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Book details
ISBN: 9780073511160 / 0073511161
Division: Higher Education
Pub Date: JAN-11
Pages: 1128

Copyright: 2012
Edition: 1
Format: Hardback
Chemistry: Atoms First

Julia Burdge, Jason Overby


About the book

The atoms first approach provides a consistent and logical method for teaching general chemistry. This approach starts with the fundamental building block of matter, the atom, and uses it as the stepping stone to understanding more complex chemistry topics. Once mastery of the nature of atoms and electrons is achieved, the formation and properties of compounds are developed. Only after the study of matter and the atom will students have sufficient background to fully engage in topics such as stoichiometry, kinetics, equilibrium, and thermodynamics. Thus, the Atoms First method empowers instructors to present the most complete and compelling story of general chemistry. Far from a simple re-ordering of topics, this is a book that will truly meet the needs of the growing atoms-first market.
Key features

  • Consistent problem-solving skill development. Burdge/Overby fosters a consistent problem-solving approach providing the skill set for students to master the basics of critical thinking. Each Worked Example is followed by two practice problems. Practice Problem "A" allows the student to solve the problem using the same steps in the Sample Problem above. Practice Problem "B" probes comprehension of the same concept as Practice Problem "A", but is generally sufficiently different that it cannot be solved using the exact approach that is used in the Worked Example.
  • Engaging real-life examples and applications. Each chapter is introduced with an engaging photo and short interesting, relevant explanation of the photo to interest the student. Applications titled "Thinking Outside the Box" are available in every chapter and contain a topic that is applicable to the chapter but not necessarily covered in the course. If the instructor wants the students to read these, there are end-of-chapter problems that can be assigned.
  • Outstanding pedagogy for student learning. The Section Reviews (many with visuals), Rewind and Fast Forward Buttons are meant to enhance student understanding and comprehension by reinforcing current concepts and interconnecting new concepts to others throughout the text.
  • McGraw-Hill's CONNECT: With Connect Chemistry, instructors can deliver assignments, quizzes, and tests online. The problems directly from the end-of-chapter material in the textbook are presented in an auto-gradable format. The online homework system incorporates new and exciting and interactive tools including the market standard drawing tool - ChemDraw. Julia Burdge and Jason Overby's problem-solving methodology is carried over from the textbook into the online homework system. Over 2,200 end-of-chapter problems and additional problems are available to assign within the Connect program.

    Instructors can edit existing questions and write entirely new problems; track individual student performance – by question, assignment, concept, or in relation to the class overall – with automatic grading; provide instant feedback to students; and secure storage of detailed grade reports online.

  • Presentation Center. Build instructional materials wherever, whenever, and however you want! Presentation Center is an online digital library containing assets such as photos, artwork, animations, PowerPoint Lecture Outlines, Image Power Points, and other types of media that can be used to create customized lectures, visually enhanced tests and quizzes, compelling course websites, or attractive printed support materials. Access to your book, access to all books! This ever-growing resource gives instructors the power to utilize assets specific to their adopted textbook as well as content from other McGraw-Hill books in the library. Presentation Center’s dynamic search engine allows you to explore by discipline, course, textbook chapter, asset type, or keyword. Simply browse, select, and download the files you need to build engaging course materials. All assets are copyrighted by McGraw-Hill Higher Education but can be used by instructors for classroom purposes.
  • Atoms First offers an exciting visual program of both unique and conventional art figures that enhance student understanding of chemical concepts. The art includes Visualizing Chemistry process pieces, macro-micro art, and three-dimensional art. The art breaks down the chemical processes from complex into simpler, more user-friendly concepts. You will find 18 Visualizing Process Piece art-spreads that emphasize the fundamental, vitally important principles of chemistry.

