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Unformatted text preview: As atomic radius gets larger, bond length gets longer. a. C-F length is 135 pm b. C-Br length is 194 pm c. C-I length is 214 pm Factors affecting bond strength: 1. orbital overlap. Good overlap leads to stronger bonds. Cyclopropane has poor overlap so the bonds are weaker than in propane. 2. bond polarity. More polar bonds are usually stronger, greater skew in electronegativity leads to greater electronic attraction relevant to repulsion within the bond. 3. dependent on bond order and bond length. a. Shorter bonds are stronger, more pi character leads to stronger bonds 4. More s character leads to stronger bonds because it holds the electrons tighter to the nucleus. 5. strong adherence to the idealized bond angle leads to less strain, hence greater stability. Question 6. Draw an orbital diagram. C C N C C C N sugar H H...
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This note was uploaded on 04/07/2008 for the course PSY 101 taught by Professor Gauthier during the Spring '08 term at Vanderbilt.
- Spring '08