NEET (UG) Chemistry Syllabus: Check the Latest Syllabus

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

• Physical quantities
• Some physical quantities
• Types of Physical quantities
  (i) Fundamental quantities
  (ii) Derived quantities
• Measurement

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

• Units
• Types of units : Fundamental and Derived units

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

• Introduction
• Experiment

• Definition: Limiting Reagent or Limiting Reactant
• Law: Gay-Lussac's Law of Combining Volumes

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

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

• Percentage composition
• Chemical formula
  1) Empirical formula
  2) Molecular formula
• Steps involved in determining the empirical formula
• Steps for determination of the molecular formula of a compound

• 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

• Introduction
• Examples

• Atomic number or Nuclear charge
• Nucleons
• Mass number
• Relationship between atomic number and mass number
• Representation of element
• Number of Neutrons (n)

• Definition: Isotopes
• Examples

• Origin
• Structure of an Atom
• Structure of Nucleus
• Atomic Number
• Mass Number

• 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

• Perfectly black body 
• Ferry's black body
• Spectrum of black body radiation in terms of wavelength

• Photoelectric Effect
• Dual Behaviour of Electromagnetic Radiation

• Experimental Set-up of Photoelectric Effect
• Observations from Experiments on Photoelectric Effect
• Failure of Wave Theory to Explain the Observations from Experiments on Photoelectric Effect
• Einstein’s Postulate of Quantization of Energy and the Photoelectric Equation
• Dual behaviour of electromagnetic spectrum

• Emission and Absorption Spectra
• Line Spectrum of Hydrogen

• Introduction
• Bohr’s stable orbit atomic model
• Merits and Demerits

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

• 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

• 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

• Definition: Periodic Trends
• Definition: valency

• 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

• 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

• 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

• 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

• Effects of hydrogen bonding

1. Dissociation
2. Association: High melting and boiling point, examples
3. Solubility
4. Volatility
5. Viscosity and surface tension
6. Density of water

• 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

• Classification of Thermodynamic Processes

1. Quasi-static (nearly static) process
2. Isothermal process
3. Adiabatic process
4. Isobaric process
5. Isochoric process
6. Polytropic process
7. Cyclic process
8. Non-cyclic process
9. Reversible process
10. Irreversible process

• Internal energy (U)
• Characteristics of internal energy
• Change in internal energy (ΔU)
• Heat (q) and work (w)
• Units of heat and work
• Sign conventions for heat and work
• Zeroth 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

• Henry's law

• 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

• Homogeneous reactions and Heterogeneous reactions
• Equilibrium constant for heterogeneous equilibria
• Units of equilibrium constant

• 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

• Chemical equilibrium
• Two types of chemical equilibrium
  1) Homogeneous equilibrium
  2) Heterogeneous equilibrium
• Characteristics of equilibria involving chemical processes
• Graphical representation of chemical equilibrium

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

• Introduction
• Acid
• Base
• Salt

• Redox reactions
• Half reactions

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

• Metal activity series or electrochemical series

• 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

• 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)

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

• 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

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

• Atomic radius

• Covalent radius
• Metallic radius
• Periodic Trends in Atomic Radius

1. Variation in Periods
2. Effective nuclear charge
3. Variation in Group

• Ionic radius
• Ionisation energy

• Successive Ionisation energies
• Periodic Trends in Ionisation Energy
• Periodic variation in group
• Ionisation energy and shielding effect

• Electron Affinity

• Variation of Electron Affinity in a period
• Variation of Electron affinity in a group

• Electronegativity

• Variation of Electronegativity in a period
• Variation of Electronegativity in a group

• Chemical reactivity
• Nature of oxides

• Retention factor (R_f)

• Definition: Organic Chemistry
• Definition: Inorganic Chemistry

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

• Definition: Homologous Series
• Key Points: Homologous Series

• Definition: Isomers

• Definition: Hydrocarbons
• Definition: Saturated Hydrocarbons
• Definition: Unsaturated Hydrocarbons
• Definition: Alkanes
• Definition: Alkenes
• Definition: Alkynes
• Key Points: Hydrocarbons

