Chemistry Olympiad Class Syllabus

Chapter 1 - Chemical Foundations
1.1 Chemistry: An Overview
1.2 Units of Measurement
1.3 Uncertainty in Measurement
1.4 Significant Figures and Calculations
1.5 Temperature
1.6 Density
1.7 Classification of Matter
1.8 Elements and Compounds

Chapter 2 – The Structure of the Atoms
2.1 The Early History of Chemistry
2.2 Fundamental Chemical Laws
2.3 Dalton's Atomic Theory
2.4 Early Experiments to Characterize the Atom
2.5 Olympiad Exam

Chapter 3 - Atomic Structure and Periodicity
3.1 Electromagnetic Radiation
3.2 The Particle Nature of Light
3.3 The Wave-Particle Duality of Matter
3.4 The Atomic Spectrum of Hydrogen
3.5 The Bohr Model
3.6 The Quantum Mechanical Model of the Atom
3.7 Quantum Numbers
3.8 Orbital Shapes and Energies
3.9 Electron Spin and the Pauli Principle
3.10 Polyelectronic Atoms
3.11 The Aufbau Principle
3.12 Classification of the elements
3.13 The History of the Periodic Table
3.14 Periodic Trends in Atomic Properties
3.15 Atomic Properties and Chemical Reactivity
3.16* Shielding
3.17 Challenge and Integrative Problems
3.18 Olympiad Exam

Chapter 4 - Bonding: General Concepts
4.1 Types of Chemical Bonds
4.2 The formation of the ionic bonds
4.3 Energy Effects in Binary Ionic Compounds
4.4 Predicting Formula of Ionic compounds
4.5 The Covalent Chemical Bonds
4.6 Electronegativity and Bond Polarity
4.7 The Metallic Bonds
4.8 Naming Simple Compounds
4.9 Molecular Structures
4.10 Lewis Structures
4.11 Exceptions to the Octet Rule
4.12 Resonance
4.13 Molecular Structure: The VSEPR Model
4.14* Electronegativity and Bond Angles
4.15 Bond Polarity and Dipole Moments
4.16 Covalent Network Solids
4.17 Oxidation States (Numbers)
4.18 Challenge and Integrative Problems
4.19 Olympiad Exam
Chapter 5 - Covalent Bonding: Orbitals
5.1 Hybridization and the Localized Electron Model
5.2 Hybridization
5.3 Molecular orbitals
5.4 Challenge and Integrative Problems
5.5 Olympiad Exam

Chapter 6 - Chemical Reactions 
6.1 Reactions and Equations
6.2 The Reactions in Aqueous Solutions
6.3 The Nature of Aqueous Solution
6.4 The Reactions That Form Precipitate, Gases and Water
6.5 Oxidation-Reduction Reactions
6.6 Balancing Oxidation-Reduction Equations
6.7 Challenge and Integrative Problems
6.8 Olympiad Exam

Chapter 7 - Stoichiometry
7.1 Atomic Masses
7.2 The Mole
7.3 Molar Mass
7.4 Percent Composition of Compounds
7.5 Determining the Formula of a Compound
7.6 Stoichiometry
7.7 Stoichiometric Calculations: Amounts of Reactants and Products
7.8 Calculations Involving a Limiting Reactant
7.9 Calculating Percent Yield
7.10 The Composition of Solutions
7.11 Challenge and Integrative Problems
7.12 Olympiad Exam

Chapter 8 – Gases
8.1 Pressure
8.2 The Gas Laws of Boyle, Charles, Avogadro, and Gay-Lussac
8.3 The Ideal Gas Law
8.4 Applications of ideal Gas Law
8.5 Gas Stoichiometry
8.6 Gas Density and Molar Mass of a Gas
8.7 The Stoichiometry of Reaction Gases
8.8 Dalton's Law of Partial Pressures
8.9 The Kinetic Molecular Theory of Gases
8.10 Effusion and Diffusion
8.11 Real Gases
8.12 The Liquefaction of Gas
8.13 Chemistry in the Atmosphere
8.14 Challenge problems
8.15 Olympiad Exam

Chapter 9 - Liquids and Solids
9.1 Intermolecular Forces
9.2 Intermolecular Forces and Biological Macromolecules
9.3 The Liquid State
9.4 An Introduction to Structures and Types of Solids
9.5 Structure and Bonding in Metals
9.6 Carbon and Silicon: Network Atomic Solids
9.7 Molecular Solids
9.8 Ionic Solids
9.9 Vapor Pressure and Changes of State
9.10 Phase Diagrams
9.11 Challenge problems
9.12 Olympiad Exam

