General and Inorganic Chemistry

Matter and states of matter. Classification of matter (elements, compounds, and mixtures).
Properties of matter. Introduction to modern atomic theory. Chemical symbols, atomic number, and mass number. Isotopes. Atomic masses, mole and molar mass.
Introduction to the periodic table. Pure compounds: molecules and ionic compounds.
Empirical formula, molecular formula, and structural formula. Chemical reactions and chemical equations. Balancing reactions. Stoichiometric calculations: theoretical yield and percent yield, limiting reagent and excess reagent.
Solutions. Strong, weak, and non-electrolytes. Oxidation numbers. Redox reactions.
Wave nature of light. Electromagnetic radiation. Quantization of energy. Blackbody problem and photoelectric effect. Line emission spectra. Bohr's atomic model. Quantum mechanics. Heisenberg's uncertainty principle. Schrödinger equation, wave functions, and probability density. Quantum numbers and atomic orbitals. Shielding effect and orbital energies. Orbital diagrams. Electronic configurations of atoms. Pauli exclusion principle and Hund's rule. Periodic properties: atomic and ionic sizes, ionization energy, electron affinity. Electronegativity.
Covalent and ionic bonding. Lewis structures. Multiple bonds. VSEPR theory (Valence Shell Electron Pair Repulsion). Electron domain geometries and molecular geometries. Lone pairs, single bonds, and multiple bonds: effect on molecular geometry. Bond polarity and molecular polarity. Correlation between geometry and polarity of molecules.
Valence bond theory. Hybrid orbitals and electron domain geometry. Sigma and pi bonds (single and double bonds). Isomers. Cis-trans isomerism.
Diamagnetism and paramagnetism. Molecular orbital theory. Bonding and antibonding orbitals (sigma and pi types). Bond order. Orbital energies for diatomic molecules. Nonbonding orbitals. Resonance.
Gases at the molecular level - ideal gases. Pressure (and its units of measurement). Gas laws (ideal): Boyle (V∝1/P), Charles (V∝T), Gay-Lussac (P∝T), and Avogadro (V∝n). Ideal gas law. Gas mixtures, partial pressures, and partial volumes.
Intermolecular forces. Ion-dipole, dipole-dipole, and London (dispersion) interactions. Hydrogen bonding. Some properties of liquids: surface tension, viscosity, and capillary action.
State functions. Enthalpy, standard enthalpy of formation, enthalpy of reaction.
The solid state. Crystalline solids. Ionic, metallic, molecular, and covalent solids. Phase changes and phase diagrams.
Unsaturated, saturated, and supersaturated solutions. Solubility. Effect of temperature and pressure on the solubility of gases. Colligative properties.
Introduction to chemical equilibrium. Equilibrium constants. Le Chatelier's principle.
Acids and bases. Arrhenius theory and its limitations. Brønsted-Lowry theory. Ion product of water. Conjugate acid-base pairs. Strength of acids and bases. Polyprotic acids. pH scale and pH calculation. Relationship between Kw, Ka, and Kb.
Solubility and solubility product. Precipitation reactions. Complex ions. Ionic, neutral, monodentate, and polydentate ligands. Formation equilibria of complexes (and effect on solubility). Other reactions in solution: gas-evolving reactions (and effect on solubility).
Entropy, Gibbs free energy. Spontaneity of chemical reactions.
Elements of chemical kinetics. Average and instantaneous reaction rates. Rate laws and rate constants. Integrated rate equations and half-life (first-order kinetics). Collision theory. Activation energy. Catalysts. Kinetic and thermodynamic aspects and spontaneity of reactions.
Voltaic cells, cell potential. Standard reduction potentials. Spontaneity of reactions. Dissolution of metals in acids and metal corrosion. Gibbs free energy and potential difference. Dependence of cell potential on concentrations: Nernst equation.
Radioactive decay. Types of decay (alpha, beta-, gamma, beta+, electron capture). Decay series. Kinetics of radioactive decay. Formation of 14C and its importance for dating materials.