Draw a Lewis structure with lowest formal charges for${\text{MnO}}_4$

The given information is to draw the lewis structure.

A coordination complex consists of a central atom or ion, which is sometimes metallic and is named the coordination centre, and a surrounding array of bound molecules or ions, that are successively called ligands or complexing agents.

Octet rule - each atom needs to be surrounded with eight electrons.
The atom with lowest electronegativity goes to the middle of the Lewis structure. Then we've to count what number valence electrons are included within the compound. One charge - add one electron.

One electric charge - subtract one electron Each single bond - after we subtract that electrons from the overall number, we place remaining electrons around each atom in keeping with octet rule. Some elements have exception from octet rule, like nonmetals from period 3 and below, which can have expanded octets because their orbitals available.

H- one bond C - two bonds N - three bonds O - two bonds Halogens - one bond

Formal charge = (number of valence $e^{-}$) -(number of bonds) (number of lone pair$e^{-}$)

Step 2

We place Mn in the center of the structure (lowest EN) Total number of valence electrons is $32\left(7\right(Mn)+4)$times 0(O) (negative charge)) We have to put the brackets around to show that this is negatively charged ion.

$$\begin{gathered} F.C.forMn=7-7-0 \\ =0 \end{gathered}$$

$$\begin{gathered} F.C.forsingle-bondedO=0-1-0 \\ =-1F \end{gathered}$$

$$\begin{gathered} F.C.fordouble-bondedO=0-2-4 \\ =0 \end{gathered}$$