Lecture11: The Shapes of Molecules, Electron Domain Theory, Secondary Bonding

author: Donald R. Sadoway, Center for Future Civic Media
recorded by: Massachusetts Institute of Technology, MIT
published: Feb. 10, 2009,   recorded: October 2004,   views: 1039
released under terms of: Creative Commons Attribution Non-Commercial Share Alike (CC-BY-NC-SA)

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"And to go beyond that really requires some intensive quantum mechanics. So, we're going to stay with s and p-block. And we saw that if we had two atomic s-orbitals, when they blended to form the molecular orbital, it took on this sort of the ellipsoidal shape.

We called that a sigma orbital. And, the characteristic of the sigma orbital is that you have continuous electron density from one nucleus to the other. We said no holidays; constant electronic density.

We could then combine an s orbital and a p orbital, as for example in the case of hydrogen fluoride. In the case of s plus p, will end up with an orbital that looks something like this. And, it is also termed a sigma orbital because, again, if you look from one nucleus to the other, there is continuous electron density, no holidays...."

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