Benjamin Cummings / Prentice Hall
Chemistry
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ISBN-10: 0131000659
ISBN-13: 9780131000650
Publisher: Prentice Hall
Copyright: 2008
Format: Cloth; 1232 pp
Temporarily out of stock
Suggested retail price: $186.80
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For two-semester or three-quarter courses in General Chemistry.
Tro provides students the support they need early so they can tackle challenging topics later. He does this by building on what students already know.
The author’s goal in writing this book is to deliver the depth of coverage faculty want with the accessibility and clarity that students need for success. Nivaldo J. Tro’s Chemistry: A Molecular Approach explains difficult chemical concepts in a concise and clear student-centered manner while also providing faculty with the flexibility to go more deeply into many key, often neglected topics, such as electron diffraction, molecular orbital theory, and free-energy changes under non-standard conditions. Chemistry is presented visually throughmulti-level images (macroscopic, molecular and symbolic representations), which helps students see the connections among the formulas (symbolic), the world around them (macroscopic), and the atoms and molecules that make up the world (molecular). Every aspect of this book focuses students on recognizing that the behavior of matter is based on the behavior of atoms and molecules.
Do you wish your current text was better at helping you motivate your students?
Tro’s Student -Oriented text encourages readers to see the relevance of chemistry as it applies to their everyday lives.
- Tro shows students why chemistry is important to them, to their future careers, and to their world. When discussing the composition of compounds (p. 103) Tro references chlorofluorocarbons (CFCs) and their impact on the earth’s ozone layer. The deterioration of the ozone layer is put into a relevant context for students, explaining why CFCs are dangerous to our environment while applying this example to the explanation of mass percent composition.
- Tro’s relevant examples and applications help students connect chemistry with their lives. Various chemical topics are discussed throughout the text such as Chemistry in the Environment (p. 100) which emphasize the chemical impact of acid rain on the environment or the legislation requiring the gasoline additive MTBE (p. 143). Other interest topics include Chemistry in Medicine, Chemistry in Your Day, and the Nature of Chemistry, all of which highlight current issues facing chemists and citizens. Tro applies these issues to chemical concepts and puts into context the chemistry students study and how chemistry impacts the world.
How do you approach developing problem solving skills?
Tro’s goal in writing a Pedagogically Driven text is to provide a consistent framework for problem solving that encourages students to think logically through the problem- solving process rather than memorizing formulas.
- Tro provides a structured, consistent, and visual problem - solving methodology because he understands that a main goal of general chemistry is to teach students how to solve problems.
- Tro’s four -step Sort, Strategize, Solve, and Check approach helps students relate the concept of the problem to the solution through an explicit conceptual plan for each problem. This method helps students understand where to start when given a problem and to think through solving the problem rather than simply formula hunting based on the given information (pp. 102-103, 104-105, 106, 108, 111, 141, 142, 145).
- Two- and three -column example formats help students to understand the logic and purpose of each step in the problem-solving process as well as the details of its implementation. Tro’s procedure maps not only work out a problem for students, but also apply the same methodology to another problem side by side (pp. 93, 110, 113, 115-116, 158-159).
- Why are some examples covered in 1-column rather than 2-columns? The answer is that some topics can be covered with just one example (with the explanation in the left column and the worked out example in the right column), while other topics are best covered by having two side-by-side examples (with the explanation in the left column and the two side-by-side examples in the center and right column). For example, turn to page 643 and look at examples 14.12 and 14.13. The two examples are nearly identical with one exception: the initial concentration of the reactant. The different initial concentrations make the x is small approximation work in one case, but not the other. By having the two examples side-by-side, students can easily see the differences and begin to learn when the x is small approximation is appropriate.
How adept are your students at connecting the macro world to the molecular world to the symbolic representation?
Multipart images include the Symbolic, Macroscopic, and Molecular perspectives that are fundamental to visualizing and understanding chemistry.
- Tro’s multipart images help students to see the relationship between the formulas they write down on paper (symbolic), the world they see around them (macroscopic), and the atoms and molecules that compose that world (molecular). The image of The Formation of an Ionic Compound (p. 85) displays the molecular interaction between sodium and chlorine on the molecular, symbolic and macro levels. The explanation of molecular models better describes the different ways chemistry is communicated (p. 87).
- Tro’s abundant molecular-level views show students the connection between everyday processes visible to the eye and what atoms and molecules are doing.
- Tro’s illustrations include extensive labels and annotations to guide students’ attention to key elements in the art and help them to understand the processes depicted. (Common Hydrocarbons Table 3.7 page 119)
Do your students perceive chemistry as a quantitative, rather than a conceptual, science?
Understanding chemistry as it applies in the Big Picture enables students to see the relevance of chemistry concepts in the world around them.
- Tro realizes students need to understand the material conceptually along with being able to solve problems symbolically/mathematically.
- The opening section of each chapter introduces many of its main themes through a compelling situation or example of real-world importance.
