An ab initio study of some noble gas monohalides
|
|
- Antonia Hubbard
- 6 years ago
- Views:
Transcription
1 JOURNAL OF CHEMICAL PHYSICS VOLUME 114, NUMBER 5 1 FEBRUARY 2001 An ab initio study of some noble gas monohalides Gerald J. Hoffman a) and Mitchell Colletto Department of Chemistry, The College of New Jersey, P. O. Box 7718, Ewing, New Jersey Received 15 September 2000; accepted 10 November 2000 Results from high-level ab initio calculations on NeF, ArF, KrF, XeF, and XeCl are reported and compared to experiment and to previous calculations. CCSD T results for NeF and ArF ground state potentials show agreement with experimental potentials to within the probable uncertainty of the measurement. In addition to CCSD T, multireference averaged coupled-pair functional calculations are performed on KrF, XeF, and XeCl as well as calculation of spin orbit coupling of the noble gas atom. Very good agreement with experiment is observed for XeF using this technique, while poor agreement is observed for KrF; this casts some doubt on the experimental potential for KrF. Results for XeCl show semiquantitative agreement with experiment. Finally, the potentials for the charge-transfer states of XeF, XeCl, and KrF and their spectroscopic constants are presented. Improved agreement over previous calculations is observed with some experimental measurements of these constants, for XeCl in particular American Institute of Physics. DOI: / I. INTRODUCTION The noble gas monohalides, as a class of molecules, share some unusual and interesting properties. Their most important property, from a practical point of view, is the use of many of these molecules as the lasing medium in highpowered excimer lasers. The ground states of all of these molecules are weakly bound compared to typical covalently bound molecules; however, because excitation involves a net transfer of an electron from the noble gas atom to the halogen atom, the excited states are very strongly bound, held together by electrostatic attraction between the noble gas cation and the halide anion. These ground and excited state properties are what make the noble gas halides good laser media, as there is a large transition moment between the ground state and two of the charge-transfer states, and the respective bonding properties of the upper and lower states guarantee a population inversion. The importance of these molecules as laser media, as well as their unusual behavior, provides motivation for trying to understand them better. Many experimental studies have been performed on the noble gas monohalides in order to characterize their molecular potentials. Gas-phase fluorescence and photoassociation studies 1 11 and matrix isolation studies have provided much information about both the excited and ground states of some of these molecules. Atomic scattering studies have given detailed information about the ground state potentials, as well as the two other low-lying neutral states However, there have only been a limited number of computational studies on these molecules The most significant early calculations 20,21 provided a vivid picture of the chargetransfer states of the noble gas monofluorides and the xenon monohalides at a time when little was known about them; yet despite the useful information these papers still contain, the authors computational technique gave repulsive ground a Author to whom correspondence should be addressed. states, in contradiction to the experimental result. More recently, two ab initio studies have been published that succeed in showing minima in the ground state potentials for some of these molecules. 23,24 It is necessary to implement a computational technique that includes a high degree of electron correlation in order to obtain such minima. In the present study, we show the results of ab initio calculations on NeF, ArF, KrF, XeF, and XeCl using a variety of techniques and basis sets; the resulting potentials for each molecule are then compared to the corresponding experimental potential. Coupled-cluster theory calculations including singles, doubles, and noniterative triples CCSD T were applied to all of these molecules to determine their ground state potentials. The CCSD T potentials for NeF and ArF agree quite well with experiment, but significant deviation between calculation and experiment is observed for KrF, XeF, and XeCl. For these three molecules, multireference averaged coupled-pair functional MR-ACPF calculations were performed in order to take into account some of the mixing of neutral and charge-transfer states that is known to occur. 20,21 In general, agreement between the MR-ACPF potentials and experiment is significantly better. Finally, the effect of the spin orbit SO coupling of the noble gas atom is calculated from the MR-ACPF results, and its influence on the potential is assessed in each case. Also, in performing MR-ACPF-SO calculations, potentials for the lowest six states of each molecule were obtained, that is, the three neutral or covalent states, and the three charge-transfer or ionic states. The ionic potentials are also compared with experimental results, as well as previous calculations. II. COMPUTATIONAL DETAILS All calculations were performed on the Cray T90 at the San Diego Supercomputer Center SDSC using either GAUSSIAN or MOLPRO The following basis sets were used for the noble gases: /2001/114(5)/2219/9/$ American Institute of Physics
2 2220 J. Chem. Phys., Vol. 114, No. 5, 1 February 2001 G. J. Hoffman and M. Colletto TABLE I. Exponents for polarization and diffuse subshells augmenting basis sets used for various atoms. Atom, basis set Polarization subshell exponent Diffuse subshell exponent Ne, SC d s f p Ne, STUT s p Ar, SC d s f 0.90 p Ar, STUT s p Kr, STUT f s 0.07 g 0.55 p 0.04 d 0.06 Xe, SC d a a s f 0.40 b p Xe, STUT c f s 0.03 g 0.55 p 0.02 d 0.05 F, AVQZ c s 0.07 p 0.04 d 0.06 Cl, mavtz s p d a Reference 30. b Reference 31. c Reference 23. AVTZ: The augmented triple-zeta correlation consistent basis sets of Dunning et al. AUG-cc-pVTZ 27,28 used without modification Ne and Ar only. SC: The so-called shape-consistent averaged relativistic effective core potential ECP basis sets of Christiansen et al. 28,29 augmented by s and p diffuse subshells Ne, Ar, and Xe. The XE basis set had in addition two d and one f polarization subshells. 30,31 Exponents for these additional subshells can be found in Table I. 29,30 STUT: The Stuttgart ECP basis sets of Nicklass et al. 28,32 including the polarization subshells provided, and augmented with s and p diffuse subshells. For Kr and Xe, this basis set was further augmented by replacing the single f polarization subshell with three f subshells, and adding a g polarization subshell and a d diffuse subshell also. 23 Exponents for these additional subshells can be found in Table I. Spin orbit ECPs are included for Kr and Xe, in order to allow the calculation of spin-orbit coupling in molecules containing these atoms. The following basis sets were used for the halogens, F and Cl: AVTZ: Same as above. mavtz: Same as AVTZ, except augmented with additional s, p and d diffuse subshells Cl only. Exponents for the diffuse subshells can be found in Table I. AVQZ: The augmented quadruple-zeta correlation consistent basis sets of Dunning et al. AUG-cc-pVQZ, 27,28 augmented with additional s, p, and d diffuse subshells F only. 23 Exponents for the diffuse subshells can be found in Table I. TABLE II. Spin orbit coupling calculations on Kr and Xe compared with experimental values energy in units of ev. Kr Xe MR-ACPF Experiment Coupled-cluster calculations were performed using both GAUSSIAN 94 and MOLPRO 98. CCSD T was the coupledcluster technique of choice because it has been shown previously to result in ground state minima for the xenon monohalides 23 and for KrF. 24 Inclusion of triply excited configurations had a significant influence on the quality of these earlier results. 23,24 For ArF, XeF, and XeCl, GAUSSIAN s CCSD T 33 option was used; results for KrF using this program have been published previously. 24 For NeF, KrF, XeF, and XeCl, the spin-restricted open-shell CCSD T option RCCSD T 34 of MOLPRO was used also. Earlier calculations have shown that there is a significant amount of multiconfigurational character to the ground state of the monohalides of the heavier noble gases Kr and Xe ; 20,21 this suggests the choice of a multireference technique might yield better results for these particular molecules. The multireference averaged coupled-pair functional option MR-ACPF, 35 one of the multireference configuration interaction MRCI techniques in MOLPRO, was chosen as a technique to study KrF, XeF, and XeCl as it has been used previously on XeF with good results. 23 However, as ACPF is only approximately size consistent, a calculation on each molecule is performed at large internuclear separation 50 Å in order to provide a reference energy for the separated atoms. The basis sets used were STUT including the SO ECP for the noble gas, and AVQZ for fluorine, or mavtz for chlorine. The wave functions resulting from a simultaneous multiconfigurational self-consistent field MCSCF calculation on the six lowest states three neutral and three charge-transfer were used as input for the MR- ACPF step. MR-ACPF calculations were performed for each symmetry of the MCSCF wave function 2 and the two Cartesian components of 2, and in each, two reference states were included neutral and charge-transfer. Note that these 6 states correspond to the six possible arrangements of 11 electrons in the 6 molecular orbitals of a diatomic molecule resulting from interaction of the outer p subshells of each. The energy of the lowest 2 state is taken to be the ground state energy. The MR-ACPF results for all six states, described above, were used to perform spin orbit calculations on KrF, XeF, and XeCl using MOLPRO with the STUT noble gas ECP basis sets, including the spin orbit ECPs. Again, this follows the lead of the previous study on XeF, 23 although we have chosen a different method by which to perform this calculation. Because all states are calculated simultaneously, they all have the same reference energy. Spin orbit couplings of the J 1/2 and J 3/2 states for Kr and Xe calculated using this technique compared with experimental values are shown in Table II. The calculated values are about 10% smaller than the experimentally measured values; as SO coupling is a
