Consider the following reactions :(i) F_2 + 2 | vedclass

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(D) The reactivity of halogens as oxidizing agents decreases down the group: $F_2 > Cl_2 > Br_2 > I_2$.Reaction $(i)$: $F_2$ is a stronger oxidizing a

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$(i), (ii)$

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(D) The reactivity of halogens as oxidizing agents decreases down the group: $F_2 > Cl_2 > Br_2 > I_2$.Reaction $(i)$: $F_2$ is a stronger oxidizing agent than $Cl_2, Br_2,$ and $I_2$,so it can displace them from their halide ions. This reaction is correct.Reaction $(ii)$: $Cl_2$ is a stronger oxidizing agent than $Br_2$ and $I_2$,so it can displace them from their halide ions. This reaction is correct.Reaction $(iii)$: $I_2$ is a weaker oxidizing agent than $Br_2$,so it cannot displace $Br_2$ from $Br^-$. This reaction is incorrect.Therefore,only reactions $(i)$ and $(ii)$ are correct.

Consider the following reactions :
$(i)$ $F_2 + 2X^{-} \to 2F^{-} + X_2$ $(X = Cl, Br, I)$
$(ii)$ $Cl_2 + 2X^{-} \to 2Cl^{-} + X_2$ $(X = Br, I)$
$(iii)$ $I_2 + 2Br^{-} \to 2I^{-} + Br_2$
Which option has only the correct set of reactions?

Similar Questions

Which one of the following liberates oxygen immediately when passed into water?

$1$. $KClO_3 \xrightarrow{\Delta }$
$2$. $XeF_2 \xrightarrow{H_2O}$
$3$. $XeF_4 \xrightarrow{H_2O}$
$4$. $PbO_2 \xrightarrow{\Delta }$
$5$. $XeF_6 \xrightarrow{H_2O}$
In how many of the above processes,$O_2$ will be one of the products?

Which statement is not true?

The halogen that is most easily reduced is

Unlike other halogens,fluorine does not show higher oxidation states because:

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Consider the following reactions :$(i)$ $F_2 + 2X^{-} \to 2F^{-} + X_2$ $(X = Cl, Br, I)$$(ii)$ $Cl_2 + 2X^{-} \to 2Cl^{-} + X_2$ $(X = Br, I)$$(iii)$ $I_2 + 2Br^{-} \to 2I^{-} + Br_2$Which option has only the correct set of reactions?