The document discusses acid-base theories including Bronsted-Lowry acids and bases, Lewis acids and bases, and monoprotic and polyprotic acids. Under the Bronsted-Lowry definition, an acid is a proton donor and a base is a proton acceptor in a proton transfer reaction. A Lewis acid is an electron pair acceptor that forms a covalent bond, while a Lewis base is an electron pair donor. Monoprotic acids donate one proton, while polyprotic acids like sulfuric acid can donate multiple protons in successive reactions.

1. Acid-base theoriesSection 15 - 2

2. ObjectivesDefine and recognize Bronsted-Lowry acids and bases.Define a Lewis acid and a Lewis base.Name compounds that are acids under the Lewis definition but are not acids under the Bronsted-Lowry definitions

3. Bronsted-Lowry Acids and BasesExpansion of Arrhenius acid definitionBronsted-Lowry AcidMolecule or ion that is a proton donorHCl + NH3 NH4+ + Cl-H+ is a protonHCl donates H+ (proton) to NH3H Cl + H N H H N H + Cl H HBronsted-Lowry BaseMolecule or ion that is a proton acceptorNH3 accepts H+ (proton) from HClBronsted-Lowry acid-base reactionProtons are transferred from one reactant (the acid) to another (the base)+H_::::::::::::::::

4. Monoprotic and Polyprotic AcidsMonoproticAcid that only donates one protonHCl + H2O H3O++ Cl-PolyproticAcid that can donate more than one proton per molecule.H2SO4+ H2O H3O+ + HSO4-HSO4-+ H2O H3O+ + SO42-Diprotic and triproticObvious!

5. Lewis Acids and BasesLewis AcidAtom, ion, or molecule that accepts an electron pair to form a covalent bond.Broadest of 3 definitionsLewis BaseAn atom , ion, or molecule that donates an electron pair to form a covalent bond.Lewis acid-base reactionFormation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor:::::::::::::::::::::::::::::::HHFFF B + N H F B N H F H F H: