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Question 2:

part a:

ClO^- + 2H+ ---->

5Br^- + Br O2^---->

CCl4+ Ne2 ---->

IO2^- + KIO2 ---->

b:

The strongest oxidizing agent (among the halogens) is____

c:

The strongest reducing agent (among the halogens) is_

d:

If fluorine were included in the series, where should it go?

______________________________________________________________

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If you could answer the rest of Question 1 from the 6th and 7th picture and then Question 3 from the 8th and 9th picture

11 Oxidation-Reduction Reactions Introduction We encounter oxi uction reactions every day Examples include the combustion of coal natural gas, oil, and gasoline, the operation of automobile's battery and the sains by a Although there are a variety of oxidation-reduction reactions .when you compare a number of you can some common featu Each these of simultaneous oxidation and reduction because electrons are lost by one atom and gained by another one. Moreover, the reactants include an agent and a reducing agent always lost agent and gained by the oxidizing agent (Ebbing/Gammon, Section 4.5) Purpose You will begin by preparing aqueous solutions of three halogens: Cl2, Bra, and Iz. You will prepare these substances in solution from stoichiometric quantities of certain oxidizing and agents. By observing the effect ofthese halogens on the corresponding halides (CI,Br, and you will be able the halogens according to their oxidizing strengths and the halides according to their reducing strengths. Your subsequent observations on the reactions of two halides, Br and I with two common oxidizing agents will enable you to rank the latter according to their oxidizing strengths. You will also find that the products obtained from an oxidation-reduction reaction in an acidic solution can differ markedly from those obtained in a basic solution. Finally, and most important, you will write a balanced equation for each reaction that you have observed The Halogens and the Halides You will deal with halogens and halides in each part ofthis experiment. A brief description of some of their properties will enable you to understand some of your observations more easily. The halogens are found in Group VIIA of the periodic table. The members of this group are fluorine (F) chlorine (CI, bromine (B), iodine (i) and astatine these elements belong to the same 12, group, have many similar properties. For example, their elemental diatomic (F2.cl. Br2, they Atal, and each of them is an oxidizing agent. This experiment uses only Cl, Bra, and Iz, however, because F is such a strong oxidizing agent that special conditions are required for its study and because astatine is radioactive. Aqueous solutions ofcl, be prepared either by dissolving these elements in water or by generating them in Br, reactions. Aqueous solutions of these halogens are solution as products of certain oxidation-reduction respectively. Each called chlorine water, brominee and iodine thickness solution. has its own characteristic color, depending on the concentration and red-brown to water is colorless to yellow; bromine water is yellow to red-brown; and iodine water is brown These halogens are also soluble in cyclohexane (C6H12, a substance that is itselfinsoluble in water. layer When cyclohexane is added to an aqueous solution of a halogen, two layers are formed. The upper is cyclohexane, because it is insoluble and less dense than water. A portion of the halogen passes from the aqueous layer to the upper cyclohexane layer (a process called extraction). A characteristic color is then imparted to this layer. The color ofa halogen in cyclohexane differs somewhat from its color in an aqueous solution, as you will discover during the experiment. be scanned, copied or duplicated or possed toa publicly accessible webwie, iawhole or in Cengage Leaming All Rights Resened c 2013

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