JEE Main Chemistry (JEE Main) Syllabus: Check the Latest Syllabus

• Introduction of Atom
• Discovery of Charged Particles and the Structure of an Atom

• Molecule
• Properties of molecule

• Experiment 
• Elements

• Introduction
• Experiment 1
• Experiment 2

• Properties and Measurement of Matter
• SI Units and Base Quantities

• Definition: Mass
• Definition: Weight

• Introduction
• Experiment

• Definition: Atom
• Definition: Molecule
• Definition: Avogadro's Law

• Atomic Mass
• Average Atomic Mass
• Molecular Mass
• Formula Mass

• Introduction of Atomic Mass
• Properties of Mass Number
• Determination of Relative Atomic Mass

• Definition: Mole
• Definition: Avogadro's Number

• Definition: Percentage Composition
• Formula: Percentage Composition

• Chemical reactions: Reactants, Products, Chemical equation
• Stoichiometry
• Steps for writing balanced chemical equation
• Mass relationship
• Calculations based on stoichiometry
  1) Mole to mole relationships
  2) Mass-mass relationships
  3) Mass-volume relationship
  4) Volume-volume relationship
• Limiting reactant
• Excess reactant

• Reactions in solutions

1. Mass percentage
2. Mole fraction
3. Molarity
4. Molality
5. Volume percentage

• Definition: Accuracy
• Definition: Precision
• Definition: Uncertainty
• Activity: Measuring with Uncertainty
• Real-Life Examples

1. Pure Substances: Elements and Compounds
2. Mixture: Homogeneous and Heterogeneous mixture

• Three States of Matter
• Comparison of Solids, Liquids, and Gases

• Van der Waals forces

• Types of Intermolecular Forces

1. Dipole-dipole interactions
2. Ion-dipole interactions
3. Dipole-Induced dipole interaction
4. London Dispersion Force
5. Hydrogen Bonding

• Intermolecular Forces and Thermal energy

• Definition: Gas Equation
• Definition: Absolute Scale or Klevin Scale
• Law: Boyle's Law
• Law: Charle's Law

• Definition: Atom
• Definition: Molecule
• Definition: Avogadro's Law

• Kinetic molecular theory of gases
• Postulates of kinetic molecular theory
• Kinetic gas equation
• Calculation of kinetic energy (K.E.)
• Molecular speeds
• Types of speed
  a) Most probable speed (u_mp)
  b) Average speed (u_av)
  c) Root mean square speed (u_r.m.s.)
• Relation between molecular speeds, temperature, and molecular mass

• Real gases
• Reasons for deviations
• van der Waals equation for real gases
• Effect of pressure
• Compressibility factor (Z)
• Effect of temperature
• Compressibility factor for real gases
• Pressure-Volume isotherms of Carbon dioxide
• Difference between Ideal gas and real gas

• Liquefaction of gases
• Critical constants
  i) Critical temperature
  ii) Critical pressure
  iii) Critical volume
• Isotherms of CO₂

• Classification of solids

1. Crystalline solids
2. Amorphous solids

• The distinction between Crystalline and Amorphous Solids
• Isomorphous solids and polymorphous solids

• Unit cell
• Crystal lattice or space lattice
• Two-dimensional lattice and unit cell
• Three-dimensional lattice and unit cell

• Primitive Unit Cells
• Centred Unit Cells
  1) Body-Centred Unit Cells
  2) Face-Centred Unit Cells
  3) End-Centred Unit Cells
• Bravais lattices

• Primitive Cubic Unit Cell
• Body-Centred Cubic Unit Cell
• Face-Centred Cubic Unit Cell

• Packing in solids
• Close Packing in One Dimension
  1) Coordination number
• Close Packing in Two Dimensions
  1) Square close packing in two dimensions
  2) Hexagonal close packing of spheres in two dimensions
• Close Packing in Three Dimensions
• Three-dimensional close-packed structure

• Stage I - Linear packing in one dimension
• Stage II - Planar packing in two dimensions
  1) AAAA type, square close-packed structure
  2) ABAB type, hexagonal close-packed structure
• Stage III - Close packing in three dimensions
  1) AAAA type, simple cubic structure
  2) ABAB type, hexagonal close-packed structure
  3) ABCABC type, cubic close-packed structure

• Number of voids per atom in hcp and ccp structures
• Locating tetrahedral and octahedral voids: locating tetrahedral voids, Locating octahedral voids

