Name: Solutions Manual to accompany Introduction to Chemical Principles 11th 0321814630 / 9780321814630
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This is completed downloadable of Solutions Manual to accompany Introduction to Chemical Principles 11th 0321814630 / 9780321814630

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ISBN-10 ‏ : ‎ 0321814630
ISBN-13 ‏ : ‎ 978-0321814630
Author: H. Stephen Stoker

Newly updated based on extensive reviewer feedback, this affordable introductory text remains focused on the essentials necessary for success in General Chemistry. Introduction to Chemistry Principles, Eleventh Edition focuses on the most important topics ― omitting organic and biochemistry chapters ― and teaches the problem-solving skills readers need. Each topic is introduced and developed step by step until reaching the level of sophistication required for further course work.

Table of Content:

Chapter 1 The Science of Chemistry
1.1 Chemistry—A Scientific Discipline
1.2 Scientific Research and Technology
1.3 The Scope of Chemistry
1.4 How Chemists Discover Things—The Scientific Method
Experiments, Observations, and Data
Example 1.1 Distinguishing between Qualitative and Quantitative Data
Solution
Scientific Facts
Scientific Laws
Scientific Hypotheses
Example 1.2 Relating Scientific Hypotheses to Experimental Information
Solution
Example 1.3 Differentiating among Terminologies Associated with the Scientific Method
Solution
Scientific Theories
1.5 The Limitations of the Scientific Method
1.6 Application Limitations for Methods of Science
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
Scientific Disciplines (Sec. 1.1)
Scientific Research and Technology (Sec. 1.2)
The Scientific Method (Sec. 1.4)
Multiple-Choice Practice Test
Chapter 2 Numbers from Measurements
2.1 The Importance of Measurement
2.2 Exact and Inexact Numbers
2.3 Accuracy, Precision, and Error
Example 2.1 Determining the Accuracy and Precision of a Series of Measurements
Solution
2.4 Uncertainty in Measurements
Example 2.2 Recording Measurements to the Proper Uncertainty Level
Solution
2.5 Significant Figures
Example 2.3 Determining the Number of Significant Figures in a Numerical Value
Solution
Example 2.4 Determining the Number of Significant Figures and Magnitude of Uncertainty in a Numerical Value
Solution
Example 2.5 Uncertainty and the Number of Significant Figures in a Measurement
Solution
2.6 Significant Figures and Mathematical Operations
Rounding Off Numbers
Example 2.6 Rounding Numbers to a Specified Number of Significant Figures
Solution
Operational Rules for Mathematical Operations
Example 2.7 Predicting the Number of Significant Figures That Should be Present in the Answer to a Multiplication Problem
Solution
Example 2.8 Expressing Multiplication/Division Answers to the Proper Number of Significant Figures
Solution
Example 2.9 Expressing Addition/Subtraction Answers to the Proper Number of Significant Figures
Solution
Significant Figures and Exact Numbers
Multiplication by a Small Whole Number
Example 2.10 Significant Figures in Calculations Involving Multiplication by a Small Whole Number
Solution
2.7 Expressing Numbers in Scientific Notation
Exponents
Converting from Decimal to Scientific Notation
Example 2.11 Expressing Decimal Numbers in Scientific Notation
Solution
Significant Figures and Scientific Notation
Converting from Scientific to Decimal Notation
Example 2.12 Expressing Scientific Notation Numbers in Decimal Notation
Solution
Uncertainty and Scientific Notation
Example 2.13 Determining the Uncertainty Associated with Numbers Expressed in Scientific Notation
Solution
Example 2.14 Uncertainty Considerations for a Number Expressed in Scientific Notation
Solution
2.8 Mathematical Operations in Scientific Notation
Multiplication in Scientific Notation
Example 2.15 Multiplication of Scientific Notation Numbers
Solution
Example 2.16 Multiplication of Numbers in Scientific Notation Form
Solution
Division in Scientific Notation
Example 2.17 Division of Scientific Notation Numbers
Solution
Addition and Subtraction in Scientific Notation
Example 2.18 Addition and Subtraction of Scientific Notation Numbers
Solution
Example 2.19 Adding Scientific Notation Numbers without Equalizing Exponents
Solution
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
Exact and Inexact Numbers (Sec. 2.2)
Accuracy and Precision (Sec. 2.3)
Uncertainty in Measurements (Sec. 2.4)
Significant Figures (Sec. 2.5)
Rounding Off (Sec. 2.6)
Significant Figures in Multiplication and Division (Sec. 2.6)
Significant Figures in Addition and Subtraction (Sec. 2.6)
Calculations Involving Both Significant Figure Rules (Sec. 2.6)
Significant Figures and Exact Numbers (Sec. 2.6)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 3 Unit Systems and Dimensional Analysis
3.1 The Metric System of Units
SI Units
Metric System Prefixes
Example 3.1 Recognizing the Mathematical Meanings of Metric System Prefixes
Solution
3.2 Metric Units of Length
3.3 Metric Units of Mass
3.4 Metric Units of Volume
3.5 Units in Mathematical Operations
3.6 Conversion Factors
English-to-English Conversion Factors
Metric-to-Metric Conversion Factors
Metric-to-English and English-to-Metric Conversion Factors
3.7 Dimensional Analysis
Metric-to-Metric Conversion Factor Use
Example 3.2 One-Step Metric-to-Metric Conversion Factor Problem
Solution
Example 3.3 Two-Step Metric-to-Metric Conversion Factor Problem
Solution
Example 3.4 Metric-to-Metric Conversion Factor Problem Involving Cubic Dimensions
Solution
English-to-English Conversion Factor Use
Example 3.5 Multistep English-to-English Conversion Factor Problem
Solution
English-to-Metric and Metric-to-English Conversion Factor Use
Example 3.6 English-to-Metric Conversion Factor Problem
Solution
Example 3.7 Multistep Metric-to-English Conversion Factor Problem
Solution
Example 3.8 Metric-to-English Conversion Factor Problem Involving Cubic Units
Solution
Units Involving More Than One Type of Measurement
Example 3.9 Conversion Factor Problem Involving Two Types of Units
Solution
3.8 Density
Example 3.10 Using Mass and Volume to Calculate Density
Solution
Using Density as a Conversion Factor
