Chemistry Class 11 CBSE (Science) CBSE Topics and Syllabus

• Importance of Chemistry 
• Historical Approach to Particulate Nature of Matter 
• Nature of Matter 
• Properties of Matter and Their Measurement 
  • The International System of Units (Si) 

    Base Physical Quantities and their Units, Definitions of SI Base Units, Prefixes used in the SI System
    

  • Mass and Weight 

    Volume, Density, Temperature

• Uncertainty in Measurement 
  • Scientific Notation 

    Multiplication and Division, Addition and Subtraction

  • Significant Figures 

    Addition and Subtraction of Significant Figures, Multiplication and Division of Significant Figures, Precision, Accuracy

  • Dimensional Analysis 
• Laws of Chemical Combination 
  • Law of Conservation of Mass 
  • Law of Definite Proportions 
  • Law of Multiple Proportions 
  • Gay Lussac’S Law of Gaseous Volumes 
  • Avogadro Law 
• Dalton'S Atomic Theory 
• Atomic and Molecular Masses 
  • Atomic Mass 
  • Average Atomic Mass 
  • Molecular Mass 
  • Formula Mass 
• Mole Concept and Molar Masses 
  • Mole
  • Molar Mass
• Percentage Composition 

  Empirical Formula for Molecular Formula

• Stoichiometry and Stoichiometric Calculations - Introduction 
• Limiting Reagent 
• Stoichiometry and Stoichiometric Calculations - Reactions in Solutions 

  Mass per cent or weight per cent (w/w %), Mole fraction, Molarity, Molality

• Introduction of Some Basic Concepts of Chemistry 

General Introduction: Important and scope of chemistry. 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 and empirical and molecular formula; chemical reactions, stoichiometry and calculations based on stoichiometry.

• Subatomic Particles 
  • Discovery of Electron 
  • Charge to Mass Ratio of Electron 
  • Charge on the Electron 
  • Discovery of Protons and Neutrons 

    Millikan’s Oil Drop Method

• Concept of Atomic Models 
• J. J. Thomson’s Atomic model 
• Lord Rutherford’s Atomic model 
• Atomic Number (Z) 
• Mass Number (A) or Atomic Mass 
• Isobars 
• Isotopes 
• Drawbacks of Rutherford Atomic Model 
• Wave Nature of Electromagnetic Radiation 
• Electromagnetic Waves : Numericals 
• Particle Nature of Electromagnetic Radiation: Planck'S Quantum Theory 

  Photoelectric Effect, Dual Behaviour of Electromagnetic Radiation

• Evidence for the Quantized Electronic Energy Levels - Atomic Spectra 

  Emission and Absorption Spectra, Line Spectrum of Hydrogen

• Bohr'S Model for Hydrogen Atom 
  • The Spectral Lines for Atomic Hydrogen
  • Explanation of Line Spectrum of Hydrogen
  • Limitations of Bohr’s Model
• Towards Quantum Mechanical Model of the Atom 
  • Dual Behaviour of Matter 

    de Broglie's relationship

  • Heisenberg’S Uncertainty Principle 

    Significance of Uncertainty Principle, Reasons for the Failure of the Bohr Model

• Concept of Quantum Mechanical Model of the Atom 

  Hydrogen Atom and the Schrödinger Equation

• Quantum Mechanical Model of the Atom - Orbitals and Quantum Numbers 
• Quantum Mechanical Model of the Atom - Concept Of Shells and Subshells 
• Quantum Mechanical Model of the Atom - Shapes of Atomic Orbitals 

  shapes of s,p and d orbitals

• Quantum Mechanical Model of the Atom - Energies of Orbitals 
• Quantum Mechanical Model of the Atom - Filling of Orbitals in Atom 

  Aufbau Principle, Pauli Exclusion Principle, Hund’s Rule of Maximum Multiplicity

• Quantum Mechanical Model of the Atom - Electronic Configuration of Atoms 
• Quantum Mechanical Model of the Atom - Stability of Completely Filled and Half Filled Subshells 

  Symmetrical distribution of electrons, Exchange Energy

• Structure of Atom Numericals 

Discovery of Electron, Proton and Neutron, Atomic number, isotopes and isobars. Concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship, Heisenberg uncertainty principle, concept of orbital, quantum numbers, shapes of s,p and d orbitals, rules for filling electrons in orbitals- Aufbau principle, Pauli exclusion principles and Hund’s rule, electronic configuration of atoms, stability of half filled and completely filled orbitals

