Introduction: Measurement
1.1) SI base units
1.2) Significant figures and scientific notation
1.3) Dimensional analysis

Elements, Compounds, Chemical equations and Stoichiometric calculations
2.1) Symbols, formulas and naming of elements, molecules and compounds.
2.2) Definitions of the atom, ion, molecule and compound. Mass relationships of atoms: atomic number,
mass number, and isotopes. Atomic masses (average), the mole concept/Avogadro’s number.
2.3) Molecular formula, empirical formula, molecular mass, formula mass, percent composition of compounds.
2.4) Experimental determination of empirical formulas and molecular formulas.
2.5) Writing and balancing chemical equations.
2.6) Stoichiometric calculations: Amounts of reactants and products, limiting reactants and reaction yield

Atomic Structure and Periodicity
3.1) Introduction to the electron, proton, neutron and isotopes.
3.2) Planck’s quantum theory, Bohr’s theory of the hydrogen atom (Rydberg equation)
3.3) Quantum Mechanics and the quantum numbers (n,l,ml,ms); Pauli’s exclusion principle, Hund’s rule and Aufbau’s principle.
3.4) Atomic orbitals and the electron configuration of atoms and ions.

Periodic Table
4.1) Development of the periodic table and the classification of the elements.
4.2) Periodic variation in physical properties: atomic and ionic radii, electronegativity, ionization energy and electron affinity.

Chemical bonding
5.1) Valence electrons and the Lewis dot symbol.
5.2) The ionic bond of ionic compounds
5.3) The covalent bond, the octet rule and writing Lewis structures for covalent molecules.
5.4) The VSEPR Model: Molecular Geometry
5.5) Dative covalent bond, hydrogen bond, van der Waal forces and metallic bond

Chemical Equilibrium
6.1) Kc and Kp
6.2) Equilibrium expressions
6.3) Factors affecting Kc and Kp
6.4) Conversion of Kc and Kp
6.5) Le Chatetier’s Principle
6.6) Effect of temperature, pressure, concentration and catalyst on chemical equilibrium

Acid-Base Reactions
7.1 Definitions of acid and base by Arrhenius, Bronsted-Lowry and Lewis.
7.2 Definition of weak/strong vs concentrated/dilute acids and bases.
7.3 Preparation of standard solutions and the dilution process.
7.4 Volumetric analysis, titration curves and indicator choice.
7.5 pH, pOH, Kw, pKw
7.6 Ka, Kb, pKa and pKb
7.7 Degree and percentage ionization
7.8 Buffer definition
7.9 Buffer action: acidic and basic buffer

Oxidation-Reduction (Redox) Reactions
8.1) The concept of oxidation states
8.2) The characteristics of oxidation-reduction reactions
8.3) Balancing oxidation-reduction reactions in acidic and basic medium.
8.4) Stoichiometry of redox reactions.

The Gaseous State
9.1) Substances that exist as gases and pressure of a gas.
9.2) The gas laws: Boyle’s law, Charles’ law and Gay-Lussac’s law, and Avogadro’s law.
9.3) Density calculations and molar mass determination of a gaseous substance.
9.4) Stoichiometry involving gases.
9.5) Dalton’s law of partial pressures.
9.6) Graham’s law of diffusion and effusion.

Q1 : What is the requirement to enroll this course?
A1 : No specific requirement as long as you have interest in basic chemistry