• Calculation of density of unit cell

point defects and line defects

• Discovery of electron
• Discovery of proton
• Discovery of neutron

• Introduction
• Examples

• Discovery of Electrons
• Thomson’s Plum Pudding Model of the Atom
• Merits and Demerits

• Introduction
• Rutherford’s Nuclear atomic model
• Merits and Demerits

• Wave Theory
• Salient features of the wave theory of light
• Drawbacks of wave theory
• Wave motion
• Characteristics of wave motion
  1) Wavelength (λ)
  2) Frequency (v)
  3) Velocity (c)
  4) Wave number
  5) Amplitude (A)
• Electromagnetic spectrum

• Emission and Absorption Spectra
• Line Spectrum of Hydrogen

• Explanation of the line spectrum of hydrogen using Bohr theory
• Bohr's theory and atomic spectrum of hydrogen
• Ionization energy

• Schrodinger wave equation
• Physical significance of Ψ and Ψ²
• Radial probability distribution curves
• Difference between orbit and orbital
• Atomic orbitals and quantum numbers
• Shapes of atomic orbitals
• Energies of orbitals
• Aufbau principle
• Electronic configuration of atoms and its representation 
• Electronic configurations of Cu and Cr

1. Chromium
2. Copper
3. Isoelectronic species

• Quantum number
• Principal quantum number (n)
• Azimuthal quantum number (l)
• Magnetic quantum number (m or m_l)
• Spin quantum number (s or m_s)
• Values of quantum number l and m for n = 1 to 4 principal shell

• Shells
• Distribution of electrons in various shells
• Number and designation of subshells
• Accommodation of electrons in a given subshell

• s-Orbital
• p-Orbitals
• d-Orbitals
• f-Orbitals
• Spherical (radial) nodes
• Nodal plane

• Energies of orbitals
• Effective nuclear charge (Z_eff)

• Aufbau principle
• Pauli's exclusion principle
• Hund's rule of maximum multiplicity

• Electronic configuration
• General representation of electronic configuration of an atom
• Valence shell electronic configuration
• Pictorial representation of electronic configuration of an atom
• Electronic configurations of the elements with atomic numbers 1 to 30

• Stability of completely filled and half-filled subshells

1. Symmetrical distribution of electrons
2. Exchange Energy

• Definition: Chemical Bond

• Kossel and Lewis theory
• Lewis symbols
• Significance of Lewis symbols
• Lewis symbols and valence of elements

• Covalent bond
  a) Formation of chlorine molecule
  b) Formation of water molecule
• Types of covalent bonds: Single, Double and Triple bond
• Conditions for formation of covalent bond
  i) Number of valence electrons
  ii) Electronegativity difference
  iii) Small decrease in energy

• Formal charge (F.C.)
• Assigning formal charge

• Limitations of the octet rule

1. The incomplete octet of the central atom
2. The expanded octet
3. Odd-electron molecules
4. Shape and geometry of a molecule
5. Other drawbacks of the octet theory

• Definition: Ion
• Definition: Cation
• Definition: Anion
• Definition: Electropositive Element
• Definition: Electronegative Element
• Definition: Electrovalent Bond
• Definition: Electrovalent (or Ionic) Compounds
• Definition: Electrovalency

• Bond Parameters
• Bond length
• Bond order
• Bond angle
• Bond enthalpy
• Resonance

• VSEPR theory
• Main postulates of VSEPR theory
• Geometry of some molecules
• Geometry of some molecules
• Steps to predict the molecular geometry using VSEPR theory

• Postulates of Valence Bond Theory
• Interacting forces during covalent bond formation
  i) Force of repulsion
  ii) Force of attraction
• Formation of hydrogen molecule on the basis of valence bond theory (VBT)
• Overlap of atomic orbitals
• Limitation of VBT

• 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)

• Types of overlap of atomic orbitals

1. Axial overlap: s-s overlap, s-p overlap, p-p overlap 
2. Lateral overlap: p-p overlap

• Difference between sigma (σ) bond and pi (π) bond

• Formation of molecular orbitals
• Conditions for the combination of Atomic Orbitals
• Types of molecular orbitals
• Energy levels and electronic configuration
• Key ideas of MO theory
• MO description of simple diatomic Molecules

