Chemistry 13 Wednesday, September 27, 2006

Chemistry 13 Wednesday, September 27, 2006 - Wednesday...

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Wednesday, September 27, 2006 Chemistry COMPOUND REVIEW Are all covalent bonds the same? What info can you get from a Lewis structure? How do you quantify compounds? Text: Sections 5.5-5.2, 5.9, 1.5 Appendix A.8- A.9 BOND LENGTHS AND ENERGIES (sec 1.5) 1. Bonding e- like “glue” that holds the atom together 2. single double triple Less Glue More Glue Weaker Bond Strong Bond Smaller Bond E Larger Bond E Longer Bond Shorter Bond Table 5.3 Bond Bond Energy Bond Length C C 347 1.54 C C 612 1.33 C C 820 1.22 E 0 Blue – Single Red – Double R 3. Fractional bond orders in-between single, double, triple
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Wednesday, September 27, 2006 BOND POLARITY 1. up to now = a. covalent bond/e- equally shared 2. ex. HCl δ+ δ- H Cl - Cl has bigger EN i. e- pair pulled towards Cl - δ+ = partial + charge (~ 0.2 +) i. “+ pole” - a polar molecule/ a dipole 3. Continuum of bonds Covalent/polar/ionic Atom: H Cl F Na EN: 2.1 3.0 4.0 .09 Difference in EN Type H - H 0 Covalent H - Cl 0.9 Polar Covalent H – F 1.9 More Polar Na – Cl 2.1 Ionic 4. reality: a continuum of “ ionic character” and “covalent character” Fig 5.4
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