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In reviewing for the final I'm trying to figure out easy ways to remember concepts. So can somebody correct me on whether or not the following concept is correct? When identifying Lewis acids and bases, are the acids typically the molecules without lone pairs on the central atoms while bases are molecules with lone pairs on the central atom, and if not can you give an example of why this concept doesn't work. Also if this concept isn't correct, what is another way to distinguish between Lewis acids and bases when given a molecule? Thanks.
From what I understand, this is correct. Lewis bases have lone pairs that they are able to donate to a bond, while the acids have room to accept that electron pair. I found this online: "A Lewis acid is a chemical species that contains an empty orbital which is capable of accepting an electron pair from a Lewis base. A Lewis base, then, is any species that has a filled orbital containing an electron pair which is not involved in bonding but may form a bond with a Lewis acid."
Ashley P 4I wrote:You two are life savers, thank you for simplifying this. Lone Pairs= Base No lone pairs= Acid
Are there any exceptions for this or is it pretty reliable as a quick way to determine whether it is a base or acid?
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