Pearson eText Basic Chemistry -- Access Card

Master the math and problem solving you'll use in your future chemistry classes.
Basic Chemistry introduces the essential scientific and mathematical concepts of general chemistry while providing the scaffolded support students need to succeed in the course.

For courses in introductory, preparatory, and basic chemistry.

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Karen Timberlake is Professor Emerita of Chemistry at Los Angeles Valley College, where she taught chemistry for allied health and preparatory chemistry for 36 years. She received her bachelor’s degree in chemistry from the University of Washington and her master’s degree in biochemistry from the University of California at Los Angeles.

Professor Timberlake has been writing chemistry textbooks for more than 40 years. During that time, her name has become associated with the strategic use of pedagogical tools that promote student success in chemistry and the application of chemistry to real-life situations. More than one million students have learned chemistry using texts, laboratory manuals, and study guides written by Karen Timberlake. In addition to Basic Chemistry, sixth edition, she is also the author of General, Organic, and Biological Chemistry: Structures of Life, sixth edition, with the accompanying Study Guide, and Chemistry: An Introduction to General, Organic, and Biological Chemistry, thirteenth edition, with the accompanying Study Guide and Selected Solutions Manual, Laboratory Manual, and Essential Laboratory Manual.

Professor Timberlake belongs to numerous scientific and educational organizations including the American Chemical Society (ACS) and the National Science Teachers Association (NSTA). She has been the Western Regional Winner of Excellence in College Chemistry Teaching Award given by the Chemical Manufacturers Association. She received the McGuffey Award in Physical Sciences from the Textbook Authors Association for her textbook Chemistry: An Introduction to General, Organic, and Biological Chemistry, eighth edition. She received the “Texty” Textbook Excellence Award from the Textbook Authors Association for the first edition of Basic Chemistry. She has participated in education grants for science teaching including the Los Angeles Collaborative for Teaching Excellence (LACTE) and a Title III grant at her college. She speaks at conferences and educational meetings on the use of student-centered teaching methods in chemistry to promote the learning success of students.

Her husband, William Timberlake, who is the coauthor of this text, is Professor Emeritus of Chemistry at Los Angeles Harbor College, where he taught preparatory and organic chemistry for 36 years. He received his bachelor’s degree in chemistry from Carnegie Mellon University and his master’s degree in organic chemistry from the University of California at Los Angeles.

When the Professors Timberlake are not writing textbooks, they relax by playing tennis, ballroom dancing, hiking, traveling, trying new restaurants, cooking, and enjoying their grandchildren, Daniel and Emily.

