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About JEE Advanced Exam

IIT JEE advanced exam is the next step after the IIT JEE mains exam. Students scoring a minimum of 75% marks and above in the Main exam are the only ones allowed to apply. This exam is the ultimate test for every aspiring engineer. Students who manage to get good scores in this exam are granted entry into IIT coourses and other prestigous institutions such as IISTs, ISMs and more.


JEE (Advanced) Chemistry Grades

The IIT JEE chemistry exam is divided into 2 separate tests. Chemistry is an integral part in both tests. Both tests have chemistry, physics and biology as their subjects. Out of the three, chemistry has the highest number of questions and marks allotted.

Subject paper 1 marks paper 2 marks
Chemistry 32 32
Physics 15 18
Mathematics 15 12

The Exam


The JEE (Advanced) exam has 2 tests

Each test of the IITJEE advanced exam is 3 hours long. the number of questions for each subject vary for each test. The student is reuired to perform well in both tests to gain meaningful merit.



Details Physics Chemistry Mathematics
No of questions 5 8 5
Marks per question 3 4 3
Negative Marking -1 -2 0

JEE Exam Calculator Policy

The use of calculators in strictly prohibited in the IIT JEE advanced exam. we highlly recommend learning and remember essential values and conversions to avoid roadblocks related to calculators.



JEE (Advanced) Chemistry Exam Course Content Outlined Below


Section A - Physical Chemistry


Unit -1 Basic Concepts -General topics

1.1 Concept of Atoms and Molecules.

1.2 Dalton’s Atomic Theory.

1.3 Mole concept.

1.4 Chemical formulae.

1.5 Balanced Chemical Equations Including Redox.

1.6 Calculations (based on mole concept) involving common oxidation-reduction.

1.7 Neutralisation, and displacement reactions.

1.8 Concentration in terms of

(a) Mole fraction.
(b) Molarity.
(c) Molality.
(d) Normality.


Unit -2 Gaseous and Liquid states


2.1 Absolute scale of temperature.

2.2 Ideal gas equation.

2.3 Deviation from ideality.

2.4 Van der Waals Equation.

2.5 Kinetic Theory of gases.

2.6 Average, Root mean Square and most Probable Velocities and their Relation with Temperature.

2.7 Law of partial pressures.

2.8 Vapour pressure.

2.9 Diffusion of gases.


Unit -3 -Atomic structure and chemical bonding


3.1 Bohr Model.

3.2 Spectrum of Hydrogen Atom.

3.3 Quantum Numbers.

3.4 Wave-Particle Duality.

3.5 de Broglie Hypothesis.

3.6 Uncertainty Principle.

3.7 Qualitative Quantum Mechanical Picture of Hydrogen Atom.

3.8 shapes of s, p and d orbitals.

3.9 Electronic Configurations of Elements (up to atomic number 36).

3.10 Aufbau principle.

3.11 Pauli’s Exclusion Principle and Hund’s Rule.

3.12 Orbital Overlap and Covalent Bond; Hybridization involving s, p and d orbitals only.

3.13 Orbital Energy Diagrams for Homonuclear Diatomic Species; Hydrogen bond.

3.14 Polarity in Molecules, Dipole Moment (Qualitative Aspects only).

3.15 VSEPR model and shapes of molecules.
(a) Linear
(b) Angular
(c) Triangular
(d) Square planar
(e) Pyramidal
(f) Square pyramidal
(g) Trigonal bipyramidal
(h) Tetrahedral and
(i) Octahedral


Unit -4- Energetics


4.1 First law of thermodynamics.
(a) Internal energy.
(b) Work and pressure-volume work.
(c) Heat.

4.2 Enthalpy.
(a) Heat of reaction.
(b) Fusion and.
(c) vapourization.

4.3 Hess’s law.

4.4 Second law of thermodynamics.
(a) Entropy.
(b) Free energy.
(c) Criterion of spontaneity.


Unit -5-Chemical equilibrium


5.1 Law of mass action.

5.2 Equilibrium constant.

5.3 Le Chatelier’s principle
(a) Effect of concentration.
(b) Temperature.
(c) Pressure.
(d) Effect of catalyst.

5.4 Significance of ΔG and ΔG0 in chemical equilibrium.

5.5 Solubility product.

5.6 Common ion effect.

5.7 Acids and bases (Bronsted and Lewis concepts).

5.8 pH and pOH.