- Each chapter includes several Conceptual Connections, in which students are asked to think about concepts and solve problems without doing any math.
Do you find yourself compromising between the chemistry you would like to teach and the chemistry your students could understand?
Tro emphasizes the Rigorous treatment of numerous topics in appropriate depth while ensuring that students are able to understand these challenging topics.
- Presents topics in such a way that is both chemically thorough and understandable for students.
- Derivation of ideal gas law from kinetic molecular theory
- Electron diffraction and the photoelectric effect
- Molecular orbital theory
- Non-Ideal Solutions
- Collision theory and reactions rates
- Simplifying assumptions in equilibrium calculations
- Free energy changes for non-standard states
- Stoichiometry is a challenging first- semester topic. In chapter 4 (p. 133 and p. 137) Tro likens reaction stoichiometry to a cooking recipe. He explains how making pizza with various ingredients is analogous to the concept of stoichiometry. This example is used to further discuss the limiting reactant, theoretical yield, and percent yield. Clear and understandable, this and other fundamental topics are put into the context of life and relevantly applied through example problems and conceptual connections.
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When you aren’t with your students, what tools do they use to study?
MasteringChemistry steps students through problem solving while promoting understanding of chemical concepts outside of the classroom.
- Backed by NSF funding, this online homework, assessment, and tutorial system helps students figure out where they are going wrong when problem solving by providing answer specific feedback.
- The program enables professors to compare their class performance against the national average on specific questions or topics. At a glance, professors can see class distribution of grades, time spent, most difficult problems, most difficult steps and even the most common answer.
Chapter 1
Matter, Measurement, and Problem Solving
1.1 Atoms and Molecules
1.2 The Scientific Approach to Knowledge
The Nature of Science: Thomas S. Kuhn and Scientific Revolutions
1.3 The Classification of Matter
The States of Matter: Solid, Liquid and Gas
Classifying Matter According to Its Composition: Elements, Compounds, and Mixtures
Separating Mixtures
1.4 Physical and Chemical Changes and Physical and Chemical Properties
1.5 Energy: A Fundamental Part of Physical and Chemical Change
1.6 The Units of Measurement
A Meter: A Measure of Length
The Kilogram: A Measure of Mass
The Second: A Measure of Time
The Kelvin: A Measure of Temperature
Prefix Multipliers
Derived Units: Volume and Density
Calculating Density
Chemistry and Medicine: Bone Density
1.7 The Reliability of a Measurement
Counting Significant Figures
Exact Numbers
Significant Figures in Calculations
Precision and Accuracy
Chemistry in Your Day: Integrity in Data Gathering
1.8 Solving Chemical Problems
Converting From One Unit to Another
General Problem-Solving Strategy
Units Raised to a Power
Order of Magnitude Estimations
Problems Involving an Equation
Chapter 2
Atoms and Elements
2.1 Imaging and Moving Individual Atoms
2.2 Early Ideas about the Building Blocks of Matter
2.3 Modern Atomic Theory and the Laws That Led to It
The Law of Conservation of Mass
The Law of Definite Proportions
The Law of Multiple Proportions
John Dalton and The Atomic Theory
Chemistry in Your Day: Atoms and Humans
2.4 The Discovery of the Electron
Cathode Rays
Millikan’s Oil Drop Experiment: The Charge of the Electron
2.5 The Structure of The Atom
2.6 Subatomic Particles: Protons, Neutrons, and Electrons in Atoms
Elements: Defined by Their Number of Protons
Isotopes: When the Number of Neutrons Varies
Ions: Losing and Gaining Electrons
2.7 Finding Patterns: The Periodic Law and the Periodic Table
Ions and The Periodic Table
Chemistry and Medicine: The Elements of Life
2.8 Atomic Mass: The Average Mass of an Element’s Atoms
Mass Spectrometry: Measuring the Mass of Atoms and Molecules
2.9 Molar Mass: Counting Atoms by Weighing Them
The Mole: A Chemist’s “Dozen”
Converting between Number of Moles and Number of Atoms
Converting between Mass and Amount (Number of Moles)
Chapter 3
Molecules, Compounds and Chemical Equations
3.1 Hydrogen, Oxygen, and Water
3.2 Chemical Bonds
3.3 Representing Compounds: Chemical Formulas and Molecular Models
Types of Chemical Formulas
Molecular Models
3.4 An Atomic-Level Perspective of Elements and Compounds
3.5 Ionic Compounds: Formulas and Names
Writing Formulas for Ionic Compounds
Naming Ionic Compounds
Naming Binary Ionic Compounds
Naming Binary Ionic Compounds Containing a Metal that Forms More than One Kind of Cation
