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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 states−1, +1 (a strongly basic oxide)
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[5]
Molar magnetic susceptibility+17.0×10−6 cm3/mol (303 K)[6]
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[7] 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 (Template:Pron-en roo-BID-ee-əm) is a chemical element with the symbol Rb and atomic number 37. Rubidium is a soft, silvery-white metallic element of the alkali metal group.

Elemental rubidium is very soft and highly reactive, with properties similar to other elements in group 1, such as very rapid oxidation in air. Its compounds have 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.

Rubidium is not known to be necessary for any living organisms. However, like caesium, rubidium ions are handled by living organisms in a manner similar to potassium ions: it is actively taken up by plants and by living animal cells.

Rubidium has one stable isotope,85Rb. The isotope 87Rb which composes almost 28% of naturally occurring rubidium is slightly radioactive, with a half-life of 49 billion years—more than three times longer than the estimated age of the universe.

Characteristics

Rubidium is the second most electropositive of the non-radioactive alkali elements and melts at a temperature of 39.3 °C (102.7 °F). Like other group 1 elements, this metal reacts violently with water. In common 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 liberates. Rubidium has also been reported to ignite spontaneously in air. Like other alkali metals, it forms amalgams with mercury and it can form alloys with gold, caesium, sodium, and potassium. The element and its ions gives a reddish-violet color to a flame. It was named after two strong emission lines in the dark red area of the spectrum.

As a symmetrical effect of rubidium metal's high reactivity toward oxidation and tendency to subsequent formation of the rubidium cation Rb+, this cation, once formed, is very stable, and is normally unreactive toward further oxidative or reductive chemical reactions.

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 spectroscopically

Rubidium (Latin: [rubidus] Error: {{Lang}}: text has italic markup (help), deepest red) was discovered in 1861 by Robert Bunsen and Gustav Kirchhoff in the mineral lepidolite through the use of a spectroscope.[8] Processing 150 kg of lepidolite yielded only a few grams for analysis. Rubidium metal was first produced by the reduction of rubidium chloride with potassium by Bunsen.[8][9]

The first large scale isolation of caesium compounds, performed from 44,000 liters of mineral water by Bunsen and Kirchhoff, yielded, besides 7.3 grams of caesium chloride, also 9.2 grams of rubidium chloride.[8]

Occurrence

Rubidium is about the twenty-third most abundant element in the Earth's crust, roughly as abundant as zinc and rather more common than copper.[10] It occurs naturally in the minerals leucite, pollucite, carnallite and zinnwaldite, which contain up to 1% of its oxide. Lepidolite contains between 0.3% and 3.5% rubidium and this is the commercial source of the element.[11] Some potassium minerals and potassium chlorides also contain the element in commercially significant amounts. One notable source is also in the extensive deposits of pollucite at Bernic Lake, Manitoba (also a source of the related element caesium). The caesium mineral pollucite found on the Italian island Elba contains small crystals of the mineral rubicline ((Rb,K)AlSi3O8) with a rubidium content of 17.5 %.[12]

Rubidium metal can be produced by reducing rubidium chloride with calcium among other methods. In 1997, the cost of this metal in small quantities was about US$25/gram.

Isotopes

Main article: Isotopes of rubidium

There are 26 isotopes of rubidium known with naturally occurring rubidium being composed of just two isotopes; 85Rb (72.2%) and the radioactive 87Rb (27.8%).[13] Natural rubidium is radioactive with specific activity of about 670 Bq/g, enough to expose a photographic film in approximately 30 to 60 days.

Rubidium-87 has a half-life of 4.88×1010 years. It readily substitutes for potassium in minerals, and is therefore fairly widespread. Rb has been used extensively in dating rocks; 87Rb decays to stable 87Sr by emission of a negative beta particle. During fractional crystallization, Sr tends to become concentrated in plagioclase, leaving Rb in the liquid phase. Hence, the Rb/Sr ratio in residual magma may increase over time, resulting in rocks with increasing Rb/Sr ratios with increasing differentiation. Highest ratios (10 or higher) occur in pegmatites. If the initial amount of Sr is known or can be extrapolated, the age can be determined by measurement of the Rb and Sr concentrations and 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 for a more detailed discussion.[14][15]

Uses and applications

Rubidium had minimal industrial use before the 1930s. Since then, the most important use for rubidium historically has been in research and development, primarily in chemical and electronic applications. In 1995, rubidium-87 was used to make a Bose-Einstein condensate[16], for which the discoverers won the 2001 Nobel Prize in Physics[17]. Rubidium is easily ionized, so it has been considered for use in ion engines for space vehicles (but caesium and xenon are more efficient for this purpose).

Rubidium compounds are sometimes used in fireworks to give them a purple color.[18] Rubidium has also been considered for use in a thermoelectric generator using the magnetohydrodynamic principle, where rubidium ions are formed by heat at high temperature and passed through a magnetic field. 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.

Rubidium has been used for polarizing 3He (that is, producing volumes of magnetized 3He gas, with the nuclear spins aligned toward a particular direction in space, rather than randomly). Rubidium vapor is optically pumped by a laser and the polarized Rb polarizes 3He by the hyperfine interaction.[19] Spin-polarized 3He cells are becoming popular for neutron polarization measurements and for producing polarized neutron beams for other purposes.[20]

Rubidium is the primary compound used in secondary frequency references (rubidium oscillators) to maintain frequency accuracy in cell site transmitters and other electronic transmitting, networking and test equipment. Rubidium references are often used with GPS to produce a "primary frequency standard" that has greater accuracy but is less expensive than caesium standards. Rubidium references such as the LPRO series from Datum were mass-produced for the Telecom industry. The general life expectancy is 10 years or better for most designs.

