NEET (UG) Chemistry Syllabus: Check the Latest Syllabus

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

• 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

• Introduction
• Types of Unit System

• Order of magnitude
• Significant figures
• Addition and subtraction of significant figures
• Multiplication and division of significant figures
• Rules for limiting the result to the required number of significant figures
• Rules for arithmetic operations with significant figures
• Rounding-off in the measurement

• Introduction
• Experiment

• Experiment 
• Elements

• Mendeleev's Classification
• Anomalies of Mendeleev’s Periodic Table

• Introduction
• Experiment 1
• Experiment 2

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

• Molecule
• Properties of molecule

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

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

• Concept of Mole
• Quantities Related on Mole Concept and Their Formula
• Experiment

• 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

• Reactions in solutions

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

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

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

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

• Introduction of Isotopes
• Applications of Isotopes

• Introduction
• Example of Isobars
• Characteristics of Isobars

• Isotones or Isoneutronic
• Examples

• 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

• 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

• 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

• 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)

• Introduction
• Structure and Property

• Merits
• Demerits

• 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

• Nature of intermolecular forces
• Boiling point
• Solubility

• Chemical reactivity
• Nature of oxides

• Chemical bond
• Causes of chemical combination
  i) Tendency to acquire stability
  ii) Tendency to acquire noble gas configuration

• 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

• Ionic bond or Electrovalent bond
• Mechanism of formation of ionic bond
• Lattice enthalpy
• Factors affecting the formation of an ionic bond
  i) Low ionization enthalpy
  ii) High negative electron gain enthalpy
  iii) Large lattice enthalpy
• Characteristics of ionic or electrovalent compounds
• Difference between ionic bond and covalent bond
• Covalent character in ionic bond
• Fajan's rules

• 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

• 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

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

• 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

• Measurable properties of gases

1. Mass
2. Volume
3. Pressure
4. Temperature
5. Density
6. Diffusion

• The Gas Laws
• Standard variables for gas laws

1. The volume (V)
2. The pressure (P)
3. The temperature (T)

• Ideal behaviour of gases
• Gases law: Boyle's law, Charles' law, Gay Lussac's law, Avogadro's law
• Universal gas constant
• Ideal gas equation
• Ideal gas
• Nature of universal gas constant 'R'
• Values of universal gas constant 'R' in different units
• Combined gas equation
• Relation between density (d), molar mass (M), and pressure (P) of a gas
• Expression for Molar mass

• 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

1. Vapour Pressure
2. Surface Tension
3. Viscosity

• 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

• 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

• First law of thermodynamics
• Formulation of first law of thermodynamics
• First law of thermodynamics for various processes

1. Isothermal process
2. Adiabatic process
3. Isochoric process
4. Isobaric process

• Justification
• Mathematical expression
• Some useful conclusions are drawn from the law
• Limitations
• Expressions for the work done by an ideal gas under different conditions

• Enthalpy
• Relationship between ∆H and ∆U for chemical reactions
• Work done in chemical reaction

• Relation between standard Gibbs energy change and equilibrium constant

• Clausius' Statement
• Kelvin Planck's Statement
• Entropy

• Introduction
• Types of Chemical Reaction
• Experiment

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

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

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

• 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
• Introduction of Acid
• Types of acid based on the source
• Types of acid based on the presence of oxygen
• Types of acid based on the strength of the acid
• Types of acid based on its concentration
• Types of acid based on the basicity of the acid

• Dissociation constant of weak acids and weak bases
• Ostwald's dilution law

• Relative strength of inorganic acids

1. Hydrides
2. Oxyacids
3. Relative strength of organic acids
4. Relative strength of inorganic bases
5. Relative strength of organic bases

• pH of a solution
• pH scale
• Relationship between pH and pOH
• Approximate pH values of some substances
• Acidity, basicity, and neutrality of aqueous solutions
• pK value
• Measurement of pH of a solution
• Indicators
• Titration curves

• Types of buffer solutions
• Buffer action
• Buffer capacity and buffer index
• Henderson - Hasselbalch equation
• Properties of buffer solution
• Applications of buffer solution

1. In biochemical system
2. Agriculture
3. Industry
4. Medicine
5. Analytical chemistry

• 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

• Redox reactions
• Half reactions

• 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

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

• Direct redox reactions
• Daniel cell
• Standard electrode potential

• 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

• 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

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

• Uses of boron
• Uses of aluminium
• Some important alloys of aluminium
• Important compounds of aluminium

