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Unformatted text preview: Question 1 a) The bond angle between H-C-H is 109.47 ⁰ b) H-C-H bond angle is 108.12 ⁰ H-C-C bond angle is 110.79 ⁰ The two bonds are different because the CH groups repel the other and force the Hydrogen atoms closer ₃ together making the H-C-H bond angle smaller and the H-C-C bond angle slightly larger. The H-C-H bonds are different in methane and ethane because the repelling force of CH group is larger ₃ than that of lone bonded Hydrogen. c) The Largest H-C-C-H bond angle in ethane is 180 followed by 60 and -60 . ⁰ ⁰ ⁰ d) Ethanol: 1.543 Å Ethylene: 1.315 Å Acetylene: 1.187 Å The bonds differ because of the hybridization. Ethanol has no double bonds and is therefore hybridization sp3 Ethylene has a double bond and is therefore sp2 and the triple bonded Acetylene is sp. P orbital’s take up more space and make bonds longer, the less p orbital’s the shorter the bond length and vice versa....
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This lab report was uploaded on 04/17/2008 for the course CHEM 221 taught by Professor Brandt during the Fall '07 term at Rose-Hulman.
- Fall '07