(A) $Cu^{2+}$ is a strong oxidizing agent and $I^{-}$ is a strong reducing agent. $Cu^{2+}$ oxidizes $I^{-}$ to $I_2$ as follows: $2Cu^{2+} + 4I^{-}$

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$Cu^{2+}$ oxidises iodide to iodine

(A) $Cu^{2+}$ is a strong oxidizing agent and $I^{-}$ is a strong reducing agent. $Cu^{2+}$ oxidizes $I^{-}$ to $I_2$ as follows: $2Cu^{2+} + 4I^{-}$ $\longrightarrow 2CuI_2$ $\longrightarrow 2CuI + I_2$. Thus,$CuI_2$ is unstable and decomposes to form $CuI$ and $I_2$.

Class 12 Chemistry The d- and f-Block Elements Chemical properties

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All $Cu(II)$ halides are known,except the iodide. The reason for this is that:

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A
$Cu^{2+}$ oxidises iodide to iodine
B
$Cu^{2+}$ has much more negative hydration enthalpy
C
$Cu^{2+}$ ion has smaller size
D
iodide is a bulky ion

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The d- and f-Block Elements

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Chemical properties

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All $Cu(II)$ halides are known,except the iodide. The reason for this is that:

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Highest oxidation state of manganese in fluoride is $+4$ $(MnF_4)$ but highest oxidation state in oxides is $+7$ $(Mn_2O_7)$ because $..........$

The compound $AgF_2$ is an unstable compound. However,if formed,the compound acts as a very strong oxidizing agent. Why?

What is the general molecular formula of the products obtained on heating lanthanoids $(Ln)$ with sulphur?

$(a)$ Transition metals can act as catalysts because they can change their oxidation state. How does $Fe(III)$ catalyze the reaction between iodide and persulphate ions?$(b)$ Mention any three processes where transition metals act as catalysts.

How are transition metals and their oxides used in industrial processes?

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$(a)$ Transition metals can act as catalysts because they can change their oxidation state. How does $Fe(III)$ catalyze the reaction between iodide and persulphate ions?
$(b)$ Mention any three processes where transition metals act as catalysts.