In benzene, why is neither of the two given resonance structures considered to be the correct representation of the actual molecule?

(N/A) Experimentally, benzene has uniform $C-C$ bond distances of $139 \ pm$, which is an intermediate value between the $C-C$ single bond $(154 \ pm)$ and the $C=C$ double bond $(134 \ pm)$. Therefore, the actual structure of benzene does not contain pure single or double bonds, but rather a resonance hybrid of the two structures.