Example 3.11 Using Density as a Conversion Factor to Relate Mass and Volume
Solution
3.9 Equivalence Conversion Factors Other Than Density
Concentration and Dosage Relationship Conversion Factors
Example 3.12 Using Concentration Conversion Factors
Solution
Chemical Insight: VITAMIN A
Rate Relationship Conversion Factors
Example 3.13 Using Rate Conversion Factors
Solution
Cost Relationship Conversion Factors
Example 3.14 Using Cost Conversion Factors
Solution
3.10 Percentage And Percent Error
Example 3.15 Percentage Calculation
Solution
Using Percentage as a Conversion Factor
Example 3.16 Using Percentage as a Conversion Factor
Solution
Example 3.17 Multiple Use of Percentages in a Conversion Factor Problem
Solution
Percent Error
Example 3.18 Calculation of Percent Error
Solution
Student 1
Student 2
Student 3
3.11 Temperature Scales
Example 3.19 Fahrenheit-to-Celsius Temperature Conversion
Solution
Example 3.20 Celsius-to-Fahrenheit Temperature Conversion
Solution
Example 3.21 Temperature Scale Conversions
Solution
Temperature Readings and Significant Figures
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
Metric System Units (SECS. 3.1–3.4)
Area and Volume Measurements (SECS. 3.4 and 3.5)
Conversion Factors (Sec. 3.6)
Dimensional Analysis’Metric–Metric Unit Conversions (Sec. 3.7)
Dimensional Analysis—Metric–English Unit Conversions (Sec. 3.7)
Dimensional Analysis’Units Involving Two Types of Measurement (Sec. 3.7)
Density (Sec. 3.8)
Equivalence Conversion Factors (Sec. 3.9)
Percentage and Percent Error (Sec. 3.10)
Temperature Scales (Sec. 3.11)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 4 Basic Concepts About Matter
4.1 Chemistry—The Study of Matter
4.2 Physical States of Matter
4.3 Propertires of Matter
Physical and Chemical Properties
Example 4.1 Classifying Properties as Physical or Chemical
Solution
Intensive and Extensive Properties
Example 4.2 Classifying Properties as Intensive or Extensive
Solution
4.4 Changes in Matter
Use of the Terms Physical and Chemical
Example 4.3 Correct Use of the Terms Physical and Chemical
Solution
4.5 Pure Substances and Mixtures
4.6 Heterogeneous and Homogeneous Mixtures
Use of the Terms Homogeneous and Heterogeneous
4.7 Elements and Compounds
Example 4.4 “Composition” Difference between a Mixture and a Compound
Solution
Example 4.5 Classifying Substances as Element, Compound, or Mixture
Solution
4.8 Discovery and Abundance of the Elements
4.9 Names and Chemical Symbols of the Elements
Example 4.6 Writing Correct Names for Elements
Solution
Example 4.7 Writing Correct Chemical Symbols for Elements
Solution
Concepts to Remember
Key Terms Listing
Practice Problems by Topic
Physical States of Matter (Sec. 4.2)
Properties of Matter (Sec. 4.3)
Changes In Matter (Sec. 4.4)
Pure Substances and Mixtures (SECS. 4.5 AND 4.6)
Elements and Compounds (Sec. 4.7)
Discovery and Abundance of the Elements (Sec. 4.8)
Names and Chemical Symbols of the Elements (Sec. 4.9)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 5 Atoms, Molecules, and Subatomic Particles
5.1 The Atom
5.2 The Molecule
Example 5.1 Classifying Molecules Based on Numbers of and Types of Atoms Present
Solution
Example 5.2 Classifying Matter Based on Molecular, Phase, and Substance Characteristics
Solution
5.3 Natural and Synthetic Compounds
5.4 Chemical Formulas
Example 5.3 Interpreting Chemical Formulas in Terms of Atoms and Elements Present
Solution
5.5 Subatomic Particles: Protons, Neutrons, and Electrons
Arrangement of Subatomic Particles Within an Atom
Charge Neutrality of an Atom
Size Relationships within an Atom
Additional Subatomic Particles
5.6 Atomic Number and Mass Number
Atomic Number
Mass Number
Subatomic Particle Makeup of an Atom
Example 5.4 Determining the Subatomic Makeup of an Atom Given Its Atomic Number and Mass Number
Solution
Example 5.5 Determining the Subatomic Makeup of an Atom Given Its Complete Chemical Symbol
Solution
5.7 Isotopes
Example 5.6 Identifying Characteristics of Isotopes of an Element
Solution
Example 5.7 Distinguishing between Isotopes and Isobars
Solution
5.8 Atomic Masses
Relative Mass
Example 5.8 Constructing a Relative Mass Scale
Solution
Average Atom
Weighted Averages
Example 5.9 Calculation of a Weighted Average
Solution
Example 5.10 Calculation of Atomic Mass from Isotopic Masses and Percent Abundances
Solution
Mass Spectrometry Experiments
5.9 Evidence Supporting the Existence and Arrangement of Subatomic Particles
Discharge Tube Experiments
Metal Foil Experiments
Concepts to Remember
Key Terms Listing
Practice Problems by Topic
Atoms and Molecules (SECS. 5.1 AND 5.2)
Chemical Formulas (Sec. 5.4)
Subatomic Particles (Sec. 5.5)
Atomic Number and Mass Number (Sec. 5.6)
Isotopes (Sec. 5.7)
Atomic Masses (Sec. 5.8)
Evidence Supporting the Existence and Arrangement of Subatomic Particles (Sec. 5.9)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 6 Electronic Structure and Chemical Periodicity
6.1 The Periodic Law
Student Learning Focus:
6.2 The Periodic Table
Student Learning Focus:
Periods and Groups of Elements
Example 6.1 Identifying Groups, Periods, and Specially Named Groups of Elements
Solution
The Shape of the Periodic Table
6.3 The Energy of an Electron
Student Learning Focus:
6.4 Electron Shells
Student Learning Focus:
6.5 Electron Subshells
Student Learning Focus:
6.6 Electron Orbitals
Student Learning Focus:
Example 6.2 Interrelationships among Electron Shells, Electron Subshells, and Electron Orbitals
Solution
Electron Spin
6.7 Electron Configurations
Student Learning Focus:
Aufbau Principle
Aufbau Diagram
Writing Electron Configurations
Example 6.3 Writing Electron Configurations for Elements
Solution
Answer Double Check:
Chemical Insight: SELENIUM
Condensed Electron Configurations
Example 6.4 Writing Condensed Electron Configurations
Solution
Answer Double Check:
Chemical Insight: IODINE
6.8 Electron Orbital Diagrams
Student Learning Focus:
Example 6.5 Writing Electron Orbital Diagrams for the Electrons in Atoms
Solution
Answer Double Check:
Chemical Insight: TITANIUM
6.9 Electron Configurations and the Periodic Law
Student Learning Focus:
6.10 Electron Configurations and the Periodic Table
Student Learning Focus:
