Question

Despite many attempts, the perbromate ion (BrO₄⁻)(BrO4−)was not prepared in the laboratory until about 1970. (Indeed, articles were published explaining theoretically why it could never be prepared!) Draw a Lewis structure for BrO₄⁻Br₄⁻−in which all atoms have the lowest formal charges.

Answer 1

The Lewis structure for the perbromate ion (BrO₄⁻) consists of a central bromine atom bonded to four oxygen atoms and it is shown below

Each oxygen atom forms a single bond with bromine, and each oxygen also carries two lone pairs. The formal charges are minimized by distributing the negative charge on the oxygen atoms. The central bromine atom carries a formal charge of +1.

So, this arrangement ensures that each oxygen has a formal charge of -1, optimizing the overall charge distribution. The Lewis structure reflects the stability of the perbromate ion, which, despite initial theoretical skepticism, was successfully prepared in laboratories around 1970.

See correct question below

Despite many attempts, the perbromate ion (BrO₄⁻) was not prepared in the laboratory until about 1970. (Indeed, articles were published explaining theoretically why it could never be prepared!) Draw a Lewis structure for (BrO₄⁻) in which all atoms have the lowest formal charges