1 Chemistry in Our Lives

1.1 Chemistry and Chemicals

1.2 Scientific Method: Thinking Like a Scientist

1.3 Studying and Learning Chemistry

1.4 Key Math Skills for Chemistry

1.5 Writing Numbers in Scientific Notation

2 Chemistry and Measurements

2.1 Units of Measurement

2.2 Measured Numbers and Significant Figures

2.3 Significant Figures in Calculations

2.4 Prefixes and Equalities

2.5 Writing Conversion Factors

2.6 Problem Solving Using Unit Conversion

2.7 Density

3 Matter and Energy

3.1 Classification of Matter

3.2 States and Properties of Matter

3.3 Temperature

3.4 Energy

3.5 Specific Heat

3.6 Energy and Nutrition

4 Atoms and Elements

4.1 Elements and Symbols

4.2 The Periodic Table

4.3 The Atom

4.4 Atomic Number and Mass Number

4.5 Isotopes and Atomic Mass

5 Electronic Structure of Atoms and Periodic Trends

5.1 Electromagnetic Radiation

5.2 Atomic Spectra and Energy Levels

5.3 Sublevels and Orbitals

5.4 Orbital Diagrams and Electron Configurations

5.5 Electron Configurations and the Periodic Table

5.6 Trends in Periodic Properties

6 Ionic and Molecular Compounds

6.1 Ions: Transfer of Electrons

6.2 Ionic Compounds

6.3 Naming and Writing Ionic Formulas

6.4 Polyatomic Ions

6.5 Molecular Compounds: Sharing Electrons

7 Chemical Quantities

7.1 The Mole

7.2 Molar Mass

7.3 Calculations Using Molar Mass

7.4 Mass Percent Composition

7.5 Empirical Formulas

7.6 Molecular Formulas

8 Chemical Reactions

8.1 Equations for Chemical Reactions

8.2 Balancing a Chemical Equation

8.3 Types of Chemical Reactions

8.4 Oxidation—Reduction Reactions

9 Chemical Quantities in Reactions

9.1 Conservation of Mass

9.2 Mole Relationships in Chemical Equations

9.3 Mass Calculations for Chemical Reactions

9.4 Limiting Reactants

9.5 Percent Yield

9.6 Energy in Chemical Reactions

10 Bonding and Properties of Solids and Liquids

10.1 Lewis Structures for Molecules and Polyatomic Ions

10.2 Resonance Structures

10.3 Shapes of Molecules and Polyatomic Ions (VSEPR Theory)

10.4 Electronegativity and Bond Polarity

10.5 Polarity of Molecules

10.6 Intermolecular Forces Between Atoms or Molecules

10.7 Changes of State

11 Gases

11.1 Properties of Gases

11.2 Pressure and Volume (Boyle’s Law)

11.3 Temperature and Volume (Charles’s Law)

11.4 Temperature and Pressure (Gay-Lussac’s Law)

11.5 The Combined Gas Law

11.6 Volume and Moles (Avogadro’s Law)

11.7 The Ideal Gas Law

11.8 Gas Laws and Chemical Reactions

11.9 Partial Pressures (Dalton’s Law)

12 Solutions

12.1 Solutions

12.2 Electrolytes and Nonelectrolytes

12.3 Solubility

12.4 Solution Concentrations

12.5 Dilution of Solutions

12.6 Chemical Reactions in Solution

12.7 Molality and Freezing Point Lowering/Boiling Point Elevation

12.8 Properties of Solutions: Osmosis

13 Reaction Rates and Chemical Equilibrium

13.1 Rates of Reactions

13.2 Chemical Equilibrium

13.3 Equilibrium Constants

13.4 Using Equilibrium Constants

13.5 Changing Equilibrium Conditions: Le Châtelier’s Principle

14 Acids and Bases

14.1 Acids and Bases

14.2 Brønsted—Lowry Acids and Bases

14.3 Strengths of Acids and Bases

14.4 Dissociation Constants of Weak Acids and Bases

14.5 Dissociation of Water

14.6 The pH Scale

14.7 Reactions of Acids and Bases

14.8 Acid—Base Titration

14.9 Buffers

15 Oxidation and Reduction

15.1 Oxidation and Reduction

15.2 Balancing Oxidation—Reduction Equations Using Half-Reactions

15.3 Electrical Energy from Oxidation—Reduction Reactions

15.4 Oxidation—Reduction Reactions That Require Electrical Energy

16 Nuclear Chemistry

16.1 Natural Radioactivity

16.2 Nuclear Reactions

16.3 Radiation Measurement

16.4 Half-Life of a Radioisotope

16.5 Medical Applications Using Radioactivity

16.6 Nuclear Fission and Fusion

17 Organic Chemistry

17.1 Alkanes

17.2 Alkenes, Alkynes, and Polymers

17.3 Aromatic Compounds

17.4 Alcohols and Ethers

17.5 Aldehydes and Ketones

17.6 Carboxylic Acids and Esters

17.7 Amines and Amides

18 Biochemistry

18.1 Carbohydrates

18.2 Disaccharides and Polysaccharides

18.3 Lipids

18.4 Amino Acids and Proteins

18.5 Protein Structure

18.6 Proteins as Enzymes

18.7 Nucleic Acids

18.8 Protein Synthesis

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