Currently I studying about the Lewis dot structure for different compounds and my textbook says that the Lewis structure for ozone may be drawn as(as shown in the image): And then it goes on to calculate the formal charges on different oxygen atoms in it(which are shown in figure with $+/-$ signs.) In justification of the structure it says:
Formal charges help in the selection of the lowest energy structure from a number of possible Lewis structures for a given species. Generally the lowest energy structure is the one with the smallest formal charges on the atoms. The formal charge is a factor based on a pure covalent view of bonding in which electron pairs are shared equally by neighbouring atoms.
Now, my question is why can't the structure be like this:
Clearly, if this isn't a possible structure then the flaw in my understanding arises because of not understanding the term 'smallest formal charge'(as I found out that the structure I gave has all oxygen atoms with zero formal charge ) Please suggest what does it mean by the smallest formal charge ? Also why energetically the structure isn't stable. (For now please exclude any discussion about resonance hybrid of the ozone)