General Chemistry with Elements of Physical Chemistry

Atomic structure: Nuclides, isotopes and chemical elements. Molecular formula and formula unit. Atomic mass and molecular mass. Mole and Avogadro constant. Quantization of energy and photons. Atomic models. Orbitals and quantum numbers. Electronic configuration of the elements. Periodic table of elements and periodic properties.
Chemical bond and molecular geometry: Lewis structures. Ionic and covalent bonds. Electronegativity and bond polarity. Molecular geometry: VSEPR and valence bond theory. Intermolecular interactions.
Formulas and systematic nomenclature.
Solutions: Concentration. Dilution. Molar fraction. Colligative properties.
Chemical reactions: Chemical reactions and chemical equations. Balance and principle of mass conservation. Net ionic equation and principle of charge conservation. Chemical equilibrium: equilibrium constant and reaction quotient. Le Chatelier's principle. Reactions in aqueous solution: electrolytes and non-electrolytes, precipitation reactions and solubility equilibria, acid-base reactions, oxidation-reduction reactions.
Gaseous state: Pressure and temperature. Ideal gas law. Molar volume. Ideal gas constant. Gaseous mixtures: partial pressure and partial volume, Dalton's law.
Acids and bases: Definitions of acid and base. Acid-base equilibria. Calculation of pH. Buffer solutions. Titration curves.
Chemical thermodynamics: State functions. First principle of thermodynamics. Enthalpy. Exothermic and endothermic reactions. Standard conditions. Second principle of thermodynamics. Entropy. Gibbs free energy.
Electrochemistry: Electrochemical cells and standard potentials. Cell potential and equilibrium constant. Nernst's equation.

Program information:
Electrons in Atoms: Atomic particles and their properties. Chemical Elements. Atomic Weights, Formula Weights and Molecular Weights. The Avogadro Constant and the concept of the Mole. Quantum Theory. The Bohr Atom. The Uncertainty Principle. Quantum Numbers and Electron Orbitals. Electron Spin. Multielectron Atoms. Electron Configurations of the Elements.
The Periodic Law and the Periodic Table. Electron Configuration and the Periodic Table. Periodic properties: Metals and Nonmetals, Atomic Radius, Ionization Energy, Electron Affinity.
Chemical Bonding: Lewis theory. Ionic and Covalent Bonding. Electronegativity. Lewis Structures. Resonance. Exceptions to the Octet Rule. VSEPR Theory and Molecular Shapes. Introduction to the Valence Bond Theory. Hybridization of Atomic Orbitals. Intermolecular forces.
Formulas and systematic nomenclature: Oxidations States. Systematic Nomenclature of Inorganic Compounds.
Solutions: Solution Concentration. Solution Dilution. Vapour Pressures of Solutions. Freezing Point. Depression and Boiling Point Elevation, Osmotic pressure.
Chemical Reactions: Chemical reactions and the Chemical Equation. Balancing. Determining the Limiting Reagent. Chemical Equilibrium. The Equilibrium Constant Expression. The reaction Quotient. Le Chatelier's Principle. Reactions in aqueous solutions: electrolytes and nonelectrolytes, Precipitation Reactions, Acid-Base Reactions, Oxidation-Reduction Reactions.
Gases: The concept of Pressure and absolute Temperature. The Gas Laws: Boyle's law, Charles's Law and Avogadro's Law The Ideal Gas Equation. Mixtures of gases: partial pressure and partial volume. Dalton's Law and Amagat's Law. Real gas.
Acids and Bases: Arrhenius Theory. Bronsted-Lowry Theory. Strong Acids and Strong Bases. Self-ionization of water. Definition of pH and pOH. Weak Acids and Weak Bases. Polyprotic Acids. Hydrolysis. Buffer Solutions. Neutralization reactions and Titration Curves.
Thermochemistry: Functions of State. The First Law of Thermodynamics. Enthalpy. Entropy. The Second Law of Thermodynamics. Standard Free Energy Change. Free Energy Change and Equilibrium.
Electrochemistry: Electrochemical cells, standard reduction potentials