• Homonuclear diatomic molecules
• Electronic configuration, bond order, and magnetic nature of some diatomic molecules

1. Hydrogen molecule (H₂)
2. Helium molecule (He₂)
3. Lithium molecule (Li₂)
4. Carbon molecule (C₂)
5. Oxygen molecule (O₂)

• Heteronuclear diatomic molecules
• Bond Energy

• Intramolecular Hydrogen Bond
• Intermolecular hydrogen bond

• Definition: Covalent Compound
• Definition: Covalent Molecule
• Key Points: The Covalent Bond

• The System and the Surroundings
• Types of the system

1. Open System
2. Closed system
3. Isolated System
4. Homogeneous system
5. Heterogeneous system
6. Macroscopic system

• Macroscopic properties of the system

1. Intensive properties
2. Extensive properties

• The state of a system
• State variables or state functions or thermodynamic parameters
• State function: Initial and final states of the system
• Path functions
• Thermodynamic equilibrium and its types

1. Chemical equilibrium
2. Mechanical equilibrium
3. Thermal equilibrium

• Thermodynamic process and its types

1. Isothermal process
2. Adiabatic process
3. Isobaric process
4. Isochoric process
5. Cyclic process
6. Reversible process
7. Irreversible process

• Difference between reversible and irreversible process

• First law of Thermodynamics

• Relation between standard Gibbs energy change and equilibrium constant

• Equilibrium
• Equilibrium state
• Equilibrium mixture
• Dynamic equilibrium
• Chemical equilibrium
• Ionic equilibrium

1. Liquid - Vapour equilibrium 
2. Solid - liquid equilibrium
3. Solid - vapour equilibrium

• Law of mass action
• Law of chemical equilibrium
• Characteristics of the equilibrium constant
• Effect of temperature on equilibrium constant
• Types of equilibrium constant
• Relation between Kp and Kc
• Unit of equilibrium constant

• Equilibrium Constant in Gaseous Systems

• Equilibrium constant for heterogeneous equilibria

• Prediction of the direction of the reaction
• To know the extent of reaction
• To calculate equilibrium concentrations
• Link between chemical equilibrium and chemical kinetics

• Relationship between equilibrium constant, reaction quotient and change in Gibbs energy

• Application of Le-Chatelier's principle

1. Applications to the chemical equilibrium
2. Applications to the physical equilibrium
   a) Melting of ice (Ice-water system)
   b) Melting of sulphur
   c) Boiling of water (water-water vapour system)
   d) Solubility of salts

• Ionic equilibrium
• Water-soluble compounds
• Degree of ionization
• Factors affecting degree of ionization
• Weak and strong electrolytes

• Introduction
• Acid
• Base
• Salt

• Definition: Acid

• Solubility Product Constant

• Comparison of solubility product and ionic product
• Different expressions for solubility product
• Common Ion Effect on Solubility of Ionic Salts
• Applications of solubility product

• Common ion effect

• Solution of weak acid and its salt
• Solution of weak base and its salt
• Common ion effect and solubility of a sparingly soluble salt
• Applications of common ion effect

• Classical ideas of redox reactions
• Redox reaction in terms of electron transfer

• Oxidation
• Reduction
• Oxidation and reduction in terms of electron transfer
• Oxidizing agent
• Reducing agent

• Metal activity series or electrochemical series

• Oxidation number
• Rules to assign oxidation number or oxidation states to an atom
• Paradox of fractional oxidation number
• Stock notations

• Rules to assign oxidation number
• Stock notation
• Redox reaction in terms of oxidation number

• Oxidation number method
• Ion electron method (Half reaction method)

• Direct redox reactions
• Daniel cell
• Standard electrode potential

• Gibbs energy change and e.m.f. of a cell
• Standard cell potential and equilibrium constant

• Introduction
• Experiment

• Definition: Electroplating

• Definition: Corrosion

• Surface chemistry
• Surface or interface

• Unbalanced forces
• Why does adsorption occur?
• Desorption
• Sorption

• Types of adsorption

1. Physical adsorption (Physisorption or van der Waals' adsorption)
2. Chemical adsorption (Chemisorption or activated adsorption)

• Difference between physisorption and chemisorption

• Adsorption isotherm
• Freundlich adsorption isotherm
• Langmuir adsorption isotherm

• Catalyst
• Catalysis and Theories of Catalysis
• Homogeneous Catalysis
• Heterogeneous Catalysis
• Inhibitors

