What is the /_O-Cl-O in perchlorate anion, ClO_4^(-), and what is the "VSEPR" treatment of the anion?

1 Answer
Aug 9, 2017

$\text{Of perchlorate......?}$

Explanation:

$\text{Perchlorate anion}$ is a tetrahedron with $\angle O - C l - O = {109.5}^{\circ}$....

Using $\text{VESPER}$, we gets $7 + 4 \times 6 + 1 = 32 \cdot \text{electrons}$ to distribute around 5 centres.......and we gets.......

""^(-)O-Cl(=O)_3 as the Lewis structure.....and clearly the negative charge is distributed around ALL the oxygen atoms; around chlorine there are 7 electrons, hence this centre in neutral. Around the (formally) singly bound oxygen atoms there are 7 electrons (3xx"lone pairs + one electron from the "Cl-O" bond").