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1 Dec 1938

Volume 6, Issue 12, pp. 749-908

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Diffuse Electron Diffraction Patterns

J. T. Burwell

J. Chem. Phys. 6, 749 (1938); http://dx.doi.org/10.1063/1.1750164 (3 pages) | Cited 4 times

Online Publication Date: 22 December 2004

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Diffuse electron diffraction patterns taken by reflection have in the past been cited as proof that the polished surfaces of metals are amorphous or very finely crystalline. In the present work it is shown that such patterns can be obtained from a large‐grained crystalline surface and hence cannot be due to an amorphous phase but rather to the physical contour of the surface.

The Ultraviolet Absorption Bands Ascribed to HNO2

D. M. Newitt and L. E. Outridge

J. Chem. Phys. 6, 752 (1938); http://dx.doi.org/10.1063/1.1750165 (3 pages) | Cited 4 times

Online Publication Date: 22 December 2004

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Attention is drawn to the similarity of a series of absorption bands obtained by Melvin and Wulf as the results of experiments at normal temperatures with a NO☒NO2☒H2O medium and by Bone and Newitt from the explosion of a CO☒H2O☒NO medium at high pressures. The formation of these bands in explosion experiments at atmospheric pressure and in static flames is described and evidence is brought forward which suggests that they may be due to the enhancement of certain bands of the normal NO2 absorption spectrum.

The Infra‐Red Absorption of Carboxylic Acids in Solution I. Qualitative Features

M. M. Davies and G. B. B. M. Sutherland

J. Chem. Phys. 6, 755 (1938); http://dx.doi.org/10.1063/1.1750166 (12 pages) | Cited 27 times

Online Publication Date: 22 December 2004

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The absorption spectra of solutions of acetic, benzoic and trichloracetic acids in carbon tetrachloride have been studied at various concentrations and temperatures in the neighborhood of 3μ, 6μ, and 7μ. At each of these regions is a double band, one component of which is due to the monomeric, the other to the dimeric form of the molecule. The relatively small shift in each case indicates that the molecule is not radically altered on association. The absorptions in the three regions studied were due respectively to the O☒H, the C☒O and the C☒O bonds of the COOH group. It has been possible to make a first estimate of these bond distances in the monomer and dimer, as follows (in A units):
math
The values for the C☒O and C☒O distances are in satisfactory agreement with those deduced by x‐ray methods for oxalic acid but not with those obtained by electron diffraction for formic acid. The general appearance and the temperature variation of the O☒H ``association'' band in these acids appears to be very similar to that of the corresponding band in the alcohols. This is evidence in favor of Badger's explanation of the width of such bands rather than Errera's.

The Infra‐Red Absorption of Carboxylic Acids in Solution II. Intensities

M. M. Davies and G. B. B. M. Sutherland

J. Chem. Phys. 6, 767 (1938); http://dx.doi.org/10.1063/1.1750167 (4 pages) | Cited 5 times

Online Publication Date: 22 December 2004

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The integral absorption of the monomeric OH band has been measured for solutions of acetic, benzoic and lauric acids in CCl4 at various concentrations and temperatures. At any given temperature the results indicate that the integrated intensity is roughly proportional to the amount of the monomer present, assuming that there is a monomer⇌dimer equilibrium. The temperature variation of the integrated absorption gave values for the heat of association varying from 6000 to 10,000 cal./g mole, which is considerably below the accepted value of 15,000 cal./g mole. This difference is attributed to the variation in the absorption coefficient with temperature. Equally anomalous results were obtained from measurements on the intensity of the monomeric C☒O band. The variation of the absorption coefficient with concentration and with temperature was checked independently on solutions of cetyl alcohol in CCl4.

An Infra‐Red Study of Omega‐Hydroxyundecanoic Acid in Carbon Tetrachloride

Mansel M. Davies

J. Chem. Phys. 6, 770 (1938); http://dx.doi.org/10.1063/1.1750168 (5 pages) | Cited 5 times

Online Publication Date: 22 December 2004

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An infra‐red examination of a long chain omega‐hydroxycarboxylic acid has provided evidence as to the inter‐ and intramolecular association of such molecules in solution: In particular, it is believed that the occurrence of a cyclic form of the monomeric molecules in solution has been proved.

