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Osmium
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For other uses, see Osmium (disambiguation).
Osmium, 76Os
General properties
Pronunciation
/ˈɒzmiəm/ (OZ-mee-əm)
Appearance
silvery, blue cast
Standard atomic weight (Ar, standard)
7002190230000000000♠190.23(3)[1]
Osmium 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
Ru
↑
Os
↓
Hs
rhenium ← osmium → iridium
Atomic number (Z)
76
Group
group 8
Period
period 6
Element category
transition metal
Block
d-block
Electron configuration
[Xe] 4f14 5d6 6s2
Electrons per shell
2, 8, 18, 32, 14, 2
Physical properties
Phase at STP
solid
Melting point
3306 K (3033 °C, 5491 °F)
Boiling point
5285 K (5012 °C, 9054 °F)
Density (near r.t.)
22.59 g/cm3
when liquid (at m.p.)
20 g/cm3
Heat of fusion
31 kJ/mol
Heat of vaporization
378 kJ/mol
Molar heat capacity
24.7 J/(mol·K)
Vapor pressure
P (Pa)
1
10
100
1 k
10 k
100 k
at T (K)
3160 3423 3751 4148 4638 5256
Atomic properties
Oxidation states
8, 7, 6, 5, 4, 3, 2, 1, 0, −1, −2, −4 (a mildly acidic oxide)
Electronegativity
Pauling scale: 2.2
Ionization energies
1st: 840 kJ/mol
2nd: 1600 kJ/mol
Atomic radius
empirical: 135 pm
Covalent radius
144±4 pm
Spectral lines
Miscellanea
Crystal structure
hexagonal close-packed (hcp)
Speed of sound thin rod
4940 m/s (at 20 °C)
Thermal expansion
5.1 µm/(m·K) (at 25 °C)
Thermal conductivity
87.6 W/(m·K)
Electrical resistivity
81.2 nΩ·m (at 0 °C)
Magnetic ordering
paramagnetic[2]
Magnetic susceptibility
+9.9·10−6 cm3/mol (298 K)[3]
Shear modulus
222 GPa
Bulk modulus
462 GPa
Poisson ratio
0.25
Mohs hardness
7.0
Brinell hardness
3490–4000 MPa
CAS Number
7440-04-2
History
Discovery and first isolation
Smithson Tennant (1803)
Main isotopes of osmium
Isotope
Abundance
Half-life (t1/2)
Decay mode
Product
184Os
0.02% stable
185Os
syn 93.6 d ε 185Re
186Os
1.59% 2.0×1015 y α 182W
187Os
1.96% stable
188Os
13.24% stable
189Os
16.15% stable
190Os
26.26% stable
191Os
syn 15.4 d β− 191Ir
192Os
40.78% stable
193Os
syn 30.11 d β− 193Ir
194Os
syn 6 y β− 194Ir
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Osmium (from Greek ὀσμή osme, "smell") is a chemical element with symbol Os and atomic number 76. It is a hard, brittle, bluish-white transition metal in the platinum group that is found as a trace element in alloys, mostly in platinum ores. Osmium is the densest naturally occurring element, with a density of 7004225900000000000♠22.59 g/cm3. Manufacturers use its alloys with platinum, iridium, and other platinum-group metals to make fountain pen nib tipping, electrical contacts, and in other applications that require extreme durability and hardness.[4]
Contents
[hide]
1 Characteristics
1.1 Physical properties
1.2 Chemical properties
1.3 Isotopes
2 History
3 Occurrence
4 Production
5 Applications
6 Precautions
7 Price
8 References
9 External links
Characteristics[edit]
Physical properties[edit]
Osmium, remelted pellet
Osmium has a blue-gray tint and is the densest stable element, approximately twice the density of lead[5] and slightly denser than iridium.[6] Calculations of density from the X-ray diffraction data may produce the most reliable data for these elements, giving a value of 7004225620000000000♠22.562±0.009 g/cm3 for iridium versus 7004225870000000000♠22.587±0.009 g/cm3 for osmium.[7]
Osmium is a hard but brittle metal that remains lustrous even at high temperatures. It has a very low compressibility. Correspondingly, its bulk modulus is extremely high, reported between 7002395000000000000♠395 and 7011462000000000000♠462 GPa, which rivals that of diamond (7011443000000000000♠443 GPa). The hardness of osmium is moderately high at 7009400000000000000♠4 GPa.[8][9][10] Because of its hardness, brittleness, low vapor pressure (the lowest of the platinum-group metals), and very high melting point (the fourth highest of all elements, after only carbon, tungsten, and rhenium), solid osmium is difficult to machine, form or work.
