# Question #708cb

Oct 9, 2016

Do you speak of a redox reaction?

#### Explanation:

When aluminum chloride is formed, we conceive that aluminum metal is oxidized:

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

And gaseous chlorine is reduced:

$\frac{1}{2} C {l}_{2} \left(g\right) + {e}^{-} \rightarrow C {l}^{-}$ $\left(i i\right)$

As with any chemical reaction, both MASS and CHARGE are conserved.

TO represent the formation of $\text{aluminum chloride}$, we simply add, $\left(i\right) + 3 \times \left(i i\right)$:

$A l \left(s\right) + \frac{3}{2} C {l}_{2} \left(g\right) \rightarrow A l C {l}_{3} \left(s\right)$

And of course mass and charge have been conserved, as required.