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Molecules that undergo hybridization will still follow the rules we learned before about sigma and pi bonds. For a single bond (ex: C 2sp3 - H 1s in CH4), there would be a single bond between the atoms and thus a sigma bond between the atoms. For a double bond (ex: C double bond C in C2H4), there would be a pi bond present, as the there is a C sp2 - C sp2 sigma bond and a C sp - C sp pi bond between the unhybridized orbitals on each C.
Sigma and pi bonds are ways to describe bonds that form in molecules, and knowing where a sigma or a pi bond will be can help us predict orbital hybridization. A single bond is a sigma bond, a double bond is a pi-bond and a sigma bond, and a triple bond is a sigma bond plus two pi bonds. This hybridization also closely relates with VSEPR structures so it is important to know the relation between the two (ex. the C atom in HCOOH is bonded to three atoms in a trigonal planar arrangement, making it sp2 hybridized).
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