Introductory Chemistry: An Atoms First Approach

Hardcover | January 26, 2016

byJulia Burdge, Michelle Driessen

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Format:HardcoverDimensions:10.9 × 8.7 × 1.1 inPublished:January 26, 2016Publisher:McGraw-Hill EducationLanguage:English

The following ISBNs are associated with this title:

ISBN - 10:0073402702

ISBN - 13:9780073402703

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Table of Contents

Chapter 1 Atoms and Elements<_o3a_p>

1.1 The Study of Chemistry<_o3a_p>

1.2 Atoms First<_o3a_p>

1.3 Subatomic Particles and the Nuclear Model of the Atom<_o3a_p>

1.4 Elements and the Periodic Table<_o3a_p>

1.5 Organization of the Periodic Table<_o3a_p>

1.6 Isotopes<_o3a_p>

1.7 Atomic Mass<_o3a_p>

<_o3a_p> 

Chapter 2 Electrons and the Periodic Table<_o3a_p>

2.1 The Nature of Light<_o3a_p>

2.2 The Bohr Atom<_o3a_p>

2.3 Atomic Orbitals<_o3a_p>

2.4 Electron Configurations<_o3a_p>

2.5 Electron Configurations and the Periodic Table<_o3a_p>

2.6 Periodic Trends<_o3a_p>

2.7 Ions: The Loss and Gain of Electrons<_o3a_p>

<_o3a_p> 

Chapter 3 Compounds and Chemical Bonds<_o3a_p>

3.1 Matter: Classification and Properties<_o3a_p>

3.2 Ionic Bonding and Binary Ionic Compounds<_o3a_p>

3.3 Naming Ions and Binary Ionic Compounds<_o3a_p>

3.4 Covalent Bonding and Molecules<_o3a_p>

3.5 Naming Binary Molecular Compounds<_o3a_p>

3.6 Covalent Bonding in Ionic Species: Polyatomic Ions<_o3a_p>

3.7 Acids<_o3a_p>

3.8 Substances in Review<_o3a_p>

<_o3a_p> 

Chapter 4 How Chemists Use Numbers<_o3a_p>

4.1 Units of Measurement<_o3a_p>

4.2 Scientific Notation<_o3a_p>

4.3 Significant Figures<_o3a_p>

4.4 Unit Conversion<_o3a_p>

4.5 Success in Introductory Chemistry Class<_o3a_p>

<_o3a_p> 

Chapter 5 The Mole and Chemical Formulas<_o3a_p>

5.1 Counting Atoms by Weighing<_o3a_p>

5.2 Counting Molecules by Weighing<_o3a_p>

5.3 Mass Percent Composition<_o3a_p>

5.4 Using Mass Percent Composition to Determine Empirical Formula<_o3a_p>

5.5 Using Empirical Formula and Molar Mass to Determine Molecular Formula<_o3a_p>

<_o3a_p> 

Chapter 6 Molecular Shape<_o3a_p>

6.1 Drawing Simple Lewis Structures<_o3a_p>

6.2 Lewis Structures Continued<_o3a_p>

6.3 Resonance Structures<_o3a_p>

6.4 Molecular Shape<_o3a_p>

6.5 Electronegativity & Polarity<_o3a_p>

6.6 Intermolecular Forces<_o3a_p>

<_o3a_p> 

Chapter 7 Solids, Liquids, and Phase Changes<_o3a_p>

7.1 General Properties of the Condensed Phases<_o3a_p>

7.2 Types of Solids<_o3a_p>

7.3 Physical Properties of Solids<_o3a_p>

7.4 Physical Properties of Liquids<_o3a_p>

7.5 Energy and Physical Changes<_o3a_p>

<_o3a_p> 

