1009 - Summary of Hybrid Orbitals (Molecular Orbitals)...

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Section 6.5 Summary of Hybrid Orbitals (Molecular Orbitals) sp 2 trigonal planar sp linear tetrahedral
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Summary of Molecular Shapes 3 ATOMS LINEAR,  sp, 180 ° 4 ATOMS TRIGONAL PLANAR,  sp 2 , 120 ° PYRAMIDAL,  sp , 109 ° 5 ATOMS TETRAHEDRAL,  sp 3 , 109 °
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H C H C C H H C C H C H Section 6.3 LARGER MOLECULES O H C O H 3 things trigonal planar 120 ° sp 2 4 things bent ~109 ° sp 3 linear ~120 ° sp 3 things each trigonal planar
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A Word About Benzene H C H C C H H C C H C H H C H C C H H C C H C H Each C-C bond has a BO of 1.5 and an equal bond length! Watch for structures like this. Resonance Structures
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Section 6.4 BONDS IN MORE DETAIL 2 kinds of bonds Sigma ( σ ) - Pi ( π ) - bond with the electron density between  the nuclei. bond with the electron density  above and below  the internuclear axis. Sigma Pi
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Section 6.4 TO MAKE SIGMA BONDS Etc. ..  Electron density must be  between  the nuclei! sp 2 s sp s p p s s
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Section 6.4 TO MAKE PI BONDS top and bottom p y p y front and back p top and bottom d orbital Etc. ..  Electron density  not between  the nuclei!
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RECALL HYBRID ORBITALS s + 2p’s (1 p left over) s + 1p (2 p’s left over)  sp  makes  2 σ  bonds (or holds  lone pairs ) 2 p’s  make  π  bonds s + 3p’s
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This note was uploaded on 06/14/2009 for the course CH 101 taught by Professor Bigham during the Spring '08 term at N.C. State.

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1009 - Summary of Hybrid Orbitals (Molecular Orbitals)...

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