(Polar molecules, Non-polar molecules, etc.)
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Resonance structures are when the location of double bonds or triple bonds can be drawn in different locations while still being the same molecule. An example would be (NO3)- can have its double bond on any of the oxygen. This is just for Lewis structures, though. In reality, the molecule will be a blend of all three resonance structures and will be called a resonance hybrid.
Another important thing to note is that resonance stabilizes molecules. Since the electrons are more delocalized, they occupy a greater volume and the energy of the molecule is lower, making it more stable. Also, like the previous poster mentioned, the resonance structures you draw would be potential variations of the same molecule, but the actual NO3- molecule would have 3 bonds with a bond order of 1.33.
Adrian Lim 1J wrote:Does anyone know if we're expected to list all the possible resonance structures wherever applicable on the midterm?
No. The question will be specific. Draw the most stable structure and give one resonance structure, etc.
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