3 J. Chem. Phys., Vol. 114, No. 5, 1 February 2001 Noble gas halides 2221 relatively small component of the overall calculation, this level of agreement is judged to be sufficient for the purposes of this study. MOLPRO is capable of calculating spin orbit coupling either with all-electron basis sets, or with ECP basis sets, but not both in the same calculation. Hence, the spin orbit effects of the halogens are neglected by the chosen technique, as only all-electron basis sets were used for these atoms in our calculations. Calculations on XeCl were attempted using the STUT ECP basis sets for both Xe and Cl, including both spin orbit ECPs, but the resulting covalent potentials bore no resemblance to the experimental potentials, so this strategy was abandoned. Since the spin orbit couplings of the noble gas ions in the case of each molecule are more than ten times greater than those of the corresponding halogen atoms Xe ev and Kr ev vs F ev and Cl ev, one may assume that the couplings of the noble gases have the greatest influence, in effect justifying the approximation made in these calculations. However, at the outset, it is not clear how great an effect this approximation will have on the calculated potentials. Assuming the errors due to all of the other approximations implicit in these calculations do not dwarf the neglect of halogen spin orbit coupling, it is possible to judge the effect of this neglect after the fact, on comparison of the calculated potentials with the experimental ones. All calculated potentials were corrected for basis set superposition error BSSE point-by-point using the counterpoise technique. 36 While this technique does no better than estimate the BSSE, such a correction reduces an artificial bias toward dissociation energies that are too large, and bond lengths that are too small, 24 particularly for weakly bound species, such as those investigated in this work. In the specific case of the molecules reported on here, the differences between corrected and uncorrected bond lengths are quite small for the monofluorides 0.01 Å 0.08 Å, while that for XeCl is much more substantial 0.44 Å. FIG. 1. NeF potentials, computed using CCSD T and a variety of Ne basis sets, and corrected for BSSE, compared with experiment. III. RESULTS AND DISCUSSION A. Ground state potentials Calculated ground state potentials as compared with experimental potentials for NeF, ArF, KrF, XeF, and XeCl are shown in Figs. 1 5, respectively. The experimental curve shown in each plot is either the most recently published one, or the best accepted one from atomic scattering experiments ,37 1. NeF and ArF Of the molecules studied here, NeF and ArF are the most weakly bound, with dissociation energies less than 0.01 ev. Thus it is somewhat surprising that the calculated results agree with the experimental potentials for these two molecules as well as they do. Tables III and IV summarize the bond length and dissociation energy comparisons for NeF and ArF, respectively. All calculated bond lengths for NeF lie within 0.06 Å of its experimental value, while those for ArF lie within 0.12 Å of its experimental value. All calculated dissociation energies for both molecules lie within ev of their respective experimental values. These differences may well lie within uncertainties of the experimental potentials. Furthermore, the calculated and experimental potentials agree very well on the attractive portion, at separations greater than the minimum, proceeding toward separated atoms. This is significant because the scattering experiments from which these potentials originate 17,18 measure the attractive wall of the potential most accurately. 11 The forces that hold these two molecular species together are clearly van der Waals in nature. Hence, one gen- FIG. 2. ArF potentials, computed using CCSD T and a variety of Ar basis sets, and corrected for BSSE, compared with experiment.
4 2222 J. Chem. Phys., Vol. 114, No. 5, 1 February 2001 G. J. Hoffman and M. Colletto TABLE III. BSSE corrected CCSD T bond lengths and dissociation energies for NeF compared with experimental values. a Reference 18. Basis set R (Å) D e (ev) AVTZ/AVTZ SC/AVTZ STUT/AVTZ Experiment a FIG. 3. KrF potentials, computed using a variety of techniques and the STUT/AVQZ basis sets, and corrected for BSSE, compared with experiment. eral conclusion that can be drawn from these results is that CCSD T performs very well in describing van der Waals bound species. This should not be surprising, as other coupled-cluster studies have accurately determined the structures of van der Waals complexes, such as the triatomic noble gas Cl 2 complexes KrF and XeF Comparing the CCSD T results for KrF and XeF with experiment in Figs. 3 and 4, it is apparent that even with the inclusion of triply excited configurations, coupled-clusters is not giving a realistic picture of the bonding. While agreement on the attractive wall of the potential is reasonably good, the dissociation energy calculated using either CCSD T or RCCSD T falls far short of experiment. As has been stated previously, this can be ascribed to the shortcomings of single-reference coupled-cluster theory in properly accounting for the mixing of the covalent ground state with the ionic excited state of the same symmetry ( 2 ). Thus one expects that MR-ACPF will give a ground state potential closer to experiment. Furthermore, possible influence of SO coupling from the noble gas atom on the potential may be significant. Potentials for MR-ACPF and MR-ACPF-SO calculations are displayed in Figs. 3 and 4 also; bond length and dissociation energy data are summarized in Tables V and VI for KrF and XeF, respectively. For XeF, MR-ACPF shows a clear improvement in bond length and dissociation energy over the CCSD T results, and the MR-ACPF-SO result R e 2.34 Å, D e ev is very nearly in quantitative agreement with the experimental values R e 2.31 Å, D e ev, 17 and at least as good as the result of the most recent calculation R e 2.31 Å, D e 0.13 ev, but not BSSE corrected. 23 On the other hand, agreement between calculation and experiment on the attractive portion of the potential is not of the highest quality. This lack of agreement may be due to neglect of relativistic effects not taken into account by either the relativistic ECP for Xe or the technique of calculation. Correlated all-electron Dirac Fock calculations on XeF 2 and XeF 4 have resulted in quantitative agreement with experiment in bond length and dissociation energy, 39 and it is possible a similar treatment for XeF would show a higher level of quality than the results presented here. For KrF, the MR-ACPF potential lies just slightly below the one for RCCSD T, and including SO coupling has just a very small effect on this result. Despite good agreement between experiment and calculation on the attractive wall, none of the calculated bond lengths and dissociation energies are TABLE IV. BSSE corrected CCSD T bond lengths and dissociation energies for ArF compared with experimental values. Basis set R (Å) D e (ev) FIG. 4. XeF potentials, computed using a variety of techniques and basis sets, and corrected for BSSE, compared with experiment. a Reference 17. AVTZ/AVTZ SC/AVTZ STUT/AVTZ Experiment a
5 J. Chem. Phys., Vol. 114, No. 5, 1 February 2001 Noble gas halides 2223 TABLE VI. BSSE corrected computed bond lengths and dissociation energies for XeF compared with experimental values. Technique Basis set R (Å) D e (ev) CCSD T SC/AVTZ RCCSD T STUT/AVQZ MR-ACPF STUT/AVQZ MR-ACPF-SO STUT/AVQZ Previous calculation a Experiment b a Reference 23; this calculation used the same basis sets and a computational technique similar to MR-ACPF-SO here. The minimum was determined without correcting for BSSE; correcting for BSSE at the uncorrected minimum yields the energy in parentheses. b Reference 17. gas monofluorides, KrF shows the largest discrepancy between our best calculation and the accepted experimental potential. It is possible that the KrF ground state potential has not yet been characterized accurately by experiment. FIG. 5. XeCl potentials, computed using a variety of techniques and basis sets, and corrected for BSSE, compared with experiment. at all close to those from the experimental potential depicted in Fig. 3. In the case of XeF, we saw that MR-ACPF-SO gave nearly quantitative agreement with experiment; for KrF, however, this level of theory gives a bond length more than 0.2 Å longer, and a dissociation energy that is slightly more than half of the experimental value. This particular experimental potential is the most recent and is based on data from all previous scattering experiments, which sample the attractive portion of the potential, as well as fluorescence experiments, which sample the repulsive wall at separations shorter than the minimum. 