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(C) species can undergo disproportionation if the central atom exists in an intermediate oxidation state.$1$. $H_2O_2$: Oxygen is in $-1$ state (can g

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$6$

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(C) species can undergo disproportionation if the central atom exists in an intermediate oxidation state.$1$. $H_2O_2$: Oxygen is in $-1$ state (can go to $0$ and $-2$).$2$. $ClO_3^{-}$: Chlorine is in $+5$ state (can go to $+7$ and lower).$3$. $P_4$: Phosphorus is in $0$ state (can go to $-3$ and $+1, +3, +5$).$4$. $Cl_2$: Chlorine is in $0$ state (can go to $-1$ and $+1$).$5$. $Cu^{+}$: Copper is in $+1$ state (can go to $0$ and $+2$).$6$. $NO_2$: Nitrogen is in $+4$ state (can go to $+3$ and $+5$).$Ag$,$F_2$,and $K^{+}$ do not undergo disproportionation under standard conditions.Thus,the total number of species is $6$.

Total number of species from the following which can undergo disproportionation reaction . . . . . . .
$H_2O_2$,$ClO_3^{-}$,$P_4$,$Cl_2$,$Ag$,$Cu^{+}$,$F_2$,$NO_2$,$K^{+}$

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Total number of species from the following which can undergo disproportionation reaction . . . . . . .$H_2O_2$,$ClO_3^{-}$,$P_4$,$Cl_2$,$Ag$,$Cu^{+}$,$F_2$,$NO_2$,$K^{+}$