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General Chemistry

General Chemistry Chemistry

Tác giả: LibreTexts (Textmap of Petrucci's Book)
Nhà xuất bản: LibreTexts
Nguồn: LibreTexts
Giấy phép: CC BY-NC-SA
Ngôn ngữ: EN
Danh mục: Khoa học cơ bản

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01: Matter- Its Properties And Measurement
1.1: The Scientific Method
1.2: Properties of Matter
1.3: Classification of Matter
1.4: Measurement of Matter - SI (Metric) Units
1.5: Density and Percent Composition - Their Use in Problem Solving
1.6: Uncertainties in Scientific Measurements
1.7: Significant Figures
1.E: Exercises
02: Atoms and The Atomic Theory
2.1: Early Chemical Discoveries and the Atomic Theory
2.2: Electrons and Other Discoveries in Atomic Physics
2.3: The Nuclear Atom
2.4: Chemical Elements
2.5: Atomic Mass
2.6: Introduction to the Periodic Table
2.7: The Concept of Mole and the Avogadro Constant
2.8: Using the Mole Concept in Calculations
Homework Problems
03: Chemical Compounds
3.1: Types of Chemical Compounds and their Formulas
3.2: The Mole Concept and Chemical Compounds
3.3: Composition of Chemical Compounds
3.4: Oxidation States: A Useful Tool in Describing Chemical Compounds
3.5: Importance of Nomenclature
3.6: Names and Formulas of Inorganic Compounds
3.7: Names of Formulas of Organic Compounds
3.E: Homework Problems
04: Chemical Reactions
4.1: Chemical Reactions and Chemical Equations
4.2: Chemical Equations and Stoichiometry
4.3: Chemical Reactions in Solution
4.4: Determining the Limiting Reactant
4.5: Other Practical Matters in Reaction Stoichiometry
05: Introduction To Reactions In Aqueous Solutions
5.1: The Nature of Aqueous Solutions
5.2: Precipitation Reactions
5.3: Acid-Base Reactions
5.4: Oxidation-Reduction: Some General Principles
5.5: Balancing Oxidation-Reduction Equations
5.6: Oxidizing and Reducing Agents
5.7: Stoichiometry of Reactions in Aqueous Solutions: Titrations
06: Gases
6.1: Properties of Gases: Gas Pressure
6.2: The Simple Gas Laws
6.3: Combining the Gas Laws: The Ideal Gas Equation and the General Gas Equation
6.4: Applications of the Ideal Gas Equation
6.5: Gases in Chemical Reactions
6.6: Mixtures of Gases
6.7: Kinetic-Molecular Theory of Gases
6.8: Gas Properties Relating to the Kinetic-Molecular Theory
6.9: Non-ideal (Real) Gases
07: Thermochemistry
7.1: Getting Started: Some Terminology
7.2: Heat
7.3: Heats of Reactions and Calorimetry
7.4: Work
7.5: The First Law of Thermodynamics
7.6: Heats of Reactions - U and H
7.7: Indirect Determination of H - Hess's Law
7.8: Standard Enthalpies of Formation
7.9: Fuels as Sources of Energy
08: Electrons in Atoms
8.01: Electromagnetic Radiation
8.02: Atomic Spectra
8.03: Quantum Theory
8.04: The Bohr Atom
8.05: Two Ideas Leading to a New Quantum Mechanics
8.06: Wave Mechanics
8.07: Quantum Numbers and Electron Orbitals
8.08: Interpreting and Representing the Orbitals of the Hydrogen Atom
8.09: Electron Spin: A Fourth Quantum Number
8.10: Multielectron Atoms
8.11: Electron Configurations
8.12: Electron Configurations and the Periodic Table
09: The Periodic Table and Some Atomic Properties
9.1: Classifying the Elements: The Periodic Law and the Periodic Table
9.2: Metals and Nonmetals and their Ions
9.3: Sizes of Atoms and Ions
9.4: Ionization Energy
9.5: Electron Affinity
9.6: Magnetic Properties
9.7: Periodic Properties of the Elements
10: Chemical Bonding I: Basic Concepts
