Chemistry 10 Wednesday, September 20, 2006

Chemistry 10 Wednesday, September 20, 2006 - Wednesday...

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Wednesday, September 20, 2006 Chemistry ACHIEVING NOBLE GAS CONFIGURATIONS Metal + Non-Metal = Ionic Compound Gives up e- Non-Metal + Non-Metal = Covalent Compound Must share e- SHARING How do you draw the pattern of bonding in a molecule? How do you judge the quality of the drawing? Text: Sections 5.4-5.8 (first part) LEWIS STRUCTURE 1. Show distribution of valence e- a. Not orbitals or E 2. We assume “octet rule” a. 8 valence e- around each atom b. 2 valence e- around H c. Technically, elements past F can have more than 8 i. Rule limited we use it anyway! 3. Diatomic and Bond orders (Shared pair) Bonding pair FIGURE 5.6 Cl + Cl = Cl Cl Lone Pairs Cl: 7 valence e- Single Bond = Bond Order =1 O = Double bond N = Triple bond
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Wednesday, September 20, 2006 DRAWING LEWIS STRUCTURES 1. # of shared pairs in a molecule a. (assuming octets) SP = ½ [ER – VE] # shared e- required valence e- Paris give all an actually Octet available Ex. 1 N 2 : SP = ½ [ER – VE] = ½ [16 -10] N
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This note was uploaded on 03/20/2008 for the course CH 101 taught by Professor Bigham during the Fall '08 term at N.C. State.

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Chemistry 10 Wednesday, September 20, 2006 - Wednesday...

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