WBJEE 2021 Chemistry Syllabus – Download PDF Here

WBJEE 2021 Chemistry Syllabus – Chemistry Syllabus for WBJEE 2021 has been released for West Bengal Joint Entrance Examination. Interested candidates can get the WBJEE Chemistry syllabus from this page or they can also check it from the official website, wbjeeb.nic.in. Chemistry section is in paper 2 of WBJEE 2021. There are 40 questions of 50 marks. Which includes 30, 5, 5 questions respectively of category 1, 2, 3. West Bengal Joint Entrance Examination (WBJEE) is a state-level entrance examination conducted for admission into Engineering & Technology, Pharmacy and Architecture courses. Check the complete WBJEE 2021 Chemistry Syllabus, from this page.

WBJEE 2021 Chemistry Syllabus

Click here for Complete WBJEE 2021 Syllabus.

Candidates can check the topics wise syllabus related to the Chemistry subjects for WBJEE 2021 exam. Candidates go through the details topics and make better strategies for the entrance exam.

Chemistry

Atoms, Molecules and Chemical Arithmetic

Dalton’s atomic theory; Gay Lussac’s law of gaseous volume; Avogadro’s Hypothesis and its applications. Atomic mass; Molecular mass; Equivalent weight; Valency; Gram atomic weight; Gram molecular weight; Gram equivalent weight and mole concept; Chemical formulae; Balanced chemical equations; Calculations (based on mole concept) involving common oxidation-reduction, neutralization, and displacement reactions; Concentration in terms of mole fraction, molarity, molality and normality. Percentage composition, empirical formula and molecular formula; Numerical problems

Atomic Structure

Concept of Nuclear Atom – electron, proton and neutron (charge and mass), atomic number. utherford’s model and its limitations; Extranuclear structure; Line spectra of hydrogen atom. Quantization of energy (Planck’s equation E = hν); Bohr’s model of hydrogen atom and its limitations, Sommerfeld’s modifications (elementary idea); The four quantum numbers, ground state electronic configurations of many-electron atoms and monoatomic ions; The Aufbau Principle; Pauli’s Exclusion Principle and Hund’s Rule. Dual nature of matter and light, de Broglie’s relationship, Uncertainty principle; The concept of atomic orbitals, shapes of s, p and d orbitals (pictorial approach).

Radioactivity and Nuclear Chemistry

Radioactivity α-, β-, γ rays and their properties; Artificial transmutation; Rate of radioactive decay, decay constant, half-life and average age life period of radio-elements; Units of radioactivity; Numerical problems. Stability of the atomic nucleus – effect of neutron-proton (n/p) ratio on the modes of decay, group displacement law, radioisotopes and their uses (C, P, Co and I as examples) isobars and isotones (definition and examples), elementary idea of nuclear fission and fusion reactions.

The Periodic Table and Chemical Families

Modern periodic law (based on atomic number); Modern periodic table based on electronic configurations, groups (Gr. 1-18) and periods. Types of elements – representative (s-block and p- block), transition (d-block) elements and inner transition (f-block/lanthanides and actinides) and their general characteristics. Periodic trends in physical and chemical properties – atomic radii, valency, ionization energy, electron affinity, electronegativity, metallic character, acidic and basic characters of oxides and hydrides of the representative elements (up to Z = 36). Position of hydrogen and the noble gases in the periodic table; Diagonal relationships

Chemical Bonding and Molecular Structure

Valence electrons, the Octet rule, electrovalent, covalent and coordinate covalent bonds with examples; Properties of electrovalent and covalent compounds. Limitations of Octet rule (examples); Fajans Rule.Directionality of covalent bonds, shapes of poly – atomic molecules (examples); Concept of hybridization of atomic orbitals (qualitative pictorial approach): sp, sp2 , sp3 and dsp2 . Molecular orbital energy diagrams for homonuclear diatomic species – bond order and magnetic properties. Valence Shell Electron Pair Repulsion (VSEPR) concept (elementary idea) – shapes of molecules. Concept of resonance (elementary idea), resonance structures (examples). Elementary idea about electronegativity, bond polarity and dipole moment, inter- and intra-molecular hydrogen bonding and its effects on physical properties (mp, bp and solubility); Hydrogen bridge bonds in diborane.

Coordination Compounds

Introduction, Double salts and complex salts, coordination compounds (examples only), Werner’s theory,coordination number (examples of coordination number 4 and 6 only), colour, magnetic properties and shapes, IUPAC nomenclature of mononuclear coordination compounds.