10.1: Lewis Theory: An Overview
10.2: Covalent Bonding: An Introduction
10.3: Polar Covalent Bonds and Electrostatic Potential Maps
10.4: Writing Lewis Structures
10.5: Resonance
10.6: Exceptions to the Octet Rule
10.7: Shapes of Molecules
10.9: Bond Energies
11: Chemical Bonding II: Additional Aspects
11.1: What a Bonding Theory Should Do
11.2: Introduction to the Valence-Bond Method
11.3: Hybridization of Atomic Orbitals
11.4: Multiple Covalent Bonds
11.5: Molecular Orbital Theory
11.6: Delocalized Electrons: Bonding in the Benzene Molecule
11.7: Bonding in Metals
11.8: Some Unresolved Issues
11.E: Chemical Bonding II: Additional Aspects (Exercises)
12: Intermolecular Forces: Liquids And Solids
12.1: Intermolecular Forces
12.2: Some Properties of Liquids
12.3: Some Properties of Solids
12.4: Phase Diagrams
12.5: Network Covalent Solids and Ionic Solids
12.6: Crystal Structures
12.7: Energy Changes in the Formation of Ionic Crystals
13: Solutions and their Physical Properties
13.01: Types of Solutions: Some Terminology
13.02: Solution Concentration
13.03: Intermolecular Forces and the Solution Process
13.04: Solution Formation and Equilibrium
13.05: Solubilities of Gases
13.06: Vapor Pressures of Solutions
13.07: Osmotic Pressure
13.08: Freezing-Point Depression and Boiling-Point Elevation of Nonelectrolyte Solutions
13.09: Solutions of Electrolytes
13.10: Colloidal Mixtures
14: Chemical Kinetics
14.01: The Rate of a Chemical Reaction
14.02: Measuring Reaction Rates
14.03: Effect of Concentration on Reaction Rates: The Rate Law
14.04: Zero-Order Reactions
14.05: First-Order Reactions
14.06: Second-Order Reactions
14.07: Reaction Kinetics: A Summary
14.08: Theoretical Models for Chemical Kinetics
14.09: The Effect of Temperature on Reaction Rates
14.10: Reaction Mechanisms
14.11: Catalysis
14.E: Exercises
15: Principles of Chemical Equilibrium
15.1: Dynamic Equilibrium
15.2: The Equilibrium Constant Expression
15.3: Relationships Involving Equilibrium Constants
15.4: The Magnitude of an Equilibrium Constant
15.5: The Reaction Quotient Q - Predicting The Direction of Net Change
15.6: Altering Equilibrium Conditions - Le Chateliers Principle
15.7: Equilibrium Calculations - Some Illustrative Examples
16: Acids and Bases
16.1: Arrhenius Theory: A Brief Review
16.2: Brnsted-Lowry Theory of Acids and Bases
16.3: Self-Ionization of Water and the pH Scale
16.4: Strong Acids and Strong Bases
16.5: Weak Acids and Weak Bases
16.6: Polyprotic Acids
16.7: Ions as Acids and Bases
16.8: Molecular Structure and Acid-Base Behavior
16.9: Lewis Acids and Bases
17: Additional Aspects of Acid-Base Equilibria
17.1: Common-Ion Effect in Acid-Base Equilibria
17.2: Buffer Solutions
17.3: Acid-Base Indicators
17.4: Neutralization Reactions and Titration Curves
17.5: Solutions of Salts of Polyprotic Acids
17.6: Acid-Base Equilibrium Calculations: A Summary
17.E: Exercises
18: Solubility and Complex-Ion Equilibria
18.1: Solubility Product Constant Ksp
18.2: Relationship Between Solubility and Ksp
18.3: Common-Ion Effect in Solubility Equilibria
18.4: Limitations of the Ksp Concept
18.5: Criteria for Precipitation and its Completeness
18.6: Fractional Precipitation
18.7: Solubility and pH
18.8: Equilibria Involving Complex Ions
18.9: Qualitative Cation Analysis
19: Spontaneous Change: Entropy and Gibbs Energy
19.1: Spontaneity: The Meaning of Spontaneous Change
19.2: The Concept of Entropy
