Introductory Chemistry Essentials

by Tro, Nivaldo J.

• ISBN13: 9780134291802
• ISBN10: 0134291808
• eBook ISBN(s): 9780135214305, 9780135214312
• Additional ISBN(s): 9780134565620, 9780136019916, 9780321919052
• Edition: 6th
• Format: Hardcover
• Copyright: 2017-01-04
• Publisher: PEARSO
• More Book Details

Summary

For one-semester courses in Preparatory Chemistry 

 

Builds 21st century and problem solving skills, preparing students for success

Now in its 6th Edition, the best-selling Introductory Chemistry continues to encourage student interest by showing how chemistry manifests in students’ daily lives. Author Nivaldo Tro draws upon his classroom experience as an award-winning instructor to extend chemistry from the laboratory to the student’s world, capturing student attention with relevant applications and an engaging writing style. The text provides a superior teaching and learning experience, enabling deep conceptual understanding, fostering the development of problem-solving skills, and encouraging interest in chemistry with concrete examples. Extending chemistry from the lab to the student’s world, the text reveals that anyone can master chemistry. 

 

Refined to meet its purpose of teaching relevant skills, the 6th Edition includes new questions, data, and sections to help students build the 21st century skills necessary to succeed in introductory chemistry and beyond. Already a visual text, in this edition the art has been further refined and improved, making the visual impact sharper and more targeted to student learning. The new edition also includes new Conceptual Checkpoints, a widely embraced feature that emphasizes understanding rather than calculation, as well as a new category of end-of-chapter questions called Data Interpretation and Analysis, which present real data in real life situations and ask students to analyze and interpret that data.

 

Also available as a Pearson eText or packaged with Mastering Chemistry

 

Pearson eText is a simple-to-use, mobile-optimized, personalized reading experience that can be adopted on its own as the main course material. It lets students highlight, take notes, and review key vocabulary all in one place, even when offline. Seamlessly integrated videos and other rich media engage students and give them access to the help they need, when they need it. Educators can easily share their own notes with students so they see the connection between their eText and what they learn in class – motivating them to keep reading, and keep learning.

 

Mastering combines trusted author content with digital tools and a flexible platform to personalize the learning experience and improve results for each student.Built for, and directly tied to the text, Mastering Chemistry enables an extension of learning, allowing students a platform to practice, learn, and apply outside of the classroom.

 

Note: You are purchasing a standalone book; Pearson eText and Mastering Chemistry do not come packaged with this content. Students, ask your instructor for the correct package ISBN and Course ID. Instructors, contact your Pearson representative for more information.

 

If your instructor has assigned Pearson eText as your main course material, search for:

• 0135214300 / 9780135214305 Pearson eText Introductory Chemistry Essentials, 6/e -- Access Card    

OR
•  0135214319 / 9780135214312 Pearson eText Introductory Chemistry Essentials, 6/e -- Instant Access

 

If you would like to purchase both the physical text and Mastering Chemistry, search for:

0134407636 / 9780134407630   Introductory Chemistry Essentials Plus Mastering Chemistry with eText -- Access Card Package

Package consists of:

• 0134291808 / 9780134291802  Introductory Chemistry Essentials

• 0134412753 / 9780134412757  Mastering Chemistry with Pearson eText -- ValuePack Access Card -- for Introductory Chemistry

Table of Contents

1 The Chemical World

1.1 Sand and Water

1.2 Chemicals Compose Ordinary Things

1.3 The Scientific Method: How Chemists Think

1.4 Analyzing and Interpreting Data

1.5 A Beginning Chemist: How to Succeed

 

2 Measurement and Problem Solving

2.1 The Metric Mix-up: A $125 Million Unit Error

2.2 Scientific Notation: Writing Large and Small Numbers

2.3 Significant Figures: Writing Numbers to Reflect Precision

2.4 Significant Figures in Calculations

2.5 The Basic Units of Measurement

2.6 Problem Solving and Unit Conversion

2.7 Solving Multistep Unit Conversion Problems

2.8 Unit Conversion in Both the Numerator and Denominator

2.9 Units Raised to a Power

2.10 Density

2.11 Numerical Problem-Solving Strategies and the Solution Map

 

