JEE MAIN 2020 CHEMISTRY SYLLABUS
NATIONAL LEVEL ONLINE TEST
Chemistry is often considered the most scoring section by test takers and experts in JEE Main B.E/ B.Tech paper. As we know, it is divided into three parts Organic chemistry, Inorganic chemistry and Physical chemistry. All these three subdivisions vary in nature and therefore covering the chemistry syllabus requires a proper plan. Check JEE Main Exam Pattern
Through this article, we have tried to cover a range of aspects of JEE Main Chemistry Syllabus which includes, the unit wise syllabus, topic-wise weightage, video lectures, mock tests, reference books, difficulty level analysis, and tips for attempting the chemistry section and preparation strategies.
JEE Main Chemistry syllabus comprises a total of three sections spread over 28 units. Download JEE Main 2020 Official Syllabus Released by NTA
|Section A: Physical Chemistry|
|1.||Some Basic Concepts of Chemistry|
Matter and its nature, Dalton’s the atomic theory, the concept of the atom, molecule, element, and compound;
Physical quantities and their measurements in Chemistry, precision, and accuracy, significant figures, S.I. Units, dimensional analysis;
Laws of chemical combination;
Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae;
Chemical equations and stoichiometry.
|2.||States of Matter|
Classification of matter into solid, liquid and gaseous states;
Gaseous State: Measurable properties of gases; Gas laws – Boyle’s law, Charles’s law, Graham’s law of diffusion, Avogadro’s law, Dalton’s law of partial pressure;
The concept of the Absolute scale of temperature; Ideal gas equation, Kinetic theory of gases (only postulates);
The concept of average, root mean square and most probable velocities;
Real gases, deviation from Ideal behaviour, compressibility factor, van der Waals equation, liquefaction of gases, critical constants;
Liquid State: Properties of liquids – vapour pressure, viscosity and surface tension and effect of temperature on them (qualitative treatment only);
Solid State: Classification of solids-molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea);
Bragg’s Law and its applications;
Unit cell and lattices, packing in solids (fcc, bcc and hcp lattices), voids, calculations involving unit cell parameters, imperfection in solids;
Electrical, magnetic and dielectric properties.
Discovery of subatomic particles (electron, proton, and neutron);
Thomson and Rutherford atomic models and their limitations;
Nature of electromagnetic radiation, photoelectric effect;
The spectrum of hydrogen atom, Bohr model of hydrogen atom – its postulates, derivation of the relations for energy of the electron and radii of the different orbits, limitations of Bohr’s model;
Dual nature of matter, de-Broglie relationship, Heisenberg uncertainty principle;
Elementary ideas of quantum mechanics, the quantum mechanical model of an atom, its important features, the concept of atomic orbitals as one-electron wave functions;
Variation of Ψ1 and Ψ2 with r for 1s and 2s orbitals; various quantum numbers (principal, angular momentum, and magnetic quantum numbers), and their significance;
Shapes of s, p and d – orbitals, electron spin and spin quantum number;
Rules for filling electrons in orbitals – Aufbau principle, Pauli exclusion principle and Hund’s rule, electronic configuration of elements, the extra stability of half-filled, and completely filled orbitals.
|4.||Chemical Bonding and Molecular Structure|
Kossel – Lewis approach to chemical bond formation, the concept of ionic and covalent bonds;
Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy;
Covalent Bonding: Concept of electronegativity, Fajan’s rule, dipole moment; Valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules;
Quantum mechanical approach to covalent bonding: Valence bond theory, Its important features, the concept of hybridization involving s, p, and d orbitals; Resonance;
Molecular Orbital Theory: Its important features, LCAOs, types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, the concept of bond order, bond length and bond energy;
Elementary idea of metallic bonding, Hydrogen bonding, and its applications.
Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes;
First law of thermodynamics: Concept of work, heat internal energy, and enthalpy, heat capacity, molar heat capacity;
Hess’s law of constant heat summation;
Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization, and solution;
The second law of thermodynamics: Spontaneity of processes; Delta S of the universe and Delta G of the system as criteria for spontaneity, Delta Go (Standard Gibbs energy change) and equilibrium constant.
