ch10 2_Part2 - GENERAL CHEMISTRY CHAPTER 10: PART II...

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GENERAL CHEMISTRY CHAPTER 10: PART II – CHEMICAL BONDING PAGE 6 OF 15 Hybrid orbitals are oriented 180 o from each other Linear shape Only one p-orbital hybridizes Two p-orbitals are unhybridized and are oriented at 90 o angles to the sp hybrids Bond Rotation Valence bond theory tells us about rotation around a double bond Rotation about a double bond is severely restricted Because of the parallel or sideways overlap of p-orbitals, the π bond must essentially break for rotation to occur Rotation about a single bond is relatively unrestricted sp Hybridization Atoms with two charge clouds hybridize by combining one atomic s orbital with one p orbitals = two sp hybrid orbitals
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GENERAL CHEMISTRY CHAPTER 10: PART II – CHEMICAL BONDING PAGE 7 OF 15 Each of the sp orbitals is half-filled The remaining 2 electrons occupy the 2 leftover p-orbitals Two sp hybridized C atoms approach each other with the sp orbitals aligned head-on for σ bonding The unhybridized p-orbitals on the carbons are aligned for π bonding Two p-orbitals are aligned in an up/down position Two p-orbitals are aligned in an in/out position Sharing of 6 electrons = triple bond There is 1 σ sp-sp bond There are 2 π bonds There are 2 σ sp-s bonds Example: Acetylene = H-C C-H The unhybridized electron configuration of H C hybridization = sp sp 3 d Hybridization Hybridization of one s-orbital, three p-orbitals, and one d-orbital =
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This note was uploaded on 01/21/2011 for the course PHYS 4A 60865 taught by Professor L. oldewurtel during the Fall '09 term at Irvine Valley College.

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ch10 2_Part2 - GENERAL CHEMISTRY CHAPTER 10: PART II...

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