how to find charge on hybrid resonate structure???
Answers
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.
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BOTH OF U?
The best way to find the charge of a resonance structure is by using the FORMAL CHARGE method!!!!!!!!!
now how to use it
The first thing u should know to use this method is its formula
its formula is GIVEN DOWN↓↓↓↓↓↓↓
FORMAL CHARGE = number of valence electrons (free atom) − no. of lone pair electrons − x number of bonding electrons
SOME EXAMPLES:
IN THE CASE OF O₃ (OZONE)
In the attached figure each oxygen is labelled as 1, 2 & 3. This is done so we can find the charge of each oxygen molecule
Suppose lets take oxygen numbered as 1
∴ formal charge of O₂ marked as 1 = 6 - 2 - x 6= +1
Now as u have requested for H₂SO₄
Here formal charge of H marked as 1 = 1 - 0 - x 2 = 0
Now formal charge of H marked as 5 = 1 - 0 - x 2 = 0
Now formal charge of O marked as 2 = 6 - 4 - x 4 = 0
Now formal charge of O marked as 4 = 6 - 4 - x 4 = 0
Now formal charge of O marked as 3 = 6 - 6 - x 2 = -1
Now formal charge of O marked as 6 = 6 - 6 - x 2 = -1
Now formal charge of S (i have not marked any number as its only one) =
6 - 0 - x 8 = +2
→←↓↑→←↓↑→←↓↑→←↓↑→←↓↑→←↓↑→←↓↑→←↓↑→←↓↑→←↓↑→←↓↑→←↓↑→←↓↑→←
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