Lewis structure of o3 and assign the formal charges
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The formal charge of the ozone molecule is zero. Its Lewis structures do present charge separation.
Explanation:
With simple VSEPR considerations, there are 18 valence electrons to distribute around the 3 oxygen atoms (24 electrons in total; 6 are inner core).
Typically, a Lewis structure of O=..O+−O−, would be depicted. Going from left O to right Oand including the 2 inner core electrons on each atom, there are 8, 7, and 9 electrons around each oxygen centre, resulting in formal charges of 0, +1, and −1, respectively. Of course, I can draw the other resonance structure, but the Lewis structure has the same electronic formulation. The ∠O−O−O ≅117∘; this is slightly LESS than the normal sp2 bond angle of 120∘, due to disproportionate influence of the oxygen lone pair, which tends to compress ∠O−O−O.
Since the central oxygen has 3 regions of electron density, this molecule is bent.
The formal charge of the ozone molecule is zero. Its Lewis structures do present charge separation.
Explanation:
With simple VSEPR considerations, there are 18 valence electrons to distribute around the 3 oxygen atoms (24 electrons in total; 6 are inner core).
Typically, a Lewis structure of O=..O+−O−, would be depicted. Going from left O to right Oand including the 2 inner core electrons on each atom, there are 8, 7, and 9 electrons around each oxygen centre, resulting in formal charges of 0, +1, and −1, respectively. Of course, I can draw the other resonance structure, but the Lewis structure has the same electronic formulation. The ∠O−O−O ≅117∘; this is slightly LESS than the normal sp2 bond angle of 120∘, due to disproportionate influence of the oxygen lone pair, which tends to compress ∠O−O−O.
Since the central oxygen has 3 regions of electron density, this molecule is bent.
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