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Atoms First - Introductory Chemistry for Science and Engineering

Chemistry

Tác giả: Craig Cavanaugh, Kathryn Mayer, Rebekah Stassinopoulos
Nhà xuất bản: Southwestern College
Nguồn: LibreTexts
Giấy phép: CC BY-NC-SA
Ngôn ngữ: EN
Danh mục: Khoa học cơ bản

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01: Chemistry Measurements and Calculations
1.01: The Scope of Chemistry
1.02: Chemicals Compose Ordinary Things
1.03: Hypothesis Theories and Laws
1.04: The Scientific Method - How Chemists Think
1.05: Taking Measurements
1.5.01: Measurement Basics - Units and the SI System
1.5.02: Awkward Numbers and Scientific Notation
1.5.03: Measurement Uncertainty and Significant Figures
1.06: Unit Conversions and Problem Solving
1.6.01: One-Step Unit Conversions
1.6.02: Multi-step Unit Conversion
1.6.03: Units Raised to a Power - Slightly Obtuse Multi-step Conversions
1.07: Density as a Unit Conversion
1.08: Temperature - Random Motion of Molecules and Atoms
1.E: Practice Exercises - Measurements and Conversions
02: Atomic Structure
2.01: Indivisible - The Atomic Theory
2.02: The Building Blocks of Atoms - Protons Neutrons and Electrons
2.03: Tracking Subatomic Particles in Atoms
2.04: Looking for Patterns - The Periodic Table
2.05: Atoms to Ions - Losing and Gaining Electrons
2.06: Isotopes - When the Number of Neutrons Varies
2.07: Atomic Mass - The Average Mass of an Elements Atoms
2.08: Summary of Atomic Theory
2.E: Practice Exercises - Atomic Structure
03: Light Electrons and the Periodic Table
3.01: Light is Electromagnetic Radiation
3.1.01: The Electromagnetic Spectrum
3.02: Models of Electron Behavior in Atoms
3.2.01: The Bohr Model - Atoms with Orbits
3.2.02: The Quantum Mechanical Model - Atoms with Orbitals
3.03: Quantum Mechanics - Orbitals and Electron Configurations
3.04: Core and Valence Electrons
3.05: Electron Configurations and the Periodic Table
3.5.01: The Explanatory Power of the Quantum Mechanical Model
3.06: Periodic Trends - Atomic Size Ionization Energy and Metallic Character
3.E: Practice Exercises - Light Electrons and the Periodic Table
04: Matter Compounds and Nomenclature
4.01: Describing Matter
4.1.01: States of Matter
4.1.02: Physical and Chemical Properties
4.1.03: Physical and Chemical Changes
4.1.04: Conservation of Mass - There is No New Matter
4.1.05: Summary of Describing Matter
4.02: Compounds
4.2.01: Chemical Formulas - Representing Compounds
4.03: A Molecular View of Elements and Compounds
4.04: Ionic Compounds
4.4.01: Monatomic and Polyatomic Ions
4.4.02: Formulas and Ionic Compounds
4.05: What is Nomenclature
4.5.01: Nomenclature - Ionic Compounds
4.5.02: Nomenclature - Molecular Compounds
4.5.03: Nomenclature - Acids
4.06: Nomenclature - Executive Summary
4.E: Practice Exercises - Matter Compounds and Nomenclature
05: The Mole Chemical Formulas and Composition
5.01: Avogadro's Number
5.02: Conversions Between Moles and Atoms
5.03: Molar Mass
5.04: Conversions Between Moles and Mass
5.05: Conversions Between Mass and Number of Particles
5.06: Percent Composition
5.6.01: Percent of Water in a Hydrate
5.07: Determining Empirical Formulas
5.08: Determining Molecular Formulas
5.09: Mole Road Map
5.E: Practice Exercises - The Mole Chemical Formulas and Composition
06: Lewis Structures Molecular Shape and Intermolecular Forces
6.01: The Octet 'Rule'
6.1.01: Valence Electrons and Lewis Dots
6.1.02: Lewis Dots and Ionic Compounds
6.1.03: Lewis Dots and Simple Covalent Compounds
6.02: Determining Lewis Structures for Molecular Compounds (and Ions)
6.2.01: Resonance - Equivalent Lewis Structures
6.2.02: Exceptions to the Octet 'Rule'
6.03: Predicting the Shapes of Molecules - VSEPR Theory
6.04: Electronegativity Bond Polarity and Molecule Polarity
6.05: Intermolecular Forces (IMF)
