![]() The strength of a covalent bond depends on the extent of overlap of the orbitals involved. The mutual attraction between this negatively charged electron pair and the two atoms’ positively charged nuclei contributes to the link between the two atoms that we define as a covalent bond. According to valence bond theory, a covalent bond results when two conditions are met: (1) an orbital on one atom overlaps an orbital on a second atom and (2) the single electrons in each orbital combine to form an electron pair. We say that orbitals on two different atoms overlap when a portion of one orbital and a portion of a second orbital occupy the same region of space. Valence bond theory describes a covalent bond as the overlap of singly-occupied atomic orbitals that yield a pair of electrons shared between the two bonded atoms. Furthermore, VSEPR does not provide an explanation of chemical bonding. The VSEPR model, however, does not accurately predict all molecular shapes or electron domain geometries. For example, the VSEPR model has gained widespread acceptance because of its simplicity and its ability to predict the three-dimensional molecular shapes of many molecules that are consistent with experimental data. For a theory to be accepted, it must explain experimental data and be able to predict behavior. | Key Concepts and Summary | Glossary | End of Section Exercises | Valence Bond TheoryĪs we know, a scientific theory is a strongly supported explanation for observed natural laws or large bodies of experimental data. | Valence Bond Theory | sp Hybridization | sp 2 Hybridization | sp 3 Hybridization | Assigning Hybrid Orbitals to Central Atoms | Apply valence bond theory to predict orbital hybridization in atoms.
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