Chemical properties[edit]
See also: Category:Osmium compounds
Oxidation states of osmium
−2 Na
2[Os(CO)
4]
−1 Na
2[Os
4(CO)
13]
0 Os
3(CO)
12
+1 OsI
+2 OsI
2
+3 OsBr
3
+4 OsO
2, OsCl
4
+5 OsF
5
+6 OsF
6
+7 OsOF
5
+8 OsO
4, Os(NCH3)
4
Osmium forms compounds with oxidation states ranging from −2 to +8. The most common oxidation states are +2, +3, +4, and +8. The +8 oxidation state is notable for being the highest attained by any chemical element aside from iridium's +9[11] and is encountered only in xenon,[12][13] ruthenium,[14] hassium,[15] and iridium.[16] The oxidation states −1 and −2 represented by the two reactive compounds Na
2[Os
4(CO)
13] and Na
2[Os(CO)
4] are used in the synthesis of osmium cluster compounds.[17][18]
The most common compound exhibiting the +8 oxidation state is osmium tetroxide. This toxic compound is formed when powdered osmium is exposed to air. It is a very volatile, water-soluble, pale yellow, crystalline solid with a strong smell. Osmium powder has the characteristic smell of osmium tetroxide.[19] Osmium tetroxide forms red osmates OsO
4(OH)2−
2 upon reaction with a base. With ammonia, it forms the nitrido-osmates OsO
3N−
.[20][21][22] Osmium tetroxide boils at 130 °C and is a powerful oxidizing agent. By contrast, osmium dioxide (OsO2) is black, non-volatile, and much less reactive and toxic.
Only two osmium compounds have major applications: osmium tetroxide for staining tissue in electron microscopy and for the oxidation of alkenes in organic synthesis, and the non-volatile osmates for organic oxidation reactions.[23]
Osmium pentafluoride (OsF5) is known, but osmium trifluoride (OsF3) has not yet been synthesized. The lower oxidation states are stabilized by the larger halogens, so that the trichloride, tribromide, triiodide, and even diiodide are known. The oxidation state +1 is known only for osmium iodide (OsI), whereas several carbonyl complexes of osmium, such as triosmium dodecacarbonyl (Os
3(CO)
12), represent oxidation state 0.[20][21][24][25]
In general, the lower oxidation states of osmium are stabilized by ligands that are good σ-donors (such as amines) and π-acceptors (heterocycles containing nitrogen). The higher oxidation states are stabilized by strong σ- and π-donors, such as O2−
and N3−
.[26]
Despite its broad range of compounds in numerous oxidation states, osmium in bulk form at ordinary temperatures and pressures resists attack by all acids and alkalis, including aqua regia.[27]
Isotopes[edit]
Main article: Isotopes of osmium
Osmium has seven naturally occurring isotopes, six of which are stable: 184
Os, 187
Os, 188
Os, 189
Os, 190
Os, and (most abundant) 192
Os. 186
Os undergoes alpha decay with such a long half-life (2.0±1.1)×1015 years, approximately 140 000 times the age of the universe, that for practical purposes it can be considered stable. Alpha decay is predicted for all seven naturally occurring isotopes, but it has been observed only for 186
Os, presumably due to very long half-lives. It is predicted that 184
Os and 192
Os can undergo double beta decay but this radioactivity has not been observed yet.[28]
187
Os is the daughter of 187
Re (half-life 7018143902655999999♠4.56×1010 years) and is used extensively in dating terrestrial as well as meteoric rocks (see rhenium-osmium dating). It has also been used to measure the intensity of continental weathering over geologic time and to fix minimum ages for stabilization of the mantle roots of continental cratons. This decay is a reason why rhenium-rich minerals are abnormally rich in 187
Os.[29] However, the most notable application of Os isotopes in geology has been in conjunction with the abundance of iridium, to characterise the layer of shocked quartz along the Cretaceous–Paleogene boundary that marks the extinction of the dinosaurs 66 million years ago.[30]
History[edit]