5.9 Hydrolysis of salts.

5.10 Buffer solutions


UNIT 6: SOLUTIONS


6.1 Electrochemical cells and cell reactions.

6.2 Standard electrode potentials.

6.3 Nernst equation and its relation to ΔG.

6.4 Electrochemical series.

6.5 Emf of galvanic cells.

6.6 Faraday’s laws of electrolysis.

6.7 Electrolytic conductance.

6.8 specific, equivalent and molar conductivity.

6.9 Kohlrausch’s law.

6.10 Concentration cells.


Unit -7-Chemical kinetics


7.1 Rates of chemical reactions.

7.2 Order of reactions.

7.3 Rate constant.

7.4 First order reactions.

7.5 Temperature dependence of rate constant -Arrhenius equation.


Unit -8-Solid state


8.1 Classification of solids.

8.2 Crystalline state.

8.3 Seven crystal systems (cell parameters a, b, c, α, β, γ).

8.4 Close packed structure of solids (cubic).

8.5 Packing in fcc, bcc and hcp lattices.

8.6 Nearest Neighbours, Ionic Radii, Simple Ionic Compounds, Point Defects.


Unit -9-Solutions


9.1 Raoult’s law.

9.2 Molecular weight determination from
(a) Lowering of vapour pressure.
(b) Elevation of boiling point.
(c) Depression of freezing point.


Unit -10-Surface Chemistry


10.1 Elementary Concepts of Adsorption (Excluding Adsorption Isotherms).

10.2 Colloids.
(a) Types.
(b) Methods of preparation.
(c) General properties.

10.3 Elementary Ideas of Emulsions.

10.4 Surfactants and Micelles (Only Definitions and Examples).


Unit -11-Nuclear chemistry


11.1 Radioactivity.

11.2 Isotopes and Isobars.

11.3 Properties of α, β and γ rays.

11.4 Kinetics of Radioactive Decay (Decay Series Excluded).

11.5 Carbon Dating.

11.6 Stability of Nuclei with Respect to Proton-Neutron Ratio.

11.7 Brief Discussion on.
(a) fission.
(b) fusion reactions.


Section B - Inorganic Chemistry


Unit -12- Important non metals and their properties


12.1 Isolation/Preparation and Properties of the following Non-Metals
(a) Boron
(b) Silicon
(c) Nitrogen
(d) Phosphorus
(e) Oxygen
(f) Sulphur
(g) Halogens

12.2 Properties of allotropes of
(a) Carbon (only diamond and graphite).
(b) Phosphorus and.
(c) Sulphur.

12.3 Preparation and Properties of the following compounds.
(a) Compounds of sodium potassium magnesium and calcium with
i Oxides.
ii Peroxides.
iii Hydroxides.
iv Carbonates.
v Bicarbonates.
vi Chlorides.
vii Sulphates.
(b) Boron: Diborane, Boric Acid and Borax.
(c) Aluminium: Alumina, Aluminium Chloride and Alums.
(d) Carbon: Oxides and Oxyacid (Carbonic Acid).
(e) Silicon:Silicones, Silicates and Silicon Carbide.
(f) Nitrogen: Oxides, Oxyacids and Ammonia.
(g) Phosphorus: Oxides, Oxyacids (Phosphorus Acid, Phosphoric Acid) and Phosphine.
(h) Oxygen: Ozone and Hydrogen Peroxide.
(i) Sulphur: Hydrogen Sulphide, Oxides, Sulphurous Acid, Sulphuric Acid and Sodium Thiosulphate.
(j) Halogens: Hydrohalic Acids, Oxides and Oxyacids of Ohlorine, Oleaching Oowder, Xenon fluorides.


