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Chapter 11 Chemical Reactions 11.1 Describing Chemical Reactions 11.2 Types of Chemical
Reactions 11.3 Reactions in Aqueous Solution
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Classifying Reactions
Five general types of reactions:
Synthesis (combination),
decomposition,
single-replacement,
double-replacement, and
combustion.
Classifying Reactions
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Not all chemical reactions fit uniquely into one category. • Occasionally, a reaction may fit equally well
into two categories.
• Patterns allow you to predict the products of reactions.
Classifying Reactions
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A combination reaction is a chemical change in which two or more substances react to form a single new substance.
Combination Reactions
Classifying Reactions
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Magnesium metal and oxygen gas combine to form the compound magnesium oxide.
Combination Reactions
Classifying Reactions
2Mg(s) + O2 → 2 MgO(s) Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
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In all combination reactions, the product is a single substance
• The reactants in this combination reaction (Mg and O2) are 2elements, which is often the case; but
• 2 compounds may also combine to form a single substance.
Combination Reactions
Classifying Reactions
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When a metal and a nonmetal react, the product is a binary ionic compound.
2K(s) + Cl2(g) → 2KCl(s)
Combination Reactions
Classifying Reactions
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When 2 nonmetals react in a combination reaction, more than one product is often possible.
S(s) + O2(g) → SO2(g) sulfur dioxide
2S(s) + 3O2(g) → 2SO3(s) sulfur trioxide
Combination Reactions
Classifying Reactions
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More than one product may also result from the combination reaction of a transition metal and a nonmetal.
Fe(s) + S(s) → FeS(s) iron(II) sulfide
2Fe(s) + 3S(g) → Fe2S3(s) iron(III) sulfide
Combination Reactions
Classifying Reactions
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The opposite of combination reactions. Decomposition Reactions
Classifying Reactions
• When mercury(II) oxide is heated, it decomposes or breaks down into two simpler substances.
2HgO(s) 2Hg(l) + O2(g) heat
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A decomposition reaction is a chemical change in which a single compound breaks down into two or more simpler products. • 1 reactant, 2 or more products.
• Products can be any combination of elements and/or compounds.
• Most decomposition reactions require an input of energy in the form of heat, light, or electricity.
Decomposition Reactions
Classifying Reactions
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Did you know that a decomposition reaction happens when a vehicle’s air bag inflates? When a device is triggered, sodium azide pellets decompose and release nitrogen gas, which inflates the air bag quickly.
2NaN3(s) → 2Na(s) + 3N2(g)
Decomposition Reactions
Classifying Reactions
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Sample Problem 11.4
Writing Equations for Combination and Decomposition Reactions
Write a balanced equation for each of the following reactions.
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a. Combination of copper and sulfur: Cu(s) + S(s) → (two reactions possible)
b. Decomposition of water: H2O(l) electricity
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a. Two reactions are possible because Copper has more than one common ionic charge (Cu+ and Cu2+).
Sample Problem 11.4
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Skeleton equations:
Sample Problem 11.4
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a. For Copper(I): Cu(s) + S(s) → Cu2S(s)
For Copper(II): Cu(s) + S(s) → CuS(s)
b. H2O H2(g) + O2(g) electricity
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Solve Apply concepts to this problem. 2
Apply the rules for balancing equations. For Copper(I): 2Cu(s) + S(s) → Cu2S(s)
For Copper(II): the skeleton equation is already balanced. Cu(s) + S(s) → CuS(s)
Sample Problem 11.4
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Solve Apply concepts to this problem. 2
Apply the rules for balancing equations.
Sample Problem 11.4
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2H2O(l) 2H2(g) + O2(g)
electricity
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Dropping a small piece of potassium into a beaker of water creates the vigorous reaction.
2K(s) + 2H2O(l) → 2KOH(aq) + H2
Single-Replacement Reactions
Classifying Reactions
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• The released hydrogen gas can ignite explosively.
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If you drop a piece of zinc into a solution of copper nitrate, this reaction occurs:
Zn(s) + Cu(NO3)2(aq) → Cu(s) + Zn(NO3)2(aq)
Single-Replacement Reactions
Classifying Reactions
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These equations describe two examples of single-replacement reaction.
2K(s) + 2H2O(l) → 2KOH(aq) + H2(g)
Zn(s) + Cu(NO3)2(aq) → Cu(s) + Zn(NO3)2
• In a single-replacement reaction both the reactants and the products consist of an element and a compound.
Single-Replacement Reactions
Classifying Reactions
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Sample Problem 11.5
Writing Equations for Single-Replacement Reactions
Write a balanced equation for the single-replacement reaction.
Cl2(aq) + NaBr(aq) →
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Chlorine is a more reactive halogen than bromine; therefore Cl displaces Br in compounds.
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Solve Apply concepts to this problem. 2
• Write the skeleton equation. Cl2(aq) + NaBr(aq) → NaCl(aq) + Br2(aq)
Sample Problem 11.5
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• Apply the rules for balancing equations.
Cl2(aq) + 2NaBr(aq) → 2NaCl(aq) + Br2(aq) (balanced)
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A halogen can replace a less active halogen from a compound.
