Chapter 10.4_10.5 student version

Chapter 10.4_10.5 student version - Valence Bond Theory and...

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Valence Bond Theory and Shape 10.4 If we only used the set of atomic orbitals to make bonds, then the shapes of molecules would be very limited. For example, the p-orbitals only point in the x, y and z directions. Based on the p-orbitals, one would expect only octahedral shapes with 90 degree angles. How is it possible to make a tetrahedral shape, with its strange angles?
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Valence Bond Theory and NH 3 N – 1s 2 2s 2 2p 3 3 H – 1s 1 Using the 3 2p orbitals predict 90º Actual H-N-H bond angle is 107.3º 10.4 Example : If the bonds form from overlap of 3 2p orbitals on nitrogen with the 1s orbital on each hydrogen atom, what would the molecular geometry of NH 3 be?
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Orbital Hybridization and Shape 10.4 Since electrons are waves, the electrons in orbitals can constructively and destructively interfere with one another. Since orbitals are the region of space that electrons move in, that means orbitals constructively and destructively interfere with one another. Using the wave properties of electrons, we can combine atomic orbitals to form hybrid orbitals.
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Formation of sp 3 Hybrid Orbitals this part added up this part cancelled + - + -
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Chapter 10.4_10.5 student version - Valence Bond Theory and...

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