37 The minimum itself must be interpolated between the two data sets, which is a difficult and uncertain process. Comparisons of computed results with the two other potentials from the literature that feature a minimum, given in Table V, show better agreement with respect to bond length, although there is still significant disagreement with dissociation energy. While the calculated results shown here are not free from approximation, and thus not exact, it is nonetheless significant that, of all the noble TABLE V. BSSE corrected computed bond lengths and dissociation energies for KrF compared with experimental values. Technique Basis set R (Å) D e (ev) RCCSD T STUT/AVQZ MR-ACPF STUT/AVQZ MR-ACPF-SO STUT/AVQZ Previous calculation a Experiment b b c c 3.0 d d a Reference 24; this is the BSSE corrected CCSD T result using the SC basis set for Kr and an atomic natural orbital basis set for F. b Reference 37. c Reference 11. d Reference XeCl The comparison between calculated potentials and experiment for XeCl is shown in Fig. 5, and bond length and dissociation energy data are collected in Table VII. Interestingly, while the GAUSSIAN CCSD T calculation falls far short in comparing it to experimental bond length and dissociation energy, the MOLPRO RCCSD T calculation does much better with its dissociation energy. All of the calculated bond lengths are significantly longer than the experimental result, by more than 0.3 Å in all but one case, and the multireference calculations overshoot the dissociation energy, although all are within ev of the experimental value. Note that while the previous calculation has a shorter bond length and larger dissociation energy than any of our results, 23 this difference is because the previous result was not corrected for BSSE. Such correction reduces D e and increases R e. 24 The cause of this discrepancy is not clear, but possible culprits include the neglect of some relativistic effects, as in the XeF calculation, as well as the neglect of the Cl atom in the calculation of the SO coupling. B. Charge-transfer states of XeF, XeCl, and KrF A consequence of performing SO calculations on XeF, XeCl, and KrF is that the energies of the six lowest states are calculated, the lower three covalent and the upper three ionic. Hence, this is an opportunity to update the calcula- TABLE VII. BSSE corrected computed bond lengths and dissociation energies for XeCl compared with experimental values. Technique Basis set R (Å) D e (ev) CCSD T SC/AVTZ RCCSD T STUT/AVQZ MR-ACPF STUT/AVQZ MR-ACPF-SO STUT/AVQZ Previous calculation a Experiment b a Reference 23; this calculation used the same technique and basis sets as RCCSD T here, but was not corrected for BSSE. b Reference 19.
6 2224 J. Chem. Phys., Vol. 114, No. 5, 1 February 2001 G. J. Hoffman and M. Colletto FIG. 6. XeF neutral and charge-transfer state potentials calculated using MR-ACPF-SO and STUT/AVQZ. FIG. 7. XeCl neutral and charge-transfer state potentials calculated using MR-ACPF-SO and STUT/mAVTZ. tions performed on these molecules by Dunning and Hay and published in ,21 The six states can be classified by the quantum number total component of angular momentum along the internuclear axis, either by numbering or by using the spectroscopists letter designation of the state. The latter system will be used here, so the three covalent states are X(1/2) ground state, A(3/2), and A (1/2), while the three ionic states are B(1/2), C(3/2), and D(1/2). In each group covalent or ionic, the two 1/2 states are the split states. In a particular group of states, at infinite atomic separation, the lower 1/2 state will correlate to the same limit as the 3/2 state, which is 1 S 0 2 P 3/2, while the upper 1/2 state correlates to 1 S 0 2 P 1/2. In the calculations presented here, all three covalent states correlate to the same energy at infinite atomic separation because the SO splitting of the neutral halogen has been neglected. However, the depiction of all three ionic states ought to be correct. Figures 6, 7, and 8 show the potential curves for all six states calculated using MR-ACPF-SO for XeF, XeCl, and KrF, respectively. For each of the ionic potentials of each molecule, the harmonic frequency and anharmonicity were determined by numerically integrating the Schrödinger equation using the shooting method to find the first 16 eigenvalues, and then performing a Birge Sponer fit. 40 All of these results are catalogued and compared with experiment and previous calculation in Tables VIII, IX, and X for XeF, XeCl, and KrF, respectively. Among general observations that can be made regarding these results, all of the newly calculated bond lengths are shorter than those previously calculated, and closer to the experimentally measured values, where such measurements are available for comparison. Note, however, that all of the new, shorter calculated bond lengths are still longer than those measured experimentally. Similarly, all of the newly calculated T e s are smaller than previous calculation, and most agree with experiment at least as well as previous calculation. Dipole moments and transition moments as functions of atomic separation were also calculated, but these are not presented here because they are almost quantitatively identical to those published previously. 20,21 For XeF, the newly calculated T e s for each of the ionic states are too small, and except for the C(3/2) state, they do not improve on the results of previous calculation. However, the ordering of the states is correct: the minimum of the C(3/2) state lies below the B(1/2) minimum. Further, the harmonic frequencies of the C(3/2) and the D(1/2) states are closer to the experimental values than previous calculations, while that for the B(1/2) state falls far short. The results for FIG. 8. KrF neutral and charge-transfer state potentials calculated using MR-ACPF-SO and STUT/AVQZ.
7 J. Chem. Phys., Vol. 114, No. 5, 1 February 2001 Noble gas halides 2225 TABLE VIII. Molecular and spectroscopic constants of XeF charge-transfer states from calculations compared with experiment and previous calculation. R e (Å) T e (ev) e (cm 1 ) e x e (cm 1 ) B(1/2) state This work Previous calculation a Experiment b C(3/2) state This work Previous calculation a Experiment c D(1/2) state This work Previous calculation a Experiment b d d b,d a References 20, 21. b Reference 5. c Reference 7. d Reference 10. XeCl were the best of the three molecules. All the newly calculated T e s for XeCl lie within 0.06 ev of the experimental values, and all calculated harmonic frequencies lie within 10 cm 1 of the experimental values. One minor error is that the ordering of the B(1/2) and C(3/2) states is opposite from experimental observation, but then the energetic separation between these two states is very small. For KrF, comparison with experimental data is somewhat difficult because only the B(1/2) state has been characterized to any degree in the gas phase, although some estimates can be found for the D(1/2) state. Such characterization is difficult to perform because the Franck Condon region of the ground state for these transitions lies high on its repulsive wall; spectra must be calculated from assumed potentials and then compared to experiment. Results of three such studies on the B(1/2) state are provided in Table X. The experimental numbers provided in Table X for the D(1/2) state are not as firmly grounded as those for the B(1/2) state; each set has a caveat. The first set of numbers TABLE IX. Molecular and spectroscopic constants of XeCl charge-transfer states from calculations compared with experiment and previous calculation. R e (Å) T e (ev) e (cm 1 ) e x e (cm 1 ) B(1/2) state This work Previous calculation a Experiment b C(3/2) state This work Previous calculation a Experiment c D(1/2) state This work Previous calculation a Experiment b a Reference 21. b Reference 6. c Reference 8. TABLE X. Molecular and spectroscopic constants of KrF charge-transfer states from calculations compared with experiment and previous calculation. R e (Å) T e (ev) e (cm 1 ) e x e (cm 1 ) B(1/2) state This work Previous calculation a Experiment b b 330 b 2.33 c c 336 c 1.4 c 2.27 d d 310 d C(3/2) state This work Previous calculation a D(1/2) state This work Previous calculation a Experiment 2.33 c,e c,e 328 c,e 1.3 c,e f f 1.35 f a Reference 20. b Reference 11. c Reference 9. d Reference 3. e These numbers come from a fit of photoassociative excitation spectra for both B X and D X transitions that the authors found to be unsatisfactory; hence these numbers can t be assumed to be correct. f Reference 15; this is from the analysis of the excitation spectrum of KrF matrix isolated in solid Ne, so these values are expected to be red-shifted from the gas phase values. comes from the attempt of Jones et al. 9 to fit photoassociation excitation spectra, but inclusion of the D X transition produced features in the simulated spectra that did not appear in experiment; hence, the validity of these values is questionable. The second set comes from experimental data for the D(1/2) state from the excitation spectrum of KrF isolated in solid neon; 15 all of the spectroscopic constants from this spectrum are assumed to be red-shifted from their gas phase values. It is interesting to note that, despite the expected red-shift, the e of the D(1/2) state from the Ne matrix is larger than that from the gas phase estimate. No constants from experimental data for the C(3/2) state have ever been published. The newly calculated T e values for the B(1/2) and D(1/2) states fall below the experimental values presented, even the red-shifted T e for the D(1/2) state. This indicates that all of the new T e values are too small. In this light, it is likely that the old and new calculated values for the T e of the C(3/2) state serve as upper and lower bounds, respectively, to the correct value. With regard to vibrational parameters, the new calculated value for the harmonic frequency of the B(1/2) state is slightly larger than either the experimental numbers or the previously calculated e, but agreement is still within 10 cm 1 of most of these values. Interestingly, the newly calculated anharmonicity for this state is quite large. The newly calculated values for the e s of the C(3/2) and D(1/2) states are slightly smaller than the previously calculated ones, but in the case of the D(1/2) state, this smaller value is closer to its experimental estimates.