Naming Ionic Compounds Containing Polyatomic Ions
Hydrated Ionic Compounds
3.6 Molecular Compounds: Formulas and Names
Naming Molecular Compounds
Naming Acids
Naming Binary Acids
Naming Oxyacids
Chemistry in the Environment: Acid Rain
3.7 Formula Mass and The Mole Concept for Compounds
Molar Mass of a Compound
Using Molar Mass to Count Molecules by Weighing
3.8 Composition of Compounds
Mass Percent Composition as a Conversion Factor
Conversion Factors from Chemical Formulas
Chemistry and Medicine: Methylmercury in Fish
3.9 Determining a Chemical Formula from Experimental Data
Calculating Molecular Formulas for Compounds
Combustion Analysis
3.10 Writing and Balancing Chemical Equations
How to Write Balanced Chemical Equations
3.11 Organic Compounds (optional section)
Hydrocarbons
Functionalized Hydrocarbons
Chapter 4
Chemical Quantities and Aqueous Reactions
4.1 Global Warming and the Combustion of Fossil Fuels
4.2 Reaction Stoichiometry: How Much Carbon Dioxide?
Making Pizza: The Relationship among Ingredients
Making Molecules: Mole-to-Mole Conversions
Making Molecules: Mass-to-Mass Conversions
4.3 Limiting Reactant, Theoretical Yield, and Percent Yield
Limiting Reactant, Theoretical Yield, and Percent Yield From Initial Reactant Masses
Chemistry in the Environment: MTBE in Gasoline
4.4 Solution Concentration and Solution Stoichiomentry
Using Molarity in Calculations
Solution Dilution
Solution Stoichiomentry
4.5 Types of Aqueous Solutions and Solubility
Electrolyte and Nonelectrolyte Solutions
The Solubility of Ionic Compounds
4.6 Precipitation Reactions
4.7 Representing Aqueous Reactions: Molecular, Ionic, and Complete Ionic Equations
4.8 Acid-Base and Gas-Evolution Reactions
Acid-Base Reactions
Acid-Base Titrations
Gas-Evolution Reactions
4.9 Oxidation-Reduction Reactions
Oxidation States
Identifying Redox Reactions
Chemistry in Your Day: Bleached Blonde
Combustion Reactions
Chapter 5
Gases
5.1 Water from Wells: Atmospheric Pressure at Work
5.2 Pressure: The result of Molecular Collisions
Pressure Units
The Manometer: A Way to Measure Pressure in the Laboratory
Chemistry and Medicine: Blood Pressure
5.3 The Simple Gas Laws: Boyle’s Law, Charles’s Law and Avogadro’s Law
Boyle’s Law: Volume and Pressure
Chemistry in Your Day: Extra-Long Snorkels
Charles’s Law: Volume and Temperature
Avogadro’s Law: Volume and Amount (in Moles)
5.4 The Ideal Gas Law
5.5 Applications of the Ideal Gas Law: Molar Volume, Density and Molar Mass of a Gas
Molar Volume at Standard Temperature and Pressure
Density of a Gas
Molar Mass of a Gas
5.6 Mixtures of Gases and Partial Pressures
Deep Sea Diving and Partial Pressure
Collecting Gases Over Water
5.7 Gases in Chemical Reactions: Stoichiometry Revisited
Molar Volume and Stoichiometry
5.8 Kinetic Molecular Theory: A Model for Gases
Kinetic Molecular Theory and the Ideal Gas Law
Temperature and Molecular Velocities
5.9 Mean Free Path, Diffusion, and Effusion of Gases
5.10 Real Gases: The Effects of Size and Intermolecular Forces
The Effect of the Finite Volume of Gas Particles
The Effect of Intermolecular Forces
Van der Waal’s Equation
Real Gases
5.11 Chemistry of the Atmosphere: Air Pollution and Ozone Depletion
Air Pollution
Ozone Depletion
Chapter 6
Thermochemistry
6.1 Light the Furnace: The Nature of Energy and Its Transformations
The Nature of Energy: Key Definitions
Units of Energy
6.2 The First Law of Thermodynamics: There Is No Free Lunch
Chemistry in Your Day: Redheffer’s Perpetual Motion Machine
Internal Energy
6.3 Quantifying Heat and Work
Heat
Work: Pressure-Volume Work
6.4 Measuring DE for Chemical Reactions: Constant-Volume Calorimetry
6.5 Enthalpy: The Heat Evolved in a Chemical Reaction at Constant Pressure
Exothermic and Endothermic Processes: A Molecular View
Stoichiometry Involving DH: Thermochemical Equations
6.6 Constant Pressure Calorimetry: Measuring DHrxn
6.7 Relationships Involving DHrxn
6.8 Enthalpies of Reaction from Standard Heats of Formation
Standard States and Standard Enthalpy Changes
Calculating The Standard Enthalpy Change for a Reaction
6.9 Energy Use and The Environment
Environmental Problems Associated With Fossil Fuel Use
Chemistry and The Environment: Renewable Energy
Chapter 7
The Quantum-Mechanical Model of the Atom
7.1 Quantum Mechanics: A Theory That Explains the Behavior of the Absolutely Small
