Trimethylphosphine

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Trimethylphosphine
Stereo, skeletal formula of trimethylphosphine with the lone pair of electrons shown, and all explicit hydrogens added
Ball and stick model of trimethylphosphine
Trimethylphosphine-3D-vdW.png
Names
Preferred IUPAC name
Trimethylphosphane
Systematic IUPAC name
Trimethylphosphane[1] (substitutive)
Trimethylphosphorus[1] (additive)
Identifiers
3D model (JSmol)
969138
ChEBI
ChemSpider
ECHA InfoCard 100.008.932 Edit this at Wikidata
EC Number
  • 209-823-1
MeSH trimethyl+phosphine
UN number 1993
Properties
C3H9P
Molar mass 76.079 g·mol−1
Appearance Colorless liquid
Density 735 mg cm−3
Melting point −86 °C (−123 °F; 187 K)
Boiling point 38 to 39 °C (100 to 102 °F; 311 to 312 K)
Vapor pressure 49.9 kPa (at 20 °C)
Structure
Trigonal pyramidal
Dipole moment
 1.19 Debye
Hazards
GHS pictograms GHS02: Flammable GHS07: Harmful
GHS Signal word Danger
GHS hazard statements
 H225, H315, H319, H335
P210, P261, P305+351+338
Flash point −19 °C (−2 °F; 254 K)
Related compounds
Related compounds
 PEt3
NMe3
PH3
PPh3
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Trimethylphosphine is the organophosphorus compound with the formula P(CH3)3, commonly abbreviated as PMe3. This colorless liquid has a strongly unpleasant odor, characteristic of alkylphosphines. The compound is a common ligand in coordination chemistry.

Structure and bonding[]

It is a pyramidal molecule with approximate C3v symmetry. The C–P–C bond angles are approximately 98.6°.[2]

The C–P–C bond angles are consistent with the notion that phosphorus predominantly uses the 3p orbitals for forming bonds and that there is little sp hybridization of the phosphorus atom. The latter is a common feature of the chemistry of phosphorus. As a result, the lone pair of trimethylphosphine has predominantly s-character as is the case for phosphine, PH3.[3]

PMe3 can be prepared by the treatment of triphenyl phosphite with methylmagnesium chloride:[4]

3 CH3MgCl + P(OC6H5)3 → P(CH3)3 + 3 C6H5OMgCl

The synthesis is conducted in dibutyl ether, from which the more volatile PMe3 can be distilled.

Reactions[]

With a pKa of 8.65, PMe3 reacts with strong acids to give salts [HPMe3]X.[2] This reaction is reversible. With strong bases, such as alkyl lithium compounds, a methyl group undergoes deprotonation to give PMe2CH2Li.

PMe3 is easily oxidised to the phosphine oxide with oxygen. It reacts with methyl bromide to give tetramethylphosphonium bromide.[5]

Coordination chemistry[]

Trimethylphosphine is a highly basic ligand that forms complexes with most metals. As a ligand, trimethylphosphine's Tolman cone angle is 118°.[6] This angle is an indication of the amount of steric protection that this ligand provides to the metal that to which it is bound.

Being a relatively compact phosphine, several can bind to a single transition metal, as illustrated by the existence of Pt(PEt3)4.[7] Its complex with silver iodide, AgI(PMe3) is an air-stable solid that releases PMe3 upon heating.

Structure of HW(PMe3)4(Me2PCH2), "W(PMe3)5".[8]

Safety[]

PMe3 is toxic and pyrophoric. It converts to a much safer phosphine oxide upon treatment with sodium hypochlorite or hydrogen peroxide.[9]

References[]

  1. ^ Jump up to: a b "Trimethylphosphine (CHEBI:35890)". Chemical Entities of Biological Interest (ChEBI). UK: European Bioinformatics Institute. 6 June 2006. IUPAC Names. Retrieved 25 September 2011.
  2. ^ Jump up to: a b Annette Schier and Hubert Schmidbaur"P-Donor Ligands" in Encyclopedia of Inorganic Chemistry 2006, Wiley-VCH, Weinheim. doi:10.1002/0470862106.ia177
  3. ^ E. Fluck, The chemistry of phosphine, Topics in Current Chemistry Vol. 35, 64 pp, 1973.
  4. ^ Leutkens, Jr., M. L.; Sattelberger, A. P.; Murray, H. H.; Basil, J. D.; Fackler, Jr. J. P. (1990). "Trimethylphosphine". Inorganic Syntheses. 28: 305–310. doi:10.1002/9780470132593.ch76.CS1 maint: multiple names: authors list (link)
  5. ^ H. F. Klein (1978). "Trimethylphosphonium Methylide (Trimethyl Methylenephosphorane)". Inorganic Syntheses. XVIII: 138–140. doi:10.1002/9780470132494.ch23.
  6. ^ G. L. Miessler and D. A. Tarr Inorganic Chemistry, 3rd Ed, Pearson/Prentice Hall publisher, ISBN 0-13-035471-6.
  7. ^ T. Yoshida T. Matsuda S. Otsuka (1990). "Tetrakis(Triethylphosphine)Platinum(0)". Inorganic Syntheses. 28: 122. doi:10.1002/9780470132593.ch32.CS1 maint: uses authors parameter (link)
  8. ^ Sattler, A.; Parkin, G. (2011). "Formation of a cationic alkylidene complex via formal hydride abstraction: synthesis and structural characterization of [W(PMe3)4([small eta]2-CHPMe2)H]X (X = Br, I)". Chemical Communications. 47: 12828–12830. doi:10.1039/C1CC15457E.CS1 maint: uses authors parameter (link)
  9. ^ http://www.sigmaaldrich.com/catalog/product/aldrich/324116?lang=en&region=US&cm_sp=Insite-_-prodRecCold_xorders-_-prodRecCold2-2
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