Abstract
Ab initio calculations rest on solving the Schrödinger equation; the nature of the necessary approximations determines the level of the calculation. In the simplest approach, the Hartree-Fock method, the total molecular wavefunction Ψ is approximated as a Slater determinant composed of occupied spin orbitals. To use these in practical calculations, the spatial part of the spin orbitals is approximated as a linear combination (a weighted sum) of basis functions. Electron correlation methods are also discussed. The main uses of the ab initio method are calculating molecular geometries, energies, vibrational frequencies, spectra, ionization energies and electron affinities, and properties like dipole moments which are connected with electron distribution. These calculations find theoretical and practical applications, since, for example, enzyme-substrate interactions depend on shapes and charge distributions and reaction equilibria and rates depend on energy differences, and spectroscopy plays an important role in identifying and understanding novel molecules. The visualization of calculated phenomena can be very important in interpreting results.
“I could have done it in a much more complicated way,” said the Red Queen, immensely proud.
Attributed, probably apocryphally, to Lewis Carroll
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Notes
- 1.
Douglas Hartree, born in Cambridge, England, 1897. Ph.D. Cambridge, 1926. Professor applied mathematics, theoretical physics, Manchester, Cambridge. Died Cambridge, 1958.
- 2.
John Slater, born in Oak Park Illinois, 1900. Ph.D. Harvard, 1923. Professor of physics, Harvard, 1924–1930; MIT 1930–1966; University of Florida at Gainesville, 1966–1976. Author of 14 textbooks, contributed to solid-state physics and quantum chemistry, developed X-alpha method (early density functional theory method). Died Sanibel Island, Florida, 1976.
- 3.
John Pople, born in Burnham-on-Sea, Somerset, England, 1925. Ph.D. (Mathematics) Cambridge, 1951. Professor, Carnegie-Mellon University, 1960–1986, Northwestern University (Evanston, Illinois) 1986–2004. Nobel Prize in Chemistry in 1998 (with Walter Kohn, Chapter 5, Section 7.1). Died in Chicago, 2004.
- 4.
Møller-Plesset: the Danish-Norwegian letter ø is pronounced like French eu or German ö.
- 5.
F. Neese, personal communication, 2022, July 22.
- 6.
Richard Bader, born in Kitchener, Ontario, Canada, 1931. Ph.D. Massachusetts Institute of Technology, 1958. Professor, University of Ottawa, 1959–1963, McMaster University, 1963–2012. Died in Burlington, Ontario, 2012.
- 7.
R. Hoffmann, personal communication, 2009 August 12.
References
General discussions of and references to ab initio calculations are found in: (a) Levine IN (2014) Quantum chemistry, 7th ed. Prentice Hall, Engelwood Cliffs. (b) Lowe JP (1993) Quantum chemistry, 2nd edn. Academic, New York. (c) Pilar FL (1990) Elementary quantum chemistry, 2nd edn. McGraw-Hill, New York. (d) An advanced book: Szabo A, Ostlund NS (1989) Modern quantum chemistry McGraw-Hill, New York. (e) Foresman JB, Frisch Æ (1996) Exploring chemistry with electronic structure methods. Gaussian Inc., Pittsburgh. (f) Leach AR (2001) Molecular modelling, 2nd edn. Prentice Hall, Essex. (g) A useful reference is still: Hehre WJ, Radom L, Schleyer PvR, Pople JA (1986) Ab initio molecular orbital theory. Wiley, New York. (h) An evaluation of the state and future of quantum chemical calculations, with the emphasis on ab initio methods: Head-Gordon M (1996) J Phys Chem 100:13213. (i) Jensen F (2007) Introduction to computational chemistry, 2nd edn. Wiley, Hoboken. (j) Dewar MJS (1969) The molecular orbital theory of organic chemistry. McGraw-Hill, New York. This book contains many trenchant comments by one of the major contributors to computational chemistry; begins with basic quantum mechanics and ab initio theory, although it later stresses semiempirical theory. (k) Young D (2001) Computational chemistry. A practical guide for applying techniques to real world problems. Wiley, New York. (l) Cramer CJ (2004) Essentials of computational chemistry, 2nd edn. Wiley, Chichester. (m) Hehre WJ (1995) Practical strategies for electronic structure calculations. Wavefunction, Inc., Irvine
Regarding the first use of the term in chemistry: Dewar casts aspersions on this (Dewar MJS (1992) A semiempirical life. In: Seeman JI (ed) Profiles, pathways and dreams series. American Chemical Society, Washington, DC, p. 129) by saying that in the paper in which it evidently first appeared (Parr RG, Craig DP, Ross IG (1950) J Chem Phys 18:1561) it merely meant that the collaboration of Parr on the one hand with Craig and Ross on the other had been carried through from the start in Parr’s lab. However, the PCR paper states “The computations, which are heavy, were carried through independently ab initio by RGP on the one hand, and DPC and IGR on the other.” In this author’s view this means either that both groups did the calculations independently from the beginning, or it is conceivably a nod to the complexity of evaluating complicated integrals without semiempirical assistance in those pre-computer days, and may then indeed be taken as being consonant with the current meaning of the term. Rudenberg states (Rudenberg K, Schwarz WHE (2013) Chapter 1 In: Strom ET, Wilson AK (eds) Pioneers of quantum chemistry. ACS Symposium Series 1122. American Chemical Society, Washington, DC, p 36) that he recalled the use of ab initio by Mulliken in a lecture at the University of Chicago sometime in 1953–1955. The first appearance in print in its unambiguous modern sense seems to be Chen TC (1955) J Chem Phys 23:2200, where it is explicitly contrasted with the term semiempirical