• Important features of solid catalysts

1. Catalytic activity
2. Catalytic selectivity
3. Shape selective catalysis by zeolites

• Examples of colloids
• Classification of colloids
• Preparation of Colloids
• Purification of colloidal solution
• Properties of colloidal dispersions
• Methods to effect coagulation
• Emulsions
• Applications of colloids
• Dispersed phase and dispersion medium
• True solutions, colloids, and suspensions
• Types of colloidal systems

• Chemical methods
• Electrical disintegration or Bredig’s Arc method
• Peptization

• Dialysis
• Electro-dialysis
• Ultrafiltration

• Colligative properties
• Tyndall effect
• Colour
• Brownian movement
• Charge on colloidal particles
• Electrophoresis
• Coagulation of lyophilic sols
• Coagulation or precipitation
• Methods to effect coagulation
• Methods to prevent coagulation of colloids (Protection of colloids)

• Emulsion
• Types of emulsions
  1) Oil-in-water emulsion (O/W type)
  2) Water-in-oil emulsion (W/O type)
• Properties of emulsions
• Deemulsification

• Colloids in our daily life

1. Natural phenomena
   a) Blue colour of sky and sea
   b) Fog, mist, and rain
   c) Soils
   d) Delta formation
   e) Food articles 
   f) Blood
2. Industrial applications
   a) Electrical precipitation of smoke
   b) Purification of drinking water
   c) Colloidal medicines
   d) Photographic plates
   e) Artificial rain
   f) Rubber industry
   g) Tanning
   h) Miscellaneous

• Unitary theory (1815)
• Law of Triads (1817)
• Cooke's Homologous series (1854)
• Law of octaves (1865)
• Contribution of the German chemist, Lothar Meyer (1869)
• Mendeleev's periodic law (1869)

• Modern periodic law (1913)

• Development of modern periodic law
• Modern periodic table (Long form of the periodic table)
  i) Periods
  ii) Groups

• Notation for IUPAC Nomenclature of Elements

• Electronic Configurations in Periods
• Electronic configuration in groups
• Electronic configuration in the four blocks - s-Block, p-Block, d-Block, f-Block

• Introduction
• Definition: Ionic Compounds
• Table: Electronic Configurations
• Key Points: Electronic Configurations

• Valence or Oxidation States
• Periodicity of Valence or Oxidation States
• Anomalous properties of second period elements

• Diagonal Relationship

• Periodic Trends and Chemical Reactivity

• Chemical reactivity
• Nature of oxides

• Definition: Elements
• Definition: Modern Periodic Table
• Key Points: Modern Periodic Table

• Definition: Minerals
• Definition: Ores
• Key Points: Occurrence of Metals

• Definition: Concentration of Ores
• Key Points: Concentration of Ores

• Pulverization
• Concentration of an ore
• Types of separation or concentration of an ore

1. Hydraulic (gravity separation) method or Levigation method
2. Magnetic separation method
3. Froth floatation
4. Chemical method or Leaching
5. Wilfley table method

• Conversion to oxide

1. Calcination
2. Roasting

• Reduction of oxide to the metal

1. Pyrometallurgy
2. Hydrometallurgy
3. Electrometallurgy

• Ellingham diagrams
• Significance of Ellingham diagram
• Limitations of Ellingham diagram
• Selection of reducing agent

• Extraction of iron from its oxides,
• Extraction of copper from cuprous oxide [copper(I) oxide]
• Extraction of zinc from zinc oxide

• Aluminium - Hall-Heroult process
• Copper from Low Grade Ores and Scraps

• Principles and methods of extraction - Refining

1. Distillation
2. Liquation 
3. Electrolytic refining (electrolytic method)
4. Zone refining
5. Vapour phase refining
6. Chromatographic methods

• Hydrogen
• Position of hydrogen in the periodic table

• Occurrence
• Position of hydrogen in the periodic table
• Isotopes of Hydrogen
• Preparation of dihydrogen
• Properties of dihydrogen
• Uses of dihydrogen

• Occurrence of dihydrogen
• Isotopes of Hydrogen
• Physical constants of H₂, D₂, and T₂

