The Reaction
Cl₂ (g) + 2Br⁻ (aq) → 2Cl⁻ (aq) + Br₂ (l)
Explanation
* Chlorine is more reactive than bromine. This is due to chlorine's smaller atomic size and stronger electronegativity, making it easier for chlorine to gain electrons.
* Chlorine displaces bromine from bromide ions. The chlorine gas reacts with the bromide ions, pulling electrons away from the bromide ions and forming chloride ions (Cl⁻). This results in the formation of bromine gas (Br₂).
* The reaction is an oxidation-reduction (redox) reaction. Chlorine is reduced (gains electrons) while bromine is oxidized (loses electrons).
Observations
* Color change: If you mix chlorine gas with a solution containing bromide ions, you'll observe a color change. The initially colorless bromide solution will turn reddish-brown as bromine (Br₂) forms.
* Formation of bromine liquid: If the reaction is carried out in a solution, the bromine produced may be seen as a reddish-brown liquid at the bottom of the container.
Importance
This reaction demonstrates the relative reactivity of halogens, and it's an important principle used in the production of bromine from seawater.
