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Why is the lewis structure of so 2 not similar to o 3? Both s and o atoms belong to group vi a of the periodic table which means they have 6 valence electrons each. In both so 2 and o 3 molecules, the central atom is bonded to two o atoms, so each molecule has a total of 18 valence electrons.
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So the above obtained lewis structure of so2 is not stable. We have to minimize these charges by shifting the electron pairs towards the sulfur atom. After shifting the electron pair from oxygen atom to sulfur atom, the lewis structure of so2 becomes more stable. Lewis structures are meant to be as efficient as possible but its moreso in my experience to keep count of the electrons and witness resonance structures.
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Theyre important and based on how the molecule is set up it can determine reactivity. Drawing the lewis structure for so2 is essential for understanding its molecular bonding and chemical properties. So2 is kinda weird. We have these things called resonance structures and it turns out so2 has three of them. We use what we call formal charges to deduce the best or most representative lewis structure and as it turns out it is the third one.
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