Given: $E^{\circ }\left({\mathrm{Sn}}^{2+},{\mathrm{Sn}}^{4+}\mid \mathrm{Pt}\right)=0.15\mathrm{V},E^{\circ }\left({\mathrm{Hg}}_2^{2+},{\mathrm{Hg}}^{2+}\mid \mathrm{Pt}\right)=0.92\mathrm{V}$ and $E^{\circ }\left({\mathrm{Pb}}^{2+},{\mathrm{H}}^{+}\mid {\mathrm{PbO}}_2\right)=1.45\mathrm{V}$Based on this data, which of the following is correct?

Larger the reduction potential, larger the oxidation tendency of the ion being reduced. Hence, the oxidizing tendency follows the order ${\mathrm{Pb}}^{4+}>{\mathrm{Hg}}^{2+}>{\mathrm{Sn}}^{4+}$

Lesser the reduction potential, larger the reduction tendency of the ion formed in the reduction reaction. Hence, the reducing tendency follows the order ${\mathrm{Sn}}^{2+}>{\mathrm{Hg}}^{2+}>{\mathrm{Pb}}^{2+}$