3 Matter and Energy

3.1 In Your Room

3.2 What Is Matter?

3.3 Classifying Matter According to Its State: Solid, Liquid, and Gas

3.4 Classifying Matter According to Its Composition: Elements, Compounds, and Mixtures

3.5 Differences in Matter: Physical and Chemical Properties

3.6 Changes in Matter: Physical and Chemical Changes

3.7 Conservation of Mass: There Is No New Matter

3.8 Energy

3.9 Energy and Chemical and Physical Change

3.10 Temperature: Random Motion of Molecules and Atoms

3.11 Temperature Changes: Heat Capacity

3.12 Energy and Heat Capacity Calculations

 

4 Atoms and Elements

4.1 Experiencing Atoms at Tiburon

4.2 Indivisible: The Atomic Theory

4.3 The Nuclear Atom

4.4 The Properties of Protons, Neutrons, and Electrons

4.5 Elements: Defined by Their Numbers of Protons

4.6 Looking for Patterns: The Periodic Law and the Periodic Table

4.7 Ions: Losing and Gaining Electrons

4.8 Isotopes: When the Number of Neutrons Varies

4.9 Atomic Mass: The Average Mass of an Element’s Atoms

 

5 Molecules and Compounds

5.1 Sugar and Salt

5.2 Compounds Display Constant Composition

5.3 Chemical Formulas: How to Represent Compounds

5.4 A Molecular View of Elements and Compounds

5.5 Writing Formulas for Ionic Compounds

5.6 Nomenclature: Naming Compounds

5.7 Naming Ionic Compounds

5.8 Naming Molecular Compounds

5.9 Naming Acids

5.10 Nomenclature Summary

5.11 Formula Mass: The Mass of a Molecule or Formula Unit

 

6 Chemical Composition

6.1 How Much Sodium?

6.2 Counting Nails by the Pound

6.3 Counting Atoms by the Gram

6.4 Counting Molecules by the Gram

6.5 Chemical Formulas as Conversion Factors

6.6 Mass Percent Composition of Compounds

6.7 Mass Percent Composition from a Chemical Formula

6.8 Calculating Empirical Formulas for Compounds

6.9 Calculating Molecular Formulas for Compounds

 

7 Chemical Reactions

7.1 Grade School Volcanoes, Automobiles, and Laundry Detergents

7.2 Evidence of a Chemical Reaction

7.3 The Chemical Equation

7.4 How to Write Balanced Chemical Equations

7.5 Aqueous Solutions and Solubility: Compounds Dissolved in Water

7.6 Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid

7.7 Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations

7.8 Acid–Base and Gas Evolution Reactions

7.9 Oxidation–Reduction Reactions

7.10 Classifying Chemical Reactions

 

8 Quantities in Chemical Reactions

8.1 Climate Change: Too Much Carbon Dioxide

8.2 Making Pancakes: Relationships between Ingredients

8.3 Making Molecules: Mole-to-Mole Conversions

8.4 Making Molecules: Mass-to-Mass Conversions

8.5 More Pancakes: Limiting Reactant, Theoretical Yield, and Percent Yield

8.6 Limiting Reactant[JJ2] , Theoretical Yield, and Percent Yield from Initial Masses of Reactants

8.7 Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction

 

9 Electrons in Atoms and the Periodic Table

9.1 Blimps, Balloons, and Models of the Atom

9.2 Light: Electromagnetic Radiation

9.3 The Electromagnetic Spectrum

9.4 The Bohr Model: Atoms with Orbits

9.5 The Quantum-Mechanical Model: Atoms with Orbitals

9.6 Quantum-Mechanical Orbitals and Electron Configurations

9.7 Electron Configurations and the Periodic Table

9.8 The Explanatory Power of the Quantum-Mechanical Model

9.9 Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character

 

10 Chemical Bonding

10.1 Bonding Models and AIDS Drugs

10.2 Representing Valence Electrons with Dots

10.3 Lewis Structures of Ionic Compounds: Electrons Transferred

10.4 Covalent Lewis Structures: Electrons Shared

10.5 Writing Lewis Structures for Covalent Compounds

10.6 Resonance: Equivalent Lewis Structures for the Same Molecule

10.7 Predicting the Shapes of Molecules

10.8 Electronegativity and Polarity: Why Oil and Water Don’t Mix

 

