MCQ
In $PO_4^{3 - }$ ion, the formal charge on each oxygen atom and $P - O$ bond order respectively are
- ✓$-0.75,1.25$
- B$ - 0.75,1.0$
- C$ - 0.75,0.6$
- D$-3,1.25$
✓
Answer
Correct option: A.
$-0.75,1.25$
(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
$\frac{-3}{4}$ =$-0.75$.
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