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Sigma bonds are always the first bonds to form and are single bonds and the remaining bonds are pi bonds. In an example of N2, the 2 pi bonds will appear to surround the single sigma bond when the electron densities of the pi bonds combine.
Yes, every double bond has 1 sigma and 1 pi bond. The first bond is always sigma and then subsequently they are pi bonds. So single bonds have 1 sigma bond, double bonds have 1 sigma and 1 pi, and tripe bonds have 1 sigma and 2 pi bonds.
sigma bonds result from the formation of a molecular orbital by the head-to-head overlap of atomic orbitals, and pi bonds result by side-to-side overlap (with p orbitals). pi bonds can only happen when the head to head overlapping of orbitals has also already occurred. however, a sigma bond can happen without side-to-side overlap.
If every double bond is one sigma and one pie bond, why not simply denote double bonds as such since the beginning? Or is this statement not reversible, in which a sigma and pie bond together do not always make a double bond?
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