1. why is lower energy resonance form is more stable than the higher? 2. An aver

Question

1. why is lower energy resonance form is more stable than the higher?

2. An average S–O single bond length is 1.59 Å, and the S=O double bond length is 1.42 Å. For sulfur (third row of the periodic table), how much do the resonance structures which obey the octet rule, but which have charge separation, contribute to the resonance hybrid?

3. Suggest a reason that a single resonance form dominates the hybrid even more than in the case of protonated formaldehyde.

4. There is a conclusion we can draw about the nature of resonance forms A and B of protonated formaldehyde, as calculated using molecular orbital theory. Since the calculated values are identical, they must represent the same species. This species is called a (two words):

Explanation / Answer

1. At high energies electrons will be in excited state and the resonance structure will be less stable. Generally low energies are more stable.

2. While writing resonance structures, it is important to follow that number of electrons remains the same in all structures, and shift of pi and lone pair electrons takes place. This can be done even with charges separation, only their contribution varies based on less/more charge separation.

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