Bismuth

lead ← bismuth → polonium
Sb
↑
Bi
↓
Uup
Appearance
lustrous silver
General properties
Name, symbol, number bismuth, Bi, 83
Pronunciation /ˈbɪzməθ/ BIZ-məth
Element category post-transition metal
Group, period, block 15, 6, p
Standard atomic weight 208.98040g·mol−1
Electron configuration [Xe] 4f14 5d10 6s2 6p3
Electrons per shell 2, 8, 18, 32, 18, 5 (Image)
Physical properties
Phase solid
Density (near r.t.) 9.78 g·cm−3
Liquid density at m.p. 10.05 g·cm−3
Melting point 544.7 K, 271.5 °C, 520.7 °F
Boiling point 1837 K, 1564 °C, 2847 °F
Heat of fusion 11.30 kJ·mol−1
Heat of vaporization 151 kJ·mol−1
Specific heat capacity (25 °C) 25.52 J·mol−1·K−1
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 941 1041 1165 1325 1538 1835
Atomic properties
Oxidation states 3, 5
(mildly acidic oxide)
Electronegativity 2.02 (Pauling scale)
Ionization energies
(more)		 1st: 703 kJ·mol−1
2nd: 1610 kJ·mol−1
3rd: 2466 kJ·mol−1
Atomic radius 156 pm
Covalent radius 148±4 pm
Van der Waals radius 207 pm
Miscellanea
Crystal structure trigonal[1]
Magnetic ordering diamagnetic
Electrical resistivity (20 °C) 1.29 µΩ·m
Thermal conductivity (300 K) 7.97 W·m−1·K−1
Thermal expansion (25 °C) 13.4 µm·m−1·K−1
Speed of sound (thin rod) (20 °C) 1790 m/s
Young's modulus 32 GPa
Shear modulus 12 GPa
Bulk modulus 31 GPa
Poisson ratio 0.33
Mohs hardness 2.25
Brinell hardness 94.2 MPa
CAS registry number 7440-69-9
Most stable isotopes
Main article: Isotopes of bismuth
iso NA half-life DM DE (MeV) DP
207Bi syn 31.55 y ε, β+ 2.399 207Pb
208Bi syn 368,000 y ε, β+ 2.880 208Pb
209Bi 100% (19 ± 2) ×1018y α 3.14 205Tl
210mBi syn 3.04 ×106y IT 0.271 210Bi

Bismuth (pronounced /ˈbɪzməθ/, BIZ-məth) is a chemical element that has the symbol Bi and atomic number 83. This trivalent poor metal chemically resembles arsenic and antimony. Bismuth is heavy and brittle; it has a silvery white color with a pink tinge owing to the surface oxide. Bismuth is the most naturally diamagnetic of all metals, and only mercury has a lower thermal conductivity. It is generally considered to be the last naturally occurring stable, non-radioactive element on the periodic table, although it is actually slightly radioactive. Its only non-synthetic isotope bismuth-209 decays via alpha decay into thallium-205, with an extremely long half-life of 1.9 × 1019 years.[2]

Bismuth compounds are used in cosmetics, medicines, and in medical procedures. As the toxicity of lead has become more apparent in recent years, alloy uses for bismuth metal as a replacement for lead have become an increasing part of bismuth's commercial importance.

Contents

Characteristics

Bismuth crystal with an iridescent oxide surface
Bismuth crystals

Bismuth is a brittle metal with a white, silver-pink hue, often occurring in its native form with an iridescent oxide tarnish showing many colors from yellow to blue. The spiral stair stepped structure of a bismuth crystal is the result of a higher growth rate around the outside edges than on the inside edges. The variations in the thickness of the oxide layer that forms on the surface of the crystal causes different wavelengths of light to interfere upon reflection, thus displaying a rainbow of colors. When combusted with oxygen, bismuth burns with a blue flame and its oxide forms yellow fumes.[3] Its toxicity is much lower than that of its neighbors in the periodic table such as lead, tin, tellurium, antimony, and polonium.