• Definition: Alkanes

• Definition: Alkenes

• Definition: Isomers

• Key Points: Physical Properties of Alkenes

• Key Points: Chemical Properties of Alkenes

• Definition: Alkynes

• Environment
• Elements of environment
  1) Non-living or Physical
  2) Living or Biological
• Environmental chemistry
• Goals of environmental chemistry

• Smog
• Types of smog

1. Classical or London smog
2. Photochemical smog or Los Angeles smog

• Effects of smog
• Control of photochemical smog

• Key Points: Greenhouse Effect and Global Warming

• Types of industrial waste

1. Biodegradable wastes
2. Non-biodegradable wastes

• Fluoride, Lead, Sulphate, Nitrate, Other metals

• 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

• 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

• Preparation of aluminium
• Properties of aluminium
• Reaction with acids
• Reaction with alkalies

• The tendency for catenation

• Definition: Aromatic Compounds
• Key Points: Straight Chains, Branched Chains, and Rings of Carbon Atoms

• Graphite
• Experiment
• Uses of Graphite

• Fullerene
• Uses of Fullerene

• Crystalline Forms
• Diamond
• Uses of Diamond

• 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

• Experiment 1
• Experiment 2
• Experiment 3
• Experiment 4
• Substance (Matter)
• Physical Nature of matter
• Chemical properties

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

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

• Introduction
• Definition: Ideal Gas Equation
• Law: Boyle's Law
• Law: Charles' Law
• Law: Gay-Lussac's Law
• Deriving the Ideal Gas Equation
• Formula Combines GAs Law
• Example
• Real-Life Applications
• Key Points: Ideal Gas Equation

• 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

• Hydrogen
• Position of hydrogen in the periodic table

• 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

• Softening of water

1. Removal of temporary hardness
   a) By boiling
   b) Clark's method
2. Removal of permanent hardness
   a) By washing soda method
   b) lon-exchange/Permutit method
   c) Calgon method
   d) Synthetic resins method
   ⇒ Ion exchange resins are of two types
   i) Cation exchange resins
   ii) Anion exchange resins

• Degree of hardness of water

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

• 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

• Biomolecules
• Importance of biomolecules

• Carbohydrates
• Classification of carbohydrates

• Optical activity

• Classification of ketones

1. Simple or symmetrical ketones
2. Mixed or unsymmetrical ketones

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

• Classification of carboxylic acids

1. Aliphatic carboxylic acids
   a) Mono-carboxylic acids
   b) Dicarboxylic acids
   c) Tricarboxylic acids
   d) Polycarboxylic acids
2. Aromatic carboxylic acids
   a) Aromatic mono-carboxylic acids
   b) Aromatic dicarboxylic 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

• Designing of a drug
• Drug target
• Action of drugs on targets

• Catalytic action of enzymes
• Drug-enzyme interaction

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

• Artificial Sweetening Agents
• Food Preservatives
• Antioxidants in Food

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

• Definition: Metallurgy
• Key Points: Metallurgy

• 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

• Aluminium
• Physical Properties of Aluminium
• Chemical Properties of Aluminium
• Uses of Aluminium

• Key Points: Extraction of Metals

• Occurrence
• Extraction of zinc
• Refining

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

• 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

• Analytical chemistry
• Analytical chemistry deals with methods for

1. Qualitative analysis
2. Quantitative analysis

• Basic laboratory techniques

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

• Definition: Functional Group

• Acetanilide
• p-Nitroacetanilide
• Aniline yellow/p-aminoazobenzene
• lodoform

• Mohr's salt
• Potash alum

• Titrimetric analysis
• Concentration or strength of a solution
• Normality
• Equivalent weight
• Types of titrations
• Acid base titrations
• Determination of the concentration .(strength) of a given solution of sodium hydroxide by titrating it against a standard solution of oxalic acid
• Determination of the concentration (strength) of a given solution of hydrochloric acid by titrating it against a standard solution of sodium carbonate
• Redox titrations
• Determination of the concentration/molarity of KMnO₄ solution by titrating it against a 0.1 M standard solution of oxalic acid
• Determination of the concentration/molarity of potassium permanganate (KMnO₄) solution by titrating it against standard solution of ferrous ammonium sulphate (Mohr's salt)