Hartree DR (1928) Proc Cambridge Phil Soc 24:89
(a) The relativistic one-electron Schrödinger equation is called the Dirac equation. It can be used with the Hartree-Fock approach to do Dirac-Fock (Dirac-Hartree-Fock) calculations; see Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs, section 16.11. (b) For a brief discussion of spin-orbit interaction see I. Levine N (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs, section 11.6
The many-body problem in chemistry has been reviewed: Tew DP, Klopper W, Helgaker T (2007) J Comp Chem, 28:1307
Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs, sections 13.4, 13.5 and pp 425–426
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(a) Pauling L (1928) Chem Rev 5:173; see p 208 of this paper. (b) Slater JC (1929) Phys Rev 34:1293. The simple-seeming representation of a wavefunction as a spin orbital determinant made it much easier for physicists to deal with electron spin than by group theory, with which many were, ca. 1930, unfamiliar. In his biography (“Solid-state and molecular theory: a scientific biography”, Wiley-Interscience, New York, 1975), Slater, while acknowledging Pauling’s 1928 paper, says this was his most popular publication, since it was responsible for slaying the Gruppenpest (German for group theory plague). (c) Fock V (1930) Z Physik 61:126. (d) Slater JC (1930) Phys Rev 35:210. In his biography ((b) above, p. 79) Slater says “I had planned to work out these additional terms [with electron exchange], but did not have the opportunity on account of other things I was working on, and in the meantime Fock… independently suggested the method and worked out the details.” This “Note on Hartree’s method” occupies ca. one page; Fock’s paper extends over 23 pages, replete with equations
Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs. sections 7.7 and 10.1
Although it is sometimes convenient to speak of electrons as belonging to a particular atomic or molecular orbital, and although they sometimes behave as if they were localized, no electron is really confined to a single orbital, and in a sense all the electrons in a molecule are delocalized; Dewar MJS (1969) The molecular orbital theory of organic chemistry. McGraw-Hill, New York, pp 139–143
Pilar FL (1990) Elementary quantum chemistry, 2nd edn. McGraw-Hill, New York, pp 200–204
(a) Pople JA, Beveridge DL (1970) Approximate molecular orbital theory. McGraw-Hill, New York, chapters 1 and 2. (b) The first clear, explicit presentation of the UHF procedure: Pople JA, Nesbet RK (1954) J Chem Phys 22:571
Lowe JP (1993) Quantum chemistry, 2nd edn. Academic, New York. Appendix 7
Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs, pp 267–268, 321
Dewar MJS (1969) The molecular orbital theory of organic chemistry. McGraw-Hill, New York. chapter 2
Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs, p 430
Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs, pp 197–198
(a) See e.g. Perrin CL (1970) Mathematics for chemists. Wiley-Interscience, New York, pp 39–41. (b) A caveat on the use of Lagrangian multipliers: Goedecke GH (1966) Am J Phys 34:571
Lowe JP (1993) Quantum chemistry, 2nd edn. Academic, New York, pp 354–355
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Pilar FL (1990) Elementary quantum chemistry, 2nd edn. McGraw-Hill, New York, pp 288–299
(a) Frequencies and zero point energies are discussed in [1g], section 6.3. Some quantum chemists are moving beyond this standard treatment in which electron and nuclear motion are regarded as being uncoupled: Császár AG, Fábri C, Szidarovszky T, Mátyus E, Furtenbacher T, Czakó G (2012) Phys Chem Chem Phys 14:1085. They consider this as characterizing “The fourth age of quantum chemistry”, the first three ages being those seeing increasingly sophisticated treatment of (nuclear-uncoupled) electron motion. So far the fourth (electron-nuclear motion coupled) age seems limited to very small molecules. (b) Cśaszár AG, Furtenbacher T (2015) J Phys Chem A 119:10229
GAUSSIAN 92, Revision F.4: Frisch MJ, Trucks GW, Head-Gordon M, Gill PMW, Wong MW, Foresman JB, Johnson BG, Schlegel HB, Robb MA, Repogle ES, Gomperts R, Andres JL, Raghavachari K, Binkley JS, Gonzales C, Martin RL, Fox DJ, Defrees DJ, Baker J, Stewart JJP, Pople JA (1992) Gaussian, Inc., Pittsburgh
See e.g. Porter GJ and Hill DR (1996) Interactive linear algebra: a laboratory course using mathcad. Springer, New York
Szabo A, Ostlund NS (1989) Modern quantum chemistry. McGraw-Hill, New York, pp 152–171
Szabo A, Ostlund NS (1989) Modern quantum chemistry. McGraw-Hill, New York. Appendix A
Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs. section 15.16
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Gaussian is available for several operating systems; see Gaussian, Inc., http://www.gaussian.com, 340 Quinnipiac St., Bldg. 40, Wallingford, CT 06492, USA. As of 2023, the latest “full” version (as distinct from more frequent smaller revisions) of the Gaussian suite of programs was Gaussian 16. A graphical interface designed specifically for Gaussian is GaussView, also available from Gaussian, Inc.