• Significance of Classification of Elements 
• Genesis of Periodic Classification 

  Dobereiner’s Triads, Newlands’ Octaves, Mendeleev’s Periodic Table

• Modern Periodic Law and the Present Form of the Periodic Table 

  Extra nuclear structure as the basis of periodicity

• Nomenclature of Elements with Atomic Number Greater than 100 

  Notation for IUPAC Nomenclature of Elements

• Periodic Table and Electronic Configuration 
  • Electronic Configurations in Periods
  • Electronic configuration in groups
  • Electronic configuration in the four blocks - s-Block, p-Block, d-Block, f-Block
• Electronic Configurations and Types of Elements 
  • The s-Block Elements 
  • The p-Block Elements 
  • The d-Block Elements (Transition Elements) 
  • The f-Block Elements (Inner-transition Elements) 
    • Electronic configuration of Lanthanoids
    • Oxidation state of lanthanoids
    • Cause of lanthanoid contraction
    • Oxidation state of actinoids
    • Differences between lanthanoids and actinoids
  • Metals, Non-metals and Metalloids 
• Physical Properties 
  • Atomic Radius 
  • Ionic Radius 
  • Ionization Enthalpy 
  • Electron Gain Enthalpy 
  • Electronegativity 
• Periodic Trends in Chemical Properties 
  • Periodicity of Valence Or Oxidation States 
  • Anomalous Properties of Second Period Elements 
• Periodic Trends and Chemical Reactivity 
• Classification of Elements and Periodicity in Properties Numericals 

Significance of Classification, brief history of the development of Periodic table, Modern periodic law and long form of periodic table, periodic trends in properties of elements- atomic radii, ionic radii, ionization enthalpy, electron gain enthalpy, electronegativity, valence. Nomenclature of elements with automic number greater than 100.

• Concept of Kossel-lewis Approach to Chemical Bonding 
  • Ionic bond
    I. Formation of sodium chloride (NaCl)
    II. Formation of calcium chloride (CaCl₂)
  • Ionic solids and Lattice Enthalpy
  • Covalent bond 
    I. Formation of H₂ molecule
    II. Formation of Cl₂
    III. Formation of Multiple bonds
  • Lewis structures (Lewis representations of simple molecules)
  • Steps to write Lewis dot structures
• Kossel-lewis Approach to Chemical Bonding - Octet Rule 
• Kossel-lewis Approach to Chemical Bonding - Covalent Bond 
• Kossel-lewis Approach to Chemical Bonding - Lewis Representation of Simple Molecules (The Lewis Structures) 
• Kossel-lewis Approach to Chemical Bonding - Formal Charge 
• Kossel-lewis Approach to Chemical Bonding - Limitations of the Octet Rule 
  • Molecules with an incomplete octet
  • Molecules with an expanded octet
  • Odd electron molecules
• Concept of Ionic Or Electrovalent Bond 
  • Factors influencing the formation of ionic bond, e.g electron gain enthalpy, ionisation enthalpy, lattice energy and electronegativity
  • Lattice Enthalpy
• Bond Parameters 
  • Bond Length 
  • Bond Angle 
  • Bond Enthalpy 
  • Bond Order 
  • Resonance Structures 

    resonance, geometry of covalent molecules

  • Polarity of Bonds 

    covalent character of ionic bond

• The Valence Shell Electron Pair Repulsion (Vsepr) Theory 
  • Rules of VSEPR
    1. Ammonia NH₃ 
    2. Water molecule H₂O
  • Advanced theories of Bonding
• Valence Bond Theory 
  • Postulates of Valence Bond Theory
  • Interacting forces during covalent bond formation
  • Overlap of atomic orbitals -
    1. sigma bond (σ)
    a. s-s overlap
    b. p-p overlap
    c. s-p σ bond
    2. pi bond (π)
  • Hybridization
  • Steps considered in Hybridization
    i) Formation of the excited state
    ii) Mixing and Recasting of orbitals
  • Types of Hybridization and Geometry of Molecules 
    i) sp3 Hybridization - Formation of methane (CH₄) molecule
    ii) sp² Hybridization - Formation of C₂H₄ molecule
    iii) sp hybridization - Formation of acetylene molecule
  • Importance and limitation of valence bond theory
  • Limitations of valence bond theory
  • Salient features of VB Theory
• Valence Bond Theory - Orbital Overlap Concept 
  • Sigma and Pi bonds
  • Formation of hydrogen (H₂) Molecule 

