Borohydride

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Ball-and-stick model of the tetrahydroborate anion, [BH4]−

Borohydride refers to the anion [

cyanoborohydride or cyanotrihydroborate [BH3(CN)]− and triethylborohydride or triethylhydroborate [BH(CH2CH3)3]−. Borohydrides 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 first described in 1940 by Hermann Irving Schlesinger and Herbert C. Brown. They synthesized lithium borohydride Li[BH4] from diborane B2H6:[4][5]

2 MH + B2H6 → 2 M[BH4], where M = Li, Na, K, Rb, Cs, etc.

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

Structure

In the borohydride anion and most of its modifications,

tetrahedral structure.[6]
The reactivity of the B−H bonds depends on the other ligands. Electron-releasing ethyl groups as in triethylborohydride render the B−H center highly nucleophilic. In contrast, cyanoborohydride is a weaker reductant owing to the electron-withdrawing cyano substituent. The countercation also influences the reducing power of the reagent.

Selected properties of various borohydride salts
Borohydride
[CAS no.]		 molecular weight
(g/mol)		 Hydrogen density Density
(g/cm3)		 melting point
(°C)		 Solubility in water
(g/100 mL at 25 °C)		 Solubility in MeOH
(g/100 mL, 25 °C)		 Solubility in Et2O
(g/100 mL, 25 °C)		 Solubility in THF
(g/100 mL at 25 °C)
Li[BH4]
[16949-15-8] 		21.78 18.5 0.66 280 20.9 decomposes (44 in EtOH) 4.3 22.5
Na[BH4]
[16940-66-2] 		37.83 10.6 1.07 505 55 16.4 (at 20 °C) insoluble 0.1 (at 20 °C)
Na[BH3(CN)]
[25895-60-7] 		62.84 6.4 1.20 240 with decomposition tolerated[7] 217 insoluble 36
K[BH4]
[13762-51-1] 		53.94 7.4 1.17 585 (under H2) 19 insoluble insoluble insoluble
Li[BHEt3]
[22560-16-3] 		105.94 0.95 unknown unknown decomposes decomposes N/A high (supplied commercially)

Uses

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

Na[BH4] + 8 NaOH + 8 SO2 → 4 Na2S2O4 + NaBO2 + 6 H2O

Dithionite is used to bleach wood pulp.

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

Ball-and-stick model of Zr[BH4]4

In its coordination complexes, the borohydride ion is bound to the metal by means of one to three bridging hydrogen atoms.[9][3][10] In most such compounds, the [BH4]− ligand is bidentate. Some homoleptic borohydride complexes are volatile. One example is uranium borohydride.

Metal borohydride complexes can often be prepared by a simple salt elimination reaction:[11]

TiCl4 + 4 Li[BH4] + Et2O (solvent) → Ti[BH4]4·Et2O + 4 LiCl

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 (CVD), a way of depositing thin films of metal borides.[12] For example, zirconium diboride ZrB2 and hafnium diboride HfB2 can be prepared through CVD of the zirconium(IV) tetrahydroborate Zr[BH4]4 and hafnium(IV) tetrahydroborate Hf[BH4]4:[12]

M[BH4]4 → MB2 + B2H6 + 5 H2

Metal diborides find uses as coatings because of their hardness, high melting point, strength, resistance to wear and corrosion, and good electrical conductivity.[12]

References

  1. ^ "Tetrahydroborate". Chemspider.com. Retrieved 26 February 2013.
  2. ^
    ISBN 978-3527306732
    .
  3. ^
    doi:10.1070/RC2000v069n09ABEH000580
    .
  4. doi:10.1021/ja01869a039
    .
  5. doi:10.1021/ja01097a053
    .
  6. ISBN 978-0-08-037941-8
    .
  7. ISBN 978-0471936237
    .
  8. PMID 23503711
    .
  9. doi:10.1021/cr60306a004
    .
  10. ISBN 978-3-540-78633-7
    .
  11. doi:10.1002/zaac.654270202
    .
  12. ^
    doi:10.1021/ja00213a058
    .

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