7.2 The Nature of Light
The Wave Nature of Light
The Electromagnetic Spectrum
Chemistry and Medicine: Radiation Treatment for Cancer
Interference and Diffraction
The Particle Nature of Light
7.3 Atomic Spectroscopy and the Bohr Model
Chemistry in Your Day: Atomic Spectroscopy, a Bar Code for Atoms
7.4 The Wave Nature of Matter: The de Broglie Wavelength, t he Uncertainty Principle, and Probability
The de Broglie Wavelength
The Uncertainty Principle
Indeterminacy and Probability Distribution Maps
7.5 Quantum Mechanics and the Atom
Solutions to the Schrödinger Equation for the Hydrogen Atom
Atomic Spectroscopy Explained
7.6 The Shapes of Atomic Orbitals
p Orbitals (l = 1)
d Orbitals (l = 2)
f Orbitals (l = 3)
Chapter 8
Periodic Properties of the Elements
8.1 Nerve Signal Transmission
8.2 The Development of the Periodic Table
8.3 Electron Configurations: How Electrons Occupy Orbitals
Electron Spin and the Pauli Exclusion Principle
Sublevel Energy Splitting in Multi-electron Atoms
Electron Configurations for Multi-electron Atoms
8.4 Electron Configurations, Valence Electrons, and The Periodic Table
Orbital Blocks in the Periodic Table
Writing and Electron Configuration for an Element from Its position in The Periodic Table
The Transition and Inner Transition Elements
8.5 The Explanatory Power of the Quantum-Mechanical Model
8.6 Periodic Trends in the Size of Atoms and Effective Nuclear Charge
Effective Nuclear Charge
Atomic Radii and the Transition Elements
8.7 Ions: Electron Configurations, Magnetic Properties, Ionic Radii, and Ionization Energy
Electron Configurations and Magnetic Properties of Ions
Ionic Radii
Ionization Energy
Trends in First Ionization Energy
Exceptions to Trends in First Ionization Energy
Trends in Second and Successive Ionization Energies
8.8 Electron Affinities and Metallic Character
Electron Affinity
Metallic Character
8.9 Some Examples of Periodic Chemical Behavior: The Alkali Metals, The Halogens and The Noble Gases
The Alkali Metals (Group 1A)
The Halogens (Group 7A)
Chemistry and Medicine: Potassium Iodide in Radiation Emergencies
The Noble Gases (Group 8A)
Chapter 9
Chemical Bonding I: Lewis Theory
9.1 Bonding Models and AIDS Drugs
9.2 Types of Chemical Bonds
9.3 Representing Valance Electrons with Dots
9.4 Ionic Bonding: Lewis Structures and Lattice Energies
Ionic Bonding and Electron Transfer
Lattice Energy: The Rest of the Story
The Born-Haber Cycle
Trends in Lattice Energies: ion Size
Trends in Lattice Energies: Ion Charge
Ionic Bonding: Models and Reality
Chemistry and Medicine: Ionic Compounds as Drugs
9.5 Covalent Bonding: Lewis Structure
Single Covalent Bonds
Double and Triple Covalent Bonds
Covalent Bonding: Models and Reality
9.6 Electronegativity and Bond Polarity
Electronegativity
Bond Polarity, Dipole Moment, and Percent Ionic Character
9.7 Lewis Structures of Molecular Compounds and Polyatomic Ions
Writing Lewis Structures for Molecular Compounds
Writing Lewis Structures for Polyatomic Ions
9.8 Resonance and Formal Charge
Resonance
Formal Charge
9.9 Exceptions to the Octet Rule: Odd Electron Species, Incomplete Octets, and Expanded Octets
Odd Electron Species
Chemistry and the Environment: Free Radicals and the Atmospheric Vacuum Cleaner
Incomplete Octets
Expanded Octets
9.10 Bond Energies and Bond Lengths
Bond Energy
Using Bond Energies to Estimate Enthalpy Changes for Reactions
Bond Lengths
Chemistry and The Environment: The Lewis Structure of Ozone
9.11 Bonding in Metals: The Electron Sea Model
Chapter 10
Chemical Bonding II: Molecular Shapes, Valance Bond Theory, and Molecular Orbital Theory
10.1 Artificial Sweeteners: Fooled by Molecular Shape
10.2 VSPER Theory: The Five Basic Shapes
Two Electron Groups: Linear Geometry
Three Electron Groups: Trigonal Planar Geometry
Four Electron Groups: Tetrahedral Geometry
Five Electron Groups: Octahedral Geometry
10.3 VSPER Theory: The Effect of Lone Pairs
Four Electron Groups with Lone Pairs
Five Electron Groups with Lone Pairs
Six Electron Groups with Lone Pairs
Summary of VSPER theory
10.4 VSPER Theory: Predicting Molecular Geometries
Predicting the Shapes of Larger Molecules
10.5 Molecular Shape and Polarity
Chemistry in Your Day: How Soap Works
10.6 Valence Bond Theory: Orbital Overlap as a Chemical Bond
