Covalent bonds and electronegativity

Polar Covalent Bonding Electronegativity and Dipole Moments... 

Polar Covalent Bonds, Electronegativity, and Bond Dipoles 11... 

Covalent Bonding, Electronegativity, and Bond Polarity (Sections 8.3 and 8.4)... 

Electronegativity (Section 2.1) The ability of an atom to attract electrons in a covalent bond. Electronegativity increases across the periodic table from right to left and from bottom to top. 

These descriptors have been widely used for the past 25 years to study chemical reactivity, i.e., the propensity of atoms, molecules, surfaces to interact with one or more reaction partners with formation or rupture of one or more covalent bonds. Kinetic and/or thermodynamic aspects, depending on the (not always obvious and even not univoque) choice of the descriptors were hereby considered. In these studies, the reactivity descriptors were used as such or within the context of some principles of which Sanderson s electronegativity equalization principle [16], Pearson s hard and soft acids and bases (HSAB) principle [17], and the maximum hardness principle [17,18] are the three best known and popular examples. 

Know the meaning of electropositive, electronegative, ionic and covalent bonds, radical, catenation, polar covalent bond, single and multiple bonds, nonbonding or unshared electron pair, bond length, bond energy. 

This chapter provides a substantial introduction to molecular structure by coupling experimental observation with interpretation through simple classical models. Today, the tools of classical bonding theory—covalent bonds, ionic bonds, polar covalent bonds, electronegativity, Lewis electron dot diagrams, and VSEPR Theory—have all been explained by quantum mechanics. It is a matter of taste whether to present the classical theory first and then gain deeper insight from the... 

To assess the importance of nucleophilic substitution reactions of naturally occurring nucleophiles it is necessary to have some measure of their reactivity, relative to OH" and HjO. A number of properties of nucleophiles, all of which are some measure of the nucleophile s ability to donate electrons to an electrophile, have been used to correlate nucleophilic reactivity. These closely related properties include basicity, oxidation potential, polarizability, ionization potential, electronegativity, energy of the highest filled molecular orbital, covalent bond strength, and size (Jencks, 1987). 

Only limited comparisons can be made with the transition metal data, but the same broad trends are discernible electronegative ligands such as the halide ions and O-donor ligands give small values, and the much more covalently bonded hydride and carbanionic ligands give the most negative values. The tin data seem to show rather less discrimination between the... 

The unequal distribution of charge produced when elements of different electronegativities combine causes a polarity of the covalent bond joining them and, unless this polarity is balanced by an equal and opposite polarity, the molecule will be a dipole and have a dipole moment (for example, a hydrogen halide). Carbon tetrachloride is one of a relatively few examples in which a strong polarity does not result in a molecular dipole. It has a tetrahedral configuration... 

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