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Chem 2A: Introductory Chemistry I

Introduction to fundamental principles of inorganic chemistry; structure and bonding, nomenclature, chemical equations and reactions, stoichiometry, acids, bases, and chemical equilibrium, redox, gases, solutions, and nuclear chemistry.

Chemistry

Tác giả: Julie Brown
Nhà xuất bản: Woodland Community College
Nguồn: LibreTexts
Giấy phép: CC BY-NC-SA
Ngôn ngữ: EN
Danh mục: Khoa học cơ bản

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Mục lục· 141 mục

01: Matter and Measurements
1.01: Chemistry - The Central Science
1.02: States of Matter
1.03: Classification of Matter
1.04: Chemical Elements and Symbols
1.05: Elements and the Periodic Table
1.06: Chemical Reaction- An Example of a Chemical Change
1.07: Physical Quantities
1.08: Measuring Mass Length and Volume
1.09: Measurement and Significant Figures
1.10: Scientific Notation
1.11: Rounding Off Numbers
1.12: Problem Solving - Unit Conversions and Estimating Answers
1.13: Temperature Heat and Energy
1.14: Density and Specific Gravity
02: Atoms and the Periodic Table
2.01: Atomic Theory
2.02: Elements and Atomic Number
2.03: Isotopes and Atomic Weight
2.04: The Periodic Table
2.05: Some Characteristics of Different Groups
2.06: Electronic Structure of Atoms
2.07: Electron Configurations
2.08: Electron Configurations and the Periodic Table
2.09: Electron-Dot Symbols
03: Ionic Compounds
3.01: Ions
3.02: Periodic Properties and Ion Formation
3.03: Ionic Bonds
3.04: Some Properties of Ionic Compounds
3.05: Ions and the Octet Rule
3.06: Ions of Some Common Elements
3.07: Naming Ions
3.08: Polyatomic Ions
3.09: Formulas of Ionic Compounds
3.10: Naming Ionic Compounds
3.11: H and OH- Ions- An Introduction to Acids and Bases
04: Molecular Compounds
4.01: Covalent Bonds
4.02: Covalent Bonds and the Periodic Table
4.03: Multiple Covalent Bonds
4.04: Coordinate Covalent Bonds
4.05: Characteristics of Molecular Compounds
4.06: Molecular Formulas and Lewis Structures
4.07: The Shapes of Molecules
4.08: Polar Covalent Bonds and Electronegativity
4.09: Polar Molecules
4.10: Naming Binary Molecular Compounds
05: Classification and Balancing of Chemical Reactions
5.01: Chemical Equations
5.02: Balancing Chemical Equations
5.03: Classes of Chemical Reactions
5.04: Precipitation Reactions and Solubility Guidelines
5.05: Acids Bases and Neutralization Reactions
5.06: Redox Reactions
5.07: Recognizing Redox Reactions
5.08: Net Ionic Equations
06: Chemical Reactions - Mole and Mass Relationships
6.01: The Mole and Avogadros Number
6.02: GramMole Conversions
6.03: Mole Relationships and Chemical Equations
6.04: Mass Relationships and Chemical Equations
6.05: Limiting Reagent and Percent Yield
07: Chemical Reactions - Energy Rates and Equilibrium
7.01: Energy and Chemical Bonds
7.02: Heat Changes during Chemical Reactions
7.03: Exothermic and Endothermic Reactions
7.04: Why Do Chemical Reactions Occur Free Energy
7.05: Effects of Temperature Concentration and Catalysts on Reaction Rates
7.06: How Do Chemical Reactions Occur Reaction Rates
7.07: Reversible Reactions and Chemical Equilibrium
7.08: Equilibrium Equations and Equilibrium Constants
7.09: Le Chateliers Principle - The Effect of Changing Conditions on Equilibria
08: Gases Liquids and Solids
8.01: States of Matter and Their Changes
8.02: Intermolecular Forces
8.03: Gases and the Kinetic - Molecular Theory
8.04: Pressure
8.05: Boyles Law - The Relation between Volume and Pressure
8.06: Charless Law - The Relation between Volume and Temperature
8.07: Gay-Lussacs Law - The Relation between Pressure and Temperature
8.08: The Combined Gas Law
8.09: Avogadros Law - The Relation between Volume and Molar Amount
8.10: The Ideal Gas Law
8.11: Partial Pressure and Daltons Law
8.12: Liquids
8.13: Water - A Unique Liquid
8.14: Solids
8.15: Changes of State
09: Solutions
9.01: Mixtures and Solutions
9.02: The Solution Process
9.03: Solid Hydrates
9.04: Solubility
9.05: The Effect of Temperature on Solubility
9.06: The Effect of Pressure on Solubility - Henrys Law
9.07: Units of Concentration
9.08: Dilution
9.09: Ions in Solution - Electrolytes
9.10: Electrolytes in Body Fluids - Equivalents and Milliequivalents
9.11: Osmosis and Osmotic Pressure
9.12: Dialysis
10: Acids and Bases
10.01: Acids and Bases in Aqueous Solution
10.02: Some Common Acids and Bases
10.03: The BrnstedLowry Definition of Acids and Bases
10.04: Acid and Base Strength
10.05: Acid Dissociation Constants
10.06: Water as Both an Acid and a Base
10.07: Measuring Acidity in Aqueous Solution- pH
10.08: Working with pH
10.09: Laboratory Determination of Acidity
10.10: Buffer Solutions
10.11: Acid and Base Equivalents
10.12: Some Common AcidBase Reactions
10.13: Titration
10.14: Acidity and Basicity of Salt Solutions
11: Nuclear Chemistry
11.01: Nuclear Reactions
11.02: The Discovery and Nature of Radioactivity
11.03: Stable and Unstable Isotopes
11.04: Nuclear Decay
11.05: Radioactive Half-Life
11.06: Radioactive Decay Series
11.07: Ionizing Radiation
11.08: Detecting Radiation
11.09: Measuring Radiation
11.10: Artificial Transmutation
11.11: Nuclear Fission and Nuclear Fusion
12: Introduction to Organic Chemistry - Alkanes
12.01: The Nature of Organic Molecules
12.02: Families of Organic Molecules - Functional Groups
12.03: The Structure of Organic Molecules - Alkanes and Their Isomers
12.04: Drawing Organic Structures
12.05: The Shapes of Organic Molecules
12.06: Naming Alkanes
12.07: Properties of Alkanes
12.08: Reactions of Alkanes
12.09: Cycloalkanes
12.10: Drawing and Naming Cycloalkanes
13: Chapters