10.7 Valence Bond Theory: Hybridization of Atomic Orbitals
sp2 Hybridization and Double Bonds
Everryday Chemistry: The Chemistry of Vision
sp Hybridization and Triple Bonds
sp3d and sp3d2 Hybridization
Writing Hybridization and Bonding Schemes
10.8 Molecular Orbital Theory: Electron Delocalization
Linear Combination of Atomic Orbitals (LCAO)
Main Ideas in Applying LCAO-MO Theory
Period Two Homonuclear Diatomic Molecules
Period Two Heteronuclear Diatomic Molecules
Polyatomic Molecules
Chapter 11
Liquids, Solids, and Intermolecular Forces
11.1 Climbing Geckos and Intermolecular Forces
11.2 Solids, Liquids, and Gases: A Molecular Comparison
Changes Between Phases
11.3 Intermolecular Forces: The Forces that Hold Condensed Phases Together
Dispersion Force
Dipole-Dipole Force
Hydrogen Bonding
Ion-dipole Force
Chemistry and Medicine: Hydrogen Bonding in DNA
11.4 Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action
Surface Tension
Viscosity
Chemistry in Your Day: Viscosity and Motor Oil
Capillary Action
11.5 Vaporization and Vapor Pressure
The Process of Vaporization
The Energetics of Vaporization
Vapor Pressure and Dynamic Equilibrium
Temperature Dependence of Vapor Pressure and Boiling Point
The Clausius Clapeyron Equation
The Critical Point: The Transition to an Unusual Phase of Matter
11.6 Sublimation and Fusion
Sublimation
Fusion
Energetics of Melting and Freezing
11.7 Heating Curve for Water
11.8 Phase Diagrams
The Major Features of a Phase Diagram
Navigation Within a Phase Diagram
The Phase Diagrams of Other Substances
11.9 Water: An Extraordinary Substance
Chemistry in the Environment: Water Pollution
11.10 Crystalline Solids: Determining Their Structure by X-Ray Crystallography
11.11 Crystalline Solids: Unit Cells and Basic Structures
Simple Cubic Unit Cell
Close-Packed Structures
11.12 Crystalline Solids: The Fundamental Types
Molecular Solids
Ionic Solids
Atomic Solids
11.13 Crystalline Solids: Band Theory
Doping: Controlling the Conductivity of Semiconductors
Chapter 12
Solutions
12.1 Thirsty Solutions: Why You Should Not Drink Seawater
12.2 Types of Solutions and Solubility
Nature’s Tendency Toward Mixing: Entropy
The Effect of Intermolecular Forces
12.3 Energetics of Solution Formation
Aqueous Solutions and Heats of Hydration
12.4 Solution Equilibrium and Factors Affecting Solubility
The Temperature Dependence of the Solubility of Solids
Factors Affecting the Solubility of Gases in Water
Chemistry in the Environment: Lake Nyos
12.5 Expressing Solution Concentration
Molarity
Molality
Parts by Mass and Parts by Volume
Mole Fraction and Mole Percent
12.6 The Vapor Pressure of a Solution
Ionic Solutes and Vapor Pressure
Ideal and Non-Ideal Solutions
12.7 Freezing Point Depression, Boiling Point Elevation, and Osmosis
Freezing Point Depression
Chemistry in Your Day: Antifreeze in Frogs
Boiling Point Elevation
Osmosis
Colligative Properties of Ionic Solutions
Colligative Properties and Medical Solutions
12.8 Colloids
Chapter 13
Chemical Kinetics
13.1 Catching Lizards
13.2 Rate of a Chemical Reaction
Measuring Reaction Rates
13.3 The Rate Law: The Effect of Concentration on Reaction Rate
Determining the Order of a Reaction
Reaction Order for Multiple Reactants
13.4 The Integrated Rate Law: The Dependence of Concentration on Time
First-order Integrated Rate Law
Second-order Integrated Rate Law
Zero-order Integrated Rate Law
The Half-Life of a Reaction
First-order Reaction Half-Life
Second-order Reaction Half-Life
Zero-order Reaction Half-Life
13.5 The Effect of Temperature on Reaction Rate
Arrhenius Plots: Experimental Measurements of the Frequency Factor and the Activation Energy
The Collision Model: A Closer Look at the Frequency Factor
13.6 Reaction Mechanisms
Rate Laws for Elementary Steps
Rate-Determining Steps and Overall Reaction rate Laws
Mechanisms with a Fast Initial Step
13.7 Catalysis
Homogenous and Heterogenous Catalysis
Enzymes: Biological Catalysts
Chemistry and Medicine: Enzyme Catalysis and the Role of Chymotrypsin in Digestion
Chapter 14
Chemical Equilibrium
14.1 Fetal Hemoglobin and Equilibrium
14.2 The Concept of Dynamic Equilibrium
Chemistry and Medicine: Life and Equilibrium
14.3 The Equilibrium Constant (K)
Expressing Equilibrium Constants for Chemical Reactions
The Significance of the Equilibrium Constant