  1. Formation of fl uorine molecule (F₂)
  2. Formation of HF molecule
  3. Formation of oxygen molecule (O₂)
• Valence Bond Theory - Directional Properties of Bonds 
• Valence Bond Theory - Overlapping of Atomic Orbitals 
• Valence Bond Theory - Types of Overlapping and Nature of Covalent Bonds 
• Valence Bond Theory - Strength of Sigma and Pi Bonds 
• Hybridisation 
  • Hybridisation - Introduction 
    • Salient features of hybridisation, Important conditions for hybridisation
    • Types of hybridisation and geometry of molecules
    • Bonding in Ethylene
    • Formation of sigma bond
    • Formation of Pi (π ) bond
    • Bonding in acetylene
  • Types of Hybridisation 

    sp, sp², sp³

  • Hybridisation of Elements Involving d Orbitals 

    dsp², sp³d, sp³d²,d²sp³

• Molecular Orbital Theory - Introduction 
• Molecular Orbital Theory 
  • Formation of Molecular Orbitals - Linear Combination of Atomic Orbitals (Lcao) 
  • Conditions for the Combination of Atomic Orbitals 
  • Types of Molecular Orbitals 
  • Energy Level Diagram for Molecular Orbitals 
  • Electronic Configuration and Molecular Behaviour 
• Bonding in Some Homonuclear Diatomic Molecules 

  Hydrogen, Helium, Lithium, Carbon, Oxygen

• Hydrogen Bonding - Introduction 
  • Intramolecular Hydrogen Bond
  • Intermolecular hydrogen bond
• Hydrogen Bonding 
  • Cause of Formation of Hydrogen Bond 
  • Types of H-Bonds 

    Intermolecular hydrogen bond, Intramolecular hydrogen bond

• Chemical Bonding and Molecular Structure Numericals 
• States of Matter:- Gases and Liquids Numericals 

Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, valence bond theory, resonance, geometry of 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.

• Intermolecular Forces - Introduction 

  van der Waals forces

• Intermolecular Forces 
  • Dispersion Forces Or London Forces 
  • Dipole - Dipole Forces 
  • Dipole-induced Dipole Forces 
  • Hydrogen Bond 
• Thermal Energy 
• Intermolecular Forces Vs. Thermal Interactions 
• The Gaseous State 
• The Gas Laws 
  • Boyle’S Law (Pressure - Volume Relationship) 
  • Charles’ Law (Temperature - Volume Relationship) 
  • Gay Lussac’S Law (Pressure- Temperature Relationship) 
• Laws of Chemical Combination 
  • Avogadro Law 
• Ideal Gas Equation 
  • Derivation of Ideal Gas Equation 
  • Density and Molar Mass of a Gaseous Substance 
  • Dalton’S Law of Partial Pressures 
• Kinetic Molecular Theory of Gases 

  kinetic energy and molecular speeds (elementary idea)

• Behaviour of Real Gases:- Deviation from Ideal Gas Behaviour 
  • van der Waal's equation
  • Compressibility factor Z
  • Compressibility factor for real gases
  • Pressure-Volume isotherms of Carbon dioxide
• Liquifaction of Gases 

  critical temperature

• Liquid State 
  • Vapour Pressure 
  • Surface Tension 
  • Viscosity 
• States of Matter:- Gases and Liquids Numericals 

Three states of matter, intermolecular interactions, types of bonding, melting and boiling points, role of gas laws of elucidating the concept of the molecule, Boyle’s law, Charle’s law, Gay Lussac’s law, Avogadro’s law, ideal behaviour of gases, empirical derivation of gas equation. Avogadro number, ideal gas equation. Kinetic energy and molecular speeds (elementary idea), deviation from ideal behaviour, liquefaction of gases, critical temperature. Liquid State- Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations).