Unit -13-Transition elements (3d series)


13.1 Definition and General Characteristics of Transition Metals.

13.2 Oxidation States and their Stabilities.

13.3 Colour (Excluding the details of Electronic Transitions).

13.4 Calculation of spin-only Magnetic Moment.

13.5 Coordination compounds
(a) Nomenclature of Mononuclear Coordination Compounds.
(b) Cis-trans and Ionization Isomerism.
(c) Hybridization and Geometries of Mononuclear Coordination Compounds (Linear, Tetrahedral, Square Planar and Octahedral).

Unit -14-Preparation and Properties of the following Compounds


14.1 Oxides and Chlorides of Tin and Lead.

14.2 Oxides, Chlorides and Sulphates of Fe2+, Cu2+ and Zn2+.

14.3 Potassium Permanganate, Potassium Dichromate.

14.4 Silver Oxide, Silver Nitrate, Silver Thiosulphate.


Unit -15 -Ores and minerals


15.1 Commonly Occurring Ores and Minerals of
(a) Iron.
(b) Copper.
(c) Tin.
(d) Lead.
(e) Magnesium.
(f) Aluminum.
(g) Zinc.
(h) Silver.

15.2 Extractive metallurgy.
(a) Chemical principles reactions only (Industrial Details Excluded).
(b) Carbon reduction method (Iron and Tin).
(c) Self reduction method (Copper and Lead).
(d) Electrolytic reduction method (Magnesium and Aluminium).
(e) Cyanide process (Silver and Gold).

Unit -16-Principles of Qualitative Analysis


16.1 (a) Groups I to V (only Ag+, Hg2+, Cu2+, Pb2+, Bi3+, Fe3+, Cr3+, Al3+, Ca2+, Ba2+, Zn2+, Mn2+ and Mg2+).

16.2 (b) Nitrate, Halides (Excluding Fluoride), Sulphate and Sulphide.


Section C - Organic Chemistry


Unit -17-Concepts


17.1 Hybridisation of carbon
(a) σ and π-bonds.
(b) Shapes of Simple Organic Molecules.

17.2 Isomerism
(a) Structural Isomerism.
(b) Geometrical isomerism.
(c) Optical isomerism of compounds containing up to two asymmetric centres, (R,S and E,Z nomenclature excluded).

17.3 IUPAC nomenclature of simple organic compounds (only hydrocarbons, mono-functional and bi-functional compounds).

17.4 Conformations of ethane and butane (Newman projections).

17.5 Resonance.

17.6 Hyperconjugation.

17.7 Keto-enoltautomerism.

17.8 Determination of empirical and molecular formulae of simple compounds (only combustion method).

17.9 Hydrogen bonds: Definition and their Effects on Physical Properties of Alcohols and Carboxylic Acids.

17.11 Polarity and Inductive Effects in Alkyl Halides.

17.12 Reactive Intermediates Produced During Homolytic and Heterolytic Bond Cleavage.

17.13 Formation, Structure and Stability of Carbocations, Carbanions and free Radicals.


Unit -18-Preparation, Properties and Reactions of Alkanes


18.1 Homologous series,

18.2 Physical properties of alkanes (melting points, boiling points. and density).

18.3 Combustion and halogenation of alkanes.

18.4 Preparation of alkanes by Wurtz reaction.

18.5 Decarboxylation reactions.


Unit -19-Preparation, Properties and Reactions of Alkenes and Alkynes

19.1 Physical properties of alkenes and alkynes (boiling points, density and dipole moments).

19.2 Acidity of alkynes.

19.3 Acid catalysed hydration of alkenes and alkynes (excluding the stereochemistry of addition and elimination).

19.4 Oxidation Reactions of alkenes with KMnO4 and ozone.

19.5 Reduction of alkenes and alkynes.

19.6 Preparation of alkenes and alkynes by Elimination reactions.

19.7 Electrophilic Addition Reactions Of Alkenes with
(a) X2,
(b) HX,
(c) HOX and
(d) H2O(X=halogen)

19.8 Addition Reactions of Alkynes.

19.9 Metal acetylides.


Unit-20-Reactions of Benzene


20.1 Structure and Aromaticity.

20.2 Electrophilic Substitution Reactions:
(a) Halogenation.
(b) Nitration.
(c) Sulphonation.
(d) Friedel-Crafts alkylation and acylation.