• The activity of halogens decreases as you go down Group 17
• Bromine is more active than iodine, so this reaction occurs:
Br2(aq) + 2NaI(aq) → 2NaBr(aq) + I2(aq)
• But Br is less active than chlorine, so this reaction does not occur:
Br2(aq) + NaCl(aq) → No reaction
Single-Replacement Reactions
Classifying Reactions
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Whether one metal will displace another metal from a compound depends upon the relative reactivities of the two metals.
Single-Replacement Reactions
Classifying Reactions
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• Fe can displace Cu
• Fe does not displace Zn or Ca.
Activity Series of Metals Name Symbol Lithium Li Calcium Ca Sodium Na
Magnesium Mg Aluminum Al
Zinc Zn Iron Fe Lead Pb
Copper Cu Mercury Hg Silver Ag
Dec
reas
ing
reac
tivity
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Single-Replacement Reactions
Classifying Reactions
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• The activity series of metals lists metals in order of decreasing reactivity.
• A reactive metal will replace any metal listed below it in the activity series.
Activity Series of Metals Name Symbol Lithium Li Calcium Ca Sodium Na
Magnesium Mg Aluminum Al
Zinc Zn Iron Fe Lead Pb
Copper Cu Mercury Hg Silver Ag
Dec
reas
ing
reac
tivity
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Double-Replacement Reactions
Classifying Reactions
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Mixing aqueous solutions of potassium iodide and lead(II) nitrate results in a chemical reaction in which a yellow precipitate of solid lead(II) iodide is formed.
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Double-Replacement/Displacement Reactions
Chemical change involving an exchange of positive ions between two compounds.
• Usually take place in aqueous solution [both reactants are (aq)]
Classifying Reactions
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2KI(aq) + Pb(NO3)2(aq) → PbI2 + 2KNO3(aq)
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Double-Replacement Reactions For a double-replacement reaction to occur, one of the following is usually true:
1. One of the products is only slightly soluble and precipitates from solution.
2. One of the products is a gas.
3. One product is a molecular compound such as water.
Classifying Reactions
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Sample Problem 11.6
Writing Equations for Double-Replacement Reactions A precipitate of barium carbonate is formed when aqueous solutions of barium chloride react with potassium carbonate. Write a balanced chemical equation for the double-replacement reaction.
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K2CO3(aq) + BaCl2(aq) →
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Solve Apply concepts to this problem. 2
• Write the skeleton equation.
K2CO3(aq) + BaCl2(aq) → KCl(aq) + BaCO3(s)
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Sample Problem 11.6
• Apply the rules for balancing equations. K2CO3(aq) + BaCl2(aq) → 2KCl(aq) + BaCO3(s)
(balanced)
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Combustion Reactions
Classifying Reactions
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A chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light.
• A combustion reaction always involves oxygen (O2) as a reactant.
• Often the other reactant is a hydrocarbon
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Combustion Reactions The complete combustion of a hydrocarbon produces carbon dioxide (CO2) and water (H2O).
Classifying Reactions
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• But if the supply of oxygen is limited during a reaction, the combustion will not be complete.
• Elemental carbon (soot) and toxic carbon monoxide gas may be additional products.
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Combustion Reactions The complete combustion of a hydrocarbon releases a large amount of energy as heat.
Classifying Reactions
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• That’s why hydrocarbons such as methane (CH4), propane (C3H8), and butane (C4H10) are important fuels.
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
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Combustion Reactions Gasoline is a mixture of hydrocarbons that can be approximately represented by the formula C8H18.
Classifying Reactions
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• The complete combustion of gasoline in a car engine is shown by this equation:
C8H18(l) + 5O2(g) → CO2(g) + H2O(g)
2C8H18(l) + 25O2(g) → 16CO2(g) + 18H2O(g)
Balanced:
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Combustion Reactions The reactions between oxygen and some elements other than carbon are also examples of combustion reactions.
Classifying Reactions
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• Notice that the reactions could also be classified as combination reactions.
• For our purposes, these will be classified as synthesis reactions
2Mg(s) + O2(g) → 2MgO(s)
S(s) + O2(g) → SO2(s)
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Sample Problem 11.7
Writing Equations for Combustion Reactions An alcohol lamp often uses ethanol as its fuel. Write a balanced equation for the complete combustion of ethanol.
C2H6O(l)
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Solve Apply concepts to this problem. 2
• Write the skeleton equation.
C2H6O(l) + O2(g) → CO2(g) + H2O(g)
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Sample Problem 11.7
• Apply the rules for balancing equations.
C2H6O(l) + 3O2(g) → 2CO2(g) + 3H2O(g) (balanced)
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Classifying Reactions
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In a combination reaction, two or more reactants (elements or compounds) combine to form a single product.
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Classifying Reactions
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In a decomposition reaction, a single compound is the reactant; two or more substances are the products.
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Classifying Reactions
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An element and a compound are the reactants in a single-replacement reaction.
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Classifying Reactions
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In a double-replacement reaction, two ionic compounds are the reactants; two new compounds are the products.
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Classifying Reactions
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The reactants in a combustion reaction are oxygen and usually a hydrocarbon. The products of most combustion reactions are carbon dioxide and water.
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Why might you want to classify a chemical reaction?
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Why might you want to classify a chemical reaction?
Classifying a chemical reaction helps you predict what products will form.
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