Infra‐Red Bands of Methylamine and the Phenomenon of Free Rotation

H. W. Thompson and H. A. Skinner

J. Chem. Phys. 6, 775 (1938); http://dx.doi.org/10.1063/1.1750169 (4 pages) | Cited 5 times

Online Publication Date: 22 December 2004

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Two bands in the absorption spectrum of methylamine have been measured in the photographic infra‐red. One of the bands shows rotational structure. The bands have been interpreted as involving excitation of the frequencies 3νCH+νCN). The rotational structure of the latter band suggests that it is a perpendicular‐type band, and the precise spacing of the Q branches suggests that the molecule behaves approximately like a rigid symmetric top. The inference of hindered internal rotation is in agreement with other independent data.

Kinetics of OH Radicals Determined by Their Absorption Spectrum IV. Pressure Broadening and the Line Spectrum as Background

O. Oldenberg and F. F. Rieke

J. Chem. Phys. 6, 779 (1938); http://dx.doi.org/10.1063/1.1750170 (4 pages) | Cited 11 times

Online Publication Date: 22 December 2004

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For the measurement of the concentration of OH radicals the intensity of the absorption spectrum is measured more easily with an emission line background than with a continuous background, provided that the pressure broadening is known. The total broadening of the OH absorption lines at 1473° K and 1 atmos. (⅔O2+⅓H2O) is observed to be 0.58 cm—1; 36 percent of this value is Doppler broadening, the rest is pressure broadening. With this figure, recent intensity measurements of the OH bands by Avramenko and Kondratjew are reinterpreted. The resulting f values of approximately 3×10—4 are in reasonable agreement with our previous measurements. The conditions are discussed under which the simple method using the line spectrum as a background is applicable.

The Alpha‐Particle Reactions in Carbon Monoxide, Oxygen and Carbon Dioxide Systems

Joseph O. Hirschfelder and Hugh S. Taylor

J. Chem. Phys. 6, 783 (1938); http://dx.doi.org/10.1063/1.1750171 (8 pages) | Cited 7 times

Online Publication Date: 22 December 2004

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The methods developed by Eyring, Hirschfelder and Taylor for the analysis of the alpha‐particle reactions in hydrogen and hydrogen‐bromine systems have been extended to the corresponding reactions in carbon monoxide, oxygen, and carbon‐dioxide systems and to mixtures of these gases. It has been shown that experimentally known processes of ionization and of excitation, together with the probable neutralization processes, with consequent chemical reactions involving the atomic species so produced, suffice to account quantitatively for the observed experimental results. This extends the scope of the method employed to typical alpha‐particle reactions of decomposition, ozonization and oxidation hitherto interpreted in terms of a clustering mechanism.

Slow Electron Scattering and the Apparent Electron Affinity of Mercury

J. H. Simons and R. P. Seward

J. Chem. Phys. 6, 790 (1938); http://dx.doi.org/10.1063/1.1750172 (5 pages) | Cited 9 times

Online Publication Date: 22 December 2004

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The scattering of slow electrons by gaseous molecules is discussed with the object of explaining the curves obtained when the apparent scattering area is plotted against a function of the electron velocity. The peaks frequently observed at about the ionization potential for most substances and the abnormally high values for the alkali metals are explained as being due to the formation or presence of positive ions. The rise in the curves for some substances, as the accelerating potential is diminished below the ionization potential, is explained as the result of an attractive force between the electron and the neutral molecule. It is shown that this attractive force for mercury approximates an inverse fourth‐power law. From this law and an assumption of the diameter of the negative mercury ion, a reasonable value for the apparent electron affinity of mercury is calculated.