  • Table of contents

    Chapter 1—Chemistry: The Science of Change
    1.1 The Study of Chemistry
    1.1 Classification of Matter
    1.3 The Properties of Matter
    1.4 Scientific Measurement
    1.5 Uncertainty in Measurement
    1.6 Using Units and Solving Problems
    Chapter 2—Atoms and the Periodic Table
    2.1 Atoms First
    2.2 Subatomic Particles and Atomic Structure
    2.3 Atomic Number, Mass Number, and Isotopes
    2.4 Average Atomic Mass
    2.5 The Periodic Table
    2.6 The Mole and Molar Masses
    Chapter 3—Quantum Theory and the Electronic Structure of Atoms
    3.1 Energy and Energy Changes
    3.2 The Nature of Light
    3.3 Quantum Theory
    3.4 Bohr’s Theory of the Hydrogen Atom
    3.5 Wave Properties of Matter
    3.6 Quantum Mechanics
    3.7 Quantum Numbers
    3.8 Atomic Orbitals
    3.9 Electron Configuration
    3.10 Electron Configurations and the Periodic Table
    Chapter 4—Periodic Trends of the Elements
    4.1 Development of the Periodic Table
    4.2 The Modern Periodic Table
    4.3 Effective Nuclear Charge
    4.4 Periodic Trends in Properties of Atoms
    4.5 Electron Configuration of Ions
    4.6 Ionic Radius
    Chapter 5—Ionic and Covalent Compounds
    5.1 Compounds
    5.2 Lewis Dot Symbols
    5.3 Ionic Compounds and Bonding
    5.4 Naming Ions and Ionic Compounds
    5.5 Covalent Molecules and Bonding
    5.6 Naming Molecular Compounds
    5.7 Covalent Bonding in Ionic Species
    5.8 Molecular and Formula Masses
    5.9 Percent Composition of Compounds
    5.10 The Mole and Molar Masses
    Chapter 6—Representing Molecules
    6.1 The Octet Rule
    6.2 Electronegativity and Polarity
    6.3 Drawing Lewis Structures
    6.4 Lewis Structures and Formal Charge
    6.5 Resonance
    6.6 Exceptions to the Octet Rule
    Chapter 7—Molecular Geometry and Bonding Theories
    7.1 Molecular Geometry
    7.2 Molecular Geometry and Polarity
    7.3 Valence Bond Theory
    7.4 Hybridization of Atomic Orbitals
    7.5 Hybridization in Molecules Containing Multiple Bonds
    7.6 Molecular Orbital Theory
    7.7 Bonding Theories and Descriptions of Molecules with Delocalized Bonding
    Chapter 8—Chemical Reactions
    8.1 Chemical Equations
    8.2 Combustion Analysis
    8.3 Calculations with Balanced Chemical Equations
    8.4 Limiting Reactants
    8.5 Periodic Trends in Reactivity of the Main Group Elements
    Chapter 9—Chemical Reactions in Aqueous Solutions
    9.1 General Properties of Aqueous Solutions
    9.2 Precipitation Reactions
    9.3 Acid-Base Reactions
    9.4 Oxidation–Reduction Reactions
    9.5 Concentration of Solutions
    9.6 Aqueous Reactions and Chemical Analysis
    Chapter 10—Thermochemistry
    10.1 Energy Changes in Chemical Reactions
    10.2 Introduction to Thermodynamics
    10.3 Enthalpy
    10.4 Calorimetry
    10.5 Hess’s Law
    10.6 Standard Enthalpies of Formation
    10.7 Bond Enthalpy and the Stability of Covalent Molecules
    10.8 Lattice Energy and the Stability of Ionic Solids
    Chapter 11—Gases
    11.1 Properties of Gases
    11.2 The Kinetic Molecular Theory of Gases
    11.3 Pressure
    11.4 The Gas Laws
    11.5 The Ideal Gas Equation
    11.6 Real Gases
    11.7 Gas Mixtures
    11.8 Reactions with Gaseous Reactants and Products
    Chapter 12—Intermolecular Forces and the Physical Properties of Condensed Phases
    12.1 Intermolecular Forces
    12.2 Properties of Liquids
    12.3 Crystal Structure
    12.4 Types of Crystals
    12.5 Amorphous Solids
    12.6 Phase Changes
    12.7 Phase Diagrams
    Chapter 13—Physical Properties of Solutions
    13.1 Types of Solutions
    13.2 A Molecular View of the Solution Process
    13.3 Concentration Units
    13.4 Factors that Affect Solubility
    13.5 Colligative Properties
    13.6 Calculations Using Colligative Properties