• Thermodynamic Terms 
  • The System and the Surroundings
  • Types of the system :- Open System, Closed system, Isolated System
• The State of the System 
• The Internal Energy as a State Function - Work 
• The Internal Energy as a State Function - Heat 
• The Internal Energy as a State Function - The General Case 

  First law of Thermodynamics

• Thermodynamics Applications 
  • Work 

    pressure-volume work, reversible processes, irreversible processes. Isothermal and free expansion of an ideal gas

  • Enthalpy, H - A Useful New State Function 
  • Enthalpy, H - Extensive and Intensive Properties 
  • Enthalpy, H - Heat Capacity 
  • Enthalpy, H - The Relationship Between Cp and Cv for an Ideal Gas 
• Measurement of ∆U and ∆H Calorimetry - ∆U Measurements 
• Measurement of ∆U and ∆H Calorimetry - ∆H Measurements 
• Enthalpy Change, ∆_rH of a Reaction - Reaction Enthalpy 
  • Standard Enthalpy of Reactions 
  • Enthalpy Changes During Phase Transformations 
  • Standard Enthalpy of Formation 
  • Thermochemical Equations 
    • Heat of combustion
    • Molar heat capacities
    • Relation between Cp and Cv for an ideal gas
• Chemical Thermodynamics and Energetic 
  • Hess’ Law of Constant Heat Summation 
• Enthalpies for Different Types of Reactions 
  • Standard Enthalpy of Combustion 
  • Enthalpy of Atomization 

    enthalpy of bond sublimation

  • Bond Enthalpy 

    Bond dissociation enthalpy, Mean bond enthalpy with reference to diatomic and polyatomic molecules

  • Enthalpy of Solution 
  • Lattice Enthalpy 

    enthalpy of ionization

• Spontaneity 
  • Is Decrease in Enthalpy a Criterion for Spontaneity 
  • Entropy and Spontaneity 
  • Gibbs Energy and Spontaneity 
• Gibbs Energy Change and Equilibrium 

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, combustion, formation, atomization, sublimation, phase transition, ionization, solution and dilution. Introduction of entropy as state function, Second law of thermodynamics, Gibbs energy change for spontaneous and non-spontaneous process, criteria for equilibrium and spontaneity. Third law of thermodynamics- Brief introduction.

• Concept of Equilibrium 
• Equilibrium in Physical Processes 
  • Solid-liquid Equilibrium 
  • Liquid-vapour Equilibrium 
  • Solid - Vapour Equilibrium 
  • Equilibrium Involving Dissolution of Solid in Liquids 
  • Equilibrium Involving Dissolution of Gases in Liquids 
  • General Characteristics of Equilibria Involving Physical Processes 
• Equilibrium in Chemical Processes - Dynamic Equilibrium 
• Law of Chemical Equilibrium and Equilibrium Constant 
• Homogeneous Equlibria 
  • Equilibrium Constant in Gaseous Systems 
• Heterogeneous Equlibria 
  • Equilibrium constant for heterogeneous equilibria
• Applications of Equilibrium Constants 
  • Predicting the Extent of a Reaction 
  • Predicting the Direction of the Reaction 
  • Calculating Equilibrium Concentrations 
• Relationship Between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G 
• Le Chatelier’S Principle and Its Applications to Chemical Equilibria 
  • Change of concentration 

    Chemical Equilibria

    Factors Affecting Equilibria - Effect of Concentration Change

  • Change of Pressure 

    Chemical Equilibria

    Factors Affecting Equilibria - Effect of Pressure Change

  • Addition of Inert Gas 

    Chemical Equilibria

    Factors Affecting Equilibria - Effect of Inert Gas Addition

  • Change of Temperature 

    Chemical Equilibria

    Factors Affecting Equilibria - Effect of Temperature Change

  • Effect of Catalyst 

    Chemical Equilibria

    Factors Affecting Equilibria - Effect of a Catalyst

• Ionic Equilibrium in Solution 
• Concept of Acids, Bases and Salts 

  Introduction

• Acids, Bases and Salts 
  • Arrhenius, BroNsted-lowry and Lewis Concept of Acids and Bases 

    Arrhenius Concept of Acids and Bases

    The Brönsted-Lowry Acids and Bases

    Lewis Acids and Bases

• Concept of Ionization of Acids and Bases 
• Ionization of Acids and Bases 
  • The Ionization Constant of Water and Its Ionic Product 
  • The pH Scale 
    • Relationship between pH and pOH
    • Acidity, basicity and neutrality of aqueous solutions
  • Ionization Constants of Weak Acids 

