Chemistry 6th edition

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John McMurry and Robert C. Fay
Publisher: Pearson Education


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  • Chapter 1: Chemistry: Matter and Measurement
    • 1: Key Concept Problems (1)
    • 1: Conceptual Problems (5)
    • 1.1: Approaching Chemistry: Experimentation
    • 1.2: Chemistry and the Elements
    • 1.3: Elements and the Periodic Table
    • 1.4: Some Chemical Properties of the Elements (15)
    • 1.5: Experimentation and Measurement
    • 1.6: Mass and Its Measurement
    • 1.7: Length and Its Measurement
    • 1.8: Temperature and Its Measurement (6)
    • 1.9: Derived Units: Volume and Its Measurement
    • 1.10: Derived Units: Density and Its Measurement (4)
    • 1.11: Derived Units: Energy and Its Measurement (1)
    • 1.12: Accuracy, Precision, and Significant Figures in Measurement
    • 1.13: Rounding Numbers (16)
    • 1.14: Calculations: Converting from One Unit to Another (7)
    • 1: Chapter Problems (10)
    • WebAssign Answer Entry Tutorials (1)

  • Chapter 2: Atoms, Molecules, and Ions
    • 2: Key Concept Problems (1)
    • 2: Conceptual Problems (5)
    • 2.1: The Conservation of Mass and the Law of Definite Proportions
    • 2.2: The Law of Multiple Proportions and Dalton's Atomic Theory (9)
    • 2.3: Atomic Structure: Electrons
    • 2.4: Atomic Structure: Protons and Neutrons
    • 2.5: Atomic Numbers
    • 2.6: Atomic Masses and the Mole (14)
    • 2.7: Nuclear Chemistry: The Change of One Element into Another
    • 2.8: Radioactivity
    • 2.9: Nuclear Stability (5)
    • 2.10: Mixtures and Chemical Compounds; Molecules and Covalent Bonds
    • 2.11: Ions and Ionic Bonds (12)
    • 2.12: Naming Chemical Compounds (5)
    • 2: Chapter Problems (7)
    • WebAssign Answer Entry Tutorials (1)

  • Chapter 3: Mass Relationships in Chemical Reactions
    • 3: Key Concept Problems (1)
    • 3: Conceptual Problems (4)
    • 3.1: Balancing Chemical Equations (2)
    • 3.2: Representing Chemistry on Different Levels
    • 3.3: Chemical Arithmetic: Stoichiometry (7)
    • 3.4: Yields of Chemical Reactions
    • 3.5: Reactions with Limiting Amounts of Reactants (2)
    • 3.6: Concentrations of Reactants in Solution: Molarity
    • 3.7: Diluting Concentrated Solutions
    • 3.8: Solution Stoichiometry
    • 3.9: Titration (4)
    • 3.10: Percent Composition and Empirical Formulas
    • 3.11: Determining Empirical Formulas: Elemental Analysis (3)
    • 3.12: Determining Molecular Masses: Mass Spectrometry
    • 3: Chapter Problems (2)
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  • Chapter 4: Reactions in Aqueous Solution
    • 4: Key Concept Problems (3)
    • 4: Conceptual Problems (3)
    • 4.1: Some Ways that Chemical Reactions Occur
    • 4.2: Electrolytes in Aqueous Solution
    • 4.3: Aqueous Reactions and Net Ionic Equations (2)
    • 4.4: Precipitation Reactions and Solubility Guidelines (1)
    • 4.5: Acids, Bases, and Neutralization Reactions
    • 4.6: Oxidation—Reduction (Redox) Reactions
    • 4.7: Identifying Redox Reactions
    • 4.8: The Activity Series of the Elements (4)
    • 4.9: Balancing Redox Reactions: The Half-Reaction Method (3)
    • 4.10: Redox Stoichiometry (4)
    • 4.11: Some Applications of Redox Reactions
    • 4: Chapter Problems
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  • Chapter 5: Periodicity and the Electronic Structure of Atoms
    • 5: Key Concept Problems (1)
    • 5: Conceptual Problems (3)
    • 5.1: Light and the Electromagnetic Spectrum
    • 5.2: Electromagnetic Energy and Atomic Line Spectra
    • 5.3: Particlelike Properties of Electromagnetic Energy (3)
    • 5.4: Wavelike Properties of Matter
    • 5.5: Quantum Mechanics and the Heisenberg Uncertainty Principle (1)
    • 5.6: Wave Functions and Quantum Numbers
    • 5.7: The Shapes of Orbitals
    • 5.8: Quantum Mechanics and Atomic Line Spectra
    • 5.9: Electron Spin and the Pauli Exclusion Principle (3)
    • 5.10: Orbital Energy Levels in Multielectron Atoms