8 2226 J. Chem. Phys., Vol. 114, No. 5, 1 February 2001 G. J. Hoffman and M. Colletto IV. CONCLUSIONS An ab initio study of the ground state potentials of NeF, ArF, KrF, XeF, and XeCl, and of the charge-transfer state potentials of KrF, XeF, and XeCl, has been presented, and the results compared with experimental results and previous calculations. Of the fluorides, good agreement between calculation and experiment is observed for NeF, ArF, and XeF. For NeF and ArF, theory at the level of CCSD T is sufficient to give quantitative agreement with experiment. For XeF, it is necessary to invoke a multireference technique MR-ACPF and to include SO coupling to achieve quantitative agreement between theory and experiment. This is because of the significant amount of mixing that occurs between covalent and ionic 2 states, and because the SO coupling associated with Xe is large enough to affect the ground state potential. On the other hand, no level of theory attempted here has resulted in quantitative agreement with the best accepted experimental ground state potential for KrF, suggesting possible error in the experimental potential. Application of MR-ACPF to KrF made only a small improvement over CCSD T, and the difference due to SO coupling is almost negligible. Semiquanititative agreement between experimental and calculated potentials is observed for XeCl, suggesting the breakdown of one or more of the approximations made. Overall, the application of high-level ab initio techniques in order to determine accurate results for weakly bound species presents a substantial challenge. The newly calculated charge-transfer state potentials overall show a level of agreement with experiment as good as or better than previous calculation with regard to bond length and, often, with regard to T e and vibrational parameters also. The best agreement is observed for XeCl. While agreement is not as good for XeF and KrF, the correct ordering of the charge-transfer states of XeF is obtained. ACKNOWLEDGMENTS This research was supported by NSF cooperative agreement ACI through a grant of computer time on the Cray T90 at the San Diego Supercomputer Center SDSC, administered by the National Partnership for Advanced Computing Infrastructures NPACI. The College of New Jersey has granted release time from teaching to GJH for the purpose of pursuing research; this grant is gratefully acknowledged. Dr. J. R. Greenberg, Dr. K. Milfield, and especially Dr. J. N. Harvey are thanked for invaluable advice on performing calculations using MOLPRO, and Dr. L. C. Allen for providing library access. Dr. R. J. Cave, Dr. S. K. Knudsen, R. Danell, and A.-M. Chen are thanked for contributions in the early stages of this research. Dr. R. J. Cave is also thanked for his many helpful suggestions during the course of this work, and for his critical review of the manuscript. 1 Excimer Lasers, 2nd ed., edited by Ch. K. Rhodes Springer, Berlin, 1984 provides a broad review of the early work on these molecules. 2 J. Tellinghuisen, J. M. Hoffman, G. C. Tisone, and A. K. Hays, J. Chem. Phys. 64, J. Tellinghuisen, A. K. Hays, J. M. Hoffman, and G. C. Tisone, J. Chem. Phys. 65, J. Tellinghuisen, P. C. Tellinghuisen, G. C. Tisone, J. M. Hoffman, and A. K. Hays, J. Chem. Phys. 68, P. C. Tellinghuisen, J. Tellinghuisen, J. A. Coxon, J. E. Velazco, and D. W. Setser, J. Chem. Phys. 68, A. Sur, A. K. Hui, and J. Tellinghuisen, J. Mol. Spectrosc. 74, H. Helm, D. L. Huestis, M. J. Dyer, and D. C. Lorents, J. Chem. Phys. 79, C. Jouvet, C. Lardeux-Dedonder, and D. Solgadi, Chem. Phys. Lett. 156, R. B. Jones, J. H. Schloss, and J. G. Eden, J. Chem. Phys. 98, K. Johnson and J. Tellinghuisen, Chem. Phys. Lett. 228, G. Lo and D. W. Setser, J. Chem. Phys. 100, J. Goodman and L. E. Brus, J. Chem. Phys. 65, B. S. Ault and L. Andrews, J. Chem. Phys. 65, G. Zerza, G. Sliwinski, N. Schwentner, G. J. Hoffman, D. G. Imre, and V. A. Apkarian, J. Chem. Phys. 99, C. Bressler, W. G. Lawrence, and N. Schwentner, J. Chem. Phys. 105, C. H. Becker, P. Casavecchia, and Y. T. Lee, J. Chem. Phys. 69, ; 70, V. Aquilanti, E. Luzzatti, F. Pirani, and G. G. Volpi, J. Chem. Phys. 89, V. Aquilanti, R. Candori, D. Cappelletti, E. Luzzatti, and F. Pirani, Chem. Phys. 145, V. Aquilanti, D. Cappelletti, V. Lorent, E. Luzzatti, and F. Pirani, Chem. Phys. Lett. 192, T. H. Dunning, Jr. and P. J. Hay, J. Chem. Phys. 69, P. J. Hay and T. H. Dunning, Jr., J. Chem. Phys. 69, G. F. Adams and C. F. Chubalowski, J. Phys. Chem. 98, D. Schröder, J. N. Harvey, M. Aschi, and H. Schwarz, J. Chem. Phys. 108, G. J. Hoffman, L. A. Swafford, and R. J. Cave, J. Chem. Phys. 109, GAUSSIAN 94 Revision E.1 M. J. Frisch, G. W. Tracks, H. B. Schlegel et al. Gaussian, Inc., Pittsburgh, PA, MOLPRO is a package of ab initio programs written by H.-J. Werner and P. J. Knowles, with contributions from J. Almlöf, R. D. Amos, A. Berning et al. 27 T. H. Dunning, Jr., J. Chem. Phys. 90, ; R. A. Kendall, T. H. Dunning, Jr., and R. J. Harrison, ibid. 96, Basis sets were obtained from the Extensible Computational Chemistry Environment Basis Set Database, Version 1.0, as developed and distributed by the Molecular Science Computing Facility, Environmental and Molecular Sciences Laboratory which is part of the Pacific Northwest Laboratory, P.O. Box 999, Richland, Washington 99352, and funded by the U.S. Department of Energy. The Pacific Northwest Laboratory is a multi-program laboratory operated by Battelle Memorial Institute for the U.S. Department of Energy under Contract No. DE-AC06-76RLO Contact David Feller, Karen Schuchardt, or Don Jones for further information. 29 L. F. Pacios and P. A. Christiansen, J. Chem. Phys. 82, ; M. M. Hurley, L. F. Pacios, P. A. Christiansen, R. B. Ross, and W. C. Ermler, ibid. 84, ; L. A. LaJohn, P. A. Christiansen, R. B. Ross, T. Atashroo, and W. C. Ermler, ibid. 87, Gaussian Basis Sets for Molecular Calculations, edited by S. Huzinaga Elsevier, Amsterdam, H. Bürger, R. Kuna, S. Ma, J. Breidung, and W. Thiel, J. Chem. Phys. 101, A. Nicklass, M. Dolg, H. Stoll, and H. Preuss, J. Chem. Phys. 102, J. A. Pople, R. Krishnan, H. B. Schlegel, and J. S. Binkley, Int. J. Quantum Chem. 14, ; J. Cizek, Adv. Chem. Phys. 14, ; G. D. Purvis and R. J. Bartlett, J. Chem. Phys. 76, ; G.E.Scuseria, C. L. Janssen, and H. F. Schaefer III, ibid. 89, ; G.E. Scuseria and H. F. Schaefer III, ibid. 90, ; R. J. Bartlett and G. D. Purvis, Int. J. Quantum Chem. 14, ; J. A. Pople, M. Head- Gordon, and K. Raghavachari, J. Chem. Phys. 87, P. J. Knowles, C. Hampel, and H.-J. Werner, J. Chem. Phys. 99, ; J. D. Watts, J. Gauss, and R. J. Bartlett, ibid. 98, H.-J. Werner and P. J. Knowles, J. Chem. Phys. 89, ; P.J. Knowles and H.-J. Werner, Chem. Phys. Lett. 145, S. F. Boys and F. Bernardi, Mol. Phys. 19, D. Cappelletti, F. Pirani, and V. Aquilanti, private communication June 2, This potential was first published in Ref F. Y. Naumkin and F. R. W. McCourt, J. Chem. Phys. 107, ;
