WBJEE 2025 Apply Online, Eligibility, Exam Dates

WBJEE 2025 Information Bulletin has been released: WBJEE 2025 Information Bulletin has been Announced by WBJEE. As per the Official Brochure, the WBJEE exam will be held on April 27, 2025 in two Shifts. Paper-1 Mathematics Exam will be Conducted During First Session i.e., from 11 AM to 1PM and Paper-2 Subjects ( Physics & Chemistry) Exam Will be Organized during Second Half of the Day i.e., from 2PM to 4PM. Aspiring candidates are requested to go through the Board’s website at (www.wbjeeb.nic.in/ www.wbjeeb.in) from time to time for detailed information.

পশ্চিমবঙ্গের বিভিন্ন বিশ্ববিদ্যালয় ও কলেজে ইঞ্জিনিয়ারিং, টেকনোলজি, ফার্মাসি ও আর্কিটেকচার কোর্সে ভর্তি হওয়ার পরীক্ষা (WBJEE -২০২৫) আগামী ২৭ শে এপ্রিল, ২০২৫ (রবিবার) অনুষ্ঠিত হবে। বিশদ বিবরণের জন্য ছাত্রছাত্রীদের নিয়মিতভাবে বোর্ডের ওয়েবসাইট (www.wbjeeb.nic.in/ www.wbjeeb.in) দেখতে অনুরোধ করা হচ্ছে

• Information Bulletin WBJEE 2025
• Press Release WBJEE 2025

WBJEEB will conduct OMR based Common Entrance Examination (WBJEE-2025) for admission into Undergraduate Courses in Engineering & Technology, Pharmacy and Architecture of different Universities, Government Colleges as well as Self Financing Engineering & Technological Institutes in the State of West Bengal for the academic session 2025-26.

WBJEE Introduction

West Bengal Joint Entrance Examinations Board (WBJEEB) conducts the West Bengal Joint Entrance Examination (WBJEE) as a state-level exam Every Year. WBJEE – Common Entrance Test for admission to UG Courses in Engineering/Technology, Pharmacy and Architecture courses in various universities, government, Private and self-financing engineering Colleges in the State of West Bengal. The Exam will be conducted through OFFLINE mode for those candidates who completed their XII Class (10+2) Exam in the state.

WBJEE 2025 Exam Date & Time

WBJEEB will conduct OMR based Common Entrance Examination (WBJEE-2025) for admission in the academic session 2025-25 for Undergraduate Courses in Engineering/Technology, Pharmacy and Architecture courses of different Universities, Government Colleges as well as Self-Financing Engineering/Technological Institutes in the State of West Bengal.

The test will be held once a year and there shall be no further examination under any circumstances for those who cannot appear on the date and time mentioned above.

Overview of WBJEE 2025

Eligibility Criteria for WBJEE 2025

Please note that candidates appearing for 12^th board examination in 2025 are also eligible to appear for WBJEE 2025 but they must pass the qualifying exam with the required score as mentioned above before Counselling Date.

WBJEE 2025 Age Limit

• A candidate must be at least 17 years of age (as on December 31, 2020) to appear for the exam. This means an aspirant should have been born on or before December 31, 2003. There is no upper age limit for appearing in the WBJEE 2025.
• However, for admission to the Marine Engineering Course, the lower age limit is 17 years as on December 31, 2025 and the upper age limit is 25 years as on December 31, 2020.

Application Fee for WBJEE 2025

WBJEE 2025 Exam Centers

The exam is conducted in 23 districts of West Bengal and Silchar (Assam) and Agartala (Tripura).

How to Apply for WBJEE 2025

• Step 1 – Registration: Firstly, the candidates will have to register by entering their name, date of birth, gender, parent’s name, identity proof details and more. A password also has to be generated by the candidates.

• Step 2 – Filling of Application Form: After registration, the candidates will have to fill their personal, academic and category details.

• Step 3 – Uploading of Scanned Documents: Next, the candidates will have to upload their photograph and signature as per the specifications mentioned by the authorities.

