Organic+Chemistry

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 * __The Structure of Benzene__**

The structure of benzene that we recognize with six hexagonal C that form a ring was first proposed by Kekule to explain how the molecular formula C6H6 was possible. This structure accurately satisfies carbon's need for four bonds yet it fails to explain why the double bonds do not undergo additional reactions. For example it would be expected that a carbon double bond would react with bromine but this only happens in bright light or a catalyst. When the reaction occurs it isn't an additional reaction. The reason the bonds are so special is because all the carbons are joined by a one and a half bond. This means that all of these bonds are the same length and have the same number of electrons and that is why there aren't additional reactions. The resonance of the structure is also different and adds to the structure's stability. Benzene uses about a third of the energy used in making a typical covalent bond. These are some reasons why benzene will only undergo substitution, where one or more of the hydrogen atoms are replaced during a reaction.

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The bonds between carbon atoms in a benzene molecule are neither single bonds, nor double bonds, but act as both at the same time. This is because the electrons in these bonds are not fixed in place but become delocalized. This allows them to move around the ring of benzene and not actually stay in one specific place, which is why the bonds between carbon atoms cannot be specified as either double or single bonds because all of them are indeed both double and single bonds at the same time.

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