1. Aluminium chloride, AlCl₃
2. Potash alum K₂SO₄.Al₂(SO₄)₃.24H₂O

• 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

• Physical Properties of Carbon
• Chemical Properties of Carbon

• Organic chemistry
• Importance of organic chemistry
• Characteristics of organic compounds

1. Composition
2. Type of linkage
3. Catenation
4. Isomerism
5. Polymerization
6. Solubility
7. Melting and boiling point
8. Odour
9. Functional group
10. Combustibility
11. Homologous series

• 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

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

• Homologous Series in Organic Chemistry
• Examples of Homologous Series

• Common Naming System
• IUPAC Nomenclature

• Structural isomerism

1. Chain isomerism
2. Position isomerism
3. Functional group isomerism
4. Metamerism
5. Tautomerism

• Stereoisomerism
• Geometrical isomerism/Cis-trans isomerism
• Optical isomerism: enantiomers, dextrorotatory, laevorotatory, diastereomers, racemic mixture/ racemate, resolution.

• Fundamental concepts in organic reaction mechanism
• Bond fission
• Types of fission
  1) Homolytic bond fission/Homolysis
  2) Heterolytic bond fission/Heterolysis
• Reaction intermediates
• Relative stability order of reaction intermediates

1. Free radicals
2. Carbocation
3. Carbanion

• Differences between carbocation and carbanion

• Introduction
• Properties of Covalent Compounds
• Saturated Hydrocarbons
• Unsaturated Hydrocarbons

• Classification of hydrocarbons

1. Saturated hydrocarbons
   a) Straight chain alkanes
   b) Branched-chain alkanes
2. Unsaturated hydrocarbons
   a) Alkenes
   b) Alkynes
3. Aromatic hydrocarbons
   a) Benzenoids
   b) Non-benzenoids

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

• Alkenes
• General formula
• Occurrence

• Isomerism in alkenes
• Preparation of alkenes
• Physical properties of alkenes
• Chemical properties of alkenes
• Uses of alkenes

• Structural isomerism

1. Chain isomerism
2. Position isomerism
3. Functional group isomerism
4. Metamerism
5. Tautomerism

• Stereoisomerism
• Geometrical isomerism/Cis-trans isomerism
• Optical isomerism: enantiomers, dextrorotatory, laevorotatory, diastereomers, racemic mixture/ racemate, resolution.

• Chemical properties of alkenes

1. Addition reactions: Addition of dihydrogen, Addition of hydrogen (catalytic hydrogenation), Addition of halogens, Addition of hydrogen halides, Addition reaction of HBr to symmetrical alkenes, Markovnikov's rule, Anti-Markovnikov's rule or Peroxide effect, Oxymercuration demercuration (Indirect hydration of alkenes), Addition of sulphuric acid, Addition of water, Oxidation, Addition of ozone (ozonolysis)
2. Mechanism of electrophilic reaction
3. Oxidation reactions: Combustion, Hydroboration-oxidation, Oxidation with potassium permanganate (alkaline), Oxidation with acidic or hot potassium permanganate or potassium dichromate, Catalytic oxidation/ Epoxidation
4. Polymerization reaction
5. Uses of alkenes

• Isomerism in alkynes
• Preparation of alkynes
• Physical properties of alkynes
• Chemical properties of alkynes
• Uses of acetylene

• 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

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

• Bio-degradable pollutants
• Non bio-degradable pollutants 
• Water Pollution
• Air Pollution
• Noise Pollution

• Smog
• Types of smog

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

• Effects of smog
• Control of photochemical smog

• Acid rain
• Formation of acid rain
• Harmful effects of acid rain

1. Effect on vegetation
2. Effect on aquatic life
3. Effect on fertility of the soil
4. Effect on buildings and monuments

• Effect on human health
• Effect on ecological balances

• Effects of Global Warming
• Sources of Green House Gases Emission (Natural and Anthropogenic)
• Strategies to deal with Global Warming
• Ozone depletion
• Effects of Ozone depletion

• Types of industrial waste

1. Biodegradable wastes
2. Non-biodegradable wastes

• Water Pollution
• Types of Water Pollutants
• Causes of Water Pollution
• Reasons of Water Pollution

• Soil pollution
• Sources of soil pollution 

1. Dumping of non-biodegradable waste
2. Acid rain
3. Radioactive substances
4. Pesticides
5. Herbicides
6. Artificial fertilizers
7. Pesticides
8. Fungicides

• Biomagnification

• 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

• Classification of solids

1. Crystalline solids
2. Amorphous solids

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

• Classification of crystalline solids

1. Molecular solids:
   a) Polar molecular solids
   b) Non-polar molecular solids
   c) Hydrogen-bonded molecular solids
2. Ionic Solids
3. Metallic solids
4. Covalent or Network Solids

• Structure and properties of diamond, graphite, and fullerene

• 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

Electrical properties: Conductors, semiconductors (n & p types) and insulators (Band Theory), piezoelectricity and pyroelectricity.

