What is the Lewis structure for a perchlorate ion?

Question

Wyatt Adkins · Accepted Answer

For #"perchlorate anion, "ClO_4^-#, there are #7+4xx6+1=32" valence electrons"# to distribute.

Thus, there are 16 electron pairs that need to be split among 5 centers. #""^(-)O-Cl(=O)_3# You must fill in the lone pairs. Clearly, the negatuve charge is localized on oxygen in this representation, but all the oxygen atoms are formally equivalent.

Avery Adams · Answer

undefined Oxygen with a double bond to chlorine, three single bonds to other oxygen atoms.

Wyatt Adkins · Answer

undefined The Lewis structure for a perchlorate ion (ClO4-) consists of a central chlorine atom bonded to four oxygen atoms. The chlorine atom forms single bonds with each of the oxygen atoms, and each oxygen atom is surrounded by three lone pairs of electrons. The formal charge on the chlorine atom is +1, while each oxygen atom carries a formal charge of -1. This Lewis structure satisfies the octet rule for all atoms, and it represents the most stable arrangement of electrons for the perchlorate ion.