    Degree of ionization

  • Ionization of Weak Bases 
  • Relation Between Ka and Kb 
  • Di- and Polybasic Acids and Di- and Polyacidic Bases 
  • Factors Affecting Acid Strength 
  • Common Ion Effect in the Ionization of Acids and Bases 
  • Hydrolysis of Salts and the Ph of Their Solutions 
• Ionic Equilibria 
  • Buffer Solutions 
    • Types of buffer solutions
    • Buffer action
    • Properties of buffer solution
    • Applications of buffer solution
    • Buffer capacity and buffer index
    • Henderson – Hasselbalch equation 
• Concept of Solubility Equilibria of Sparingly Soluble Salts 

  Solubility Product Constant

  Common Ion Effect on Solubility of Ionic Salts

Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of chemical equilibrium, 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 solutions, Henderson equation, solubility product, common ion effect (with illustrative examples).

• Classical Idea of Redox Reactions - Oxidation and Reduction Reactions 
• Redox Reactions in Terms of Electron Transfer Reactions - Introduction 
• Redox Reactions in Terms of Electron Transfer Reactions - Competitive Electron Transfer Reactions 
• Oxidation Number - Introduction 
• Oxidation Number 
  • Types of Redox Reactions 
    • Combination reactions
    • Decomposition reactions
    • Displacement reactions
    • Disproportionation reactions
  • Redox Reactions as the Basis for Titrations 
  • Limitations of Concept of Oxidation Number 
• Balancing of Redox Reactions 
  • Oxidation Number Method
  • Ion electron method (Half reaction method)
• Redox Reactions and Electrode Processes 

  Standard Electrode Potential

Concept of oxidation and oxidation and reduction, redox reactions oxidation number, balancing redox reactions in terms of loss and gain of electron and change in oxidation numbers. applications of redox reactions.

• Position of Hydrogen in the Periodic Table 
• Dihydrogen 
  • Occurrence
  • Isotopes of Hydrogen
• Preparation of Dihydrogen 
  • Laboratory Preparation of Dihydrogen
  • Commercial Production of Dihydrogen
• Properties of Dihydrogen 
  • Physical Properties
  • Chemical Properties
  • Uses of Dihydrogen
• Hydrides 
  • Ionic Or Saline Hydrides 
  • Covalent Or Molecular Hydride 
  • Metallic Or Non-stoichiometric (Or Interstitial) Hydrides 
• Water 
  • Physical Properties of Water 
  • Structure of Water 
  • Structure of Ice 
  • Chemical Properties of Water 

    Amphoteric Nature, Redox Reactions Involving Water, Hydrolysis Reaction, Hydrates Formation

  • Hard and Soft Water 
  • Temporary Hardness of Water 

    Boiling, Clark's method

  • Permanent Hardness of Water 

    Treatment with washing soda (sodium carbonate), Calgon’s method, Ion-exchange method, Synthetic resins method

• Preparation of Hydrogen Peroxide 
  • Laboratory Preparation
  • Industrial Production 
  • Preparation of Deuterium

  • Electrolysis of heavy water

  • Preparation of Tritium
• Physical Properties of Hydrogen Peroxide 
• Structure of Hydrogen Peroxide 
• Chemical Properties of Hydrogen Peroxide 
• Storage of Hydrogen Peroxide 
• Uses of Hydrogen Peroxide 
• Heavy Water 
  • D₂O
  • Chemical properties of heavy water
  • Uses of heavy water
• Dihydrogen as a Fuel 

Position of Hydrogen in periodic table, Occurrence, isotopes, preparation, properties and uses of hydrogen; hydrides-ionic, covalent and interstitial; physical and chemical properties of water, heavy water; hydrogen peroxide-preparation, reactions, uses and structure; Hydrogen as fuel.

• Group 1 Elements - Alkali Metals 

  Electronic Configuration

  Atomic and Ionic Radii

  Ionization Enthalpy

  Hydration Enthalpy

  Physical Properties

  Chemical Properties - Reactivity towards air, water, dihydrogen, halogens. Reducing nature. Solutions in liquid ammonia.