Osmium was discovered in 1803 by Smithson Tennant and William Hyde Wollaston in London, England.[31] The discovery of osmium is intertwined with that of platinum and the other metals of the platinum group. Platinum reached Europe as platina ("small silver"), first encountered in the late 17th century in silver mines around the Chocó Department, in Colombia.[32] The discovery that this metal was not an alloy, but a distinct new element, was published in 1748.[33] Chemists who studied platinum dissolved it in aqua regia (a mixture of hydrochloric and nitric acids) to create soluble salts. They always observed a small amount of a dark, insoluble residue.[27] Joseph Louis Proust thought that the residue was graphite.[27] Victor Collet-Descotils, Antoine François, comte de Fourcroy, and Louis Nicolas Vauquelin also observed iridium in the black platinum residue in 1803, but did not obtain enough material for further experiments.[27] Later the two French chemists Antoine-François Fourcroy and Nicolas-Louis Vauquelin identified a metal in a platinum residue they called ‘ptène’.[34]
In 1803, Smithson Tennant analyzed the insoluble residue and concluded that it must contain a new metal. Vauquelin treated the powder alternately with alkali and acids[35] and obtained a volatile new oxide, which he believed was of this new metal—which he named ptene, from the Greek word πτηνος (ptènos) for winged.[36][37] However, Tennant, who had the advantage of a much larger amount of residue, continued his research and identified two previously undiscovered elements in the black residue, iridium and osmium.[27][35] He obtained a yellow solution (probably of cis–[Os(OH)2O4]2−) by reactions with sodium hydroxide at red heat. After acidification he was able to distill the formed OsO4.[36] He named it osmium after Greek osme meaning "a smell", because of the ashy and smoky smell of the volatile osmium tetroxide.[38] Discovery of the new elements was documented in a letter to the Royal Society on June 21, 1804.[27][39]
Uranium and osmium were early successful catalysts in the Haber process, the nitrogen fixation reaction of nitrogen and hydrogen to produce ammonia, giving enough yield to make the process economically successful. At the time, a group at BASF led by Carl Bosch bought most of the world's supply of osmium to use as a catalyst. Shortly thereafter, in 1908, cheaper catalysts based on iron and iron oxides were introduced by the same group for the first pilot plants, removing the need for the expensive and rare osmium.[40]
Nowadays osmium is obtained primarily from the processing of platinum and nickel ores.[41]
Occurrence[edit]
Native platinum containing traces of the other platinum group metals
Osmium is one of the even-numbered elements, which puts it in the upper half of elements commonly found in space. It is, however, the least abundant stable element in Earth's crust, with an average mass fraction of 50 parts per trillion in the continental crust.[42]
Osmium is found in nature as an uncombined element or in natural alloys; especially the iridium–osmium alloys, osmiridium (osmium rich), and iridosmium (iridium rich).[35] In nickel and copper deposits, the platinum group metals occur as sulfides (i.e., (Pt,Pd)S)), tellurides (e.g., PtBiTe), antimonides (e.g., PdSb), and arsenides (e.g., PtAs2); in all these compounds platinum is exchanged by a small amount of iridium and osmium. As with all of the platinum group metals, osmium can be found naturally in alloys with nickel or copper.[43]
Within Earth's crust, osmium, like iridium, is found at highest concentrations in three types of geologic structure: igneous deposits (crustal intrusions from below), impact craters, and deposits reworked from one of the former structures. The largest known primary reserves are in the Bushveld Igneous Complex in South Africa,[44] though the large copper–nickel deposits near Norilsk in Russia, and the Sudbury Basin in Canada are also significant sources of osmium. Smaller reserves can be found in the United States.[44] The alluvial deposits used by pre-Columbian people in the Chocó Department, Colombia are still a source for platinum group metals. The second large alluvial deposit was found in the Ural Mountains, Russia, which is still mined.[41][45]
Production[edit]
Osmium crystals, grown by chemical vapor transport.
