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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Capital on December 11, 2012, 06:51:16 PM

Title: Why does diatomic carbon have two pi bonds?
Post by: Capital on December 11, 2012, 06:51:16 PM
Using the molecular bond theory, the MO configuration for carbon is σ2s^2, σ*2s^2, pi2p^4

The bond order is then (4+2-2)/2 = 2. (double bond)

I thought when there is a double bond, there is always one sigma and one pi bond but why are both bonds in diatomic carbon pi?

I'm specifically wondering why the p orbitals would produce two pi bonds instead of a sigma and a pi bond. Why are the p orbitals sideways overlapped?