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

1 Answer
anor277
Aug 9, 2017

#"Of perchlorate......?"#

Explanation:

#"Perchlorate anion"# is a tetrahedron with #/_O-Cl-O=109.5^@#....

Using #"VESPER"#, we gets #7+4xx6+1=32*"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"#).

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