Osmium is obtained commercially as a by-product from nickel and copper mining and processing. During electrorefining of copper and nickel, noble metals such as silver, gold and the platinum group metals, together with non-metallic elements such as selenium and tellurium settle to the bottom of the cell as anode mud, which forms the starting material for their extraction.[46][47] Separating the metals requires that they first be brought into solution. Several methods can achieve this, depending on the separation process and the composition of the mixture. Two representative methods are fusion with sodium peroxide followed by dissolution in aqua regia, and dissolution in a mixture of chlorine with hydrochloric acid.[44][48] Osmium, ruthenium, rhodium and iridium can be separated from platinum, gold and base metals by their insolubility in aqua regia, leaving a solid residue. Rhodium can be separated from the residue by treatment with molten sodium bisulfate. The insoluble residue, containing Ru, Os and Ir, is treated with sodium oxide, in which Ir is insoluble, producing water-soluble Ru and Os salts. After oxidation to the volatile oxides, RuO
4 is separated from OsO
4 by precipitation of (NH4)3RuCl6 with ammonium chloride.
After it is dissolved, osmium is separated from the other platinum group metals by distillation or extraction with organic solvents of the volatile osmium tetroxide.[49] The first method is similar to the procedure used by Tennant and Wollaston. Both methods are suitable for industrial scale production. In either case, the product is reduced using hydrogen, yielding the metal as a powder or sponge that can be treated using powder metallurgy techniques.[50]
Neither the producers nor the United States Geological Survey published any production amounts for osmium. In 1971, estimations of the United States production of osmium as a byproduct of copper refining was 2000 troy ounces (62 kg).[51] In 2012, the estimated US import of osmium for consumption was 75 kg.[52]
Applications[edit]
Because of the volatility and extreme toxicity of its oxide, osmium is rarely used in its pure state, but is instead often alloyed with other metals for high-wear applications. Osmium alloys such as osmiridium are very hard and, along with other platinum-group metals, are used in the tips of fountain pens, instrument pivots, and electrical contacts, as they can resist wear from frequent operation. They were also used for the tips of phonograph styli during the late 78 rpm and early "LP" and "45" record era, circa 1945 to 1955. Osmium-alloy tips were significantly more durable than steel and chromium needle points, but wore out far more rapidly than competing, and costlier, sapphire and diamond tips, so they were discontinued.[53]
Osmium tetroxide has been used in fingerprint detection[54] and in staining fatty tissue for optical and electron microscopy. As a strong oxidant, it cross-links lipids mainly by reacting with unsaturated carbon–carbon bonds and thereby both fixes biological membranes in place in tissue samples and simultaneously stains them. Because osmium atoms are extremely electron-dense, osmium staining greatly enhances image contrast in transmission electron microscopy (TEM) studies of biological materials. Those carbon materials have otherwise very weak TEM contrast (see image).[23] Another osmium compound, osmium ferricyanide (OsFeCN), exhibits similar fixing and staining action.[55]
The tetroxide and a related compound potassium osmate are important oxidants for chemical synthesis, despite being very poisonous. For the Sharpless asymmetric dihydroxylation, which uses osmate for the conversion of a double bond into a vicinal diol, Karl Barry Sharpless won the Nobel Prize in Chemistry in 2001.[56][57] OsO4 is very expensive for this use, so KMnO4 is often used instead, even though the yields are less for this cheaper chemical reagent.[58]
