How can the C–C bonds in benzene be neither single nor double bonds?
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The C-C bonds in benzene can be neither single nor double bonds due to the concept of resonance. Resonance refers to the delocalization of electrons within a molecule, resulting in the distribution of electron density over multiple atoms or bonds. In the case of benzene, the six carbon atoms are bound to each other in a hexagonal ring, with alternating single and double bonds. However, the actual electron structure of benzene involves the delocalization of electrons over all six carbon atoms, creating a system of three equivalent bonds with intermediate bond lengths. This delocalization of electrons gives benzene its unique stability and aromaticity.
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Open access•Posted Content | The paper proposes a new theoretical model of the chemical bond based on the Heisenberg uncertainty principle. It suggests that the C-C bonds in benzene can be represented by a three-electron bond, which explains the aromatic nature of benzene and the delocalization of electrons. |
5 Citations | The provided paper does not discuss the nature of C-C bonds in benzene. It focuses on a photoinduced dehydrogenative homo-coupling reaction of alkylarenes to form strained C-C single bonds. |
| The provided paper does not discuss the nature of C-C bonds in benzene. | |
| The provided paper does not directly address the question of how the C-C bonds in benzene can be neither single nor double bonds. |
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