Although ununpentium is theoretically more diamagnetic, no other metal is verified to be more naturally diamagnetic than bismuth.[3] (Superdiamagnetism is a different physical phenomenon.) Of any metal, it has the second lowest thermal conductivity (after mercury) and the highest Hall coefficient. It has a high electrical resistance.[3] When deposited in sufficiently thin layers on a substrate, bismuth is a semiconductor, rather than a poor metal.[4]

Elemental bismuth is one of very few substances of which the liquid phase is denser than its solid phase (water being the best-known example). Bismuth expands 3.32% on solidification; therefore, it was long an important component of low-melting typesetting alloys, where it compensated for the contraction of the other alloying components.[3]

Though virtually unseen in nature, high-purity bismuth can form distinctive hopper crystals. These colorful laboratory creations are typically sold to collectors. Bismuth is relatively nontoxic and has a low melting point just above 271 °C, so crystals may be grown using a household stove, although the resulting crystals will tend to be lower quality than lab-grown crystals.

Isotopes

While bismuth was traditionally regarded as the element with the heaviest stable isotope, bismuth-209, it had long been suspected to be unstable on theoretical grounds. This was finally demonstrated in 2003 when researchers at the Institut d'Astrophysique Spatiale in Orsay, France, measured the alpha emission half-life of 209Bi to be 1.9 × 1019 years,[5] over a billion times longer than the current estimated age of the universe. Owing to its extraordinarily long half-life, for all presently known medical and industrial applications bismuth can be treated as if it is stable and non-radioactive. The radioactivity is of academic interest, however, because bismuth is one of few elements whose radioactivity was suspected, and indeed theoretically predicted, before being detected in the laboratory.

Creation

Bismuth is unique in that it has the longest half life. Bismuth-209's half life is in fact a lot longer than estimated age of the universe. As such, while it is not technically stable, it is practically stable. It is created in supernovas via the r-process, and in stars via the s-process.

History

Bismuth (New Latin bisemutum from German Wismuth, perhaps from weiße Masse, "white mass") was confused in early times with tin and lead because of its resemblance to those elements. Bismuth has been known since ancient times, and so no one person is credited with its discovery. Agricola, in De Natura Fossilium states that bismuth is a distinct metal in a family of metals including tin and lead in 1546 based on observation of the metals and their physical properties.[6] Claude François Geoffroy demonstrated in 1753 that this metal is distinct from lead and tin.[3]

"Artificial bismuth" was commonly used in place of the actual metal. It was made by hammering tin into thin plates, and cementing them by a mixture of white tartar, saltpeter, and arsenic, stratified in a crucible over an open fire.

Bismuth was also known to the Incas and used (along with the usual copper and tin) in a special bronze alloy for knives.[7]

Occurrence and production

New York prices (2007)[8]
Time Price (USD/lb.)
December 2000 3.85–4.15
November 2002 2.70–3.10
December 2003 2.60–2.90
June 2004 3.65–4.00
September 2005 4.20–4.60
September 2006 4.50–4.75
November 2006 6.00–6.50
December 2006 7.30–7.80
March 2007 9.25–9.75
April 2007 10.50–11.00
June 2007 18.00–19.00
November 2007 13.50–15.00
Bismite mineral
Bismuth output in 2005

In the Earth's crust, bismuth is about twice as abundant as gold. It is not usually economical to mine it as a primary product. Rather, it is usually produced as a byproduct of the processing of other metal ores, especially lead, tungsten (China), tin, copper, and also silver (indirectly) or other metallic elements.

The most important ores of bismuth are bismuthinite and bismite.[3] In 2005, China was the top producer of bismuth with at least 40% of the world share followed by Mexico and Peru, reports the British Geological Survey. Native bismuth is known from Australia, Bolivia, and China.

