# An Fe^(2+) salt is oxidized by elemental chlorine. What occurs to chlorine in this reaction?

## $\text{A. Chlorine is oxidized;}$ $\text{B. Chlorine is reduced;}$ $\text{C. Chlorine disproportionates;}$ $\text{D. Chlorine is neither oxidized nor reduced.}$

Apr 21, 2017

$\text{Option B}$

#### Explanation:

Formally, reduction is the GAIN of electrons, and a net DECREASE in oxidation number........

Dichlorine oxidizes the $F e \left(I I\right)$ centre to $F e \left(I I I\right)$, but is itself REDUCED in the process, as it is conceived to accept electrons from the iron centre.

$\stackrel{0}{C} {l}_{2} + 2 {e}^{-} \rightarrow 2 \stackrel{- I}{C} l$

The zerovalent element is reduced to the univalent anion.........