CHEM266 Chapter Notes - Chapter 4: Lone Pair, Conjugate Acid, Lewis Acids And Bases
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1 Oct 2016
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Base attacking another molecule, presented in terms of base strength. Attacking molecule can either donate its e- to a hydrogen or act as a nucleophile and attack an electrophilic center. Lewis acid-base theory: any electron-deficient atom can accept electrons, not just protons. Most organic reactions are lewis acid-lewis base reactions. A solution is acidic if the proton is not bonded to the acid. Strength of acid is dependent on ability to donate a proton to another base. The stronger the acid, more shift to the right for equilibrium: larger the ka, smaller the pka. Equilibrium will shift to form the weaker acid-base pair, and will shift to form the stronger acid- hydrogen bond and the weaker base. Electronegativity: more electronegative, greater ability to stabilize a negative charge, when going across the periodic table, electronegativity is an important factor for determining conjugate base strength.
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