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Objective: To investigate the order of oxidizing ability of the halogens Cl2, Br2, and I2 in aqueous solution

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Name: Subasri Thomas Name of lab partner: Ranjini Sri Naransamy Date: 3/7/2012 Title: Halogen ? halide reactions in aqueous solution Objective: To investigate the order of oxidizing ability of the halogens Cl2, Br2, and I2 in aqueous solution Apparatus / Materials: Test tubes, Bromine water ,Br2(aq) ,Chlorine water, Cl2(aq), Iodine solution,I2 (in KI aq),Potassium Bromide solution( KBr),Potassium chloride solution(KCl), Potassium iodide solution(KI),Hexane(C6H14) Procedure: 1. Reaction (if any) of iodide with chlorine and bromine 1. About 1mL of Potassium iodide solution is added to each of two test tubes 2. About the same volume of chlorine water is added to one of these tubes and the other was added with the same volume of bromine water 3. The test tubes is shake and the color changes is noted-(if any) 4. A few drops of hexane is added to each tube, shake and allow it to settled and the color of each layer is noted. 5. Reaction that taken place is observed and a copy of result is completed in table 11.1. 1. Reaction (if any) of bromide with chlorine and iodine 1. About 1mL of Potassium bromide solution is added to each of two test tubes 2. ...read more.


orange purple lower X Light yellow light red Conclusion X No visible reaction observed No visible reaction observed Discussions: Halogens act as oxidizing agents (electron acceptors) in the majority of their reactions. X2 + 2 e 2 X-(aq) When going down the group, the atomic size increases. As the atomic size increases, the ns2np5 valence electron in outermost shell is further apart from the nucleus. Thus the electronegativity decreases down the group. As the electronegativity decreased the oxidizing power of the halogens also decreases because of the size of the element and the electron affinity as well as hydration energy decreases. The halogens which are higher in the group can oxidize halide ions lower in the group. The arrangements of elements of group 17 according to periodic table is Fluorine,Chlorine,Bromine,Iodine and Astatine. Since Fluorine, F2 is higher in the group it is the strongest oxidizing agent in halogens group. It can oxidize chloride ion. This is obviously a redox reaction in which oxidation and reduction occurs simultaneously. F2 + 2 Cl- 2 F- + Cl2 In this experiment iodide reacted with chlorine and bromine water. ...read more.


In the reaction of iodide ions with chlorine and bromine, iodine has been extracted from the solution after adding hexane. That means iodide ion is displaced by chlorine and bromine. For the reaction of bromide ion with chlorine and iodine, only Br2 will extracted from chlorine solution after shake with hexane, and the bromine ions cannot be displaced by iodine because of the oxidizing power. For the reaction between chloride ion with bromine and iodine, there has no any reaction occur, and the bromine and iodine are extracted from both solutions respectively. From there, it can know that chloride ions cannot displace by any of bromine and iodine. Hence, the strongest oxidizing agent is chlorine, follow by bromine and iodine. I2 < Br2 < Cl2 Questions: 1. 1. I2 (aq KI) does not oxidize Cl- (aq)and Br-(aq) 2. Br2 (aq) does not oxidize Cl- (aq) but oxidize I-(aq) 3. Cl2 oxidize Br-(aq) and I-(aq) 2. 1. Chlorine can oxidized the bromide ions in potassium bromide aqueous solution and also iodide ions in potassium iodide aqueous solution. 1. Cl2 + 2Br- 2Cl- + Br2 2. Cl2 + 2I- 2Cl- + I2 1. Bromine can oxidized the iodide ions in potassium iodide aqueous solution 1. Br2 + 2I- 2Br- + I2 3. ...read more.

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