Topics
Basic Concepts of Chemistry and Chemical Calculations
- Chemistry - the Centre of Life
- Classification of Matter
- Atomic Mass
- Mole Concept
- Gram Equivalent Concept
- Empirical Formula and Molecular Formula
- Stoichiometry and Stoichiometric Calculations
- Concept of Redox Reactions
Quantum Mechanical Model of Atom
- Introduction to Atom Models
- Wave Particle Duality of Matter
- Heisenberg’s Uncertainty Principle
- Quantum Mechanical Model of Atom – SchröDinger Equation
- Quantum Numbers
- Filling of Orbitals
Periodic Classification of Elements
- Classification of Elements
- Classification of Elements
- Moseley's Work and Modern Periodic Law
- Nomenclature of Elements with Atomic Number Greater than 100
- Grouping of Elements Based on Electronic Configurations
- Periodic Trends in Properties of Elements
- Periodic Trends in Chemical Properties
Hydrogen
- Hydrogen
- Preparation of Hydrogen Peroxide
- Properties of Hydrogen
- Uses of Hydrogen Peroxide
- Compounds of Hydrogen
- Heavy Water
- Hydrogen Peroxide
- Hydrides
- Hydrogen Bonding
Alkali and Alkaline Earth Metals
- The s-Block Elements
- Group 1 Elements - Alkali Metals
- General Characteristics of the Compounds of Alkali Metals
- Biological Importance of Sodium and Potassium
- Group 2 Elements - Alkaline Earth Metals
- Important Compounds of Calcium Quick Lime, Cao
- Biological Importance of Magnesium and Calcium
Gaseous State
- The Gaseous State
- Gas Laws
- Ideal Gas Equation
- Mixture of Gases - Dalton’S Law of Partial Pressures
- Behaviour of Real Gases: Deviation from Ideal Gas Behaviour
- Derivation of Critical Constants from Van Der Waals Constant
- Liquefaction of Gases and Critical Constant
Thermodynamics
- Thermodynamics
- System and Surrounding
- Measurement of Temperature
- First Law of Thermodynamics
- Enthalpy (H)
- Thermochemical Equations
- Calorimetric Measurement of ΔU and ΔH
- Hess’s Law of Constant Heat Summation
- Lattice Energy
- Entropy and Second Law of Thermodynamics
- Various Statements of the Second Law of Thermodynamics
- Gibbs Free Energy (G)
- Absolute Entropy and Third Law of Thermodynamics
Physical and Chemical Equilibrium
- Physical and Chemical Equilibrium
- Introduction of Chemical Equilibrium
- Homogeneous Equilibria
- Equilibrium Constant
- Applications of Equilibrium Constants
- Le-Chatelier's Principle
- Van't Hoff Factor
Solutions
- Introduction to Solutions
- Types of Solutions
- Expressing Concentration of Solutions
- Solubility of the Solutes
- Solutions of Gases in Liquids
- Vapour Pressure of Liquid
- Vapour Pressure of Liquid Solutions
- Ideal and Non-ideal Solutions
- Colligative Properties
- Reverse Osmosis (RO)
- Abnormal Molar Masses
Chemical Bonding
- Concept of Chemical Bonding
- Ionic or Electrovalent Bond
- Coordinate Covalent Bond
- Bond Parameters
- Valence Shell Electron Pair Repulsion (VSEPR) Theory
- Valence Bond Theory (VBT)
- Valence Bond Theory - Orbital Overlap Concept
- Hybridisation
- Molecular Orbital Theory
Fundamentals of Organic Chemistry
- Organic Chemistry
- Classification of Organic Compounds
- Nomenclature
- Structural Representation of Organic Compounds
- Isomerism in Organic Compounds
- Detection of Elements: Lassaigne's Test
- Estimation of Elements
- Purification of Organic Compounds
Basic Concept of Organic Reactions
- Basic Concept of Organic Reactions
- Different Types of Organic Reactions
Hydrocarbons
- Introduction and Classification of Alkanes
- Alkanes
- Alkenes
- Alkynes
- Aromatic Hydrocarbons
Haloalkanes and Haloarenes
- Introduction to Haloalkanes and Haloarenes
- Classification of Organic Halogen Compounds
- Haloalkanes
- Organo Metallic Compounds
- Haloarenes
- Poly Halogen Compounds
Environmental Chemistry
- Atmospheric Pollution
- Types of Environmental Pollution
- Stratospheric Pollution
- Quality of Drinking Water
- Soil Pollution
- Strategies to Control Environmental Pollution
- Green Chemistry - Introduction
Estimated time: 2 minutes
CBSE: Class 12
Key Points: Third Law of Thermodynamics and Absolute Entropy
Third Law: The entropy of a perfectly ordered crystalline substance at absolute zero (0 K) is zero.
Absolute Entropy (Standard Molar Entropy, S°): The entropy value of a substance at 298 K and 1 bar pressure, relative to 0 K.
- Unlike the enthalpy of formation, the absolute entropy of elements is not zero at standard conditions.
- Standard entropy of reaction: \[\Delta_{r}S^{\circ}=\sum S_{products}^{\circ}-\sum S_{reactants}^{\circ}\]
