[Dazedandconfused]

I'm supposed to draw all of the resonance structures of the ClO3- ion. The ones I drew, I put a single bond between each O and the Cl, gave two of the O 3 lone pairs and one O 2 lone pairs, and the Cl 2 lone pairs. It makes sense to me, because if you subtract the 26 total valence electrons from the 32 total noble gas configuration electrons, you get 6 bonding electrons, which makes 3 single bonds. That gives me a trigonal bipyramidal shape. However, why is it that everywhere I look on the internet, Cl only has one lone pair, and at least one bond is a double?

Thanks!

[Dan]

and one O 2 lone pairs

The O with 2 lone pairs and a single bond (as you describe) only has 6 electrons in its outer shell. Perhaps this will help you correct your structure...

Also, you may find this helpful: http://www.youtube.com/watch?v=Bx5_ae6mA-A

[Dazedandconfused]

Ahh, I get it. The way I did it forms a much less stable molecule. Thanks a lot for your assistance!