(Polar molecules, Non-polar molecules, etc.)
5 posts • Page 1 of 1
You figure that out by drawing the Lewis structure. You should follow all the rules that we learned the past few weeks (most atoms must have complete octets, you want the lowest possible formal charge, etc)
You can tell if there are lone pairs based on how the structure is drawn. For part a there has to be lone pairs because of how the other bonds are at an angle which means they are being repelled by a lone pair. For part b there is no obvious repulsion but there can still be lone pairs if there was a pair on both sides of the central atom which would make still create a linear shape with the atoms.
Who is online
Users browsing this forum: No registered users and 1 guest