• Magnetic properties:

1. Magnetising field
2. Magnetic permeability
3. Intensity of magnetisation
4. Magnetic induction or total magnetic field
5. Magnetic susceptibility

• Substances can be classified into five categories:

1. Paramagnetic
2. Diamagnetic
3. Ferromagnetic
4. Antiferromagnetic
5. Ferrimagnetic

1. Gaseous Solutions
2. Liquid Solutions
3. Solid Solutions

• Mass percentage (w/w)
• Volume percentage (V/V)
• Mass by volume percentage (w/V)
• Parts per million
• Mole fraction
• Molarity
• Molality
• Standard solutions and working standards
• Advantages of using standard solutions

• Factors affecting solubility

1. Nature of solute and solvent
2. Effect of temperature on solubility
3. Effect of pressure on solubility

• Solid solutions
• Types of solid solutions

1. Substitutional solid solutions
2. Interstitial solid solutions

• Ideal Solutions
• Non-ideal Solutions

• Non-ideal solutions - positive deviation from Rauolt's Law
• Non-ideal solutions - negative deviation from Rauolt's Law

• Factors responsible for deviation from Raoult’s law

1. Solute-solvent interactions
2. Dissociation of solute
3. Association of solute
4. Temperature
5. Pressure
6. Concentration

• Abnormal molecular masses
  a) Association of solute particles
  b) Dissociation of solute particles
• Van't Hoff Factor
• Significance of van't Hoff factor
  a) Degree of dissociation
  b) Degree of association

• Redox reactions
• Half reactions

• Electrochemical reactions
• Electrodes
• Types of electrochemical cells

1. Galvanic cell
2. Electrolytic cells

• 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

• Galvanic or Voltaic cells

• Reduction half-cell
• Oxidation half-cell
• Joining half-cells
• Anodic oxidation
• Cathodic reduction
• Completion of circuit
• Consumption of Electrodes

• Salt bridge
• Cell notation or representation of a galvanic cell
• Cell electromotive force (e.m.f.)

• Electrode potential
• Cell potential or e.m.f.
• Difference between e.m.f. and potential difference
• Standard electrode potential
• Dependence of cell potential on concentration (Nernst equation)

• Reference electrode
• Standard Hydrogen Electrode (SHE): Construction, Electrode reactions, Application, Limitations
• Calomel electrode: Construction, Electrode reactions, Advantages of calomel electrode

• Electrochemical series
• Convention used in the construction of electrochemical series
• Applications of electrochemical series

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

• Derivation of Nernst equation
• Applications of Nernst equation

• Conductors
• Difference between Electronic and Electrolytic conduction
• Non-electrolytes
• Factors affecting electronic or metallic conduction
• Factors affecting electrical conductivity of electrolytic solutions
• Electrolytic conduction (Conductance in electrolytic solutions)

• Electrolytic cells
• Process of electrolysis
• Preferential Discharge Theory
• Some Examples of Electrolysis
• Quantitative Aspects of Electrolysis
• Faraday's laws of electrolysis
  1) Faraday's First Law of Electrolysis
  2) Faraday's Second Law of Electrolysis

• Fuel cells
• Hydrogen-oxygen fuel cell
• Advantage and disadvantage of fuel cell

• Corrosion
• Experiment
• Rusting Process and Corrosion Effect

• Various factors influencing the rate of a chemical reaction

1. Concentration of reactants
2. Pressure of gaseous reactants
3. Temperature of the system
4. Presence of a catalyst

• Dependence of Rate on Concentration, temperature, catalyst
• Rate Expression and Rate Constant/ Rate law and Specific Rate Constant
• Order of a Reaction
• Molecularity of a Reaction

• Rate law
• Applications of the rate law
• Rate constant
• Difference between rate of reaction and rate constant