Relationships Between the Equilibrium Constant and the Chemical Equation
14.4 Expressing the Equilibrium Constant in Terms of Pressure
Units of K
14.5 Heterogenous Equilibria: Reactions Involving Solids and Liquids
14.6 Calculating the Equilibrium Constant From Measured Equilibrium Concentrations
14.7 The Reaction Quotient: Predicting the Direction of Change
14.8 Finding Equilibrium Concentrations
Simplifying Approximations in Working Equilibrium Problems
14.9 Le Châtelier’s Principle: How a System at Equilibrium Responds to Disturbances
The Effect of a Concentration Change on Equilibrium
The Effect of a Volume (or Pressure) Change on Equilibrium
The Effect of a Temperature Change on Equilibrium
Chapter 15
Acids and Bases
15.1 Heartburn
15.2 The Nature of Acids and Bases
15.3 Definitions of Acids and Bases
The Arrhenius Definition
The Brønsted-Lowry definition
15.4 Acid Strength and the Acid Dissociation Constant (Ka)
Strong Acids
Weak Acids
The acid ionization constant (Ka)
15.5 Autoionization of Water and pH
The pH Scale: A Way to Quantify Acidity and Basicity
pOH and Other p Scales
Chemistry and Medicine: Ulcers
15.6 Finding the [H3O+] and pH of Strong and Weak Acid Solutions
Percent Ionization of a Weak Acid
Mixtures of Acids
A Strong Acid and a Weak Acid
A Mixture of Two Weak Acids
15.7 Base Solutions
Strong Bases
Weak Bases
Finding [OH-] and pH of Basic Solutions
Chemistry and Medicine: What’s in my Antacid?
15.8 The Acid-Base Properties of Ions and Salts
Anions as Weak Bases
Cations as Weak Acids
Classifying Salt Solutions as Acidic, Basic, or Neutral
15.9 Polyprotic Acids
Finding the pH of Polyprotic Acid Solutions
Finding the concentration of the anions for a weak diprotic acid solutions
15.10 Acid Strength and Molecular Structure
Binary Acids
Oxyacids
15.11 Lewis Acids and Bases
Molecules that act as Lewis Acids
Cations that act as Lewis Acids
15.12 Acid rain
Effects of Acid Rain
Chapter 16
Aqueous Ionic Equilibrium
16.1 The Danger of Antifreeze
16.2 Buffers: Solutions That Resist pH Change
Calculating the pH of a Buffer Solution
The Henderson-Hasselbalch Equation
Calculating pH Changes in a Buffer Solution
Buffers Containing a Base and Its Conjugate Acid
16.3 Buffer Effectiveness: Buffer Capacity and Buffer Range
Relative Amounts of Acid and Base
Absolute concentrations of the acid and conjugate base
Buffer Range
Buffer Capacity
Chemistry and Medicine: Buffer Effectiveness in Human Blood
16.4 Titrations and pH Curves
The Titration of a Strong Acid with a Strong Base
The Titration of a Weak Acid with a Strong Base
Titration of a Polyprotic Acid
Indicators: pH-Dependent Colors
16.5 Solubility Equilibria and the Solubility Product Constant
Ksp and Molar Solubility
Chemistry in Your Day: Hard Water
Ksp and Relative Solubility
The Effect of a Common Ion on Solubility
The Effect of pH on Solubility
16.6 Precipitation
Selective Precipitation
16.7 Qualitative Chemical Analysis
Group I: Insoluble Chlorides
Group II: Acid-Insoluble Sulfides
Group III: Base-Insoluble Sulfides and Hydroxides
Group IV: Insoluble Carbonates
Group V: Alkali Metals and NH4+
16.8 Complex Ion Equilibria
The Effect of Complex Ion Equilibria in Solubility
The Solubility of Amphoteric Metal Hydroxides
Chapter 17
Free Energy and Thermodynamics
17.1 Nature’s Heat Tax: You Can’t Win and You Can’t Break Even
17.2 Spontaneous and Nonspontaneous Processes
17.3 Entropy and the Second Law of Thermodynamics
Entropy
The Second Law of Thermodynamics
The Entropy Change Associated with a Change in State
17.4 Heat Transfer and Changes in the Entropy of the Surroundings
The Temperature Dependence of ΔSsurr
Quantifying Entropy Changes in the Surroundings
17.5 Gibbs Free Energy
The Effect of ΔH, ΔS, and T on Spontaneity
17.6Entropy Changes in Chemical Reactions: Calculating ΔSrxn°
Standard Molar Entropies (S°)and the Third Law of Thermodynamics
Relative Standard Entropies: Gases, Liquids, and Solids
Relative Standard Entropies: Molar Mass
Relative Standard Entropies: Allotropes
Relative Standard Entropies: Molecular Complexity
Relative Standard Entropies: Dissolution
Calculating the Standard Entropy Change (ΔSrxn°) for a Reaction
17.7 Free Energy Changes in Chemical Reactions: Calculating (ΔGrxn°)
Calculating Free Energy Changes using ΔGrxn° = ΔHrxn° - T ΔSrxn°.