11 Gases

11.1 Extra-Long Straws

11.2 Kinetic Molecular Theory: A Model for Gases

11.3 Pressure: The Result of Constant Molecular Collisions

11.4 Boyle’s Law: Pressure and Volume

11.5 Charles’s Law: Volume and Temperature

11.6 The Combined Gas Law: Pressure, Volume, and Temperature

11.7 Avogadro’s Law: Volume and Moles

11.8 The Ideal Gas Law: Pressure, Volume, Temperature, and Moles

11.9 Mixtures of Gases

11.10 Gases in Chemical Reactions

 

12 Liquids, Solids, and Intermolecular Forces

12.1 Spherical Water

12.2 Properties of Liquids and Solids

12.3 Intermolecular Forces in Action: Surface Tension and Viscosity

12.4 Evaporation and Condensation

12.5 Melting, Freezing, and Sublimation

12.6 Types of Intermolecular Forces: Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion–Dipole

12.7 Types of Crystalline Solids: Molecular, Ionic, and Atomic

12.8 Water: A Remarkable Molecule

 

13 Solutions

13.1 Tragedy in Cameroon

13.2 Solutions: Homogeneous Mixtures

13.3 Solutions of Solids Dissolved in Water: How to Make Rock Candy

13.4 Solutions of Gases in Water: How Soda Pop Gets Its Fizz

13.5 Specifying Solution Concentration: Mass Percent

13.6 Specifying Solution Concentration: Molarity

13.7 Solution Dilution

13.8 Solution Stoichiometry

13.9 Freezing Point Depression and Boiling Point Elevation: Making Water Freeze Colder and Boil Hotter

13.10 Osmosis: Why Drinking Saltwater Causes Dehydration

 

14 Acids and Bases

14.1 Sour Patch Kids and International Spy Movies

14.2 Acids: Properties and Examples

14.3 Bases: Properties and Examples

14.4 Molecular Definitions of Acids and Bases

14.5 Reactions of Acids and Bases

14.6 Acid–Base Titration: A Way to Quantify the Amount of Acid or Base in a Solution

14.7 Strong and Weak Acids and Bases

14.8 Water: Acid and Base in One

14.9 The pH and pOH Scales: Ways to Express Acidity and Basicity

14.10 Buffers: Solutions That Resist pH Change

 

15 Chemical Equilibrium

15.1 Life: Controlled Disequilibrium

15.2 The Rate of a Chemical Reaction

15.3 The Idea of Dynamic Chemical Equilibrium

15.4 The Equilibrium Constant: A Measure of How Far a Reaction Goes

15.5 Heterogeneous Equilibria: The Equilibrium Expression for Reactions Involving a Solid or a Liquid

15.6 Calculating and Using Equilibrium Constants

15.7 Disturbing a Reaction at Equilibrium: Le Châtelier’s Principle

15.8 The Effect of a Concentration Change on Equilibrium

15.9 The Effect of a Volume Change on Equilibrium

15.10 The Effect of a Temperature Change on Equilibrium

15.11 The Solubility-Product Constant

15.12 The Path of a Reaction and the Effect of a Catalyst

 

16 Oxidation and Reduction

16.1 The End of the Internal Combustion Engine?

16.2 Oxidation and Reduction: Some Definitions

16.3 Oxidation States: Electron Bookkeeping

16.4 Balancing Redox Equations

16.5 The Activity Series: Predicting Spontaneous Redox Reactions[JJ3]

16.6 Batteries: Using Chemistry to Generate Electricity

16.7 Electrolysis: Using Electricity to Do Chemistry

16.8 Corrosion: Undesirable Redox Reactions

 

17 Radioactivity and Nuclear Chemistry

17.1 Diagnosing Appendicitis

17.2 The Discovery of Radioactivity

17.3 Types of Radioactivity: Alpha, Beta, and Gamma Decay

17.4 Detecting Radioactivity

17.5 Natural Radioactivity and Half-Life

17.6 Radiocarbon Dating: Using Radioactivity to Measure the Age of Fossils and Other Artifacts

17.7 The Discovery of Fission and the Atomic Bomb

17.8 Nuclear Power: Using Fission to Generate Electricity

17.9 Nuclear Fusion: The Power of the Sun

17.10 The Effects of Radiation on Life

17.11 Radioactivity in Medicine