* Barium's Electron Configuration: Barium is in group 2 of the periodic table, meaning it has two valence electrons (electrons in its outermost shell). Its electron configuration is [Xe] 6s².
* Losing Electrons: To achieve a stable octet (eight electrons in its outermost shell), barium readily loses its two valence electrons. This results in a positively charged ion with a +2 charge.
* Lewis Structure: The Lewis structure for Ba²⁺ simply represents the barium atom with a +2 charge, indicating the loss of two electrons. There are no dots around the symbol because it has no valence electrons left.
In summary: When a barium atom forms an ion, it loses two electrons to become a cation with a +2 charge. This process is driven by the desire to achieve a stable electron configuration.