Example 6.6 Using the Periodic Table as a Guide in Obtaining Information about Distinguishing Electrons
Solution
Chemical Insight: CALCIUM
Example 6.7 Using the Periodic Table as a Guide in Writing an Electron Configuration
Solution
Answer Double Check:
Chemical Insight: MERCURY
6.11 Classification Systems for the Elements
Student Learning Focus:
6.12 Chemical Periodicity
Student Learning Focus:
Metallic and Nonmetallic Character
Atomic Size
Example 6.8 Predicting Atomic Size Relationships, Using General Periodic Table Trends
Solution
Chemical Insight: NITROGEN INFLATION
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
Periodic Law and Periodic Table (SECS. 6.1 AND 6.2)
Terminology Associated With Electron Arrangements (SECS. 6.3–6.6)
Electron Configurations (Sec. 6.7)
Electron Orbital Diagrams (Sec. 6.8)
Electron Configurations and the Periodic Law (Sec. 6.9)
Electron Configurations and the Periodic Table (Sec. 6.10)
Classification Systems for the Elements (Sec. 6.11)
Chemical Periodicity (Sec. 6.12)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 7 Chemical Bonds
7.1 Types of Chemical Bonds
Student Learning Focus:
7.2 Valence Electrons and Lewis Symbols
Student Learning Focus:
Example 7.1 Determining the Number of Valence Electrons an Atom Possesses
Solution
Example 7.2 Writing Lewis Symbols for Elements
Solution
7.3 The Octet Rule
Student Learning Focus:
7.4 The Ionic Bond Model
Student Learning Focus:
Example 7.3 Writing Chemical Symbols for Ions
Solution
Answer Double Check:
Example 7.4 Determining the Number of Protons and Electrons in Ions
Solution
Answer Double Check:
7.5 The Sign and Magnitude of Ionic Charge
Student Learning Focus:
Example 7.5 Predicting Sign and Magnitude of Ionic Charge
Solution
Isoelectronic Species
7.6 Lewis Structures for Ionic Compounds
Student Learning Focus:
Example 7.6 Using Lewis Structures to Depict Ionic Compound Formation
Solution
Chemical Insight: Aluminum Oxide
7.7 Chemical Formulas for Ionic Compounds
Student Learning Focus:
Example 7.7 Using Ionic Charges to Determine the Chemical Formula of an Ionic Compound
Solution
Answer Double Check:
Chemical Insight: Magnesium Chloride
7.8 Structure of Ionic Compounds
Student Learning Focus:
7.9 Polyatomic Ions
Student Learning Focus:
Example 7.8 Writing Chemical Formulas for Ionic Compounds Containing Polyatomic Ions
Solution
Answer Double Check:
7.10 The Covalent Bond Model
Student Learning Focus:
7.11 Lewis Structures for Molecular Compounds
Student Learning Focus:
Example 7.9 Writing Lewis Structures for Simple Molecular Compounds
Solution
Chemical Insight: Phosphine
7.12 Single, Double, and Triple Covalent Bonds
Student Learning Focus:
7.13 Valence Electron Count and Number of Covalent Bonds Formed
Student Learning Focus:
Example 7.10 Predicting Chemical Formulas for Simple Molecular Compounds
Solution
7.14 Coordinate Covalent Bonds
Student Learning Focus:
7.15 Resonance Structures
Student Learning Focus:
7.16 Systematic Procedures for Drawing Lewis Structures
Student Learning Focus:
Example 7.11 Drawing a Lewis Structure for a Molecular Compound, Using Systematic Procedures
Solution
Answer Double Check:
Chemical Insight: Acid Rain
Example 7.12 Drawing a Lewis Structure for a Polyatomic Ion, Using Systematic Procedures
Solution
Answer Double Check:
Chemical Insight: Sodium Sulfite
Example 7.13 Drawing a Lewis Structure for a Molecule That Has Resonance Forms
Solution
Answer Double Check:
Chemical Insight: Ozone
7.17 Molecular Geometry
Student Learning Focus:
Electron Pairs versus Electron Groups
Molecules with Two VSEPR Electron Groups
Molecules with Three VSEPR Electron Groups
Molecules with Four VSEPR Electron Groups
Example 7.14 Using VSEPR Theory to Predict Molecular Geometry
Solution
Answer Double Check:
7.18 Electronegativity
Student Learning Focus:
Example 7.15 Predicting Electronegativity Relationships, Using General Periodic Table Trends
Solution
7.19 Bond Polarity
Student Learning Focus:
Example 7.16 Predicting the Polarity Characteristics of Chemical Bonds
Solution
7.20 Molecular Polarity
Student Learning Focus:
Example 7.17 Predicting the Polarity of Molecules Given Their Lewis Structure and Molecular Geometry
Solution
Chemical Insight: Hydrogen Sulfide
Concepts to Remember
Key Terms Listing
Practice Problems by Topic
Valence Electrons (Sec. 7.2)
Lewis Symbols for Atoms (Sec. 7.2)
Notation for Ions (Sec. 7.4)
The Sign and Magnitude of Ionic Charge (Sec. 7.5)
Lewis Structures for Ionic Compounds (Sec. 7.6)
Chemical Formulas for Ionic Compounds (Sec. 7.7)
Polyatomic-Ion-Containing Ionic Compounds (Sec. 7.9)
Lewis Structures for Covalent Compounds (SECS. 7.10–7.15)
Systematic Procedures for Drawing Lewis Structures (Sec. 7.16)
Molecular Geometry (Vsepr Theory) (Sec. 7.17)
Electronegativity (Sec. 7.18)
Bond Polarity (Sec. 7.19)
Molecular Polarity (Sec. 7.20)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 8 Chemical Nomenclature
8.1 Classification of Compounds for Nomenclature Purposes
Student Learning Focus:
Example 8.1 Classifying Compounds for Nomenclature Purposes
Solution
8.2 Types of Binary Ionic Compounds
Student Learning Focus:
8.3 Nomenclature for Binary Ionic Compounds
Student Learning Focus:
Fixed-Charge Binary Ionic Compounds
Example 8.2 Naming Fixed-Charge Binary Ionic Compounds, Given Their Chemical Formulas
Solution
Answer Double Check:
Example 8.3 Writing Chemical Formulas for Fixed-Charge Binary Ionic Compounds, Given Their Names
Solution
Answer Double Check:
Variable-Charge Binary Ionic Compounds
Example 8.4 Naming Variable-Charge Binary Ionic Compounds, Given Their Chemical Formulas
Solution
Answer Double Check:
Example 8.5 Writing Chemical Formulas for Variable-Charge Binary Ionic Compounds, Given Their Names
Solution
Example 8.6 Naming Variable-Charge Binary Ionic Compounds Using the -ic, -ous System for denoting metal Ion charge
Solution
8.4 Chemical Formulas for Polyatomic Ions
Student Learning Focus:
8.5 Nomenclature for Ionic Compounds Containing Polyatomic Ions
Student Learning Focus:
Example 8.7 Naming Polyatomic-Ion-Containing Compounds, Given Their Chemical Formulas
Solution
Answer Double Check:
Example 8.8 Writing Chemical Formulas for Polyatomic-Ion-Containing Compounds, Given Their Names
