Chlorine is highly electronegative; they form ionic compounds with polar bonding. As you go down group seven electronegativity decreases.
The equation for this reaction is:
Cl2 (aq) +2K+I- (aq) 2K+Cl- (aq) + I2
This is a redox reaction, this is because Cl oxidises I- (oxidation state –1) to iodine (oxidation state 0). Chlorine, Cl2 (oxidation state 0 ) is reduced to Cl- (oxidation state –1). So the more reactive halogen (Cl) will oxidise the halide ions of a less reactive one (Br). The other equation for the reaction are:
Cl2 (aq) +2K+Br- (aq) 2K+Cl- (aq) + Br2
When bromine solution is added to potassium chloride there is no change because chlorine is more reactive than bromine. What happens is that the solution becomes more dilute and lighter, see equation below.
Br + KCl Br + KCl
But when bromine is added to potassium iodide a displacement reaction occurs
The bromine displaces the iodide because it is more reactive. See equation below.
Br2 (aq) +2K+I- (aq) 2K+Br- (aq) + I2
C) When aqueous solutions of potassium halides are added to silver nitrate solution a precipitate starts to appear immediately. For example when potassium chloride is added to silver nitrate white precipitate appears immediately. This is a test to prove that the element is chlorine when you add cyclohexane.
KCl (aq) + AgNO3 KNO3 (aq) + AgCl White precipitation
Here are the other equation:
KI (aq) + AgNO3 KNO3 (aq) + AgI Yellow precipitation
KBr (aq) + AgNO3 KNO3 (aq) + AgBr Cream precipitation
The appearances of the silver halides are:
Silver chloride White Precipitate
Silver bromide Cream Precipitate
Silver iodide Yellow Precipitate
D) When adding aqueous solutions of potassium halides to lead nitrate solution a precipitate appears. For example, when potassium chloride solution is added to lead nitrate solution white precipitate forms immediately and collects at the bottom.
This is because the Cl displaces the NO3 and becomes PbCl + KNO3. The test to prove that the element is chlorine you need to add cyclohexane and the precipitate will be White, and for bromine it will be Cream, and for iodine yellow precipitate will appear.
KCl (aq) + PbNO3 KNO3 (aq) + PbCl White precipitation
Here are the other equations:
KCl (aq) + PbNO3 KNO3 (aq) + PbCl Yellow precipitation
KCl (aq) + PbNO3 KNO3 (aq) + PbCl Cream precipitation
By Akash Patel