CHEM 113 1nd Edition Lecture 24 Outline of Last Lecture- Acid Base Buffers- Common-ion effect- The Henderson-Hasselbalch EquationOutline of Current Lecture- The Lewis acid-base definitiono Lewis Acido Lewis BaseCurrent Lecture*Note: In class we went out of order when it comes to following the book. This section comes from the end of Chapter 18, not Chapter 19!- The Lewis acid-base definitiono A Lewis base is any species that donates and electron pair to form a bond A Lewis base must have a lone pair of electrons to donate Any substance that is a Bronsted-Lowry base is also a Lewis base Examples include H2O, OH, NH3o A Lewis acid is any species that accepts an electron pair to form a bond A Lewis acid must have a vacant orbital (or be able to rearrange its bonds to form one) to accept a lone pair and form a new bond This definition expands the definition so more substances can be called acids.- Therefore not all Bronsted-Lowry acids are Lewis acids Things to help you identify Lewis acids- B and Al are often form electron-deficient molecules, which have an unoccupied p orbital (meaning it has a spot for and electron), and therefore can accept a pair of electrons.- Molecules that contain a polar multiple bond often function as Lewis acidsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.- Metal cations also act as Lewis acids when it dissolves to form a hydrated ion Sample problem 18.15 utilizes these ideas in order to solve.o The Lewis definition views an acid-base reaction as the donation and acceptance pair to form a covalent
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