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SPARTAN is an integrated molecular mechanics, ab initio and semiempirical program with an excellent input/output graphical interface, available for several operating systems: see Wavefunction Inc., http://www.wavefun.com, 18401 Von Karman, Suite 370, Irvine CA 92715, USA. As of 2023, the latest version of Spartan was SPARTAN‘20, available in several versions
Hehre WJ, Radom L, Schleyer P v R, Pople JA (1986) Ab initio molecular orbital theory. Wiley, New York. chapter 4
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Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs. section 15.4
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(a) Lewars E (1998) J Mol Struct (Theochem) 423:173. (b) Lewars E (2000) J Mol Struct (Theochem) 507:165. (c) Kenny JP, Krueger KM, Rienstra-Kiracofe JC, Schaefer HF (2001) J Phys Chem A, 105:7745
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Wiest O, Montiel DC, Houk KN (1997) J Phys Chem A 101:8378. and references therein
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(a) Whole issue of Chem Rev 2015, 115 (12) (b) Clary DC (2006) Science 314:265
Basis sets without polarization functions evidently make lone-pair atoms like tricoordinate N and tricoordinate O+ too flat: Pye CC, **dos JD, Poirer RA, Burnell DJ (1997) J Phys Chem A 101:3371. Other problems with the 3-21G(*) basis are that cation-metal distances tend to be too short (e.g. Rudolph W, Brooker MH, Pye CC (1995) J Phys Chem 99:3793) and that adsorption energies of organics on aluminosilicates are overestimated, and charge separation is exaggerated (private communication ca. 2000 from G. Sastre, Instituto de Technologica Quimica, Universidad Polytechnica de Valencia). Nevertheless, the 3-21G(*) basis apparently usually gives good geometries (section 5.5.1)
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(a) Fowler JE, Galbraith JM, Vacek G, Schaefer HF (1994) J Am Chem Soc 116:9311; (b) Vacek G, Galbraith JM, Yamaguchi Y, Schaefer HF, Nobes RH, Scott AP, Radom L (1994) J Phys Chem 98:8660
DeYonker NJ, Peterson KA, Wilson AK (2007) J Phys Chem A 111:11383, and references therein. This whole issue (number 44) of J Phys Chem A is a tribute to Dunning, and includes a short autobiography
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(a) The special theory of relativity (the one germane to chemistry, since gravity is irrelevant to our science) and its chemical consequences are nicely reviewed in Balasubramanian K (1997) Relativistic effects in chemistry. Parts A and B, Wiley, New York. (b) For a tirade against the conventional way of viewing the effect of velocity on mass see Okum L, Physics Today, 1989, June, 30
See e.g. Jacoby M (1998) Chem Eng News, 23 March, 48. Calculations on an analogue of xenon tetrafluoride with elements 117 and 118
Dirac PAM (1929) [relativity is]…of no importance in the consideration of atomic and molecular structure, and ordinary chemical reactions…. Proc R Soc A123:714
Krauss M, Stevens WJ (1984) Annu Rev Phys Chem 35:357; Szasz L (1985) Pseudopotential theory of atoms and molecules. Wiley, New York. (b) Relativistic Dirac-Fock calculations on closed-shell molecules: Pisani L, Clementi E (1994) J Comput Chem 15:466
(a) Figg T, Webb JR, Cundari TR, Gunnoe TB (2012) J Am Chem Soc 134:2332. (b) Rabilloud F, Harb M, Ndome H, Archirel P (2010) J Phys Chem A 114:6451
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Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs. section 16.11
(a) A good source of information on various kinds of calculations on transition metal compounds is McCleverty JA, Meyer TJ (eds) (2004) Comprehensive coordination chemistry. II. Elsevier, Amsterdam. (b) A detailed review: Frenking G, Antes I, Böhme M, Dapprich S, Ehlers AW, Jonas V, Neuhaus A, Otto M, Stegmann R, Veldkamp A, Vyboishchikov S (1996) Chapter 2. In: Lipkowitz KB, Boyd DB (eds) Reviews in computational chemistry, Volume 8, VCH, New York. (c) The main points of reference [51a] are presented in Frenking G, Pidun U (1997) J Chem Soc Dalton Trans 1653; (d) Cundari TR, Sommerer SO, Tippett, L (1995) J Chem Phys 103:7058
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(a) Hehre WJ, Huang WW, Klunzinger PE, Deppmeier BJ, Driessen AJ (1997) A spartan tutorial. Wavefunction Inc., Irvine. (b) Hehre WJ, Yu J, Klunzinger PE (1997) A Guide to Molecular Mechanics and Molecular Orbital Calculations in Spartan. Wavefunction Inc., Irvine. (c) Hehre WJ, Shusterman AJ, Huang WW (1996) A laboratory book of computational organic chemistry. Wavefunction Inc., Irvine
Bachrach SM (2014) Computational organic chemistry, 2nd edn. Wiley-Interscience, p 298
At the HF level calculated rotation barriers of methyltoluenes become less accurate with very big bases: del Rio A, Boucekkine A, Meinnel J (2003) J Comp Chem 24:2093
At correlated levels bigger bases did not always give better results for metal hydrides; the authors say this “refutes the dogma” that bigger basis sets are necessarily better:: Klein RA, Zottola MA (2006) Chem Phys Lett 419:254