    • 5.11: Electron Configurations of Multielectron Atoms
    • 5.12: Some Anomalous Electron Configurations
    • 5.13: Electron Configurations and the Periodic Table (3)
    • 5.14: Electron Configurations and Periodic Properties: Atomic Radii (2)
    • 5: Chapter Problems
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  • Chapter 6: Ionic Bonds and Some Main—Group Chemistry
    • 6: Key Concept Problems
    • 6: Conceptual Problems (4)
    • 6.1: Electron Configurations of Ions
    • 6.2: Ionic Radii
    • 6.3: Ionization Energy
    • 6.4: Higher Ionization Energies
    • 6.5: Electron Affinity (8)
    • 6.6: The Octet Rule
    • 6.7: Ionic Bonds and the Formation of Ionic Solids
    • 6.8: Lattice Energies in Ionic Solids (3)
    • 6.9: Some Chemistry of the Alkali Metals
    • 6.10: Some Chemistry of the Alkaline-Earth Metals
    • 6.11: Some Chemistry of the Halogens
    • 6.12: Some Chemistry of the Noble Gases
    • 6: Chapter Problems (1)
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  • Chapter 7: Covalent Bonds and Molecular Structure
    • 7: Key Concept Problems
    • 7: Conceptual Problems (1)
    • 7.1: Covalent Bonding in Molecules
    • 7.2: Strengths of Covalent Bonds
    • 7.3: A Comparison of Ionic and Covalent Compounds
    • 7.4: Polar Covalent Bonds: Electronegativity (2)
    • 7.5: Electron–Dot Structures
    • 7.6: Electron–Dot Structures of Polyatomic Molecules
    • 7.7: Electron–Dot Structures and Resonance (9)
    • 7.8: Formal Charges (6)
    • 7.9: Molecular Shapes: The VSEPR Model (4)
    • 7.10: Valence Bond Theory
    • 7.11: Hybridization and sp3 Hybrid Orbitals
    • 7.12: Other Kinds of Hybrid Orbitals
    • 7.13: Molecular Orbital Theory: The Hydrogen Molecule
    • 7.14: Molecular Orbital Theory: Other Diatomic Molecules
    • 7.15: Combining Valence Bond Theory and Molecular Orbital Theory (3)
    • 7: Chapter Problems (10)
    • WebAssign Answer Entry Tutorials (2)

  • Chapter 8: Thermochemistry: Chemical Energy
    • 8: Key Concept Problems
    • 8: Conceptual Problems (2)
    • 8.1: Energy and Its Conservation
    • 8.2: Internal Energy and State Functions
    • 8.3: Expansion Work (2)
    • 8.4: Energy and Enthalpy
    • 8.5: The Thermodynamic Standard State
    • 8.6: Enthalpies of Physical and Chemical Change (4)
    • 8.7: Calorimetry and Heat Capacity (3)
    • 8.8: Hess's Law
    • 8.9: Standard Heats of Formation (2)
    • 8.10: Bond Dissociation Energies (1)
    • 8.11: Fossil Fuels, Fuel Efficiency, and Heats of Combustion
    • 8.12: An Introduction to Entropy
    • 8.13: An Introduction to Free Energy (4)
    • 8: Chapter Problems (1)
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  • Chapter 9: Gases: Their Properties and Behavior
    • 9: Key Concept Problems
    • 9: Conceptual Problems (3)
    • 9.1: Gases and Gas Pressure (1)
    • 9.2: The Gas Laws
    • 9.3: The Ideal Gas Law (4)
    • 9.4: Stoichiometric Relationships with Gases (3)
    • 9.5: Partial Pressure and Dalton's Law (1)
    • 9.6: The Kinetic—Molecular Theory of Gases
    • 9.7: Graham's Law: Diffusion and Effusion of Gases (2)
    • 9.8: The Behavior of Real Gases
    • 9.9: The Earth's Atmosphere
    • 9: Chapter Problems (1)
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  • Chapter 10: Liquids, Solids, and Phase Changes
    • 10: Key Concept Problems (2)
    • 10: Conceptual Problems (3)
    • 10.1: Polar Covalent Bonds and Dipole Moments
    • 10.2: Intermolecular Forces
    • 10.3: Some Properties of Liquids (2)
    • 10.4: Phase Changes
    • 10.5: Evaporation, Vapor Pressure, and Boiling Point (4)
    • 10.6: Kinds of Solids
    • 10.7: Probing the Structure of Solids: X-Ray Crystallography
    • 10.8: Unit Cells and the Packing of Spheres in Crystalline Solids
    • 10.9: Unit Cells and the Packing of Spheres in Crystalline Solids (2)
    • 10.10: Unit Cells and the Packing of Spheres in Crystalline Solids
    • 10.11: Phase Diagrams (1)
    • 10: Chapter Problems (2)
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  • Chapter 11: Solutions and Their Properties
    • 11: Key Concept Problems