9 J. Chem. Phys., Vol. 114, No. 5, 1 February 2001 Noble gas halides 2227 ibid. 109, ; S. M. Cybulski and J. S. Holt, ibid. 110, G. L. Malli, J. Styszynski, and A. B. F. Da Silva, Int. J. Quantum Chem. 55, ; J. Styszynski and G. L. Malli, ibid. 55, For each set of points, a nonlinear least-squares fit to the functional form of a Rittner potential was performed. The difference between the best-fit Rittner function and the calculated points was obtained, and if any of these residuals exceeded 0.01 ev, a second nonlinear least-squares fit was performed using a function with properties that mimicked the variation observed in the residuals. The potential function used in the numerical integration of the Schrödinger equation was then the sum of the Rittner function and the residuals function.
Approximating the basis set dependence of coupled cluster calculations: Evaluation of perturbation theory approximations for stable molecules
JOURNAL OF CHEMICAL PHYSICS VOLUME 113, NUMBER 18 8 NOVEMBER 2000 Approximating the basis set dependence of coupled cluster calculations: Evaluation of perturbation theory approximations for stable molecules
More informationRelativistic and correlation effects on molecular properties. II. The hydrogen halides HF, HCl, HBr, HI, and HAt
Relativistic and correlation effects on molecular properties. II. The hydrogen halides HF, HCl, HBr, HI, and HAt L. Visscher Laboratory of Chemical Physics and Materials Science Center, University of Groningen,
More informationAccurate multireference configuration interaction calculations on the lowest 1 and 3 electronic states of C 2,CN, BN, and BO
Accurate multireference configuration interaction calculations on the lowest 1 and 3 electronic states of C 2,CN, BN, and BO Kirk A. Peterson a) Department of Chemistry, Washington State University and
More informationRelativistic and correlation effects on molecular properties. I. The dihalogens F 2,Cl 2,Br 2,I 2, and At 2
Relativistic and correlation effects on molecular properties. I. The dihalogens F 2,Cl 2,Br 2,I 2, and At 2 L. Visscher Laboratory of Chemical Physics and Material Science Center, University of Groningen,
More informationRadiative Transition Probabilities and Lifetimes for the Band Systems A 2 Π X 2 Σ + of the Isovalent Molecules BeF, MgF and CaF
950 Brazilian Journal of Physics, vol. 35, no. 4A, December, 2005 Radiative Transition Probabilities and Lifetimes for the Band Systems of the Isovalent Molecules BeF, MgF and CaF Marina Pelegrini a, Ciro
More informationFull configuration interaction potential energy curves for breaking bonds to hydrogen: An assessment of single-reference correlation methods
JOURNAL OF CHEMICAL PHYSICS VOLUME 118, NUMBER 4 22 JANUARY 2003 Full configuration interaction potential energy curves for breaking bonds to hydrogen: An assessment of single-reference correlation methods
More informationSystematic ab initio calculations on the energetics and stability of covalent O 4
JOURNAL OF CHEMICAL PHYSICS VOLUME 120, NUMBER 21 1 JUNE 2004 Systematic calculations on the energetics and stability of covalent O 4 Ramón Hernández-Lamoneda a) Centro de Investigación en Química, Universidad
More informationBenchmark calculations with correlated molecular wave functions
Theor Chem Acc (1997) 97:251±259 Benchmark calculations with correlated molecular wave functions XII. Core correlation e ects on the homonuclear diatomic molecules B 2 -F 2 Kirk A. Peterson 1, Angela K.
More informationRelativistic and correlated calculations on the ground, excited, and ionized states of iodine
Relativistic and correlated calculations on the ground, excited, and ionized states of iodine W. A. de Jong, L. Visscher, a) and W. C. Nieuwpoort Laboratory for Chemical Physics and Materials Science Centre,
More informationAb initio study of spectroscopic and radiative characteristics of ion-pair states of the Cl 2 molecule
JOURNAL OF CHEMICAL PHYSICS VOLUME 115, NUMBER 20 22 NOVEMBER 2001 Ab initio study of spectroscopic and radiative characteristics of ion-pair states of the Cl 2 molecule D. B. Kokh, a) A. B. Alekseyev,
More informationAb initio calculations on the ground and low-lying excited states of InI
MOLECULAR PHYSICS, 1OCTOBER 23, VOL. 11, NO. 19, 2963 2968 Ab initio calculations on the ground and low-lying excited states of InI WENLI ZOU, MEIRONG LIN*, XINZHENG YANG and BAOZHENG ZHANG Institute of
More informationElectron Configuration and Chemical Periodicity
Electron Configuration and Chemical Periodicity The Periodic Table Periodic law (Mendeleev, Meyer, 1870) periodic reoccurrence of similar physical and chemical properties of the elements arranged by increasing
More informationPeriodic Trends in Properties of Homonuclear
Chapter 8 Periodic Trends in Properties of Homonuclear Diatomic Molecules Up to now, we have discussed various physical properties of nanostructures, namely, two-dimensional - graphene-like structures:
More informationA fully relativistic Dirac Hartree Fock and second-order Mo ller Plesset study of the lanthanide and actinide contraction
JOURNAL OF CHEMICAL PHYSICS VOLUME 109, NUMBER 24 22 DECEMBER 1998 A fully relativistic Dirac Hartree Fock and second-order Mo ller Plesset study of the lanthanide and actinide contraction J. K. Laerdahl
More informationLewis Structures and Bonding
Lewis Structures and Bonding (If we did it after molecular shape- AKA VSEPR- it would be a prequel to What shape are your molecules in? ) World of Chemistry, Zumdahl Chpt 12 pp 358-381 (Lewis) 1 You ll
More informationTheoretical determination of the heat of formation of methylene
Theoretical determination of the heat of formation of methylene Nikos L. Doltsinis and Peter J. Knowles School of Chemistry, University of Birmingham, Edgbaston, Birmingham B5 2TT, United Kingdom The heat
More informationComputational Material Science Part II. Ito Chao ( ) Institute of Chemistry Academia Sinica
Computational Material Science Part II Ito Chao ( ) Institute of Chemistry Academia Sinica Ab Initio Implementations of Hartree-Fock Molecular Orbital Theory Fundamental assumption of HF theory: each electron
More informationAtoms, Molecules and Solids (selected topics)
