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Hybridization of Atomic Orbitals

The predecessors. Lewis StructuresShow the arrangement of valence electronsVSEPR TheoryPredicts the molecular geometry of a molecule or ionHybridizationIs the third piece of a puzzle known as the localized electron model. Hybridization. Uses modifications of molecular models to account for obs

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Hybridization of Atomic Orbitals

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    1. Hybridization of Atomic Orbitals Put on your 3-D glasses!

    2. The predecessors Lewis Structures Show the arrangement of valence electrons VSEPR Theory Predicts the molecular geometry of a molecule or ion Hybridization Is the third piece of a puzzle known as the localized electron model

    3. Hybridization Uses modifications of molecular models to account for observed structures of molecules or ions Is a mixing of the native atomic orbitals to form special hybrid orbitals for bonding The special orbitals will then strive to be as far away from each other in space as they can be

    4. Types of Hybridization sp3 sp2 sp dsp3 d2sp3

    5. Types of Bonds Sigma (s) bonds End-to-end bonding There is an overlap One in every type of bond Pi (p) bonds Side-to-side bonding There is no overlap 1 in a double bond 2 in a triple bond

    11. Hybrid sp3 orbitals Draw the Lewis dot structure for methane, CH4

    18. Hybrid sp2 orbitals Draw the Lewis dot structure for ethene, C2H4

    25. Hybrid sp orbitals Draw the Lewis dot structure for ethyne, C2H2

    30. In a Nutshell

    31. Practice Draw the Lewis structure and state the bond angle(s) and shape of the molecule or ion, and hybridization of the requested atom. CO2(Cs hybridization) NH3....(Ns hybridization) AsF5(Ass hybridization) BCl3(Bs hybridization)

    32. Practice 5. XeF4....(Xes hybridization) 6. H2O(Os hybridization) 7. SiCl4(Sis hybridization) 8. N2H2....(either Ns hybridization) 9. SO32-(Ss hybridization)

    33. Practice The Lewis structure for ascorbic acid (Vitamin C) is below: CH2OH HOCH O HC C=O C C HO OH

    34. Practice 10. Illustrate all of the bonds and lone pairs in the molecule and determine: a. the hybridization of each carbon b. the total number of sigma bonds c. the total number of pi bonds d. the bond angle of an O to a C to an O e. the bond angle of an H to an O to a C

    35. Double Bonds have 1 sigma and one pi Triple Bonds have 1 sigma and two pi

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