' N Eq. (28), 0.11.87 should be replaced by +~ (0.1173). J ls In the third member of Eq. (32), 15/8 should be replaced by 15/32. On the top of page 8, 0.96 Nk/2S should be replaced by 0.96 (2NkS). In Eq. (97), a term —NzJS should be added to the right-hand sIde. In Eq. (120), 0.1187 should be replaced by 0.1173/(SI—S2) and 2JSIS2 should be replaced by 4JSIS2. Below Eq. (121), SIS2/S{SI—S2) should appear as twice this quantity, and (gIS&—g2S&)p should appear multiplied by a factor (q).

Comparative Study of Potential Energy Functions for Diatomic Molecules

Publisher Summary Attractive forces of different orders of magnitude can occur between two neutral atoms or molecules. If the electron spins of two approaching atoms are parallel or if one or both of the partners are rare gas atoms, or molecules for which chemical bonding is not possible, only an extremely weak attractive potential is observed. This potential has a maximum depth of only 10 ˉ 3 to10 ˉ 1 eV and extends out to distances of about > 10 A, which is large compared with the gas kinetic radius of the partners; this phenomena is called the van der Waals potential. If, on the other hand, the two atoms can form a stable molecule (antiparallel electron spins), an extremely strong attractive potential appears at smaller distances of approach. A strong attractive potential may also appear if an atom or molecule reacts with another molecule. In both instances, the potential may have a depth of several electron volts, corresponding to, in the case of two atoms, the dissociation energy of the stable molecule. This is called the chemical potential. If chemical forces exist, the van der Waals potential are observable only at very large separations. At very close distances of approach, these attractive potentials are more than compensated for by an extremely strong rapidly rising repulsive potential. Moreover, in the interaction of two atoms, the quantum mechanical dispersion force is largely responsible for the attractive potential. This potential comes about due to the mutual perturbation of the electrons in the two atomic systems.

The Study of Intermolecular Potentials with Molecular Beams at Thermal Energies

A vacuum ultraviolet monochromator has been combined with a mass spectrometer to study photoionization processes between 1570 and 430 A. Monochromatic photons were used to ionize, A, He, Ne, O2, N2, CO, NO, CO2, N2O, and NO2; and preliminary measurements of ion intensity as a function of photon energy have been obtained for the parent ions together with their fragments. The appearance of ionization and the structure of curves, in which ions per unit photon flux versus λ are plotted, will be related to previously reported energy levels, to photoionization cross sections, and to dissociative photoionization mechanisms.

Photoionization Analysis by Mass Spectroscopy

Cross Sections for the Excitation of the Metastable 2s State of Atomic Hydrogen by Electron Collision

The electron-induced dissociation of nitrogen by essentially monoenergetic electrons has been studied in a mass spectrometer. It has been found that there are three ways by which the atomic nitrogen ions are produced, namely, those in which the accompanying nitrogen atom is produced in its three states, 4 S 0 , 2 D 0 , and 2 P 0 ; the atomic nitrogen ion being always formed in its ground ( 3 P ) state. The appearance potentials at which these three processes occur lead unequivocally to the conclusion that the dissociation energy of the nitrogen molecule is 9·756 eV.

The dissociation energy of the nitrogen molecule

An attempt has been made to observe the thermal dissociation of N2 in order to choose between the two values, 7385 ev and 9765 ev, for the dissociation energy of N2 At the highest available temperatures no dissociation could be observed, and a lower limit of 880 ev is set for D(N2)

Dissociation Energy of N2

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Dissociation Energy of N2