The Energy of the Triatomic Hydrogen Molecule and Ion, V

Joseph O. Hirschfelder

J. Chem. Phys. 6, 795 (1938); http://dx.doi.org/10.1063/1.1750173 (12 pages) | Cited 105 times

Online Publication Date: 22 December 2004

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In previous papers, the energy of H3 and of H3+ has been obtained by the variational method for linear configurations. In this treatment we are able to evaluate the difficult three center integrals for nonlinear configurations with the aid of the differential analyzer and to compute the energy of H3 and of H3+ as a function of the angle between the nuclei. The excited states as well as the ground states are considered. Direct comparison of calculated energy values for the equilateral triangle show that the molecular orbital approximation is inferior to the method of homopolar bond functions. The triatomic hydrogen molecule has its lowest energy for linear configurations. The angle dependence calculated by the variational method agrees well with that calculated on the basis of the Eyring semi‐empirical scheme. By the theorem of Jahn and Teller there could not be a minimum in the energy for the equilateral triangle, as here the lowest electronic state is doubly degenerate. The triatomic hydrogen ion, H3+, is very stable (when left to itself) and has an energy lower by more than 184. kcal. than two separated hydrogen atoms and a proton. Thus the chemical reaction:
math
is certainly exothermic by more than 11 kcal. and probably is exothermic by 38 kcal. The triatomic hydrogen ion has a stable configuration corresponding to separation between the nuclei of about 1.79A with the nuclei lying intermediate between a right and an equilateral triangle. The vibration frequencies of H3+ are estimated but their exact value as well as the exact configuration of the stable state are somewhat in doubt. Two of these frequencies should be infra‐red active and susceptible to direct experimental measurement.

Integrals Required for Computing the Energy of H3 and of H3+

Joseph O. Hirschfelder and Cornelius N. Weygandt

J. Chem. Phys. 6, 806 (1938); http://dx.doi.org/10.1063/1.1750174 (5 pages) | Cited 29 times

Online Publication Date: 22 December 2004

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Some of the difficult integrals required for the variational method calculation of the energy of the triatomic hydrogen molecule and positive ion were evaluated with the aid of the differential analyzer. The integral ∫ 0πexp(−B(1−A cos θ)½)dθ is tabulated for a complete range of the parameters, A and B. The integral K(c,ab) = (1/π) ∫ rc−1exp(−ra−rb)dτ is tabulated for many configurations of the three electrons or nuclei: a, b, and c. Numerical tables are given of all of the integrals occurring in the Sugiura treatment of the ground state of H2. The values of all of the other integrals used in the calculation of the energy of H3 and of H3+ are given. It is expected that these tables will be useful for many problems of molecular quantum mechanics.

The Reaction of Hydrogen Atoms with Carbon Tetrachloride

John E. Vance and W. C. Bauman

J. Chem. Phys. 6, 811 (1938); http://dx.doi.org/10.1063/1.1750175 (8 pages) | Cited 3 times

Online Publication Date: 22 December 2004

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Reaction rate constants have been obtained at seven temperatures between 21° and 200° for the reaction H+CCl4=HCl+CCl3. The change of reaction rate with temperature is satisfactorily represented by the classical bimolecular reaction theory with a steric factor of 0.007 and an activation energy of 3.45 kcal. per mole. A comparison of the amount of HCl formed with the number of hydrogen atoms entering indicates that complete conversion of atomic hydrogen into HCl by the reaction may be attained at 150–200° under conditions which are determined in the experiments.

The Calculation of Bond Strengths from Photochemical Evidence

Milton Burton

J. Chem. Phys. 6, 818 (1938); http://dx.doi.org/10.1063/1.1750176 (6 pages) | Cited 12 times

Online Publication Date: 22 December 2004

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When predissociation manifests itself in polyatomic molecules by a sudden broadening of the rotation lines of a discrete absorption spectrum, a close correspondence is to be expected between the beginning of the predissociation region and the strength of the bond involved. This principle is used to calculate the bond strengths of C☒C in ethane, acetaldehyde, acetone and free acetyl (values: 72.1, 93.1, 96.5 and — 19.4 kcal., respectively) and of C☒H in methane, acetaldehyde O(CH3C−H), formaldehyde and free formyl (values: 94.8, 114.7, 103.3, and 0.1 kcal., respectively), where the bond strength is defined in reference to the state of the molecule at 0°K. Assuming the validity of the method, the bond strength values given are shown to be accurate within 1.0 kcal. The limitations of the method as well as some implications of the results are indicated.

The Optical Activity of Secondary Butyl Alcohol

Everett Gorin, John Walter, and Henry Eyring

J. Chem. Phys. 6, 824 (1938); http://dx.doi.org/10.1063/1.1750177 (9 pages) | Cited 17 times

Online Publication Date: 22 December 2004

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A calculation of the optical activity of secondary butyl alcohol is presented based upon a one‐electron model. The chromophoric electron is considered to be one of the nonbonding electrons on the oxygen atom. This electron is considered to be moving in a field of the other nuclei and electrons considered as charge distributions. The fields of the other electrons are obtained from the Slater type eigenfunctions for the various atoms. This amounts to a rough solution of the Hartree approximation for the chromophoric electron. The results obtained are somewhat larger or somewhat smaller than the experimental value depending on the exact orientation of the groups in their rotation about single bonds. The assignment of an absolute configuration in these calculations follows provided the exact orientation of the rotating groups is known. The orientations which we consider most likely lead to an assignment of the absolute configuration in agreement with that of Kuhn.

