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Valence Bond Theory:

Valence Bond Theory:. Basic Overlap of orbitals in H 2 , HF and F 2. Important points for orbital overlaps (valence bond):. 1. Orbitals overlap to form a bond. Theories of Bonding. 2. Two electrons fit in the overlapping space. Usually each atom supplies 1 electron.

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Valence Bond Theory:

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  1. Valence Bond Theory: Basic Overlap of orbitals in H2, HF and F2 Important points for orbital overlaps (valence bond): 1. Orbitals overlap to form a bond Theories of Bonding 2. Two electrons fit in the overlapping space. Usually each atom supplies 1 electron 3. Both electrons are simultaneously attracted to both nuclei, and are hence most likely to be found between the nuclei

  2. tetrahedral The Problem: p orbitals Simple orbital overlap doesn’t work as well when larger/multiple atoms are involved. For example, why is methane, CH4, tetrahedral? Theories of Bonding Traditional “p” orbitals do not make sense for the linear, trig planar, tetrahedral, trig bipyr, and octahedral shapes that we observe …

  3. Hybridization: Theories of Bonding

  4. Hybridization: Draw sp3 hybridized orbitals (tetrahedral) CCl4 is an example of sp3 hybridized orbitals Theories of Bonding

  5. Hybridization: Draw sp2 hybridized orbitals (trigonal planar) BF3 is an example of sp2 hybridized orbitals Theories of Bonding

  6. Hybridization: Linear Geometries: sp hybridized orbitals are formed Draw the sp hybrid orbitals BeCl2 is an example of sp hybridized orbitals Theories of Bonding

  7. Hybridization: Describe the bonding in ethane, C2H6 - What is the hydridization of any central atoms? - What orbitals overlap to produce the C – H bond? - What orbitals overlap to produce the C – C bond? - Type of bond? - Draw it!!! Theories of Bonding

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