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Unformatted text preview: Acid: any species that can donate a proton (H+ ion)… proton donor Base: any species that can accept a proton (H+ ion)… proton acceptor Practice: Classify the following as acids or bases. CO 3 2-H 3 N CH 3 COOH NO 3-PH 3 BF 3 BF 3 cannot be defined using the Bronsted-Lowry theory – new definition needed Lewis Definition Acid: electron pair acceptor Base: electron pair donor Practice: Classify the following as acids or bases: Al 2 Cl 6 + 2Cl − 2AlCl 4 − AlF 3 + 3F − AlF 6 3− 2F − + SiF 4 SiF 6 2− Conclusions Acids and bases can be defined 3 ways: Arrhenius (middle school definitions) Acids – release H+ ions Bases – release OH- ions Bronsted-Lowry Acids – proton donors Bases – proton acceptors Lewis Acids – electron pair acceptors Bases – electron pair donors...
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This note was uploaded on 01/01/2012 for the course CHEM 101 taught by Professor Donahue during the Spring '11 term at Long Island U..
- Spring '11