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Chem 1402:General Chemistry I
This text builds upon a knowledge foundation in chemistry and offers inquiry into topics of scientific measurement, chemical nomenclatures, expressing qualitative and quantitative statements about chemistry reactions, qualitative atomic theory, electronic and molecular structure models, chemical periodicity, thermochemistry, gases, kinetics molecular theory, and nuclear chemistry.
- Author
- Robert Belford
- Publisher
- University of Arkansas at Little Rock
- Source
- LibreTexts
- License
- CC BY-NC-SA
- Language
- EN
- Category
- Basic Sciences
Contents· 94 sections
- 1.A: Basic Concepts of Chemistry
- 1.01: Matter: Elements and Atoms Compounds and Molecules
- 1.02: Physical and Chemical Properties
- 1A.3: Classifying Matter
- 1A.4: Elements
- 1A.5: Compounds
- 1A.6: Physical Properties
- 1A.7: Physical and Chemical Changes
- 1A.8: Energy: Some Basic Principles
- 1.B: Review of the Tools of Quantitative Chemistry
- 1B.1: Units of Measurement
- 1B.2: Making Measurements: Experimental Error Accuracy Precision Standard Deviation and Significant Figures
- 1B.3: Mathematics in Chemistry
- 1B.4: Problem Solving by Dimensional Analysis
- 1B.5: Graphs and Graphing
- 1B.6: Algebra Review
- 2: Atoms Molecules and Ions
- 2.01: Atoms: Their Composition and Structure
- 2.02: Atomic Number and Atomic Mass Unit
- 2.03: Isotope Abundance and Atomic Weight
- 2.04: The Periodic Table
- 2.05: Chemical Compounds
- 2.06: Ionic Compounds and Formulas
- 2.07: Nomenclature
- 2.08: Atoms and the Mole
- 2.09: Molecules Compounds and the Mole
- 2.10: Percent Composition
- 2.11: Empirical and Molecular Formulas
- 2.12: Hydrates
- 3: Chemical Reactions
- 3.1: Introduction to Chemical Equations
- 3.2: Types of Chemical Reactions
- 3.3: Balancing Chemical Equations
- 3.4: Aqueous Reactions
- 3.5: Acid-Base Reactions
- 3.6: Redox Reactions
- 4: Stoichiometry: Quantitative Information about Chemical Reactions
- 4.1: Stoichiometry
- 4.2: Limiting and Excess Reagents
- 4.3: Percent Yield
- 4.4: Measuring Concentrations of Solutions
- 4.5: pH scale for concentration of Acids and Bases
- 4.6: Stoichiometry of Reactions in Aqueous Solutions
- 4.7: Chemical Equations and Quantitative Analysis
- 4.8: Spectrophotometry
- 5: Energy and Chemical Reactions
- 5.1: Energy
- 5.2: Heat Capacity
- 5.3: Energy and Phase Transitions
- 5.4: First Law of Thermodynamics
- 5.5: Enthalpy Changes of Chemical Reactions
- 5.6: Calorimetry
- 5.7: Enthalpy Calculations
- 6: The Structure of Atoms
- 6.1: Electromagnetic Radiation
- 6.2: Quantization: Planck Einstein Energy and Photons
- 6.3: Atomic Line Spectra and Niels Bohr
- 6.4: Wave-Particle Duality
- 6.5: The Modern View of Electronic Structure
- 6.6: The Shapes of Atomic Orbitals
- 6.7: Electron Spin and the Pauli Exclusion Principle
- 7: The Structure of Atoms and Periodic Trends
- 7.1: Orbitals of Polyelectronic Atoms
- 7.2: Electron Configurations of Atoms and Monatomic Ions
- 7.3: Atomic Properties and Periodic Trends
- 8: Bonding and Molecular Structure
- 8.1: Chemical Bond Formation: An Introduction
- 8.2: Covalent Bonding and Lewis Structures
- 8.3: Resonance
- 8.4: Formal Charge
- 8.5: Drawing Lewis Dot Structures
- 8.6: Molecular Geometries
- 8.7: Bond Polarity and Electronegativity ((chi))
- 8.8: Bond and Molecular Polarity
- 8.9: Covalent Bond Properties: Order Length and Energy
- 9: DNA Revisited
- 9: Orbital Hybridization and Molecular Orbitals
- 9.1: Orbitals and Theories of Chemical Bonding
- 9.2: Valence Bond Theory
- 9.3: Molecular Orbital Theory
- 10: Gases
- 10.1: Gas Properties
- 10.2 Gas Laws
- 10.3: Gas Phase Reactions
- 10.4: Gas Mixtures
- 10.5: Kinetic Molecular Theory of Gases
- 10.6: Diffusion and Effusion
- 10.7: Nonideal Gases
- 11: Intermolecular Forces and Liquids
- 11.1: States of Matter and Intermolecular Forces
- 11.2: Ion-Dipole Forces
- 11.3: Dipole-Dipole Forces
- 11.4: NonPolar Molecules and IMF
- 11.5: Hydrogen Bonds