In 1898 an Austrian chemist Auer von Welsbach developed the Oslamp with a filament made of osmium, which he introduced commercially in 1902. After only a few years, osmium was replaced by the more stable metal tungsten. Tungsten has the highest melting point among all metals, and its use in light bulbs increases the luminous efficacy and life of incandescent lamps.[36]
The light bulb manufacturer Osram (founded in 1906, when three German companies, Auer-Gesellschaft, AEG and Siemens & Halske, combined their lamp production facilities) derived its name from the elements of osmium and Wolfram (the latter is German for tungsten).[59]
Like palladium, powdered osmium effectively absorbs hydrogen atoms. This could make osmium a potential candidate for a metal-hydride battery electrode. However, osmium is expensive and would react with potassium hydroxide, the most common battery electrolyte.[60]
Osmium has high reflectivity in the ultraviolet range of the electromagnetic spectrum; for example, at 600 Å osmium has a reflectivity twice that of gold.[61] This high reflectivity is desirable in space-based UV spectrometers, which have reduced mirror sizes due to space limitations. Osmium-coated mirrors were flown in several space missions aboard the Space Shuttle, but it soon became clear that the oxygen radicals in the low Earth orbit are abundant enough to significantly deteriorate the osmium layer.[62]
The only known clinical use of osmium is synovectomy in arthritic patients in Scandinavia.[63] It involves the local administration of osmium tetroxide (OsO4), which is a highly toxic compound. The lack of reports of long-term side effects suggest that osmium itself can be biocompatible, though this depends on the osmium compound administered. In 2011, osmium(VI)[64] and osmium(II)[65] compounds were reported to show anticancer activity in vivo, it indicated a promising future for using osmium compounds as anticancer drugs.[66]
The Sharpless dihydroxylation:
RL = largest substituent; RM = medium-sized substituent; RS = smallest substituent
Post-flight appearance of Os, Ag, and Au mirrors from the front (left images) and rear panels of the Space Shuttle. Blackening reveals oxidation due to irradiation by oxygen atoms.[67][68]
Precautions[edit]
Metallic osmium is harmless[69] but finely divided metallic osmium is pyrophoric[51] and reacts with oxygen at room temperature, forming volatile osmium tetroxide. Some osmium compounds are also converted to the tetroxide if oxygen is present.[51] This makes osmium tetroxide the main source of contact with the environment.
Osmium tetroxide is highly volatile and penetrates skin readily, and is very toxic by inhalation, ingestion, and skin contact.[70] Airborne low concentrations of osmium tetroxide vapor can cause lung congestion and skin or eye damage, and should therefore be used in a fume hood.[19] Osmium tetroxide is rapidly reduced to relatively inert compounds by polyunsaturated vegetable oils, such as corn oil.[71]
Price[edit]
Osmium is usually sold as a minimum 99.9% pure powder. Like other precious metals, it is measured by troy weight and by grams. Its price in 2012 was about US$400 per troy ounce (or about $13,000 per kilogram), depending on the quantity, its purity and its supplier.[72][73]
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Jump up ^ Tennant, S. (1804). "On Two Metals, Found in the Black Powder Remaining after the Solution of Platina". Philosophical Transactions of the Royal Society. 94: 411–418. doi:10.1098/rstl.1804.0018. JSTOR 107152.
Jump up ^ Smil, Vaclav (2004). Enriching the Earth: Fritz Haber, Carl Bosch, and the Transformation of World Food Production. MIT Press. pp. 80–86. ISBN 978-0-262-69313-4.