(a) Bartlett RJ, Schweigert IV, Lotrich VF (2006) J Mol Struct (Theochem) 771:1; (b) Lotrich VF, Bartlett RJ, Grabowski I (2005) Chem Phys Lett 405:43. (c) Wilson AK (2004) Abstracts, 60th Southwest Regional meeting of the American Chemical Society, Fort Worth, TX, united States, September 29-October 4; (d) Yau AD, Perera SA, Bartlett RJ (2002) Mol Phys 100:835
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(a) Raghavachari K, Anderson JB (1996) J Phys Chem 100:12960. (b) A historical review: Löwdin P-O (1995) Int J Quantum Chem 55:77. (c) Fermi and Coulomb holes and correlation: [1c], pp 296–297
Pilar FL (1990) Elementary quantum chemistry, 2nd edn. McGraw-Hill, New York, p 286
For example: Hurley AC (1976) Introduction to the electron theory of small molecules. Academic, New York, pp 286–288, or Ermler WC, Kern CW (1974) J Chem Phys 61:3860
Löwdin P-O (1959) Advan Chem Phys 2:207
(a) Scott AP, Radom L (1996) J Phys Chem 100:16502. (b) Sibaev M, Crittenden DL (2015) J Phys Chem A 119:13107
Blanksby SJ, Ellison GB (2003) Acc Chem Res 36:255; Chart 1
See e.g. Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs., chapter 16
Park JW, Al-Saadon R, MacLeod MK, Shiozaki T, Vlaisavljevich B (2020) Chem Rev 120:5878
Brief introductions to the MP treatment of atoms and molecules: (a) Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs, section 16.3. (b) Lowe JP (1993) Quantum chemistry, 2nd edn. Academic, New York, section 11–13. (c) Leach AR (2001) Molecular modelling, 2nd edn. Prentice Hall, Essex., section 3.3.2
Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs. chapter 9
Møller C, Plesset MS (1934) Phys Rev 46:618
Binkley JS, Pople JA (1975) Int J Quantum Chem 9:229
Cramer CJ (2004) Essentials of computational chemistry, 2nd edn. Wiley, Chichester, p section 7.4
Lowe JP (1993) Quantum chemistry, 2nd edn. Academic, New York, pp 367–368
See e.g. Szabo A, Ostlund NS (1989) Modern quantum chemistry. McGraw-Hill, New York, p 353; Leach AR (2001) Molecular modelling, 2nd edn. Prentice Hall, Essex, p 115
See e.g. Prasad VK, Otero-de-la-Rosa A, DiLabio GA (2022) J Chem Theory Comput 18:2208
Boldyrev A, Schleyer PvR, Higgins D, Thomson C, Kramarenko SS (1992) J Comput Chem 9:1066. Fluoro- and difluorodiazomethanes are minima by HF calculations, but are transition states by the MP2 method
H2C=CHOH reaction The only quantitative experimental information on the barrier for this reaction seems to be: Saito S (1976) Chem Phys Lett 42:399, halflife in the gas phase in a Pyrex flask at room temperature ca. 30 minutes. From this one calculates (Sect. 5.5.2.3.4, Eq. (5.202)) a free energy of activation of 93 kJ mol−1. Since isomerization may be catalyzed by the walls of the flask, the purely concerted reaction may have a much higher barrier. This paper also shows by microwave spectroscopy that ethenol has the O-H bond syn to the C=C. The most reliable measurement of the ethenol/ethanal equilibrium constant, by flash photolysis, is 5.89 × 10−7 in water at room temperature (Chiang Y, Hojatti M, Keeffe JR, Kresge AK, Schepp NP, Wirz J (1987) J Am Chem Soc 109:4000). This gives a free energy of equilibrium of 36 kJ mol−1 (ethanal 36 kJ mol−1 below ethenol). HNC reaction The barrier for rearrangement of HNC to HCN has apparently never been actually measured. The equilibrium constant in the gas phase at room temperature was calculated (Maki AG, Sams RL (1981) J Chem Phys 75:4178) at 3.7 × 10−8, from actual measurements at higher temperatures; this gives a free energy of equilibrium of 42 kJ mol−1 (HCN 42 kJ mol−1 below HNC). According to high-level ab initio calculations supplemented with experimental data (Active Thermochemical Tables) HCN lies 62.35±0.36 kJ mol-1 (converting the reported spectroscopic cm-1 energy units to kJ mol−1) below HNC; this is “a recommended value…based on all currently available knowledge”: Nguyen TL, Baraban JH, Ruscic B, Stanton JF (2015) J Phys Chem A 119:10929. CH3NC reaction The reported experimental activation energy is 161 kJ mol−1 (Wang D, Qian X, Peng J (1996) Chem Phys Lett 258:149; Bowman JM, Gazy B, Bentley JA, Lee TJ, Dateo CE (1993) J Chem Phys 99:308; Rabinovitch BS, Gilderson PW (1965) J Am Chem Soc 87:158; Schneider FW, Rabinovitch BS (1962) J Am Chem Soc 84:4215). The energy difference between CH3NC and CH3CN has apparently never been actually measured. Cyclopropylidene reaction Neither the barrier nor the equilibrium constant for the cyclopropylidene/allene reaction have been measured. The only direct experimental information of these species come from the failure to observe cyclopropylidene at 77 K (Chapman OL (1974) Pure and applied chemistry 40:511). This and other experiments (references in Bettinger HF, Schleyer PvR, Schreiner PR, Schaefer HF (1997) J Org Chem 62:9267 and in Bettinger HF, Schreiner PR, Schleyer PvR, Schaefer HF (1996) J Phys Chem 100:16147) show that the carbene is much higher in energy than allene and rearranges very rapidly to the latter. Bettinger et al. 1997 (above) calculate the barrier to be 21 kJ mol−1 (5 kcal mol−1).