20.3 Effect of o-, m- and p-directing groups in monosubstituted benzenes.


Unit -21-Phenols


21.1 Acidity.

21.2 Electrophilic Substitution Reactions
(a) Halogenation.
(b) Nitration and.
(c) Sulphonation.

21.3 Reimer-Tieman reaction.

21.4 Kolbe reaction.


Unit -22-Characteristic Reactions of the following (Including those Mentioned above)


22.1 Alkyl halides
(a) Rearrangement Reactions of alkyl Carbocation.
(b) Grignard Reactions.
(c) Nucleophilic Substitution Reactions.

22.2 Alcohols:
(a) Esterification.
(b) Dehydration and.
(c) Oxidation.
(d) Reaction with sodium.
(e) Phosphorus halides.
(f) ZnCl2/concentrated HCl.
(g) Conversion of alcohols into aldehydes and ketones.

22.3 Ethers
(a) Preparation by Williamson’s Synthesis;

22.4 Aldehydes and Ketones:
(a) Oxidation.
(b) Reduction.
(c) Oxime and.
(d) Hydrazone formation.
(e) Pldol condensation.
(f) Perkin reaction.
(g) Cannizzaro reaction.
(h) Haloform reaction and.
(i) Nucleophilic addition reactions (Grignard addition).

22.5 Carboxylic acids.
(a) Formation of Esters, acid Chlorides and Amides, Ester Hydrolysis;

22.6 Amines.
(a) Basicity of substituted anilines and aliphatic amines, p
(b) Reparation from nitro compounds.
(c) Reaction with nitrous acid.
(d) Azo coupling reaction of diazonium salts of aromatic amines.
(e) Sandmeyer and related reactions of diazonium salts.
(f) Carbylamine reaction.

22.7 Haloarenes
(a) Nucleophilic Aromatic substitution in Haloarenes and Substituted Haloarenes (Excluding Benzyne Mechanism and Cine Substitution).


Unit -23-Carbohydrates


23.1 Classification mono- and di-saccharides (Glucose and Sucrose);

23.2 Oxidation, Reduction.

23.3 Glycoside formation and Hydrolysis of Sucrose.


Unit -24-Amino Acids and Peptides


24.1 General Structure (only primary structure for peptides) and physical properties.


Unit -25-Properties and uses of some important polymers


25.1 Natural Rubber.
(a) Cellulose
(b) Nylon
(c) Teflon and
(d) PVC


Unit -26 -Practical Organic Chemistry


26.1 Detection of Elements (N, S, Halogens).

26.2 Detection and Identification of the following functional groups:
(a) Hydroxyl (Alcoholic and phenolic).
(b) Arbonyl (Aldehyde and ketone).
(c) Carboxyl (Amino and Nitro).

26.3 Chemical methods of separation of mono-functional organic compounds from binary mixtures.





7.1 Exceptions to the Aufbau Principle.

7.2 Assignment of quantum numbers to the electron.

7.3 Phase diagram.

7.4 Calculations of molality, percent by mass and percent by volume.

7.5 Colligative properties.

7.6 Weaker hydrogen bonding: Hydrogen bonding due to high electronegative elements N, O, F will be tested.

7.7 Crystal shapes or structures.

7.8 Use of Formal change to explain why certain molecules do not obey the octet rule.

7.9 Limitations of Lewis dot model.

7.10 Molecules orbital diagrams, and filling of orbital diagrams.

7.11 Varieties of crystal lattices for ionic compounds.

7.12 Lewis- acid- Base concepts.

7.13 Language of reducing agent and oxidizing agent.

7.14 Labeling electrodes as positive or negative.

7.15 Nernst Equation Calculations. Qualitative reasoning based on the Nernst Equation is the part of the exam.

7.16 Calculations based on Arrhenius equation. Conceptual aspects and interpretation of graphs is the part of the course.

7.17 Calculations of the Concentration of each species present in the titration curve for polyprotic acids.

7.18 Calculations of the Change in pH due to addition of an acid or a base to a Buffer.

7.19 The Derivation of the Henderson – Hasselbalch Equation.

7.20 Memorization of Solubility rules’ Other than that all salts of first group ions, Ammonium and nitrates are Soluble in water.


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