U Can, 1 by Moore, John T. -- Read -- Imperial Library of Trantor

Index

Cover Title Page Table of Contents Introduction

About This Book Foolish Assumptions Beyond the Book Where to Go from Here

Part I: Getting Started with Chemistry

Chapter 1: Looking at Numbers Scientifically

Using Exponential and Scientific Notation to Report Measurements Multiplying and Dividing in Scientific Notation Using Scientific Notation to Add and Subtract Distinguishing between Accuracy and Precision Identifying Significant Figures Doing Arithmetic with Significant Figures

Chapter 2: Using and Converting Units

Familiarizing Yourself with Base Units and Metric System Prefixes Looking at Density Using Conversion Factors Working with the Factor Label Method

Chapter 3: Breaking Down Atoms into Their Subatomic Particles

The Atom: Protons, Electrons, and Neutrons A Brief History of the Atom Deciphering Chemical Symbols: Atomic and Mass Numbers Accounting for Isotopes Using Atomic Masses

Chapter 4: Surveying the Periodic Table of the Elements

Organizing the Periodic Table Putting Electrons in Their Places: Electron Configurations Quantifying Quantum Numbers Predicting Properties and Valence Electrons from Periodic Trends Forming Ions Measuring the Amount of Energy (or Light) an Excited Electron Emits

Part II: M aking and Breaking Bonds through Reactions

Chapter 5: Building Bonds

Pairing Charges with Ionic Bonds Forming Sodium Chloride Ionic Salts Sharing Electrons with Covalent Bonds Drawing the Structural Formulas of Molecules Occupying and Overlapping Molecular Orbitals Polarity: Sharing Electrons Unevenly Shaping Molecules: VSEPR Theory and Hybridization Wondering About Water and Intermolecular Forces

Chapter 6: Naming Compounds and Writing Formulas

Labeling Ionic Compounds and Writing Their Formulas Getting a Grip on Ionic Compounds with Polyatomic Ions Naming Covalent Compounds and Writing Their Formulas Addressing Acids Mixing the Rules for Naming and Formula Writing Beyond the Basics: Naming Organic Carbon Chains

Chapter 7: Understanding the Many Uses of the Mole

The Mole Conversion Factor: Avogadro’s Number Doing Mass and Volume Mole Conversions Determining Percent Composition Calculating Empirical Formulas Using Empirical Formulas to Find Molecular Formulas

Chapter 8: Getting a Grip on Chemical Equations

Translating Chemistry into Equations and Symbols Understanding How Reactions Occur Balancing Chemical Equations Recognizing Reactions and Predicting Products Canceling Spectator Ions: Net Ionic Equations

Chapter 9: Putting Stoichiometry to Work

Using Mole-Mole Conversions from Balanced Equations Putting Moles at the Center: Conversions Involving Particles, Volumes, and Masses Limiting Your Reagents Counting Your Chickens after They’ve Hatched: Percent Yield Calculations

Part III: Examining Changes in Energy and Solutions

Chapter 10: Understanding States of Matter in Terms of Energy

Describing States of Matter and Their Phase Changes Changing States of Matter Classifying Pure Substances and Mixtures Nice Properties You’ve Got There Taking a Look at Energy and Temperature Measuring Energy Figuring Out Phase Diagrams

Chapter 11: Warming Up to Thermochemistry

Understanding the Basics of Thermodynamics Working with Specific Heat Capacity and Calorimetry Absorbing and Releasing Heat: Endothermic and Exothermic Reactions Summing Heats with Hess’s Law

Chapter 12: Obeying Gas Laws

Working with the Kinetic Molecular Theory Measuring and Converting Pressure Boyle’s Law: Playing with Pressure and Volume Charles’s Law and Absolute Zero: Looking at Volume and Temperature Gay-Lussac’s Law: Examining Pressure and Temperature Combining Pressure, Temperature, and Volume into One Law Dealing with Amounts: Avogadro’s Law and the Ideal Gas Law Mixing It Up with Dalton’s Law of Partial Pressures Diffusing and Effusing with Graham’s Law

