Matter: Definition. Pure substances, compounds, and mixtures; Atomic theory of matter.
Subatomic particles: protons, electrons, and neutrons. Atomic number and mass number.
Isotopes. Atomic mass.
Structure of the atom. Electromagnetic radiation and matter. Bohr atomic model.
Introduction to the quantum-mechanical description of the atom. Quantum numbers, atomic orbitals.
Pauli exclusion principle. Hund's rule. Aufbau method; Periodic table of the elements.
Periodic properties;
Chemical bonding: Ionic and covalent bonding, Lewis structures, bond lengths, energies, and polarity.
The concept of resonance. Formal charge and oxidation number. Molecular geometry: VSEPR theory. Valence bond theory: hybrid orbitals. Molecular polarity: intermolecular forces; States of matter. Gaseous state: ideal gas laws. Liquid and solid states: amorphous and crystalline solids. Phase transitions. Solutions.
Concentration. Colligative properties of solutions;
Chemical thermodynamics. Heat capacity. First law. Enthalpy: Hess's law.
Entropy: second law. Gibbs free energy and spontaneity of chemical reactions;
Chemical kinetics. Factors affecting reaction rate. Rate law. Reaction mechanism. Catalysis;
Chemical equilibrium. Equilibrium constant. Le Chatelier’s principle;
Acids and bases. Arrhenius and Brønsted–Lowry theories. Strength of acids and bases. Buffer solutions; Dissolution/precipitation equilibria. Solubility and solubility product.
Electrochemistry: redox reactions.
Stoichiometry
● Atomic and molecular mass, mole concept
● Chemical equations – balancing
● Mass relationships
Gaseous systems
Solutions – concept of concentration, colligative properties
Chemical equilibrium – equilibrium constants, shifts in equilibrium
● Salt solutions – Hydrolysis
pH concept: acid and base solutions
Buffer solutions
Solubility equilibria – Solubility product
Electrochemistry