^ Jump up to: a b George, Micheal W. "2006 Minerals Yearbook: Platinum-Group Metals" (PDF). United States Geological Survey USGS. Retrieved 2008-09-16.
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Jump up ^ Xiao, Z.; Laplante, A. R. (2004). "Characterizing and recovering the platinum group minerals—a review". Minerals Engineering. 17 (9–10): 961–979. doi:10.1016/j.mineng.2004.04.001.
^ Jump up to: a b c Seymour, R. J.; O'Farrelly, J. I. (2001). "Platinum-group metals". Kirk Othmer Encyclopedia of Chemical Technology. Wiley. doi:10.1002/0471238961.1612012019052513.a01.pub2.
Jump up ^ "Commodity Report: Platinum-Group Metals" (PDF). United States Geological Survey USGS. Retrieved 2008-09-16.
Jump up ^ George, M. W. (2008). "Platinum-group metals" (PDF). U.S. Geological Survey Mineral Commodity Summaries. USGS Mineral Resources Program.
Jump up ^ George, M. W. 2006 Minerals Yearbook: Platinum-Group Metals (PDF). United States Geological Survey USGS. Retrieved 2008-09-16.
Jump up ^ Renner, H.; Schlamp, G.; Kleinwächter, I.; Drost, E.; et al. (2002). "Platinum group metals and compounds". Ullmann's Encyclopedia of Industrial Chemistry. Wiley. doi:10.1002/14356007.a21_075.
Jump up ^ Gilchrist, Raleigh (1943). "The Platinum Metals". Chemical Reviews. 32 (3): 277–372. doi:10.1021/cr60103a002.
Jump up ^ Hunt, L. B.; Lever, F. M. (1969). "Platinum Metals: A Survey of Productive Resources to industrial Uses" (PDF). Platinum Metals Review. 13 (4): 126–138. Retrieved 2008-10-02.
^ Jump up to: a b c Smith, Ivan C.; Carson, Bonnie L.; Ferguson, Thomas L. (1974). "Osmium: An Appraisal of Environmental Exposure". Environmental Health Perspectives. 8: 201–213. doi:10.2307/3428200. JSTOR 3428200. PMC 1474945  . PMID 4470919.
Jump up ^ "PLATINUM-GROUP METALS" (PDF). USGS. Retrieved 27 May 2013.
Jump up ^ Stephen D. Cramer & Bernard S. Covino, Jr. (2005). ASM Handbook Volume 13B. Corrosion: Materials. ASM International. ISBN 978-0-87170-707-9.
Jump up ^ MacDonell, Herbert L. (1960). "The Use of Hydrogen Fluoride in the Development of Latent Fingerprints Found on Glass Surfaces". The Journal of Criminal Law, Criminology, and Police Science. 51 (4): 465–470. doi:10.2307/1140672. JSTOR 1140672.
Jump up ^ Chadwick, D. (2002). Role of the sarcoplasmic reticulum in smooth muscle. John Wiley and Sons. pp. 259–264. ISBN 0-470-84479-5.
Jump up ^ Kolb, H. C.; Van Nieuwenhze, M. S.; Sharpless, K. B. (1994). "Catalytic Asymmetric Dihydroxylation". Chemical Reviews. 94 (8): 2483–2547. doi:10.1021/cr00032a009.
Jump up ^ Colacot, T. J. (2002). "2001 Nobel Prize in Chemistry" (PDF). Platinum Metals Review. 46 (2): 82–83.
Jump up ^ Osmium tetroxide as a reagent in organic chemistry — Master Organic Chemistry. Masterorganicchemistry.com. Retrieved on 2012-12-07.
Jump up ^ Bowers, B., B. (2001). "Scanning our past from London: the filament lamp and new materials". Proceedings of the IEEE. 89 (3): 413–415. doi:10.1109/5.915382.
