Consider the following reduction processes :
$\mathrm{Zn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(\mathrm{s}) ; \mathrm{E}^{\circ}=-0.76 \mathrm{~V}$
$\mathrm{Ca}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Ca}(\mathrm{s}) ; \mathrm{E}^{\circ}=-2.87 \mathrm{~V}$
$\mathrm{Mg}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mg}(\mathrm{s}) ; \mathrm{E}^{\circ}=-2.36 \mathrm{~V}$
$\mathrm{Ni}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Ni}(\mathrm{s}) ; \mathrm{E}^{\circ}=-0.25 \mathrm{~V}$
The reducing power of the metals increases in the order:
Correct Option: , 2
Higher the oxidation potential better will be reducing power.
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