Explaining the Chemical Bond: Idealisation and Concretisation

  • Hinne Hettema
Chapter
Part of the European Studies in Philosophy of Science book series (ESPS, volume 7)

Abstract

In this chapter, I focus on the ‘chemical bond’ – the phenomenon of bonding between two atoms – as an example of potential Nagelian reduction. There are two main competing theories, the Molecular Orbital and the Valence Bond theory, which provide a view from quantum mechanics on the phenomenon of bonding. The efficacy of both theories can be compared. It is furthermore interesting that there are systemic ways in which these theories can be improved, leading to the same computational view on the phenomenon of bonding. This means that the resulting structure is an idealisation/concretisation pair.

References

  1. Bader RFW (1990) Atoms in molecules: a quantum theory. Oxford/New York, Clarendon Press.Google Scholar
  2. Bader RFW (2009) Bond paths are not chemical bonds. J Phys Chem 113:10391–10396CrossRefGoogle Scholar
  3. Brush SG (1999a) Dynamics of theory change in chemistry: part 1. The benzene problem 1865–1945. Stud Hist Philos Sci A 30(1):21–79. http://www.sciencedirect.com/science/article/B6V70-3VTSBDX-2/2/9817d70b722935077a85e5f9ce1499ef CrossRefGoogle Scholar
  4. Brush SG (1999b) Dynamics of theory change in chemistry: part 2. Benzene and molecular orbitals, 1945–1980. Stud Hist Philos Sci A 30(2):263–302. http://www.sciencedirect.com/science/article/B6V70-3WG368S-3/2/3808ad4dafb8ac2cae28f47662e7a9ca CrossRefGoogle Scholar
  5. Coulson CA (1952) Valence. Oxford University Press, New YorkGoogle Scholar
  6. Darden L, Maull N (1977) Interfield theories. Philos Sci 44(1):43–64. http://www.jstor.org/stable/187099 CrossRefGoogle Scholar
  7. Goeppert-Mayer M, Sklar D (1938) Calculation of the lower excited levels of Benzene. J Chem Phys 6:645–652CrossRefGoogle Scholar
  8. Hall GG (1951) The molecular orbital theory of chemical valency. VIII. A method of calculating ionization potentials. Proc R Soc Lond A Math Phys Sci 205(1083):541–552. http://www.jstor.org/stable/98703 CrossRefGoogle Scholar
  9. Harris ML (2008) Chemical reductionism revisited: Lewis, Pauling and the physico-chemical nature of the chemical bond. Stud Hist Philos Sci 39(1):78–90. doi:10.1016/j.shpsa.2007.11.006CrossRefGoogle Scholar
  10. Healy E (2011) Heisenberg’s chemical legacy: resonance and the chemical bond. Found Chem 13:39–49. doi:10.1007/s10698-011-9104-2, http://dx.doi.org/10.1007/s10698-011-9104-2 CrossRefGoogle Scholar
  11. Heitler W, London F (1927) Wechselwirkung neutraler Atome und homöopolare Bindung nach der Quantenmechanik. Z Phys 44:455–472CrossRefGoogle Scholar
  12. Hendry RF (2004) The physicists, the chemists, and the pragmatics of explanation. Philos Sci 71:1048–1059CrossRefGoogle Scholar
  13. Hendry RF (2008) Two conceptions of the chemical bond. Philos Sci 75(5):909–920. doi:10.1086/594534, http://www.journals.uchicago.edu/doi/abs/10.1086/594534, http://www.journals.uchicago.edu/doi/pdf/10.1086/594534
  14. Hettema H (2000) Quantum chemistry: classical scientific papers. World Scientific, SingaporeCrossRefGoogle Scholar
  15. Hettema H (2008) A note on Michael Weisberg’s: challenges to the structural conception of chemical bonding. Found Chem 10(2):135–142. doi:10.1007/s10698-008-9045-6, http://www.springerlink.com/content/xhg58121742640h3 CrossRefGoogle Scholar
  16. Hückel E (1931) Quantentheoretische Beiträge zum Benzolproblem. Z Phys 70(3):204–286. http://dx.doi.org/10.1007/BF01339530 CrossRefGoogle Scholar
  17. Hund F (1927) Zur Deutung der Molekelspektren. I. Z Phys 40(10):742–764. doi:10.1007/BF01400234CrossRefGoogle Scholar
  18. Hylleraas EA (1929) Neue Berechnung der Energie des Heliums im Grundzustande, sowie des tiefsten Terms von Ortho-Helium. Z Phys 54(5):347–366. http://dx.doi.org/10.1007/BF01375457 CrossRefGoogle Scholar
  19. Kuipers TAF (2000) From instrumentalism to constructive realism. Synthese library, vol 287. Kluwer Academic Publishers, DordrechtGoogle Scholar
  20. Lagowski JJ (1966) The chemical bond. No. G-2 in classic researches in general chemistry. Houghton Mifflin, BostonGoogle Scholar
  21. Lennard-Jones JE (1929) The electronic structure of some diatomic molecules. Trans Faraday Soc 25:668CrossRefGoogle Scholar