  Uses

• General Characteristics of the Compounds of the Alkali Metals 

  Oxides and Hydroxides, Halides and Salts of Oxo-Acids

• Anomalous Properties of Lithium 
  • Points of Difference between Lithium and other Alkali Metals
  • Points of Similarities between Lithium and Magnesium
• Some Important Compounds of Sodium 

  Sodium Carbonate (Washing Soda), Na₂CO₃ 10H₂O

  Sodium Chloride, NaCl

  Sodium Hydroxide (Caustic Soda), NaOH

  Sodium Hydrogencarbonate (Baking Soda), NaHCO₃

• Biological Importance of Sodium and Potassium 
• Group 2 Elements - Alkaline Earth Metals 
  • General characteristics of alkaline earth metals
  • Electronic Configuration
  • Atomic and Ionic Radii
  • Ionization Enthalpies
  • Hydration Enthalpies
  • Physical Properties
  • Chemical Properties - Reactivity towards air, water, halogens, hydrogen. Reducing nature.
  • Distinctive behavior of beryllium 
  • Solutions in liquid ammonia.
  • Uses
• General Characteristics of the Compounds of the Alkaline Earth Metals 

  Oxides and Hydroxides, Halides and Salts of OxoAcids - Carbonates, Sulphanates, Nitrates

• Anomalous Behaviour of Beryllium 

  Diagonal Relationship between Beryllium and Aluminium

• Some Important Compounds of Calcium 

  Calcium Oxide or Quick Lime, CaO

  Calcium Hydroxide (Slaked lime), Ca(OH)₂

  Calcium Carbonate, CaCO₃

  Calcium Sulphate (Plaster of Paris), CaSO₄½ H₂O

• Biological Importance of Magnesium and Calcium 

Group I and group 2 elements: General introduction, electronic configuration, occurrence, anomalous properties of the first element of each group, diagonal relationship, trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii), trends in chemical reactivity with oxygen, water, hydrogen and halogens; uses. Preparation and Properties of Some important Compounds: Sodium carbonate, sodium chloride, sodium hydroxide and sodium hydrogencarbonate, biological importance of sodium and potassium. Industrial use of lime and limestone, biological importance of Mg and Ca.

• P-block Elements - Introduction 
• Group 13 Elements - The Boron Family 
  • Electronic Configuration
  • Atomic Radii
  • Ionization Enthalpy
  • Electronegativity
  • Physical Properties
  • Chemical Properties - Oxidation state and trends in chemical reactivity ((i) Reactivity towards air, (ii) Reactivity towards acids and alkalies, (iii) Reactivity towards halogens)
• Important Trends and Anomalous Properties of Boron 
• Some Important Compounds of Boron 
  • Borax
  • Orthoboric acid
  • Diborane, B₂H₆
• Uses of Boron and Aluminium and Their Compounds 
• Group 14 Elements - The Carbon Family 
  • Electronic Configuration
  • Covalent Radius
  • Ionization Enthalpy
  • Electronegativity
  • Physical Properties
  • Chemical Properties - Oxidation states and trends in chemical reactivity ((i) Reactivity towards oxygen, (ii) Reactivity towards water, (iii) Reactivity towards halogen)
• Important Trends and Anomalous Behaviour of Carbon 
• Allotropes of Carbon - Diamond 
• Allotropes of Carbon - Graphite 
• Allotropes of Carbon - Fullerenes 
• Allotropes of Carbon - Uses of Carbon 
• Some Important Compounds of Carbon and Silicon - Carbon Monoxide 
• Some Important Compounds of Carbon and Silicon - Carbon Dioxide 
• Some Important Compounds of Carbon and Silicon - Silicon Dioxide 
• Some Important Compounds of Carbon and Silicon - Silicones 
• Some Important Compounds of Carbon and Silicon - Silicates 
• Some Important Compounds of Carbon and Silicon - Zeolites 

General Introduction to p-Block Elements. Group 13 elements: General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous properties of first element of the group; Boron, some important compounds: borax, boric acids, boron hydrides. Aluminium: uses, reactions with acids and alkalies. General 14 elements: General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous behaviour of first element. Carbon, allotropic forms, physical and chemical properties: uses of some important compounds: oxides. Important compounds of silicon and a few uses: silicon tetrachloride, silicones, silicates and zeolites, their uses.

