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

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(A) The bond order is calculated as: $	ext{Bond order} = \frac{	ext{Total number of bonds}}{	ext{Total number of resonating structures}}$.For $PO_4

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$-0.75, 1.25$

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(A) The bond order is calculated as: $	ext{Bond order} = \frac{	ext{Total number of bonds}}{	ext{Total number of resonating structures}}$.For $PO_4^{3-}$,there are $5$ bonds in the Lewis structure and $4$ equivalent resonance structures.$	ext{Bond order} = \frac{5}{4} = 1.25$.The total formal charge of $-3$ is distributed equally over $4$ oxygen atoms in the resonance hybrid.$	ext{Formal charge on each oxygen} = \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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