Final answer:
In the Lewis structure of O₂, the right oxygen atom has two bonding pairs, forming a double bond with the other oxygen, and two lone pairs, completing its octet for a stable configuration.
Step-by-step explanation:
The right oxygen atom in the Lewis structure of the O₂ molecule has two bonding pairs and two lone pairs. A bonding pair is a pair of electrons that are shared between two atoms to form a covalent bond, represented by a line between the atoms. In the case of O₂, the bonding pairs are shared between the two oxygen atoms, forming a double bond (represented as O=O). Each oxygen atom also has two lone pairs, which are pairs of valence electrons that are not shared with another atom and instead remain on the oxygen atom.
Thus, around the right oxygen atom in the O₂ molecule, there are two bonding pairs of electrons due to the double bond and two lone pairs of electrons that are not shared. The oxygen atom completes its octet with this arrangement of electron pairs, which is a stable configuration.