• Tetravalence of Carbon - Shapes of Organic Compounds 
  • The Shapes of Carbon Compounds
  • Some Characteristic Features of π Bonds
• Structural Representations of Organic Compounds 
  • Complete, Condensed and Bond-line Structural Formulas 
  • Three-dimensional Representation of Organic Molecules 
• Classification of Organic Compounds 
  • Classification based on the carbon skeleton - Acyclic or open-chain compounds, Cyclic compounds, Alicyclic compounds, Aromatic compounds.
  • Classification based on the functional group - Homologous series
• Nomenclature of Organic Compounds 
  • The IUPAC System of Nomenclature 
  • IUPAC Nomenclature of Alkanes 

    Straight chain hydrocarbons, Branched chain hydrocarbons, Nomenclature of branched chain alkanes, Cyclic Compounds

  • Nomenclature of Organic Compounds Having Functional Group(s) 
  • Nomenclature of Substituted Benzene Compounds 
• Isomerism 
  • Structural isomerism
    a) Chain isomerism 
    b) Position isomerism
    c) Functional group isomerism
    d) Metamerism
    e) Tautomerism
• Fundamental Concepts in Organic Reaction Mechanism 
  • Fission of a Covalent Bond 

    heterolytic cleavage, homolytic cleavage

  • Nucleophiles and Electrophiles 
  • Electron Movement in Organic Reactions 
  • Electron Displacement Effects in Covalent Bonds 
  • Inductive Effect 
  • Resonance Structure 
  • Resonance Effect 
    • Positive Resonance Effect (+R effect)
    • Negative Resonance Effect (- R effect)
  • Electromeric Effect (E Effect) 
  • Hyperconjugation 
  • Types of Organic Reactions and Mechanisms 

    Substitution reactions, Addition reactions, Elimination reactions, Rearrangement reactions

• Methods of Purification of Organic Compounds - Introduction 
  • types (name only), purity, sharp melting point, boiling point
  • Sublimation
  • Crystallization
  • Distillation
  • Steam distillation
  • Azeotropic Distillation
  • Differential extraction
  • Chromatography
• Methods of Purification of Organic Compounds - Sublimation 
• Purification of Solids 
  • Crystallization 
  • Distillation 
    • Simple distillation
    • Fractional Distillation
    • Distillation under Reduced Pressure
• Methods of Purification of Organic Compounds - Differential Extraction 
• Methods of Purification of Organic Compounds - Chromatography 

  Adsorption chromatography, Column chromatography, Thin Layer Chromatography and Partition Chromatography

• Qualitative Analysis of Organic Compounds - Detection of Carbon and Hydrogen 

  Test for Nitrogen, Test for Sulphur, Test for Halogens and Test for Phosphorus

• Qualitative Analysis of Organic Compounds - Detection of Other Elements 

  Test for Nitrogen, Test for Sulphur, Test for Halogens and Test for Phosphorus

• Quantitative Analysis of Carbon and Hydrogen 
• Quantitative Analysis of Nitrogen 

  Dumas method, Kjeldahl’s method

• Quantitative Analysis of Halogens 

  Carius method

• Quantitative Analysis of Sulphur 
• Quantitative Analysis of Phosphorus 
• Quantitative Analysis of Oxygen 

General introduction, methods of purification qualitative and quantitative analysis, classification and IUPAC nomenclature of organic compounds. Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radials, carbocations, carbanions; electrophiles and nucleophiles, types of organic reactions.

• Classification of Hydrocarbons 

  Saturated, Unsaturated and aromatic

• Alkanes - Introduction 
• Alkanes 
  • Nomenclature and Isomerism 
  • Preparation of Alkanes from Unsaturated Hydrocarbons, Alkyl Halides and Carboxylic Acids 
  • Conformations (Ethane) 

    Sawhorse projections, Newman projections

• Physical Properties of Alkanes 
• Chemical Properties of Alkanes 
  • Substitution reactions - Halogenation, Mechanism
  • Combustion
  • Controlled oxidation
  • Isomerisation
  • Aromatization
  • Reaction with steam
  • Pyrolysis
• Alkenes - Introduction 
• Alkenes 
  • Structure of Double Bond 
  • Nomenclature 
  • Preparation of Alkenes from Alkynes, Alkyl Halides, Vicinal Dihalides and Alcohols by Acidic Dehydration 
• Isomerism 
  • Structural isomerism
    a) Chain isomerism 
    b) Position isomerism
    c) Functional group isomerism
    d) Metamerism
    e) Tautomerism
• Physical Properties of Alkenes 
• Chemical Properties of Alkenes 