    13.7 Colloids
    Chapter 14—Chemical Kinetics
    14.1 Reaction Rates
    14.2 Collision Theory of Chemical Reactions
    14.3 Measuring Reaction Progress and Expressing Reaction Rate
    14.4 Dependence of Reaction Rate on Reactant Concentration
    14.5 Dependence of Reactant Concentration on Time
    14.6 Dependence of Reaction Rate on Temperature
    14.7 Reaction Mechanisms
    14.8 Catalysis
    Chapter 15—Chemical Equilibrium
    15.1 The Concept of Equilibrium
    15.2 The Equilibrium Constant
    15.3 Equilibrium Expressions
    15.4 Using Equilibrium Expressions to Solve Problems
    15.5 Factors That Affect Chemical Equilibrium
    Chapter 16—Acids and Bases
    16.1 Brønsted Acids and Bases
    16.2 Molecular Structure and Acid Strength
    16.3 The Acid-Base Properties of Water
    16.4 The pH Scale
    16.5 Strong Acids and Bases
    16.6 Weak Acids and Acid Ionization Constants
    16.7 Weak Bases and Base Ionization Constants
    16.8 Conjugate Acid–Base Pairs
    16.9 Diprotic and Polyprotic Acids
    16.10 Acid–Base Properties of Salt Solutions
    16.11 Acid–Base Properties of Oxides and Hydroxides
    16.12 Lewis Acids and Bases
    Chapter 17—Acid-Base Equilibria and Solubility Equilibria
    17.1 The Common Ion Effect
    17.2 Buffer Solutions
    17.3 Acid–Base Titrations
    17.4 Solubility Equilibria
    17.5 Factors Affecting Solubility
    17.6 Separation of Ions Using Differences in Solubility
    Chapter 18—Entropy, Free Energy, and Equilibrium
    18.1 Spontaneous Processes
    18.2 Entropy
    18.3 Entropy Changes in a System
    18.4 Entropy Changes in the Universe
    18.5 Predicting Spontaneity
    18.6 Free Energy and Chemical Equilibrium
    18.7 Thermodynamics in Living Systems
    Chapter 19—Electrochemistry
    19.1 Balancing Redox Reactions
    19.2 Galvanic Cells
    19.3 Standard Reduction Potentials
    19.4 Spontaneity of Redox Reactions Under Standard-State Conditions
    19.5 Spontaneity of Redox Reactions Under Conditions Other than Standard-State
    19.6 Batteries
    19.7 Electrolysis
    19.8 Corrosion
    Chapter 20—Nuclear Chemistry
    20.1 Nuclei and Nuclear Reactions
    20.2 Nuclear Stability
    20.3 Natural Radioactivity
    20.4 Nuclear Transmutation
    20.5 Nuclear Fission
    20.6 Nuclear Fusion
    20.7 Uses of Isotopes
    20.8 Biological Effects of Radiation
    Chapter 21—Metallurgy and the Chemistry of Metals
    21.1 Occurrence of Metals
    21.2 Metallurgical Processes
    21.3 Band Theory of Conductivity
    21.4 Periodic Trends in Metallic Properties
    21.5 The Alkali Metals
    21.6 The Alkaline Earth Metals
    21.7 Aluminum
    Chapter 22—Coordination Chemistry
    22.1 Coordination Compounds
    22.2 Structure of Coordination Compounds
    22.3 Bonding in Coordination Compounds: Crystal Field Theory
    22.4 Reactions of Coordination Compounds
    22.5 Applications of Coordination Compounds
    Chapter 23—Nonmetallic Elements and Their Compounds
    23.1 General Properties of Nonmetals
    23.2 Hydrogen
    23.3 Carbon
    23.4 Nitrogen and Phosphorus
    23.5 Oxygen and Sulfur
    23.6 The Halogens
    Chapter 24—Organic Chemistry
    24.1 Why Carbon is Different
    24.2 Classes of Organic Compounds
    24.3 Representing Organic Molecules
    24.4 Isomerism
    24.5 Organic Reactions
    24.6 Organic Polymers
    Chapter 25—Materials
    25.1 Polymers
    25.2 Ceramics and Composite Materials
    25.3 Liquid Crystals
    25.4 Biomedical Materials
    25.5 Nanotechnology
    25.6 Semiconductors
    25.7 Superconductors
  • Appendix 1 – Mathematical Operations
  • Appendix 2 – Thermodynamic Data at 1 ATM and 25°C
  • Appendix 3 – Ionization Constants of Weak Acids and Bases at 25°C
  • Appendix 4 – Solubility Product Constants at 25°C


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