Consider the following Lewis structure in which each letter corresponds to an element from the first and second periods of the periodic table. To make the formal charges of all atoms are equal to zero, provide the identity of each element.

The possible structures for BCl₃ are shown below.

Based on the concept of formal charges, determine the Lewis structure that would be dominant for BCl₃.

Determine the formal charges of the highlighted elements for the following structure:

Why does the best Lewis structure of BeBr₂ contain two single Be–Br bonds instead of two double Be=Br bonds?

Shown below is the Lewis structure of bromate ion:

A. What is the formal charge on the bromine (Br) atom?

B. What is the formal charge of each of the oxygen (O) atoms labeled a, b, and c?

S is the terminal atom in SiS₂ but S is the central atom in SCl₂. Explain using formal charges.