Why does benzene have bond length intermediary between a c-c single bond and a c=c double bond?

Benzene is an aromatic compound which is highly stable due to a process called RESONANCE i.e, delocalisation of electrons. Due to this effect, the bond length of the bonds b/w diff. carbon atoms is between a c-c single bond and a c=c double bond.

Why does benzene have bond length intermediary between a c-c single bond and a c=c double bond?c++ cli

Every answer here seems right, except stroha

Stroha, not to pick on her too much, is fundamentally wrong because if benzene consisted of 3 conjugated pi bonds, with no aromaticity, you'd expect to get an addition reaction when you added concentrated HCl to it. You'd get rearrangements, from the conjugation, but you'd still expect a product. The truth is that HCl won't react with benzene.

Why does benzene have bond length intermediary between a c-c single bond and a c=c double bond?dev c++

Kerkule dreamed of snakes with their neighbors tails in their mouths, and there you go...

Since benzene consists of a ring of six carbons having covalent bonds so as to form a hexagon shape, and each carbon has a valence of four (you can think of it as having four "arms" each of which needs to be holding on to something), the convention is to draw benzene with alternating single and double bonds to graphically illustrate that all bonds are satisfied.

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Why does benzene have bond length intermediary between a c-c single bond and a c=c double bond?

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