In a single replacement reaction, a metal and a metal compound may react so that the metal will replace the metal in the compound, producing the replaced metal and a new compound with the original metal. #"A + BC"##rarr##"B + AC"#, where #"A"# and #"B"# are metals, and #"C"# is a negative ion. In order to determine whether this will actually happen, you consult an activity series of metals. An activity series of metals lists metals in descending order of reactivity. This means that a metal can only replace a metal below it in the series. Example 1: Will the following single replacement reaction occur? #"Cu(s) + Zn(NO"_3)_2("aq")"##rarr##"Zn(s) + Cu(NO"_3)_2"# If we look at the activity series above, we see that copper is below zinc, so it cannot replace the zinc in the zinc nitrate compound. So this reaction will not occur. We would write it as: #"Cu(s) + Zn(NO"_3)_2("aq")"##rarr##"no reaction"# Example 2: Will the following single replacement reaction occur? #"2Al(s) + 3CuSO"_4("aq")"##rarr##"3Cu(s) + Al"_2("SO"_4)_3"# If we look at the activity series, we see that aluminum is above copper, so this reaction will occur, and the aluminum will replace the copper to form aluminum sulfate. The video shows an experiment to determine the placement of three different metals (Cu, Zn and Mg) on the activity series.
Learning Objectives
Up to now, we have presented chemical reactions as a topic, but we have not discussed how the products of a chemical reaction can be predicted. Here we will begin our study of certain types of chemical reactions that allow us to predict what the products of the reaction will be. A single-replacement reaction is a chemical reaction in which one element is substituted for another element in a compound, generating a new element and a new compound as products. For example, 2 HCl(aq) + Zn(s) → ZnCl2(aq) + H2(g) is an example of a single-replacement reaction. The hydrogen atoms in HCl are replaced by Zn atoms, and in the process a new element—hydrogen—is formed. Another example of a single-replacement reaction is 2 NaCl(aq) + F2(g) → 2 NaF(s) + Cl2(g) Here the negatively charged ion changes from chloride to fluoride. A typical characteristic of a single-replacement reaction is that there is one element as a reactant and another element as a product. Not all proposed single-replacement reactions will occur between two given reactants. This is most easily demonstrated with fluorine, chlorine, bromine, and iodine. Collectively, these elements are called the halogens and are in the next-to-last column on the periodic table (see Figure 4.1 “Halogens on the Periodic Table”). The elements on top of the column will replace the elements below them on the periodic table but not the other way around. Thus, the reaction represented by CaI2(s) + Cl2(g) → CaCl2(s) + I2(s) will occur, but the reaction CaF2(s) + Br2(ℓ) → CaBr2(s) + F2(g) will not because bromine is below fluorine on the periodic table. This is just one of many ways the periodic table helps us understand chemistry.
Figure 4.1 Halogens on the Periodic Table The halogens are the elements in the next-to-last column on the periodic table.
Will a single-replacement reaction occur? If so, identify the products.
Solution
Test Yourself Will a single-replacement reaction occur? If so, identify the products. FeI2 + Cl2 → ? Answer Yes; FeCl2 and I2 Chemical reactivity trends are easy to predict when replacing anions in simple ionic compounds—simply use their relative positions on the periodic table. However, when replacing the cations, the trends are not as straightforward. This is partly because there are so many elements that can form cations; an element in one column on the periodic table may replace another element nearby, or it may not. A list called the activity series does the same thing the periodic table does for halogens: it lists the elements that will replace elements below them in single-replacement reactions. A simple activity series is shown below. Activity Series for Cation Replacement in Single-Replacement Reactions
Using the activity series is similar to using the positions of the halogens on the periodic table. An element on top will replace an element below it in compounds undergoing a single-replacement reaction. Elements will not replace elements above them in compounds.
Use the activity series to predict the products, if any, of each equation.
Solution
Test Yourself Use the activity series to predict the products, if any, of this equation. AlPO4 + Mg → ? Answer Mg3(PO4)2 and Al A double-replacement reaction occurs when parts of two ionic compounds are exchanged, making two new compounds. A characteristic of a double-replacement equation is that there are two compounds as reactants and two different compounds as products. An example is CuCl2(aq) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 AgCl(s) There are two equivalent ways of considering a double-replacement equation: either the cations are swapped, or the anions are swapped. (You cannot swap both; you would end up with the same substances you started with.) Either perspective should allow you to predict the proper products, as long as you pair a cation with an anion and not a cation with a cation or an anion with an anion.
Predict the products of this double-replacement equation: BaCl2 + Na2SO4 → ? Solution Thinking about the reaction as either switching the cations or switching the anions, we would expect the products to be BaSO4 and NaCl. Test Yourself Predict the products of this double-replacement equation: KBr + AgNO3 → ? Answer KNO3 and AgBr Predicting whether a double-replacement reaction occurs is somewhat more difficult than predicting a single-replacement reaction. However, there is one type of double-replacement reaction that we can predict: the precipitation reaction. A precipitation reaction occurs when two ionic compounds are dissolved in water and form a new ionic compound that does not dissolve; this new compound falls out of solution as a solid precipitate. The formation of a solid precipitate is the driving force that makes the reaction proceed. To judge whether double-replacement reactions will occur, we need to know what kinds of ionic compounds form precipitates. For this, we use solubility rules, which are general statements that predict which ionic compounds dissolve (are soluble) and which do not (are not soluble or insoluble). Table 4.1 “Some Useful Solubility Rules” lists some general solubility rules. We need to consider each ionic compound (both the reactants and the possible products) in light of the solubility rules in Table 4.1 “Some Useful Solubility Rules”. If a compound is soluble, we use the (aq) label with it, indicating it dissolves. If a compound is not soluble, we use the (s) label with it and assume that it will precipitate out of solution. If everything is soluble, then no reaction will be expected.
Table 4.1 Some Useful Solubility Rules
For example, consider the possible double-replacement reaction between Na2SO4 and SrCl2. The solubility rules say that all ionic sodium compounds are soluble and all ionic chloride compounds are soluble except for Ag+, Hg22+, and Pb2+, which are not being considered here. Therefore, Na2SO4 and SrCl2 are both soluble. The possible double-replacement reaction products are NaCl and SrSO4. Are these soluble? NaCl is (by the same rule we just quoted), but what about SrSO4? Compounds of the sulfate ion are generally soluble, but Sr2+ is an exception: we expect it to be insoluble—a precipitate. Therefore, we expect a reaction to occur, and the balanced chemical equation would be Na2SO4(aq) + SrCl2(aq) → 2 NaCl(aq) + SrSO4(s) You would expect to see a visual change corresponding to SrSO4 precipitating out of solution (Figure 4.2 “Double-Replacement Reactions”).
Will a double-replacement reaction occur? If so, identify the products.
Solution
Test Yourself Will a double-replacement equation occur? If so, identify the products. Sr(NO3)2 + KCl → ? Answer No reaction; all possible products are soluble. |