Assertion : PbI_4, BiCl_5, FeI_3, CuI_2 do no | vedclass

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(D) The assertion is true because $Pb^{4+}, Bi^{5+}, Fe^{3+},$ and $Cu^{2+}$ are strong oxidizing agents in the presence of iodide ions $(I^-)$. These

Vedclass · Accepted Answer

Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

Vedclass · Answer

(D) The assertion is true because $Pb^{4+}, Bi^{5+}, Fe^{3+},$ and $Cu^{2+}$ are strong oxidizing agents in the presence of iodide ions $(I^-)$. These metal ions oxidize $I^-$ to $I_2$ and get reduced to lower stable oxidation states (e.g.,$Pb^{2+}, Bi^{3+}, Fe^{2+}, Cu^+$). For example: $PbI_4 \rightarrow PbI_2 + I_2$. Thus,the higher oxidation state cannot exist in the presence of the strong reducing agent $I^-$. Therefore,both Assertion and Reason are true,and the Reason is the correct explanation of the Assertion.

Assertion : $PbI_4, BiCl_5, FeI_3, CuI_2$ do not exist. Reason : Higher oxidation states of metal ions are strong oxidising agents which give redox reactions with the iodide ion.

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