The formal charge on the O atom and the P-O b | vedclass

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(A) In the $PO_4^{3-}$ ion,the central $P$ atom is bonded to four $O$ atoms. According to the Lewis structure,there are $5$ valence electrons of $P$ a

Vedclass · Accepted Answer

$-0.75, 1.25$

Vedclass · Answer

(A) In the $PO_4^{3-}$ ion,the central $P$ atom is bonded to four $O$ atoms. According to the Lewis structure,there are $5$ valence electrons of $P$ and $6$ valence electrons of each $O$ atom,plus $3$ extra electrons for the charge,totaling $32$ electrons. The structure consists of one $P=O$ double bond and three $P-O$ single bonds. However,due to resonance,the charge is delocalized over all four $O$ atoms. The formal charge on each $O$ atom is calculated as $\frac{	ext{Total charge}}{	ext{Number of } O 	ext{ atoms}} = \frac{-3}{4} = -0.75$. The bond order is calculated as $\frac{	ext{Total number of bonds}}{	ext{Number of resonating positions}} = \frac{1 	ext{ (double)} + 3 	ext{ (single)}}{4} = \frac{5}{4} = 1.25$.

The formal charge on the $O$ atom and the $P-O$ bond order in the $PO_4^{3-}$ ion are,respectively,.......

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