View Single Post
Jun19-09, 08:37 PM
P: 5
Hi, first time poster.

Quick question:

Why is the bond energy for a bond that contains a more highly substituted (tertiary) carbon weaker than the bond energy of a bond that contains a less substituted (primary) carbon?

Let me clarify with an example. Say Bond A is a single bond between a methyl carbon and a carbon that has a double bond. Another bond (Bond B) also has a single bond but between a tertiary carbon and another carbon that has a double bond. So, both share an sp2-hybridized and an sp3-hybridized carbon. Now, I know that Bond B has a weaker bond energy because it contains the more highly substituted carbon, but I don't know why that is the case. I figured that the carbons pull some of the electron density away from Bond B, therefore, lengthening the bond and decreasing the bond energy. Is that correct?

Much thanks!

Edit: Hmmm. Now that I think about it, I don't know if this question should be posted on this board. Sorry about that.
Phys.Org News Partner Physics news on
New complex oxides could advance memory devices
'Squid skin' metamaterials project yields vivid color display
Scientists control surface tension to manipulate liquid metals (w/ Video)