3: Chemical Bond
- Page ID
- 426416
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- 3.1: Lewis Structures
- hemical bond refers to the forces holding atoms together to form molecules and solids. This force is of an electric nature, and the attraction between electrons of one atom to the nucleus of another atom contributes to what is known as chemical bonds. Various theories regarding chemical bonds have been proposed over the past 300 years, during which our interpretation of the world has also changed.
- 3.2: Valence Bond Theory
- Valence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. When the orbitals overlap along an axis containing the nuclei, they form a σ bond. When they overlap in a fashion that creates a node along this axis, they form a π bond.
- 3.4: Molecular Orbital Theory
- The positions and energies of electrons in molecules can be described in terms of molecular orbitals. A particular spatial distribution of electrons in a molecule that is associated with a particular orbital energy.—a spatial distribution of electrons in a molecule that is associated with a particular orbital energy. As the name suggests, molecular orbitals are not localized on a single atom but extend over the entire molecule. Hence, the molecular orbital approach is a delocalized approach.
- 3.7: Photoelectron Spectroscopy
- A photoelecton spectrum can show the relative energies of occupied molecular orbitals by ionization. (i.e. ejection of an electron). A photoelectron spectrum can also be used to determine energy spacing between vibrational levels of a given electronic state. Each orbital energy band has a structure showing ionization to different vibrational levels.