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Electron Diffraction Study of the Structure of Trimethylphosphine
dc.contributor.authorBartell, Lawrence S.en_US
dc.contributor.authorBrockway, Lawrence Olinen_US
dc.date.accessioned2010-05-06T21:50:03Z
dc.date.available2010-05-06T21:50:03Z
dc.date.issued1960-02en_US
dc.identifier.citationBartell, L. S.; Brockway, L. O. (1960). "Electron Diffraction Study of the Structure of Trimethylphosphine." The Journal of Chemical Physics 32(2): 512-515. <http://hdl.handle.net/2027.42/70229>en_US
dc.identifier.urihttps://hdl.handle.net/2027.42/70229
dc.description.abstractThe structural parameters of gaseous trimethylphosphine, including standard errors, were found to be as follows: center of gravity bond distances were rCP=1.8465±0.003 A, and rCH=1.091±0.006 A; angles were <C☒P☒C=98.6±0.3°, and <P☒C☒H=110.7±0.5°; root‐mean‐square amplitudes of vibration were lCP=0.054±0.003 A, lCH=0.073±0.006 A, lP— —H=0.110±0.006 A, and lC— —C=0.084±0.005 A. The methyl groups were observed to be in staggered configurations analogous to those in ethane, with rotational barriers probably 1.5 kcal/mole or higher. A brief structural comparison with halogen derivatives and hydrides is presented.en_US
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dc.format.extent349935 bytes
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dc.publisherThe American Institute of Physicsen_US
dc.rights© The American Institute of Physicsen_US
dc.titleElectron Diffraction Study of the Structure of Trimethylphosphineen_US
dc.typeArticleen_US
dc.subject.hlbsecondlevelPhysicsen_US
dc.subject.hlbtoplevelScienceen_US
dc.description.peerreviewedPeer Revieweden_US
dc.contributor.affiliationumDepartment of Chemistry, University of Michigan, Ann Arbor, Michiganen_US
dc.contributor.affiliationotherDepartment of Chemistry, Iowa State University, Ames, Iowaen_US
dc.description.bitstreamurlhttp://deepblue.lib.umich.edu/bitstream/2027.42/70229/2/JCPSA6-32-2-512-1.pdf
dc.identifier.doi10.1063/1.1730726en_US
dc.identifier.sourceThe Journal of Chemical Physicsen_US
dc.identifier.citedreferenceSee for example R. S. Mulliken, J. Am. Chem. Soc. 77, 887 (1955); W. Kolos, J. Chem. Phys. 23, 1554 (1955); C. E. Mellish and J. W. Linnett, Trans. Faraday Soc. 50, 657 (1954); and articles to which the above papers refer.en_US
dc.identifier.citedreferenceD. R. Lide, Jr., and D. E. Mann, J. Chem. Phys. 29, 914 (1958).en_US
dc.identifier.citedreferenceL. O. Brockway and L. S. Bartell, Rev. Sci. Instr. 25, 569 (1954).en_US
dc.identifier.citedreferenceL. S. Bartell and L. O. Brockway, J. Appl. Phys. 24, 656 (1953).en_US
dc.identifier.citedreferenceL. S. Bartell, J. Appl. Phys. 32, 252 (1960).en_US
dc.identifier.citedreferenceBartell, Brockway, and Schwendeman, J. Chem. Phys. 23, 1854 (1955).en_US
dc.identifier.citedreferenceJ. A. Ibers and J. A. Hoerni, Acta Cryst. 7, 405 (1954).en_US
dc.identifier.citedreferenceR. A. Bonham and L. S. Bartell, J. Chem. Phys. 31, 702 (1959).en_US
dc.identifier.citedreferenceThe term rgrg corresponds to the rg(0)rg(0) of L. S. Bartell, J. Chem. Phys. 23, 1219 (1955).en_US
dc.identifier.citedreferenceR. A. Bonham and L. S. Bartell, J. Am. Chem. Soc. 81, 3491 (1959).en_US
dc.identifier.citedreferenceLide reported the angle H‐C‐H. In the present comparison it seemed preferable to avoid converting the diffraction ∠P‐C‐H to ∠H‐C‐H, as the operational (rg)(rg) diffraction angles may not transform according to simple geometrical laws. Spectroscopic angles, which are intrinsically no more precisely denned at present, do transform simply (by hypothesis), since the individual angles are not independently defined.en_US
dc.identifier.citedreferenceD. W. J. Cruickshank and A. P. Robertson, Acta Cryst. 6, 698 (1953).en_US
dc.identifier.citedreferenceL. S. Bartell, J. Chem. Phys. 23, 1219 (1955); P. M. Morse, Phys. Rev. 34, 57 (1929).en_US
dc.identifier.citedreferenceH. D. Springall and L. O. Brockway, J. Am. Chem. Soc. 60, 996 (1938).en_US
dc.identifier.citedreferenceH. J. M. Bowen, Trans. Faraday Soc. 50, 783 (1954).en_US
dc.identifier.citedreferenceV. Schomaker quoted by P. W. Allen and L. E. Sutton, Acta Cryst. 3, 46 (1950); R. L. Livingston and G. Vaughan, J. Am. Chem. Soc. 78, 4866 (1956).en_US
dc.identifier.citedreferenceBonham, Bartell, and Kohl, J. Am. Chem. Soc. 81, 4765 (1959).en_US
dc.identifier.citedreferenceL. S. Bartell and R. A. Bonham, J. Chem. Phys. 31, 400 (1959).en_US
dc.identifier.citedreferenceL. S. Bartell, J. Chem. Phys. (to be published).en_US
dc.identifier.citedreferenceRosenbaum, Rubin, and Sandberg, J. Chem. Phys. 8, 366 (1940).en_US
dc.identifier.citedreferenceD. R. Lide, Jr., and D. E. Mann, J. Chem. Phys. 28, 572 (1958).en_US
dc.identifier.citedreferenceL. E. Sutton, Tables of Interatomic Distances and Configuration in Molecules and Ions (The Chemical Society, London, 1958).en_US
dc.identifier.citedreferenceThe empirical generalizations of Mellish and Linnett (reference 1) regarding these compounds fail in the comparison of PF3PF3 and PH3,PH3, and hence cannot be expected to apply in the case of P(CH3)3.P(CH3)3.en_US
dc.identifier.citedreferenceM. J. S. Dewar and H. N. Schmeising, Tetrahedron 5, 166 (1959).en_US
dc.identifier.citedreferenceL. S. Bartell, Federov Session on Crystallography, May 26, 1959, Leningrad, U.S.S.R. (to be published).en_US
dc.identifier.citedreferenceReference 17. In the calculation of the angle H‐C‐H from the angle C‐C‐H given in the reference, a slight correction has been made for the effect of the large amplitude of vibration of hydrogen atoms.en_US
dc.owningcollnamePhysics, Department of


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