General chemistry I

General Chemistry (I) Chapter 1: Significant Figures, Measuring Instruments and Stoichiometry 1-1 Chemistry a Basic science 1-1-1 Chemistry: Principles and Applications 1-1-2 Chemistry Science: A General Urgent 1-2 Measurement and Significant Figures 1-2-1 Significant Figures: Addition and Subtraction 1-2-2 Significant Figures: Multiplication and Division 1-2-3 Significant Figures: Logarithm 1-3 Measuring Instruments 1-3-1 Origin of Units of Measurement 1-3-2 Measurement Units and Mathematical Operations 1-3-3 Measurement Units and Conversion Factor 1-3-4 Temperature Measurement Units and Their Conversion 1-4 Compounds, Elements, Pure Substances, Molecules and Mixtures 1-5 The Origin of the Elements 1-6 Daltons Atomic Theory 1-7 Stoichiometry 1-7-1 Mole and Molecular Weight 1-7-2 Stoichiometry of Chemical Reactions 1-7-2-1 The Reaction Moles Method 1-7-2-2 The Conversion Factor Method 1-7-2-3 Limiting Reagents 1-7-2-4 Percent Yield 1-8 Nomenclature of Molecular and Ionic Compound Chapter 2: Atomic Structure and Quantum Theory 2-1 Subatomic Particles 2-1-1 The Discovery of Electrons: Cathodic Rays Experiment 2-1-2 Calculation of the (e/m) Ratio of the Electron: Thomson's Experiment 2-1-3 Determination of the Electron Charge: Millikan's Experiment 2-1-4 Discovery of the Atomic Nucleus (Proton and Neutron): Rutherford's and Chadovich's Experiments 2-1-5 Rutherford's and Thomson's Atomic Models 2-2 Electromagnetic Radiation: Classical theory of Radiation and Black Body Radiation 2-3 Planck's Quantum Theory 2-4 Photoelectric Effects 2-5 Atomic Spectra 2-6 Bohr's Atomic Theory 2-7 Dual Nature (Wave-Particle) of the Electron 2-8 The Heisenberg Uncertainty Principle 2-9 Schrödinger Equation 2-9-1 Particle in One-Dimensional Box and Schrödinger Equation 2-9-2 Hydrogen Atom and Schrödinger Equation 2-9-3 Quantum Numbers 2-9-4 Orbital Shape and Size 2-10 The Spin of the Electron (Stern-Gerlach Experiment) 2-11 Electronic Configuration of Atoms 2-11-1 Pauli Exclusion Principle 2-11-2 Hund’s Rule, Hund’s Rule of maximum multiplicity and Spin Magnetic Moment 2-11-3 Aufbau Principle Chapter 3: Periodic Table 3-1 General History of the Classification of the Elements 3-2 Periodic Table (Moseley’s and Mendeleev’s Viewpoints) 3-3 Metals, Nonmetals and Metalloids 3-4 Periodic Properties of the Elements in Periodic Table 3-4-1 Effective Nuclear Charge 3-4-2 Atomic and Ionic radii 3-4-3 Ionization Energy 3-4-4 Electron affinity 3-4-5 Electronegativity Chapter 4: Chemical Bonds: Covalence Bond and Molecular Structure 4-1 Ionic Bond 4-2 Covalence Bond 4-3 Lewis Structure 4-4 Formal Charge 4-5 Oxidation Number 4-6 Covalence Bond Length and Covalence Bond Energy 4-6-1 Bond Dissociation Energy 4-6-2 Dipole Moment and Polar Bands 4-6-3 Bond Energy and Electronegativity 4-7 Valence Bond Theory 4-7-1 Valence Bond Theory, Hybridization Theory and Molecular Geometry 4-7-1-1 Hybridized Orbitals of Main Group Elements 4-7-1-2 Hybridized Orbitals of Transition Metal Complexes 4-7-2 Valence Bond Theory and Resonance Structures 4-8 Valence Shell Electron Pair Repulsion (VSEPR) Theory: Molecular Geometry 4-9 Molecular Orbital Theory 4-9-1 Molecular Orbital Energy Diagram of Homonuclear Diatomic Molecules 4-9-2 Molecular Orbital Energy Diagram of Heteronuclear Diatomic Molecules 4-9-3 Molecular Orbital Theory and Electron Delocalization: π-Bonding in Benzene Molecule 4-10 Pπ-dπ Bond Chapter 5: Solids and Liquids 5-1 Adhesion Force and Kinetic Energy: Physical States 5-2 Intermolecular Forces 5-2-1 London forces 5-2-2 Hydrogen Bonding 5-2-3 Van der Waals Molecules and the Lennard-Jones Potential Function 5-3 Solids 5-3-1 