Units and Topics
# | Unit/Topic | Marks |
---|---|---|
100 | Some Basic Concepts of Chemistry | - |
200 | Structure of Atom | - |
300 | Classification of Elements and Periodicity in Properties | - |
400 | Chemical Bonding and Molecular Structure | - |
500 | States of Matter:- Gases and Liquids | - |
600 | Chemical Thermodynamics | - |
700 | Equilibrium | - |
800 | Redox Reactions | - |
900 | Hydrogen | - |
1000 | S-block Elements (Alkali and Alkaline Earth Metals) | - |
1100 | Some P-block Elements | - |
1200 | Organic Chemistry - Some Basic Principles and Techniques | - |
1300 | Hydrocarbons | - |
1400 | Environmental Chemistry | - |
Total | - |
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
- The International System of Units (Si)
- 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
- Scientific Notation
- Laws of Chemical Combination
- Dalton'S Atomic Theory
- Atomic and Molecular Masses
- 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 Protons and Neutrons
Millikan’s Oil Drop Method
- Discovery of Protons and Neutrons
- Concept of Atomic Models
- The Structure of an Atom
- Concept of Atomic Number
- Concept of Mass Number
- Concept of Isobars
- Concept of 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
- Dual Behaviour of Matter
- 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
- Physical Properties
- Periodic Trends in Chemical Properties of 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
- Ionic bond
- 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
- Resonance Structures
resonance, geometry of covalent molecules
- Polarity of Bonds
covalent character of ionic bond
- Resonance Structures
- The Valence Shell Electron Pair Repulsion (Vsepr) Theory
- Rules of VSEPR
1. Ammonia NH3
2. Water molecule H2O - Advanced theories of Bonding
- Rules of VSEPR
- 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
- Valence Bond Theory - Orbital Overlap Concept
- 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
sp, sp2, sp3
- Hybridisation of Elements Involving d Orbitals
dsp2, sp3d, sp3d2,d2sp3
- Hybridisation - Introduction
- Molecular Orbital Theory - Introduction
- Molecular Orbital Theory
- Bonding in Some Homonuclear Diatomic Molecules
Hydrogen, Helium, Lithium, Carbon, Oxygen
- Hydrogen Bonding - Introduction
- Hydrogen Bonding
- Types of H-Bonds
Intermolecular hydrogen bond, Intramolecular hydrogen bond
- Types of H-Bonds
- 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
- Thermal Energy
- Intermolecular Forces Vs. Thermal Interactions
- The Gaseous State
- The Gas Laws
- Laws of Chemical Combination
- Ideal Gas Equation
- 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
- Liquifaction of Gases
critical temperature
- Liquid State
- 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
- Work
- Measurement of ∆U and ∆H Calorimetry - ∆U Measurements
- Measurement of ∆U and ∆H Calorimetry - ∆H Measurements
- Enthalpy Change, ∆_rH of a Reaction - Reaction Enthalpy
- Chemical Thermodynamics and Energetic
- Enthalpies for Different Types of Reactions
- Enthalpy of Atomization
enthalpy of bond sublimation
- Bond Enthalpy
Bond dissociation enthalpy, Mean bond enthalpy with reference to diatomic and polyatomic molecules
- Lattice Enthalpy
enthalpy of ionization
- Enthalpy of Atomization
- 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
- Equilibrium in Chemical Processes - Dynamic Equilibrium
- Law of Chemical Equilibrium and Equilibrium Constant
- Homogeneous Equlibria
- Heterogeneous Equlibria
- Equilibrium constant for heterogeneous equilibria
- Applications of Equilibrium Constants
- 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
- Change of concentration
- 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
- Arrhenius, BroNsted-lowry and Lewis Concept of Acids and Bases
- Concept of Ionization of Acids and Bases
- Ionization of Acids and Bases
- The pH Scale
- Relationship between pH and pOH
- Acidity, basicity and neutrality of aqueous solutions
- Ionization Constants of Weak Acids
Degree of ionization
- The pH Scale
- Ionic Equilibria
- Buffer Solutions
- Types of buffer solutions
- Buffer action
- Properties of buffer solution
- Applications of buffer solution
- Buffer Solutions
- 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
- Types of Redox Reactions
- 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
- Water
- Chemical Properties of Water
Amphoteric Nature, Redox Reactions Involving Water, Hydrolysis Reaction, Hydrates Formation
- 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
- Chemical Properties of Water
- Preparation of Hydrogen Peroxide
- 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
- 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
- Electronic Configuration
- Atomic and Ionic Radii
- Ionization Enthalpies
- Hydration Enthalpies
- Physical Properties
- Chemical Properties - Reactivity towards air, water, halogens, hydrogen. Reducing nature.
- 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
- 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
- IUPAC Nomenclature of Alkanes
Straight chain hydrocarbons, Branched chain hydrocarbons, Nomenclature of branched chain alkanes, Cyclic Compounds
- IUPAC Nomenclature of Alkanes
- Isomerism
- Structural isomerism
a) Chain isomerism
b) Position isomerism
c) Functional group isomerism
d) Metamerism
e) Tautomerism
- Structural isomerism
- Fundamental Concepts in Organic Reaction Mechanism
- Fission of a Covalent Bond
heterolytic cleavage, homolytic cleavage
- Resonance Effect
- Positive Resonance Effect (+R effect)
- Negative Resonance Effect (- R effect)
- Types of Organic Reactions and Mechanisms
Substitution reactions, Addition reactions, Elimination reactions, Rearrangement reactions
- Fission of a Covalent Bond
- Methods of Purification of Organic Compounds - Introduction
types (name only), purity, sharp melting point, boiling point
- Methods of Purification of Organic Compounds - Sublimation
- Purification of Solids
- Distillation
- Simple distillation
- Fractional Distillation
- Distillation under Reduced Pressure
- Distillation
- 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
- Conformations (Ethane)
Sawhorse projections, Newman projections
- Conformations (Ethane)
- Physical Properties of Alkanes
- Chemical Properties of Alkanes
- Substitution reactions - Halogenation, Mechanism
- Combustion
- Controlled oxidation
- Isomerisation
- Aromatization
- Reaction with steam
- Pyrolysis
- Alkenes - Introduction
- Alkenes
- Isomerism
- Structural isomerism
a) Chain isomerism
b) Position isomerism
c) Functional group isomerism
d) Metamerism
e) Tautomerism
- Structural isomerism
- 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
- 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
- Structure of Benzene
Resonance and stability of benzene
- 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
- Structure of Benzene
- 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
- 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
- Tropospheric Pollution - Gaseous Air Pollutants
- Water Pollution
- Causes of Water Pollution
Pathogens, Organic wastes
- International Standards for Drinking Water
Fluoride, Lead, Sulphate, Nitrate, Other metals
- Causes of Water Pollution
- Soil Pollution - Pesticides, Herbicides
- Industrial Waste
- Strategies to Control Environmental Pollution
Waste Management - Collection and Disposal
- Green Chemistry - Introduction
- 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.