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A Lewis acid is a lone pair acceptor, and a Lewis pair is a lone pair donor. I believe they are similar to covalent bonds, except they typically form as separate molecules and join to fulfill their individual needs
Lewis acids and bases involve coordinate covalent bonds, in which two atoms share a pair of electrons but both of the electrons come from one atom. Lewis acids are electron pair acceptors and Lewis bases are electron pair donors
A friend gave me the mnemonic "Lewis has e" which reminds me that Lewis acids and bases focus on electron exchange. After this, I just think about H+, which is acidic, and how it can accept electrons. Therefore, Lewis acids are electron acceptors.
Michelle Xie 3A wrote:A lewis base would donate a pair of electrons and a lewis acid would accept a pair of electrons.
What is the acid/base name for the definition that says it donates/accepts protons? Is that a Bronsted acid/base?
Lewis acid is an electron pair acceptor, while Lewis base donates nonbonding electrons. The bond in which both electrons come from one of the atoms is called a coordinate covalent bond. You can find this information in 2C.3 in the textbook.
Lewis acids accept electron pairs and lewis bases donate that electron pair. The example that Dr. Lavelle used was with BF3 as a lewis acid and F- as a lewis base. Since Fluorine does not make double bonds, and since three fluorines bonded to a boron atom only gives boron 6 valence electrons, the only way for Boron to get an octet is to coordinate covalently bond with a lewis base, F- in this case, which provides both of the electrons needed to complete boron's octet.
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