Solution
Answer Double Check:
8.6 Nomenclature for Binary Molecular Compounds
Student Learning Focus:
Example 8.9 Determining the Correct Order of Elemental Symbols in the Chemical Formula of a Binary Molecular Compound
Solution
Example 8.10 Naming Binary Molecular Compounds, Given Their Chemical Formulas
Solution
Common Names for Binary Molecular Compounds
8.7 Nomenclature for Acids
Student Learning Focus:
Example 8.11 Naming Hydrogen-Containing Compounds as Acids, Given Their Chemical Formulas
Solution
Answer Double Check:
Example 8.12 Writing Chemical Formulas for Acids, Given Their Names
Solution
8.8 Systematic Procedures for Using Nomenclature Rules
Student Learning Focus:
Example 8.13 Naming Compounds Given Their Chemical Formulas Using Systematic Procedures to Decide Which Nomenclature Rules Apply
Solution
Example 8.14 Writing Chemical Formulas for Compounds Given Their Names Using Systematic Procedures to Decide Which Nomenclature Rules Govern Each Situation
Solution
Concepts to Remember
Key Terms Listing
Practice Problems by Topic
Nomenclature Classifications for Compounds (Sec. 8.1)
Types of Binary Ionic Compounds (Sec. 8.2)
Nomenclature for Binary Ionic Compounds (Sec. 8.3)
Chemical Formulas for Polyatomic Ions (Sec. 8.4)
Nomenclature for Polyatomic-Ion-Containing Compounds (Sec. 8.5)
Nomenclature for Binary Molecular Compounds (Sec. 8.6)
Nomenclature for Acids (Sec. 8.7)
Systemic Procedures for Using Nomenclature Rules (Sec. 8.8)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 9 Chemical Calculations: The Mole Concept and Chemical Formulas
9.1 The Law of Definite Proportions
Student Learning Focus:
Example 9.1 Using Decomposition Data to Illustrate the Law of Definite Proportions
Solution
Chemical Insight: AMMONIA
9.2 Calculation of Formula Masses
Student Learning Focus:
Example 9.2 Using Chemical Formulas and Atomic Masses to Calculate Formula Masses
Solution
Chemical Insight: Ferric Oxide
9.3 Significant Figures and Formula Mass
Student Learning Focus:
Example 9.3 Treating Formula Mass Calculations as Addition Problems
Solution
Answer Double Check:
9.4 Mass Percent Composition of a Compound
Student Learning Focus:
Example 9.4 Using a Compound’s Chemical Formula to Calculate Its Percent by Mass Composition
Solution
Answer Double Check:
Chemical Insight: Acetaminophen
Example 9.5 Using Synthesis Data to Calculate Percent by Mass Composition
Solution
Answer Double Check:
Chemical Insight: Adrenaline
9.5 The Mole: The Chemist’s Counting Unit
Student Learning Focus:
Example 9.6 Calculating the Number of Objects in a Molar Quantity
Solution
Answer Double Check:
9.6 The Mass of a Mole
Student Learning Focus:
Example 9.7 Calculating the Mass, in Grams, of a Molar Quantity
Solution
Answer Double Check:
Summary of Mass Terminology
Example 9.8 Calculating Molar Mass from Mass and Mole Data
Solution
Chemical Insight: Nitric Oxide
9.7 Significant Figures and Avogadro’s Number
Student Learning Focus:
9.8 Relationship Between Atomic Mass Units and Gram Units
Student Learning Focus:
Example 9.9 Using the Relationship between Grams and Atomic Mass Units as a Conversion Factor
Solution
9.9 The Mole and Chemical Formulas
Student Learning Focus:
Example 9.10 Calculating Molar Quantities of Compound Components
Solution
Answer Double Check:
Chemical Insight: Menthol
9.10 The Mole and Chemical Calculations
Student Learning Focus:
Example 9.11 Calculating the Number of Particles in a Given Mass of Substance
Solution
Answer Double Check:
Chemical Insight: Nicotine
Example 9.12 Calculating the Mass of a Given Number of Particles of a Substance
Solution
Answer Double Check:
Chemical Insight: Nitrogen Dioxide
Example 9.13 Calculating the Mass of a Single Atom or a Single Molecule
Solution
Answer Double Check:
Example 9.14 Calculating the Mass of an Element Present in a Given Mass of Compound
Solution
Answer Double Check:
Chemical Insight: Caffeine
Example 9.15 Calculating the Number of Atoms of an Element Present in a Given Mass of a Compound
Solution
Chemical Insight: Cholesterol
9.11 Purity of Samples
Student Learning Focus:
Example 9.16 Calculating Masses of Substances in an Impure Sample
Solution
Answer Double Check:
Chemical Insight: Nitric Acid
Example 9.17 Calculating Atoms of a Substance in an Impure Sample
Solution
Answer Double Check:
Chemical Insight: Steel
9.12 Empirical and Molecular Formulas
Student Learning Focus:
Example 9.18 Obtaining Empirical Formulas from Molecular Formulas
Solution
Answer Double Check:
9.13 Determination of Empirical Formulas
Student Learning Focus:
Empirical Formulas from Direct Analysis Data
Example 9.19 Determining an Empirical Formula from Percent by Mass Composition Data
Solution
Chemical Insight: Chlorofluorocarbons
Example 9.20 Determining an Empirical Formula Using Mass Data
Solution
Answer Double Check:
Chemical Insight: Ibuprofen and Naproxen
Empirical Formulas from Indirect Analysis Data
Example 9.21 Determining an Empirical Formula Using Combustion Analysis Data
Solution
Chemical Insight: Ethylene
Example 9.22 Determining an Empirical Formula Using Combustion Analysis Data
Solution
Answer Double Check:
Chemical Insight: Acetone
9.14 Determination of Molecular Formulas
Student Learning Focus:
Example 9.23 Calculating a Molecular Formula from an Empirical Formula and Molecular Formula Mass Data
Solution
Answer Double Check:
Example 9.24 Calculating a Molecular Formula from Mass Percent Composition and Molecular Formula Mass Data
Solution
Chemical Insight: Natural Gas
Concepts to Remember
Key Terms Listing
Practice Problems by Topic
Law of Definite Proportions (Sec. 9.1)
Formula Masses (Secs. 9.2 and 9.3)
Mass Percent Composition (Sec. 9.4)
The Mole: The Chemist’s Counting Unit (Sec. 9.5)
Molar Mass (Sec. 9.6)
Relationship Between Atomic Mass Units and Gram Units (Sec. 9.8)
The Mole and Chemical Formulas (Sec. 9.9)
The Mole and Chemical Calculations (Sec. 9.10)
Purity of Samples (Sec. 9.11)
Determination of Empirical Formulas (Secs. 9.13 and 9.14)
Empirical Formula Determination Using Combustion Analysis (Sec. 9.13)
Determination of Molecular Formulas (Sec. 9.14)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 10 Chemical Calculations Involving Chemical Equations