  22. Lennard-Jones J (1949a) The molecular orbital theory of chemical valency. I. The determination of molecular orbitals. Proc R Soc Lond A 198:1–13. doi:10.1098/rspa.1949.0083CrossRefGoogle Scholar
  23. Lennard-Jones J (1949b) The molecular orbital theory of chemical valency. II. Equivalent orbitals in molecules of known symmetry. Proc R Soc Lond A Math Phys Sci 198(1052): 14–26. doi:10.1098/rspa.1949.0084, http://rspa.royalsocietypublishing.org/content/198/1052/14.abstract, http://rspa.royalsocietypublishing.org/content/198/1052/14.full.pdf+html
  24. Lewis GN (1916) The atom and the molecule. J Am Chem Soc 38:762–785CrossRefGoogle Scholar
  25. Lewis GN (1933) The chemical bond. J Chem Phys 1:17–28CrossRefGoogle Scholar
  26. London F (1928) Zur Quantentheorie der homöopolaren Valenzzahlen. Z Phys 46:455–477CrossRefGoogle Scholar
  27. McWeeny R (1979) Coulson’s valence. Oxford University Press, Oxford/New York/TorontoGoogle Scholar
  28. Mulliken RS (1928a) The assignment of quantum numbers for electrons in molecules. I. Phys Rev 32(2):186–222. doi:10.1103/PhysRev.32.186CrossRefGoogle Scholar
  29. Mulliken RS (1928b) The assignment of quantum numbers for electrons in molecules. II. Correlation of molecular and atomic electron states. Phys Rev 32(5):761–772. doi:10.1103/PhysRev.32.761Google Scholar
  30. Mulliken RS (1931) The interpretation of band spectra. Part IIc. Empirical band types. Rev Mod Phys 3(1):89–155. http://link.aps.org/abstract/RMP/v3/p89 Google Scholar
  31. Mulliken RS (1932) Electronic structures of polyatomic molecules and valence. Phys Rev 40(1):55–62. http://link.aps.org/abstract/PR/v40/p55 CrossRefGoogle Scholar
  32. Mulliken RS (1935) Electronic structures of polyatomic molecules and valence VI. On the method of molecular orbitals. J Chem Phys 3(7):375–378. http://link.aip.org/link/?JCP/3/375/1 CrossRefGoogle Scholar
  33. Nagel E (1961) The structure of science: problems in the logic of scientific explanation. Routledge and Kegan Paul, LondonGoogle Scholar
  34. Nowak L (1980) The structure of idealization. D. Reidel, Dordrecht/BostonCrossRefGoogle Scholar
  35. Nye MJ (1993) From chemical philosophy to theoretical chemistry: dynamics of matter and dynamics of disciplines 1800–1950. University of California Press, BerkeleyGoogle Scholar
  36. Park BS (2000) The contexts of simultaneous discovery: Slater, Pauling and the origins of hybridisation. Stud Hist Philos Mod Phys 31B:451–474CrossRefGoogle Scholar
  37. Pauling L (1928) The shared-electron chemical bond. Proc Natl Acad Sci U S A 14(4):359–362CrossRefGoogle Scholar
  38. Pauling L (1931) The nature of the chemical bond. Application of results obtained from the quantum mechanics and from a theory of paramagnetic susceptibility to the structure of molecules. J Am Chem Soc 53(4):1367–1400CrossRefGoogle Scholar
  39. Roothaan CCJ (1951) New developments in molecular orbital theory. Rev Mod Phys 23(2):69–89. doi:10.1103/RevModPhys.23.69CrossRefGoogle Scholar
  40. Russell C (1971) The history of valency. Leicester University Press, LeicesterGoogle Scholar
  41. Slater JC (1931a) Directed valence in polyatomic molecules. Phys Rev 37(5):481–489. doi:10.1103/PhysRev.37.481CrossRefGoogle Scholar
  42. Spector M (1978) Concepts of reduction in physical science. Philosophical monographs, second annual series. Temple University Press, PhiladelphiaGoogle Scholar
  43. Stranges AN (1982) Electrons and valence: development of the theory, 1900–1925, 1st edn. Texas A&M University Press, College StationGoogle Scholar
  44. Sutcliffe BT (1996) The development of the idea of a chemical bond. Int J Quantum Chem 58(6):645–655. http://dx.doi.org/10.1002/(SICI)1097-461X(1996)58:6<645::AID-QUA7>3.0.CO;2-Y
  45. Van Vleck JH, Sherman A (1935) The quantum theory of valence. Rev Mod Phys 7(3):167–228. doi:10.1103/RevModPhys.7.167CrossRefGoogle Scholar
  46. Weisberg M (2008) Challenges to the structural conception of chemical bonding. Philos Sci 75:932–946CrossRefGoogle Scholar
  47. Woody AI (2000) Putting quantum mechanics to work in chemistry: The power of diagrammatic representation. Philos Sci 67(Suppl):S612–S627. Proceedings of the 1998 biennial meetings of the philosophy of science association. Part II: symposia papersGoogle Scholar

Copyright information

© Springer International Publishing AG 2017

Authors and Affiliations

  • Hinne Hettema
    • 1
  1. 1.Department of PhilosophyUniversity of AucklandAucklandNew Zealand

Personalised recommendations