(Polar molecules, Non-polar molecules, etc.)
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I'm not exactly sure about radicals and shapes, but I know that for 2E.5 when they ask OClO they aren't asking about a molecule ClO2, they are just taking about the bond formed between those three atoms (O, Cl, and O). Hope that helps!
I believe question 2E.5 asks about the ClO2 cation, so in total it would have 18 valance electrons due to the positive charge and subtraction of one electron. This would cause the shape to be trigonal planar due to the lone pair on the central Cl atom.
Because it is ClO2+ ion there are 18 valence electrons because the + means to subtract 1 electron. Therefore draw the lewis structure with Cl as the central atom and O atoms connected by double bonds to Cl, then 2 sets of lone electron pairs on each O and 1 set of lone electron pair on the Cl. Then if you look at a VSEPR chart you will see that the shape is angular.
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