A Kinetic Approach to the Theory of Conductance of Infinitely Dilute Solutions, Based on the ``Cage'' Model of Liquids

Milton J. Polissar

J. Chem. Phys. 6, 833 (1938); http://dx.doi.org/10.1063/1.1750178 (12 pages) | Cited 22 times

Online Publication Date: 22 December 2004

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Attention is called to the disparity between the hydrodynamic model of an electrolytic solution and its physical counterpart. The ``cage'' theory of liquids is reviewed, and some of its equations developed with the purpose of bringing to the surface the underlying assumptions. A quantitative comparison is carried out between the behavior of an ion subject to Brownian motion and that of the placidly moving ion of the hydrodynamic theory. The conclusion is drawn that the tremendous difference between the two models casts doubt upon the validity of the hydrodynamic equations. The possibility is mentioned that the hydrodynamic theory, while giving fortuitously approximately correct values of ionic radii, may still be incorrect in its theoretical implications. Stress is laid on the desirability of a kinetic theory of electrolytic conductance. An approach to a kinetic theory is made, based on the cage model of liquids. In this method, the ionic migration is considered as the cumulative effect of a feeble, sporadic, but directed perturbation of the violent but random Brownian movement. The method leads to an experimentally substantiated relation between the diffusion and the conductivity of an electrolyte. It offers a plausible explanation of the high temperature coefficient of the slow‐moving ions. For the ions of an infinitely dilute aqueous solution of potassium chloride, the method yields the following data: Heat of activation for a cage‐to‐cage jump, 4230 calories; frequency of cage‐to‐cage jumps, 1.12×1011 sec.—1; frequency of oscillation within the cage, 8.3×1013 sec.—1; average number of oscillations in each cage, 740.

An Equation for Transference Numbers

Theodore Shedlovsky

J. Chem. Phys. 6, 845 (1938); http://dx.doi.org/10.1063/1.1750179 (2 pages) | Cited 3 times

Online Publication Date: 22 December 2004

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The following transference number equation is proposed,
math
The values for the constant A are in accord with the Onsager theory for most uni‐univalent electrolytes in water, but not for abnormal salts, such as silver nitrate, or for higher valence salts. However, the transference equation appears to have quite general applicability.

Molecular Interaction in Mixed Monolayers on Aqueous Subsolutions I. Mixtures of Alcohols, Acids and Amines

William D. Harkins and Robert T. Florence

J. Chem. Phys. 6, 847 (1938); http://dx.doi.org/10.1063/1.1750180 (9 pages) | Cited 10 times

Online Publication Date: 22 December 2004

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Mixed films are of fundamental importance in biological systems, so mixtures of long chain alcohols, acids, and amines on acidic and basic subsolutions have been investigated. The principal effect of mixing is to change the conditions with respect to the pressure, area, and temperature at which one surface phase changes into another.
In general a mixture of two liquid films gives a monolayer of the same type, with the mean molecular area: a liquid expanded film is made more condensed by admixture of a substance which gives a condensed film, and the condensing action increases with the length of the hydrocarbon chain; an alcohol condenses an acid more than the corresponding acid. The interaction, or departure from the mean value may be either positive or negative, and on acid subsolutions is greatest when one of the components is an amine. Only in amine‐acid mixtures is there an indication of chemical action. The 1 : 1 mixture of stearyl alcohol and stearic acid ``freezes'' at a much larger area than the film given by either component, so the area of the solid mixed film is abnormally high. The area interaction with an amine present is negative, and the potential interaction has a high value and is positive. Calcium ions in a basic subsolution condense a Type II to a solid Type I monolayer.