  Addition of dihydrogen, Addition of halogens, Addition of hydrogen halides, Addition reaction of HBr to symmetrical alkenes, Addition reaction of HBr to unsymmetrical alkenes (Markovnikov Rule), Anti Markovnikov addition or peroxide effect or Kharash effect, Addition of sulphuric acid, Addition of water, Oxidation, Ozonolysis and Polymerisation

• Alkynes - Introduction 
• Alkynes 
  • Nomenclature and Isomerism 
  • Structure of Triple Bond 
  • Preparation of Alkynes from Calcium Carbide and Vicinal Dihalides 
• Physical Properties of Alkynes 
• Chemical Properties of Alkynes 
  • Acidic character of alkyne
  • Addition reactions - Addition of dihydrogen, Addition of halogens, Addition of hydrogen halides, Addition of water and Polymerisation
• Aromatic Hydrocarbons - Introduction 
• Aromatic Hydrocarbons 
  • Nomenclature and Isomerism 
  • Structure of Benzene 

    Resonance and stability of benzene

  • Aromaticity 
  • Preparation of Benzene 

    Cyclic polymerisation of ethyne, Decarboxylation of aromatic acids, Reduction of phenol

  • Electrophilic Substitution Reactions 

    Nitration, Halogenation, Sulphonation, Friedel-Crafts alkylation reaction and Friedel-Crafts acylation reaction

  • Mechanism of Electrophilic Substitution Reactions 
    • Generation of the eletrophile
    • Formation of carbocation intermediate
    • Removal of proton from the carbocation intermediate
    • Addition reactions - Combustion
  • Directive Influence of a Functional Group in Monosubstituted Benzene 

    Ortho and para directing groups, Meta directing group

• Physical Properties of Aromatic Hydrocarbons 
• Chemical Properties of Aromatic Hydrocarbons 
• Carcinogenicity and Toxicity 

Alkanes- Nomenclature, isomerism, conformations (ethane only), physical properties, chemical reactions including free radical mechanism of halogenation, combustion and pyrolysis.

Alkanes-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 Craft’s alkylation and acylation; directive influence of functional group in mono-substituted benzene; carcinogenicity and toxicity.

• Environmental Pollution - Introduction 
  • Bio-degradable pollutants
  • Non bio-degradable pollutants 
• Atmospheric Pollution 
  • Tropospheric Pollution - Gaseous Air Pollutants 

    Oxides of Sulphur

    Oxides of Nitrogen

    Hydrocarbons

    Oxides of Carbon - Carbon monoxide, Carbon dioxide (Global Warming and Greenhouse Effect, Acid rain)

  • Tropospheric Pollution - Particulate Pollutants 

    Smoke, dust, mists, classical smog, photochemical smog, Formation of photochemical smog, Effects of photochemical smog, photochemical smog control

  • Stratospheric Pollution 
    • Formation and Breakdown of Ozone, The Ozone Hole and Effects of Depletion of the Ozone Layer
• Water Pollution 
  • Causes of Water Pollution 
    • Microbiological (Pathogens) 
    • Organic wastes
    • Chemical wastes
  • International Standards for Drinking Water 

    Fluoride, Lead, Sulphate, Nitrate, Other metals

• Soil Pollution - Pesticides, Herbicides 
  • Sources of soil pollution 

  1. Artificial fertilizers
  2. Pesticides
• Industrial Waste 
• Strategies to Control Environmental Pollution 

  Waste Management - Collection and Disposal

• Green Chemistry - Introduction 
  • Green chemistry in day-to-day life 
• Green Chemistry in Day-to-day Life 

  Dry Cleaning of Clothes, Bleaching of Paper, Synthesis of Chemicals

Environmental pollution: Air, water and soil pollution, chemical reactions in atmosphere, smogs, major atmospheric pollutants; acid rain ozone and its reactions, effects of depletion of ozone layer, greenhouse effect and global warming- pollution due to industrial wastes; green chemistry as an alternative tool for reducing pollution, strategy for control of environmental pollution.