What is the geometry of the molecule ozone according to its Lewis structure?

The geometry of the ozone molecule (O3) is classified as bent due to its Lewis structure, which reveals an arrangement of the atoms and lone pairs of electrons. In ozone, the central oxygen atom is bonded to two outer oxygen atoms. The central atom has a single bond to one of the outer oxygens and a double bond to the other, creating a resonance structure.

This arrangement leads to a situation where there are lone pairs of electrons on the central oxygen atom. According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, the presence of these lone pairs influences the molecular geometry by occupying space and repelling the bonded electron pairs. Predominantly, the molecule adopts a bent shape rather than a linear one, because the lone pairs push the bonded atoms closer together.

In summary, ozone's bent geometry arises from the arrangement of three electron domains around the central atom, considering both bonding pairs and lone pairs. This results in the molecule having an angle of approximately 117 degrees between the bonds, characteristic of a bent molecular geometry.