Different methods for expressing the concentration of a solution: molality, molarity, mole fraction, percentage (by volume and mass both), the vapour pressure of solutions and Raoult’s Law;
Ideal and non-ideal solutions, vapour pressure – composition, plots for ideal and non-ideal solutions;
Colligative properties of dilute solutions, relative lowering of vapour pressure, depression of freezing point, elevation of boiling point and osmotic pressure;
Determination of molecular mass using colligative properties;
Abnormal value of molar mass, Hoff factor, and its significance.
Meaning of equilibrium, the concept of dynamic equilibrium;
Equilibria involving physical processes: Solid – liquid, liquid – gas and solid – gas equilibria, Henry’s law, a general characteristic of equilibrium involving physical processes;
Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of Delta G and Delta Go in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, the effect of the catalyst;
Le Chatelier’s principle;
Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Bronsted-Lowry and Lewis) and their ionization, acid-base equilibria (including multistage ionization) and ionization constants, ionization of water, pH scale, common ion effect, hydrolysis of salts and pH of their solutions, solubility of sparingly soluble salts and solubility products, buffer solutions.
|8.||Redox Reactions and Electrochemistry|
Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, balancing of redox reactions;
Electrolytic and metallic conduction, conductance in electrolytic solutions, specific and molar conductivities and their variation with concentration;
Kohlrausch’s law and its applications;
Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half – cell and cell reactions, emf of a Galvanic cell and its measurement;
Nernst equation and its applications; Relationship between cell potential and Gibbs’ energy change;
Dry cell and lead accumulator, Fuel cells;
Corrosion and its prevention.
The rate of a chemical reaction, factors affecting the rate of reactions: concentration, temperature, pressure, and catalyst.
Elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units, differential and integral forms of zero and first order reactions, their characteristics and half-lives, the effect of temperature on the rate of reactions.
Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions (no derivation).
Adsorption: Physisorption and chemisorption and their characteristics, factors affecting the adsorption of gases on solids: Freundlich and Langmuir adsorption isotherms, adsorption from solutions.
Catalysis: Homogeneous and heterogeneous, activity and selectivity of solid catalysts, enzyme catalysis, and its mechanism.
Colloidal state: Distinction among true solutions, colloids, and suspensions, classification of colloids: lyophilic, lyophobic.
Multimolecular, macromolecular and associated colloids (micelles), preparation and properties of colloids: Tyndall effect, Brownian movement, electrophoresis, dialysis, coagulation, and flocculation.
Emulsions and their characteristics.
|Section B: Inorganic Chemistry|
|11.||Classification of Elements and Periodicity in Properties|
Modern periodic law and present form of the periodic table.
s, p, d and f block elements.
Periodic trends in properties of elements atomic and ionic radii, ionization enthalpy.
Electron gain enthalpy, valence, oxidation states and chemical reactivity.
|12.||General Principles and Process of Isolation of Metals|
Modes of occurrence of elements in nature, minerals, ores.
Steps involved in the extraction of metals: concentration, reduction (chemical and electrolytic methods) and refining with special reference to the extraction of Al, Cu, Zn, and Fe.
Thermodynamic and electrochemical principles involved in the extraction of metals.
The position of hydrogen in periodic table, isotopes, preparation, properties, and uses of hydrogen.
Physical and chemical properties of water and heavy water.
Structure, preparation, reactions, and uses of hydrogen peroxide.
Classification of hydrides: ionic, covalent and interstitial.
Hydrogen as a fuel.
|14.||S Block Elements (Alkali and Alkaline Earth Metals)|
Group 1 and Group 2 Elements: General introduction, electronic configuration and general trends in physical and chemical properties of elements, anomalous properties of the first element of each group, diagonal relationships.
Preparation and properties of some important compounds: sodium carbonate, sodium chloride, sodium hydroxide and sodium hydrogen carbonate.
Industrial uses of lime, limestone, Plaster of Paris and cement.
The biological significance of Na, K, Mg and Ca.
|15.||P Block Elements|
Group 13 to Group 18 Elements: General Introduction, Electronic configuration, and general trends in physical and chemical properties of elements across the periods and down the groups; unique behaviour of the first element in each group. Groupwise study of the p block elements.
Group 13: Preparation, properties, and uses of boron and aluminium; Structure, properties and uses of borax, boric acid, diborane, boron trifluoride, aluminium chloride, and alums.
Group 14: Tendency for catenation; Structure, properties, and uses of allotropes and oxides of carbon, silicon tetrachloride, silicates, zeolites, and silicones.