10.1 The Law of Conservation of Mass
10.2 Writing Chemical Equations
10.3 Chemical Equation Coefficients
Example 10.1 Using Both Equation Coefficients and Chemical Formulas to Determine Number of Atoms Present
Solution
10.4 Balancing Procedures for Chemical Equations
Example 10.2 Balancing a Chemical Equation
Solution
Example 10.3 Balancing a Chemical Equation
Solution
Example 10.4 Deriving a Balanced Chemical Equation from Molecular Models of Reactants and Products
Solution
10.5 Special Symbols Used in Chemical Equations
10.6 Classes of Chemical Reactions
Synthesis Reactions
Decomposition Reactions
Single-Replacement Reactions
Double-Replacement Reactions
Example 10.5 Classification of Chemical Reactions into the Categories Synthesis, Decomposition, Single-Replacement, and Double-Replacement
Solution
Combustion Reactions
Example 10.6 Writing and Balancing an Equation for a Combustion Reaction
Solution
10.7 Chemical Equations and the Mole Concept
Example 10.7 Calculating Molar Quantities Using a Balanced Chemical Equation
Solution
10.8 Balanced Chemical Equations and the Law of Conservation of Mass
Example 10.8 Verifying the Law of Conservation of Mass Using a Balanced Chemical Equation
Solution
10.9 Calculations Based on Chemical Equations’Stoichiometry
Example 10.9 Calculating the Needed Mass of a Reactant in a Chemical Reaction
Solution
Example 10.10 Calculating the Mass of a Product in a Chemical Reaction
Solution
Example 10.11 Calculating Moles of Product Produced in a Chemical Reaction
Solution
Example 10.12 Calculating the Amount of a Substance Produced in a Chemical Reaction
Solution
10.10 The Limiting Reactant Concept
Example 10.13 Determining a Limiting Reactant in a Nonchemical Context
Solution
Example 10.14 Determining the Limiting Reactant from Given Reactant Amounts
Solution
Example 10.15 Calculating the Mass of Product from Masses of Reactants
Solution
10.11 Yields: Theoretical, Actual, and Percent
Example 10.16 Calculating the Theoretical Yield and Percent Yield for a Chemical Reaction
Solution
10.12 Simultaneous and Sequential Chemical Reactions
Example 10.17 A Calculation Based on Simultaneous Chemical Reactions
Solution
Example 10.18 A Calculation Based on Sequential Chemical Reactions
Solution
Combining Sequential Chemical Reaction Equations into a Single Overall Chemical Reaction Equation
Example 10.19 Combining Sequential Chemical Equations to Produce a Single Overall Chemical Equation
Solution
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
The Law of Conservation of Mass (Sec. 10.1)
Chemical Equation Notation (Secs. 10.2 and 10.5)
Balancing Chemical Equations (Sec. 10.4)
Classes of Chemical Reactions (Sec. 10.6)
Chemical Equations and The Mole Concept (Sec. 10.7)
Balanced Chemical Equations and The Law of Conservation of Mass (Sec. 10.8)
Calculations Based on Chemical Equations (Sec. 10.9)
Limiting Reactant Calculations (Sec. 10.10)
Theoretical Yield and Percent Yield (Sec. 10.11)
Simultaneous Chemical Reactions (Sec. 10.12)
Sequential Chemical Reactions (Sec. 10.12)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 11 States of Matter
11.1 Factors that Determine Physical State
Student Learning Focus:
11.2 Property Differences among Physical States
Student Learning Focus:
11.3 The Kinetic Molecular Theory of Matter
Student Learning Focus:
11.4 The Solid State
Student Learning Focus:
11.5 The Liquid State
Student Learning Focus:
11.6 The Gaseous State
Student Learning Focus:
11.7 A Comparison of Solids, Liquids, and Gases
Student Learning Focus:
11.8 Endothermic and Exothermic Changes of State
Student Learning Focus:
11.9 Heat Energy and Specific Heat
Student Learning Focus:
Heat Energy Units
Example 11.1 Interrelationships among Heat Energy Units
Solution
Answer Double Check:
Chemical Insight: Ethyl Alcohol
Specific Heat
Example 11.2 Calculating the Amount of Heat Energy Absorbed by a Substance Undergoing a Specific Temperature Increase
Solution
Answer Double Check:
Chemical Insights: Beryllium
Example 11.3 Calculating the Temperature Change Caused by Addition of a Specific Amount of Heat Energy
Solution
Answer Double Check:
Example 11.4 Using Heat Capacity Data to Calculate Specific Heat
Solution
Answer Double Check:
Chemical Insight: Gold
Example 11.5 Calculation Involving “Heat Lost Is Equal to Heat Gained.”
Solution
Answer Double Check:
11.10 Temperature Changes as a Substance is Heated
Student Learning Focus:
11.11 Energy and Changes of State
Student Learning Focus:
Example 11.6 Calculating the Heat Energy Absorbed as a Substance Melts
Solution
Chemical Insight: Copper
Example 11.7 Calculating the Heat of Vaporization from Given Thermochemical Data
Solution
Answer Double Check:
11.12 Heat Energy Calculations
Student Learning Focus:
Example 11.8 Thermochemical Calculation Involving Both Change of State and Change of Temperature
Solution
Answer Double Check:
Example 11.9 Thermochemical Calculation Involving All Three States of Matter
Solution
Answer Double Check:
11.13 Evaporation of Liquids
Student Learning Focus:
Rate of Evaporation and Temperature
Evaporation and Equilibrium
11.14 Vapor Pressure of Liquids
Student Learning Focus:
11.15 Boiling and Boiling Points
Student Learning Focus:
Factors that Affect Boiling Point
11.16 Intermolecular Forces in Liquids
Student Learning Focus:
Dipole–Dipole Interactions
Hydrogen Bonds
Example 11.10 Predicting Whether Molecules Can Participate in Hydrogen Bonding
Solution
London Forces
Ion–Dipole Interactions
Ion–Ion Interactions
11.17 Hydrogen Bonding and The Properties of Water
Student Learning Focus:
Vapor Pressure
Thermal Properties
Density
Surface Tension
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
Physical States of Matter (Secs. 11.1 and 11.2)
Kinetic Molecular Theory of Matter (Secs. 11.3–11.6)
Physical Changes of State (Sec. 11.8)
Heat Energy and Specific Heat (Sec. 11.9)
Energy and Changes of State (Sec. 11.11)
Heat Energy Calculations (Sec. 11.12)
Properties of Liquids (Secs. 11.13–11.15)
Intermolecular Forces in Liquids (Sec. 11.16)
Hydrogen Bonding and The Properties of Water (Sec 11.17)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 12 Gas Laws
