Class 11
- General Introduction: Importance and scope of Chemistry
- Nature of matter
- Laws of chemical combination
- Dalton's atomic theory
- Concept of elements, atoms and molecules
- Atomic and molecular masses
- Mole concept and molar mass
- Percentage composition
- Empirical and molecular formula
- Chemical reactions
- Stoichiometry and calculations based on stoichiometry
- Discovery of Electron, Proton and Neutron
- Atomic number
- Isotopes and isobars
- Thomson's model and its limitations
- Rutherford's model and its limitations
- Bohr's model and its limitations
- Concept of shells and subshells
- Dual nature of matter and light
- de Broglie's relationship
- Heisenberg uncertainty principle
- Concept of orbitals
- Quantum numbers
- Shapes of s, p and d orbitals
- Rules for filling electrons in orbitals — Aufbau principle, Pauli's exclusion principle and Hund's rule
- Electronic configuration of atoms
- Stability of half-filled and completely filled orbitals
- Significance of classification
- Brief history of the development of periodic table
- Modern periodic law and the present form of periodic table
- Periodic trends in properties of elements — atomic radii
- Periodic trends in properties of elements — ionic radii
- Periodic trends in properties of elements — inert gas radii
- Periodic trends in properties of elements — ionization enthalpy
- Periodic trends in properties of elements — electron gain enthalpy
- Periodic trends in properties of elements — electronegativity
- Periodic trends in properties of elements — valency
- Nomenclature of elements with atomic number greater than 100
- Valence electrons
- Ionic bond
- Covalent bond
- Bond parameters
- Lewis structure
- Polar character of covalent bond
- Covalent character of ionic bond
- Valence bond theory
- Resonance
- Geometry of covalent molecules
- VSEPR theory
- Concept of hybridization involving s, p and d orbitals and shapes of some simple molecules
- Molecular orbital theory of homonuclear diatomic molecules (qualitative idea only)
- Hydrogen bond
- Concepts of System and types of systems
- Surroundings
- Work
- Heat
- Energy
- Extensive and intensive properties
- State functions
- First law of thermodynamics - internal energy and enthalpy
- Heat capacity and specific heat
- Measurement of ∆U and ∆H
- Hess's law of constant heat summation
- Enthalpy of bond dissociation
- Enthalpy of combustion
- Enthalpy of formation
- Enthalpy of atomization
- Enthalpy of sublimation
- Enthalpy of phase transition
- Enthalpy of ionization
- Enthalpy of solution and dilution
- Second law of Thermodynamics (brief introduction)
- Introduction of entropy as a state function
- Gibb's energy change for spontaneous and non- spontaneous processes
- Criteria for equilibrium
- Third law of thermodynamics (brief introduction)
- Equilibrium in physical and chemical processes
- Dynamic nature of equilibrium
- Law of mass action
- Equilibrium constant
- Factors affecting equilibrium — Le Chatelier's principle
- Ionic equilibrium — ionization of acids and bases
- Strong and weak electrolytes
- Degree of ionization
- Ionization of polybasic acids
- Acid strength
- Concept of pH
- Hydrolysis of salts (elementary idea)
- Buffer solution
- Henderson equation
- Solubility product
- Common ion effect (with illustrative examples)
- Concept of oxidation and reduction
- Redox reactions
- Oxidation number
- Balancing redox reactions
- Oxidation–reduction in terms of loss and gain of electrons
- Oxidation–reduction in terms of change in oxidation number
- Applications of redox reactions
- General introduction
- Methods of purification
- Qualitative and quantitative analysis
- Classification and IUPAC nomenclature of organic compounds
- Electronic displacements in a covalent bond: inductive effect, electrometric effect, resonance and hyperconjugation
- Homolytic and heterolytic fission of a covalent bond
- Free radicals, carbocations, carbanions, electrophiles and nucleophiles
- Types of organic reactions
- Aliphatic Hydrocarbons
- Alkanes - Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions including free radical mechanism of halogenation, combustion and pyrolysis.
- Alkenes - Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov's addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition.
- Alkynes - Nomenclature, structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions: acidic character of alkynes, addition reaction of hydrogen, halogens, hydrogen halides and water.
- Aromatic Hydrocarbons
- Introduction, IUPAC nomenclature, benzene: resonance, aromaticity, chemical properties: mechanism of electrophilic substitution.
- Nitration, sulphonation, halogenation, Friedel–Crafts alkylation and acylation.
- Directive influence of functional group in mono-substituted benzene.
- Carcinogenicity and toxicity.