Measurements of depolarization ratios and polarizability anisotropies of gaseous molecules

Baas, F.; Hout, K. D. van den

doi:10.1016/0378-4371(79)90035-9

Cited by 72 publications

(13 citation statements)

References 13 publications

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“…'See Ref. 13. mA relatively large uncertainty of ± 3x 10-4 has been placed on all values of p which do not specifically exclude vibrational Raman interferences (see text).…”

Section: Molecular Observablesmentioning

confidence: 99%

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An interacting segment model of molecular electric tensor properties: Application to dipole moments, polarizabilities, and hyperpolarizabilities for the halogenated methanes

Miller

Orr

Ward

1981

The Journal of Chemical Physics

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Articles you may be interested inNonmetallic electronegativity equalization and point-dipole interaction model including exchange interactions for molecular dipole moments and polarizabilities J. Chem. Phys. 131, 044101 (2009); 10.1063/1.3166142 Accurate electric dipole and quadrupole moment, dipole polarizability, and first and second dipole hyperpolarizability of ozone from coupled cluster calculations A complete description of the electric dipole moment, polarizability, and hyperpolarizability tensors of hydrogen peroxide J. Chem. Phys. 96, 6048 (1992); 10.1063/1.462646 An interacting segment model of molecular electric tensor properties: Theory and application to electric dipole moments of the halogenated methanes A group-dipole interaction model of the molecular polarizability and the molecular first and second hyperpolarizabilities A previously developed interacting segment model [ISM-see J. Chern. Phys. 67, 2109Phys. 67, (1977] is applied to a full-scale treatment of the electric dipole moments, isotropic and anisotropic polarizabilities, and hyperpolarizabilities of a series of t 2 halogenated methane molecules CXn Y 4-n(X, Y = H,F ,Ct; n = 0-4). The ISM scheme enables the molecular properties considered to be fitted in terms of a set of "bare" electric tensor parameters for each bond, which are modified ("dressed") by intramolecular electrostatic interactions. The computed results of the ISM scheme, and of a corresponding interaction-free bond additivity model, are discussed in relation to the following: choice of geometric and bond parameters, quality of fit to experimentally determined molecular and bond properties, and predictive potential and general physical validity of the model. It is concluded that the ISM approach represents a substantial improvement over simple bond additivity as a basis for understanding molecular electric tensor properties.An optical polarizability anisotropy which contributes directly to the Kerr effect 4858

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“…'See Ref. 13. mA relatively large uncertainty of ± 3x 10-4 has been placed on all values of p which do not specifically exclude vibrational Raman interferences (see text).…”

Section: Molecular Observablesmentioning

confidence: 99%

“…(16); (x) evaluate J3~ and ~i from Eqs. (13) and (17); (xi) evaluate Y~ and Y I from Eqs. (14) and (18); (xii) evaluate mOlecular observables using the dressed bond parameters calculated in steps (vii)-(xi) and the molecular geometry from step (i);…”

Section: Theory and Computational Proceduresmentioning

confidence: 99%

An interacting segment model of molecular electric tensor properties: Application to dipole moments, polarizabilities, and hyperpolarizabilities for the halogenated methanes

Miller

Orr

Ward

1981

The Journal of Chemical Physics

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“…(10). Unfortunately, the only other depolarization ratio measured for O 2 at 632.8 nm, namely the 100 0 = (2.9 ± 0.1) obtained by Baas and van den Hout [22], is some 4.2% smaller than Bridge and Buckingham's value. As Bogaard et al have argued [23], while the precision of a set of 0 values measured by a given investigator can be as high as 0.5% or better, the determinations of different investigators can be discrepant by as much as 4%, so that the accuracy of depolarization ratios is assumed to be no better than ≈±3%.…”

Section: Experiments and Resultsmentioning

confidence: 89%

“…If the ˛ of Baas and van den Hout (together with its uncertainty quoted in [22]) is used instead of that of Bridge and Buckingham, the combined 15 measurements yield a quadrupole moment of = (−1.062 ± 0.042) × 10 −40 C m 2 .…”

Section: Experiments and Resultsmentioning

confidence: 99%

The electric quadrupole moment of O 2

Couling¹,

Ntombela²

2014

Chemical Physics Letters

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“…Optical-polarizability anisotropies for these molecules have been obtained previously from measurements of depolarized Rayleigh scattering. 2 " 5 The linear polarizability anisotropy is relevant to an understanding of a broad range of molecular properties, including the Kerr effect and longrange intermolecular interactions. 6 It is also pivotal in determining the adequacy of molecular models: The bond-additivity model, which appears adequate for the isotropic polarizability, fails for the anisotropic polarizability.…”

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confidence: 99%

Polarizability Anisotropies of CO2,N2O, and OCS from Measuremen

Elliott

Ward

1981

Phys. Rev. Lett.

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Intensity-dependent dispersion of the refractive index has been measured in gaseous C0 2 , N 2 0, and OCS with use of a single-path, double-frequency interference technique. The measurements yield molecular optical-polarizability anisotropics (Ace = a^ -a ± ): Aa(N 2 0) = 2.92(12) A 3 , Ace(OCS) = 4.04(17) A 3 relative to Aa(CQ 2 ) = 2.11 A 3 . These results are in good agreement with existing data. extracted from the measurements.Third-order polarizabilities are also

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Measurements of depolarization ratios and polarizability anisotropies of gaseous molecules

Cited by 72 publications

References 13 publications

An interacting segment model of molecular electric tensor properties: Application to dipole moments, polarizabilities, and hyperpolarizabilities for the halogenated methanes

An interacting segment model of molecular electric tensor properties: Application to dipole moments, polarizabilities, and hyperpolarizabilities for the halogenated methanes

The electric quadrupole moment of O 2

Polarizability Anisotropies of CO2,N2O, and OCS from Measuremen

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