Chemistry - CHEMICAL BONDING Question with Solution | TestHub

A neutral oxygen atom (O) belongs to Group 16 of the periodic table and contains 6 valence electrons. The oxide ion (O²⁻) carries a $-2$ charge, which means it has gained 2 extra electrons to achieve a stable octet.

Adding these electrons gives the O²⁻ ion a total of 8 valence electrons ($6+2=8$).

Therefore, its correct Lewis dot structure must show the symbol O surrounded by 8 dots/crosses enclosed in square brackets with a $2-$ charge.