The group 14 elements A and B have the first | vedclass

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(C) In group $14$,the first ionisation enthalpy decreases down the group due to the increase in atomic size,but $Pb$ shows a higher value than $Sn$ du

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reducing and oxidising

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(C) In group $14$,the first ionisation enthalpy decreases down the group due to the increase in atomic size,but $Pb$ shows a higher value than $Sn$ due to the inert pair effect and poor shielding of $4f$ electrons. Given the values,$A$ corresponds to $Sn$ $(708 \ kJ \ mol^{-1})$ and $B$ corresponds to $Pb$ $(715 \ kJ \ mol^{-1})$. $Sn^{2+}$ acts as a reducing agent because it tends to get oxidised to $Sn^{4+}$,which is the more stable oxidation state for $Sn$. $Pb^{4+}$ acts as an oxidising agent because it tends to get reduced to $Pb^{2+}$,which is the more stable oxidation state for $Pb$ due to the inert pair effect. Therefore,$A^{2+}$ is reducing and $B^{4+}$ is oxidising.

The group $14$ elements $A$ and $B$ have the first ionisation enthalpy values of $708$ and $715 \ kJ \ mol^{-1}$ respectively. These values are the lowest among their group members. The nature of their ions $A^{2+}$ and $B^{4+}$ respectively is:

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