* Electrochemical Series: Chlorine is higher in the electrochemical series than bromine. This means chlorine has a stronger tendency to gain electrons and form negative ions (anions).
* Reaction Mechanism: When chlorine gas is bubbled through a potassium bromide solution, the following reaction takes place:
```
Cl2(g) + 2KBr(aq) → 2KCl(aq) + Br2(l)
```
* Displacement: Chlorine atoms are more reactive and readily accept electrons from bromide ions (Br-), forming chloride ions (Cl-). This leaves the bromine atoms to bond together, forming liquid bromine (Br2), which is observed as a reddish-brown color in the solution.
In simpler terms: Chlorine is a "stronger" non-metal than bromine and "wants" the electrons more. So, it "steals" the electrons from bromine, forcing it out of the potassium bromide solution.