Group 15: Properties and uses of nitrogen and phosphorus; Allotropic forms of phosphorus; Preparation, properties, structure, and uses of ammonia, nitric acid, phosphine and phosphorus halides, (PCl3, PCl5); Structures of oxides and oxoacids of nitrogen and phosphorus.
Group 16: Preparation, properties, structures and uses of dioxygen and ozone; Allotropic forms of sulfur; Preparation, properties, structures, and uses of sulfur dioxide, sulphuric acid (including its industrial preparation); Structures of oxoacids of sulfur.
Group 17: Preparation, properties, and uses of chlorine and hydrochloric acid; Trends in the acidic nature of hydrogen halides; Structures of Interhalogen compounds and oxides and oxyacids of halogens.
Group 18: Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon.
|16.||D and F Block Elements|
Transition Elements: General introduction, electronic configuration, occurrence and characteristics, general trends in properties of the first-row transition elements: physical properties, ionization enthalpy, oxidation states, atomic radii, colour, catalytic behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation.
Preparation, properties, and uses of K2Cr2O7 and KMnO4.
Inner Transition Elements: Lanthanides, Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction, and Actinoids: Electronic configuration and oxidation states.
Introduction to coordination compounds, Werner’s theory.
ligands, coordination number, denticity, chelation.
IUPAC nomenclature of mononuclear coordination compounds, isomerism.
Bonding-Valence bond approach and basic ideas of Crystal field theory, colour and magnetic properties.
Importance of coordination compounds (in qualitative analysis, extraction of metals and in biological systems).
Environmental pollution: Atmospheric, water, and soil.
Atmospheric pollution: Tropospheric and stratospheric.
Gaseous pollutants: Oxides of carbon, nitrogen, and sulfur, hydrocarbons; their sources, harmful effects, and prevention.
Greenhouse effect and Global warming, acid rain.
Particulate pollutants: Smoke, dust, smog, fumes, mist; their sources, harmful effects, and prevention.
Stratospheric pollution: Formation and breakdown of ozone, depletion of ozone layer its mechanism and effects.
Water Pollution: Major pollutants such as pathogens, organic wastes, and chemical pollutants; their harmful effects and prevention.
Soil pollution: Major pollutants such as Pesticides (insecticides, herbicides and fungicides) their harmful effects and prevention.
Strategies to control environmental pollution.
|Section C: Organic Chemistry|
Purification and Characterisation of Organic Compounds
Purification: Crystallization, sublimation, distillation, differential extraction, and chromatography principles and their applications.
Qualitative analysis: Detection of nitrogen, sulfur, phosphorus, and halogens.
Quantitative analysis (basic principles only): Estimation of carbon, hydrogen, nitrogen, halogens, sulfur, phosphorus.
Calculations of empirical formula and molecular formulae; Numerical problems in organic quantitative analysis.
Some Basic Principles of Organic Chemistry
Tetravalency of carbon; Shapes of simple molecules – hybridization (s and p).
Classification of organic compounds based on functional groups: -C = C- and those containing halogens, oxygen, nitrogen, and sulfur; Homologous series.
Isomerism: structural and stereoisomerism.
Nomenclature (Trivial and IUPAC): Covalent bond fission Homolytic and heterolytic: free radicals, carbocations, and carbanions; stability of carbocations and free radicals, electrophiles and nucleophiles.
Electronic displacement in a covalent bond: Inductive effect, electromeric effect, resonance, and hyperconjugation.
Common types of organic reactions: Substitution, addition, elimination, and rearrangement.
Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and reactions.
Alkanes: Conformations; Sawhorse and Newman projections (of ethane); Mechanism of halogenation of alkanes.
Alkenes: Geometrical isomerism.
Mechanism of electrophilic addition: addition of hydrogen, halogens, water, hydrogen halides (Markownikoff’s and peroxide effect); Ozonolysis, oxidation, and polymerization.
Alkynes: Acidic character; Addition of hydrogen, halogens, water and hydrogen halides; Polymerization.
Aromatic hydrocarbons: Nomenclature, benzene structure and aromaticity.
Mechanism of electrophilic substitution: halogenation, nitration, Friedel Crafts alkylation and acylation, directive influence of the functional group in monosubstituted benzene.
Organic Compounds Containing Halogens
General methods of preparation, properties, and reactions.
Nature of C-X bond.
Mechanisms of substitution reactions.
Uses, Environmental effects of chloroform, iodoform, freons, and DDT.