Molecular Interaction in Mixed Monolayers II. Unstable Mixtures with Unsaturated Acids

Robert T. Florence and William D. Harkins

J. Chem. Phys. 6, 856 (1938); http://dx.doi.org/10.1063/1.1750181 (5 pages) | Cited 6 times

Online Publication Date: 22 December 2004

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This investigation concerns the effect of the form of a molecule, with otherwise identical composition and structure, on its binding to the acidic or basic water of the subphase and to the molecules of the film itself. The binding to the water by the carboxyl group should be approximately the same for stearic acid and for the unsaturated acids, oleic and elaidic acid, with the double bond in the middle of the hydrocarbon chain. By compression of the film oleic acid may be squeezed out practically completely, from a mixed monolayer in which a saturated long chain alcohol, acid, or amine is the other constituent. Thus the energy of binding of the oleic acid to the other molecules in the film is weaker than that between the saturated molecules. However, earlier work in this laboratory has shown that the presence of the double bond does not decrease, but very slightly increases, the attraction between molecules.
Thus it seems to be the shape of the molecule which reduces the energy of binding of oleic acid in the film. Oleic acid is a cis form, so a nine carbon atom chain R2 is bent backward with respect to the other 9C chain R1 which ends in the carboxyl group. It may be assumed that the whole molecule is free to rotate, with the carboxyl group in contact with the water, and that the group R2 is free to vibrate or ``flagellate.'' Thus the oleic acid molecule would occupy a larger area than a saturated acid and this increased distance together with a lessening of the length of the contact between this and the other molecules in the film, decreases greatly the energy of binding. Space models of oleic and elaidic acid have been used in the study of these relations.
By a greater straightening of the chain, as in the transcompound, elaidic acid, the energy of binding should become intermediate between that of oleic and stearic acid, and much above that for oleic acid. On this basis compression should segregate elaidic acid slightly from the mixed film, but by no means completely, and this is what the experiments demonstrate.

Migration and Photochemical Action of Excitation Energy in Crystals

James Franck and Edward Teller

J. Chem. Phys. 6, 861 (1938); http://dx.doi.org/10.1063/1.1750182 (12 pages) | Cited 106 times

Online Publication Date: 22 December 2004

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A crystal which has absorbed a light quantum can be treated either as an assembly of molecules or else as a giant molecule. If the exchange of excitation energy between crystal cells is slow as compared to the periods of vibration, the first description is preferable; if it is fast, the second picture is better. Both cases are discussed in connection with the following question: To what extent can excitation energy absorbed by an arbitrary cell of the crystal be used photochemically at a specific point which may be far removed from the absorbing cell? The results are applied to the behavior of polymerized pseudoisocyanines, to the hypothetical photosynthetic unit and to the theory of sensitized photographic plates.

The Role of Attractive and Repulsive Forces in the Formation of Tactoids, Thixotropic Gels, Protein Crystals and Coacervates

