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All sigma bonds are hybridized as sigma bonds are defined as single bonds between two atoms created by the hybridization of their orbitals. In order for a sigma bond to be formed, hybrid orbitals must be created. Pi bonds are not hybridized as they are composed of the overlap between two atoms' p orbitals, which are unhybridized orbitals.
I think a good example for this idea is ethane, C2H4, because both of the carbon atoms in the molecule are sp2 hybridized and they will each have one unpaired electron in the p orbital. So this parallel overlap of the p-orbitals will be unhybridized.
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