Organic Compounds Containing Oxygen
General methods of preparation, properties, reactions, and uses.
Alcohols: Identification of primary, secondary and tertiary alcohols; mechanism of dehydration.
Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration, and sulphonation, Reimer Tiemann reaction.
Aldehyde and Ketones: Nature of carbonyl group; Nucleophilic addition to >C=O group, relative reactivities of aldehydes and ketones.
Important reactions such as Nucleophilic addition reactions (addition of HCN, NH3 and its derivatives), Grignard reagent; oxidation; reduction (Wolff Kishner and Clemmensen); the acidity of hydrogen, aldol condensation, Cannizzaro reaction, Haloform reaction.
Chemical tests to distinguish between aldehydes and Ketones.
Carboxylic Acids: Acidic strength and factors affecting it.
Organic Compounds Containing Nitrogen
General methods of preparation, properties, reactions, and uses.
Amines: Nomenclature, classification, structure, basic character and identification of primary, secondary and tertiary amines and their basic character.
Diazonium Salts: Importance in synthetic organic chemistry.
General introduction and classification of polymers, general methods of polymerization addition and condensation, co-polymerization.
Natural and synthetic rubber and vulcanization.
Some important polymers with emphasis on their monomers and uses, polyethene, nylon, polyester, and bakelite.
General introduction and importance of biomolecules.
Carbohydrates: Classification: aldoses and ketoses; monosaccharides (glucose and fructose), constituent monosaccharides or oligosaccharides (sucrose, lactose, maltose) and polysaccharides (starch, cellulose, glycogen).
Proteins: Elementary Idea of amino acids, peptide bond, polypeptides; Proteins: primary, secondary, tertiary and quaternary structure (qualitative idea only), denaturation of proteins, enzymes.
Vitamins: Classification and functions.
B Chemical constitution of DNA and RNA. Biological functions of nucleic acids.
Chemistry in Everyday Life
Chemicals in medicines: Analgesics, tranquilizers, antiseptics, disinfectants, antimicrobials, antifertility drugs, antibiotics, antacids, antihistamines their meaning and common examples.
Chemicals in food: Preservatives, artificial sweetening agents common examples.
Cleansing agents: Soaps and detergents, cleansing action.
Principles Related to Practical Chemistry
Detection of extra elements (N, S, halogens) in organic compounds.
Detection of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl and amino groups in organic compounds.
The chemistry involved in the preparation of the following: Inorganic compounds: Mohr’s salt, potash alum, and Organic compounds: Acetanilide, p-nitro acetanilide, aniline yellow, iodoform.
The chemistry involved in the titrimetric exercises: Acids bases and the use of indicators, oxalic-acid vs KMnO4, Mohr’s salt vs KMnO4.
Chemical principles involved in the qualitative salt analysis: Cations: Pb2+, Cu2+, AI3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, NH4+, and Anions: CO32-, S2-, SO42-, NO2-, NO3-, CI-, Br, I. (Insoluble salts excluded).
Chemical principles involved in the following experiments: Enthalpy of solution of CuSO4, Enthalpy of neutralization of strong acid and strong base, Preparation of lyophilic and lyophobic sols, and Kinetic study of the reaction of iodide ion with hydrogen peroxide at room temperature.
Chemistry questions are often well spread out amongst various topics, the topic wise weightage of chemistry questions with respect to number of questions and marks is as follows:
Number of Questions
Transition Elements and Coordination Chemistry
Periodic table and Representative Elements
Thermodynamics And Gaseous State
Chemical And Ionic Equilibrium
Solid State And Surface Chemistry
Nuclear Chemistry And Environment
Solution and Colligative Properties
General Organic Chemistry
Carboxylic Acid and their Derivatives
Carbohydrates,amino acid and Polymers
NTA has provided online video lectures by IIT Faculty and experts for the preparation of JEE Main Chemistry section . The steps to access the video lectures are as follows:
Visit the official website of NTA i.e. nta.ac.in.
Click on the “CONTENT BASED LECTURES - FOR JEE MAIN AND NEET-UG BY IIT PROFESSORS / SUBJECT EXPERTS” tab.
You will be redirected to the page containing the name of different subjects.
Choose the video lecture by clicking on the subject.
Analyzing your approach towards the exam is one of the most important aspects of the preparation. One must constantly check if their strategies for the exam are accurate and how good their hold is on various concepts with the help of mock tests.