(a) Saebø S, Pulay P (1987) J Chem Phys 86:914; Pulay P (1983) Chem Phys Lett 100:151. (b) Vahtras O, Almlöf J, Feyereisen MW, Pulay P (1993) Chem Phys Lett 213:514. (c) Feyereisen M, Fitzgerald G, Komornicki A (1993) Chem Phys Lett 208:359. (d) The virtues of RI-MP2 are extolled in: Jurečka P, Nachtigall P, Hobza P (2001) Phys Chem Chem Phys 3:4578. (e) Deng J, Gilbert ATB, Gill PMW (2015) J Chem Theory Comput 11:1639. (f) Soydaş E, Bozkaya U (2015) J Chem Theory Comput 11:1564
(a) An excellent brief introduction to CI is given in I. Levine N (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs, section 16.2. (b) A comprehensive review of the development of CI: Shavitt (1998) Mol Phys 94:3. (c) See also Lowe JP (1993) Quantum chemistry, 2nd edn. Academic, New York, pp 363–369; Pilar FL (1990) Elementary quantum chemistry, 2nd edn. McGraw-Hill, New York, pp 388–393; Szabo A, Ostlund NS (1989) Modern quantum chemistry. McGraw-Hill, New York, chapter 4; Hehre WJ, Radom L, Schleyer PvR, Pople JA (1986) Ab initio molecular orbital theory. Wiley, New York, pp 29–38
Levine IN (2014) Quantum chemistry, 7th edn. Prentice Hall, Engelwood Cliffs. p 299 and section 16.2
Ben-Amor N, Evangelisti S, Maynau D, Rossi EPS (1998) Chem Phys Lett 288:348
(a) Woodward RB, Hoffmann R (1970) The conservation of orbital symmetry. Academic, New York., chapter 6. (b) Foresman JB, Frisch Æ (1996) Exploring chemistry with electronic structure methods. Gaussian Inc., Pittsburgh, pp 228–236 shows how to do CASSCF calculations. For CAvSSCF calculations on the Diels-Alder reaction, see Li Y, Houk KN (1993) J Am Chem Soc 115:7478. (c) Systematic expansion of active spaces beyond the CASSCF limit: a GASSCF/SplitGAS benchmark study: Vogiatzis KD, Manni GL, Stoneburner SJ, Ma D, Gagliardi L (2015) J Chem Theory Comput 11:3010. (d) Stochastic multiconfigurational self-consistent field theory: Thomas RE, Sun Q, Alavi A, Booth GH (2015) J Chem Theory Comput 11:5316
Cacelli I, Ferretti A, Prampolini G, Barone V (2024) J Chem Theory Comput 2015:11
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(a) Karlstrom G, Lindh R, Malmqvist P-Å, Roos BO, Ryde U, Veryazov V, Widmark P-O, Cossi M Schimmelpfennig B, Neogrady P, Seijo L (2003) Comput Mater Sci 28:222. (b) Anderssson K, Malmqvist P-Å, Roos BO (1992) J Chem Phys 96:1218
Szabo A, Ostlund NS (1989) Modern quantum chemistry. McGraw-Hill, New York. chapter 6
A paper boldly titled “Quadratic CI versus Coupled-Cluster Theory…”: Hrusak J, Ten-no S, Iwata S (1997) J Chem Phys 106:7185
Alberts IL, Handy NC (1988) J Chem Phys 89:2107
(a) Neese F, Wennmohs F, Becker U, Riplinger C (2020) J Chem Phys, 152, 224108. (b) Eriksen JJ, Baudin P, Ettenhuber P, Kristensen K, Kjærgaard T, Jørgensen P (2015) J Chem Theory Comput 11:2984
Bartlett RJ (1981) Ann Rev Phys Chem 32:359
The water dimer has been extensively studied, theoretically and experimentally: (a) Schuetz M, Brdarski S, Widmark P-O, Lindh R, Karlström G (1997) J Chem Phys 107:4597; these report an interaction energy of −20.7 kJ mol−1 (−4.94 kcal mol−1), and give a method of implementing the counterpoise correction with modest basis sets. (b) Halkier A, Koch H, Jorgensen P, Christiansen O, Nielsen MB, Halgaker T (1997) Theor Chem Acc 97:150.; these report an interaction energy of −20.9 kJ mol−1 (−5.0 kcal mol−1). (c) Feyereisen MW, Feller D, Dixon DA (1996) J Phys Chem 100:2993; these workers “best estimate” of binding electronic energy is −20.9 kJ mol−1 (−5.0 kcal mol−1). (d) A general review of the hydrogen bond: Gordon MS, Jensen JH (1996) Acc Chem Res 29:536
For discussions of BSSE and the counterpoise method see: (a) Clark T (1985) A handbook of computational chemistry. Wiley, New York, pp 289–301; (b) Martin JM (1998) Computational thermochemistry. In: Irikura KK, Frurip DJ (eds) American Chemical Society, Washington, D.C., p 223. (c) Thompson MGK, Lewars EG, Parnis JM (2005) J Phys Chem A 109: 9499. (d) van Duijneveldt FB, van Duijneveldt-van JGCM de Rijdt JH van Lenthe Chem Rev, 1994, 94, 1873. (e) L. M. Mentel, E. J. Baerends, J Chem Theory Comput, 2014, 10, 252. (f) References [106] give leading references to BSSE and [106(a)] describes a method for bringing the counterpoise correction closer to the basis set limit. (g) Methods designed to be free of BSSE: Halasz GJ, Vibok A, Mayer I (1999) J Comput Chem 20:274
(a) Xu X, Goddard WA (2004) J Phys Chem A 108:2313. (b) Garza J, Ramírez J-Z, Vargas R (2005) J Phys Chem A 109:643
(a) Conrad JA, Gordon MS (2015) J Phys Chem A 119:5377. (b) Goldey MB, Belzunces B, Head-Gordon M (2015) J Chem Theory Comput 11:4159; (c) Řezáč J, Riley KE, Hobza P (2012) J Chem Theory Comput 8:4285. (d) Řezáč J, Hobza P (2014) J Chem Theory Comput 10:3066. (e) Strutyński K, Gomes JA, Melle-Franco M (2014) J Phys Chem A 118:9561
