Bismuth compounds

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See also: Category:Bismuth compounds
Bismuth(III) oxide powder

Bismuth forms mainly trivalent and a few pentavalent compounds. Many of its chemical properties are similar to those of arsenic and antimony, although much less toxic.[1]

Oxides and sulfides[edit]

At elevated temperatures, vaporized bismuth metal and oxygen combine into the yellow trioxide, Bi
2O
3.[2][3] At temperatures above 710 °C, this (molten) oxide corrodes all known oxides and even platinum.[4] It forms two series of oxyanions in basic conditions: linear, chain-polymeric BiO−
2; and cubic BiO3−
3. In Li
3BiO
3, the anion forms the octamer Bi
8O24−
24; in Na
3BiO
3, the tetramer.[5]

The dark red bismuth(V) oxide, Bi
2O
5, is unstable, liberating O
2 gas upon heating.[6] The compound NaBiO3 is a strong oxidant.[7]

Bismuth sulfide, Bi
2S
3, occurs naturally in bismuth ores,[8] but can be synthesized from molten bismuth and sulfur.[9]

Halides[edit]

In oxidation state +3, bismuth forms salts with all the halogens: BiF
3, BiCl
3, BiBr
3, and BiI
3. All hydrolyze in water except BiF
3.[5] Bismuth(III) chloride reacts with hydrogen chloride in ether solution to produce the acid HBiCl
4.[10]

The oxidation state +5 is less frequently encountered. One such compound is the powerful oxidant and fluorinator, BiF
5. It is also a strong fluoride acceptor, forming the XeF+
3 cation from xenon tetrafluoride:[10]

BiF
5 + XeF
4 → XeF+
3BiF−
6

The low-oxidation-state bismuth halides adopt unusual cluster structures. What was originally thought bismuth(I) chloride, BiCl, is in fact a lattice of Bi5+
9 cations and BiCl2−
5 and Bi
2Cl2−
8 anions.[5][11] The Bi5+
9 cation has a distorted tricapped trigonal prismatic molecular geometry and is also found in Bi
10Hf
3Cl
18, 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.[5]: 50  Other polyatomic bismuth cations are also known, such as Bi2+
8, found in Bi
8(AlCl
4)
2.[11]

There is a true monoiodide, BiI, which contains chains of Bi
4I
4 units. BiI decomposes upon heating to the triiodide, BiI
3, and elemental bismuth.[5]

Bismuth forms at least two "monobromides": one isostructural to "BiCl"[citation needed] and one isostructural to Bi
4I
4.[5]

Aqueous species and the bismuthyl cation[edit]

In aqueous solution, the Bi3+
 ion is solvated to form the aqua ion Bi(H
2O)3+
8 in strongly acidic conditions.[12] At pH > 0 polynuclear species exist, the most important of which is believed to be the octahedral complex [Bi
6O
4(OH)
4]6+
.[13]

Bismuth oxychloride (BiOCl) structure (mineral bismoclite). Bismuth atoms are shown as grey, oxygen red, chlorine green.

Bismuth oxychloride (BiOCl) and bismuth oxynitrate (BiONO3) stoichiometrically appear simple anionic salts of the bismuthyl(III) cation (BiO+), which commonly occurs in aqueous bismuth compounds. However, in the case of BiOCl, the salt crystal forms alternating plates of Bi, O, and Cl atoms. Each oxygen coordinates with four bismuth atoms in the adjacent plane.[14]

Bismuthine and bismuthides[edit]

Unlike the lighter pnictogens nitrogen, phosphorus, and arsenic, but similar to antimony, bismuth does not form a stable hydride. Bismuth hydride, bismuthine (BiH
3), is an endothermic compound that spontaneously decomposes at room temperature. It is stable only below −60 °C.[5] Bismuthides are intermetallic compounds between bismuth and other metals.[15]

In 2014 researchers discovered that sodium bismuthide admits bulk 3D Dirac fermions. As a topological Dirac semi-metal, it is a three-dimensional counterpart to graphene with similar electron mobility and velocity. While sodium bismuthide (Na
3Bi) is too unstable to be used in devices without packaging, it may offer distinct efficiency and fabrication advantages over planar graphene in semiconductor and spintronics applications.[16][17]

Applications[edit]

Coloration[edit]

Bismuth vanadate, a yellow pigment
  • Bismuth subnitrate is an iridescent component of glazes and paint pigment.
  • Bismuth oxychloride is a pigment and cosmetic.[14]
  • Bismuth vanadate is an opaque yellow pigment used by some artists' oil, acrylic, and watercolor paint companies, primarily as a replacement for the more toxic cadmium sulfide yellows in the greenish-yellow (lemon) to orange-toned yellow range. It performs practically identically to the cadmium pigments in UV resistance, opacity, tinting strength, and inertness when mixed with other pigments. The most commonly-used variety by artists' paint makers is lemon in color.
The vanadate also replaces older zinc, lead, and strontium chromate pigments for much the same reason. With a green pigment and barium sulfate (for increased transparency), it can also replace the greenish-tinted barium chromate. Unlike lead chromates, it does not blacken from atmospheric hydrogen sulfide and possesses a particularly brighter color. The difference is especially apparent with the lemon, which has a more concentrated lead sulfate mixture.
Vanadate paints are also used, on a limited basis due to its cost, on vehicles.[18][19]

Electrics and electronics[edit]

  • Bismuth strontium calcium copper oxide (BSCCO) is a superconducting compound family discovered in 1988. Its members exhibit the highest superconducting transition temperatures at standard pressure.[22]
  • δ-Bismuth oxide is a solid electrolyte for oxygen. This form is stable only at high temperature, but can be electrodeposited well below this temperature in highly alkaline solution.
  • Bismuth telluride is a semiconductor and thermoelectric.[14][23] Bi2Te3 diodes are used in mobile refrigerators, CPU coolers, and as detectors in infrared spectrophotometers.[14]
  • Bismuth germanate is a scintillator in X-ray and gamma ray detectors.

