@Sammy1024
I'm pretty sure you are approaching this incorrectly.
In the both figures you are looking at the middle carbon. Look at what that carbon is bonded to and compare the electronegativities.
1) If the middle carbon is bonded to another carbon, the charge is 0.
2) If the middle carbon is bonded to something MORE electronegative (like an oxygen), the middle carbon get's a "+"
3) If the middle carbon is bonded to something LESS electronegative (like a hydrogen), the middle carbon gets a "-"
So looking at the left figure:
The middle carbon is bonded to 2 carbons (providing middle carbon with charge = 0), a hydrogen (
providing middle carbon with charge = -1), and an oxygen (
providing middle carbon with charge = +1)
Right figure:
The middle carbon is bonded to 2 carbons (providing middle carbon with charge = 0) and two oxygens (each providing middle carbon with +1 charge).
You can do the same analysis for the Oxygen in the left figure.
Oxygen is bonded to carbon (providing oxygen with a negative charge), and to a hydrogen (also providing oxygen with a negative charge). Both carbon and hydrogen provide oxygen with negative charges since O is more electronegative than both.