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There would be two pi bonds in CH3CN since there is a triple bond between the second carbon and the nitrogen atom in the lewis structure. You can find unhybridized orbitals from an electron configuration first by drawing the normal electron configuration, then combining (hybridizing) the highest energy levels of the valence electrons if they are at the same energy level and making an orbital based on how many regions of electron density are attached to the central atom (3 regions = sp2, 4 regions = sp3, etc.) then filling that orbital with one electron then moving up to the unhybridized orbital if necessary.
I think you would first need to draw out the Lewis structures. Unhybridized p-orbitals are used to form pi bonds. For a single pi bond, 2 unhybridized orbitals (1 from each atom) overlap side to side. CH3CN has 2 pi bonds both between the C and N, therefore the N has 2 unhybridized orbitals, as does the C it's connected to.
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