Aluminium borohydride

Aluminium borohydride[1]

Names
IUPAC name

Aluminium borohydride

Other names

Aluminium borohydride, aluminium tetrahydroborate

Identifiers

CAS Number

* 16962-07-5 Y[chemspider]

3D model (JSmol)

* Interactive image

ChemSpider |

* 55734 Y

PubChem CID

* 6328559 PubChem has bad formula

UNII |

* 7OBU10UOXG Y

UN number | 2870

InChI

* InChI=1S/Al.3BH4/h;3*1H4/q+3;3*-1 Y

Key: LNJYEMMRSAGORU-UHFFFAOYSA-N Y

* InChI=1/Al.3BH4/h;3*1H4/q+3;3*-1

Key: LNJYEMMRSAGORU-UHFFFAOYAC

SMILES

* [Al+3].[BH4-].[BH4-].[BH4-]

Properties

Chemical formula

| AlB3H12
Molar mass | 71.51 g·mol−1
Appearance  | colorless liquid
Melting point |  −64.5 °C (−84.1 °F; 208.7 K)
Boiling point |  44.5 °C (112.1 °F; 317.6 K)

Solubility in water

| reacts
Hazards
Flash point | Spontaneously ignites

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

Aluminium borohydride, also known as aluminium tetrahydroborate, is the chemical compound with the formula Al(BH4)3. It is a volatile pyrophoric liquid which is used as a reducing agent in laboratories. Unlike most other metal–borohydrides, which are ionic structures, aluminium borohydride is a covalent compound.[2][3]

## Contents

* 1 Preparation
* 2 Reactions
* 3 References
* 4 Further reading

## Preparation

Aluminium borohydride is formed by the reaction between sodium borohydride with aluminium chloride:[4]

3 NaBH4 \+ AlCl3 → Al(BH4)3 \+ 3 NaCl

or as the non-pyrophoric tetrahydrofuran (THF) adduct, by the analogous reaction of calcium borohydride and aluminium chloride in THF:[2]

3 Ca(BH4)2 \+ 2 AlCl3 → 3 CaCl2 \+ 2 Al(BH4)3

## Reactions

Like most borohydrides, this compound is a reducing agent and hydride donor. It reacts with water to give elemental hydrogen gas,[4] and reduces carboxylic esters, aldehydes, and ketones to alcohols.[2]

It is used to prepare metal complexes of borohydride:[5]

AnF4 \+ 2 Al(BH4)3 → An(κ3-BH4)4 \+ 2AIF2BH4 (An = actinide metal)

When aluminium borohydride is heated, diborane is released, and a dialuminium dihydride forms:[6]

2 Al(BH4)3 → Al2H2(BH4)4 \+ B2H6

## References

1. ↑ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–39. ISBN 0-8493-0594-2.
2. ↑ 2.0 2.1 2.2 J. Kollonitsch & O. Fuchs (1955). "Preparation of Aluminium Borohydride and its Applications in Organic Reductions". Nature 176 (4492): 1081. doi:10.1038/1761081a0. Bibcode: 1955Natur.176.1081K.
3. ↑ Miwa, K.; Ohba, N.; Towata, S.; Nakamori, Y.; Züttel, A.; Orimo, S. (2007). "First-principles study on thermodynamical stability of metal borohydrides: Aluminum borohydride Al(BH4)3". J. Alloys Compd. 446–447: 310–314. doi:10.1016/j.jallcom.2006.11.140.
4. ↑ 4.0 4.1 Perry, Dale L.; Phillips, Sidney L. (1995). Handbook of Inorganic Compounds. CRC Press. pp. 3–4. ISBN 0-8493-8671-3. https://books.google.com/books?id=0fT4wfhF1AsC. Retrieved 2007-12-09.
5. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 168. ISBN 978-0-08-037941-8.
6. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 230. ISBN 978-0-08-037941-8.

## Further reading

* Fletcher, Edward; Foster, Hampton; Straight, David (1959). "Aluminum Borohydride and Mixtures with Hydrocarbons in Jet Engine Combustor Ignition". Industrial & Engineering Chemistry 51 (11): 1389. doi:10.1021/ie50599a044.
* Hinkamp, James B.; Hnizda, Vincent (1955). "Aluminum Borohydride Preparation". Industrial & Engineering Chemistry 47 (8): 1560. doi:10.1021/ie50548a032.

* v
* t
* e

Aluminium compounds

Al(I)|

* AlBr
* AlCl
* AlF
* AlI
* Al2O

Al(II)|

* AlB2
* AlB12
* AlO

Al(III)|

* AlAs
* Al(BH4)3
* AlBr3
* AlCl3
* AlF3
* AlH3
* AlI3
* AlN
* Al(NO3)3
* Al2(CO3)3
* Al(OH)3
* Al(OH)2OAc
* Al(OH)(OAc)2
* Al(OAc)3
* Al2SO4(OAc)4
* AlP
* AlPO4
* AlSb
* Al(C5H7O2)3
* Al(MnO4)3
* Al2(MoO4)3
* Al2O3
* Al2S3
* Al2(SO4)3
* Al2Se3
* Al2Te3
* Al2SiO5
* Al4C3
* AlOHO
* Al(OH)2CO2C17H5
* NaAlH2(OC2H4OCH3)2
* LiAlH2(OC2H4OCH3)2

| Alums|

* (NH4)Al(SO4)2
* KAl(SO4)2
* NaAl(SO4)2

|

Organoaluminium(III) compounds|

* (Al(CH3)3)2
* (Al(C2H5)3)2
* Al(CH2CH(CH3)2)3
* Al(C2H5)2Cl
* Al(C2H5)2CN
* Al(CH2CH(CH3)2)2H
* Al(C2H5)2Cl2C2H5Cl
* Ti(C5H5)2CH2ClAl(CH3)2

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