Chapter 8 Gases<_o3a_p>

8.1 Properties of Gases<_o3a_p>

8.2 Pressure<_o3a_p>

8.3 The Gas Equations<_o3a_p>

8.4 The Gas Laws<_o3a_p>

8.5 Gas Mixtures<_o3a_p>

<_o3a_p> 

Chapter 9 Physical Properties of Solutions <_o3a_p>

9.1 General Properties of Solutions<_o3a_p>

9.2 Aqueous Solubility<_o3a_p>

9.3 Solution Concentration<_o3a_p>

9.4 Solution Composition<_o3a_p>

9.5 Solution Preparation<_o3a_p>

9.6 Colligative Properties<_o3a_p>

<_o3a_p> 

Chapter 10 Chemical Reactions and Chemical Equations<_o3a_p>

10.1 Recognizing Chemical Reactions<_o3a_p>

10.2 Representing Chemical Reactions with Chemical Equations<_o3a_p>

10.3 Balancing Chemical Equations<_o3a_p>

10.4 Types of Chemical Reactions<_o3a_p>

10.5 Chemical Reactions and Energy<_o3a_p>

10.6 Chemical Reactions in Review<_o3a_p>

<_o3a_p> 

Chapter 11 Using Balanced Chemical Equations<_o3a_p>

11.1 Mole to Mole Conversions<_o3a_p>

11.2 Mass to Mass Conversions<_o3a_p>

11.3 Limitations on Reaction Yield<_o3a_p>

11.4 Aqueous Reactions<_o3a_p>

11.5 Gases in Chemical Reactions<_o3a_p>

11.6 Chemical Reactions and Heat<_o3a_p>

<_o3a_p> 

Chapter 12 Acids and Bases<_o3a_p>

12.1 Properties of Acids and Bases<_o3a_p>

12.2 Definitions of Acids and Bases<_o3a_p>

12.3 Water as an Acid; Water as a Base<_o3a_p>

12.4 Strong Acids and Bases<_o3a_p>

12.5 pH and pOH Scales<_o3a_p>

12.6 Weak Acids and Bases<_o3a_p>

12.7 Acid-Base Titrations<_o3a_p>

12.8 Buffers<_o3a_p>

<_o3a_p> 

Chapter 13 Equilibrium<_o3a_p>

13.1 Reaction Rates<_o3a_p>

13.2 Chemical Equilibrium<_o3a_p>

13.3 Equilibrium Constants<_o3a_p>

13.4 Factors that Affect Equilibrium<_o3a_p>

<_o3a_p> 

Chapter 14 Organic Chemistry<_o3a_p>

14.1 Why Carbon is Different<_o3a_p>

14.2 Hydrocarbons<_o3a_p>

14.3 Isomers<_o3a_p>

14.4 Functional Groups<_o3a_p>

14.5 Alcohols and Ethers<_o3a_p>

14.6 Aldehydes & Ketones<_o3a_p>

14.7 Carboxylic Acids and Esters<_o3a_p>

14.8 Amines and Amides<_o3a_p>

14.9 Polymers<_o3a_p>

<_o3a_p> 

Chapter 15 Biochemistry<_o3a_p>

15.1 Biologically Important Molecules<_o3a_p>

15.2 Lipids<_o3a_p>

15.3 Proteins<_o3a_p>

15.4 Carbohydrates<_o3a_p>

15.5 Nucleic Acids<_o3a_p>

<_o3a_p> 

Chapter 16 Nuclear Chemistry<_o3a_p>

16.1 Radioactive Decay<_o3a_p>

16.2 Detection of Radiation and its Biological Effects<_o3a_p>

16.3 Dating using Radioactive Decay<_o3a_p>

16.4 Medical Applications of Radioactivity<_o3a_p>

16.5 Nuclear Fission and Nuclear Fusion<_o3a_p>

<_o3a_p> 

Chapter 17 Electrochemistry<_o3a_p>

17.1 Balancing Oxidation-Reduction Reactions using the Half-Reaction Method<_o3a_p>

17.2 Batteries<_o3a_p>

17.3 Corrosion<_o3a_p>

17.4 Electrolysis<_o3a_p>