6.E: Practice Exercises - Lewis Structures Shapes and IMF
07: Aqueous Solutions
7.01: Types of Solutions
7.1.01: How Solutions Form
7.1.02: Types of Aqueous Solutions
7.02: Aqueous (Ionic) Solutions
7.03: Describing Solubility
7.3.01: Solubility of Solids
7.04: Quantifying Solutions - Concentration
7.4.01: Measuring Concentration with Mass and Volume Percents
7.4.02: Measuring Concentration with Molarity
7.05: Solutions and Dilution
7.E: Practice Exercises - Aqueous Solutions
08: Chemical Reactions
8.01: Evidence for Chemical Reactions
8.02: Chemical Reactions in Words
8.03: Chemical Reactions and Skeleton Equations
8.04: Complete (Balanced) Chemical Equations
8.05: Types of Reactions
8.06: Double Displacement Reactions
8.6.01: DD - Precipitation Reactions
8.6.02: DD - Acid Base Neutralization and Gas Evolution Reactions
8.6.03: Representing Aqueous Reactions - Complete Chemical Total Ionic and Net Ionic Equations
8.07: Oxidation and Reduction (Redox) Reactions
8.7.01: Combination Reactions
8.7.02: Decomposition Reactions
8.7.03: Combustion Reactions
8.7.04: Single Displacement Reactions
8.7.05: Oxidation States and Assigning Oxidation Numbers
8.7.06: Using Oxidation Numbers to Identify Redox Reactions
8.08: A (long) Summary of Chemical Reactions
8.E: Practice Exercises - Chemical Reactions
09: Stoichiometry - Quantities in Chemical Reactions
9.01: Stoichiometry - Moles are Key to Understanding
9.1.01: Stoichiometry - Mass to Mass Conversions
9.1.02: Stoichiometry - Volume to Volume Conversions
9.1.03: Gases and Moles - A Quick Aside
9.1.04: Stoichiometry - Now with Gases
9.1.05: Titrations - Revisiting Solution-based Stoichiometry
9.02: Limiting Reagent (Reactant)
9.03: Theoretical Yield vs Percent Yield
9.04: Tracking Heat Flow Using Stoichiometry
9.E: Practice Exercises - Stoichiometry
10: Solids Liquids and Gases
10.01: Properties of Solids Liquids and Gases
10.1.01: Types of Crystalline Solids
10.1.02: Gases and the Kinetic Molecular Theory
10.02: Vocab is Important - Temperature vs Heat vs Energy
10.2.01: Energy Work and Heat
10.2.02: Tracking Energy Flows with Heat
10.2.03: Quantifying Heat Using Changes in Temperature
10.03: Phase Transitions
10.3.01: Evaporation (l to g) and Condensation (g to l)
10.3.02: Melting (s to l) Freezing (l to s) and Sublimation (s to g)
10.3.03: Quantifying Heat During Phase Transitions
10.04: Heating and Cooling Curves
10.E: Practice Exercises - Solids Liquids and Gases
11: Acids and Bases
11.01: Properties of Acids and Bases
11.1.01: Acids - Properties and Examples
11.1.02: Bases - Properties and Examples
11.02: Chemistry of Acids and Bases
11.2.01: Molecular Definitions of Acids and Bases
11.2.02: Reactions of Acids and Bases
11.2.03: Acids and Bases - Strong vs Weak
11.03: Acid Base Equilibria
11.3.01: Water - An Acid and a Base in One Molecule
11.3.02: pH and pOH - Tracking Acidity
11.04: Buffer Solutions
11.E: Practice Exercises - Acids and Bases
12: Chemical Equilibrium
12.01: Before Equilibrium - Let's Discuss Rate of Reactions and Collisions
12.1.01: Effects of Temperature Concentration and Catalysts on Reaction Rates
12.02: Dynamic Equilibrium
12.03: The Equilibrium Constant Expression
12.04: Le Chatelier's Principle
12.05: Some Special Types of Equilibria
12.E: Practice Exercises - Chemical Equilibrium
13: Radioactivity and Nuclear Chemistry
13.01: The Discovery of Radioactivity
13.02: Types of Radioactivity - Alpha Beta and Gamma Decay
13.03: Radioactivity and Half-Life
13.04: Detecting Radioactivity
13.05: Applications of Nuclear Chemistry
13.5.01: Radiocarbon Dating
13.5.02: The Discovery of Fission and the Atomic Bomb
13.5.03: Nuclear Power - Using Fission to Generate Electricity
13.5.04: Nuclear Fusion - The Power of the Sun
13.5.05: The Effects of Radiation on Life
13.5.06: Radioactivity in Medicine
13.E: Practice Exercises - Radioactivity and Nuclear Chemistry