A1 - CHM 2120 Assignment #1 In this assignment: - Lewis...

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CHM 2120 – Assignment #1 In this assignment: - Lewis structures, formal charge - Electronegativity, dipoles - Resonance - Acid/base 1. Draw the following molecules as full Lewis structures. Many molecules below possess a charge that is not shown—calculate the formal charge on each atom and indicate the location of the charge where applicable. Hint: each atom has a full octet, so start by adding electrons to each atom to complete its octet. The only atoms we will encounter in this course that lack an octet are carbon (a carbocation lacks an octet) and metals (B, Al, Mg, Li, etc). SH 2 example: C C C C C S H H H H H H H H H H H H H Formal charge (FC) = # valence electrons in neutral atom - # bonds - # lone electrons For the carbons: FC = 4 - 4 - 0 = 0 (the carbons are all neutral in this molecule) For the sulfur: FC = 6 - 3 - 2 = +1 (so a "+" is placed beside the S) O O H PhO O O H OH 2 Ph O Et NH Me N Me H C a) b) c) d) e) f) g) h) i) j) k) O- t -Bu O N H Note: the central carbon does not possess lone pairs.
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This note was uploaded on 06/24/2010 for the course CHM 2131 taught by Professor Johnmayer during the Spring '10 term at U. Memphis.

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A1 - CHM 2120 Assignment #1 In this assignment: - Lewis...

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