Given the balanced ionic equation representing a reaction below. In this reaction, where are electrons transferred from?

Jun 10, 2017

This is a redox reaction in which electrons are formally transferred....

Explanation:

$\text{Oxidation reaction}$

$M g \rightarrow M {g}^{2 +} + 2 {e}^{-}$ $\left(i\right)$

$\text{Reduction reaction}$

$A {l}^{3 +} + 3 {e}^{-} \rightarrow A l$ $\left(i i\right)$

And we cross multiply the individual redox equations so that electrons are absent from the final redox equation, i.e. $3 \times \left(i\right) + 2 \times \left(i i\right) = \ldots \ldots \ldots . .$

$3 M g + 2 A {l}^{3 +} + \cancel{6 {e}^{-}} \rightarrow 2 A l + 3 M {g}^{2 +} + \cancel{6 {e}^{-}}$

And finally.............

$3 M g + 2 A {l}^{3 +} \rightarrow 2 A l + 3 M {g}^{2 +}$

Jun 10, 2017