• Preparation of Dihydrogen

• By the action of water with metals
• By the action of water on alkali and alkaline earth metal hydrides
• By the reaction of metals like Zn, Sn, and Al with alkalies (NaOH or KOH)
• By the action of metals with acids
• By the electrolysis of acidified water
• Laboratory method
• Preparation of pure hydrogen
• Commercial Production of Dihydrogen
  1) From hydrocarbon or coal
  2) Bosch process
  3) Lane's process
  4) By electrolysis of water

• Physical Properties
• Physical constants of atomic and molecular properties
• Chemical Properties

1. Reaction with metals
2. Reaction with non-metals
3. Reaction with metal ions and metal oxides
4. Reaction with organic compounds

• Uses of Dihydrogen

• Hydrides
• Classification of hydrides

1. Saline or ionic hydrides
2. Molecular or covalent hydrides
   a. Electron-rich molecular hydrides
   b. Electron-precise molecular hydrides
   c. Electron-deficient molecular hydrides
3. Metallic or non-stoichiometric (or interstitial) hydrides

• Physical Properties of Water:

1. Nature
2. Boiling point
3. The freezing point of water or melting point of ice
4. Density
5. Anomalous expansion of water
6. Latent heat of fusion of ice
7. Latent heat of vaporization of water
8. Specific heat capacity

• Chemical properties

1. Dissociation of water
2. Amphoteric nature
3. Oxidising and reducing nature
4. Hydrolytic reactions
5. Formation of hydrates with metal salts

• Soft and Hard water
• Types of Hard water

1. Temporary Hardness
2. Permanent Hardness

• Hydrogen peroxide (H₂O₂)
• Preparation of hydrogen peroxide (H₂O₂)

1. Merck's. process (Laboratory method)
2. By the action of sulphuric acid or phosphoric acid on hydrated barium peroxide BaO₂.8H₂O
3. Industrial method
4. By redox process

• Preparation of Deuterium

• Electrolysis of heavy water

• Preparation of Tritium

• Chemical properties of H₂O₂

1. Decomposition
2. Oxidizing and reducing nature
3. Oxidizing character
4. Reducing character
5. Bleaching action
6. Storage of H₂O₂

• Heavy water (D₂O)
• Preparation
• Properties of heavy water
• Reactions
• Uses of heavy water

• Electronic configuration of group 1 elements
• Occurrence of group 1 elements
• Atomic and ionic radii of group 1 elements
• Ionization Enthalpy
• Electropositive character
• Electronegativity
• Hydration Enthalpy
• Anomalous properties
• Physical properties of group 1 elements

1. Nature and appearance
2. Density
3. Conductivity
4. Melting and boiling points
5. Photoelectric effect
6. Characteristic flame colour
7. Atomic and physical properties of group 1 elements

• Chemical Properties - Reactivity towards air, water, dihydrogen, halogens, Reducing nature, Solutions in liquid ammonia
• Uses of alkali metals: lithium, sodium, potassium

• Oxides and hydroxides
• Halides
• Salts of Oxo-Acids

• Points of Difference between Lithium and other Alkali Metals
• Anomalous behaviour of lithium
• Lithium differs from other alkali metals
• Diagonal relationship of Li with Mg
• Similarities between Li and Mg

• Sodium Carbonate (Washing Soda), Na₂CO₃ 10H₂O
• Sodium Chloride, NaCl
• Sodium Hydroxide (Caustic Soda), NaOH
• Sodium Hydrogencarbonate (Baking Soda), NaHCO₃

• General characteristics of alkaline earth metals
• Electronic configuration of group 2 elements
• Occurrence of group 2 elements
• Atomic and ionic radii of group 2 elements
• Ionization enthalpy of group 2 elements
• Electropositive character
• Electronegativity
• Hydration enthalpy
• Physical properties of group 2 elements

1. Nature and appearance
2. Density
3. Conductivity
4. Melting and boiling points
5. Characteristic flame colour
6. Atomic and physical properties of group 2 elements

• Chemical Properties - Reactivity towards air and water, halogens, hydrogen, Reducing nature, Covalent and ionic character, Solubility.
• Distinctive behavior of beryllium 
• Solutions in liquid ammonia
• Reducing nature
• Reactivity towards acids
• Uses: beryllium, magnesium, calcium, barium, radium

• General characteristics of some compounds of the alkaline earth metals

1. Oxides and Hydroxides
2. Halides - Structure of BeCl₂
3. Salts of Oxoacids

• Carbonates of group 2 elements
• Sulphates of group 2 elements
• Nitrates of group 2 elements