Chemical catalysis[edit]

Other[edit]

See also[edit]

References[edit]

  1. ^ Levason, W.; Reid, G. (2003). "Coordination Chemistry of the s, p, and f Metals". Comprehensive Coordination Chemistry II. Amsterdam: Elsevier Pergamon. doi:10.1016/B0-08-043748-6/02023-5. ISBN 0-08-043748-6.
  2. ^ Wiberg, p. 768.
  3. ^ Greenwood, p. 553.
  4. ^ Krüger, p. 185
  5. ^ a b c d e f g 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 978-0-7514-0389-3.
  6. ^ Scott, Thomas; Eagleson, Mary (1994). Concise encyclopedia chemistry. Walter de Gruyter. p. 136. ISBN 978-3-11-011451-5.
  7. ^ Greenwood, p. 578.
  8. ^ An Introduction to the Study of Chemistry. Forgotten Books. p. 363. ISBN 978-1-4400-5235-4.
  9. ^ Greenwood, pp. 559–561.
  10. ^ a b Suzuki, p. 8.
  11. ^ a b Gillespie, R. J.; Passmore, J. (1975). Emeléus, H. J.; Sharp A. G. (eds.). Advances in Inorganic Chemistry and Radiochemistry. Academic Press. pp. 77–78. ISBN 978-0-12-023617-6.
  12. ^ Persson, Ingmar (2010). "Hydrated metal ions in aqueous solution: How regular are their structures?". Pure and Applied Chemistry. 82 (10): 1901–1917. doi:10.1351/PAC-CON-09-10-22.
  13. ^ Näslund, Jan; Persson, Ingmar; Sandström, Magnus (2000). "Solvation of the Bismuth(III) Ion by Water, Dimethyl Sulfoxide, N,N'-Dimethylpropyleneurea, and N,N-Dimethylthioformamide. An EXAFS, Large-Angle X-ray Scattering, and Crystallographic Structural Study". Inorganic Chemistry. 39 (18): 4012–4021. doi:10.1021/ic000022m. PMID 11198855.
  14. ^ a b c d Krüger, p. 184.
  15. ^ "bismuthide". Your Dictionary. Retrieved 2020-04-07.
  16. ^ "3D counterpart to graphene discovered [UPDATE]". KurzweilAI. 20 January 2014. Retrieved 28 January 2014.
  17. ^ Liu, Z. K.; Zhou, B.; Zhang, Y.; Wang, Z. J.; Weng, H. M.; Prabhakaran, D.; Mo, S. K.; Shen, Z. X.; Fang, Z.; Dai, X.; Hussain, Z.; Chen, Y. L. (2014). "Discovery of a Three-Dimensional Topological Dirac Semimetal, Na3Bi". Science. 343 (6173): 864–7. arXiv:1310.0391. Bibcode:2014Sci...343..864L. doi:10.1126/science.1245085. PMID 24436183. S2CID 206552029.
  18. ^ Tücks, Andreas; Beck, Horst P. (2007). "The photochromic effect of bismuth vanadate pigments: Investigations on the photochromic mechanism". Dyes and Pigments. 72 (2): 163. doi:10.1016/j.dyepig.2005.08.027.
  19. ^ Müller, Albrecht (2003). "Yellow pigments". Coloring of plastics: Fundamentals, colorants, preparations. Hanser Verlag. pp. 91–93. ISBN 978-1-56990-352-0.
  20. ^ Croteau, Gerry; Dills, Russell; Beaudreau, Marc; Davis, Mac (2010). "Emission factors and exposures from ground-level pyrotechnics". Atmospheric Environment. 44 (27): 3295. Bibcode:2010AtmEn..44.3295C. doi:10.1016/j.atmosenv.2010.05.048.
  21. ^ Ledgard, Jared (2006). The Preparatory Manual of Black Powder and Pyrotechnics. Lulu. pp. 207, 319, 370, 518, search. ISBN 978-1-4116-8574-1.
  22. ^ "BSCCO". National High Magnetic Field Laboratory. Archived from the original on 12 April 2013. Retrieved 18 January 2010.
  23. ^ Tritt, Terry M. (2000). Recent trends in thermoelectric materials research. Academic Press. p. 12. ISBN 978-0-12-752178-7.
  24. ^ Hammond, C. R. (2004). The Elements, in Handbook of Chemistry and Physics (81st ed.). Boca Raton (FL, US): CRC press. p. 4–5. ISBN 978-0-8493-0485-9.
  25. ^ DiMeglio, John L.; Rosenthal, Joel (2013). "Selective conversion of CO2 to CO with high efficiency using an bismuth-based electrocatalyst". Journal of the American Chemical Society. 135 (24): 8798–8801. doi:10.1021/ja4033549. PMC 3725765. PMID 23735115.
  26. ^ Planas, Oriol; Wang, Feng; Leutzsch, Markus; Cornella, Josep (2020). "Fluorination of arylboronic esters enabled by bismuth redox catalysis". Science. 367 (6475): 313–317. Bibcode:2020Sci...367..313P. doi:10.1126/science.aaz2258. hdl:21.11116/0000-0005-DB57-3. PMID 31949081. S2CID 210698047.
  27. ^ Mortier, Roy M.; Fox, Malcolm F.; Orszulik, Stefan T. (2010). Chemistry and Technology of Lubricants. Springer. p. 430. Bibcode:2010ctl..book.....M. ISBN 978-1-4020-8661-8.
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