Hybridization maximizes orbital overlap. Hybridization provides the electron densities with the maximum separation. Without hybridization, measured bond angles (ex. 109.5 of tetrahedral) would conflict with predicted 90 of p-orbitals of valence bond theory without hybridization.
The link below reviews the common shapes, briefly overviews hybridization then provides a 'flow chart' to help connect central attributes (atoms attached & lone pairs) to the type of hybridization. At the bottom of the page are some sample questions. If you construct the Lewis structure for each, you should be able to identify the hybridization type and then the bond angle.
http://misterguch.brinkster.net/VSEPR.html
Once the last hybridization lesson is given, for any molecule you should be able to:
- draw its Lewis structure
- draw a 3-D representation (include bond angle, shape name, polarity of bonds & overall dipole of molecule)
- use energy level diagrams to show required hybridization of central atom
- provide a labeled* orbital sketch of the bonding [*sp3/sp2/sp & pi/sigma bonds]
From today you were asked to complete energy level diagrams and orbital sketches for both CHCl3 and NF3 , plus the questions on page 235 (11-14)
[I am a little pressed for time this afternoon, so I am going to fall back on the old polar jokes. Ready? What's the difference between a polar bear and a panda? {Answer: About 2500 kilometers. another? Where do polar bears keep their money? In snow banks.][Still looking for the link to explain bond angle measuring. :<]
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