• Order of a reaction
• Reactions of different orders

1. Zero order reactions
2. First order reactions
3. Second order reactions
4. Third order reactions
5. Reactions of fractional order

• Determination of rate law using initial rates

• Elementary reaction
• Complex reactions
• Molecularity of reaction
• Order and molecularity of elementary reactions
• Rate determining step
• Reaction intermediate
• Differences between order and molecularity

• Integrated rate law for zero order reactions
• Units of rate constant of zero order reactions
• Graphical representation of zero order reaction
• Examples of zero order reactions

• Integrated rate law for first order reactions
• Units of rate constant for the first order reaction
• Graphical representation of first order reaction
• Examples of first order reactions
• Various forms of the integrated rate law for the first order reactions

• Half life of the first order reactions (`t _(1/2)`)
• Half life and rate constant of the first order reaction
• Graphical representation of Half life period of first order reaction
• Half life of zero order reactions

• Activation energy
• Arrhenius equation
• Most probable kinetic energy
• Effect of Catalyst

• Collision between reactant molecules
• Energy requirement - Activation energy
• Orientation of reactant molecules

• 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

• Factors affecting adsorption of gases on solids

1. Nature of the gas (adsorbate)
2. Nature of adsorbent
3. Surface area of the adsorbent
4. Temperature of the surface
5. Pressure of gas

• 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

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

• 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)

• 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

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

• Occurrence of metals
• Minerals and ores

• Introduction
• Metallurgical Process

• 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

• Hoope's electrolytic process

• Occurrence
• Extraction of zinc
• Refining

• 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)

• Compounds of Xenon

1. Xenon fluorides
   a) Xenon difluoride (XeF₂)
   b) Xenon tetrafluoride (XeF₄)
   c) Xenon hexafluoride (XeF₆)
2. Xenon oxides
   a) Xenon trioxide (XeO₃)
   b) Xenon tetraoxide (XeO₄)
   c) XeOF₄ and XeO₂F₂

• Uses of Helium
• Uses of Neon
• Uses of Argon
• Uses of Krypton
• Uses of Xenon
• Uses of Radon

• Occurrence and characteristics of transition metals

• Properties of the first-row transition metals – metallic character
• Atomic and ionic radii
• Metallic character
• Melting and boiling points
• Colour
• Physical Properties
• Variation in Atomic and Ionic Sizes of Transition Metals
• Ionisation Enthalpies
• Oxidation States
• Standard electrode potentials
• Trends in the M²⁺/M Standard Electrode Potentials
• Trends inthe M³⁺/M²⁺ Standard Electrode Potentials
• Trends in Stability of Higher Oxidation States
• Chemical Reactivity and E^θ Values
• Magnetic Properties
• Formation of Coloured Ions
• Formation of Complex Compounds
• Catalytic Properties
• Complex formation
• Formation of Interstitial Compounds
• Alloy Formation
• Oxides and oxoanions of transition metals

• Potassium dichromate K₂Cr₂O₇
• Potassium permanganate KMnO₄

• Limitations of Werner’s theory

Coordination entity, Central atom/ion, Ligands, Colour, Shapes, Coordination number, Coordination sphere, Coordination polyhedron, Oxidation number of central atom, Homoleptic and heteroleptic complexes, charge number

• Stereoisomers
• Structural isomers (Constitutional isomers)
• Optical Isomerism

• Bonding in metal carbonyls
• Structures of metal carbonyls

• Stability of coordination compounds
• Factors which govern stability of the complex

1. Charge to size ratio of the metal ion
2. Nature of the ligand
3. Stability of chelates

• 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

• Common and IUPAC names of some monohalogen derivatives

• Preparation of Haloalkanes

1. By halogenation of alkanes
2. By halogenation of alkenes
3. By addition of hydrogen halides to alkenes
4. From alcohols
5. By halogen exchange

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. By electrophilic substitution
2. Sandmeyer's reaction

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

• Dichloromethane/methylene chloride (CH₂Cl₂)
• Chloroform/trichloromethane (CHCl₃)
• Carbon tetrachloride/tetrachloromethane (CCl₄)
• Idoform or triiodomethane (CHI₃)
• Freons
• Dichlorodiphenyltrichloroethane (DDT)

• 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

• From alkenes
  (i) By acid catalysed hydration: Mechanism of dehydration
  (ii) By hydroboration-oxidation
• From carbonyl compounds
  (i) By reduction of aldehydes and ketones
  (ii) By reduction of carboxylic acids and esters
• From Grignard reagents

