That's a good way to visualize resonance, but it's not quite the full picture. While electron pairs do move rapidly between resonance structures, thinking of it as a "flipping" back and forth can be misleading.

Here's why:

* Resonance structures are theoretical: They are not real, individual structures that exist in a molecule. They are simply representations we use to depict the delocalization of electrons.

* The actual molecule is a hybrid: The true structure of a molecule exhibiting resonance is a blend of all the contributing resonance structures. It's not that the electrons are flipping between structures; they are spread out over the entire molecule, creating a more stable, delocalized electron cloud.

* Resonance stabilization: This delocalization of electrons is what makes resonance structures more stable than any single contributing structure. It's not just about the movement of electrons but the resulting distribution of electron density.

Analogy: Imagine a wave that is a combination of multiple smaller waves. We can represent the wave with individual sine curves, but the actual wave is a blend of these curves. Resonance is like that - the molecule is represented by multiple structures, but the actual structure is a hybrid of them all.

In summary, resonance structures are a tool for understanding the distribution of electrons in a molecule, not literal snapshots of its state. The electrons are not "flipping" but are delocalized over the entire molecule, resulting in increased stability.