    • 11: Conceptual Problems (3)
    • 11.1: Solutions
    • 11.2: Energy Changes and the Solution Process (4)
    • 11.3: Units of Concentration (11)
    • 11.4: Some Factors Affecting Solubility (2)
    • 11.5: Physical Behavior of Solutions: Colligative Properties
    • 11.6: Vapor—Pressure Lowering of Solutions: Raoult's Law
    • 11.7: Boiling—Point Elevation and Freezing—Point Depression of Solutions
    • 11.8: Osmosis and Osmotic Pressure (10)
    • 11.9: Some Uses of Colligative Properties (2)
    • 11.10: Fractional Distillation of Liquid Mixtures
    • 11: Chapter Problems (5)
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  • Chapter 12: Chemical Kinetics
    • 12: Key Concept Problems (1)
    • 12: Conceptual Problems (5)
    • 12.1: Reaction Rates (1)
    • 12.2: Rate Laws and Reaction Order
    • 12.3: Experimental Determination of a Rate Law (2)
    • 12.4: Integrated Rate Law for a First-Order Reaction (7)
    • 12.5: Half—Life of a First-Order Reaction
    • 12.6: Radioactive Decay Rates (4)
    • 12.7: Second—Order Reactions
    • 12.8: Zeroth—Order Reactions
    • 12.9: Reaction Mechanisms
    • 12.10: Rate Laws for Elementary Reactions
    • 12.11: Rate Laws for Overall Reactions (6)
    • 12.12: Reaction Rates and Temperature: The Arrhenius Equation
    • 12.13: Using the Arrhenius Equation (3)
    • 12.14: Catalysis
    • 12.15: Homogeneous and Heterogeneous Catalysts (4)
    • 12: Chapter Problems (7)
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  • Chapter 13: Chemical Equilibrium
    • 13: Key Concept Problems
    • 13: Conceptual Problems (3)
    • 13.1: The Equilibrium State
    • 13.2: The Equilibrium Constant K
    • 13.3: The Equilibrium Constant Kp
    • 13.4: Heterogeneous Equilibria (8)
    • 13.5: Using the Equilibrium Constant (7)
    • 13.6: Factors That Alter the Composition of an Equilibrium Mixture: Le Châtelier' s Principle
    • 13.7: Altering an Equilibrium Mixture: Changes in Concentration
    • 13.8: Altering an Equilibrium Mixture: Changes in Pressure and Volume
    • 13.9: Altering an Equilibrium Mixture: Changes in Temperature
    • 13.10: The Effect of a Catalyst on Equilibrium (6)
    • 13.11: The Link between Chemical Equilibrium and Chemical Kinetics (2)
    • 13: Chapter Problems (8)
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  • Chapter 14: Aqueous Equilibria: Acids and Bases
    • 14: Key Concept Problems (1)
    • 14: Conceptual Problems (5)
    • 14.1: Acid—Base Concepts: The BrØnsted—Lowry Theory
    • 14.2: Acid Strength and Base Strength (4)
    • 14.3: Hydrated Protons and Hydronium Ions
    • 14.4: Dissociation of Water
    • 14.5: The pH Scale
    • 14.6: Measuring pH (4)
    • 14.7: The pH in Solutions of Strong Acids and Strong Bases (1)
    • 14.8: Equilibria in Solutions of Weak Acids
    • 14.9: Calculating Equilibrium Concentrations in Solutions of Weak Acids
    • 14.10: Percent Dissociation in Solutions of Weak Acids (2)
    • 14.11: Polyprotic Acids (1)
    • 14.12: Equilibria in Solutions of Weak Bases
    • 14.13: Relation between Ka and Kb (1)
    • 14.14: Acid—Base Properties of Salts (3)
    • 14.15: Factors That Affect Acid Strength (2)
    • 14.16: Lewis Acids and Bases (1)
    • 14: Chapter Problems (2)
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  • Chapter 15: Applications of Aqueous Equilibria
    • 15: Key Concept Problems
    • 15: Conceptual Problems (5)
    • 15.1: Neutralization Reactions (1)
    • 15.2: The Common—Ion Effect (3)
    • 15.3: Buffer Solutions
    • 15.4: The Henderson—Hasselbalch Equation (3)
    • 15.5: pH Titration Curves
    • 15.6: Strong Acid–Strong Base Titrations
    • 15.7: Weak Acid–Strong Base Titrations
    • 15.8: Weak Base–Strong Acid Titrations
    • 15.9: Polyprotic Acid–Strong Base Titrations (2)
    • 15.10: Solubility Equilibria
    • 15.11: Measuring Ksp and Calculating Solubility from Ksp (3)
    • 15.12: Factors That Affect Solubility (3)
    • 15.13: Precipitation of Ionic Compounds
    • 15.14: Separation of Ions by Selective Precipitation