• Anomalous behaviour of beryllium
• Be differs from other alkaline earth metals
• Diagonal Relationship between Beryllium and Aluminium
• Reasons for diagonal relationship
• Similarities between Be and Al

• Calcium oxide or Quick Lime (CaO)
• Uses of lime
• Calcium Hydroxide (Slaked lime), Ca(OH)₂
• Uses of slaked lime
• Calcium Carbonate (CaCO₃) or limestone
• Uses of limestone
• Calcium Sulphate (Plaster of Paris), CaSO₄.½ H₂O
• Uses of plaster of Paris
• Uses of cement

• Role of Mg in biological system
• Role of Ca in biological system

• General introduction of p-block elements
• Electronic configuration of p-block elements
• General characteristics of p-block elements

1. Oxidation states
2. Metallic and nonmetallic character
3. Variation in physical properties
4. Difference in behaviour of first element of each group

• Occurrence,
• Electronic Configuration,
• Atomic and Ionic Radii,
• Ionisation Enthalpy,
• Electropositivity or metallic character,
• Electronegativity,
• Atomic and physical properties of group 13 elements,
• Physical Properties and Chemical Properties,
• Trends in chemical reactivity: Oxidation state.

• Structure, properties, and uses of some important compounds of Boron
  (1) Borax or sodium tetraborate decahydrate (Na₂B₄O ₇.10H₂O) or Na₂[B₄O₅(OH)₄].8H₂O
  (2) Boric acid or orthoboric acid (H₃BO₃)
  (3) Diborane (B₂H₆)
  (4) Boron trifluoride

• Structure, properties, and uses of some important compounds of Aluminum:
  (1) Aluminum chloride
  (2) Alums

• Electronic Configuration
• Occurrence
• Atomic and ionic radii
• Covalent Radius
• Ionization Enthalpy
• Metallic character
• Electronegativity
• Physical Properties and Chemical Properties
• Trends in chemical reactivity: oxidation states

• The tendency for catenation

• Graphite
• Experiment
• Uses of Graphite

• Fullerene
• Uses of Fullerene

• Crystalline Forms
• Diamond
• Uses of Diamond

• Occurrence
• Electronic Configuration
• Atomic and Ionic Radii
• Ionisation Enthalpy
• Electronegativity
• Physical Properties and Chemical Properties

Occurrence, Electronic Configuration, Atomic and Ionic Radii, Ionisation Enthalpy, Electron Gain Enthalpy, Electronegativity, Physical Properties and Chemical Properties (Oxidation states and trends in chemical reactivity and Anomalous behaviour of oxygen)

Occurrence, Electronic Configuration, Atomic and Ionic Radii, Ionisation Enthalpy, Electron Gain Enthalpy, Electronegativity, Physical Properties and Chemical Properties (Oxidation states and trends in chemical reactivity and Anomalous behaviour of fluorine)

• Preparation
• Uses of Grignard reagent 

• Fluoride, Lead, Sulphate, Nitrate, Other metals

• Types of industrial waste

1. Biodegradable wastes
2. Non-biodegradable wastes

• Strategy to control environmental pollution

1. Incineration
2. Digestion
3. Collection and disposal
4. Sewage treatment
5. Other strategies

• Dry Cleaning of Clothes
• Bleaching of Paper
• Synthesis of Chemicals
• ‘Green Solution’ to Clean Turbid Water

• Introduction
• Experiment

• Retention factor (R_f)

• Test for Nitrogen
• Test for Sulphur
• Test for Halogens
• Test for Phosphorus

• Dumas method
• Kjeldahl’s method

• Carius method

• Determination of Empirical Formula from Elemental Analysis Data
• Calculation of Molecular Formula from Empirical Formula

• Tetravalency of carbon
• The Shapes of Carbon Compounds
• Some Characteristic Features of σ and π Bonds

• Definition: Organic Compounds
• Key Points: Organic Compounds

• Classification based on carbon skeleton
• Classification based on functional group
• Homologous Series

• Definition: Nomenclature
• Key Points: Nomenclature of Carbon Compounds

• Definition: Isomers

• Alkanes (Paraffins)
• General formula
• Occurrence
• Structure of alkanes
• Classification
• Uses of alkanes