Other potential or current uses of rubidium include a working fluid in vapor turbines, a getter in vacuum tubes,a photocell component, The resonant element in atomic clocks due to the hyperfine structure of rubidium's energy levels, an ingredient in special types of glass, the production of superoxide by burning in oxygen, The study of potassium ion channels in biology, locating of brain tumors due to its slight radioactivity.[10], and as the vapor to make atomic magnetometers (87Rb is currently being used, with other alkali metals, in the development of spin-exchange relaxation-free (SERF) magnetometers)[21]

Compounds

See also: Category:Rubidium compounds

Rubidium chloride is probably the most-used rubidium compound; it is used in biochemistry to induce cells to take up DNA, and as a biomarker since it is readily taken up to replace potassium, and does not normally occur in living organisms. Rubidium hydroxide is the starting material for most rubidium-based chemical processes; rubidium carbonate is used in some optical glasses.

Rubidium has a number of oxides, including Rb6O and Rb9O2 which form if rubidium metal is exposed to air; the final product of reacting with oxygen is the superoxide RbO2. Rubidium forms salts with most anions. Some common rubidium compounds are rubidium chloride (RbCl), rubidium monoxide (Rb2O) and rubidium copper sulfate Rb2SO4·CuSO4·6H2O.RbAg4I5 has the highest room temperature conductivity of any known ionic crystal. This property could be useful in thin film batteries and in other applications.[22][23]

Precautions

Rubidium reacts violently with water and can cause fires. To ensure health, safety and purity, this element must be kept under a dry mineral oil, and in practice is usually sealed in glass ampoules in an inert atmosphere. Rubidium forms peroxides on exposure to even air diffusing into oil, and is thus subject to some of the same peroxide precautions as storage of metallic potassium.

Biological effects

Rubidium, like sodium and potassium, is almost always in its +1 oxidation state when dissolved in water, and this includes all biological systems. 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). The ions are not particularly toxic, and are relatively quickly removed in the sweat and urine. As a result of changes in the blood brain barrier in brain tumors, rubidium collects more in brain tumors than normal brain tissue, allowing short-lived radioisotopes of rubidium to be used in nuclear medicine to locate and image brain tumors.

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, 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. ^ a b c Kirchhoff,, G.; Bunsen, R. (1861). "Chemische Analyse durch Spectralbeobachtungen". Annalen der Physik und Chemie. 189 (7): 337–381. doi:10.1002/andp.18611890702.{{cite journal}}: CS1 maint: extra punctuation (link)
  9. ^ Weeks, Mary Elvira (1932). "The discovery of the elements. XIII. Some spectroscopic discoveries". Journal of Chemical Education. 9 (8): 1413–1434. doi:10.1021/ed009p1413.
  10. ^ a b Chemical Olympics. Rubidium
  11. ^ Wise, M. A. (1995). "Trace element chemistry of lithium-rich micas from rare-element granitic pegmatites". Mineralogy and Petrology. 55 (13): 203–215. doi:10.1007/BF01162588.
  12. ^ 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.
  13. ^ Audi, Georges (2003). "The NUBASE Evaluation of Nuclear and Decay Properties". Nuclear Physics A. 729. Atomic Mass Data Center: 3–128. doi:10.1016/j.nuclphysa.2003.11.001.
  14. ^ Attendorn, H. -G.; Bowen, Robert (1988). "Rubidium-Strontium Dating". Isotopes in the Earth Sciences. Springer. pp. 162–165. ISBN 9780412537103.
  15. ^ Walther, John Victor (1988 2009). "Rubidium-Strontium Systematics". Essentials of geochemistry. Jones & Bartlett Learning. pp. 383–385. ISBN 9780763759223. {{cite book}}: Check date values in: |year= (help)
  16. ^ "Press Release: The 2001 Nobel Prize in Physics". Retrieved 2010-02-01.
  17. ^ Levi, Barbara Goss (2001). "Cornell, Ketterle, and Wieman Share Nobel Prize for Bose-Einstein Condensates". Search & Discovery. Physics Today online. Retrieved 2008-01-26.
  18. ^ Koch, E.-C. (2002). "Special Materials in Pyrotechnics, Part II: Application of Caesium and Rubidium Compounds in Pyrotechnics". Journal Pyrotechnics. 15: 9–24. (Abstract).
  19. ^ Gentile, T. R.; Chen, W. C.; Jones, G. L.; Babcock, E.; Walker, T. G. "Polarized 3He spin filters for slow neutron physics" (PDF). Journal of Research of the National Institute of Standards and Technology. 100: 299–304.
  20. ^ "Neutron spin filters based on polarized helium-3". NIST Center for Neutron Research 2002 Annual Report. Retrieved 2008-01-11.
  21. ^ Li, Zhimin; Wakai, Ronald T.; Walker, Thad G. (2006). "Parametric modulation of an atomic magnetometer". Applied Physics Letters. 89: 134105. doi:10.1063/1.2357553.
  22. ^ Smart, Lesley (1995). "RbAg4I5". Solid state chemistry: an introduction. CRC Press. pp. 176–177. ISBN 9780748740680. {{cite book}}: Unknown parameter |coauthor= ignored (|author= suggested) (help)
  23. ^ Bradley, J. N. (1967). "Relationship of structure and ionic mobility in solid MAg4I5". Trans. Faraday Soc. 63: 2516. doi:10.1039/TF9676302516. {{cite journal}}: Unknown parameter |coauthor= ignored (|author= suggested) (help)

Further reading

  • Louis Meites, Handbook of Analytical Chemistry (New York: McGraw-Hill Book Company, 1963)
  • Daniel A. Steck. "Rubidium-87 D Line Data" (PDF). Los Alamos National Laboratory (technical report LA-UR-03-8638).

External links

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