In PO_4^{3 - } ion, the formal charge on each | vedclass

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Question

(a) Bond order $ = \frac{{{\rm{Total number of bonds between atoms}}}}{{{\rm{Total number of resonating structure}}}}$

$ = \frac{5}{4} = 1.25$

I

Vedclass · Accepted Answer

$-0.75,1.25$

Vedclass · Answer

(a) Bond order $ = \frac{{{\rm{Total number of bonds between atoms}}}}{{{\rm{Total number of resonating structure}}}}$

$ = \frac{5}{4} = 1.25$

In a given resonance structure, the $O$ atom that forms double bond has formal charge of $O$ and the remaining $3O$ atoms have formal charge of $-1$ each.In the resonance hybrid, a total of $-3$ charge is distributed over $4$ O atoms. Thus the formal charge of each $O$ atom is

$\frac{-3}{4}$ =$-0.75$.

In $PO_4^{3 - }$ ion, the formal charge on each oxygen atom and $P - O$ bond order respectively are

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