Question

answer:

ideal bonding model would be the one to simplicity of the localized electrons model but with the delocalization characteristics of the molecular orbital model. This is achieved by combing the two models to describe molecules that require resonance. In case of Benzene and O3, the double bond that show charges in positions in the resonance structure. Since the double bond involves one ? and one? Bond, there is a ? bond between all bound atoms in each resonance structure. It is really the ?? bond that has difference locations in the various structure. Therefore, we can conclude that the ? bonds in the molecule can be describes as being localized with no apparent problems. It is the ? bonding the must be treated as being delocalized. Thus, for molecules that require resonance, use the localized electron model to describe the ? bonding and the molecular model to describe the ? bonding. This allows to keep the bonding model as simple as possible and give more physically accurate description of molecules.

In benzene, it consists of a plana hexagon of carbon atoms with on H atom bound to each carbon atoms. In this molecule all 6 C-C bonds are equivalent. The ? bonds of carbon involve 2p^2 orbitals. These ? bonds are all centers in the plane of the model. Since each carbon atoms is sp^2 hybridized, a p orbital perpendicular to the plane of the ring remains on each carbon atom. these 6 p orbitals can be used to form ? molecular orbitals. The electrons in the resulting? Molecular orbitals are delocalized above and below the plane of the ring. This give 6 equivalent C-C bonds.

please fill in ??

question:

What is delocalized π boding, and what does it explain? Explain the delocalized π bonding system in C6H6 (benzene) and O3 (ozone)

Answer 1

'?' replaced by bold, italic underlined words

ideal bonding model would be the one to simplicity of the localized electrons model but with the delocalization characteristics of the molecular orbital model. This is achieved by combing the two models to describe molecules that require resonance. In case of Benzene and O3, the double bond that show charges in positions in the resonance structure. Since the double bond involves one sigma and one pie Bond, there is a sigma bond between all bound atoms in each resonance structure. It is really the pie bond that has difference locations in the various structure. Therefore, we can conclude that the sigma bonds in the molecule can be described as being localized with no apparent problems. It is the pie bonding/electrons that must be treated as being delocalized. Thus, for molecules that require resonance, use the localized electron model to describe the sigma bonding and the molecular model to describe the pie bonding. This allows to keep the bonding model as simple as possible and give more physically accurate description of molecules.

In benzene, it consists of a plana hexagon of carbon atoms with one H atom bound to each carbon atom. In this molecule all 6 C-C bonds are equivalent. The sigma bonds of carbon involve 2p² orbitals. These sigma bonds are all centers in the plane of the model. Since each carbon atom is sp² hybridized, a p orbital perpendicular to the plane of the ring remains on each carbon atom. these 6 p orbitals can be used to form pie molecular orbitals. The electrons in the resulting pie Molecular orbitals are delocalized above and below the plane of the ring. This give 6 equivalent C-C bonds.