Question

Which of the followings has the most stable $+2$ oxidation state ?

• A. $Sn$
• B. $Pb$
• C. $Fe$
• D. $Ag$

Answer 1

Answer: (B)

$Pb$

In the periodic table, inert pair effect increases down the group. So in group 14, the stability of smaller oxidation state of +2 goes on increasing down the group. This makes $P{b}^{2+}$ a stable oxidation state.

In $F{e}^{2+}\left(3d^6\right)$, the d-orbital is not completely filled.

$A{g}^{+}\left(4d^{10}\right)$ is the most stable oxidation state of silver due to fully filled d-subshell, removal of the second electron is very difficult.