Solid State, Liquid State, Gaseous State

Solid State:

Classification of solids based on different binding forces: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea). Unit cell in two dimensional and three dimensionallattices, calculation of density of unit cell, packing in solids, packing efficiency, voids, number of atoms per unit cell in a cubic unit cell, point defects, electrical and magnetic properties. Band theory of metals, conductors, semiconductors and insulators and n & p type semiconductors

Liquid State:

Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations).

Gaseous State:

Measurable properties of gases. Boyle’s Law and Charles Law, absolute scale of temperature, kinetic theory of gases, ideal gas equation – average, root mean square and most probable velocities and their relationship with temperature. Daltons Law of partial pressure, Grahams Law of gaseous diffusion. Deviations from ideal behavior. Liquefaction of gases, real gases, van der Waals equation; Numerical problems.

Chemical Energetics and Chemical Dynamics

Chemical Energetics – Conservation of energy principle, energy changes in physical and chemical transformations. First law of thermodynamics; Internal energy, work and heat, pressure-volume work; Enthalpy. Internal energy change (ΔE) and Enthalpy change (ΔH) in a chemical reaction. Hess’s Law and its applications (Numerical problems). Heat of reaction, fusion and apourization; Second law of thermodynamics; Entropy; Free energy; Criterion of spontaneity. Third law of thermodynamics (brief introduction)

Chemical Equilibria – The Law of mass action, dynamic nature of chemical equilibria. Equilibrium constants, Le Chateliers Principle. Equilibrium constants of gaseous reactions (Kp and Kc) and relation between them(examples). Significance of ΔG and ΔGº.

Chemical Dynamics – Factors affecting the rate of chemical reactions (concentration, pressure, temperature, catalyst), Concept of collision theory. Arrhenius equation and Concept of activation energy.

Order and molecularity (determination excluded); First order reactions, rate constant, half-life (numerical problems), examples of first order and second-order reactions.

Physical Chemistry of Solutions

Colloidal Solutions – Differences from true solutions; Hydrophobic and hydrophilic colloids (examples and uses); Coagulation and peptization of colloids; Dialysis and its applications; Brownian motion; Tyndall effect and its applications; Elementary idea of emulsion, surfactant and micelle.

Electrolytic Solutions – Specific conductance, equivalent conductance, ionic conductance, Kohlrausch’s law, Faraday’s laws of electrolysis, applications. Numerical problems.

Non-electrolytic Solutions – Types of solution, vapour pressure of solutions. Raoult’s Law; Colligative properties – lowering of vapour pressure, elevation of boiling point, depression of freezing point, osmotic pressure and their relationships with molecular mass (without derivations); Numerical problems.

Ionic and Redox Equilibria

Ionic and Redox Equilibria: Ionic equilibria – ionization of weak electrolytes, Ostwald’s dilution law. Ionization constants of weak acids and bases, ionic product of water, the pH – scale, pH of aqueous solutions of acids and bases; Buffer solutions, buffer action and Henderson equation.

Acid-base titrations, acid – base indicators (structures not required). Hydrolysis of salts (elementary idea), solubility product, common ion effect (no numerical problems).

Redox Equilibria: Oxidation – Reduction reactions as electron transfer processes, oxidation numbers, balancing of redox reactions by oxidation number and ion-electron methods. Standard electrode potentials (E°), Electrochemical series, feasibility of a redox reaction. Significance of Gibb’s equation: ΔG° = – nFΔE° (without derivation), no numerical problems. Redox titrations with (examples); Nernst equations (Numerical problems).

Hydrogen

Position of hydrogen in periodic table, occurrence, isotopes, preparation, properties and uses of hydrogen, hydrides-ionic covalent and interstitial; physical and chemical properties of water, heavy water, hydrogen peroxide – preparation, reactions and structure and use; hydrogen as a fuel.

Chemistry of Non-Metallic Elements and Their Compounds

Carbon – occurrence, isotopes, allotropes (graphite, diamond, fullerene); CO and CO2 production, properties and uses. Nitrogen and Phosphorus – occurrence, isotopes, allotopes, isolation from natural sources and purification, reactivity of the free elements. Preparation, properties, reactions of NH3, PH3, NO, NO2, HNO2, HNO3, P4O10, H3PO3 and H3PO4.

Oxygen and Sulphur – Occurrence, isotopes, allotropic forms, isolation from natural sources and purification, properties and reactions of the free elements. Water, unusual properties of water, heavy water (production and uses). Hydrogen peroxide and ozone (production, purification, properties and uses).

Halogens – comparative study, occurrence, physical states and chemical reactivities of the free elements, peculiarities of fluorine and iodine; Hydracids of halogens (preparation, properties, reactions and uses), inter-halogen compounds (examples); Oxyacids of chlorine.