12.1 Properties of Some Common Gases
Student Learning Focus:
12.2 Gas Law Variables
Student Learning Focus:
Example 12.1 Interconverting between Various Pressure Units
Solution
Answer Double Check:
Pressure Readings and Significant Figures
12.3 Boyle’s Law: A Pressure–Volume Relationship
Student Learning Focus:
Example 12.2 Calculating Final Volume of a Gas Using Boyle’s Law with Pressure Values Given in the Same Units
Solution
Answer Double Check:
Example 12.3 Calculating Final Volume of a Gas Using Boyle’s Law with Pressure Values Given in Different Units
Solution
Answer Double Check:
12.4 Charles’s Law: A Temperature–Volume Relationship
Student Learning Focus:
Example 12.4 Calculating Final Volume of a Gas Using Charles’s Law
Solution
Answer Double Check:
12.5 Gay-Lussac’s Law: A Temperature–Pressure Relationship
Student Learning Focus:
Example 12.5 Calculating Final Temperature of a Gas Using Gay-Lussac’s Law
Solution
Answer Double Check:
12.6 The Combined Gas Law
Student Learning Focus:
Example 12.6 Mathematical Manipulation of the Combined Gas Law
Solution
Example 12.7 Calculating Final Volume of a Gas Using the Combined Gas Law
Solution
Answer Double Check:
Chemical Insight: Hydrogen
Example 12.8 Calculating Final Temperature of a Gas Using the Combined Gas Law
Solution
Answer Double Check:
Chemical Insight: Helium
12.7 Avogadro’s Law
Student Learning Focus:
Example 12.9 Calculating Final Volume of a Gas Using Avogadro’s Law
Solution
Answer Double Check:
Chemical Insight: Helium
Example 12.10 Calculating Final Volume of a Gas When None of the Other Gas Law Variables Are Constant
Solution
Answer Double Check:
Chemical Insight: Nitrogen
12.8 An Ideal Gas
Student Learning Focus:
12.9 The Ideal Gas Law
Student Learning Focus:
Example 12.11 Calculating the Volume of a Gas Using the Ideal Gas Law
Solution
Answer Double Check:
Chemical Insight: Carbon Monoxide
Example 12.12 Calculating the Temperature of a Gas Using the Ideal Gas Law
Solution
Answer Double Check:
Chemical Insight: Nitrous Oxide
12.10 Modified Forms of the Ideal Gas Law Equation
Student Learning Focus:
The Molar Mass of a Gas
Example 12.13 Calculating the Molar Mass of a Gas Using the Ideal Gas Law in Modified Form
Solution
Answer Double Check:
Chemical Insight: Chlorine
The Density of a Gas
Example 12.14 Calculating the Density of a Gas Using the Ideal Gas Law in Modified Form
Solution
Using Density to Calculate Molar Mass
Example 12.15 Calculating the Molar Mass of a Gas Given Its Density
Solution
Answer Double Check:
12.11 Volumes of Gases in Chemical Reactions
Student Learning Focus:
Example 12.16 Using Gay-Lussac’s Law of Combining Volumes to Determine Reactant–Product Volume Relationships
Solution
Answer Double Check:
Chemical Insight: Ammonia
12.12 Volumes of Gases and The Limiting Reactant Concept
Student Learning Focus:
Example 12.17 Calculating a Limiting Reactant Using Volumes of Gases
Solution
Answer Double Check:
Chemical Insight: AcetylenE
12.13 Molar Volume of a Gas
Student Learning Focus:
Example 12.18 Calculating the Molar Volume of a Gas
Solution
Answer Double Check:
Example 12.19 Calculating the Molar Volume of a Gas
Solution
Answer Double Check:
Standard Temperature and Standard Pressure Conditions
Using Molar Volume to Calculate Density
Example 12.20 Calculating Density Using Molar Volume and Molar Mass
Solution
Chemical Insight: Hyrdogen Cyanide
12.14 Chemical Calculations Using Molar Volume
Student Learning Focus:
Example 12.21 Calculating the Volume of a Gas at STP Given Its Mass
Solution
Answer Double Check:
Chemical Insight: FlUOrine
Example 12.22 Calculating the Mass of a Gas Given Its Volume
Solution
Answer Double Check:
Example 12.23 Calculating the STP Volume of a Gaseous Reactant in a Chemical Reaction
Solution
Answer Double Check:
Chemical Insight: Lithium
Example 12.24 Calculating the Mass of a Reactant from the Volume of a Gaseous Product
Solution
Chemical Insight: Oxygen
Example 12.25 Calculating Gaseous Product Volume from Gaseous Reactant Volumes
Solution
Chemical Insight: Nitrogen
12.15 Mixtures of Gases
Student Learning Focus:
Example 12.26 Applying the Ideal Gas Law to a Mixture of Gases
Solution
Answer Double Check:
12.16 Dalton’s Law of Partial Pressures
Student Learning Focus:
Example 12.27 Using Dalton’s Law to Calculate a Partial Pressure
Solution
Example 12.28 Calculating the Mole Fraction for a Gas in a Gaseous Mixture
Solution
Answer Double Check:
Example 12.29 Calculating Partial Pressures Using Mole Fractions
Solution
Answer Double Check:
Example 12.30 Calculating the Partial Pressure of a Gas Using the Ideal Gas Law
Solution
Answer Double Check:
Example 12.31 Calculating the Partial Pressure of a Gas Collected over Water
Solution
Example 12.32 Expressing Gaseous Mixture Composition in Mole Percent, Pressure Percent, and Volume Percent
Solution
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
Measurement of Pressure (Sec. 12.2)
Boyle’s Law (Sec. 12.3)
Charles’s Law (Sec. 12.4)
Gay-Lussac’s Law (Sec. 12.5)
The Combined Gas Law (Sec. 12.6)
Avogadro’s Law (Sec. 12.7)
The Ideal Gas Law (Sec. 12.9)
Modified Forms of the Ideal Gas Law Equation (Sec. 12.10)
Volumes of Gases in Chemical Reactions (Sec. 12.11)
Volumes of Gases and The Limiting Reactant Concept (Sec. 12.12)
Molar Volume of a Gas (Sec. 12.13)
Chemical Calculations Using Molar Volume (Sec. 12.14)
Mixtures of Gases (Sec. 12.15)
Dalton’s Law of Partial Pressures (Sec. 12.16)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 13 Solutions
13.1 Characteristics of Solutions
Student Learning Focus:
13.2 Solubility
Student Learning Focus:
Effect of Temperature on Solubility
Effect of Pressure on Solubility
Terminology for Relative Amount of Solute in a Solution
Aqueous and Nonaqueous Solutions
13.3 Solution Formation
Student Learning Focus:
Factors Affecting the Rate of Solution Formation
13.4 Solubility Rules
Student Learning Focus:
Example 13.1 Using Solubility Guidelines to Predict Compound Solubilities
Solution
13.5 Solution Concentrations
Student Learning Focus:
13.6 Percentage Concentration Unit
Student Learning Focus:
Example 13.2 Calculating Mass Percent Concentration from Mass of Solute and Mass of Solvent