Calculating ΔGrxn° using Tabulated Values of Free Energies of Formation
Determining ΔGrxn° for a Stepwise Reaction from the Changes in Free Energy for Each of the Steps
Chemistry in Your Day: Making a Nonspontaneous Process Spontaneous
Why Free Energy is “Free”
17.8 Free Energy Changers for Non-Standard States: The Relationship between ΔGrxn° and ΔGrxn
The Free Energy of reaction under Nonstandard Conditions
17.9 Free Energy and Equilibrium: Relating ΔGrxn° to the Equilibrium Constant (K)
The Temperature Dependence of the Equilibrium Constant
Chapter 18
Electrochemistry
18.1 Pulling the Plug on the Power Grid
18.2 Balancing Oxidation-Reduction Equations
18.3 Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions
Electrochemical Cell Notation
18.4 Standard Reduction Potentials
Predicting the Spontaneous Direction of an Oxidation-Reduction Reaction
Predicting Whether a Metal Will Dissolve in Acid
18.5 Cell Potential, Free Energy, and the Equilibrium Constant
The Relationship Between ΔGo and Eocell
The Relationship between Eocell and K
18.6 Cell Potential and Concentration
Concentration
Chemistry and Medicine: Concentration Cells in Human Nerve Cells
18.7 Batteries: Using Chemistry to Generate Electricity
Dry-Cell Batteries
Lead-Acid Storage Batteries
Other Rechargeable Batteries
Fuel Cells
Chemistry In Your Day: The Fue-Cell Breathalyzer
18.8 Electrolysis: Driving Non-spontaneous Chemical Reactions with Electricity
Predicting the Products of Electrolysis
Stoichiometry of Electrolysis
18.9 Corrosion: Undesirable Redox Reactions
Preventing Corrosion
Chapter 19
Radioactivity and Nuclear Chemistry
19.1 Diagnosing Appendicitis
19.2 The Discovery of Radioactivity
19.3 Types of Radioactivity
Alpha (α) Decay
Beta (β) Decay
Gamma (γ) Ray Emission
Postitron Emission
Electron Capture
19.4 The Valley of Stability: Predicting the Type of Radioactivity
Magic Numbers
Radioactive Decay Series
19.5 Detecting Radioactivity
19.6 The Kinetics of Radioactive Decay and Radiometric Dating
Chemistry in the Environment: Environmental Radon
The Integrated Rate Law
Radiocarbon Dating: Using Radioactivity to Measure the Age of Fossils and Artifacts
Chemistry in your Day: Radiocarbon Dating and The Shroud of Turin
Uranium-Lead Dating
The Age of the Earth
19.7 The Discovery of Fission: The Atomic Bomb and Nuclear Power
Nuclear Power: Using Fission to Generate Electricity
19.8 Converting Mass to Energy: Mass Defect and Nuclear Binding Energy
Mass Defect
19.9 Nuclear Fusion: The Power of the Sun
19.10 Nuclear Transmutation and Transuranium Elements
19.11 The Effects of Radiation on Life
Acute Radiation Damage
Increased Cancer Risk
Genetic Defects
Measuring Radiation Exposure
19.12 Radioactivity in Medicine and Other Applications
Diagnosis in Medicine
Radiotherapy in Medicine
Other Applications
Chapter 20
Organic Chemistry
20.1 Fragrances and Odor
20.2 Carbon: Why It Is Unique
Chemistry In Your Day: Vitalism and the Perceived Difference Between Organic and Inorganic
20.3 Hydrocarbons: Compounds Containing Only Carbon and Hydrocarbon
Drawing Hydrocarbon Structures
Stereo and Optical Isomerism
20.4 Alkanes: Saturated Hydrocarbons
Naming Alkanes
20.5 Alkenes and Alkynes
Naming Alkenes and Alkynes
Geometric (cis-trans) Isomerism in Alkenes
20.6 Hydrocarbon Reactions
Reactions of Alkanes
Reactions of Alkenes and Alkynes
20.7 Aromatic Hydrocarbons
Naming Aromatic Hydrocarbons
Reactions of Aromatic Compounds
20.8 Functional Groups
20.9 Alcohols
Naming Alcohols
About Alcohols
Alcohol Reactions
20.10 Aldehydes and Ketones
Naming Aldehydes and Ketones
About Aldehydes and Ketones
Aldehyde and Ketone Reactions
20.11 Carboxylic Acids and Esters
Naming Carboxylic Acids and Esters
About Carboxylic Acids and Esters
Carboxylic Acid and Ester Reactions
20.12 Ethers
Naming Ethers
About Ethers
20.13 Amines
Amine Reactions
20.14 Polymers
Chemistry in Your Day: Kevlar
Chapter 21
Biochemistry
21.1 Diabetes and the Synthesis of Human Insulin
21.2 Lipids
Fatty Acids
Fats and Oils
Chemistry and Health: Dietary Fat: The Good, the Bad, and the Ugly
Other Lipids
21.3 Carbohydrates
Simple Carbohydrates: Monosaccharides and Disaccharides
