Borohydride

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File:Borohydride-3D-balls.png
Ball-and-stick model of the borohydride anion, BH4−

Borohydride refers to the anion BH4− and its salts.[1] Borohydride is also the term used for compounds containing BH4-nXn−, for example cyanoborohydride (B(CN)H3−) and triethylborohydride (B(C2H5)3H−). Such compounds find wide use as reducing agents in organic synthesis. The most important borohydrides are lithium borohydride and sodium borohydride, but other salts are well known (see Table).[2] Tetrahydroborates are also of academic and industrial interest in inorganic chemistry.[3]

History

Alkali metal borohydrides were described in 1940 by Hermann Irving Schlesinger and Herbert C. Brown. They synthesized lithium borohydride (LiBH4) from diborane (B2H6):[4][5]

2 MH + B2H6 → 2 M[BH4]     (M = Li, Na, K, etc.)

Current methods involve reduction of trimethyl borate with sodium hydride.[2]

Structure

The borohydride anion has a tetrahedral structure with boron in the center and the hydrogens located at the four vertices of the tetrahedron.[6] In metal complexes, the borohydride ion is bound to the metal by means of bridging hydrogen atoms, usually in one of three different ways: monodentate (one hydrogen bridge), bidentate (two hydrogen bridges), and tridentate (three hydrogen bridges)[7] (η1, η2, or η3).[3] The preferred coordination mode is strongly affected by the nature of the metal and its oxidation state.

Selected Properties of Various Borohydride Salts
Hydride CAS registry number Mol.Wt. Hydrogen Density Density g/cm3 m.p. (°C) solubility in water (g/100 mL, 25 °C) solubility in CH3OH (g/100 mL, 25 °C) solubility in ether (g/100 mL, 25 °C) solubility in THF (g/100 mL, 25 °C)
LiBH4

[16949-15-8]

 21.78 18.5 0.66 280 20.9 decomp. (44 in EtOH) 4.3 22.5
NaBH4

[16940-66-2]

 37.83 10.6 1.07 505 55 16.4 (20 °C) insol. 0.1 (20 °C)
NaBH3CN

[25895-60-7]

 62.84 6.4 1.20 240 with deccomp. deccomp. 217 insol. 36
KBH4

[13762-51-1]

 53.94 7.4 1.17 585 (under H2) 19 insol. insol. insol.
LiBH(C2H5)3

[22560-16-3]

 105.94 0.95 unknown unknown decomp. decomp. na high (supplied commercially)

Uses

Sodium borohydride is the borohydride that is produced on the largest scale industrially, estimated at 5000 tons/y in 2002. The main use is for the reduction of sulfur dioxide to give sodium dithionite:

NaBH4 + 8 NaOH + 8 SO2 → 4 Na2S2O4 + NaBO2 + 6 H2O

Dithionite is used to bleach wood pulp.[2] Sodium borohydride is also used to reduce aldehydes and ketones in the production of pharmaceuticals including chloramphenicol, thiophenicol, vitamin A, atropine, and scopolamine, as well as many flavorings and aromas.

Potential applications

Because of their high hydrogen content, borohydride complexes and salts have been of interest in the context of hydrogen storage.[8] Reminiscent of related work on ammonia borane, challenges are associated with slow kinetics and low yields of hydrogen as well as problems with regeneration of the parent borohydrides.

Coordination complexes

File:Zirconium-borohydride-3D-balls-A.png
Ball-and-stick model of Zr(BH4)4

Borohydrides can serve as ligands for many metals, and there is a large coordination chemistry of the borohydride ion.[9] In most such compounds, the BH4− ligand is bidentate. Some binary borohydrides (i.e., containing only BH4− ligands) are highly volatile. One example is uranium borohydride.

Metal borohydride complexes can often be prepared by a simple salt elimination reaction:

TiCl4 + LiBH4 → Ti(BH4)3(Et2O) in diethyl ether[10]

Decomposition

Some metal tetrahydroborates transform on heating to give metal borides. When the borohydride complex is volatile, this decomposition pathway is the basis of chemical vapor deposition, a way of depositing thin films of metal borides.[11] For example, zirconium and hafnium diborides, ZrB2 and HfB2, can be prepared through CVD of the tetrahydroborates Zr(BH4)4 and Hf(BH4)4:

M(BH4)4 → MB2 + B2H6 + 5H2 [11]

Metal diborides find uses as coatings because of their hardness, high melting point, strength, resistance to wear and corrosion, and good electrical conductivity.[11] The diboride films can be deposited on a variety of substances including glass, copper, aluminum, and steel.[11]

References

  1. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  2. ↑ 2.0 2.1 2.2 Rittmeyer, P.; Wietelmann, U. “Hydrides” in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a13_199
  3. ↑ 3.0 3.1 Makheav, V.D. Russ. Chem. Rev. 2000, 69, 727-746.doi:10.1070/RC2000v069n09ABEH000580
  4. ↑ Schlesinger, H.C.; Brown, H.R. "Metallo Borohydrides. III. Lithium Borohydride" J. Am. Chem. Soc. 1940, 62, 3429-3435. doi:10.1021/ja01869a039
  5. ↑ Schlesinger, H.C.; Brown, H.R.; Hoekstra, L.R. "Reactions of Diborane with Alkali Metal Hydrides and Their Addition Compounds. New Syntheses of Borohydrides. Sodium and Potassium Borohydrides" J. Am. Chem. Soc. 1953, 75, 199–204. doi:10.1021/ja01097a053
  6. ↑ Zuttel, A.; Borgschulte, A.; Orimo, S. Scripta Materialia 2007, 56, 823–828. doi:10.1016/j.scriptamat.2007.01.010
  7. ↑ Marks, T.J.; Kolb, J.R. Chem. Rev. 1977, 77, 263.
  8. ↑ [1].
  9. ↑ Besora, M.; Lledós, A. "Coordination Modes and Hydride Exchange Dynamics in Transition Metal Tetrahydroborate Complexes" Structure and Bonding (2008) volume 130, p. 149–202. doi:10.1007/430_2007_076
  10. ↑ Franz, H.; Fusstetter, H.; Nöth. H. Z. Anorg. Allg. Chem. 1976, 427, 97–113.
  11. ↑ 11.0 11.1 11.2 11.3 Jensen, J. A.; Gozum, J. E.; Pollina, D. M.; Girolami, G. S. "Titanium, zirconium, and hafnium tetrahydroborates as "tailored" CVD precursors for metal diboride thin films" J. Am. Chem. Soc. 1988, 110, 1643–1644. doi:10.1021/ja00213a058

External links

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