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Jump up ^ Torr, Marsha R. (1985). "Osmium coated diffraction grating in the Space Shuttle environment: performance". Applied Optics. 24 (18): 2959. Bibcode:1985ApOpt..24.2959T. doi:10.1364/AO.24.002959. PMID 18223987.
Jump up ^ Gull, T. R.; Herzig, H.; Osantowski, J. F.; Toft, A. R. (1985). "Low earth orbit environmental effects on osmium and related optical thin-film coatings". Applied Optics. 24 (16): 2660. Bibcode:1985ApOpt..24.2660G. doi:10.1364/AO.24.002660. PMID 18223936.
Jump up ^ Sheppeard, H.; D. J. Ward (1980). "Intra-articular osmic acid in rheumatoid arthritis: five years' experience". Rheumatology. 19 (1): 25–29. doi:10.1093/rheumatology/19.1.25. PMID 7361025.
Jump up ^ Lau, T.-C; W.-X. Ni; W.-L. Man; M. T.-W. Cheung; et al. (2011). "Osmium(vi) complexes as a new class of potential anti-cancer agents". Chem. Commun. 47 (7): 2140–2142. doi:10.1039/C0CC04515B.
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Jump up ^ Fu, Ying; Romero, María J.; Habtemariam, Abraha; et al. (2012). "The contrasting chemical reactivity of potent isoelectronic iminopyridine and azopyridine osmium(II) arene anticancer complexes". Chemical Science. 3 (8): 2485–2494. doi:10.1039/C2SC20220D.
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Jump up ^ McLaughlin, A. I. G.; Milton, R.; Perry, Kenneth M. A. (July 1946). "Toxic Manifestations of Osmium Tetroxide". British Journal of Industrial Medicine. 3 (3): 183–186. doi:10.1136/oem.3.3.183. ISSN 0007-1072. PMC 1035752  . PMID 20991177.
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Jump up ^ "How to Handle Osmium Tetroxide". University of California, San Diego. Archived from the original on February 21, 2006. Retrieved 2009-06-02.
Jump up ^ Osmium. Los Alamos National Laboratory's Chemistry Division
Jump up ^ Live Osmium prices. TaxFreeGold.com. Accessed 6 April 2010
External links[edit]
Wikimedia Commons has media related to Osmium.
Look up osmium in Wiktionary, the free dictionary.
Chemistry in its element podcast (MP3) from the Royal Society of Chemistry's Chemistry World: Osmium
Lide, D. R., ed. (2004). CRC Handbook of Chemistry and Physics (84th ed.). CRC Press. ISBN 978-0-8493-0484-2.
Osmium at The Periodic Table of Videos (University of Nottingham)
FLEGENHEIMER, J. (2014). The mystery of the disappearing isotope. Revista Virtual de Química. V. XX. Available at http://www.uff.br/RVQ/index.php/rvq/article/viewFile/660/450
Chisholm, Hugh, ed. (1911). "Osmium". Encyclopædia Britannica. 20 (11th ed.). Cambridge University Press. p. 352.
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Periodic table (Large cells)
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
1
H He
2
Li Be B C N O F Ne
3
Na Mg Al Si P S Cl Ar
4
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
5
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
6
Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
7
Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
Alkali metal Alkaline earth metal Lanthanide Actinide Transition metal Post-transition metal Metalloid Reactive nonmetal Noble gas Unknown
chemical
properties
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Osmium compounds
Os(0)
Os3(CO)12
Os(0,I)
H2Os3(CO)10
Os(I)
OsB
Os(I,II)
Os2B3
Os(II)
OsB2
Organoosmium(II) compounds
Os(C5H5)2
Os(IV)
OsO2
OsCl4
Os(VI)
OsF6
Os(VIII)
OsO4
OsS4
Authority control
LCCN: sh85095926
GND: 4172906-7
NDL: 00568958
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text:
Jelly bean
From Wikipedia, the free encyclopedia
Jump to: navigation, search
For other uses, see Jelly bean (disambiguation).
