Detailed Course Description

The Atom
Ions
Matter and Mass
Mass and Weight
Properties of Matter
Elements and the Periodic Table
Compounds and Mixtures
States of Matter
Measurements
Density
The Metric System
SI Units
Conversion Problems
Significant Figures
Scientific Notation
Avogadro's Number
Percents and Percent Error
Lab 1: Volume Graphs

Introduction
Philosophers Contemplate Matter
Dalton 's Atomic Theory
Looking At Atoms
Investigating Atomic Structure
The Planetary Theory of Atomic Structure
Modern Atomic Theory
Subatomic Particles
The Atomic Nucleus
The Bohr Model of Atomic Structure
Quantum Theory
The Schroedinger Model of Atomic Structure
Atomic Particles
Atomic Number
Ions
Isotopes
Atomic Weight
Nuclear Chemistry
Radioactive Decay
Alpha Radiation
Beta Radiation
Gamma Radiation
Fission
Fusion
Bombardment

Atomic Structure
Atomic Number
The Discovery of the Electron
Electronic Orbits
Evidence for Electron Transitions
Photon Emission
The Electromagnetic Spectrum
Wavelengths and Frequencies
Contributions to Quantum Theory
Planck's Contribution
Einstein's Contribution [The Photoelectric Effect]
Bohr's Contribution
Quantum Theory
Electron Energy Levels
Sublevels Explained
Quantum Mechanics
Orbital Shape
Electrons as both Particles and Waves
Heisenberg's Uncertainty Principle
Wave/Particle Duality
Electrons In Orbit
Adding Electrons to Atoms
The Pauli Principle
Hund's Rule
Characterizing Electrons
Electron Energy Level Values
The Electron Energy Diagram
The Aufbau Principle
Building the Periodic Table

Historical Steps Behind the Periodic Table
Early Tables were Based on Atomic Mass
Dobereiner's Triads
Newlands' Octaves
Mendeleev – The Father of the Modern Periodic Table
Moseley Determined Atomic Number
The Modern Periodic Table Based on Atomic Number
The Modern Periodic Table
Each Element is Depicted by Its Symbol
Boxes, or Tags, Give Information About Elements
Occurring Isotopes
Periodic Table Arrangement 
Periodic Trends
State of Matter and Metallic Character
Atomic Radii
Ionic Radii
Ionization Energy
Electrons from Closed Shells
Electron Affinity 
Electronegativity

Introduction
Atomic and Molecular elements
Chemical Nomenclature
Naming the Elements
Appearance and Source
People and Places
Properties and Mythology
The Periodic Table
Categories of Elements
Atomic Structure
Ions
Monoatomic Cations
Monoatomic Anions
Stock System
Classical Method
Compounds
Chemical formulas
Compound names
Organic compounds
Inorganic compounds
Ionic and Molecular compounds
Naming Compounds
Naming Molecular compounds
Naming Ionic compounds
Polyatomic Ions
Naming Oxyanions
Naming Polyatomic Compounds
Naming Acids

A Review of Orbital Diagrams
Electron Configurations, and Valence Shells
The Octet Rule
Ionic Bonds
Lewis Dot Diagrams
Types of Ions
Naming Ions
Binary Ionic Compounds
Empirical Formulas
Properties of Ionic Compounds
Metallic Bonds
Properties of Metals
Covalent Bonds
Molecular Formulas
Lewis Structures
Multiple Bonds
Resonance Structures
Properties of Covalent Bonds
Lewis Structures
The Octet Rule
Common Molecular Shapes and Bond Angles
VSEPR Theory and Lone Pairs
Hybrid Orbitals
Sigma and Pi Bonds
Polarity
Electronegativity
Intermolecular forces: London Dispersion, Dipole Interactions, and Hydrogen Bonding
Intermolecular Forces Affect the Three States of Matter

