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When comparing the relative strengths of an acid, we can look at the bond length connecting the anion with the H+. When doing so, the longer the bond means the acid is more likely to dissociate and release a proton. Therefore, longer bond lengths correspond with stronger acids. However, we discussed that those structures with resonance allows for a more delocalization of electrons making the anion more stable, which means the acid with more features of resonance is stronger. In Lyndon's review session, we discussed the property of induction. How does induction relate to the determination of relative strength of an acid?
The inductive effect is the ability to polarize a bond based on the electronegativity of an atom. So, if an atom has more electronegativity, there’s more induction, so the acid would be stronger. It’s pulling at the negative charge more to stabilize the anion.
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