NTA provides official mock tests for the assistance of candidates. These official mock tests can be accessed by the mock test from the official website of NTA i.e.nta.ac.in. A total of 18 mock tests have been released on the official website of NTA in which 15 tests are for Paper 1 while 3 are for Paper 2. Mock Tests can be accessed in English, Hindi, and Gujarati language.
Free online mock tests have been launched by BIE Telangana for candidates appearing for JEE Main 2020. It’s a unique platform where Telangana Education Department will be holding daily, weekly and grand mock tests series. For candidates who have android based smartphones, BIE has also launched a smartphone application that can help them take the mock tests conveniently using their phones.Click Here to Register
The level of difficulty of JEE Main Chemistry section varies in different sessions. For the understanding of candidates, a basic distribution of number of questions in terms of difficulty level of B.E/ B. Tech paper of JEE Main 2020 January session is tabulated below:
Although as per the above analysis, chemistry seems to be the toughest section in the January B.E/ B.Tech paper but candidates must keep in mind that level of difficulty is a subjective concern and chemistry still remains one of the most quick in terms of attempting and scoring sections.
It is often advised by experts out of three sections of B.E/ B. Tech paper of JEE Main, chemistry should be attempted first.
Chemistry questions include a major portion of fact based questions. Therefore solving them first will be a quick process. The extra time left can be then utilized for the physics and maths sections which are considered more time consuming.
In chemistry too, It is a good move to start with questions of inorganic chemistry, for example, reading well through chapters like P, S-block and Classification of elements and periodicity in property. Questions from these topics are direct and can be answered through direct application of knowledge of concepts.
Experts suggest that the entire JEE Main Chemistry section should be solved in not more than 40-45 minutes.
The advisable order within the chemistry section of B.E/ B. Tech paper is Inorganic chemistry ( 6- 8 min) followed by Organic chemistry ( 12- 15 min) followed by Physical chemistry ( 15 - 17 min). The 5 numerical value based questions have to be solved in the remaining time out of the total of 40-45 minutes.
Must Read Interviews of JEE Main 2020 Toppers (NTA Score 100)
For physical chemistry practice is the key to success, so books with good questions becomes very important. For theory preparation, read NCERT textbooks and class notes (of school or coaching) only because side books contain additional topics too which are not in the syllabus of any exam. For practicing questions refer books by:
Being the most scoring section, chemistry often turns out to be a major rank uplifter for one’s overall performance in JEE Main. However, chemistry is often proves troublesome in terms of preparation for candidates, here are some tips that can assist the candidates in their preparation for JEE Main Chemistry:
Use limited and accurate resources: Don’t try to cover the syllabus from multiple sources, you must practice from NCERT well. Other than that, you can read different concepts from a few acknowledged sources. Make voice notes or written notes and revise them regularly.
Solve Questions Everyday: Retention is one of the factors resulting in a good attempt in the chemistry section, and retention can only be assured with practice. Candidates should make a habit of solving 40-50 questions on a daily basis. Whether you mix the questions from various topics or handle questions from a specific topic everyday totally depends on you.The way to maximize your score in Chemistry is to ensure a balance between analytical skills and memorization skills.
Identify answers through approximations: It is not wise to test your mathematics skills while solving the chemistry questions. You must remember that the time is limited and solve accordingly. Candidates can get an approximate answer and pick the option closest to it, unless the options are really close to each other.
Practice with previous year papers and mock tests: Practicing is the most essential component of your preparation as per all the experts. Practice and analyze your performance constantly to know the productivity of your current plan.
Invest your time wisely: The importance of time management in the chemistry paper is of utmost importance, candidates can save time in direct questions and invest the same in questions that will take longer in terms of attemption.
While NCERT textbooks of class XI and XII are considered the best source of preparation for JEE Main Chemistry Section as many direct questions are asked form these texts, here is a list of some other books that can be of help to candidates:
Concept of Physical Chemistry for JEE Main & Advanced
Solomons and Fryhle
Morrison and Boyd
Arihant's Practice Book Chemistry for JEE Main And Advanced
J D Lee
Concise Inorganic Chemistry
Freedman and Young
Elementary problems in Organic Chemistry
Physical Chemistry; Organic Chemistry
Modern Approach to Chemical Calculations
*The article might have information for the previous academic years, which will be updated soon subject to the notification issued by the University/College