Electrons in the \(σ^∗_s\) orbitals are located well away from the region between the two nuclei. Adding electrons to these orbitals creates a force that holds the two nuclei together, so we call these orbitals bonding orbitals. Electrons in a σ s orbital are attracted by both nuclei at the same time and are more stable (of lower energy) than they would be in the isolated atoms. The asterisk signifies that the orbital is an antibonding orbital. The out-of-phase addition (which can also be thought of as subtracting the wave functions) produces a higher energy \(σ^∗_s\) m olecular orbital (read as "sigma-s-star") molecular orbital in which there is a node between the nuclei. The mathematical process of combining atomic orbitals to generate molecular orbitals is called the linear combination of atomic orbitals (LCAO). The in-phase combination produces a lower energy σ s molecular orbital (read as "sigma-s") in which most of the electron density is directly between the nuclei. The two types are illustrated in Figure 8.4.3. There are two types of molecular orbitals that can form from the overlap of two atomic s orbitals on adjacent atoms. (b) When out-of-phase waves combine, destructive interference produces a wave with less (or no) amplitude. creates bonds from overlap of atomic orbitals ( s, p, d ) and hybrid orbitals ( sp, sp2, sp3 ) combines atomic orbitals to form molecular orbitals (,, , ) forms or bonds. considers electrons delocalized throughout the entire molecule. Atomic orbitals depict the location where the electron can probably be found in the atom where as molecular orbitals describe the probable location in a. \): (a) When in-phase waves combine, constructive interference produces a wave with greater amplitude. considers bonds as localized between one pair of atoms.
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