• Methanol
• Ethanol

1. Alcohols as nucleophiles
2. Protonated alcohols as electrophiles

• Chemical reactions of alcohols

1. Reactions involving breaking of O-H bond
   a) Action of metals
   b) Acidic nature of alcohols
   c) Alcohols are weaker acids than water
   d) Esterification
2. Reactions involving breaking of C-O bond
   a) Reaction with hydrogen halides (HBr, HCI and HI)
   b) Reaction with phosphorus halides (PX₃/PX₅) and thionyl chloride (SOCl₂)
3. Oxidation of alcohols
   a) Primary alcohols
   b) Secondary alcohols
   c) Tertiary alcohols
   d) Action of copper on alcohol

• Classification of phenols

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

• Nomenclature of phenols

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

• From chlorobenzene: Dow's method (Commercial method)
• From benzene sulphonic acid
• From diazonium salts
• From cumene (Commercial method)
• From Aniline (Diazotization method)

• Chemical Properties of Phenol

1. Reactions involving cleavage of O-H bond: Reaction with metals, Esterification, Acetylation
2. Electrophilic aromatic substitution reactions of phenol
   (i) Nitration
   (ii) Halogenation (bromination)
3. Kolbe's reaction
4. Reimer-Tiemann reaction
5. Reaction of phenol with zinc dust
6. Catalytic hydrogenation
7. Oxidation reaction

• Distinguishing test between alcohols and phenols
• Differentiation between alcohols and phenols

• Simple or Symmetrical
• Mixed or Unsymmetrical

• Isomerism

1. Chain isomerism
2. Functional isomerism
3. Metamerism

• Chemical properties of ethers
• Laboratory test for ethers
• Reaction involving alkyl group of ether
• Action of hydrogen halide
• Hydrolysis (action of dilute H₂SO₄)
• Reaction with PCl₅
• Electrophilic substitution reactions: Halogenation, Nitration and Friedel-crafts reaction

• Classification of ketones

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

• Classification of mono and di carboxylic acids with examples.

• 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 amines

1. Aliphatic amines
2. Aromatic amines

• Introduction
• Resonance structure 
• Method of preparation of Diazonium salts
• Physical properties 
• Chemical reactions

1. Replacement reactions involving loss of nitrogen 
2. Reactions involving retention of diazo group

• Introduction 
• alkyl cyanides and alkyl isocyanides

1. Alkyl cyanides - Preparation, Properties, and reactions
2. Alkyl isocyanides: Preparation, Properties, and reactions

• Biomolecules
• Importance of biomolecules

• Carbohydrates
• Classification of carbohydrates

• Classification of carbohydrates

• On the basis of hydrolysis

1. Simple carbohydrates
   i) Monosaccharides: Aldoses and Ketoses
2. Complex carbohydrates
   i) Oligosaccharides: Disaccharides, Trisaccharides, Tetrasaccharides
   ii) Polysaccharides: Homopoly-saccharides and Heteropoly-saccharides

• On the basis of solubility

1. Sugars: Reducing and Non-reducing sugars
2. Non-sugars

• Optical activity

Chemical Coordination

1. Autocrine 
2. Paracrine 
3. Endocrine 
4. Pheromone 

• Classification and functions of vitamins 

• Structure of DNA
• Structure of RNA
• Differences between DNA and RNA

• 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

• Poly β-hydroxybutyrate – co-β-hydroxy valerate (PHBV)
• Nylon 2– nylon 6
• Biodegradable and non-biodegradable polymers

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

• 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

• Antibiotics
• Antiseptics and disinfectants

• Artificial Sweetening Agents
• Food Preservatives
• Antioxidants in Food

• Types of cleansing agents
  a) Soaps
  b) Synthetic detergents
• Mechanism of cleansing action
• Differences between soaps and detergents

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

• Anionic Detergents
• Cationic Detergents
• Non-ionic Detergents

• 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

• Functional group
• Test for alcoholic (R-OH) group

1. Presence of R-OH group
2. Distinguishing between 1°, 2°, and 3° alcohols (Lucas test)

• Test for phenolic (Ar-OH) group

1. Presence of Ar-OH group
2. Colours produced by some phenolic compounds

• Test for carbonyl group
• Test for carboxyl (-COOH) group
• Test for amino (-NH₂) 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