CHM227 - Review Exam #2

CHM227 - Review Exam #2 - KEY POINTS IN ACID-BASE REACTIONS...

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KEY POINTS IN ACID-BASE REACTIONS Bronsted-Lowrey - Acid = proton donor - Base = proton acceptor Lewis - Acid = electron acceptor - Base = electron donor Acidity Constant - pK a = -log(K a ) Equilibrium favors the formation of the weaker acid and the weaker base Strong Acid K a >1 Negative pK a Weak conjugate base Weak Acid K a <1 Positive pK a Strong conjugate base Acid Strengths - Smaller pK a (OR a larger K a ) is a stronger acid - Effect of atom bonded to the Hydrogen o As you move left to right acidity increases, due to electronegativity o As you move top to bottom acidity increases, due to poorer overlap and larger anions can better accommodate negative charge (polarizability) - Inductive Effect o It destabilizes the acid and stabilizes to conjugate base o Electron-Withdrawing Group = one that pulls more electron density away from its bond partner than does hydrogen –N + R 3 –O=N + –O - O –S–R O –C≡N O –C– OH O –C–R –OH
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CHM227 - Review Exam #2 - KEY POINTS IN ACID-BASE REACTIONS...

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