Self-Assessment on Hybridization Model

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

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
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
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: pi bond. That typically leads you to sp 2 hybridization. For a triple bond youll need a sigma and two pi bonds, so youll need two leftover p orbitals on each atom involved in order to generate two pi bonds. That typically leads you to sp hybridization. Now youre 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...
View Full Document

Page1 / 2

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

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online