2.0.Introduction 2.1. Sub Atomic Particles 2.1.1. Discovery of Electron 2.1.2. Charge to Mass Ratio of Electron 2.1.3. Charge on Electron 2.1.4. Discovery of Protons and Neutrons 2.2. Atomic Models 2.2.1. Thomson Model of Atom 2.2.2. Rutherford's Model of Atom 2.2.3. Atomic Number and Mass Number 2.2.4. Isobars and Isotopes 2.2.5. Drawbacks of Rutherford Model 2.3. Developments leading to the BOHR's Model of Atom 2.3.1. Wave Nature of Electromagnetic Radiation 2.3.2. Particle Nature of Electromagnetic Radiation: Planck's Quantum Theory 2.3.2.1.Photo Electric Effect 2.3.2.2.Duel Behaviour of Electromagnetic Radiation 2.3.3. Evidence for the Quantized Electronic Energy Levels: Atomic Spectra 2.3.3.1.Emission and Absorption Spectra 2.3.3.2.Line Emission Spectra 2.3.3.3.Rydberg Constant 2.4. BOHR's Model for Hydrogen Atom 2.4.1. Explanation of Line Spectrum of Hydrogen 2.4.2. Limitations of BOHR's Model 2.5. Towards Quantum Mechanical Model of Atom 2.5.1. Dual Behavior of Matter 2.5.2. Heisenberg's uncertainty Principle 2.5.3.Significance of Uncertainty Principle 2.5.4.Reasons for the failure of the BOHR Model 2.6. Quantum Mechanical Model of Atom 2.6.1. Orbitals and Quantum Numbers 2.6.1. Orbitals and Quantum Numbers 2.6.2. Shapes of Atomic Orbitals 2.6.3. Energies of Orbitals 2.6.3. Energies of Orbitals 2.6.4. Filling of Orbitals in Atom 2.6.5. Electronic Configuration of Atom 2.6.5. Electronic Configuration of Atom 2.6.6. Stability of Completely Filled and Half Filled Shells
1.Some Basic Points of Chemistry 2.Structure of Atom 3.Classification of Elements and Periodicity in Properties 4.Chemical Bonding and Molecular Structure 5.States of Matter 6.Thermodynamics 7.Equilibrium 8.Redox Reactions 9.Hydrogen 10.The s-Block Elements 11. The p-Block Elements 12.Organic Chemistry - Some Basic Principles and Techniques 13.Hydrocarbons 14.Environmental Chemistry