Chapter 13: Dissolving into Solutions

Seeing Different Forces at Work in Solubility Concentrating on Molarity and Percent Solutions Changing Concentrations by Making Dilutions Altering Solubility with Temperature

Chapter 14: Playing Hot and Cold: Colligative Properties

Portioning Particles: Molality and Mole Fractions Too Hot to Handle: Elevating and Calculating Boiling Points How Low Can You Go? Depressing and Calculating Freezing Points Determining Molecular Masses with Boiling and Freezing Points

Chapter 15: Working with Acids and Bases

Getting to Know Acids and Bases Acids and Bases at the Atomic Level Measuring Acidity and Basicity: pH, pOH, and KW Dissociating with Strong and Weak Acids

Chapter 16: Achieving Neutrality with Titrations and Buffers

Using Indicators and Titration to Figure Out Molarity Maintaining Your pH with Buffers Measuring Salt Solubility with KSP

Part IV: Reaching Equilibrium

Chapter 17: Exploring Rates and Equilibrium

Measuring Rates Focusing on Factors that Affect Rates Measuring Equilibrium

Chapter 18: Accounting for Electrons in Redox

Oxidation Numbers: Keeping Tabs on Electrons Balancing Redox Reactions under Acidic Conditions Balancing Redox Reactions under Basic Conditions

Chapter 19: Galvanizing Yourself to Do Electrochemistry

Identifying Anodes and Cathodes Calculating Electromotive Force and Standard Reduction Potentials Coupling Current to Chemistry: Electrolytic Cells

Chapter 20: Doing Chemistry with Atomic Nuclei

Decaying Nuclei in Different Ways Measuring Rates of Decay: Half-Lives Making and Breaking Nuclei: Fusion and Fission

Part V: The Part of Tens

Chapter 21: Ten Tips for Acing a Chemistry Test

Don’t Cram Figure Out What Is Probably on the Test Allocate Your Study Time Wisely Know the Basics Do Example Problems Be Confident Spend Time with the Numbers Know Your Resources Eat and Sleep Don’t Get Discouraged

Chapter 22: Ten Chemistry Formulas You Should Remember

The Combined Gas Law Dalton’s Law of Partial Pressures The Dilution Equation Rate Laws The Equilibrium Constant Free Energy Change Constant-Pressure Calorimetry Hess’s Law pH, pOH, and KW KA and KB

Chapter 23: Ten Annoying Exceptions to Chemistry Rules

Hydrogen Isn’t an Alkali Metal The Octet Rule Isn’t Always an Option Some Electron Configurations Ignore the Orbital Rules One Partner in a Coordinate Covalent Bond Giveth Electrons; the Other Taketh All Hybridized Orbitals Are Created Equal Use Caution When Naming Compounds with Transition Metals You Must Memorize Polyatomic Ions Liquid Water Is Denser Than Ice No Gas Is Truly Ideal Common Names for Organic Compounds Hearken Back to the Old Days

Chapter 24: Ten (Or So) Great Chemists

Amedeo Avogadro Niels Bohr Marie Curie John Dalton Michael Faraday Antoine Lavoisier Dmitri Mendeleev Linus Pauling Ernest Rutherford Glenn Seaborg That Third-Grader Experimenting with Vinegar and Baking Soda

Chapter 25: Ten Serendipitous Discoveries in Chemistry

Taking the Measure of Volume Keeping Rubber Solid Right- and Left-Handed Molecules Finding a Shortcut to Color: Artificial Dye Dreaming Up the Ring Structure Discovering Radioactivity Finding Really Slick Stuff: Teflon Stick ’Em Up! Sticky Notes Growing Hair Speaking of Sweet Somethings

Glossary About the Authors Cheat Sheet Advertisement Page Connect with Dummies End User License Agreement

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