Chemistry of Metals

General principles of metallurgy – occurrence, concentration of ores, production and purification of metals, mineral wealth of India. Typical metals (Na, Ca, Al, Fe, Cu and Zn) – occurrence, extraction, purification (where applicable), properties and reactions with air, water, acids and non-metals. Manufacture of steels and alloy steel (Bessemer, Open-Hearth and L.D. process).

Principles of chemistry involved in electroplating, anodizing and galvanizing. Preparation and properties of K2Cr2O7 and KMnO4.

Lanthanoids – Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction and its consequences.

Actinoids – Electronic configuration, oxidation states and comparison with lanthanoids.

Chemistry in Industry

Large scale production (including physicochemical principles where applicable, omitting technical details) and uses of Sulphuric acid (contact process), Ammonia (Haber’s process), Nitric acid (Ostwald’s process), sodium bi-carbonate and sodium carbonate (Solvey process).

Polymers

Natural and synthetic polymers, methods of polymerization (addition and condensation), copolymerization, some important polymers – natural and synthetic like polythene, nylonpolyesters, bakelite, rubber. Biodegradable and non-biodegradable polymers.

Surface Chemistry

Adsorption – physisorption and chemisorption, factors affecting adsorption of gases on solids, catalysis, homogenous and heterogenous activity and selectivity; enzyme catalysis colloidal state distinction between true solutions, colloids and suspension; lyophilic , lyophobic multimolecular and macromolecular colloids; properties of colloids; Tyndall effect, Brownian movement, electrophoresis, coagulation, emulsion – types of emulsions.

Environmental Chemistry

Common modes of pollution of air, water and soil. Ozone layer, ozone hole – important chemical reactions in the atmosphere, Smog; major atmospheric pollutants; Green House effect; Global warming pollution due to industrial wastes, green chemistry as an alternative tool for reducing pollution, strategies for control of environment pollution.

Chemistry of Carbon Compounds

Hybridization of carbon: σ – and π – bonds. Isomerism – constitutional and stereoisomerism; Geometrical and optical isomerism of compounds containing upto two asymmetric carbon atoms. IUPAC nomenclature of simple organic compounds – hydrocarbons, mono and bifunctional molecules only (alicyclic and heterocyclic compounds excluded).

Conformations of ethane and n-butane (Newman projection only). Electronic Effects: Inductive, resonance and hyperconjugation. Stability of carbocation, carbanion and free radicals; Rearrangement of carbocation;Electrophiles and nucleophiles, tautomerism in β-dicarbonyl compounds, acidity and basicity of simple organic compounds.

Compounds

Alkanes – Preparation from alkyl halides and carboxylic acids; Reactions — halogenation and combustion.

Alkenes and Alkynes – Preparation from alcohols; Formation of Grignard reagents and their synthetic applications for the preparation of alkanes, alcohols, aldehydes, ketones and acids; SNl and SN2 reactions (preliminary concept). Markownikoff’s and anti-Markownikoff’s additions; Hydroboration;

Oxymercuration-demercuration, reduction of alkenes and alkynes (H2/Lindler catalyst and Na in liquid NH3), metal acetylides.

Haloalkenes and Haloarenes

Haloalkanes – Preparation from alcohols; Nomenclature, nature of C -X bond, physical and chemical properties, mechanism of substitution reactions, optical rotation. Formation of Grignard reagents and their synthetic applications for the preparation of alkanes, alcohols, aldehydes, ketones and acids; SN1 and SN2 reactions (preliminary concept ). Uses and environmental effects of – dichloromethane, trichloromethane, tetrachloromethane, iodoform, freons, DDT.

Alcohols, Ethers and Carboxylic acids

Alcohols: Preparation of alcohols from carbonyl compounds and esters. Reaction – dehydration, oxidation, esterification, reaction with sodium, ZnCl2/HCl, phosphorous halides.

Ethers – Preparation by Williamson’s synthesis; Cleavage with HCl and HI. Aldehydes and Ketones – Preparation from esters, acid chlorides, gem-dihalides, Ca-salt of carboxylic acids. Reaction – Nucleophilic addition with HCN, hydrazine, hydroxyl amines, semi carbazides, alcohols; Aldol condensation, Clemmensen and Wolff – Kishner reduction, haloform, Cannizzaro and Wittig reactions.

Carboxylic Acids – Hydrolysis of esters (mechanism excluded) and cyanides; Hunsdicker and HVZ reactions.

Aliphatic Amines – Preparation from nitro, cyano and amido compounds. Distinction of 1º, 2º and 3º amines (Hinsberg method); Reaction with HNO2; Carbyl amine reaction.