According to the USGS, world 2006 bismuth mine production was 5,700 tonnes, of which China produced 3,000 tonnes, Mexico 1,180 tonnes, Peru 950 tonnes, and the balance Canada, Kazakhstan and other nations. World 2006 bismuth refinery production was 12,000 tonnes, of which China produced 8,500 tonnes, Mexico 1,180 tonnes, Belgium 800 tonnes, Peru 600 tonnes, Japan 510 tonnes, and the balance Canada and other nations.[9]

For the year 2007, the USGS Minerals Yearbook stated that world bismuth refinery production was of 15,000 tonnes, of which China was responsible for 77%, Mexico 8% and Belgium 5%.[10]

The difference between world bismuth mine production and refinery production reflects bismuth's status as a byproduct metal. Bismuth travels in crude lead bullion (which can contain up to 10% bismuth) through several stages of refining, until it is removed by the Kroll-Betterton process or the Betts process. The Kroll-Betterton process uses a pyrometallurgical separation from molten lead of calcium-magnesium-bismuth drosses containing associated metals (silver, gold, zinc, some lead, copper, tellurium, and arsenic), which are removed by various fluxes and treatments to give high-purity bismuth metal (over 99% Bi). The Betts process takes cast anodes of lead bullion and electrolyzes them in a lead fluorosilicate-hydrofluorosilicic acid electrolyte to yield a pure lead cathode and an anode slime containing bismuth. Bismuth will behave similarly with another of its major metals, copper. Thus world bismuth production from refineries is a more complete and reliable statistic.

According to the Bismuth Advocate News,[8] the price for bismuth metal from year-end 2000 to September 2005 was stuck in a range from $2.60 to $4.15 per lb., but after this period the price started rising rapidly as global bismuth demand as a lead replacement and other uses grew rapidly. New mines in Canada and Vietnam may relieve the shortages, but prices are likely to remain above their previous level for the foreseeable future. The Customer-Input price for bismuth is more oriented to the ultimate consumer; it started at US$39.40 per kilogram ($17.90 per pound) in January 2008 and reached US$35.55 per kg (US$16.15 per lb.) in September 2008.[11]

Recycling

While bismuth is most available today as a byproduct, its sustainability is more dependent on recycling. Bismuth is mostly a byproduct of lead smelting, along with silver, zinc, antimony, and other metals, and also of tungsten production, along with molybdenum and tin, and also of copper production. Recycling bismuth is difficult in many of its end uses, primarily because of scattering. Probably the easiest to recycle would be bismuth-containing fusible alloys in the form of larger objects, then larger soldered objects. Half of the world solder consumption is in electronics (i.e., circuit boards).[12] As the soldered objects get smaller or contain little solder or little bismuth, the recovery gets progressively more difficult and less economic, although solder with a sizable silver content will be more worth recovering. Next in recycling feasibility would be sizeable catalysts with a fair bismuth content, perhaps as bismuth phosphomolybdate, and then bismuth used in galvanizing and as a free-machining metallurgical additive. Finally, the bismuth in the uses where it gets scattered the most, in stomach medicines (bismuth subsalicylate), paints bismuth vanadate on a dry surface, pearlescent cosmetics (bismuth oxychloride), and bismuth-containing bullets. The bismuth is so scattered in these uses as to be unrecoverable with present technology. Bismuth can also be available sustainably from greater efficiency of use or substitution, most likely stimulated by a rising price. For the stomach medicine, another active ingredient could be substituted for some or all of the bismuth compound . It would be more difficult to find an alternative to bismuth oxychloride in cosmetics to give the pearlescent effect. However, there are many alloying formulas for solders and therefore many alternatives.

The most important sustainability fact about bismuth is its byproduct status, which can either improve sustainability (i.e., vanadium or manganese nodules) or, for bismuth from lead ore, constrain it; bismuth is constrained. The extent that the constraint on bismuth can be ameliorated or not is going to be tested by the future of the lead storage battery, since 90% of the world market for lead is in storage batteries for gasoline or diesel-powered motor vehicles.

The life-cycle assessment of bismuth will focus on solders, one of the major uses of bismuth, and the one with the most complete information. The average primary energy use for solders is around 200 MJ per kg, with the high-bismuth solder (58% Bi) only 20% of that value, and three low-bismuth solders (2% to 5% Bi) running very close to the average. The global warming potential averaged 10 to 14 kg carbon dioxide, with the high-bismuth solder about two-thirds of that and the low-bismuth solders about average. The acidification potential for the solders is around 0.9 to 1.1 kg sulfur dioxide equivalent, with the high-bismuth solder and one low-bismuth solder only one-tenth of the average and the other low-bismuth solders about average.[13] There is very little life-cycle information on other bismuth alloys or compounds.

