3 posts • Page 1 of 1
Could someone please explain the differences between Lewis acids and bases? I know that the acids don't fill an octet and bases do or have a lone pair of electrons in the center, but what exactly does that mean? Thanks!
Similar to how regular acids and bases are electron recipients and donors respectively, Lewis acids are molecules that do not have a full valence shell like H+ that when bonding receive a pair of electrons to fill it up whereas Lewis bases like NH3 have an extra pair of electrons to donate when forming a covalent bond. I hope this helps!!
Lewis acid is a species that accepts an electron pair while Lewis base is a species that donates an electron pair. The Lewis acid and base theory is in contrast with the Bronsted-Lowry Acid and Base theory, in which Bronsted-Lowry Acid (BLA) is the proton donor while Bronsted-Lowry Base (BLB) is the proton receptor.
Who is online
Users browsing this forum: No registered users and 3 guests