Atoms, Molecules and Solids (selected topics) Part I: Electronic configurations and transitions Transitions between atomic states (Hydrogen atom) Transition probabilities are different depending on the
More informationAtom-molecule molecule collisions in spin-polarized polarized alkalis: potential energy surfaces and quantum dynamics
Atom-molecule molecule collisions in spin-polarized polarized alkalis: potential energy surfaces and quantum dynamics Pavel Soldán, Marko T. Cvitaš and Jeremy M. Hutson University of Durham with Jean-Michel
More informationAn Accurate Calculation of Potential Energy Curves and Transition Dipole Moment for Low-Lying Electronic States of CO
Commun. Theor. Phys. 59 (2013) 193 198 Vol. 59, No. 2, February 15, 2013 An Accurate Calculation of Potential Energy Curves and Transition Dipole Moment for Low-Lying Electronic States of CO LU Peng-Fei
More informationDensity functional theory predictions of anharmonicity and spectroscopic constants for diatomic molecules
JOURNAL OF CHEMICAL PHYSICS VOLUME 115, NUMBER 6 8 AUGUST 2001 Density functional theory predictions of anharmonicity and spectroscopic constants for diatomic molecules Mutasem Omar Sinnokrot and C. David
More informationExercise 1: Structure and dipole moment of a small molecule
Introduction to computational chemistry Exercise 1: Structure and dipole moment of a small molecule Vesa Hänninen 1 Introduction In this exercise the equilibrium structure and the dipole moment of a small
More informationA contribution to the understanding of the structure of xenon hexafluoride
A contribution to the understanding of the structure of xenon hexafluoride T. Daniel Crawford, a) Kristen W. Springer, b) and Henry F. Schaefer III Center for Computational Quantum Chemistry, University
More informationSolution of the Electronic Schrödinger Equation. Using Basis Sets to Solve the Electronic Schrödinger Equation with Electron Correlation
Solution of the Electronic Schrödinger Equation Using Basis Sets to Solve the Electronic Schrödinger Equation with Electron Correlation Errors in HF Predictions: Binding Energies D e (kcal/mol) HF Expt
More informationAb initio calculations of F-H-Br system with linear geometry
Current Chemistry Letters 5 (016) 1 6 Contents lists available atgrowingscience Current Chemistry Letters homepage: www.growingscience.com/ccl Ab initio calculations of F-H-Br system with linear geometry
More informationManuel Díaz-Tinoco and J. V. Ortiz Department of Chemistry and Biochemistry Auburn University Auburn AL Abstract
JCP Comment on Are polynuclear superhalogens without halogen atoms probable? A high level ab initio case study on triple bridged binuclear anions with cyanide ligands [J. Chem. Phys. 140, 094301 (2014)]
More informationChapter 8: Periodic Properties of the Elements
C h e m i s t r y 1 A : C h a p t e r 8 P a g e 1 Chapter 8: Periodic Properties of the Elements Homework: Read Chapter 8. Work out sample/practice exercises Check for the MasteringChemistry.com assignment
More informationPotential energy curves for neutral and multiply charged carbon monoxide
PRAMANA c Indian Academy of Sciences Vol. 74, No. 1 journal of January 2010 physics pp. 49 55 Potential energy curves for neutral and multiply charged carbon monoxide PRADEEP KUMAR 1 and N SATHYAMURTHY
More informationCalculation of Potential Energy Curves of Excited States of Molecular Hydrogen by Multi-Reference Configuration-interaction Method
Calculation of PECs of Excited States of H 2 by MRCI Bull. Korean Chem. Soc. 203, Vol. 34, No. 6 77 http://dx.doi.org/0.502/bkcs.203.34.6.77 Calculation of Potential Energy Curves of Excited States of
More informationCHEMISTRY XL-14A CHEMICAL BONDS
CHEMISTRY XL-14A CHEMICAL BONDS July 16, 2011 Robert Iafe Office Hours 2 July 18-July 22 Monday: 2:00pm in Room MS-B 3114 Tuesday-Thursday: 3:00pm in Room MS-B 3114 Chapter 2 Overview 3 Ionic Bonds Covalent
More informationChapter 3 Classification of Elements and Periodicity in Properties
Question 3.1: What is the basic theme of organisation in the periodic table? The basic theme of organisation of elements in the periodic table is to classify the elements in periods and groups according
More informationCHEM 103 Quantum Mechanics and Periodic Trends
CHEM 103 Quantum Mechanics and Periodic Trends Lecture Notes April 11, 2006 Prof. Sevian Agenda Predicting electronic configurations using the QM model Group similarities Interpreting measured properties
More informationChemistry (www.tiwariacademy.com)
() Question 3.1: What is the basic theme of organisation in the periodic table? Answer 1.1: The basic theme of organisation of elements in the periodic table is to classify the elements in periods and
More informationThe electronic spectrum of pyrrole
JOURNAL OF CHEMICAL PHYSICS VOLUME 111, NUMBER 2 8 JULY 1999 The electronic spectrum of pyrrole Ove Christiansen a) and Jürgen Gauss Institut für Physikalische Chemie, Universität Mainz, D-55099 Mainz,
More informationQuestion 3.2: Which important property did Mendeleev use to classify the elements in his periodic table and did he stick to that?
Question 3.1: What is the basic theme of organisation in the periodic table? The basic theme of organisation of elements in the periodic table is to classify the elements in periods and groups according
More informationConcepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds. David A. Katz Pima Community College Tucson, AZ
Concepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds David A. Katz Pima Community College Tucson, AZ Chemical Bonds Three basic types of bonds: Ionic Electrostatic attraction
More informationLecture 9 Electronic Spectroscopy
Lecture 9 Electronic Spectroscopy Molecular Orbital Theory: A Review - LCAO approximaton & AO overlap - Variation Principle & Secular Determinant - Homonuclear Diatomic MOs - Energy Levels, Bond Order
More informationTheoretical study of spin-orbit coupling constants for O 2
JOURNAL OF CHEMICAL PHYSICS VOLUME 115, NUMBER 16 22 OCTOBER 2001 Theoretical study of spin-orbit coupling constants for O 2 A 2 3Õ2,1Õ2u, v Ä0 17 and a 4 5Õ2,3Õ2,1Õ2,À1Õ2u, v Ä0 25 D. G. Fedorov, M. S.
More informationA coupled cluster study of the spectroscopic properties and electric dipole moment functions of nitrous sulfide
A coupled cluster study of the spectroscopic properties and electric dipole moment functions of nitrous sulfide Youngshang Pak and R. Claude Woods Department of Chemistry, University of Wisconsin Madison,
More information2. Why do all elements want to obtain a noble gas electron configuration?