Chemistry

See also Category: Bismuth compounds

Bismuth forms trivalent and pentavalent compounds. The trivalent compounds are more common. Many of its chemical properties are similar to other elements in its group; namely, arsenic and antimony, although it is less toxic than those elements.

Bismuth is stable to both dry and moist air at ordinary temperatures. At elevated temperatures, the vapours of the metal combine rapidly with oxygen, forming the yellow trioxide, Bi2O3.[14] On reaction with base, this oxide forms two series of oxyanions: BiO−2, which is polymeric and forms linear chains, and BiO3−3. The anion in Li3BiO3 is actually a cubic octameric anion, Bi8O24−24, whereas the anion in Na3BiO3 is tetrameric.[15]

Bismuth sulfide, Bi2S3, occurs naturally in bismuth ores.[16] It is also produced by the combination of molten bismuth and sulfur.[14]

Unlike earlier members of group 15 elements such as nitrogen, phosphorus, and arsenic, and similar to the previous group 15 element antimony, bismuth does not form a stable hydride analogous to ammonia and phosphine. Bismuth hydride, bismuthine (BiH3), is an endothermic compound that spontaneously decomposes at room temperature. It is stable only below −60°C.[15]

The halides of bismuth in low oxidation states have been shown to have unusual structures. What was originally thought to be bismuth(I) chloride, BiCl, turns out to be a complex compound consisting of Bi5+9 cations and BiCl2−5 and Bi2Cl2−8 anions.[15][17] The Bi5+9 cation has a distorted tricapped trigonal prismic molecular geometry, and is also found in Bi10Hf3Cl18, which is prepared by reducing a mixture of hafnium(IV) chloride and bismuth chloride with elemental bismuth, having the structure [Bi+][Bi5+9][HfCl2−6]3.[15]:50 Other polyatomic bismuth cations are also known, such as Bi2+8, found in Bi8(AlCl4)2.[17] Bismuth also forms a low-valence bromide with the same structure as "BiCl". There is a true monoiodide, BiI, which contains chains of Bi4I4 units. BiI decomposes upon heating to the triiodide, BiI3, and elemental bismuth. A monobromide of the same structure also exists.[15]

In oxidation state +3, bismuth forms trihalides with all of the halogens: BiF3, BiCl3, BiBr3, and BiI3. All of these, except BiF3, are hydrolysed by water to form the bismuthyl cation, BiO+, a commonly encountered bismuth oxycation.[15] Bismuth(III) chloride reacts with hydrogen chloride in ether solution to produce the acid HBiCl4.[18]

Bismuth dissolves in nitric acid to form bismuth(III) nitrate, Bi(NO3)3. In the presence of excess water or the addition of a base, the Bi3+ ion reacts with the water to form BiO+, which precipitates as (BiO)NO3.[19]

The oxidation state +5 is less frequently encountered. One such compound is BiF5, a powerful oxidising and fluorinating agent. It is also a strong fluoride acceptor, reacting with xenon tetrafluoride to form the XeF+3 cation:[18]

BiF5 + XeF4 → XeF+3BiF−6

The dark red bismuth(V) oxide, Bi2O5, is unstable, liberating O2 gas upon heating.[20]

In aqueous solution, the Bi3+ ion exists in various states of hydration, depending on the pH:

pH range Species
<3 Bi(H2O)3+6
0-4 Bi(H2O)5OH2+
1-5 Bi(H2O)4(OH)2+
5-14 Bi(H2O)3(OH)3
>11 Bi(H2O)2(OH)4−

These mononuclear species are in equilibrium. Polynuclear species also exist, the most important of which is BiO+, which exists in hexameric form as the octahedral complex [Bi6O4(OH)4]6+ (or 6 [BiO+]·2 H2O).[21]

Applications

Bismuth oxychloride is sometimes used in cosmetics. Bismuth subnitrate and bismuth subcarbonate are used in medicine.[3]

Health

  • Killing some bacteria that cause diarrhea
  • Reducing inflammation/irritation of stomach and intestinal lining
  • Retarding the expulsion of fluids into the digestive system by irritated tissues, by "coating" them.