    • 15.15: Qualitative Analysis
    • 15: Chapter Problems (1)
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  • Chapter 16: Thermodynamics: Entropy, Free Energy, and Equilibrium
    • 16: Key Concept Problems
    • 16: Conceptual Problems (2)
    • 16.1: Spontaneous Processes (2)
    • 16.2: Enthalpy, Entropy, and Spontaneous Processes: A Brief Review
    • 16.3: Entropy and Probability
    • 16.4: Entropy and Temperature (6)
    • 16.5: Standard Molar Entropies and Standard Entropies of Reaction (2)
    • 16.6: Entropy and the Second Law of Thermodynamics (2)
    • 16.7: Free Energy (4)
    • 16.8: Standard Free–Energy Changes for Reactions
    • 16.9: Standard Free Energies of Formation (7)
    • 16.10: Free–Energy Changes and Composition of the Reaction Mixture
    • 16.11: Free Energy and Chemical Equilibrium (6)
    • 16: Chapter Problems (13)
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  • Chapter 17: Electrochemistry
    • 17: Key Concept Problems (2)
    • 17: Conceptual Problems (4)
    • 17.1: Galvanic Cells
    • 17.2: Shorthand Notation for Galvanic Cells (3)
    • 17.3: Cell Potentials and Free—Energy Changes for Cell Reactions
    • 17.4: Standard Reduction Potentials
    • 17.5: Using Standard Reduction Potentials (9)
    • 17.6: Cell Potentials and Composition of the Reaction Mixture: The Nernst Equation
    • 17.7: Electrochemical Determination of pH (5)
    • 17.8: Standard Cell Potentials and Equilibrium Constants (4)
    • 17.9: Batteries
    • 17.10: Fuel Cells
    • 17.11: Corrosion (4)
    • 17.12: Electrolysis and Electrolytic Cells
    • 17.13: Commercial Applications of Electrolysis
    • 17.14: Quantitative Aspects of Electrolysis (3)
    • 17: Chapter Problems (4)
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  • Chapter 18: Hydrogen, Oxygen, and Water
    • 18: Key Concept Problems (1)
    • 18: Conceptual Problems (5)
    • 18.1: Hydrogen
    • 18.2: Isotopes of Hydrogen
    • 18.3: Preparation and Uses of Hydrogen
    • 18.4: Reactivity of Hydrogen
    • 18.5: Binary Hydrides (7)
    • 18.6: Oxygen
    • 18.7: Preparation and Uses of Oxygen
    • 18.8: Reactivity of Oxygen
    • 18.9: Oxides
    • 18.10: Peroxides and Superoxides
    • 18.11: Hydrogen Peroxide
    • 18.12: Ozone (7)
    • 18.13: Water
    • 18.14: Hydrates (3)
    • 18: Chapter Problems (5)
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  • Chapter 19: The Main Group Elements
    • 19: Key Concept Problems
    • 19: Conceptual Problems (2)
    • 19.1: A Review of General Properties and Periodic Trends
    • 19.2: Distinctive Properties of the Second—Row Elements (12)
    • 19.3: The Group 3A Elements (3)
    • 19.4: Boron
    • 19.5: Aluminum
    • 19.6: The Group 4A Elements
    • 19.7: Carbon
    • 19.8: Silicon (3)
    • 19.9: The Group 5A Elements
    • 19.10: Nitrogen
    • 19.11: Phosphorus (3)
    • 19.12: The Group 6A Elements
    • 19.13: Sulfur (4)
    • 19.14: The Halogens: Oxoacids and Oxoacid Salts (2)
    • 19: Chapter Problems (3)
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  • Chapter 20: Transition Elements and Coordination Chemistry
    • 20: Key Concept Problems (2)
    • 20: Conceptual Problems (3)
    • 20.1: Electron Configurations
    • 20.2: Properties of Transition Elements (3)
    • 20.3: Oxidation States of Transition Elements (3)
    • 20.4: Chemistry of Selected Transition Elements (4)
    • 20.5: Coordination Compounds
    • 20.6: Ligands (5)
    • 20.7: Naming Coordination Compounds (3)
    • 20.8: Isomers
    • 20.9: Enantiomers and Molecular Handedness (2)
    • 20.10: Color of Transition Metal Complexes
    • 20.11: Bonding in Complexes: Valence Bond Theory
    • 20.12: Crystal Field Theory (2)
    • 20: Chapter Problems (2)
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  • Chapter 21: Metals and Solid—State Materials
    • 21: Key Concept Problems (5)
    • 21: Conceptual Problems (2)
    • 21.1: Sources of the Metallic Elements (2)
    • 21.2: Metallurgy (6)
    • 21.3: Iron and Steel (1)
    • 21.4: Bonding in Metals (3)
    • 21.5: Semiconductors