Irving Langmuir

J. Chem. Phys. 6, 873 (1938); http://dx.doi.org/10.1063/1.1750183 (24 pages) | Cited 235 times

Online Publication Date: 22 December 2004

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The formation of tactoids from thixotropic sols, of Schiller layers from iron‐oxide sols, the separation of tobacco virus solutions and bentonite sols into two liquid layers and the crystallization of proteins are regarded as examples of unipolar coacervation (micelles having like charges) which must involve attractive forces.
Kallmann, Willstätter, Freundlich, De Boer, Hamaker, Houwink and others have assumed that the attraction is due to van der Waals forces. They have also analyzed the stability of colloid systems by diagrams giving the potential energy as a function of the distance between micelles. It is now shown that the Coulomb attraction between the micelles and the oppositely charged ions in the solution gives an excess of attractive force which must be balanced by the dispersive action of thermal agitation and another repulsive force. Thus there is no need to assume long range van der Waals forces. The past use of energy diagrams is criticized because it has ignored the effect of the thermal agitation and the attraction of the ``gegenions'' in solution. Instead of potential energy it is proposed that osmotic pressure p be used, which includes these previously neglected factors. A maximum in p as the colloid concentration increases is the condition for the separation into two phases (coacervation).
The Debye‐Hückel theory (1st approximation) for the osmotic pressure of electrolytes takes into account both these factors and permits a rough calculation of the conditions under which coacervation occurs. The 2nd approximation, which considers particle size, does not agree as well with experiment as the first approximation. The reasons for this lack of agreement are discussed.
The micelles in unipolar coacervates are not in contact, but are separated by relatively large distances (10–5000A). Either a specific repulsive force or a decrease in the Coulomb attraction as the concentration increases (due to decreased charges on micelles) can account for stable coacervates. The assumption of a definite ζ‐potential, rather than a definite charge on the micelles, gives automatically just such a decrease in attraction.
The general mathematical theory of coacervation presents great difficulties because the approximations of the Debye‐Hückel theory cannot be used. However, the one‐dimensional problem of the forces acting between parallel colloidal platelets can be solved rigorously in terms of elliptic integrals. For highly charged particles in sufficiently dilute solutions of electrolytes, the pressure p in the liquid between the two plates is given by p = (π/2)D(kT/eb)2 = 8.9×10—7/b2 dynes/cm2 where b is the distance in cm between the plates and D is the dielectric constant (81 for water at T = 293°K). This pressure which tends to force the plates apart is independent of the charge on the plates and on the electrolyte concentration (univalent ions only). Polyvalent ions decrease the force. This force is of the right magnitude to account for the stability of unipolar coacervates. It also furnishes a quantitative explanation of the Jones‐Ray effect, by which low salt concentrations decrease the capillary rise in surface tension experiments with water.
Experimental determinations were made of the relaxation times τ for the decay of birefringence in bentonite and vanadium pentoxide sols, after stirring was stopped. In one sample of bentonite, τ varied with the 22nd power of the concentration, while in V2O5 sols the exponent was 1.8. The temperature coefficients of τ were also measured and the activation energies were calculated.
A theory of the relaxation of birefringence was developed, according to which the micelles in dilute thixotropic bentonite sols are arranged normally in a cubic lattice (isotropic). Temporary shear in the liquid orients the micelles and produces birefringence although the lattice remains cubic. The experimental data confirm the theory and indicate that the energy barrier opposing reorientation of micelles in a particular bentonite sol varied with the inverse 20th power of the distance between the micelles. With V2O5 this exponent was about 4. Further support for the theory was obtained by experiments which gave ``angles of isocline'' for bentonite particles in a flowing sol that varied from 65° to 78°.
In bipolar coacervates (which contain micelles of unlike polarities) the electric fields and the charges on the micelles increase as the micellar concentration increases. When a certain concentration is reached, the field rises to a value so high as to cause increased hydration which holds the micelles apart and gives stability to the coacervate.

Quadrupole Contributions to London's Dispersion Forces

Henry Margenau

J. Chem. Phys. 6, 896 (1938); http://dx.doi.org/10.1063/1.1750184 (4 pages) | Cited 43 times

Online Publication Date: 22 December 2004

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The contribution of terms in R—8 and R—10 to the dispersion forces is expressed by a simple, approximate formula (Eq. (7)) involving only measurable quantities (polarizability, absorption frequency, oscillator strength). The formula is applicable when the dispersion curve of the substance can be represented with the use of a single resonant frequency. Numerical values of the terms in question are calculated for a number of molecules (Table II). Except in the case of the alkalies, where the convergence of the sequence in inverse powers of R fails at distances around 6A, the R—10 term is generally negligible, while the R—8 term contributes appreciably in the region of the van der Waals minimum.

Internal Rotation of Propane and Propylene; the Origin of the Internal Restricting Potentials

G. B. Kistiakowsky, J. R. Lacher, and W. W. Ransom

J. Chem. Phys. 6, 900 (1938); http://dx.doi.org/10.1063/1.1750185 (2 pages) | Cited 12 times

Online Publication Date: 22 December 2004

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A Note on the Raman Spectra of Nitrogen

Charles E. Miller

J. Chem. Phys. 6, 902 (1938); http://dx.doi.org/10.1063/1.1750186 (3 pages) | Cited 2 times

Online Publication Date: 22 December 2004

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Correction: On the Paramagnetic Conversion of Parahydrogen and Orthodeuterium in the Presence of Nitrous Oxide (The Magnetic Moment of the Deuteron)

L. Farkas and U. Garbatski

J. Chem. Phys. 6, 904 (1938); http://dx.doi.org/10.1063/1.1750187 (1 page)

Online Publication Date: 22 December 2004

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The Dielectric Polarization of Formic Acid Vapor

I. E. Coop, N. R. Davidson, and L. E. Sutton

J. Chem. Phys. 6, 905 (1938); http://dx.doi.org/10.1063/1.1750188 (1 page) | Cited 11 times

Online Publication Date: 22 December 2004

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