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Introductory_Chemistry_at_Solano_College

Chemistry

Tác giả: Commodore St Germain
Nhà xuất bản: Solano College
Nguồn: LibreTexts
Ngôn ngữ: EN
Danh mục: Khoa học cơ bản

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Mục lục· 197 mục

01: Introduction To Chemistry
1.01: Scope of Chemistry
1.02: Areas of Chemistry
1.03: Research
1.04: Scientific Problem Solving
02: Numbers From Measurements
2.01: Accuracy and Precision
2.02: Percent Error
2.03: Measurement Uncertainty
2.04: Significant Figures
2.05: Rounding
2.06: Significant Figures in Addition and Subtraction
2.07: Significant Figures in Multiplication and Division
2.08: Scientific Notation
03: Unit Systems and Dimensional Analysis
3.01: SI Base Units
3.02: Metric Prefixes
3.03: Length and Volume
3.04: Mass and Weight
3.05: Metric Unit Conversions
3.06: Derived Units
3.07: Dimensional Analysis
3.08: Density
3.09: Kinetic Energy
3.10: Temperature and Temperature Scales
04: Matter and Change
4.01: Matter Mass and Volume
4.02: States of Matter
4.03: Physical Properties
4.04: Chemical Properties and Chemical Reactions
4.05: Extensive and Intensive Properties
4.06: Physical Change
4.07: Chemical Change
4.08: Recognizing Chemical Reactions
4.09: Pure Substances
4.10: Mixture
4.11: Heterogeneous Mixtures
4.12: Homogeneous Mixture
4.13: Separating Mixtures
4.14: Elements
4.15: Compounds
4.16: Chemical Symbols and Formulas
4.17: A Molecular View of Elements and Compounds
05: Atoms Molecules and Subatomic Particles
5.01: Atom
5.02: Protons
5.03: Neutrons
5.04: Electrons
5.05: Atomic Nucleus
5.06: Atomic Number
5.07: Mass Number
5.08: Isotopes
5.09: Atomic Mass Unit
5.10: Calculating Average Atomic Mass
5.11: Ion
06: Electronic Structure and Chemical Periodicity
6.01: Periodic Law
6.02: Modern Periodic Table- Periods and Groups
6.03: Blocks of the Periodic Table
6.04: Energy Level
6.05: Orbitals
6.06: Electron Configurations
6.07: Noble Gas Configuration
6.08: Hund's Rule and Orbital Filling Diagrams
6.09: Aufbau Principle
6.10: Periodic Trends- Atomic Radius
6.11: Metals
6.12: Nonmetals
6.13: Metalloids
07: Chemical Bonds
7.01: Chemical Bond
7.02: Electron Dot Diagrams
7.03: Octet Rule
7.04: Cation Formation
7.05: Anion Formation
7.06: Ionic Bonding
7.07: Polyatomic Ions
7.08: Covalent Bond
7.09: Lewis Electron-Dot Structures
7.10: Single Covalent Bonds
7.11: Multiple Covalent Bonds
7.12: Valence Electrons
7.13: Coordinate Covalent Bond
7.14: Resonance
7.15: VSEPR Theory
7.16: Molecular Shapes- No Lone Pairs on Central Atoms
7.17: Molecular Shapes - Lone Pair(s) on Central Atom
7.18: Bond Polarity
7.19: Polar Molecules
08: Chemical Nomenclature
8.01: Molecular Formula
8.02: Empirical Formula
8.03: Cations
8.04: Anions
8.05: Transition Metal Ions
8.06: The Stock System of Nomenclature
8.07: Naming Binary Ionic Compounds
8.08: Formulas for Binary Ionic Compounds
8.09: Polyatomic Ions
8.10: Ternary Ionic Compounds- Naming and Formulas
8.11: Binary Molecular Compounds- Naming and Formulas
8.12: Acids - Naming and Formulas
8.13: Bases- Naming and Formulas
09: The Mole
9.01: Law of Definite Proportions
9.02: Avogadro's Number
9.03: Conversions Between Moles and Atoms
9.04: Molar Mass
9.05: Conversions Between Moles and Mass
9.06: Conversions Between Mass and Number of Particles
9.07: Avogadro's Hypothesis and Molar Volume
9.08: Conversions Between Moles and Gas Volume
9.09: Gas Density
9.10: Mole Road Map
9.11: Percent Composition
9.12: Percent of Water in a Hydrate
9.13: Determining Empirical Formulas
9.14: Determining Molecular Formulas
10: Chemical Calculations Involving Chemical Equations
10.01: Law of Conservation of Mass
10.02: Word Equations
10.03: Chemical Equations
10.04: Balancing Equations
10.05: Combination Reactions
10.06: Decomposition Reactions
10.07: Combustion Reactions
10.08: Single Replacement Reactions
10.09: Activity Series
10.10: Double Replacement Reactions
10.11: Everyday Stoichiometry
10.12: Mole Ratios
10.13: Mass-Mole Stoichiometry
10.14: Mass-Mass Stoichiometry
10.15: Volume-Volume Stoichiometry
10.16: Mass-Volume Stoichiometry
10.17: Limiting Reactant
10.18: Determining the Limiting Reactant
10.19: Theoretical Yield and Percent Yield
11: States of Matter
11.01: Physical Properties and Intermolecular Forces
11.02: Hydrogen Bonding
11.03: Kinetic Molecular Theory
11.04: Gas Pressure
11.05: Atmospheric Pressure
11.06: Pressure Units and Conversions
11.07: Average Kinetic Energy and Temperature
11.08: Physical Properties and Intermolecular Forces
11.09: Surface Tension
11.10: Evaporation
11.11: Vapor Pressure
11.12: Boiling
11.13: Vapor Pressure Curves
11.14: Melting
11.15: Sublimation
11.16: Heating and Cooling Curves
11.17: General Phase Diagram
11.18: Phase Diagram for Water
12: Gas Laws
13: Solutions
13.01: Solute-Solvent Combinations
13.02: Rate of Dissolution
13.03: Saturated and Unsaturated Solutions
13.04: How Temperature Influences Solubility
13.05: Supersaturated Solutions
13.06: Predicting Precipitates Using Solubility Rules
13.07: Percent Solutions
13.08: Molarity
13.09: Preparing Solutions
13.10: Dilution
13.11: Molality
13.12: Calculating Molar Mass
13.13: Electrolytes and Nonelectrolytes
13.14: Strong and Weak Electrolytes
13.15: Molecular and Ionic Equations
13.16: Net Ionic Equations
14: Acids and Bases
14.01: Properties of Acids
14.02: Properties of Bases
14.03: Arrhenius Acids
14.04: Arrhenius Bases
14.05: Brnsted-Lowry Acids and Bases
14.06: Brnsted-Lowry Acid-Base Reactions
14.07: Ion-Product of Water
14.08: The pH Scale
14.09: Calculating pH of Acids and Bases
14.10: The pOH Concept
14.11: Strong and Weak Acids and Acid Ionization Constant (left( K texta right))
14.12: Strong and Weak Bases and Base Ionization Constant
14.13: Calculating Acid and Base Dissociation Constants
14.14: Calculating pH of Weak Acid and Base Solutions
14.15: Neutralization Reaction and Net Ionic Equations for Neutralization Reactions
14.16: Titration Experiment
14.17: Titration Calculations
14.18: Titration Curves
14.19: Indicators
14.20: Hydrolysis of Salts - Equations
14.21: Calculating pH of Salt Solutions