Rationalise the given statements and give chemical reactions.
(i) Lead (II) chloride reacts with $C{{l}{2}}$ to give
$PbC{{l}{4}}$.
(ii) Lead (IV) chloride is highly unstable towards heat.
(111) Lead is known not to form an iodide, ${Pb I }_{ 4 }$.
(i) Due to inert pair effect, Pb is more stable in + 2 state than in + 4 oxidation state. Therefore, lead (II) chloride does not react with $C{{l}{2}}$ to give lead (IV) chloride.
(ii) Lead (IV) chloride on heating decomposes to give lead (II) chloride and Cl 2 because lead in + 2 oxidation state is more stable than in + 4 oxidation state.
$PbC{{l}{4}}$ ------------->
$PbC{{l}{2}}$ +
$C{{l}{2}}$
(iii) Due to strong oxidising power of ${{Pb}{4}}^{+}$ ion and reducing power of ${{I}^{-}}$ion,
${ PbI }{ 4 }$ does not exist.