AP Chemistry Ms. Ye Name Date Block Do Now: 1. Complete the table based on the example given Location Element Electron Configuration Metal, Nonmetal or Semi-metal Metalloid)? Group 1, Period 1 Group 11,
More informationIntroduction to computational chemistry Exercise I: Structure and electronic energy of a small molecule. Vesa Hänninen
Introduction to computational chemistry Exercise I: Structure and electronic energy of a small molecule Vesa Hänninen 1 Introduction In this exercise the equilibrium structure and the electronic energy
More informationCorrelation effects in MgO and CaO: Cohesive energies and lattice constants
PHYSICAL REVIEW B VOLUME 54, NUMBER 19 15 NOVEMBER 1996-I Correlation effects in MgO and CaO: Cohesive energies and lattice constants Klaus Doll and Michael Dolg Max-Planck-Institut für Physik Komplexer
More informationDetlev Figgen, Erich Goll, and Hermann Stoll b) Institut für Theoretische Chemie, Universität Stuttgart, D Stuttgart, Germany
JOURNAL OF CHEMICAL PHYSICS VOLUME 119, NUMBER 21 1 DECEMBER 2003 Systematically convergent basis sets with relativistic pseudopotentials. II. Small-core pseudopotentials and correlation consistent basis
More informationChapter 8 : Covalent Bonding. Section 8.1: Molecular Compounds
Chapter 8 : Covalent Bonding Section 8.1: Molecular Compounds What is a molecule? A molecular compound? A molecule is a neutral group of atoms joined together by covalent bonds A molecular compound is
More informationOrganic Chemistry. Review Information for Unit 1. Atomic Structure MO Theory Chemical Bonds
Organic Chemistry Review Information for Unit 1 Atomic Structure MO Theory Chemical Bonds Atomic Structure Atoms are the smallest representative particle of an element. Three subatomic particles: protons
More informationChapter 7 The Structure of Atoms and Periodic Trends
Chapter 7 The Structure of Atoms and Periodic Trends Jeffrey Mack California State University, Sacramento Arrangement of Electrons in Atoms Electrons in atoms are arranged as SHELLS (n) SUBSHELLS (l) ORBITALS
More informationNotes: Electrons and Periodic Table (text Ch. 4 & 5)
Name Per. Notes: Electrons and Periodic Table (text Ch. 4 & 5) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to
More informationProblems with the Wave Theory of Light (Photoelectric Effect)
CHEM101 NOTES Properties of Light Found that the wave theory could not work for some experiments e.g. the photovoltaic effect This is because the classic EM view of light could not account for some of
More informationBeyond the Hartree-Fock Approximation: Configuration Interaction
Beyond the Hartree-Fock Approximation: Configuration Interaction The Hartree-Fock (HF) method uses a single determinant (single electronic configuration) description of the electronic wavefunction. For
More informationChapter 9 Ionic and Covalent Bonding
Chem 1045 Prof George W.J. Kenney, Jr General Chemistry by Ebbing and Gammon, 8th Edition Last Update: 06-April-2009 Chapter 9 Ionic and Covalent Bonding These Notes are to SUPPLIMENT the Text, They do
More informationBasis set convergence in extended systems: infinite hydrogen fluoride and hydrogen chloride chains
Chemical Physics Letters 398 (2004) 44 49 www.elsevier.com/locate/cplett Basis set convergence in extended systems: infinite hydrogen fluoride and hydrogen chloride chains Christian Buth *, Beate Paulus
More informationJack Simons, Henry Eyring Scientist and Professor Chemistry Department University of Utah
1. Born-Oppenheimer approx.- energy surfaces 2. Mean-field (Hartree-Fock) theory- orbitals 3. Pros and cons of HF- RHF, UHF 4. Beyond HF- why? 5. First, one usually does HF-how? 6. Basis sets and notations
More informationTest Review # 4. Chemistry: Form TR4-9A
Chemistry: Form TR4-9A REVIEW Name Date Period Test Review # 4 Location of electrons. Electrons are in regions of the atom known as orbitals, which are found in subdivisions of the principal energy levels
More informationCHAPTER 2 INTERATOMIC FORCES. atoms together in a solid?
CHAPTER 2 INTERATOMIC FORCES What kind of force holds the atoms together in a solid? Interatomic Binding All of the mechanisms which cause bonding between the atoms derive from electrostatic interaction
More informationBond formation between two Hydrogen Atoms
Name Chem 162, Section: Group Number: ALE 9. Covalent Bonding (Reference: Section 9.3 - Silberberg 5 h edition) What determines the length of a covalent bond? The Model: Interactions that determine the
More informationAtoms, Molecules and Solids (selected topics)
Atoms, Molecules and Solids (selected topics) Part I: Electronic configurations and transitions Transitions between atomic states (Hydrogen atom) Transition probabilities are different depending on the
More informationComment on: Estimating the Hartree Fock limit from finite basis set calculations [Jensen F (2005) Theor Chem Acc 113:267]
Comment on: Estimating the Hartree Fock limit from finite basis set calculations [Jensen F (2005) Theor Chem Acc 113:267] Amir Karton and Jan M.L. Martin Department of Organic Chemistry, Weizmann Institute
More informationDipole Moment and Electronic Structure Calculations of the Electronic States of the molecular ion SiN +
Applied Physics Research; Vol. 8, No. 4; 2016 ISSN 1916-9639 E-ISSN 1916-9647 Published by Canadian Center of Science and Education Dipole Moment and Electronic Structure Calculations of the Electronic
More informationarxiv:cond-mat/ v2 [cond-mat.other] 21 Nov 2005
arxiv:cond-mat/0408243v2 [cond-mat.other] 21 Nov 2005 Basis set convergence in extended systems: infinite hydrogen fluoride and hydrogen chloride chains Christian Buth, Beate Paulus Max-Planck-Institut
More informationChapter 3. Crystal Binding
Chapter 3. Crystal Binding Energy of a crystal and crystal binding Cohesive energy of Molecular crystals Ionic crystals Metallic crystals Elasticity What causes matter to exist in three different forms?
More informationChapter 8. Bonding: General Concepts
Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents 8.1 Types of Chemical Bonds 8.2 Electronegativity 8.3 Bond Polarity and Dipole Moments 8.4 Ions: Electron Configurations and Sizes 8.5 Energy
More informationQUANTUM CHEMISTRY PROJECT 3: ATOMIC AND MOLECULAR STRUCTURE
Chemistry 460 Fall 2017 Dr. Jean M. Standard November 1, 2017 QUANTUM CHEMISTRY PROJECT 3: ATOMIC AND MOLECULAR STRUCTURE OUTLINE In this project, you will carry out quantum mechanical calculations of
More informationSCIENCE CHINA Physics, Mechanics & Astronomy. Potential energy curves crossing and low-energy charge transfer dynamics in (BeH 2 O) 2+ complex
SCIENCE CHINA Physics, Mechanics & Astronomy Article July 2012 Vol.55 No.7: 1258 1262 doi: 10.1007/s11433-012-4714-9 Potential energy curves crossing and low-energy charge transfer dynamics in (BeH 2 O)
More informationPerformance of Hartree-Fock and Correlated Methods
Chemistry 460 Fall 2017 Dr. Jean M. Standard December 4, 2017 Performance of Hartree-Fock and Correlated Methods Hartree-Fock Methods Hartree-Fock methods generally yield optimized geomtries and molecular
More informationStatic Dipole Moments and Electronic Structure Calculations of the Low-Lying Electronic States of the Molecule Zinc Selinum ZnSe
Modern Applied Science; Vol. 11, No. 9; 2017 ISSN 1913-1844 E-ISSN 1913-1852 Published by Canadian Center of Science and Education Static Dipole Moments and Electronic Structure Calculations of the Low-Lying
More informationChapter 8: Concepts of Chemical Bonding
Chapter 8: Concepts of Chemical Bonding Learning Outcomes: Write Lewis symbols for atoms and ions. Define lattice energy and be able to arrange compounds in order of increasing lattice energy based on
More informationName Date Class MOLECULAR COMPOUNDS. Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides
8.1 MOLECULAR COMPOUNDS Section Review Objectives Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides Vocabulary covalent bond molecule diatomic molecule
More informationChemistry 11. Unit 8 Atoms and the Periodic Table Part II Electronic Structure of Atoms
Chemistry 11 Unit 8 Atoms and the Periodic Table Part II Electronic Structure of Atoms 2 1. Atomic number and atomic mass In the previous section, we have seen that from 50 to 100 years after Dalton proposed
More informationChemistry Publications
Chemistry Publications Chemistry 2007 Accurate Ab Initio Potential Energy Curve of F2. I. Nonrelativistic Full Valence Configuration Interaction Energies Using the Correlation Energy Extrapolation by Intrinsic
More informationElectrons and Molecular Forces
Electrons and Molecular Forces Chemistry 30 Ms. Hayduk Electron Configuration Atomic Structure Atomic Number Number of protons in the nucleus Defines the element Used to organize the periodic table 1 Bohr
More informationWolfgang Demtroder. Molecular Physics. Theoretical Principles and Experimental Methods WILEY- VCH. WILEY-VCH Verlag GmbH & Co.
