The order of the oxidation state of the phosp | vedclass

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Question

(C) To find the oxidation state of $P$ in each species,let the oxidation state be $x$:$1$. In $H_3PO_4$: $3(+1) + x + 4(-2) = 0 \implies 3 + x - 8 = 0

Vedclass · Accepted Answer

$H_3PO_4 > H_4P_2O_6 > H_3PO_3 > H_3PO_2$

Vedclass · Answer

(C) To find the oxidation state of $P$ in each species,let the oxidation state be $x$:$1$. In $H_3PO_4$: $3(+1) + x + 4(-2) = 0 \implies 3 + x - 8 = 0 \implies x = +5$.$2$. In $H_4P_2O_6$: $4(+1) + 2x + 6(-2) = 0 \implies 4 + 2x - 12 = 0 \implies 2x = 8 \implies x = +4$.$3$. In $H_3PO_3$: $3(+1) + x + 3(-2) = 0 \implies 3 + x - 6 = 0 \implies x = +3$.$4$. In $H_3PO_2$: $3(+1) + x + 2(-2) = 0 \implies 3 + x - 4 = 0 \implies x = +1$.Comparing the oxidation states: $+5 (H_3PO_4) > +4 (H_4P_2O_6) > +3 (H_3PO_3) > +1 (H_3PO_2)$.

Column-$I$	Column-$II$
$A$. $\underline{N}H_4 Cl$	$P$. $+1$
$B$. $H\underline{N}O_3$	$Q$. $+5$
$C$. $\underline{N}_2 O$	$R$. $-3$
$D$. $\underline{N}H_2 OH$	$S$. $-1$

The order of the oxidation state of the phosphorus atom in $H_3PO_2$,$H_3PO_4$,$H_3PO_3$,and $H_4P_2O_6$ is:

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Column-$I$ Column-$II$
$A$. $\underline{N}H_4 Cl$ $P$. $+1$
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$C$. $\underline{N}_2 O$ $R$. $-3$
$D$. $\underline{N}H_2 OH$ $S$. $-1$

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