Question

how to find charge on hybrid resonate structure???

Answer 1

hey mate here is your answer

Choose one of four oxygen of the molecule and see what bond links to sulfur. You will find three structures with single bond and three with double bond. Calculating mean bond order:

BO=3∗1+3∗26=96=1.5BO=3∗1+3∗26=96=1.5

Each oxygen is thus linked to the sulfur by single and half bond. All oxygen are equivalent and same result arises when another oxygen is marked. A way to represent this graphically in the resonance hybrid is using a solid line (single bond) along a dotted line (half bond).

Mean formal charge can be calculated by same way. Marking one oxygen, it has zero charge in three structures and -1 charge in three structure. Calculating mean formal charge of oxygen:

FC=3∗0+3∗(−1)6=−36=−0.5FC=3∗0+3∗(−1)6=−36=−0.5

Thus, each oxygen has -0.5 formal charge in resonance hybrid.

hope it will help you now

mark me brainliest