On the structure of barium fluorodide
barium fluorodide ($BaF_ {2} $), we want to clarify its Lewis structure (Lewis Structure of $BaF_ {2} $), starting from its atomic properties. Barium ($Ba $) belongs to the second main group of the periodic table of elements, and its atom has two electrons in the outer layer, which are active and volatile, in order to stabilize the structure. In the seventh main group of fluorine ($F $), the outer layer has seven electrons, and it is extremely desirable to obtain one electron into an octet stable state.

In the system of barium fluorodide, the barium atom generously donates its two outer electrons. These two electrons are obtained by the two fluorine atoms. In this way, the barium atom forms a two-positively charged cation ($Ba ^ {2 + }$）， due to the loss of two electrons, and the two fluorine atoms each get one electron, and they all form a negatively charged anion ($F ^{-}$）。

From the Lewis Structure For $BaF_ {2} $), barium ions are represented by their symbol $Ba ^ {2 +} $, without outer valence electrons. Two fluorine ions are represented by $[: F :]^{-}$, and the octet electronic structure around the fluorine atom is shown by the octet. In the overall structure, the barium ion occupies the center, and the two fluoride ions are separated on both sides. They are closely connected by ionic bonds to form a stable barium fluoride diide structure. This structure is stable due to the electrostatic attractive force between anions and cations, and is electrically neutral. Each atom reaches a stable electronic configuration, thus forming the unique structural shape of this compound.