• Step 4 – Fee Payment: The required fee has to be paid by the candidates through online mode i.e., net banking/credit card/debit card.

• Step 5 – Print Out Confirmation Page: The generated confirmation page has to be downloaded and printed out for future use.

Exam Pattern of WBJEE 2025

All questions will be Multiple-Choice Questions (MCQ), with four options against each question. There will be three categories of questions in each subject. The number of questions, as well as the maximum marks for each, are given in the following table:

There will be 2 papers in WBJEE- Paper 1 (Mathematics) and Paper 2 (Physics and Chemistry). The questions will be based on the syllabus in a Multiple Choice Questions (MCQ) pattern with 4 options against each question.

• Mode of Exam: Offline (OMR Pattern)
• Total Marks: 200 Marks (100+100)
• Types of Questions: Multiple Choice Questions (MCQs)
• Total Number of Questions: 155
• Answering Mode: Darkening the appropriate circle in black/blue ballpoint pen only.

• Mark the answers using only blue or black ballpoint pen in OMR sheet.
• ¼ of the marks allotted to a question will be deducted as penalty for marking the wrong answer.
• No negative marking on category 3.

WBJEE 2025 Syllabus

Mathematics

 Physics

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; Gramequivalent 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, Rutherford’s model and its limitations; Extra nuclear 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 mono – atomic 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 andexamples), 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:

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- dimensional lattices, 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 withtemperature. 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. Hesss 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 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, nylon polyesters, 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 ofenvironment 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.

Haloalkanes 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.

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

Haloalkanes 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:

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 commonantiseptics, 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. Namesof essential elements in biological system.

Principles of Qualitative Analysis:

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

Acid Radicals: Cl- , S2-, SO4 2- , NO3 – , CO3 2- . 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.

Download WBJEE 2025 Detailed Syllabus

WBJEE 2025 Admit Card

WBJEE Admit Card will be Available at least 10 Days prior to the Exam Date.

WBJEE 2025 Result / Rank List

There will be two rank lists for WBJEE 2019 will be as prepared by board. They are

General Merit Rank List (GMR):

For aggregate marks scored in both papers. The students who have appeared in both papers of WBJEE and have qualified the exam as per the cut off marks will be eligible for admissions to engineering & technology/architecture courses and also for pharmacy courses offered at Jadavpur University. Moreover, the GMR list will also mention reserved category a candidate belongs to against his/her rank.
This will be Prepared as per following rules
The following methods will be used candidates who appeared for paper 1 and paper 2

• Less negative marks in Mathematics, Physics and Chemistry took together
• More positive marks in Mathematics and Physics took together
• More positive marks in Mathematics and Chemistry took together
• Less negative marks in Mathematics and Physics took together
• Less negative marks in Mathematics and Chemistry took together
• More positive marks in Mathematics for only the 2 marks questions
• More positive marks in Physics for only the 2 marks questions
• More positive marks in Chemistry for only the 2 marks questions
• Less negative marks in Mathematics for only the 2 marks questions
• Less negative marks in Physics for only the 2 marks questions

Pharmacy Merit Rank List (PMR):

The rank list of WBJEE 2019 will be based only on the marks of paper 2 candidates. The candidates who appeared for paper 2 of WBJEE 2019 and qualified for the exam as per the minimum cut off marks will be ranked in descending order of their ranks. The candidates ranking in the list will be eligible for admission in pharmacy courses of Universities and Pharmacy Institutes except at Jadavpur University.
This will be Prepared as per following rules

• Less negative marks in Physics & Chemistry
• More positive marks in Chemistry
• Less negative marks in Chemistry
• More positive marks in Chemistry for only the 2 marks questions
• Less negative marks in Chemistry for only the 2 marks questions
• More positive marks in Physics for only the 2 marks questions
• Less negative marks in Physics for only the 2 marks questions

Note: In case, if the tie still exists then the date of birth will be taken into consideration to break the tie in ranks and candidates older in age will be given preference.