(a) Boyd DB (2007) Chapter 7. In: Lipkowitz KB, Cundari TR (eds) Reviews in computational chemistry, vol 23. Wiley, Hoboken. (b) Mannhold R, Kubinyi H, Folkers G (eds) (2005) Chemoinformatics in drug discovery. VCH, New York. (c) Höltje H-D, Folkers G (1997) Molecular modelling. VCH, New York. (d) Tropsha A, Bowen JP (1997) Chapter 17. In: Zielinski TJ, Swift ML (eds) Using computers in chemistry and chemical education. American Chemical Society, Washington, DC. (e) Balbes LM, Mascarella SW, Boyd DB (1994) Chapter 7. In: Lipkowitz, KB, Boyd DB (eds) Reviews in computational chemistry, vol 5. VCH, New York. (f) Vinter JL, Gardner M (1994) Molecular modelling and drug design. Macmillan, London
(a) See e.g. Bartlett RJ, Stanton JF (1994) Chapter 2. In: Lipkowitz KB, Boyd DB (eds) Reviews in computational chemistry, vol 5. VCH, New York, p 106. (b) Burkert U, Allinger NL (1982) Molecular mechanics. ACS Monograph 177, American Chemical Society, Washington, DC, pp 6–10. See also Ma B, Lii J-H, Schaefer HF, Allinger NL (1996) J Phys Chem 100:8763; Ma M, Lii J-H, Chen K, Allinger NL (1997) J Am Chem Soc 119:2570
(a) Domenicano A, Hargittai I (eds) (1992) Accurate molecular structures. Oxford University Press, New York. (b) A “wake-up call”: Box VGS (2002) Chem Eng News, Feb. 18, 6
Petersson GA (1998) Chapter 13. In: Irikura KK, Frurip DJ (eds) Computational thermochemistry. American Chemical Society, Washington, DC
Hehre WJ, Radom L, Schleyer PvR, Pople JA (1986) Ab initio molecular orbital theory. Wiley, New York, pp 133–226; note the summary on p. 226
(a) E.g. Engelke R (1992) J Phys Chem 96: 10789. (HF/4-31G, HF/4-31G*, MP2/6-31G*). (b) For references to various calculations see: Lewars E (2008) Modeling marvels. Springer, Amsterdam, pp 151–155
Foresman JB, Frisch Æ (1996) Exploring chemistry with electronic structure methods. Gaussian Inc., Pittsburgh, p 118
Reference [1e], p. 118 (ozone) and p. 128 (FOOF)
Foresman JB, Frisch Æ (1996) Exploring chemistry with electronic structure methods. Gaussian Inc., Pittsburgh, p 36. other calculations on ozone are on pp 118, 137, and 159
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(a) Maciel GS, Bitencourt ACP, Ragni M, Aquilanti V (2007) J Phys Chem A 111:12604. (b) Ju X-H, Wang Z-Y, Yan X-F, **ao H-M (2007) J Mol Struct (Theochem) 804:95
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For thermochemical calculations, at least, fluoroorganics present special problems, e.g. Bond D (2007) J Org Chem 72:7313, and references therein; note p. 7322: “Difficulties in obtaining consistent and accurate data are found even with the simplest of the organofluoro compounds, fluoromethane”
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(a) Clausius R (1867) The mechanical theory of heat, English translation, Editor, Hirst T; John Van Voorst, London. (b) “Die Mechanische Wärmetheorie”, R. Clausius, Zweite Auflage, Druck und Verlag von Friedrich Vieweg und Sohn, 1876; see pp 21 and 33-34. Available online from e.g. https://archive.org/details/diemechanischew01claugoog
(a) Details of statistical mechanics calculations utilizing vibrational frequencies: Ochterski JW (2000) Thermochemistry in Gaussian; www.gaussian.com/g_whitepap/thermo.htm. (b) Details of the calculations of vibrational frequencies in Gaussian: Ochterski JW (2000) Thermochemistry in Gaussian.; http://www.gaussian.com/g_whitepap/vib.htm
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(a) See e.g. Deng W-Q, Han K-L, Zhan J-P, He G-Z (1988) Chem Phys 288:33. (b) Computer simulations of bimolecular reactions: Hase WL, Science 266:998. (c) Non-RRKM unimolecular reactions: Lourderaj U, Hase WL (2009) J Phys Chem A 113:2236
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(a) McGlashan ML (1979) Chemical thermodynamics. Academic, London; (b) Nash LK (1968) Elements of statistical thermodynamics. Addison-Wesley, Reading; (c) A good, brief introduction to statistical thermodynamics is given by Irikura KK (1998) Computational thermochemistry. In: Irikura KK, Frurip DJ (eds) American Chemical Society, Washington, DC, Appendix B
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See Irikura KK, Frurip DJ, chapter 1, Benson SW, Cohen N, chapter 2, and Zachariah MR, Melius CF, chapter 9. In Irikura KK, Frurip DJ (eds) Computational thermochemistry. American Chemical Society, Washington, DC
These bond energies were taken from Fox MA, Whitesell JK (1994) Organic chemistry. Jones and Bartlett, Boston, p 72
Although in the author’s opinion it works well in chemistry, the disorder concept can lead to misunderstanding: a discussion of such popular misconceptions of entropy is given by Lambert FL (1999) J Chem Educ 76:1385. Related discussions can be invoked on the web with the words “Lambert entropy”.