Macroscopic Perspectives
Introduction/Safety
Properties – taste
Properties – litmus indicators
Properties – reactivity
Properties – conductivity
Molecular Concepts
Atomic Structure of Hydrogen
Solutions
Acids and Bases Defined
Arrhenius Model
Ionization – hydroxide and hydronium ions
The Chemistry of Water
Ion Product Constant Kw
Equilibrium Expression Molarity
Arrhenius Limitations
Bronsted-Lowry Model
Lewis Model
Classes of Acids
Acid Effects on Ion Concentrations
pH
Molarity and pH
The pH Scale
Calculating pH
Interactions of Acids & Bases
Strong Acids
Acid Dissociation Constant Ka
Strong Bases
Base Dissociation Constant Kb
Neutralization
Amphoteric Compounds
Conjugate Acids & Bases
Salts
Salt Formation
Characteristics of Salts
Properties of Salts - crystalline structure
Properties of Salts – melting point
Properties of Salts – conductivity
Common Salts
Acids & Bases & the Environment
Acid Rain Formation
Effects of Acid Rain
Lab 2: Acid-Base Titration

Solutions
Terminology
Solubility
Solutions Make Reactions Easier to Study
Ions Dissociate in Aqueous Solutions
Solutions of Molecular Compounds
Chemical Equations
Word Equations
Balancing Equations
Types of Reactions
Combination Reactions
Decomposition Reactions
Single-replacement Reactions
Double-replacement Reactions
Combustion Reactions

Atomic Mass
Atomic mass unit (AMU)
Isotopes
Molar mass
Determining Chemical Formulas
Percent composition
Empirical formulas
The Mole
Avogadro's number
Molecular weights
Formula weight
Atomic vs. Molecular mass
Conversion Equations
Moles to grams
Grams to moles
Particles in a sample
Balancing chemical equations
Stoichiometry
Mass to mass stoichiometry
Mass to volume stoichiometry
Volume to volume stoichiometry
Limiting reactants
Yield
Theoretical yield
Actual yield
Percent yield

Rates of Reactions
The Concept of Rates
Reaction Rates
Factors Affecting Reaction Rates
Nature of Reactants
Temperature
Catalysts
Surface Area
Concentration
Collision Theory
Kinetic Energy
Activation Energy
Why Increasing Temp. Increases Reaction Rates
The Activated Complex
Catalysts
Rate Laws
Rate is Proportional to Concentration of Reactants
Definition of Rate Law
Calculating the Rate Constant
Reaction Order
Reaction Mechanisms

Reactions Occur in Multiple Steps
Rate Laws and Elementary Processes*
The Rate-Determining Step
Evaluating Reaction Mechanisms
Lab 3: Chemical Change

Introduction
Heterogeneous Mixtures
Homogeneous Mixtures
Components of a Solution
Types of Solutions
Liquid and Aqueous Solutions
Solid Solutions
Gas Solutions
How Solutions Form
Factors That Affect the Dissolving Rate
Temperature
Stirring
Surface Area
Solution Concentrations
Relative Terms
Molarity
Molality
Mole Fraction
Percent Solutions
Solution Dilution
Colligative Properties
Vapor Pressure Reduction
Boiling Point Elevation
Freezing Point Depression
Osmotic Pressure
Determining Molar Mass

Chemical Equilibrium

Chemical Equilibrium
Chemical Equilibrium and Reversible Reactions
Concentration vs. Time Graphs
Achieving Chemical Equilibrium
Dynamic Process
Law of Mass Action
Equilibrium Constants
Equilibrium Constant Expressions
Heterogeneous Equilibria
Calculating Equilibrium Constants
Reaction Quotients
Le Chatelier's Principle
Disturbing Equilibrium
Le Chatelier's Principle
Effect of Changes in Concentration
Effect of Changes in pressure
Effect of Temperature on Equilibrium

Factors That Affect Solubility
Dissolution and Precipitation of Ionic Compounds
Equilibrium and Balanced Equations
The Equilibrium Expression
Solubility Product Constant (Ksp)
Factors Affecting Ionic Compound Solubility
The Common Ion Effect
pH
Precipitation Reactions of Ionic Compounds
Rules of Solubility
Separating Substances from Mixtures
Filtration
Crystallization
Distillation
Chromatography
Lab 4: Solubility