Complex Carbohydrates
21.4 Proteins and Amino Acids
Amino Acids: The Building Blocks of Proteins
Peptide Bonding Between Amino Acids
Chemistry and Medicine: The Essential Amino Acids
21.5 Protein Structure
Primary Structure
Secondary Structure
Tertiary Structure
Quaternary Structure
21.6 Nucleic Acids: Blueprints for Proteins
Basic Structure of Nucleic Acids
The Genetic Code
21.7 DNA Replication, the Double Helix, and Protein Synthesis
DNA Replication and the Double Helix
Protein Synthesis
Chemistry and Medicine: The Human Genome Project
Chapter 22
Chemistry of the Nonmetals
22.1 Insulated Nanowires
22.2 The Main-Group Elements: Bonding and Properties
Atomic size and Types of Bonds
22.3 The Most Common Matter: Silicates
Quartz and Glass
Aluminosilicates
Individual Silicate Units, Silicate Chains, and Silicate Sheets
22.4 Boron: An Intersting Group 3A Element and Its Amazing Structures
Elemental Boron
Boron Compounds: Trihalides
Boron-Oxygen Compounds
Boron-Hydrogen Compounds: Boranes
22.5 Carbon, Carbides, and Carbonates
Carbon
Carbides
Carbon Oxides
Carbonates
22.6 Nitrogen and Phosphorus: Essential Elements for Life
Elemental Nitrogen and Phosphorus
Nitrogen Compounds
Nitrogen Hydrides
Nitrogen Oxides
Nitric Acid, Nitrates, and Nitrides
Phosphorus Compounds
Phosphine
Phosphorus Halides
Phosphorous Oxides
Phosphoric Acid and Phosphates
22.7 Oxygen
Elemental Oxygen
Uses for Oxygen
Oxides
Ozone
22.8 Sulfur: A Dangerous but Useful Element
Elemental Sulfur
Hydrogen Sulfide and Metal Sulfides
Sulfur Dioxide
Sulfuric Acid
22.9 Halogens: Reactive Chemicals with High Electronegativity
Elemental Fluorine and Hydrofluoric Acid
Elemental Cl and HCl
Halogen Compounds
Interhalogen Compounds
Halogen Oxides
Chapter 23
Metals and Metallurgy
23.1 Vanadium: A Problem and an Opportunity
23.2 The General Properties and Natural Distribution of Metals
23.3 Metallurgical Processes
Separation
Pyrometallurgy
Hydrometallurgy
Electrometallurgy
Powder Metallurgy
23.4 Metal Structures and Alloys
Alloys
Substitutional Alloys: Miscible Solid Solutions
Alloys with Limited Solubility
Interstital Alloys
23.5 Sources, Properties, and Products of Some of the 3d Transition Metals
Titanium
Chromium
Manganese
Cobalt
Copper
Nickel
Zinc
Chapter 24
Transition Metals and Coordination Compounds
24.1 The Colors of Rubies and Emeralds
24.2 Properties of Transition Metals
Electronic Configurations
Atomic Size
Ionization Energy
Electronegativity
Oxidation States
24.3 Coordination Compounds
Naming Coordination Compounds
24.4 Structure and Isomerization
Structural Isomerism
Stereoisomerism
24.5 Bonding in Coordinate Compounds
Valance Bond Theory
Crystal Field Theory
Octahedral Complexes
The Color of Complex Ions and Crystal Field Strength
Magnetic Properties
Tetrahedral and Square Planar Complexes
Chelating Agents
Chemical Analysis
Coloring Agents
Biomolecules
Nivaldo Tro is Professor of Chemistry at Westmont College in Santa Barbara, California, where he has been a faculty member since 1990. He received his Ph.D. in chemistry from Stanford University, for work on developing and using optical techniques to study the adsorption and desorption of molecules to and from surfaces in ultrahigh vacuum. He then went on to the University of California at Berkeley, where he did post-doctoral research on ultra-fast reaction dynamics in solution. Since coming to Westmont, Professor Tro has been awarded grants from the American Chemical Society Petroleum Research Fund, from Research Corporation, and from the National Science Foundation to study the dynamics of various processes occurring in thin adlayer films adsorbed on dielectric surfaces. He has twice been honored as Westmont's outstanding teacher of the year and has also received the college's outstanding researcher of the year award. Professor Tro lives in Santa Barbara with his wife, Ann, and their four children, Michael, Ali, Kyle, and Kaden. In his leisure time, Professor Tro enjoys reading good literature to his children and being outdoors with his family.
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Chapter 1: Matter, Measurement,
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