Solution
Answer Double Check:
Chemical Insight: Sucrose
Example 13.3 Calculating the Percent by Volume Concentration of a Solution
Solution
Answer Double Check:
Chemical Insight: Methyl Alcohol
Using Percent Concentrations as Conversion Factors
Example 13.4 Calculating the Mass of Solute Necessary to Produce a Solution of a Given Mass Percent Concentration
Solution
Answer Double Check:
Chemical Insight: Iodine
Example 13.5 Calculating the Mass of Solute Present in a Solution of a Given Mass–Volume Percent Concentration
Solution
Answer Double Check:
Chemical Insight: Vinegar
Example 13.6 Calculating the Volume of Solution Necessary to Supply a Given Mass of Solute Using Density and Mass Percent Concentration
Solution
Answer Double Check:
13.7 Parts Per Million and Parts Per Billion Concentration Units
Student Learning Focus:
Example 13.7 Expressing Concentrations in Parts per Million and Parts per Billion
Solution
Answer Double Check:
Chemical Insight: Fluoridation
Example 13.8 Calculating the Volume of Solute Present Given a Parts per Million Concentration
Solution
Chemical Insight: Carbon Monoxide
13.8 Molarity Concentration Unit
Student Learning Focus:
Example 13.9 Calculating the Molarity of a Solution from Mass/Amount and Volume Data
Solution
Answer Double Check:
Using Molarity as a Conversion Factor
Example 13.10 Calculating the Amount of Solute Present in a Given Amount of Solution Using Molarity as a Conversion Factor
Solution
Answer Double Check:
Chemical Insight: Citric Acid
Example 13.11 Calculating the Amount of Solution Necessary to Supply a Given Amount of Solute
Solution
Chemical Insight: Iron
Example 13.12 Calculating Molarity from Density and Percent by Mass
Solution
Example 13.13 Using Molarity and Density to Calculate the Amount of Solvent Present in a Solution
Solution
Answer Double Check:
Chemical Insight: Sulfuric Acid
13.9 Molarity and Chemical Reactions in Aqueous Solution
Student Learning Focus:
Example 13.14 Calculating the Volume of a Reactant Given the Volume and Concentration of Another Reactant
Solution
Answer Double Check:
Example 13.15 Calculating the Volume of a Solution of Known Concentration Needed to React With a Known Mass of Another Reactant
Solution
Answer Double Check:
Example 13.16 Calculating a Product Amount Given Two Reactant Solution Volumes
Solution
Answer Double Check:
Example 13.17 Calculating the Gaseous Volume of a Product from the Solution Volume of a Reactant
Solution
13.10 Dilution Calculations
Student Learning Focus:
Example 13.18 Calculating the Molarity of a Solution After It Has Been Diluted
Solution
Answer Double Check:
Chemical Insight: Nitric Acid
Example 13.19 Calculating the Amount of Solvent That Must Be Added to a Solution to Dilute It to a Specified Concentration
Solution
Answer Double Check:
Example 13.20 Calculating Molarity when Two Like Solutions of Differing Concentration Are Mixed
Solution
Answer Double Check:
Chemical Insight: Hydrochloric Acid
13.11 Molality Concentration Unit
Student Learning Focus:
Example 13.21 Calculating the Molality of a Solution
Solution
Answer Double Check:
Chemical Insight: Common Salt
Example 13.22 Calculating the Amount of Solute Needed to Prepare a Solution of Specified Molality
Solution
Answer Double Check:
Chemical Insight: Isopropyl Alcohol
Example 13.23 Calculating Molarity from Molality and Density
Solution
Answer Double Check:
Example 13.24 Calculating Molality from Molarity and Density
Solution
Answer Double Check:
Chemical Insight: Lactose
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
Characteristics of Solutions (Sec. 13.1)
Solubility (Sec. 13.2)
Solution Formation (Sec. 13.3)
Solubility Rules (Sec. 13.4)
Mass Percent (Sec. 13.6)
Volume Percent (Sec. 13.6)
Mass–Volume Percent (Sec. 13.6)
Parts Per Million and Parts Per Billion (Sec. 13.7)
Molarity (Sec. 13.8)
Molarity and Chemical Equations (Sec. 13.9)
Dilution (Sec. 13.10)
Molality (sec 13.11)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 14 Acids, Bases, and Salts
14.1 Arrhenius Acid–Base Theory
Student Learning Focus:
14.2 Brønsted–Lowry Acid–Base Theory
Student Learning Focus:
14.3 Conjugate Acids and Bases
Student Learning Focus:
Example 14.1 Determining the Members of a Conjugate Acid–Base Pair
Solution
Answer Double Check:
Example 14.2 Determining the Formula of One Member of a Conjugate Acid–Base Pair when Given the Other Member
Solution
Answer Double Check:
Amphiprotic Substances
14.4 Mono-, Di-, and Triprotic Acids
Student Learning Focus:
14.5 Strengths of Acids and Bases
Student Learning Focus:
14.6 SALTS
Student Learning Focus:
14.7 Reactions of Acids
Student Learning Focus:
Reaction with Metals
Reaction with Bases
Reaction with Carbonates and Bicarbonates
14.8 Reactions of Bases
Student Learning Focus:
14.9 Reactions of Salts
Student Learning Focus:
Reaction with Metals
Reaction with Acids
Reaction with Bases
Reaction of Salts with Each Other
Example 14.3 Predicting Whether a Reaction Will Occur and Writing an Equation for the Reaction If It Does Occur
Solution
Answer Double Check:
14.10 Self-Ionization of Water
Student Learning Focus:
Ion Product Constant for Water
Effect of Solutes on Water Self-Ionization
Example 14.4 Calculating the Hydroxide Ion Concentration of a Solution with a Known Hydronium Ion Concentration
Solution
Answer Double Check:
Effect of Temperature Change on Water Self-Ionization
Acidic, Basic, and Neutral Solutions
14.11 The pH Scale
Integral pH Values
Example 14.5 Calculating the pH of a Solution when Given Its Hydronium Ion or Hydroxide Ion Concentration
Solution
Nonintegral pH Values
Example 14.6 Calculating the pH of a Solution Given Its Hydronium Ion Concentration
Solution
Answer Double Check:
Example 14.7 Calculating the Molar Hydronium Ion Concentration of a Solution from the Solution’s pH
Solution
Answer Double Check:
14.12 Hydrolysis of Salts
Student Learning Focus:
Types of Salt Hydrolysis
Example 14.8 Predicting Whether a Salt’s Aqueous Solution Will Be Acidic, Basic, or Neutral
Solution
Chemical Equations for Salt Hydrolysis Reactions
Example 14.9 Writing Chemical Equations for Hydrolysis Reactions
Solution
14.13 Buffers
Student Learning Focus:
Example 14.10 Recognizing Pairs of Chemical Substances that Can Function as a Buffer in an Aqueous Solution
Solution
Answer Double Check:
Chemical Equations for Buffer Action
Example 14.11 Writing Equations for Reactions that Occur in a Buffered Solution
Solution
Answer Double Check:
14.14 Acid–Base Titrations
Student Learning Focus:
Example 14.12 Calculating an Unknown Molarity, Using Acid–Base Titration Data
Solution
Answer Double Check:
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
Acid–Base Definitions (Secs. 14.1 and 14.2)
Conjugate Acids and Bases (Sec. 14.3)
Mono-, Di-, and Triprotic Acids (Sec. 14.4)
Strength of Acids and Bases (Sec. 14.5)
Salts (Sec. 14.6)
Reactions of Acids and Bases (Secs. 14.7 and 14.8)
Reactions of Salts (Sec. 14.9)
Hydronium Ion and Hydroxide Ion Concentrations (Sec. 14.10)
The pH Scale (Sec. 14.11)
Hydrolysis of Salts (Sec. 14.12)
Buffers (Sec. 14.13)
Acid–Base Titrations (Sec. 14.14)
Multi-Concept Problems
Multiple Choice Practice Test
Chapter 15 Chemical Equations: Net Ionic and Oxidation–Reduction
15.1 Types of Chemical Equations
Student Learning Focus:
15.2 Electrolytes
Student Learning Focus:
15.3 Ionic and Net Ionic Equations
Student Learning Focus:
Example 15.1 Converting a Molecular Equation into a Net Ionic Equation
Solution
Answer Double Check:
Example 15.2 Converting a Molecular Equation into a Net Ionic Equation
Solution
Answer Double Check:
Example 15.3 Converting a Molecular Equation into a Net Ionic Equation
Solution
Answer Double Check:
15.4 Oxidation–Reduction Terminology
Student Learning Focus:
15.5 Oxidation Numbers
Student Learning Focus:
Example 15.4 Assigning Oxidation Numbers to Elements in a Compound or Polyatomic Ion
Solution
Answer Double Check:
Example 15.5 Determining Oxidation Numbers and Identifying Oxidizing Agents and Reducing Agents
Solution
Answer Double Check:
15.6 Redox and Nonredox Chemical Reactions
Student Learning Focus:
Example 15.6 Classifying Chemical Reactions as Redox or Nonredox
Solution
15.7 Balancing Oxidation–Reduction Equations
Student Learning Focus:
15.8 Oxidation Number Method for Balancing Redox Equations
Student Learning Focus:
Example 15.7 Balancing a Molecular Redox Equation Using the Oxidation Number Method
Solution
Answer Double Check:
Example 15.8 Balancing a Net Ionic Redox Equation Using the Oxidation Number Method
Solution
Answer Double Check:
Example 15.9 Balancing a Net Ionic Redox Equation Using the Oxidation Number Method
Solution
Answer Double Check:
15.9 Half-Reaction Method for Balancing Redox Equations
Student Learning Focus:
Example 15.10 Balancing a Net Ionic Redox Equation Using the Half-Reaction Method
Solution
Answer Double Check:
Example 15.11 Balancing a Net Ionic Redox Equation Using the Half-Reaction Method
Solution
Answer Double Check:
Example 15.12 Balancing a Net Ionic Redox Equation Using the Half-Reaction Method
Solution
Answer Double Check:
15.10 Disproportionation Reactions
Student Learning Focus:
Example 15.13 Balancing a Disproportionation Redox Equation
Solution
Answer Double Check:
15.11 Stoichiometric Calculations Involving Ions
Student Learning Focus:
Example 15.14 Calculating the Mass of an Ion Present in a Solution
Solution
Example 15.15 Calculating the Volume of Solution Needed to Supply a Given Amount of an Ion
Solution
Answer Double Check:
Example 15.16 Calculating the Volume of Solution Needed for a Reaction Involving Ions
Solution
Answer Double Check:
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
Electrolytes (Sec. 15.2)
Ionic and Net Ionic Equations (Sec. 15.3)
Oxidation–Reduction Terminology (Secs. 15.4 and 15.5)
Oxidation Numbers (Sec. 15.5)
Characteristics of Oxidation–Reduction Reactions (Sec. 15.5)
Redox and Nonredox Chemical Reactions (Sec. 15.6)
Balancing Redox Equations: Oxidation Number Method (Sec. 15.8)
Balancing Redox Equations: Half-Reaction Method (Sec. 15.9)
Balancing Redox Equations: Disproportionation Reactions (Sec. 15.10)
Stoichiometric Calculations Involving Ions (Sec 15.11)
Multi-Concept Problems
Multiple-Choice Practice Test
Chapter 16 Reaction Rates and Chemical Equilibrium
16.1 Collision Theory
Student Learning Focus:
Molecular Collisions
Activation Energy
Collision Orientation
16.2 Endothermic and Exothermic Chemical Reactions
Student Learning Focus:
16.3 Factors that Influence Chemical Reaction Rates
Student Learning Focus:
Physical Nature of Reactants
Reactant Concentration
Reaction Temperature
Presence of Catalysts
16.4 Chemical Equilibrium
Student Learning Focus:
16.5 Equilibrium Mixture Stoichiometry
Student Learning Focus:
Example 16.1 Determining the Composition of an Equilibrium Mixture in Terms of Moles of Each Substance Present
Solution
Answer Double Check:
16.6 Equilibrium Constants
Student Learning Focus:
Example 16.2 Using Balanced Chemical Equations to Determine Equilibrium Constant Expressions
Solution
Answer Double Check:
Example 16.3 Using Equilibrium Concentrations to Calculate the Value of an Equilibrium Constant
Solution
Answer Double Check:
16.7 Equilibrium Position
Student Learning Focus:
16.8 Temperature Dependency of Equilibrium Constants
Student Learning Focus:
16.9 Le Châtelier’s Principle
Student Learning Focus:
Concentration Changes
Henri-Louis Le Châtelier (1850–1936)
Temperature Changes
Pressure Changes
Addition of a Catalyst
Example 16.4 Using Le Châtelier’s Principle to Predict the Effects of Changes on the Equilibrium Position in an Equilibrium System
Solution
16.10 Forcing Chemical Reactions to Completion
Student Learning Focus:
Concepts to Remember
Key Terms Listing
Practice Problems By Topic
Collision Theory (Sec. 16.1)
Endothermic and Exothermic Chemical Reactions (Sec. 16.2)
Factors that Influence Chemical Reaction Rates (Sec. 16.3)
Chemical Equilibrium (Sec. 16.4)
Equilibrium Mixture Stoichiometry (Sec. 16.5)
Equilibrium Constants (Sec. 16.6)
Le Châtelier’s Principle (Sec. 16.9)
Multi-Concept Problems
Multiple Choice Practice Test
Glossary
Answers to Odd-Numbered Practice Problems
Credits
Index
A
B
C
D
E
F
G
H
I
J
K
L
M
N
O
P
Q
R
S
T
U
V
W
Y

Solutions Manual to accompany Introduction to Chemical Principles 11th 0321814630 / 9780321814630

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