Trimethylaluminium

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Trimethylaluminium
Names
IUPAC name
Trimethylalumane
Other names
Trimethylaluminum; aluminium trimethyl; aluminum trimethyl
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.000.776 Edit this at Wikidata
UNII
  • InChI=1S/3CH3.Al/h3*1H3; checkY
    Key: JLTRXTDYQLMHGR-UHFFFAOYSA-N checkY
  • InChI=1/3CH3.Al/h3*1H3;/rC3H9Al/c1-4(2)3/h1-3H3
    Key: JLTRXTDYQLMHGR-MZZUXTGEAJ
Properties
C6H18Al2
Molar mass 144.17 g/mol
72.09 g/mol (C3H9Al)
Appearance Colorless liquid
Density 0.752 g/cm3
Melting point 15 °C (59 °F; 288 K)
Boiling point 125–130 °C (257–266 °F; 398–403 K) [1][2]
Reacts
Vapor pressure
  • 1.2 kPa (20 °C)
  • 9.24 kPa (60 °C)[1]
Viscosity
  • 1.12 cP (20 °C)
  • 0.9 cP (30 °C)
Thermochemistry
155.6 J/mol·K[2]
209.4 J/mol·K[2]
−136.4 kJ/mol[2]
−9.9 kJ/mol[2]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Pyrophoric
GHS labelling:
GHS02: FlammableGHS05: Corrosive[1]
Danger
H250, H260, H314[1]
P222, P223, P231+P232, P280, P370+P378, P422[1]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneInstability 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g. hydrogen peroxideSpecial hazard W: Reacts with water in an unusual or dangerous manner. E.g. sodium, sulfuric acid
3
4
3
W
Flash point −17.0 °C (1.4 °F; 256.1 K) [1]
Related compounds
Related compounds
 Triethylaluminium
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Trimethylaluminium is one of the simplest examples of an organoaluminium compound. Despite its name it has the formula Al2(CH3)6 (abbreviated as Al2Me6 or TMA), as it exists as a dimer. This colorless liquid is an industrially important compound but must be handled with care due to its pyrophoricity; it evolves white smoke (aluminium oxides) when the vapor is released into the air.

Structure and bonding

Al2Me6 exists mostly as a dimer at room temperature and pressure,[3] analogous in structure and bonding to diborane. As with diborane, the molecules are connected by 2 3-center-2-electron bonds: the shared methyl groups bridge between the two aluminium atoms. The Al-C(terminal) and Al-C(bridging) distances are 1.97 and 2.14 Å, respectively.[4] The carbon atoms of the bridging methyl groups are each surrounded by five neighbors: three hydrogen atoms and two aluminium atoms. The methyl groups interchange readily intramolecularly and intermolecularly.

3-Centered-2-electron bonds are an example of "electron-deficient" molecules and tend to undergo reactions with Lewis bases that would give products consisting of 2-centered-2-electron bonds. For example, upon treatment with amines gives adducts R3N-AlMe3. The Lewis acid properties of AlMe3 has been thoroughly studied in hexane solutions using Lewis bases with N, O, P, and S donor atoms. [5] The enthalpy data show that AlMe3 is a hard acid and its acid parameters in the ECW model are EA =8.66 and CA = 3.68.Another reaction that gives products that follow the octet rule is the reaction of Al2Me6 with aluminium trichloride to give (AlMe2Cl)2.

The monomer species AlMe3, which has an aluminium atom bonded to three methyl groups, occurs at high temperature and low pressure.[3] VSEPR Theory predicts and electron diffraction confirms[6] that it has a trigonal planar (threefold) symmetry, as observed in BMe3.

Synthesis and applications

TMA is prepared via a two-step process that can be summarized as follows:

2 Al + 6 CH3Cl + 6 Na → Al2(CH3)6 + 6 NaCl

TMA is mainly used for the production of methylaluminoxane, an activator for Ziegler–Natta catalysts for olefin polymerisation. TMA is also employed as a methylation agent. Tebbe's reagent, which is used for the methylenation of esters and ketones, is prepared from TMA.

TMA is also used in semiconductor fabrication to deposit thin film, high-k dielectrics such as Al2O3 via the processes of chemical vapor deposition or atomic layer deposition.

TMA forms a complex with the tertiary amine DABCO, which is safer to handle than TMA itself.[7]

In combination with 20 to 100 mol % Cp2ZrCl2 (zirconocene dichloride), the (CH3)2Al-CH3 adds "across" alkynes to give vinyl aluminum species that are useful in organic synthesis in a reaction known as carboalumination.[8]

The NASA ATREX mission (Anomalous Transport Rocket Experiment) employed the white smoke that TMA forms on air contact to study the high altitude jet stream.

Semiconductor grade TMA

TMA is the preferred metalorganic source for metalorganic vapour phase epitaxy (MOVPE) of aluminium-containing compound semiconductors, such as AlAs, AlN, AlP, AlSb, AlGaAs, AlInGaAs, AlInGaP, AlGaN, AlInGaN, AlInGaNP, etc. Criteria for TMA quality focus on (a) elemental impurities, (b) oxygenated and organic impurities.

References

  1. ^ a b c d e f Sigma-Aldrich Co., Trimethylaluminum. Retrieved on 2014-05-05.
  2. ^ a b c d e http://chemister.ru/Database/properties-en.php?dbid=1&id=3290
  3. ^ a b Carlsson, J.; Gorbatkin, S.; Lubben, D.; Greene, J. E. (1991). "Thermodynamics of the homogeneous and heterogeneous decomposition of trimethylaluminum, monomethylaluminum, and dimethylaluminumhydride: Effects of scavengers and ultraviolet-laser photolysis". Journal of Vacuum Science and Technology B. 9 (6): 2759–2770. doi:10.1116/1.585642.
  4. ^ Holleman, A. F.; Wiberg, E. (2001). Inorganic Chemistry. San Diego: Academic Press. ISBN 0-12-352651-5.
  5. ^ Henrickson, C. H.; Duffy, D.; Eyman, D. P. (1968). "Lewis acidity of alanes. Interactions of trimethylalane with amines, ethers, and phosphines". Inorganic Chemistry. 7: 1047–1051. doi:10.1021/ic50064a001.
  6. ^ Almennin, A.; Halvorse, S.; Haaland, A. (2005). "Gas Phase Electron Diffraction Investigation of Molecular Structures of Trimethylaluminum Monomer and Dimer". Acta Chemica Scandinavica. 44 (15): 2232–2234. doi:10.3891/acta.chem.scand.25-1937.
  7. ^ Biswas, K.; Prieto, O.; Goldsmith, P. J.; Woodward, S. (2005). "Remarkably Stable (Me3Al)2 · DABCO and Stereoselective Nickel-Catalyzed AlR3 (R = Me, Et) Additions to Aldehydes". Angewandte Chemie International Edition. 44 (15): 2232–2234. doi:10.1002/anie.200462569. PMID 15768433.
  8. ^ Negishi, E.; Matsushita, H. (1984). "Palladium-Catalyzed Synthesis of 1,4-Dienes by Allylation of Alkenyalane: α-Farnesene [1,3,6,10-Dodecatetraene, 3,7,11-trimethyl-]". Organic Syntheses. 62: 31{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 7, p. 245.

External links

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