For good accounts of the history and meaning of the concept of entropy, see (a), (b): (a) von Baeyer HC (1998) Maxwell’s Demon. Why warmth disperses and time passes. Random House, New York. (b) Greenstein G (1998) Portraits of discovery. Profiles in scientific genius, chapter 2 (“Ludwig Boltzmann and the second law of thermodynamics”). Wiley, New York
Hehre WJ, Radom L, Schleyer P v R, Pople JA (1986) Ab initio molecular orbital theory. Wiley, New York. section 6.3.9
A sophisticated study of the calculation of gas-phase equilibrium constants: Bohr F, Henon E (1998) J Phys Chem A 102:4857
A very comprehensive treatment of rate constants, from theoretical and experimental viewpoints, is given in Steinfeld JI, Francisco JS, Hase WL (1999) Chemical kinetics and dynamics. Prentice Hall, New Jersey
For the Arrhenius equation and problems associated with calculations involving rate constants and transition states see Durant JL in Irikura KK, Frurip DJ in Computational thermochemistry. Irikura KK, Frurip DJ (eds) American Chemical Society, Washington, D.C., 1998, chapter 14
E.g., Atkins PW (1998) Physical chemistry, 6th edn. Freeman, New York, p 949
Chemical kinetics and dynamics. Prentice Hall, New Jersey, 1999, p 302
Some barriers/room temperature halflives for unimolecular reactions: (a) Decomposition of pentazole and its conjugate base: 75 kJ mol−1/10 minutes and 106 kJ mol−1/2 days, respectively: Benin V, Kaszynski P, Radziszki JG (2002) J Org Chem 67:1354. (b) Decomposition of CF3CO)OOO(COCF3): 86.5 kJ mol−1/1 min: Ahsen Sv, Garciá P, Willner H, Paci MB, Argüello G (2003) Chem Eur J 9:5135. (c) Racemization of a twisted pentacene: 100 kJ mol−1/6-9 h: Lu J, Ho DM, Vogelaar NJ, Kraml CM, Pascal Jr. RA (2004) J Am Chem Soc 126:11168
Lewars E (2008) Modeling marvels: computational anticipation of novel molecules. Springer, Netherlands; chapter 10
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The first in the series was Gaussian 70 and the latest (early 2023) is Gaussian 16. Gaussian Inc., 340 Quinnipiac St Bldg 40, Wallingford, CT 06492 USA. Info@gaussian.com
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Gaussian 94 for Windows (G94W): Gaussian 94, Revision E.1, Frisch MJ, Trucks GW, Schlegel HB, Gill PMW, Johnson BG, Robb MA, Cheeseman JR, Keith T, Petersson GA, Montgomery JA, Raghavachari K, Al-Laham MA, Zakrzewski VG, Ortiz JV, Foresman JB, Cioslowski J, Stefanov BB, Nanayakkara A, Challacombe M, Peng CY, Ayala PY, Chen W, Wong MW, Andres JL, Replogle ES, Gomperts R, Martin RL, Fox DJ, Binkley JS, Defrees DJ, Baker J, Stewart JP, Head-Gordon M, Gonzalez C, Pople JA (1995) Gaussian, Inc., Pittsburgh PA. G94 and G98 are available for both UNIX workstations and PCs
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(a) Worked examples, with various fine points: Irikura KK, Frurip DJ (1998) Computational thermochemistry, Irikura KK, Frurip DJ (eds). American Chemical Society, Washington, DC, Appendix C; (b) Heats of formation of neutral and cationic chloromethanes: Rodrigues CF, Bohme DK, Hopkinson AC (1996) J Phys Chem 100:2942. (c) Heats of formation, entropies and enthalpies of neutral and cationic enols: Turecek F, Cramer CJ (1995) J Am Chem Soc 117:12243. of neutral and cationic enols: (d) Heats of formation by ab initio and molecular mechanics: DeTar DF (1995) J Org Chem 60:7125. (e) Heats of formation and antiaromaticity in strained molecules: Glukhovtsev MN, Laiter S, Pross A (1995) J Phys Chem 99:6828. (f) Heats of formation of organic molecules with the aid of ab initio and group equivalent methods: Schmitz LR, Chen YR (1994) J Comp Chem 15:1437. (f) Isodesmic reactions in ab initio calculation of enthalpy of formation of cyclic C6 hydrocarbons and benzene isomers: Li Z, Rogers DW, McLafferty FJ, Mandziuk M, Podosenin AV (1999) J Phys Chem A 103: 426. (g) Isodesmic reactions in ab initio calculation of enthalpy of formation of benzene isomers: Cheung Y-S, Wong C-K, Li W-K (1998) Mol Struct (Theochem) 454:17
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Spartan ‘04. Wavefunction Inc., http://www.wavefun.com, 18401 Von Karman, Suite 370, Irvine CA 92715, USA
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Carefully defined atom charges are, it has been said, “in principle subject to experimental realization”: Cramer CJ (2004) Essentials of computational chemistry, 2nd edn. Wiley, Chichester, section 9.1.3
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Some examples: (a) General survey: Bridgeman A, Cavigliasso G, Ireland LR, Rothery J (2001) J Chem Soc Dalton Trans 2095; (b) Ruthenium complexes: Fowe EP, Therrien B, Suss-Fink G, Daul C (2008) Inorg Chem 47:42. (c) Simple sulfur compounds: Mayer I, Revesz M (1983) Inorganica Chimica Acta, 77: L205
Cramer CJ (2004) Essentials of computational chemistry, 2nd edn. Wiley, Chichester, pp 312–315
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(a) Coulson’s remarks: Bolcer JD, Hermann RB (1996) Chapter 1 in Reviews in computational chemistry, vol 5. Lipkowitz KB, Boyd DB (eds). VCH, New York, p 12; see too further remarks, quoted on p. 13. (b) The increase in computer speed is also dramatically shown in data provided in Gaussian News, 1993, 4, 1. The approximate times for a single-point HF/6-31G** calculation on 1,3,5-triamino-2,4,6-trinitrobenzene (300 basis functions) are reported as: ca. 1967, on a CDC 1604, 200 years (estimated); ca. 1992, on a 486 DX personal computer, 20 hours. This is a speed factor of 90,000 in 25 years. The price factor for the machines may not be as dramatic, but suffice it to say that the CDC 1604 was not considered a personal computer. In mid-2009, on a well-endowed personal computer (ca. $4000) these results were obtained for single-point HF/6-31G** calculations on 1,3,5-triamino-2,4,6-trinitrobenzene: starting from a C3 geometry, 23 seconds; starting from a C1 geometry, 42 seconds. The increase in speed represented by 42 seconds in 2009 is, cf. 200 years in 1967, a factor of about 108 in 42 years; cf. 20 hours in 1992, a factor of about 1700 in 17 years
