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Chapter 1
Chapter 1: The Chemical World 1.1: The Scope of Chemistry 1.2: Chemicals Compose Ordinary Things 1.3: Hypothesis, Theories, and Laws 1.4: The Scientific Method: How Chemists Think 1.5: A Beginning Chemist: How to Succeed
• Chapter 2
Chapter 2: Measurement and Problem Solving 2.1: Taking Measurements 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 Conversions 2.7: Solving Multistep Conversion Problems 2.8: Units Raised to a Power 2.9: Density 2.10: Numerical Problem-Solving Strategies and the Solution Map 2.E: Measurement and Problem Solving (Exercises)
• Chapter 3
Chapter 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 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 3.E: Exercises
• Chapter 4
Chapter 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
• Chapter 5
Chapter 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
• Chapter 6
Chapter 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
• Chapter 7
Chapter 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 7.11: The Activity Series
• Chapter 8
Chapter 8: Quantities in Chemical Reactions 8.1: Climate Change: Too Much Carbon Dioxide 8.2: Stoichiometry 8.3: Making Molecules: Mole-to-Mole Conversions 8.4: Making Molecules: Mass-to-Mass Conversions 8.5: Limiting Reactant, Theoretical Yield, and Percent Yield 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants 8.7: Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction
Chapter 9
Chapter 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
• Chapter 10
Chapter 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
• Chapter 11
Chapter 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: Gay-Lussac's Law: Temperature and Pressure 11.7: The Combined Gas Law: Pressure, Volume, and Temperature 11.8: Avogadro’s Law: Volume and Moles 11.9: The Ideal Gas Law: Pressure, Volume, Temperature, and Moles 11.10: Mixtures of Gases: Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen 11.11: Gases in Chemical Reactions
• Chapter 12
Chapter 12: Liquids, Solids, and Intermolecular Forces 12.1: Interactions between Molecules 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
• Chapter 13
Chapter 13: Solutions 13.1: Prelude - 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: Solution Concentration: Mass Percent 13.6: 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 Salt Water Causes Dehydration
• Chapter 14
Chapter 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
Chemistry is the study of matter and the ways in which different forms of matter combine with each other. You study chemistry because it helps you to understand the world around you. Everything you touch or taste or smell is a chemical, and the interactions of these chemicals with each other define our universe. Chemistry forms the fundamental basis for biology and medicine. From the structure of proteins and nucleic acids, to the design, synthesis and manufacture of drugs, chemistry allows you Chemistry is the branch of science dealing with the structure, composition, properties, and the reactive characteristics of matter. Matter is anything that has mass and occupies space. Thus, chemistry is the study of literally everything around us – the liquids that we drink, the gasses we breathe, the composition of everything from the plastic case on your phone to the earth beneath your feet. Moreover, chemistry is the study of the transformation of matter. Although all of us have taken science classes throughout the course of our study, many people have incorrect or misleading ideas about some of the most important and basic principles in science. We have all heard of hypotheses, theories, and laws, but what do they really mean? Before you read this section, think about what you have learned about these terms before. What do these terms mean to you? What do you read contradicts what you thought? What do you read supports what you thought? Science is a process of knowing about the natural universe through observation and experiment. Scientists go through a rigorous process to determine new knowledge about the universe; this process is generally referred to as the scientific method. Science is broken down into various fields, of which chemistry is one. Science, including chemistry, is both qualitative and quantitative. Most people can succeed in chemistry, but it often requires dedication, hard work, the right attitude and study habits!