Aromatic Compounds

Benzene – Kekule structure, aromaticity and Hückel rule. Electrophilic substitution – halogenation, sulfonation, nitration, Friedel Crafts reaction, ozonolysis. Directive influence of substituents in monosubstituted benzenes. Carcinogenicity and toxicity.

Amines – Preparation from reduction of nitro compounds; Formation of diazonium salts and their stability; Replacement of diazonium group with H, OH, X (halogen), CN and NO2, diazocoupling and reduction.

Haloarenes – Nature of C -X bond, substitution reactions; Nucleophilic substitution, cine substitution(excluding mechanism, Directive influence of halogen in monosubstituted compounds only).

Phenols – halogenation, sulfonation, nitration, Reimer – Tiemann and Kolbe reactions. Aromatic Aldehydes – Preparation by Gattermann, Gattermann-Koch, Rosenmund and Stephen’s method. Reactions – Perkin, Benzoin and Cannizzaro.

Application Oriented Chemistry

Main ingredients, their chemical natures (structures excluded) and their side effects, if any, of common antiseptics, analgesics, antacids, vitamin-C.

Introduction to Bio-Molecules

Carbohydrates – Pentoses and hexoses. Distinctive chemical reactions of glucose. Aminoacids – glycine,alanine, aspartic acid, cysteine (structures). Zwitterion structures of amino acids, peptide bond.

ADP and ATP – structures and role in bioenergetics; Nucleic acids – DNA and RNA skeleton structures. Names of essential elements in biological system.

Principle of Qualitative Analysis

Detection of water soluble non-interfering Acid and Basic Radicals by dry and wet tests from among:

Acid Radicals: Cl- , S2-, SO42- , NO3– , CO32- . Basic Radicals: Cu2+, Al3+, Fe3+, Fe2+, Zn2+, Ca2+, Mg2+, Na+ , NH4+ .

Detection of special elements (N, Cl, Br, I and S) in organic compounds by chemical tests. Identification of functional groups in: phenols, aromatic amines, aldehydes, ketones and carboxylic acids.

Also Check: WBJEE 2021 Application Form | WBJEE 2021 Admit Card

WBJEE 2021 Exam Pattern

Aspirants must acknowledge the exam pattern for any entrance exam and it can help the candidates can get a better score in the exam. Check the WBJEE 2021 exam pattern given below.

WBJEE 2021 consists of two papers: Paper 1 – Mathematics and Paper 2 – Physics and Chemistry. The candidates have to appear in both of these papers. The duration of each paper is 2 hours. Each paper has multiple-choice questions of 3 categories.

Check the distribution of questions given below.

SectionsCategory I
(Full Marks – 1)
Category II
(Full Marks – 2)
Category III
(Full Marks – 2)
Total no. of questionsTotal marks
Mathematics50151075100
Physics30554050
Chemistry30554050

Marking Scheme

Category of questionsMarking Scheme
Category 1stOnly one option is correct
Each question is of 01 mark
For each incorrect answer, 1/4 marks are deducted
0 marks for unattempted question
Category 2ndOnly one option is correct
Each question is of 2 marks
For each incorrect answer, 1/2 marks are deducted
0 marks for unattempted question
Category 3rdOne or more options can be correct
Correct responses will lead to 02 marks
Any combination of correct and incorrect response will lead to 0 marks
0 marks for un-attempted questions
For partially correct answers, marks will be calculated as:

2 x (No. of correct options marked / total number of correct options)

WBJEE 2021 Mock Test

Candidates can do a self-assessment to participate in the mock test. It helps the candidates to revise the preparation and syllabus for the WBJEE 2021. Ans also get to understand the blueprint of upcoming entrance exam problems. Multiple attempts of the Mock Test improved the quality of knowledge.

You can check the subject-wise links given below.

SectionPractice Here
MathematicsClick Here
PhysicsClick Here
ChemistryClick Here

Best Books to Prepare for WBJEE 2021

Given below are some books that can be referred by the candidates to prepare for WBJEE 2021.

BooksLinks
WB JEE Chapterwise Explorer Engineering – MathematicsBuy Here
WB JEE Engineering Solved Paper 2021Buy Here
WB JEE Chapterwise Explorer Engineering – Physics and ChemistryBuy Here
WB JEE Engineering Solved Paper 2020(Old Edition)Buy Here
NCERT Exemplar Problems-Solutions MATHEMATICS Buy Here
NCERT Exemplar Problems-Solutions PHYSICS class 12thBuy Here
NCERT Exemplar Problems-Solutions CHEMISTRY class 12thBuy Here

Check Out details of WBJEE 2021 Answer Key and WBJEE 2021 Result

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