Achieve for Interactive General Chemistry 2.0 Atoms First (1-Term Access)

CHAPTER 0 Math Review
0.1  Using a Calculator
0.2  Exponents and Scientific Notation
0.3  Order of Operations
0.4  Algebra
0.5  Logarithms and Antilogs
0.6  Percentage
0.7  Interpreting a Graph
0.8  Proportionality
0.9  Weighted Average
0.1  The Quadratic Formula

CHAPTER 1 Matter and Measurement
1.1 Classification of Matter
1.2  Properties of Matter
1.3  Matter and Energy
1.4  The Scientific Method, Hypotheses, Theories, and Laws
1.5  The International System of Units
1.6  Significant Digits
1.7  Dimensional Analysis
1.8  Density
1.9  Temperature Scales

CHAPTER 2 Atoms and the Periodic Table
2.1 Chemical Symbols
2.2 The Laws of Chemical Combination
2.3 The History of the atom
2.4 Subatomic Particles, Isotopes, and Ions
2.5 Atomic Mass
2.6 The Periodic Table
2.7 The Mole

CHAPTER 3 The Quantum Model of the Atom and Periodicity
3.1 A Brief Exploration of Light
3.2 The Bohr Model of the Atom
3.3 Wave-Particle Duality of Matter
3.4 Orbitals and Quantum Numbers
3.5 Shapes of Orbitals
3.6 Orbital Diagrams
3.7 Electron Configurations
3.8 Valence Electrons
3.9 Atomic and Ionic Sizes
3.10 Ionization Energy and Electron Affinity

CHAPTER 4 Nomenclature
4.1  Chemical Formulas
4.2  Naming Binary Covalent Compounds
4.3  Formulas for Ionic Compounds
4.4  Naming Ionic Compounds
4.5  Naming Acids
4.6  Nomenclature Review

CHAPTER 5 Compounds
5.1  Molar Mass
5.2  Percent Composition
5.3  Empirical Formulas
5.4  Molecular Formulas
5.5  Combustion Analysis

CHAPTER 6 Covalent Bonding
6.1 Ionic Bonding
6.2 Covalent Bonding
6.2  Lewis Structures
6.3  Resonance and Formal Charges
6.4  Exceptions to the Octet Rule
6.5  Polar Bonds and the Bonding Continuum

CHAPTER 7 Molecular Shape and Bonding Theories
7.1  VSEPR and Molecular Geometry
7.2  Polar and Nonpolar Molecules
7.3  Valence Bond Theory: Hybrid Orbitals and Bonding
7.4  Using Valence Bond Theory
7.5  Molecular Orbital Theory

CHAPTER 8 Chemical Reactions and Aqueous Solutions
8.1  Chemical Equations
8.2  Types of Chemical Reactions
8.3  Compounds in Aqueous Solution
8.4  Precipitation Reactions
8.5  Acid–Base Reactions
8.6  Oxidation States and Redox Reactions
8.7  Predicting Products of Redox Reactions

CHAPTER 9 Stoichiometry
9.1  Mole Calculations for Chemical Reactions
9.2  Mass Calculations for Chemical Reactions
9.3  Problems Involving Limiting Quantities
9.4  Theoretical Yield and Percent Yield
9.5  Definition and Uses of Molarity
9.6  Molarities of Ions
9.7  Calculations Involving Other Quantities
9.8  Calculations with Net Ionic Equations
9.9  Titration

CHAPTER 10 Thermochemistry
10.1  Energy and Energy Units
10.2  Energy, Heat, and Work
10.3  Energy as a State Function
10.4  Energy and Enthalpy
10.5  Specific Heat
10.6  Calorimetry: Measuring Energy Changes
10.7  Enthalpy in Chemical Reactions
10.8  Standard Enthalpies of Formation
10.9 Lattice Energy
10.10 Bond Enthalpy

CHAPTER 11 Gases
11.1  Gas Pressure
11.2  Boyles Law
11.3  Charless Law
11.4  The Combined Gas Law
11.5  Avogadros Law
11.6  The Ideal Gas Law
11.7  Daltons Law of Partial Pressures
11.8  Molar Mass and Density in Gas Law Calculations
11.9  Gases in Chemical Reactions
11.1  Kinetic Molecular Theory of Gases
11.11  Movement of Gas Particles
11.12  Behavior of Real Gases

