Atomic Structure and Periodic Table

1. Subatomic particles
2. Atomic number, mass number, and isotopes
3. Electron configuration (Bohr and quantum models)
4. Periodic trends (atomic radius, ionization energy, etc.)

Covalent Bonding and Molecular Geometry

1. Covalent bonding principles
2. Lewis structures and resonance
3. VSEPR theory
4. Molecular polarity and shape

Covalent Bonding: Orbitals

1. Valence Bond Theory
2. Hybridization (sp, sp², sp³)
3. Molecular Orbital Theory (introductory level)
4. Ionic and Metallic Bonding

• Ion formation and lattice energy
• Properties of ionic and metallic substances
• Crystal structures and conductivity

Chemical Reactions

1. Types of chemical reactions (synthesis, decomposition, etc.)
2. Predicting products
3. Balancing chemical equations
4. Activity series and reactivity

Stoichiometry

1. Mole concept and conversions
2. Empirical and molecular formulas
3. Limiting reactants and percent yield
4. Reaction calculations

States of Matter and Gas Laws

1. Kinetic Molecular Theory
2. Pressure, volume, temperature relationships
3. Boyle’s, Charles’s, Avogadro’s, and Ideal Gas Law
4. Gas mixtures and partial pressure

Thermochemistry

1. Heat vs. temperature
2. Calorimetry
3. Enthalpy changes and thermochemical equations
4. Hess’s Law

Solutions and Mixtures

1. Solubility and concentration (molarity, percent, ppm)
2. Dissociation and hydration
3. Colligative properties

Acids and Bases

1. Properties and definitions (Arrhenius, Brønsted–Lowry)
2. Strong vs. weak acids/bases
3. pH and pOH
4. Neutralization reactions

Acid-Base Equilibria

1. Acid and base dissociation constants (Ka and Kb)
2. pKa and pKb
3. Buffers and buffer calculations
4. Titration curves and indicators

Solubility and Complex Ion Equilibria

1. Solubility product constant (Ksp)
2. Common ion effect
3. Precipitation and selective precipitation
4. Complex ion formation and equilibrium

Chemical Kinetics and Equilibrium

1. Reaction rate factors
2. Rate laws and reaction mechanisms
3. Equilibrium constants (Kc and Kp)
4. Le Châtelier’s Principle

Nuclear Chemistry

1. Types of radioactive decay
2. Nuclear reactions: fission and fusion
3. Half-life calculations
4. Applications in medicine and energy

 Spontaneity & Entropy

1. Introduces entropy as a measure of disorder and explores the Second Law of Thermodynamics.
2. Students learn to calculate Gibbs Free Energy (ΔG) and determine whether reactions are spontaneous.
3. Emphasis on the relationship between enthalpy, entropy, and temperature in driving chemical processes.

Electrochemistry

1. Covers redox reactions, balancing methods, and electrochemical cells (galvanic and electrolytic).
2. Students learn to interpret standard reduction potentials and calculate cell voltages.
3. Real-world applications include batteries, corrosion, and electrolysis.

The Representative Elements

1. Focuses on the chemistry of Groups 1–2 and 13–18 in the periodic table.
2. Students explore common reactions, physical properties, and real-life uses of elements like alkali metals, halogens, and noble gases.
3. Trends like reactivity and electronegativity are reinforced across groups.

Transition Metals & Coordination Chemistry

1. Focuses on the unique behavior of transition metals, including variable oxidation states and colored compounds.
2. Covers ligands, naming coordination complexes, and the basics of crystal field theory.
3. Highlights real-world applications in medicine and biology (e.g., hemoglobin).

Organic and Biological Molecules

1. Introduces structure and reactivity of organic compounds like hydrocarbons and functional groups.
2. Explores key biomolecules: carbohydrates, proteins, lipids, and nucleic acids.
3. Connects chemistry to biological systems and polymers used in everyday life.