Bond heteropolar

Chemisorption of a gas on a metal surface may involve heteropolar bonding represented by structures (1) or (2) ... 

The simple theory of the heteropolar bond was developed rapidly in contrast to the theory of the homopolar bond where great difficulties were encountered. Nevertheless, in the last decades important advances have been made, but the enormous mathematical difficulties encountered have resulted in the strict theory being applied only to the simplest examples of chemical combination. The theory of the ionic bond has no difficulties of a mathematical kind and in consequence can be used for more complicated compounds. In the following pages this theory will be treated first, and later a very elementary, schematic presentation of the theory of the homopolar bond will be given. 

Carbon tetrachloride was cited earlier as an example of a homopolar compound here, however, it is treated as a heteropolar compound to see how far the theory of the heteropolar bond can be applied. Only when difficulties are encountered need we look for another explanation. 

A homopolar bond is non-polar where as a heteropolar bond is polar. The polar nature is described as polarity of the bond. 

This definition of the homopolar bond dissociation enthalpy has to be distinguished from its heteropolar counterpart, the dissociation of a bond into ions 1). An example of a particularly low heteropolar bond dissociation enthalpy for a C—C bond was recently discovered by Arnett6). 

A.2.2 Nonpolar Binary Intermetallic Phases. Zintl phases are characterized by the presence of markedly heteropolar bonding between the Zintl ions (electronegative polyatomic clusters) and the more electropositive metal atoms. By contrast, the bonding between heteronuclear atoms within other intermetallic compounds is primarily covalent or metallic. A number of different structure types exist for any given... 

The Schomaker-Stevenson relationship states that heteropolar bonds are always stronger and shorter than hypothetical, purely covalent bonds between the same atoms. In an ionic crystal, would you expect some covalency to shorten or lengthen the bond Explain. (Shannon, R. D. Vincent, H. Sirtict. Bonding (Berlin) 1974. 19, I.)... 

Magnasco, V. (2003) A model for the heteropolar bond. Chem. Phys. Lett., 380,397-403. 

The total core field U(x,y,z) of a molecular system [14) containing a central ion forming essentially heteropolar bonds to the surrounding ligands can be written [Ref. [8) p. 370] as... 

Hess law, 30, 85, J46 heteropolar bond, 23 heteropolymetallate, 223 high-spin complex, 213 HOMO, 75, 90 homopolar bond, 23 H ckel theory, 82 Hund s first rule, KL, 11, 70 hybridization, 73, 77 hydrazine, 162 hydride, 26,129,150 hydroformylation, 268 hydrogen bond, 79, 91, 151 hydrogen electrode, 140, 143 hydrogen peroxide, 171, 266 hydrogenation, 268 hydrothermal reaction, 41, 114, 257 hydroxide, 130,132,138,119,110 hypervalence, see octet expansion... 

Figure 2 gives the variation of the function along the line of two neighboring nuclei in several molecules. This figure clearly shows that for the homopolar bonds (the central bond of naphthalene, the hydrogen molecule, the lithium molecule) the result of the chemical bond is an increase of electrons between" the nuclei, while for the heteropolar bond (LiH) there is a transfer of charge from one atom towards the others. 

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