04-09-10 - 2 d • In triple bonds, as in acetylene, 2 sp...

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04-09-10 Hybrid Orbitals What is the hybridization of the central atom in the following compounds o I 3 - (22e-) 5sp 3 d orbitals (3 lone pairs and 2 paired with I atoms) 5sp 3 d orbitals and 4 d orbitals (1 given to the sp 3 d orbital) o SF 4 (5 sp 3 d orbitals)- 1 lone pair and 4 bonded with F atoms o SF 6 (6sp 3 d 2 orbitals)- no lone pairs 6 bonded with F atoms Sigma bonds are characterized by o Head to head overlap o Cylindrical symmetry of electron density about the inter-nuclear axis Pi bonds o Side to side overlap o E- density above and below the inter-nuclear axis In a molecule like formaldehyde an sp 2 orbital on carbon overlaps in sigma fashion with the corresponding orbital on the oxygen o Only way you can have a pi bond is if you have a p-orbital that is un- hybridized like sp
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Unformatted text preview: 2 d • In triple bonds, as in acetylene, 2 sp orbitals from a sigma bond between the carbons, and 2 pairs of p orbitals overlap in pi fashion to form the two pi bonds o Sp-2 pi bonds o Sp 2-1pi bond o Sp 3-0 pi bonds • In reality each of the 4 atoms in the Nitrate ion has a p-orbital • The p orbitals on all 3 oxygens overlap with the p orbital on the central nitrogen • The organic molecule benzene has 6 sigma bonds and a p orbital on each carbon atom • The reality the pi electron in benzene are not localized, but delocalized • Cis- isomer because the chlorines are on the same side of the double bond • Trans-isomer because the chlorines are on opposite sides of the double bond...
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This note was uploaded on 08/10/2010 for the course CHEM 1211 taught by Professor B during the Spring '10 term at Texas A&M.

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04-09-10 - 2 d • In triple bonds, as in acetylene, 2 sp...

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