Electronegativity from, 45-6

Gordy W. (1946). A new method of determining electronegativity from other atomic properties. Phys. Rev., 69 604-607. 

Crystal radius, orbital radius, and ionization potential from Karplus and Porter (1970). Electronegativity from Pauling (1970). 

Fig. 5.33 Bipherylene. Shaded ort>iiaJs have increased p character hence unshaded ortiital has increased s character, increased electronegativity. [From Streilwieser. A.. Jr. Ziegler,...

A. Domenicano, Structural Substituent Effects in Benzene Derivatives. In Accurate Molecular Structures, A. Domenicano and I. Hargittai, eds., Oxford University Press, Oxford, 1992, pp. 437-468 See, also, A. R. Campanelli, A. Domenicano, F. Ramondo, I. Hargittai, Group Electronegativities from Benzene Ring Deformations A Quantum Chemical Study. J. Phys. Chem. A, 2004, 108, 4940-1948. 

Since Parr et al. have defined electronegativity from density functional theory as the negative of the chemical potential p, the value of the electronegativity % is then given by equation (146). 

Compounds of carbon in each case maximum deviation is for COa. f Using second set of electronegativities from Table II. 

Christian Khxbiill Jorgensen Optical electronegativities from electron transfer spectra... 

Calculation of electronegativities from bond energies requires averaging over a number of compounds to cancel out experimental uncertainties and other minor effects. Methods that use ionization energies and other atomic properties can be calculated more directly. The electronegativities reported here and in Appendix B-4 are suitable for most uses, but the actual values for atoms in molecules may differ from this average, depending on their electronic environment. 

Figure 935. A. Relationship between the isotropic chemical shift and the mean Pb-O bond length in lead compounds. Filled symbols denote sites with CN < 7, open symbols denote CN > 7. B. Relation between the Pb isotropic chemical shift in lead compounds and P, a parameter defined in Equation 9.10 taking into account the degree of oxygen hybridisation and the next-nearest neighbour electronegativity. From Fayon et al. (1997), by permission of the American Chemical Society.

For methods of calculating group electronegativities from Mulliken-Ja(f< electronegativity values of the constituent atoms, see Bratsch, S. G. J. Chem. Educ. 1985, 62, 101-103. 

Table 1.3 Comparison of the characteristics of the carbon-halogen and carbon-carbon bonds (bond lengths in pm binding energies in kcal mol electronegativities from Ref [3] dipole moments in D Van derXXftials radii in pm from Ref [4] atom polarizabilities a in 10 cm from Ref [5]).

Fig. 5.33 Biphenylene. Shaded orbitals have increased p character hence unshaded orbital has increased s character, increased electronegativity. [From Streitwieser, A.. Jr. Ziegler. G. R. Mowry, P. C. Lewis. A. Lawler, R. G. J. Am. Chem. Soc. 1968, 90, 1357-1359. Reproduced with permission.)...

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