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Chapter 4: Problem 58

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens: $$\begin{array}{c}{\mathrm{Br}_{2}(a q)+2 \mathrm{Nal}(a q) \longrightarrow 2 \mathrm{NaBr}(a q)+\mathrm{I}_{2}(a q)} \\ {\mathrm{Cl}_{2}(a q)+2 \mathrm{NaBr}(a q) \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{Br}_{2}(a q)}\end{array}$$ (a) Which elemental halogen would you predict is the most stable, upon mixing with other halides? (b) Predict whether a reaction will occur when elemental chlorine and potassium iodide are mixed. (c) Predict whether a reaction will occur when elemental bromine and lithium chloride are mixed.

Short Answer

Expert verified
(a) The most stable halogen upon mixing with other halides is iodine (\(I_2\)), as stability increases going down the group of halogens. (b) A reaction will occur when elemental chlorine and potassium iodide are mixed, producing potassium chloride (\(KCl\)) and elemental iodine (\(I_2\)). (c) No reaction will occur when elemental bromine and lithium chloride are mixed, as bromine is less reactive than chlorine.

Step by step solution

01

1. Identify the Trends in Halogens

Recall that the halogens form a group in the periodic table (Group 17). Their reactivity decreases going down the group, making the higher halogens more stable than the lower ones. Using this information, we can list the halogens in decreasing order of reactivity: \(\\ Cl_2 > Br_2 > I_2\\ \).
02

2. Compare the Reactivity to Predict Stability

(a) Since reactivity decreases as we go down the halogens, stability increases. Therefore, the most stable halogen would be the one at the bottom of the list. In our case, it is iodine (\(I_2\)).
03

3. Predict the Outcome of Mixing Elemental Chlorine and Potassium Iodide

(b) The given reaction is: \(\\ Cl_2 (aq) + 2KI (aq)\\ \). Following the trend in reactivity, if the elemental chlorine is more reactive than iodine, the reaction will occur. Looking at our reactivity trend, we see that: \(\\ Cl_2 > I_2\\ \), so elemental chlorine is more reactive than iodine. Hence, the reaction will occur, producing potassium chloride (\(KCl\)) and elemental iodine (\(I_2\)): \[Cl_2(aq) + 2KI(aq) \longrightarrow 2KCl(aq) + I_2(aq)\]
04

4. Predict the Outcome of Mixing Elemental Bromine and Lithium Chloride

(c) The given reaction is: \(\\ Br_2 (aq) + 2LiCl (aq)\\ \). Similar to the previous step, if the elemental bromine is more reactive than the chloride ion (Cl), the reaction will occur. Comparing the reactivity, we see that bromine is less reactive than chlorine: \(\\ Cl_2 > Br_2\\ \), so elemental bromine is less reactive than the chloride ion. Therefore, no reaction will occur when elemental bromine and lithium chloride are mixed.

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