19.3: Evaluating Entropy and Entropy Changes
19.4: Criteria for Spontaneous Change: The Second Law of Thermodynamics
19.5: Standard Gibbs Energy Change G
19.6: Gibbs Energy Change and Equilibrium
19.7: G and K as Functions of Temperature
19.8: Coupled Reactions
19.E: Chemical Thermodynamics (Exercises)
20: Electrochemistry
20.1: Electrode Potentials and their Measurement
20.2: Standard Electrode Potentials
20.3: Ecell G and K
20.4: Cell Potential as a Function of Concentrations
20.5: Batteries: Producing Electricity Through Chemical Reactions
20.6: Corrosion: Unwanted Voltaic Cells
20.7: Electrolysis: Causing Nonspontaneous Reactions to Occur
20.8: Industrial Electrolysis Processes
20.E: Exercises
21: Chemistry of The Main-Group Elements I
21.1: Periodic Trends and Charge Density
21.2: Group 1: The Alkali Metals
21.3: Group 2: The Alkaline Earth Metals
21.4: Group 13: The Boron Family
21.5: Group 14: The Carbon Family
21.E: Exercises
22: Chemistry of The Main-Group Elements II
22.1: Periodic Trends in Bonding
22.2: Group 18 - The Noble Gases
22.3: Group 17: The Halogens
22.4: Group 16: The Oxygen Family
22.5: Group 15: The Nitrogen Family
22.6: Hydrogen: A Unique Element
22.E: Exercises
23: The Transition Elements
23.1: General Properties of Transition Metals
23.2: Principles of Extractive Metallurgy
23.3: Metallurgy of Iron and Steel
23.4: First-Row Transition Metal Elements - Scandium to Manganese
23.5: The Iron Triad: Iron Cobalt and Nickel
23.6: Group 11: Copper Silver and Gold
23.7: Group 12: Zinc Cadmium and Mercury
23.8: Lanthanides
23.9: High Temperature Superconductors
23.E: Exercises
24: Complex Ions and Coordination Compounds
24.01: Werners Theory of Coordination Compounds
24.02: Ligands
24.03: Nomenclature
24.04: Isomerism
24.05: Bonding in Complex Ions: Crystal Field Theory
24.06: Magnetic Properties of Coordination Compounds and Crystal Field Theory
24.07: Color and the Colors of Complexes
24.08: Aspects of Complex-Ion Equilibria
24.09: Acid-Base Reactions of Complex Ions
24.10: Some Kinetic Considerations
24.E: Exercises
25: Nuclear Chemistry
25.01: Radioactivity
25.02: Naturally Occurring Radioactive Isotopes
25.03: Nuclear Reactions and Artificially Induced Radioactivity
25.04: Transuranium Elements
25.05: Rate of Radioactive Decay
25.06: Energetics of Nuclear Reactions
25.07: Nuclear Stability
25.08: Nuclear Fission
25.09: Nuclear Fusion
25.10: Effect of Radiation on Matter
25.11: Applications of Radioisotopes
25.E: Exercises
26: Structure of Organic Compounds
26.1: Organic Compounds and Structures: An Overview
26.2: Alkanes
26.3: Cycloalkanes
26.4: Stereoisomerism in Organic Compounds
26.5: Alkenes and Alkynes
26.6: Aromatic Hydrocarbons
26.7: Organic Compounds Containing Functional Groups
26.8: From Molecular Formula to Molecular Structure
27: Reactions of Organic Compounds
27.01: Organic Reactions: An Introduction
27.02: Introduction to Substitution Reactions
27.03: Introduction to Elimination Reactions
27.04: Reactions of Alcohols
27.05: Introduction to Addition Reactions: Reactions of Alkenes
27.06: Electrophilic Aromatic Substitution
27.07: Reactions of Alkanes
27.08: Polymers and Polymerization Reactions
27.09: Synthesis of Organic Compounds
28: Chemistry of The Living State
28.1: Chemical Structure of Living Matter: An Overview
28.2: Lipids
28.3: Carbohydrates
28.4: Proteins
28.5: Aspects of Metabolism
28.6: Nucleic Acids