5.10: Nomenclature Summary

Chapter 1

1. Chapter 1: The Chemical World
2. 1.1: The Scope of Chemistry
3. 1.2: Chemicals Compose Ordinary Things
4. 1.3: Hypothesis, Theories, and Laws
5. 1.4: The Scientific Method: How Chemists Think
6. 1.5: A Beginning Chemist: How to Succeed

 •  Chapter 2

1. Chapter 2: Measurement and Problem Solving
2. 2.1: Taking Measurements
3. 2.2: Scientific Notation: Writing Large and Small Numbers
4. 2.3: Significant Figures: Writing Numbers to Reflect Precision
5. 2.4: Significant Figures in Calculations
6. 2.5: The Basic Units of Measurement
7. 2.6: Problem Solving and Unit Conversions
8. 2.7: Solving Multistep Conversion Problems
9. 2.8: Units Raised to a Power
10. 2.9: Density
11. 2.10: Numerical Problem-Solving Strategies and the Solution Map
12. 2.E: Measurement and Problem Solving (Exercises)

 •  Chapter 3

1. Chapter 3: Matter and Energy
2. 3.1: In Your Room
3. 3.2: What is Matter?
4. 3.3: Classifying Matter According to Its State: Solid, Liquid, and Gas
5. 3.4: Classifying Matter According to Its Composition
6. 3.5: Differences in Matter: Physical and Chemical Properties
7. 3.6: Changes in Matter: Physical and Chemical Changes
8. 3.7: Conservation of Mass: There is No New Matter
9. 3.8: Energy
10. 3.9: Energy and Chemical and Physical Change
11. 3.10: Temperature: Random Motion of Molecules and Atoms
12. 3.11: Temperature Changes: Heat Capacity
13. 3.12: Energy and Heat Capacity Calculations
14. 3.E: Exercises

 •  Chapter 4

1. Chapter 4: Atoms and Elements
2. 4.1: Experiencing Atoms at Tiburon
3. 4.2: Indivisible: The Atomic Theory
4. 4.3: The Nuclear Atom
5. 4.4: The Properties of Protons, Neutrons, and Electrons
6. 4.5: Elements: Defined by Their Numbers of Protons
7. 4.6: Looking for Patterns: The Periodic Law and the Periodic Table
8. 4.7: Ions: Losing and Gaining Electrons
9. 4.8: Isotopes: When the Number of Neutrons Varies
10. 4.9: Atomic Mass: The Average Mass of an Element’s Atoms

  •  Chapter 5

1. Chapter 5: Molecules and Compounds
2. 5.1: Sugar and Salt
3. 5.2: Compounds Display Constant Composition
4. 5.3: Chemical Formulas: How to Represent Compounds
5. 5.4: A Molecular View of Elements and Compounds
6. 5.5: Writing Formulas for Ionic Compounds
7. 5.6: Nomenclature: Naming Compounds
8. 5.7: Naming Ionic Compounds
9. 5.8: Naming Molecular Compounds
10. 5.9: Naming Acids
11. 5.10: Nomenclature Summary
12. 5.11: Formula Mass: The Mass of a Molecule or Formula Unit

  •  Chapter 6

1. Chapter 6: Chemical Composition
2. 6.1: How Much Sodium?
3. 6.2: Counting Nails by the Pound
4. 6.3: Counting Atoms by the Gram
5. 6.4: Counting Molecules by the Gram
6. 6.5: Chemical Formulas as Conversion Factors
7. 6.6: Mass Percent Composition of Compounds
8. 6.7: Mass Percent Composition from a Chemical Formula
9. 6.8: Calculating Empirical Formulas for Compounds
10. 6.9: Calculating Molecular Formulas for Compounds

  •  Chapter 7

1. Chapter 7: Chemical Reactions
2. 7.1: Grade School Volcanoes, Automobiles, and Laundry Detergents
3. 7.2: Evidence of a Chemical Reaction
4. 7.3: The Chemical Equation
5. 7.4: How to Write Balanced Chemical Equations
6. 7.5: Aqueous Solutions and Solubility: Compounds Dissolved in Water
7. 7.6: Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid
8. 7.7: Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations
9. 7.8: Acid–Base and Gas Evolution Reactions
10. 7.9: Oxidation–Reduction Reactions
11. 7.10: Classifying Chemical Reactions
12. 7.11: The Activity Series

