Aluminium borohydride

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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
CompTox Dashboard (EPA)	DTXSID801028871
InChI InChI=1S/Al.3BH4/h;31H4/q+3;3-1^Y Key: LNJYEMMRSAGORU-UHFFFAOYSA-N^Y InChI=1/Al.3BH4/h;31H4/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]

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 all 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]

References

^ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–39. ISBN 0-8493-0594-2.
^ ^a ^b ^c J. Kollonitsch & O. Fuchs (1955). "Preparation of Aluminium Borohydride and its Applications in Organic Reductions". Nature. 176 (4492): 1081. Bibcode:1955Natur.176.1081K. doi:10.1038/1761081a0.
^ 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. arXiv:cond-mat/0610853. doi:10.1016/j.jallcom.2006.11.140. S2CID 97032806.
^ ^a ^b Perry, Dale L.; Phillips, Sidney L. (1995). Handbook of Inorganic Compounds. CRC Press. pp. 3–4. ISBN 0-8493-8671-3. Retrieved 2007-12-09.

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.

Aluminium compounds

Al(I)

Organoaluminium(I) compounds	Al(C₅(CH₃)₅)

Al(II)

Al(III)

Alums	(NH₄)Al(SO₄)₂ KAl(SO₄)₂ NaAl(SO₄)₂
Organoaluminium(III) compounds	Al(C₃H₅O₃)₃ C ₃₆H ₆₉AlO ₆ (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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References

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