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Self-Assessment on Hybridization Model

Self-Assessment on Hybridization Model - pi bond That...

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Self-Assessment on Hybridization Model This assessment will help you determine if you can predict hybridization from Lewis dot structures. I recommend you try it only after you’ve done the homework for this model. In a nutshell here are some basics that will help you if you’re having trouble with those goals or if you have trouble with the examples below. Hint: First draw the Lewis dot structure carefully and determine the # of lone pairs and the # of bonding pairs. Now evaluate using the summary below: # of Hybrid Orbitals Needed Electron Group Geometry Hybridization 2 Linear sp 3 Trigonal Planar sp 2 4 Tetrahedral sp 3 5 Trigonal bipyramidal sp 3 d 6 Octahedral sp 3 d 2 Note: The actual molecular geometry will be different from the electron group geometry if there are lone pairs on the central atom. If you have multiple bonds, you’ll notice that for a double bond you need a sigma and a pi bond, so you’ll need a leftover “p” orbital on each atom involved in the

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Unformatted text preview: pi bond. That typically leads you to sp 2 hybridization. For a triple bond you’ll need a sigma and two pi bonds, so you’ll need two leftover “p” orbitals on each atom involved in order to generate two pi bonds. That typically leads you to sp hybridization. Now you’re ready to try these: 1. Give the hybridization for the C and the O in H 2 CO (formaldehyde). 2. Give the hybridization for the C and the N in HCN. 3. Give the hybridization for all three atoms in N 2 O. 4. Give the hybridization for the central atom in each of the following: a) BCl 3 b) BrF 3 c) XeF 4 d) TeF 4 5. Using these examples can you describe how the hybrid orbital model combined with Valence Bond Theory helps to explain the bonding, molecular geometries, etc. in these molecules? KEY: 1. sp 2 for both 2. sp for both 3. outer N and the O are sp 2 , inner N is sp 4. a) sp 2 b) sp 3 d c) sp 3 d 2 d) sp 3 d...
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