    • 21.6: Semiconductor Applications (7)
    • 21.7: Superconductors
    • 21.8: Ceramics
    • 21.9: Composites (5)
    • 21: Chapter Problems (6)
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  • Chapter 22: Nuclear Chemistry
    • 22: Key Concept Problems
    • 22: Conceptual Problems
    • 22.1: Energy Changes During Nuclear Reactions (6)
    • 22.2: Nuclear Fission and Fusion
    • 22.3: Nuclear Transmutation (2)
    • 22.4: Detecting and Measuring Radioactivity
    • 22.5: Applications of Nuclear Chemistry
    • 22: Chapter Problems (3)
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  • Chapter 23: Organic and Biological Chemistry
    • 23: Key Concept Problems
    • 23: Conceptual Problems (3)
    • 23.1: Organic Molecules and Their Structures: Alkanes
    • 23.2: Families of Organic Compounds: Functional Groups (4)
    • 23.3: Naming Organic Compounds (5)
    • 23.4: Unsaturated Organic Compounds: Alkenes and Alkynes
    • 23.5: Cyclic Organic Compounds
    • 23.6: Aromatic Compounds (9)
    • 23.7: Alcohols, Ethers, and Amines
    • 23.8: Carbonyl Compounds (6)
    • 23.9: An Overview of Biological Chemistry
    • 23.10: Amino Acids, Peptides, and Proteins (3)
    • 23.11: Carbohydrates (3)
    • 23.12: Lipids (5)
    • 23.13: Nucleic Acids (4)
    • 23: Chapter Problems
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Group Quantity Questions
Chapter 1: Chemistry: Matter and Measurement
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1.T 1 001
Chapter 2: Atoms, Molecules, and Ions
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2.T 1 001
Chapter 3: Mass Relationships in Chemical Reactions
3.P 25 024 031 033 034 036 039 041 049 051 053 057 061 063 069 073 083 085 087 093 095 103 105 107 119 122
Chapter 4: Reactions in Aqueous Solution
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Chapter 5: Periodicity and the Electronic Structure of Atoms
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Chapter 6: Ionic Bonds and Some Main—Group Chemistry
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Chapter 7: Covalent Bonds and Molecular Structure
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7.T 2 001 002
Chapter 8: Thermochemistry: Chemical Energy
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Chapter 9: Gases: Their Properties and Behavior
9.P 15 026 027 029 039 047 049 055 057 059 063 071 079 089 097 111
Chapter 10: Liquids, Solids, and Phase Changes
10.P 16 020 021 025 026 031 037 039 057 059 065 067 083 085 101 113 129
Chapter 11: Solutions and Their Properties
11.P 37 031 036 037 038 039 044 045 049 051 053 054 055 057 058 059 061 064 065 071 072 079 081 083 085 088 089 092 096 097 099 102 103 109 115 118 119 125
Chapter 12: Chemical Kinetics
12.P 40 019 026 028 030 031 033 037 043 049 050 051 053 054 055 057 060 067 068 069 071 074 077 080 083 084 085 090 091 092 097 098 099 100 107 108 110 114 119 120 121
Chapter 13: Chemical Equilibrium
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Chapter 14: Aqueous Equilibria: Acids and Bases
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Chapter 15: Applications of Aqueous Equilibria
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Chapter 16: Thermodynamics: Entropy, Free Energy, and Equilibrium
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Chapter 17: Electrochemistry
17.P 38 016 017 027 032 034 035 036 044 047 050 051 055 057 059 061 065 067 071 072 073 075 079 081 083 085 087 089 090 091 092 093 102 105 107 112 113 123 127
Chapter 18: Hydrogen, Oxygen, and Water
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Chapter 19: The Main Group Elements
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Chapter 20: Transition Elements and Coordination Chemistry
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Chapter 21: Metals and Solid—State Materials
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Chapter 22: Nuclear Chemistry
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Chapter 23: Organic and Biological Chemistry
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