What's the Lewis dot structure of O3-?

Question

What's the Lewis dot structure of O3-?

Answer 1

http://en.wikipedia.org/wiki/Ozone#



u can refer this site for structure .but the general lewis structure is not applicable for ozone as it is a resonance hybrid of two structures

Answer 2

Start by counting up all of the electrons.  It's a little hard to tell if you mean O3^- or O^3-.  Is it ozone with with a negative charge or an oxygen atom with a negative three charge?

I don't think either one will actually occur.  A single oxygen atom will not gain three electrons.  There is only room for two additional electrons in the 2p-sublelvel.  Adding two electrons will produce a filled energy level.  That's as many electrons as an oxygen atom will gain.  Three for an oxide ion is O^2-.

Ozone has a double bond and a single bond in the Lewis structure.  Actually it has two identical bonds, each with a bond order of 1.5 becuase of the delocalized pi bond formed from overlapping unhybridized p-orbitals on each of the oxygen atoms.

Adding another electron to get O3^- would produce an odd number of electrons and a free radical.  The Lewis structure would have single bonds between the oxygen atoms.  The terminal atoms would have octets of electrons, and the central atom would have one lone pair and a single electron.  This would not be a stable molecule.

Therefore, I reiterated that neither O3^- nor O^3- is likely to occur.