Chapter 2 - -cannot jump electrons over both a bond and an...

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Sheet1 Page 1 Chapter 2 Polar Covalent Bonds 2.3 Formal Charges formal charge = # of valence electrons - # of covalent bonds - # of non-bonding electrons 2.4 Resonance/ 2.5 Rules for Resonance Forms 1. Individual resonance forms are imaginary- real form is the resonance hybrid 2. Resonance forms differ only in the placement of their pi or nonbonding electrons 3. Different resonance forms of a substance don't have to be equivalent (different locations of pi bonds) 4. Resonance forms obey normal rules of valency 5. The resonance hybrid is more stable than any individual resonance form -no change in connectivity -cannot change net charge -look for an "electron source" and "electron sink" (nucleophile and electrophile, respectively)
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Unformatted text preview: -cannot jump electrons over both a bond and an atom when drawing resonance structures 2.7 Acids and Bases: The Bronsted-Lowry Definition an acid donates a proton to give conjugate base a base accepts a proton to give conjugate acid 2.8 Acid and Base Strength a strong acid has a high Ka and a low pKa 2.9 Predicting Acid-Base Reactions through pKa values the product acid will be weaker and less reactive than the starting acid 2.11 Acids and Bases: the Lewis Definition Sheet1 Page 2 a lewis acid is a substance that accepts an electron pair (electrophile) a lewis base is a substance that donates an electron pair (nucleophile) involves complex formation Sheet1 Page 3 Acids and Bases Sheet1 Page 4...
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This note was uploaded on 04/26/2009 for the course CHEM 227 taught by Professor Santander during the Fall '08 term at Texas A&M.

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Chapter 2 - -cannot jump electrons over both a bond and an...

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