Jelly Bean
Jelly bean (Jelly Belly brand) flavor and color assortment.
Alternative names
Jelly Belly Beans
Type
Confectionery
Place of origin
United States
Created by
William Schrafft
Main ingredients
Sugar, corn syrup, starch
Cookbook: Jelly Bean Media: Jelly Bean
Jelly beans are small bean-shaped sugar candies with soft candy shells and thick gel interiors. The confection is vended in a wide variety of colors and flavors, and is made primarily of sugar.
Contents
[hide]
1 History
2 Manufacture
3 Slang
4 References
5 External links
History[edit]
It has been claimed that jelly beans were mentioned first during 1861, when Boston confectioner William Schrafft urged people to send his jelly beans to soldiers during the American Civil War. It was not until July 5, 1905, that jelly beans were mentioned in the Chicago Daily News. The advertisement publicized bulk jelly beans sold by volume for nine cents per pound, according to the book The Century in Food: America's Fads and Favorites. Most historians contend that jelly beans were first associated with celebrations of Easter in the United States sometime during the 1930s due to their egg-like shape.[1]

Manufacture[edit]
This section possibly contains original research. Please improve it by verifying the claims made and adding inline citations. Statements consisting only of original research should be removed. (April 2013) (Learn how and when to remove this template message)
The basic ingredients of jelly beans include sugar, tapioca or corn syrup, and pectin or starch. Relatively minor amounts of the emulsifying agent lecithin, anti-foaming agents, an edible wax such as carnauba wax or beeswax, salt, and confectioner's glaze are also included.[2] The ingredients that give each bean its character are also relatively small in proportion and may vary depending on the flavor.
Most jelly beans are sold as an assortment of about eight different flavors, most of them fruit-based. Assortments of "spiced" jellybeans and gumdrops are also available, which include a similar number of spice and mint flavors. The colors of jelly beans often correspond with a fruit and a "spiced" flavor.
Some premium brands, such as Jelly Belly and The Jelly Bean Factory, are available in many different flavors, including berry, tropical fruit, soft drink, popcorn, licorice, and novelty ranges, in addition to the familiar fruit and spice flavors. While these are also sold as assortments, individual flavors can be purchased from distributors.
Slang[edit]
1920 sheet music cover.
In United States slang during the 1910s and early 1920s, a "Jellybean" or "Jelly-Bean" was a young man who dressed stylishly but had little else to recommend him, similar to the older terms dandy and fop. F. Scott Fitzgerald published a story about such a character, The Jelly-Bean, during 1920.[3] In William Faulkner's 1929 novel The Sound and the Fury, Jason complained about his niece Quentin's promiscuity, remarking that even "the town jellybeans" gave her the "go-by".
The song "Jelly Bean (He's a Curbstone Cutie)" was made popular during the 1940s by Phil Harris. It was written by Jimmie Dupre, Sam Rosen, and Joe Verges and published in New Orleans during 1920 by Universal Music Publishers, Inc.
References[edit]
Jump up ^ "Jelly Beans: A Colorful History and Association with Easter". AT&T.
Jump up ^ "How Products are Made – Volumes – Jelly Beans". Gale-Edit. Archived from the original on 2010-05-16. Retrieved 2010-02-19.
Jump up ^ Francis Scott Fitzgerald, Matthew Joseph Bruccoli, Judith Baughman, "The Jelly-Bean", Before Gatsby: the first twenty-six stories, p. 341 CS1 maint: Multiple names: authors list (link)
External links[edit]
Media related to Jelly beans at Wikimedia Commons
Retrieved from "https://en.wikipedia.org/w/index.php?title=Jelly_bean&oldid=838068350"
Categories:
American inventions
Confectionery
Easter food
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values: ஜெல்லிபீன் (இனிப்பு) – Tamil

values: เจลลี่บีน – Thai

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https://tr.wikipedia.org/wiki/Jelibon
Jelibon – Turkish
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tr
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