pi bonds

[JTieu_1L]

how would you find the unhybridized orbitals using electron configuration? what would be the pi bonds for CH3CN?

[305572629]

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.

[Jenaye Brelland 2I]

There are no pi bonds in a single bond, one in a double and two in a triple.

[ShinwooKim_3E]

Pi bonds are only seen in double or triple bonds.

[Christine Ma 3L]

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.

[Joel Meza 3I]

There would be 2 pi bonds in CH3CN between the C atom and N atom because there would be a triple bond. All bonds contain one sigma bond while double and triple bonds have additional pi bonds.

[Gian Boco 2G]

Anything that is additional to the single bond would be the pi bond, so you would have to look at the lewis structure.