Crystal System, Space Lattice and Unit Cells 5-3-2 Close-Packed Structures 5-3-3 Crystal Structure of Ionic Compounds 5-3-4 Lattice Energy of Ionic Crystals (Born-Haber Cycle) 5-4 Bond Length in Crystal Solids, X-ray diffraction 5-5 Crystal defect 5-6 Metallic Solids 5-6-1 Conductors and Semiconductors- Band Theory 5-7 Network solids 5-7-1 A Comparison of Chemical Properties of the Carbon and Silicon Compounds 5-8 Molecular Solids 5-9 Liquid Crystals 5-10 Liquids 5-10-1 Viscosity 5-10-2 Surface Tension 5-10-3 Distribution of Kinetic Energies of Molecules 5-10-3-1 Evaporation and Vapor Pressure of Liquids (The Clausius–Clapeyron Equation) 5-11 Phase Diagram Chapter 6: Gases, Behavior and Equation State 6-1 Properties of Gases 6-1-1 Gas Volume 6-1-2 Gas Pressure 6-1-3 Gas Temperature- Temperature from Molecular Viewpoint 6-2 Relation Between Variable (T, P, V) in the Gas State: State Function 6-2-1 Charles-Gay-Lussac Law: Temperature Dependence of Gas Pressure and Gas Volume 6-2-2 Boyle’s Law: Pressure Dependence of Gas Volume 6-2-3 Avogadro's Law 6-2-4 Ideal Gas Law 6-3 Ideal Gas Law Properties 6-3-1 Kelvin Scale Base on Ideal Gas Equation State 6-3-2 Pressure of Gas Mixtures: Dalton’s Law of Partial Pressure 6-3-3 Kinetic Theory of Gases and Equation State of Ideal Gas 6-4 Graham’s Law of Molecular Effusion 6-4-1 Separation of Gas and Isotopes 6-5 Relation Between of Density and Molecular Weight of Ideal Gas 6-6 Stoichiometry and Gas Reactions 6-7 Deviations from Ideal Gas: Real Gas 6-7-1 Van der Waals Equation state Chapter 7: Thermodynamic 7-1 Equilibrium: Properties of Equilibrium System 7-1-1 Thermal Equilibrium 7-1-2 Mechanical Equilibrium 7-1-3 Chemical Equilibrium 7-2 Chemical Equilibrium 7-2-1 A Qualitative study of Chemical Equilibrium 7-2-2 Factors That Affect Chemical Equilibrium: Le Chatelier's Principle 7-2-3 Quantitative study of Chemical Equilibrium: The Reaction Quotient and Equilibrium Constant 7-3 First Law of Thermodynamic 7-3-1 Work: Reversible and Irreversible Expansion 7-3-2 Heat: Heat Capacity in Constant Pressure and Constant Volume 7-3-3 Mathematical Relation of Thermodynamic First Law 7-3-4 Heat of Reaction in Constant Volume: Internal Energy (ΔE) 7-3-5 Heat of Reaction in Constant Pressure: Enthalpy (ΔH) 7-4 Thermochemistry 7-4-1 Hess’s Law 7-5 Factors That Affect Spontaneity of Chemical Reaction 7-5-1 Enthalpy Effect on Spontaneity of Chemical Reaction 7-5-2 Entropy Effect on Spontaneity of Chemical Reaction 7-5-3 Second Law of Thermodynamic: Gibbs Free Energy (ΔG) 7-5-4 The Relation Between Free Energy and Equilibrium Constant Chapter 8: Solutions 8-1 Compounds, Mixtures and Solutions 8-2 Solutions: Physical State 8-2-1 Gas Solution 8-2-2 Liquid Solution 8-2-3 Solid Solution 8-3 Factors That Affect Solubility 8-3-1 The Effect of Free Energy, Enthalpy and Entropy on Solubility 8-3-2 The Effect of Pressure and Temperature on Solubility 8-4 Concentration: Concentration Units 8-4-1 Mole Fraction and Percent 8-4-2 General Concentration 8-4-3 Molarity 8-4-4 Molality 8-4-5 Normality 8-4-6 ppm and ppb 8-4-7 Preparation of Solutions 8-5 Different Type of Solution 8-5-1 Ideal Solution, Raoult’s Law, Diagram of Vapor Pressure Versus Mole Fraction of a Two Components Solution 8-5-2 Real Solution: Diagram of Vapor Pressure Versus Mole Fraction of a Two Components Solution, Azeotrope Point 8-6 Separation by Distillation Method: Fractional Distillation 8-7 Colligative Properties of Electrolyte and Nonelectrolyte Solutions 8-7-1 Decreasing of Vapor Pressure 8-7-2 Increasing of Boiling Point 8-7-3 Decreasing of Freezing Point 8-7-4 Osmotic Pressure 8-7-4-1 Reverse Osmosis and Water Purification