• Systematic qualitative analysis of salts
• Systematic qualitative analysis of basic radicals (cations)
• Systematic qualitative analysis of acidic radicals (anions)

• Enthalpy change
• Determination of the enthalpy of dissolution of copper sulphate using calorimetric technique

• Enthalpy of neutralization
• Determination of enthalpy of neutralization of strong acid and strong base

• Colloidal solution
• Preparation of lyophilic sol
• Preparation of lyophobic sol

• Rate of reaction
• Kinetic study of reaction of iodide ion with hydrogen peroxide at room temperature

• Oxygen-containing functional groups

1. Alcohols and phenols
2. Ethers

• Classification of alcohols

• On the basis of number of -OH groups

1. Monohydric alcohol
2. Dihydric alcohol
3. Trihydric alcohol
4. Polyhydric alcohol

• On the basis of nature of C-OH bond

1. C_sp3 - OH bond: Alkyl, Allylic, Benzylic alcohols
2. C_sp2 - OH bond

• Isomerism in alcohols

1. Chain isomerism
2. Position isomerism
3. Functional isomerism
4. Optical isomerism
5. Cis-trans isomerism

• Key Points: Physical Properties of Alcohols

• Key Points: Chemical Properties of Alcohols

• Classification of phenols

1. Monohydric phenols
2. Dihydric phenols
3. Tribydric phenols

• Nomenclature of phenols

1. Monohydric phenols
2. Dihydric phenols
3. Trihydric phenols

• Isomerism

1. Chain isomerism
2. Functional isomerism
3. Metamerism

• Redox reactions
• Half reactions

• Electrodes
• Types of electrodes

1. Metal-metal ions electrode
2. Metal-sparingly soluble salt electrode
3. Gas electrode (non metal-non metal ion electrode)
4. Redox electrode

• Definition: Electrochemical Series

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

• Definition: Corrosion

• Key Points: Prevention of Corrosion

• 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

• Surface chemistry
• Surface or interface

• Catalytic activity
• Promoters
• Poisons
• Catalytic selectivity
• Shape-selective catalysis

• 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)

• 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

• Halogen derivatives of alkanes and arenes
• Haloalkanes

• Classification of haloalkanes

• Classification of haloalkanes on the basis of the number of halogen atoms

1. Monohaloalkanes
2. Dihaloalkanes
3. Trihaloalkanes
4. Polyhaloalkanes

• Classification of monohalocompounds on the basis of hybridisation of the carbon atom to which the halogen is bonded (nature of C-X bond)

1. Compounds Containing sp³ C—X Bond (X = F, Cl, Br, I)
2. Compounds Containing sp² C—X Bond

1. Nucleophilic substitution reactions
2. Elimination reactions
3. Reaction with metals
4. Laboratory test for haloalkanes

• Optical activity
• Chirality
• Enantiomers
• Racemic mixture
• R, S configuration

• Nucleophilic substitution (S_N) reaction
• S_N2 Mechanism
• S_N1 Mechanism
• Comparison between S_N2 and S_N1 reaction

• Nomenclature of haloarenes
• Nature of C- X bond in haloarenes
• Methods of preparation
• Physical properties
• Chemical properties

1. Substitution reactions
2. Reactions with metals
3. Nucleophilic substitution reactions
4. Electrophilic substitution reactions: Halogenation, Nitration, Friedel-Craft's reaction, Sulphonation
5. Reaction with sodium metal: Wurtz Fittig reaction, Fittig reaction