so its depicted with 3 double bonds and 6 carbons, however it also has it where all the bonds are identical, how does this work?
In: Chemistry
Every carbon-carbon bond in benzene is exactly the same length, experimental data shows this.
The structure that you mention with alternating single and double bonds is actually one of two resonance structures, there is another one where the double bonds are where the single bonds are.
The actual structure is an average of both of these resonance structures, so the actual bonds are somewhere between single and double bonds, the bond length (1.4 Å) reflects this (C-C single bonds are ~1.54 Å, C=C double bonds are ~1.33 Å)
Benzene is an aromatic compound, as opposed to cyclohexane which is cycloalkane.
Benzene has three double bonds which means that 4 bonnded carbons have only one bond left for hydrogen. In cyclohexane, there are no double bonds so all carbons Are bonded to two hydrogens, giving you the formula (C6H12)
Benzene is a aromatic compound consisting of 3 double bonds and 3 single bonds. The actual structure is a hybrid of the two resonance structures where each double bond is adjacent to a single carbon-carbon bond. Benzene is strange in that it is theorized and accepted that each carbon atom in benzene has one hydrogen atom coming outwards from the carbon ring and the other is delocalized into a shareable “pool” of electrons within the ring. This is a driving factor in why benzene and aromatic compounds act so strangely.
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