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Appendices
Easier Questions
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1.
In the term Hartree-Fock, what, essentially, were the contributions of each of these two people?
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2.
What is a spin orbital? A spatial orbital?
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3.
At which step in the derivation of the Hartree-Fock energy does the assumption that each electron sees an “average electron cloud” appear?
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4.
For a closed-shell molecule in the ground electronic state, the number of occupied molecular orbitals is half the number of electrons, but there is no limit to the number of virtual orbitals. Explain.
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5.
In the simple Hückel method, csi denotes the basis function coefficient for the contribution of atom number s (in whatever numbering scheme we choose) to MO number i. In the ab initio method, csi still refers to MO number i, but the s does not necessarily denote atom number s. Explain.
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6.
The derivation of the Roothaan-hall equations involves some key concepts: Slater determinant, Schrödinger equation, explicit Hamiltonian operator, energy minimization, and LCAO. Using these, summarize the steps leading to the Roothaan-Hall equations FC = Scε.
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7.
What are the similarities and the differences between the basis set of the extended Hückel method and the ab initio STO-3G basis set?
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8.
In the simple and extended Hückel methods, the molecular orbitals are calculated and then filled from the bottom-up with the available electrons. However, in ab initio calculations, the occupancy of the orbitals is taken into account as they are being calculated. Explain.
Hint: look at the expression for the Fock matrix elements in terms of the density matrix.
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9.
Isodesmic reactions have been used to investigate aromatic stabilization, but there is not a unique isodesmic reaction for each problem. Write two isodesmic reactions for the ring-opening of benzene, both of which have on each side of the equation the same number of each kind of bond. Have you any reason to prefer one of the equations to the other?
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10.
List the strengths and weaknesses of ab initio calculations compared to molecular mechanics and extended Hückel calculations. State the molecular features that can be calculated by each method.
Harder Questions
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1.
Does the term ab initio imply that such calculations are “exact”? In what sense might ab initio calculations be said to be semiempirical – or at least not fully a priori?
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2.
Can the Schrödinger equation be solved exactly for a species with two protons and one electron? Why or why not?
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3.
The input for an ab initio calculation (or a semiempirical calculation of the type discussed in Chap. 6, or a DFT calculation – Chap. 7) on a molecule is usually just the cartesian coordinates of the atoms (plus the charge and multiplicity). So how does the program know where the bonds are, that is, what the structural formula of the molecule is?
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4.
Why is it that (in the usual treatment) the calculation of the internuclear repulsion energy term is easy, in contrast to the electronic energy term?
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5.
In an ab initio calculation on H2 or HHe+, one kind of interelectronic interaction does not arise; what is it and why?
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6.
Why are basis functions not necessarily the same as atomic orbitals?
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7.
One desirable feature of a basis set is that it should be “balanced.” How might a basis set be unbalanced?
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8.
In a Hartree-Fock calculation, you can always get a lower energy (a “better” energy, in the sense that it is closer to the true energy) for a molecule by using a bigger basis set, as long as the HF limit has not been reached. Yet a bigger basis set does not necessarily give better geometries and better relative (i.e., activation and reaction) energies. Why is this so?
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9.
Why is size consistency in an ab initio method considered more important than variational behavior (MP2 is size consistent but not variational)?
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10.
A common alternative to writing a Hartree-Fock wavefunction as an explicit Slater determinant is to express it using a permutation operator \( \hat{P} \) which permutes (switches) electrons around in MOs. Examine the Slater determinant for a two-electron closed-shell molecule, and then try to rewrite the wavefunction using. \( \hat{P}. \)
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Lewars, E.G. (2024). Ab Initio Calculations. In: Computational Chemistry. Springer, Cham. https://doi.org/10.1007/978-3-031-51443-2_5
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