1) Draw the Lewis Dot Structure for the following molecule with molecular formula C5H6N+
2) Which atom or atoms carry positive charge in the above molecule?
Notice that all carbons are the same here every carbon makes one single bond to a neighbor carbon, one double bond to the other neighbor carbon and a single bond to a hydrogen, and they have no unshared electrons. Therefore, they will all have the same formal charge. The same can be said for the nitrogen it is bonding identically in the two resonance structures the difference is which carbon it is double bonded to. So lets calculate the formal charge for the H, C, and N atoms:
FC(X) = #valence e- on atom X - # bond to atom X - # unshared e-on atom X
FC(H) = 1 1 0 = 0
FC(C) = 4 4 0 = 0
FC(N) = 5 4 0 = +1, so nitrogen carries the positive charge in this molecule.