• Definition: Alkanes

• Physical properties of alkanes

1. Nature
2. Boiling point
3. Melting point
4. Solubility
5. Density

• Chemical properties of alkanes

1. Substitution reactions - Halogenation, Nitration, Sulphonation
2. Combustion of alkanes (oxidation)
3. Controlled oxidation
4. Isomerisation
5. Aromatization
6. Reaction with steam
7. Pyrolysis

• Definition: Alkenes

• Definition: Isomers

• Key Points: Physical Properties of Alkenes

• Key Points: Chemical Properties of Alkenes

• Definition: Alkynes

• Physical properties of alkynes

1. Nature
2. Solubility
3. Melting point and Boiling point

• Acidic character of alkyne

• Formation of alkali metal ethynides (acetylides)
• Formation of heavy metal ethynides (acetylides)
• Formation of alkynyl Grignard reagents

• Addition reactions

• Addition of dihydrogen
• Addition of hydrogen (catalytic hydrogenation or reduction of alkynes)
• Addition of halogens (anti-addition): Action of chlorine, Action of bromine
• Addition of halogen acids (hydrogen halides)
• Addition of water (acid-catalyzed hydration of alkynes)

• Oxidation reactions

• Combustion
• Oxidation with alkaline potassium permanganate (test for unsaturation)
• Oxidative hydroboration

• Ozonolysis reactions
• Polymerization reactions: Linear and Cyclic polymerization

• Benzene
• Structure of benzene
• Aromatic character (Huckel Rule)
• Preparation of aromatic compounds
• Physical properties of benzene
• Chemical properties of benzene
• Directive influence of a functional group in monosubstituted benzene
• Carcinogenicity and Toxicity

• Methods of Preparation of Haloalkanes:

1. From Alcohols
2. From hydrocarbons
   - From alkanes by free radical halogenation
   - From Alkenes - Addition of hydrogen haldies, Addition halogens) 
3. Halogen exchange (Finkelstein reaction, Swarts reaction)

• Methods of Preparation of Haloarenes:

1. From hydrocarbons by electrophilic substitution
2. From amines by Sandmeyer’s reaction

• Alkenes
• Occurrence
• Isomers in alkenes

• Definition: Carboxylic Acid
• Formula: Carboxylic Acid
• Key Points: Carboxylic Acid

• Mechanism of Addition Polymerisation
  1) Free radical mechanism
• Some Important Addition Polymers
  (a) Polythene
  (i) Low density polythene
  (ii) High density polythene
  (b) Polytetrafluoroethene (Teflon)
  (c) Polyacrylonitrile

• Condensation Polymerisation or Step Growth Polymerisation
• Some Important Condensation Polymers
  (a) Polyamides: Nylons
  (i) Nylon 6, 6
  (ii) Nylon 6
  (b) Polyesters
  (c) Phenol - formaldehyde polymer (Bakelite and related polymers)
  (d) Melamine - formaldehyde polymer

• Natural rubber (Vulcanisation of rubber),
• Synthetic rubbers

1. Buna-S rubber
2. Buna-N rubber or nitrile rubber
3. Neoprene rubber

Polypropene, Polystyrene, Polyvinyl chloride (PVC), Urea-formaldehyle Resin, Glyptal, Bakelite

• Biomolecules
• Importance of biomolecules

• Carbohydrates
• Classification of carbohydrates

• Proteins
• Based on our nutritional requirements, amino acids are classified as:
  1) Non-essential amino acids 
  2) Essential amino acids
• Functions of proteins
• Bonding and protein structure
  1) Peptide bond of proteins or polypeptides
• Classification of proteins
  1) Primary (Basic) structures
  2) Secondary structure
  3) Tertiary structure
  4) Quaternary structure
• Amino acids

• Classification of Drugs
  (a) On the basis of pharmacological effect
  (b) On the basis of drug action
  (c) On the basis of chemical structure
  (d) On the basis of molecular targets

• Catalytic action of enzymes
• Drug-enzyme interaction

• Tranquilizers
• Analgesics
  (i) Non-narcotic (non-addictive) analgesics
  (ii) Narcotic analgesics

• Antibiotics
• Antiseptics and disinfectants

• Artificial Sweetening Agents
• Food Preservatives
• Antioxidants in Food

• Types of soaps
• Why do soaps not work in hard water?

• Anionic Detergents
• Cationic Detergents
• Non-ionic Detergents