Other uses

In the early 1990s, research began to evaluate bismuth as a nontoxic replacement for lead in various applications:

According to the USGS, U.S. bismuth consumption in 2006 totaled 2,050 tonnes, of which chemicals (including pharmaceuticals, pigments, and cosmetics) were 510 tonnes, bismuth alloys 591 tonnes, metallurgical additives 923 tonnes, and the balance other uses.

Toxicology and ecotoxicology

Scientific literature concurs with the idea that bismuth and its compounds are less toxic than lead or its other periodic table neighbours (antimony, polonium)[27] and that it is not bioaccumulative. Its biological half-life for whole-body retention is 5 days but it can remain in the kidney for years in patients treated with bismuth compounds.[28] In the industry, it is considered as one of the least toxic heavy metals.

Bismuth poisoning exists and mostly affects the kidney and liver. Skin and respiratory irritation can also follow exposure to respective organs. As with lead, overexposure to bismuth can result in the formation of a black deposit on the gingiva, known as a bismuth line.[29]

Bismuth's environmental impacts are not very well known. It is considered that its environmental impact is small, due in part to the low solubility of its compounds.[30] Limited information however means that a close eye should be kept on its impact.

Other characteristics

Fine bismuth powder can be pyrophoric.[14]

See also


References

  1. ↑ Bismuth, mindat.org
  2. ↑ Dumé, Belle (2003-04-23). "Bismuth breaks half-life record for alpha decay". Physicsweb. http://physicsweb.org/articles/news/7/4/16. 
  3. ↑ 3.00 3.01 3.02 3.03 3.04 3.05 3.06 3.07 3.08 3.09 3.10 3.11 C. R. Hammond (2004). The Elements, in Handbook of Chemistry and Physics 81st edition. CRC press. ISBN 0849304857. 
  4. ↑ C. A. Hoffman, J. R. Meyer, and F. J. Bartoli, A. Di Venere, X. J. Yi, C. L. Hou, H. C. Wang, J. B. Ketterson, and G. K. Wong (1993). "Semimetal-to-semiconductor transition in bismuth thin films". Phys. Rev. B 48: 11431. doi:10.1103/PhysRevB.48.11431. 
  5. ↑ Marcillac, Pierre de; Noël Coron, Gérard Dambier, Jacques Leblanc, and Jean-Pierre Moalic (April 2003). "Experimental detection of α-particles from the radioactive decay of natural bismuth". Nature 422 (6934): 876–878. doi:10.1038/nature01541. PMID 12712201. 
  6. ↑ Agricola, Georgious (1546 (orig.); 1955(trans)). De Natura Fossilium. New York: Mineralogical Society of America. pp. 178. 
  7. ↑ Gordon, Robert B.; Rutledge, John W. (1984). "Bismuth Bronze from Machu Picchu, Peru". Science 223 (4636): 585–586. doi:10.1126/science.223.4636.585. PMID 17749940. http://www.jstor.org/stable/1692247. 
  8. ↑ 8.0 8.1 "Bismuth Advocate News - Price and Long-Term Outlook Issue No. 29 November – December 2007". http://www.basicsmines.com/bismuth/index.html. Retrieved 8 August 2008. 
  9. ↑ Carlin, Jr., James F.. "2006 USGS Minerals Yearbook: Bismuth" (PDF). United States Geological Survey. http://minerals.usgs.gov/minerals/pubs/commodity/bismuth/myb1-2006-bismu.pdf. Retrieved 2009-02-08. 
  10. ↑ 10.0 10.1 Carlin, Jr., James F.. "2007 USGS Minerals Yearbook: Bismuth" (PDF). United States Geological Survey. http://minerals.usgs.gov/minerals/pubs/commodity/bismuth/myb1-2007-bismu.pdf. Retrieved 2009-09-11. 