Wolfgang Demtroder Molecular Physics Theoretical Principles and Experimental Methods WILEY- VCH WILEY-VCH Verlag GmbH & Co. KGaA v Preface xiii 1 Introduction 1 1.1 Short Historical Overview 2 1.2 Molecular
More informationDownloaded from
Points to Remember Class: XI Chapter Name: Chemical Bonding and Molecular Structure Top Concepts 1. The attractive force which holds together the constituent particles (atoms, ions or molecules) in chemical
More informationElectric Dipole Moments and Chemical Bonding of. Diatomic Alkali - Alkaline Earth Molecules. Electronic Supplementary Information
Electronic Supplementary Material (ESI) for Physical Chemistry Chemical Physics. This journal is the Owner Societies 2016 Electric Dipole Moments and Chemical Bonding of Diatomic Alkali - Alkaline Earth
More informationCHAPTER 1 Atoms and bonding. Ionic bonding Covalent bonding Metallic bonding van der Waals bonding
CHAPTER 1 Atoms and bonding The periodic table Ionic bonding Covalent bonding Metallic bonding van der Waals bonding Atoms and bonding In order to understand the physics of semiconductor (s/c) devices,
More informationInvestigation of Spectroscopic Properties and Spin-Orbit Splitting in the X 2 Π and A 2 Π Electronic States of the SO + Cation
Int. J. Mol. Sci. 2012, 13, 8189-8209; doi:10.3390/ijms13078189 Article OPEN ACCESS International Journal of Molecular Sciences ISSN 1422-0067 www.mdpi.com/journal/ijms Investigation of Spectroscopic Properties
More informationCharge renormalization at the large-d limit for N-electron atoms and weakly bound systems
Charge renormalization at the large-d limit for N-electron atoms and weakly bound systems S. Kais and R. Bleil Department of Chemistry, Purdue University, West Lafayette, Indiana 47907 Received 25 January
More informationATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter is made of atoms. There are a limited number of types of atoms; these are the elements. (EU 1.A) Development of Atomic Theory Atoms are so small
More information4/4/2013. Covalent Bonds a bond that results in the sharing of electron pairs between two atoms.
A chemical bond is a mutual electrical attraction between the nucleus and valence electrons of different atoms that binds the atoms together. Why bond? As independent particles, atoms have a high potential
More informationBasis Set for Molecular Orbital Theory
Basis Set for Molecular Orbital Theory! Different Types of Basis Functions! Different Types of Atom Center Basis Functions! Classifications of Gaussian Basis Sets! Pseudopotentials! Molecular Properties
More informationThe Structure of Alkali Halide Dimers: A Critical Test of Ionic Models and New Ab Initio Results
Claremont Colleges Scholarship @ Claremont All HMC Faculty Publications and Research HMC Faculty Scholarship 5-22-1996 The Structure of Alkali Halide Dimers: A Critical Test of Ionic Models and New Ab
More informations or Hz J atom J mol or -274 kj mol CHAPTER 4. Practice Exercises ΔE atom = ΔE mol =
CHAPTER 4 Practice Exercises 4.1 10 1 2.1410 s or Hz 4.3 ΔE atom = ΔE mol = 4.5610 J atom 19 1 2.7410 J mol or -274 kj mol 5 1-1 4.5 excitation energy = 471 kj mol 1 + 275 kj mol 1 = 746 kj mol 1 Hg 4.7
More informationStuart Carter Department of Chemistry, University of Reading, Reading RG6 2AD, United Kingdom
JOURNAL OF CHEMICAL PHYSICS VOLUME 117, NUMBER 4 22 JULY 2002 The ab initio potential energy surface and vibrational-rotational energy levels of X 2 MgOH Jacek Koput a) Department of Chemistry, Adam Mickiewicz
More information362 Lecture 6 and 7. Spring 2017 Monday, Jan 30
362 Lecture 6 and 7 Spring 2017 Monday, Jan 30 Quantum Numbers n is the principal quantum number, indicates the size of the orbital, has all positive integer values of 1 to (infinity) l is the angular
More informationApplications of Newly Developed spdsmcps for First-Row Transition Metal Atoms
1st WSEAS Int. Conf. on COMPUTATIONAL CHEMISTRY, Cairo, Egypt, December 29-31, 2007 14 Applications of Newly Developed spdsmcps for First-Row Transition Metal Atoms E. MIYOSHI, 1 Y. OSANAI, 2 M. S. MON,
More informationQuantum chemistry and vibrational spectra
Chapter 3 Quantum chemistry and vibrational spectra This chapter presents the quantum chemical results for the systems studied in this work, FHF (Section 3.) and OHF (Section 3.3). These triatomic anions
More informationChapter 8 The Concept of the Chemical Bond
Chapter 8 The Concept of the Chemical Bond Three basic types of bonds: Ionic - Electrostatic attraction between ions (NaCl) Metallic - Metal atoms bonded to each other Covalent - Sharing of electrons Ionic
More informationBonding - Ch. 7. Types of Bonding
Types of Bonding I. holds everything together! II. All bonding occurs because of III. Electronegativity difference and bond character A. A between two atoms results in a when those two atoms form a bond.
More informationChapter 9 Bonding - 1. Dr. Sapna Gupta
Chapter 9 Bonding - 1 Dr. Sapna Gupta Lewis Dot Symbol Lewis dot symbols is a notation where valence electrons are shown as dots. Draw the electrons symmetrically around the sides (top, bottom, left and
More informationUptake of OH radical to aqueous aerosol: a computational study
Uptake of OH radical to aqueous aerosol: a computational study Grigory Andreev Karpov Institute of Physical Chemistry 10 Vorontsovo pole, Moscow, 105064, Russia Institute of Physical Chemistry and Electrochemistry
More informationCHEM 115 Electron Configurations and
CHEM 115 Electron Configurations and Periodic Trends Lecture 20 Prof. Sevian 1 Agenda Electron configurations Ground state vs. excited state Periodic properties Ionization energy Atomic radius Others Interpreting
More informationElectronic structures of one-dimension carbon nano wires and rings
IOP Publishing Journal of Physics: Conference Series 61 (2007) 252 256 doi:10.1088/1742-6596/61/1/051 International Conference on Nanoscience and Technology (ICN&T 2006) Electronic structures of one-dimension
More informationSpin-orbit effect in the energy pooling reaction
THE JOURNAL OF CHEMICAL PHYSICS 126, 124304 2007 Spin-orbit effect in the energy pooling reaction O 2 a 1 +O 2 a 1 \O 2 b 1 +O 2 X 3 Rui-Feng Lu and Pei-Yu Zhang Academy of Sciences, Dalian 116023, China
More informationATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter is made of atoms. There are a limited number of types of atoms; these are the elements. (EU 1.A) Development of Atomic Theory Atoms are so small
More informationIONIC AND METALLIC BONDING
Name IONIC AND METALLIC BONDING Chem 512 Homework rint this sheet, answer the questions and turn it in as a HARD COY A. Matching Match each description in Column B with the correct term in Column A. Write
More informationChapter IV: Electronic Spectroscopy of diatomic molecules
Chapter IV: Electronic Spectroscopy of diatomic molecules IV.2.1 Molecular orbitals IV.2.1.1. Homonuclear diatomic molecules The molecular orbital (MO) approach to the electronic structure of diatomic
More informationCh. 8 Chemical Bonding: General Concepts. Brady & Senese, 5th Ed
Ch. 8 Chemical Bonding: General Concepts Brady & Senese, 5th Ed Index 8.1. Electron transfer leads to the formation of ionic compounds 8.2. Lewis symbols help keep track of valence electrons 8.3. Covalent
More informationCitation. As Published Publisher. Version
Ab initio investigation of high multiplicity Rþ Rþ [sigma superscript + - sigma superscript +] optical transitions in the spectra of CN and isoelectronic species The MIT Faculty has made this article openly
More informationTheoretical study of the low-lying excited singlet states of furan
JOURNAL OF CHEMICAL PHYSICS VOLUME 119, NUMBER 2 8 JULY 2003 Theoretical study of the low-lying excited singlet states of furan E. V. Gromov, A. B. Trofimov, and N. M. Vitkovskaya Laboratory of Quantum
More informationClass XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry
Class XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents
More informationClass XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry
Class XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents
More information