Chapter 7 Chemical Reactions Section 7.1 Describing Reactions Section 7.2 Types of Reactions.
Section 1 Describing Chemical Reactions
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Transcript of Section 1 Describing Chemical Reactions
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• A chemical reaction is the process by which one or more substances change into one or more new substances.
• Reactants are the original substances in a chemical reaction.
• Products are the substances that are created in a chemical reaction.
Section 1 Describing Chemical ReactionsChapter 8
Chemical Reaction
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Visual Concepts
Chemical Reaction
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Evidence of a Chemical Reaction
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Signs of a Chemical Reaction
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Precipitate
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Evidence of a Chemical Reaction
Section 1 Describing Chemical Reactions
• solution color changes• solution bubbles• copper is used up
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Chemical Reaction Versus Physical Change
• chemical change – new substance forms with properties that differ from original substance
• density• boiling point• melting point
• physical change - changes of state • evaporation• condensation• melting• freezing
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Reactions and Energy Changes
• Energy can be released in a chemical reaction.
methane + oxygen carbon dioxide + water + energy
Energy is a product.
• Energy can be absorbed in a chemical reaction.
dinitrogen tetroxide + energy nitrogen dioxide
Energy is a reactant.
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Constructing a Chemical Equation
• A chemical equation shows the chemical formulas and relative amounts of all reactants and products.
• A word equation contains the names of the reactants and products.
• Equations must be balanced.
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Writing a Word Equation or Formula Equation
methane + oxygen carbon dioxide + water
?CH4 + ?O2 ?CO2 + ?H2O
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Equations and Reaction Information
• Physical States
NaHCO3(s) + HC2H3O2(aq) NaC2H3O2(aq) + CO2(aq) + H2O(l) solid
liquid
Section 1 Describing Chemical ReactionsChapter 8
catalystN2(g) + 3H2(g) 2NH3(g)
aqueous solutions
• Reaction Conditions 350°C, 25 000 kPa
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Equations and Reaction Information
Section 1 Describing Chemical ReactionsChapter 8
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Chemical Equation
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Reactions Conserve Mass
• Mass cannot be created or destroyed by a chemical or physical change
• Equations must be balanced.
?Na + ?H2O ?NaOH + ?H2
Section 2 Balancing Chemical EquationsChapter 8
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Balancing Equations
• The number of atoms for each element must be the same on the reactants’ side and on the products’ side.
• A coefficient multiplies the number of atoms of each element in the formula that follows.
H2O: 2 hydrogen atoms, 1 oxygen atom
2H2O: 4 hydrogen atoms, 2 oxygen atoms
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Reading a Chemical Equation
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Balancing a Chemical Equation by Inspection
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Balancing Equations
Sample Problem ABalance the equation for the reaction of iron(III) oxide with hydrogen to form iron and water.
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Balancing EquationsSample Problem A Solution1. Identify reactants and products.
reactants products
Section 2 Balancing Chemical Equations
Reactants Products Balanced?
Unbalanced formula equation Fe2O3 + H2 Fe + H2O
Iron atoms 2 1 no
Oxygen atoms 3 1 no
Hydrogen atoms 2 2 yes
3 32
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3. Insert coefficients.
2. Count atomsFe2O3 + H2 Fe + H2O
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Reactions Conserve Mass
• Balanced equations show mass conservation
?Na + ?H2O ?NaOH + ?H2
2Na + 2H2O 2NaOH + H2
• Never change subscripts to balance equationsUnbalanced: H2 + O2 H2O
Incorrect: H2 + O2 H2O2
H2O H2O2
Correct: 2H2 + O2 2H2O
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Reactions Conserve Mass
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Polyatomic Ions can be balanced as a group
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Balancing Equations
Sample Problem CAluminum reacts with arsenic acid, HAsO3, to form H2 and aluminum arsenate. Write a balanced equation for this reaction.
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Balancing EquationsSample Problem C Solution1. Identify reactants and products.
reactants productsAl + HAsO3 H2 + Al(AsO3)3
2. Count Atoms
Section 2 Balancing Chemical Equations
Reactants Products Balanced?
Unbalanced formula equation Al + HAsO3 H2 + Al(AsO3)3
Iron atoms 1 1 yes
Oxygen atoms 1 2 no
Hydrogen atoms 1 3 no
3 22 6
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3. Insert coefficients
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Section 3 Classifying Chemical Reactions
Combustion Reactions
• A combustion reaction is a reaction of a carbon-based compound with oxygen.
Combustion of propane:
C3H8 + 5O2 3CO2 + 4H2O
Combustion of ethanol:
CH3CH2OH + 3O2 2CO2 + 3H2O
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Combustion Reaction
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Section 3 Classifying Chemical Reactions
Synthesis Reactions
• In a synthesis reaction a single compound forms from two or more reactants.
• Two elements form a binary compound
C + O2 CO2
2C + O2 2CO
• Two compounds form a ternary compoundCaO(s) + H2O(l) Ca(OH)2(s)
CO2(g) + H2O(l) H2CO3(aq)
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Synthesis Reactions
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Section 3 Classifying Chemical Reactions
Decomposition Reactions
• In a decomposition reaction a single compound breaks down, often with the input of energy, into two or more elements or simpler compounds.
• Decomposition of waterelectricity
heat
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CaCO3(s) CaO(s) + CO2(g)
• A metal carbonate decomposes to form a metal oxide and carbon dioxide.
2H2O(l) O2(g) + 2H2(g)
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Decomposition Reaction
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Electrolysis
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Section 3 Classifying Chemical Reactions
Decomposition Reactions, continued Sample Problem D
Predicting Products Predict the product(s) and write a balanced equation for the reaction of potassium with chlorine.
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Section 3 Classifying Chemical Reactions
Decomposition Reactions, continued Sample Problem D Solution
• Reaction is most likely a synthesis reaction, so the product will be binary
• Potassium will lose one electron to become a 1+ ion.
• Chlorine will gain one electron to become a 1– ion.
K + Cl2 KCl
• Balance the equation.
2K + Cl2 2KCl
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Section 3 Classifying Chemical Reactions
Displacement Reactions
• In a displacement reaction a single element reacts with a compound and displaces another element from the compound.
2Al(s) + 3CuCl2(aq) 2AlCl3(aq) + 3Cu(s)
Aluminum displaces copper.
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Single Displacement Reaction
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Section 3 Classifying Chemical Reactions
Displacement Reactions, continued
• The activity series ranks the reactivity of elements
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Activity Series
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Section 3 Classifying Chemical Reactions
Displacement Reactions, continuedSample Problem E
Determining Products by Using the Activity Series Magnesium is added to a solution of lead(II) nitrate. Will a reaction happen? If so, write the equation and balance it.
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Section 3 Classifying Chemical Reactions
Displacement Reactions, continuedSample Problem E Solution
1. Identify the reactants. Magnesium will attempt to displace lead from lead(II) nitrate.
2. Check the activity series.Magnesium is more active than lead and displaces it.
3. Write the balanced equation.
Mg + Pb(NO3)2 Pb + Mg(NO3)2
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Section 3 Classifying Chemical Reactions
Double-Displacement Reactions
• In a double-displacement reaction two compounds in aqueous solution appear to exchange ions and form two new compounds.
• One of the products must be a solid precipitate, a gas, or a molecular compound, such as water.
HCl(aq) + NaOH(aq) HOH(l) + NaCl(aq)
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Double-Displacement Reaction
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Precipitation Reaction
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Identifying Reactions and Predicting Products
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