 •  Chapter 8

1. Chapter 8: Quantities in Chemical Reactions
2. 8.1: Climate Change: Too Much Carbon Dioxide
3. 8.2: Stoichiometry
4. 8.3: Making Molecules: Mole-to-Mole Conversions
5. 8.4: Making Molecules: Mass-to-Mass Conversions
6. 8.5: Limiting Reactant, Theoretical Yield, and Percent Yield
7. 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants
8. 8.7: Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction

Chapter 9

1. Chapter 9: Electrons in Atoms and the Periodic Table
2. 9.1: Blimps, Balloons, and Models of the Atom
3. 9.2: Light: Electromagnetic Radiation
4. 9.3: The Electromagnetic Spectrum
5. 9.4: The Bohr Model: Atoms with Orbits
6. 9.5: The Quantum-Mechanical Model: Atoms with Orbitals
7. 9.6: Quantum-Mechanical Orbitals and Electron Configurations
8. 9.7: Electron Configurations and the Periodic Table
9. 9.8: The Explanatory Power of the Quantum-Mechanical Model
10. 9.9: Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character

 •  Chapter 10

1. Chapter 10: Chemical Bonding
2. 10.1: Bonding Models and AIDS Drugs
3. 10.2: Representing Valence Electrons with Dots
4. 10.3: Lewis Structures of Ionic Compounds: Electrons Transferred
5. 10.4: Covalent Lewis Structures: Electrons Shared
6. 10.5: Writing Lewis Structures for Covalent Compounds
7. 10.6: Resonance: Equivalent Lewis Structures for the Same Molecule
8. 10.7: Predicting the Shapes of Molecules
9. 10.8: Electronegativity and Polarity: Why Oil and Water Don’t Mix

 •  Chapter 11

1. Chapter 11: Gases
2. 11.1: Extra-Long Straws
3. 11.2: Kinetic Molecular Theory: A Model for Gases
4. 11.3: Pressure: The Result of Constant Molecular Collisions
5. 11.4: Boyle’s Law: Pressure and Volume
6. 11.5: Charles’s Law: Volume and Temperature
7. 11.6: Gay-Lussac's Law: Temperature and Pressure
8. 11.7: The Combined Gas Law: Pressure, Volume, and Temperature
9. 11.8: Avogadro’s Law: Volume and Moles
10. 11.9: The Ideal Gas Law: Pressure, Volume, Temperature, and Moles
11. 11.10: Mixtures of Gases: Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
12. 11.11: Gases in Chemical Reactions

 •  Chapter 12

1. Chapter 12: Liquids, Solids, and Intermolecular Forces
2. 12.1: Interactions between Molecules
3. 12.2: Properties of Liquids and Solids
4. 12.3: Intermolecular Forces in Action: Surface Tension and Viscosity
5. 12.4: Evaporation and Condensation
6. 12.5: Melting, Freezing, and Sublimation
7. 12.6: Types of Intermolecular Forces: Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion-Dipole
8. 12.7: Types of Crystalline Solids: Molecular, Ionic, and Atomic
9. 12.8: Water: A Remarkable Molecule

 •  Chapter 13

1. Chapter 13: Solutions
2. 13.1: Prelude - Tragedy in Cameroon
3. 13.2: Solutions: Homogeneous Mixtures
4. 13.3: Solutions of Solids Dissolved in Water: How to Make Rock Candy
5. 13.4: Solutions of Gases in Water: How Soda Pop Gets Its Fizz
6. 13.5: Solution Concentration: Mass Percent
7. 13.6: Solution Concentration: Molarity
8. 13.7: Solution Dilution
9. 13.8: Solution Stoichiometry
10. 13.9: Freezing Point Depression and Boiling Point Elevation: Making Water Freeze Colder and Boil Hotter
11. 13.10: Osmosis: Why Drinking Salt Water Causes Dehydration

  •  Chapter 14

1. Chapter 14: Acids and Bases
2. 14.1: Sour Patch Kids and International Spy Movies
3. 14.2: Acids: Properties and Examples
4. 14.3: Bases: Properties and Examples
5. 14.4: Molecular Definitions of Acids and Bases
6. 14.5: Reactions of Acids and Bases
7. 14.6: Acid–Base Titration: A Way to Quantify the Amount of Acid or Base in a Solution
8. 14.7: Strong and Weak Acids and Bases
9. 14.8: Water: Acid and Base in One
10. 14.9: The pH and pOH Scales: Ways to Express Acidity and Basicity
11. 14.10: Buffers: Solutions That Resist pH Change

 

Contributions & Attributions

This page was constructed from content via the following contributor(s) and edited (topically or extensively) by the LibreTexts development team to meet platform style, presentation, and quality:

• Marisa Alviar-Agnew (Sacramento City College)

• Henry Agnew (UC Davis)