Lewis Acids and Bases?

[JustinHorriat_4f]

Can someone Explain what Lewis Acids and Bases are and why they are an exception to the often rule? Also, what different rxns are they involved in?

[IScarvie 1E]

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

[Brittany Tran 3I]

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

[Michelle Xie 2B]

A lewis base would donate a pair of electrons and a lewis acid would accept a pair of electrons.

[andrewcj 2C]

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.

[lauraxie2e]

an acid accepts a lone pair and a base gives one up

[Nuoya Jiang]

Lewis Acids are electron acceptors and Lewis Bases are electron donors.

[405335722]

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?

[Madeline Phan 1E]

Lewis acids accept pairs of electrons, while Lewis bases donate entire pairs so they form coordinate covalent bonds since the bases are donating an entire pair of electrons.

[Sartaj Bal 1J]

@405335722 the Bronsted-Lowry acid base model states that protons are either accepted or donated.

[Eunice Nguyen 4I]

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.

[MeeraBhagat]

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.