Chapter 10 - Properties of Solutions 
10.1 Solution Composition
10.2 The Energies of Solution Formation
10.3 Factors Affecting Solubility
10.4 Colligative Properties of Electrolyte Solutions
10.5 Boiling-Point Elevation
10.6 Freezing-Point Depression
10.7 Osmotic Pressure
10.8 Colligative Properties of Electrolyte Solutions
10.9 Colloids
10.10 Challenge problems
10.11 Olympiad Exam

Chapter 11 - Chemical Kinetics
11.1 Reaction Rates
11.2 The instantaneous Rate of Reaction
11.3 Rate Laws: An Introduction
11.4 Determining the Form of the Rate Law
11.5 The Integrated Rate Law
11.6 Rate Laws: A Summary
11.7 Reaction Mechanism
11.8 Rates and Equilibrium
11.9 A Model for Chemical Kinetics
11.10 Factors Affecting Reaction Rates
11.11 Challenge problems
11.10 Olympiad Exam

Chapter 12 - Chemical Equilibrium
12.1 The Equilibrium Condition
12.2 The Equilibrium Constant
12.3 Equilibrium Expressions Involving Pressures
12.4 Heterogeneous Equilibra
12.5 Applications of the Equilibrium Constant
12.6 Factors Affecting the Equilibrium --- Le Châtelier's Principle
12.7 Catalysts and Equilibrium
12.8 Rate and Equilibrium
12.9 Solubility Equilibra and the Solubility Product
12.10 Applications of the Solubility Product
12.11 Challenge problems
12.12 Olympiad Exam

Chapter 13 - Acids and Bases
13.1 The Nature of Acids and Bases
13.2 Acid Strength
13.3 The pH Scale
13.4 Calculating the pH of Strong Acid Solutions
13.5 Calculating the pH of Weak Acid Solutions
13.6 Bases
13.7 Polyprotic Acids
13.8 Molecular Structure and Acid Strength
13.9 Acid-Base Properties of Salts
13. 10* Calculate the pH of a Salt for Weak Acid and Weak Base       
13. 11* Generalizing the BrΦnsted-Lowry Concept: The Leveling effect
13.12 Calculate the pH of Salts of Polyprotic Acid
13.13 Composition and pH
13.14 Acid-Base Properties of Oxides
13.15 The Lewis Acid-Base Model
13.16 Challenge problems
13.17 Olympiad Exam

Chapter 14 - Applications of Aqueous Equilibria
14.1 Solutions of Acids or Bases Containing a Common Ion
14.2 Buffered Solutions
14.3 Buffering Capacity
14.4 Analytical Standards
14.5 Titrations and pH Curves
14.6: Stoichiometry of Polyprotic Acid Titrations
14.7 Acid-Base Indicators
14.8 Quantifying Redox Reactions by Titration
14. 9 Back Titration
14.10 Challenge problems
14.11 Olympiad Exam

Chapter 15 – Thermodynamics: The First Law
15.1 The Nature of Energy
15.2 System and States
15.3 Work and Energy
15.4 Heat and Energy
15.5 The First Law
15.6 Enthalpy
15.7 The Enthalpy of Physical Change
15.8 Heating Curves
15.9 Enthalpy (Heat) in Chemical Reactions and Processes
15.10 Thermochemical Equations
15.11 Calculating Enthalpy Change --- Hess's Law
15.12 Standard Enthalpies of Formation
15.13 The Born-Haber Cycle
15.14 Bond Enthalpies
15.15 Bond Strengths and the Heat Released from Fuels and Foods
15.16 Challenge Problems
15.17 Olympiad Exam

Chapter 16 - Thermodynamics: The Second and Third Laws
16.1 Spontaneous Processes and Entropy
16.2 Changes in Entropy
16.3 Entropy Changes Accompanying Changes in Physical Stats
16.4 Standard Molar Entropies
16.5 The Surroundings
16.6 The Overall change in Entropy
16.7 Equilibrium
16.8 Free Energy
16.9 Free Energy and Chemical Reactions
16.10 The Dependence of Free Energy on Pressure
16.11 Free Energy and Equilibrium
16.12 Challenge Problems
16.13 Olympiad Exam

Chapter 17 - Electrochemistry
17.1 Galvanic Cells
17.2 Standard Reduction Potentials
17.3 Cell Potential, Electrical Work, and Free Energy
17.4 Latimer diagrams
17.5 Dependence of Cell Potential on Concentration
17.6 Calculation of Equilibrium Constants
17.7 Batteries
17.8 Electrolysis
17.9 Commercial Electrolytic Processes
17.10 Corrosion
17.11 Challenge Problems
17.12 Olympiad Exam

Chapter 18 - The Nucleus: A Chemist's View
18.1 Nuclear Stability and Radioactive Decay
18.2 The Kinetics if Radioactive Decay
18.3 Nuclear Transformations
18.4 Detection and Uses of Radioactivity
18.5 Thermodynamic Stability of the Nucleus
18.6 Nuclear Fission and Nuclear Fusion
18.7 Challenge Problems