2010-02-01.
  41. ↑ 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 .
  42. ↑ 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.
  43. ↑ Boikess, Robert S; Edelson, Edward (1981). Chemical principles. Harper & Row. p. 193. ISBN   978-0-06-040808-4.
  44. ↑ 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.
  45. ↑ 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.
  46. ↑ 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.
  47. ↑ 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.
  48. ↑ "Neutron spin filters based on polarized helium-3". NIST Center for Neutron Research 2002 Annual Report. Retrieved 2008-01-11.
  49. ↑ Eidson, John C (2006-04-11). "GPS". Measurement, control, and communication using IEEE 1588. Springer. p. 32. ISBN   978-1-84628-250-8.
  50. ↑ King, Tim; Newson, Dave (1999-07-31). "Rubidium and crystal oscillators". Data network engineering. Springer. p. 300. ISBN   978-0-7923-8594-3.
  51. ↑ Marton, L. (1977-01-01). "Rubidium Vapor Cell". Advances in electronics and electron physics. Academic Press. ISBN   978-0-12-014644-4.
  52. ↑ Mittal (2009). Introduction To Nuclear And Particle Physics. Prentice-Hall Of India Pvt. Limited. p. 274. ISBN   978-81-203-3610-0.
  53. 1 2 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.
  54. ↑ 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.
  55. ↑ Jadvar, H.; Anthony Parker, J. (2005). "Rubidium-82". Clinical PET and PET/CT. Springer. p. 59. ISBN   978-1-85233-838-1.
  56. 1 2 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.
  57. ↑ 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.
  58. ↑ 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.
  59. ↑ Lake, James A. (2006). Textbook of Integrative Mental Health Care. New York: Thieme Medical Publishers. pp. 164–165. ISBN   978-1-58890-299-3.
  60. ↑ 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.
  61. ↑ "Rubidium 276332". Sigma-Aldrich.
  62. ↑ Martel, Bernard; Cassidy, Keith (2004-07-01). "Rubidium". Chemical risk analysis: a practical handbook. Butterworth-Heinemann. p. 215. ISBN   978-1-903996-65-2.
  63. ↑ 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.
  64. ↑ 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.
  65. ↑ 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.
  66. ↑ 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

This page is based on this Wikipedia article
Text is available under the CC BY-SA 4.0 license; additional terms may apply.
Images, videos and audio are available under their respective licenses.