Electronegativity orbital effects

PhysProp Effective Nuclear Charge - Ionisation energy - Electron Affinity - Covalent and Ionic Radii - Electronegativity - Orbital Energies and Promotional energies. 

Because of the absence of 7r-orbital effects, the bond strength of HX, where X is any element, depends almost entirely on the electronegativity of X. ranges from 42 kcal for CsH to 136 kcal for HF, for the Main-Group elements. For the... 

Spin-orbit effects change the strength of the ionic bonding by making the electron in a y = / — 1/2 (y = / -t-1/2) spinor more (less) electronegative. 

Due to spin-orbit interactions, Rg increases and (Og decreases for the group 17 fluorides, and the changes are more substantial for the heavier halogens, as expected. Spin-orbit effects on the molecular properties of IF are in good agreement with Cabrol et al. s CIPSI/CIPSO(MRCI) result [122]. The A o g values of 0.01 and 0.06 A for IF and AtF, respectively, are larger than those of the hydrides, whereas the A Rg of (117)F are smaller than that of (117)H. The Ag Dg of IF is very similar to that of HI. The A oDg of AtF is -0.18 eV, and about 25 % of the -0.67 eV value of HAt. The electronegative F atom can easily polarize the expanded and destabilized spinor. Since this polarization increases... 

An sp hybrid orbital of carbon has approximately the same shape as an sp hybrid orbital. However, an sp hybrid orbital has 33% s character compared to 25% s character for an sp hybrid orbital. As the percent s character of hybrid orbitals increases, the electrons in the hybrid orbitals are closer to the nucleus. Therefore, the electrons in an sp hybrid orbital are closer to the nucleus than the electrons in an sp hybrid orbital. Increasing the percent s character of a hybrid orbital effectively increases the electronegativity of the carbon atom. 

Acidity and basicity depend on the various factors that influence the position of the equilibrium between an acid HA and its conjugate base A. These include orbital effects, electronegativity, inductive effects, resonance effects, solvation hydrogen bonding, steric effects, and aromaticity. 

The PEOE method leads to only partial equalization of orbital electronegativities. Thus, each atom of a molecule retains, on the basis of Eq. (12), a residual electronegativity that measures its potential to attract further electrons. It has been shown that the values of residual electronegativities can be taken as a quantitative measure of the inductive effect [35]. 

An easy way to keep track of the effect of the s character of carbon is to associ ate It with electronegativity As the s character of carbon increases so does that carbon s electronegativity (the electrons m the bond involving that orbital are closer to carbon) The hydrogens m C—H bonds behave as if they are attached to an increasingly more electronegative carbon m the series ethane ethylene acetylene... 

In this case, the ti-MOs resemble those of butadiene. Relative to the butadiene orbitals, however, the acrolein orbitals lie somewhat lower in energy because of the effect of the more electronegative oxygen atom. This factor also increases the electron density at oxygen relative to carbon. 

---