Bond Enthalpy Transferability - is it Achievable?

  • J. A. Connor
Chapter
Part of the NATO ASI Series book series (ASIC, volume 367)

Abstract

The provision of experimental data for compiling a table of values from which the heat of every possible chemical reaction can be calculated was declared as the aim of thermochemistry by Rossini,1 many years ago. Subsequently, this purpose was broadened2 to include the derivation of the heats of formation of compounds from their constituent elements and the relationship of these results to the chemical binding energies in the molecules. The “classical” examples of chemical binding energies come close to the beginning of anyone’s serious study of chemistry. Much understanding of deep significance has followed from these data: electronegativity, ideas about aromaticity, bond polarity and ionic character, are examples. Coherent with these has been the development of a relation between bond length and bond enthalpy (strength). This leads to the still widely held perception that a “long” bond is a “weak” bond. This, in turn, is related to bond order: an interatomic bond of high order is both shorter and stronger than a bond of lower order between the same two elements. There is a lot of reliable experimental evidence to support these principles when elements of the first short period (n = 2) are considered. In the second short period (n=3; ℓ =0,1) the position is more confused. The lack of a substantial base of data for enthalpies of formation must be held responsible for this, in part at least.

Keywords

Bond Dissociation Energy Metal Carbonyl Mass Spectrometric Measurement Iron Carbonyl Bomb Calorimetry 
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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Copyright information

© Springer Science+Business Media Dordrecht 1992

Authors and Affiliations

  • J. A. Connor
    • 1
  1. 1.Chemical Laboratory University of Kent CanterburyUK

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