  11. ↑ "Customer input prices". http://customer-inputprices.blogspot.com. Retrieved 2009-02-08. 
  12. ↑ Taylor, Harold A. (2000). Bismuth. Financial Times Executive Commodity Reports. London: Financial Times Energy. p. 17. ISBN 1840833262. 
  13. ↑ "IKP, Department of Life-Cycle Engineering". http://leadfree.ipc.org/files/RoHS_15.pdf. Retrieved 2009-05-05. 
  14. ↑ 14.0 14.1 14.2 Patnaik, Patnaik (2002). Handbook of Inorganic Chemical Compounds. McGraw-Hill Professional. ISBN 0070494398. 
  15. ↑ 15.0 15.1 15.2 15.3 15.4 15.5 Godfrey, S. M.; McAuliffe, C. A.; Mackie, A. G.; Pritchard, R. G. (1998). Nicholas C. Norman. ed. Chemistry of arsenic, antimony, and bismuth. Springer. pp. 67–84. ISBN 075140389X. 
  16. ↑ Remsen, Ira (1886). An Introduction to the Study of Chemistry. Henry Holt and Company. p. 363. 
  17. ↑ 17.0 17.1 Gillespie, R. J.; Passmore, = J. (1975). Emeléus, H. J.; Sharp A. G.. ed. Advances in Inorganic Chemistry and Radiochemistry. Academic Press. pp. 77–78. ISBN 0120236176. 
  18. ↑ 18.0 18.1 Suzuki, Hitomi; Matano, Yoshihiro (2001). Organobismuth chemistry. Elsevier. p. 8. ISBN 0444205284. 
  19. ↑ Wurtz, Charles Adolphe; Greene, William Houston; Keller, H. F. (1880). Greene, William Houston. ed. Elements of modern chemistry (6th ed.). J.B. Lippincott. p. 351. 
  20. ↑ Scott, Thomas; Eagleson, Mary (1994). Concise encyclopedia chemistry. Walter de Gruyter. p. 136. ISBN 3110114518. 
  21. ↑ Holleman, Arnold F.; Wiberg, Egon (2001). Wiberg, Nils. ed. Inorganic chemistry. Translated by Mary Eagleson, William Brewer. Academic Press. p. 771. ISBN 0123526515. 
  22. ↑ Adams, Edmond (1953). "A New Permanent Magnet from Powdered Manganese Bismuthide". Rev. Mod. Phys. 25 (1): 306–307. doi:10.1103/RevModPhys.25.306. 
  23. ↑ "Unusual Electronic Properties In Bismuth-based Crystalline Material May Lead To Better Computer Chips And Solar Cells". Science Daily. February 20, 2009. http://www.sciencedaily.com/releases/2009/02/090219141530.htm. Retrieved 2009-09-09. 
  24. ↑ "BSCCO". National High Magnetic Field Laboratory. http://www.magnet.fsu.edu/magnettechnology/research/asc/research/bscco.html. Retrieved 2010-01-19. 
  25. ↑ Imam, S (2001). "Advancements in cancer therapy with alpha-emitters: a review". International Journal of Radiation Oncology Biology Physics 51: 271. doi:10.1016/S0360-3016(01)01585-1. 
  26. ↑ 26.0 26.1 Lohse, Joachim; Zangl, Stéphanie; Groß, Rita; Gensch, Carl-Otto; Deubzer, Otmar. "Adaptation to Scientific and Technical Progress of Annex II Directive 2000/53/EC" (PDF). http://rohs-elv.exemptions.oeko.info/fileadmin/user_upload/Background/Final_report_ELV_Annex_II_revision.pdf. Retrieved 2009-09-11. 
  27. ↑ HSBD Search for Bismuth Compound toxicology. Compare this data with a research on Lead compounds
  28. ↑ Fowler, B.A. (1986). "Bismuth". In Friberg, L.. Handbook on the Toxicology of Metals (2nd ed.). Elsevier Science Publishers. pp. 117. 
  29. ↑ "Bismuth line". Farlex, Inc.. http://medical-dictionary.thefreedictionary.com/bismuth+line. Retrieved 8 February 2008. 
  30. ↑ Data on Bismuth's health and environmental effects.

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