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Introductory Aspects

Conference paper
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Part of the NMR Basic Principles and Progress Grundlagen und Fortschritte book series (NMR, volume 12)

Abstract

The halogens have been described as “the most perfect series we have” [1]. The chemical properties of the halogens are indeed very similar even though important differences are apparent. The group name “halogen”, which was coined in the early 19th century, is derived from αλζ, the Greek word for sea-salt, and γεν, the Greek for produce. The group name thus emphasizes the facility with which these atoms form ionic compounds with a formal negative unit charge on the halogen (X). *) Equally well known are covalent halogen compounds with bonds of the type R-X. In fact with the exception of helium, neon and argon all elements in the Periodic Table can form halogen compounds of some kind.

Keywords

Field Gradient Nuclear Spin Quadrupole Moment Electric Field Gradient Larmor Frequency 
These keywords were added by machine and not by the authors. This process is experimental and the keywords may be updated as the learning algorithm improves.

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References to Table 1.1

  1. (a).
    Handbook of Chemistry and Physics, 51st ed. 1970/71. Cleveland: The Chemical Rubber Co.Google Scholar
  2. (b).
    Downs, A.J., Adams, C.J., in: Comprehensive Treatment of Inorganic Chemistry, Vol.2, p.1107 ff. Oxford: Pergamon Press 1973.Google Scholar
  3. (c).
    Franklin, J.L., et al.: Ionization potentials, appearance potentials and heats of formation of gaseous positive ions. National Bureau of Standards, Reference Data Series 26 (1969); U.S. Department of Commerce.Google Scholar
  4. (d).
    Mulliken, R.S.: J. Chem. Phys. 2, 782 (1934); ibid. 3, 573 (1935).CrossRefGoogle Scholar
  5. (e).
    Sanderson, R.T.: J. Phys. Chem. 63, 745 (1959).CrossRefGoogle Scholar
  6. (f).
    Dewar, M.J.S.: The Molecular Theory of Organic Chemistry. New York: McGraw-Hill 1969.Google Scholar
  7. (g).
    Allred, A.L., Rochow, E.G.: J. Inorg. Nuclear Chem. 5, 264 (1958).CrossRefGoogle Scholar
  8. (h).
    Desnoyers, J.E., Jolicoeur, C., in: Modern Aspects of Electrochemistry, Vol.5 (eds. J.O. Bockris and B. Conway). London: Butterworths 1969.Google Scholar
  9. (i).
    Lucken, E.A.C.: Nuclear Quadrupole Coupling Constants. London: Acad. Press 1969.Google Scholar
  10. (j).
    Pauling, L.: The Nature of the Chemical Bond. 3rd ed. Ithaca: Cornell Univ. Press 1960.Google Scholar
  11. (k).
    Goldschmidt, V.M., Skrifter Norske Videnskaps-Akad., Oslo: Mat. Nat. Kl. 1, 21 (1926).Google Scholar
  12. (l).
    Gourary, B.S., Adrian, F.J.: Solid State Physics 1, 127 (1960).CrossRefGoogle Scholar

Copyright information

© Springer-Verlag Berlin Heidelberg 1976

Authors and Affiliations

  1. 1.Department of Physical Chemistry Chemical CentreUniversity of LundLundSweden

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