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Material Information
- Title:
- Introductory Chemistry Online!
- Creator:
- Young, Paul R. ( Author, Primary )
- Publisher:
- LibreTexts
- Publication Date:
- September 15, 2020
Notes
- Summary:
- Introductory Chemistry Online is an open-source introductory chemistry textbook/workbook that is designed cover a college-level one-semester course. Many contemporary textbooks in chemistry seem have adopted the notion that "more is better"; the books are long, expensive, and the pages are often cluttered with interesting tidbits and restatements of what it is that you have “just learned”. The Chemistry Online text, on the other extreme, is designed to be simple, uncluttered and very much to the point. -LibreTexts ( , )
- Scope and Content:
- 1: Measurements and Atomic Structure
1.1: Why Study Chemistry
1.2: Organization of the Elements - The Periodic Table
1.3: Scientific Notation
1.4: SI and Metric Units
1.5: Unit Conversion with the Metric System
1.6: Significant Figures
1.7: Atomic Structure and Electron Configuration
1.8: Filling Orbitals with Electrons
1.S: Measurements and Atomic Structure (Summary)
2: The Physical and Chemical Properties of Matter
In this chapter, we will look more closely at matter and break it into sub-classes including pure substances and mixtures. We will look at the physical state that matter can adopt (solids, liquids, and gasses) And we will learned how to characterized these using intensive properties such as density. Finally, we will look at changes in these properties and define them in terms of simple physical changes and chemical changes, where one or more substances combine to make new substances.
2.1: Pure Substances and Mixtures
2.2: The States of Matter
2.3: Density, Proportion and Dimensional Analysis
2.4: Chemical and Physical Properties and Changes
2.5: Conservation of Mass
2.S: The Physical and Chemical Properties of Matter (Summary)
3: Chemical Bonding and Nomenclature
3.1: Compounds, Lewis Diagrams and Ionic Bonds
3.2: Covalent Bonding
3.3: Lewis Representation of Ionic Compounds
3.4: Identifying Molecular and Ionic Compounds
3.5: Polyatomic Ions
3.6: Resonance
3.7: Electronegativity and the Polar Covalent Bond
3.8: Exceptions to the Octet Rule
3.9: Common Valence States and Ionic Compounds
3.10: Nomenclature of Ionic Compounds
3.11: Nomenclature of Molecular Compounds
3.S: Chemical Bonding and Nomenclature (Summary)
4: The Mole and Measurements in Chemistry
4.1: Measurement and Scale - The Mole Concept
4.2: Molar Mass
4.3: Mole-Mass Conversions
4.4: Percentage Composition
4.5: Empirical and Molecular Formulas
4.S: The Mole and Measurements in Chemistry (Summary)
5: Chemical Reactions
5.1: Chemical Changes and Chemical Reactions
5.2: Chemical Equations
5.3: Balancing Chemical Equations
5.4: Classifying Chemical Reactions
5.5: Oxidation and Reduction Reactions
5.6: Predicting Products from Chemical Reactions
5.7: Predicting Solubility Trends
5.8: The Energetics of Chemical Reactions
5.S: Chemical Reactions (Summary)
6: Quantitative Relationships in Chemistry
6.1: An Introduction to Stoichiometry
6.2: Molar Stoichiometry in Chemical Equations
6.3: Mass Calculations
6.4: Percentage Yield
6.5: Limiting Reactants
6.S: Quantitative Relationships in Chemistry (Summary)
7: Aqueous Solutions
Water is the most remarkable solvent! The O—H bonds in water are polarized due to the differences in electronegativity between hydrogen and oxygen. When this uneven charge distribution is coupled with the fact that water has a “bent” molecular geometry, the two covalent bond dipoles combine to form a molecular dipole (shown in the electrostatic potential map on the right. This molecular dipole allows water to surround and stabilize ions in solution, making water a powerful solvent.
7.1: Hydrogen Bonding and the Properties of Water
7.2: Molecular Dipoles
7.3: Dissolution of Ionic Compounds
7.4: Concentration and Molarity
7.5: Solution Stoichiometry
7.6: Dilution of Concentrated Solutions
7.S: Aqueous Solutions (Summary)
8: Acids, Bases and pH
8.1: Hydrogen Bonding
8.2: Ionization of Acids in Solution
8.3: Conjugate Acid-Base Pairs
8.4: Acids-Bases Reactions: Neutralization
8.5: The Meaning of Neutrality: The Autoprotolysis of Water
8.6: pH Calculations
8.7: Titrations - Neutralization and Stoichiometry
8.S: Acids, Bases and pH (Summary)
9: The Gaseous State
9.1: Gasses and Atmospheric Pressure
9.5: The Ideal Gas Law
9.6: Combining Stoichiometry and the Ideal Gas Laws
9.S: The Gaseous State (Summary)
9.2: The Pressure-Volume Relationship: Boyle’s Law
9.3: The Temperature-Volume Relationship: Charles’s Law
9.4: The Mole-Volume Relationship: Avogadro’s Law
10: Principles of Chemical Equilibrium
10.1: The Concept of Equilibrium Reactions
10.2: The Equilibrium Constant
10.3: Calculating Equilibrium Values
10.4: Using Molarity in Equilibrium Calculations
10.5: Equilibria involving Acids and Bases
10.6: The pH of Weak Acid Solutions
10.7: Solubility Equilibria
10.8: Study Points
11: Nuclear Chemistry
11.1: Radioactivity
11.2: The Nuclear Equation
11.3: Beta Particle Emission
11.4: Positron Emission
11.5: Radioactive Half-Life
11.6: Nuclear Fission
11.7: Nuclear Fusion
11.S: Nuclear Chemistry (Summary)
Back Matter
Index
Glossary
- Citation/Reference:
- Young, P. R. (2022, April 8). Introductory chemistry online! LibreTexts. Retrieved from https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Book%3A_Introductory_Chemistry_Online_(Young)
Record Information
- Source Institution:
- University of Illinois at Chicago
- Holding Location:
- LibreTexts
- Rights Management:
 This item is licensed with the Creative Commons Attribution Share Alike License. This license lets others remix, tweak, and build upon this work even for commercial reasons, as long as they credit the author and license their new creations under the identical terms.
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