CHAPTER 12 Liquids and Solids
12.1  Intermolecular Forces
12.2  Properties of Liquids
12.3  Phase Changes and Heating Curves
12.4  Vapor Pressure, Boiling Point, and the Clausius–Clapeyron Equation
12.5  Phase Diagrams
12.6  Classification of Solids
12.7  The Unit Cell and the Structure of Crystalline Solids

CHAPTER 13 Solutions
13.1  The Solution Process
13.2  Saturated Unsaturated, and Supersaturated Solutions
13.3  Concentration Units
13.4  Colligative Properties of Nonelectrolytes
13.5  Colligative Properties of Electrolytes

CHAPTER 14 Chemical Kinetics
14.1  Rates of Reactions
14.2  Reaction Rates and Concentration: Rate Laws
14.3  Integrated Rate Laws and Half-Lives
14.4  Reaction Rates and Temperature: Activation Energy
14.5  Reaction Mechanisms
14.6  Catalysis

CHAPTER 15 Chemical Equilibrium
15.1  Introduction to Equilibrium
15.2  Equilibrium Constants
15.3  Using Equilibrium Expressions
15.4  The Reaction Quotient
15.5  Calculations Using ICE Tables
15.6  Le Châteliers Principle

CHAPTER 16 Acids and Bases
16.1  Ionization Reactions of Acids and Bases
16.2  Brønsted–Lowry Theory
16.3  Autoionization of Water
16.4  pH Calculations
16.5  Weak Acids and Bases
16.6  Polyprotic Acids
16.7  Acid–Base Properties of Salts
16.8  Relating Acid Strength to Structure
16.9  Lewis Acids and Bases

CHAPTER 17 Aqueous Equilibria
17.1  Introduction to Buffer Solutions
17.2  The Henderson–Hasselbalch Equation
17.3  Titrations of Strong Acids and Strong Bases
17.4  Titrations of Weak Acids and Weak Bases
17.5  Indicators in Acid–Base Reactions
17.6  Solubility Product Constant, Ksp
17.7  The Common Ion Effect and the Effect of pH on Solubility
17.8  Precipitation: Ksp versus Q
17.9  Qualitative Analysis
17.10  Complex Ion Equiliria: Kf

CHAPTER 18 Chemical Thermodynamics
18.1  Entropy and Spontaneity
18.2  Entropy Changes–Both Chemical and Physical
18.3  Entropy and Temperatures
18.4  Gibbs Free Energy
18.5  Free Energy Changes and Temperature
18.6  Gibbs Free Energy and Equilibrium

CHAPTER 19 Electrochemistry
19.1  Redox Reactions
19.2  Balancing Redox Equations
19.3  Redox Titrations
19.4  Voltaic Cells
19.5  Cell Potentials
19.6  Free Energy and Cell Potential
19.7  The Nernst Equation and Concentration Cells
19.8  Voltaic Cell applications: Batteries, Fuel Cells, and Corrosion
19.9  Electrolytic Cells and Applications of Electrolysis

CHAPTER 20 Nuclear Chemistry
20.1  Natural Radioactivity
20.2  Nuclear Stability
20.3  Half-life
20.4  Radiometric Dating
20.5  Nuclear Fission and Fusion
20.6  Energetics of Nuclear Reactions
20.7  Nuclear Binding energy

CHAPTER 21 Organic Chemistry
21.1  Introduction to Hydrocarbons
21.2  Unsaturated Hydrocarbons
21.3  Introduction to Isomerism
21.4  Organic Halides, Alcohols, Ethers, and Amines
21.5  Aldehydes, Ketones, Carboxylic Acids, Esters, and Amides
21.6  Polymers

CHAPTER 22 Coordination Chemistry
22.1  Review of Using Oxidation Numbers in Naming Compounds
22.2  The Properties of Transition Metals
22.3  Introduction to Coordination Compounds
22.4  Nomenclature of Coordination Compounds
22.5  Isomerism in Complex Ions
22.6  Crystal Field Theory
22.7  Color, Magnetism, and the Spectrochemical series

CHAPTER 23 Biochemistry
23.1  Introduction to Biomolecules
23.2  Carbohydrates
23.3  Lipids
23.4  Amino Acids, Peptides, and Proteins
23.5  Nucleic Acids and Protein Synthesis

A Appendix
A.1  Periodic Table of the Elements
A.2  Thermodynamic Properties at 298 K
A.3  Ionization Constants for Acids and Bases
A.4  Solubility-Product Constants at 298 K
A.5  Standard Reduction Potentials at 298 K