![]() ![]() Hybridization Hybridization is the idea that atomic orbitals fuse to form newly hybridized orbitals, which in turn, influences molecular geometry and bonding properties.Delocalization of Electrons To introduce the concept of electron delocalization from the perspective of molecular orbitals, to understand the relationship between electron delocalization and resonance, and to learn the principles of electron movement used in writing resonance structures in Lewis notation, known as the curved arrow formalism.This has been established in both MO and VB theory. In all three cases, there is a small and roughly identical participation of d-orbitals in the wavefunctions. The consensus is now clear that d orbitals are NOT involved in bonding in molecules like SF₆ any more than they are in SF₄ and SF₂. d-orbital Hybridization is a Useful Falsehood For main group molecules, chemists (like Pauling) thought a long time ago that hypervalence is due to expanded s²p⁶ octets.This electron density at the minimum distance between the two atoms is where the lowest potential energy is acquired, and it can be considered to be what holds the two atoms together in a chemical bond. This attraction increases as the atoms approach one another until the atoms reach a minimum distance where the electron density begins to cause repulsion between the two atoms. The theory assumes that electrons occupy atomic orbitals of individual atoms within a molecule, and that the electrons of one atom are attracted to the nucleus of another atom. Valence Bond theory describes covalent bond formation as well as the electronic structure of molecules. MO theory has been more correct in numerous instances and for this reason it is preferred. MO theory actually predicts electron transitions because of the differences in the energy levels of orbitals in the molecule. It is more difficult to learn, but predicts the actual properties of molecules better than VB theory. While Molecular Orbital (MO) theory is good for understanding bonding in general. ![]() VB theory does a good job of qualitatively describing the shapes of covalent compounds. In molecular oxygen VB theory predict that there are no unpaired electrons. This is actually an invalid assumption because many atoms bond using delocalized electrons. Valence bond (VB) theory assumes that all bonds are localized bonds formed between two atoms by the donation of an electron from each atom.
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