একাদশ শ্রেণির রসায়ন সিলেবাস ও প্রশ্ন বিন্যাস 2024-2025 | WBCHSE 11 Chemistry Syllabus & Question Pattern 2024-2025

2024-2025 শিক্ষাবর্ষ থেকে একাদশ শ্রেণির রসায়ন (Chemistry) নতুন সিলেবাস চালু হয়েছে। একাদশ শ্রেণির পরীক্ষা দুটি সেমিস্টারে হবে। 

সেমিস্টার অনুযায়ী রসায়ন সিলেবাস, প্রশ্নের ধরণ এবং প্রশ্ন বিন্যাস নিচে দেওয়া হয়েছে। 

একাদশ শ্রেণির রসায়ন সিলেবাস ও প্রশ্ন বিন্যাস 2024-2025 (WBCHSE 11 Chemistry Syllabus & Question Pattern 2024-2025)

রসায়ন (Chemistry – CHEM)

সেমিস্টার – I

পূর্ণমান – 35

সেমিস্টার – I : একাদশ শ্রেণির রসায়ন (থিয়োরি) প্রশ্ন বিন্যাস 2024-2025 (WBCHSE 11 Chemistry Question Pattern 2024-2025)

সেমিস্টার – I : একাদশ শ্রেণির রসায়ন (থিয়োরি) সিলেবাস 2024-2025 (WBCHSE 11 Chemistry Syllabus 2024-2025)

• Unit-1 : Some Basic Concepts of Chemistry (03 Marks, 07 Hours) : Laws of chemical combination. Concept of elements, atoms and molecules. Atomic and molecular masses. Mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry and calculations based on stoichiometry. Different concentration terms of solutions and related calculations.
• Unit-2 : Structure of Atom (06 Marks, 12 Hours) : Bohr’s model and its limitations, concept of shell and sub-shells, the dual nature of matter and light, de Broglie’s relationship. Heisenberg uncertainty principle, Schrödinger wave equation (elementary idea only). Concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals: Aufbau principle, Pauli exclusion principle and Hund’s rule, exchange energy, electronic configuration of atoms, stability of half-filled, completely filled orbitals.
• Unit-3 : Classification of Elements and Periodicity in Properties (04 Marks, 07 Hours) : Modern periodic law and the present form of the periodic table, periodic trends in properties of elements – atomic radii, ionic radii, van der Waals’ radii, ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic number greater than 100.
• Unit-4 : Chemical Bonding and Molecular Structure (06 Marks, 13 Hours) : Valence electrons, ionic bond, bond parameters, covalent bond, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules, VSEPR theory, concept of hybridisation, involving s, p and d orbitals and shapes of some simple molecules, intermolecular interactions, Hydrogen bonding, Molecular orbital theory of homonuclear diatomic molecules (H₂, He₂, O₂, N₂, F₂ – qualitative idea only)
• Unit-5 : States of Matter – Solids and Gases (04 Marks, 09 Hours) :
  • Classification of solids (elementary idea): molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea), unit cell in two-dimensional and three-dimensional lattices, packing efficiency, calculation of density of unit cell, packing in solids, voids, number of atoms per unit cell in a cubic unit cell, point defects. 
  • Kinetic theory of gas, molecular speeds, Dalton’s law of partial pressure, Graham’s law, deviation of ideal behaviour and van der Waals’ equation, Liquefaction of gases, critical temperature.
• Unit-6 : s-Block Elements (Group 1 and Group 2 elements) (05 Marks, 10 Hours) : Electronic configuration, occurrence, trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii), trends in chemical reactivity with oxygen, water, hydrogen and halogens, hydrides (ionic, covalent and interstitial), hydrogen peroxide (preparation, properties, structure & use), hydrogen as a fuel. Biological importance of Na, K, Mg, Ca.
• Unit-7 : p-Block Elements (Group 13 and Group 14 elements) (07 Marks, 12 Hours) : General introduction to p-block elements, electronic configuration, occurrence, variation in properties, oxidation states, and trends in chemical reactivity of group 13 and 14 elements.
  • Group 13: Boron: physical and chemical properties of compounds of Boron: Boron oxides, boric acid, borates and B₂H₆ ; Aluminium: Reactions of Al with acid and alkali, uses of Al, Preparation and uses of LiAlH₄ and Al₂O₃.
  • Group 14: Carbon: catenation, allotropic forms, nano carbon, graphene, physical and chemical properties of two oxides of carbon – CO and CO₂, Silicon: some compounds of silicon and their important uses – Silicon tetrachloride (Structure, preparation, hydrolysis and reduction reaction only), silicates [structure of open chain silicates constructing of (SiO₂)₂^2n- ions], use of zeolites,

সেমিস্টার – II

পূর্ণমান – 65

সেমিস্টার – II : একাদশ শ্রেণির রসায়ন (থিয়োরি) প্রশ্ন বিন্যাস 2024-2025 (WBCHSE 11 Chemistry Question Pattern 2024-2025)

সেমিস্টার – II : একাদশ শ্রেণির রসায়ন (থিয়োরি) সিলেবাস 2024-2025 (WBCHSE 11 Chemistry Syllabus 2024-2025)

• Unit-1 : Thermodynamics (07 Marks, 12 Hours) : Concepts of system (including types of system), surroundings. Work, heat, energy, extensive and intensive properties, state function, Zeroth law of thermodynamics and definition of temperature. The first law of thermodynamics – internal energy change (ΔU) and enthalpy change (ΔH), Enthalpy of bond dissociation, combustion, formation, atomization, ionization, solution and sublimation. Transformation of state. Hess’s law of constant heat summation, Born Haber Cycle and its application. 2nd law of thermodynamics, the introduction of entropy as a state function, Gibbs energy change for spontaneous and non-spontaneous processes, criteria for equilibrium.
• Unit-2 : Equilibrium (06 Marks, 10 Hours) : Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass reaction, equilibrium constant, factors affecting equilibrium – Le Chatelier’s principle; ionic equilibrium, ionization of acids and bases, strong and weak electrolytes, degree of ionization of polybasic acids, acid strength, concept of pH Henderson Equation. Hydrolysis of salts (elementary idea). Buffer solutions, solubility product, common ion effect (with illustrative examples).
• Unit-3 : Redox Reactions (03 Marks, 05 Hours) : Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions in terms of loss and gain of electrons and change in oxidation number, applications of redox reactions in permanganometry and dichromatometry
• Unit-4 : Organic Chemistry: Some basic principles (07 Marks, 12 Hours) : General introduction, classification and IUPAC nomenclature of organic compounds. Electronic displacements in a covalent bond: inductive effect, resonance and hyperconjugation. Homolytic and Heterolytic fission of a covalent bond: free radicals, carbocations, carbanions electrophiles and nucleophiles, types of organic reactions. Elementary idea of addition, elimination and substitution reactions.
• Unit-5 : Hydrocarbons: Classification of hydrocarbons (08 Marks, 14 Hours) :
  • Alkanes – Nomenclature, isomerism, conformations (ethane only), physical properties (up to 6 carbons) and chemical reactions including halogenations, free radical mechanism, combustion and pyrolysis.
  • Alkenes – Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties (up to 3 carbons) methods of preparation; chemical reactions; addition of hydrogen, halogen, water hydrogen halides (Markovnikov’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition.
  • Alkynes – Nomenclature, structure of triple bond (ethyne), physical properties (up to 3 carbons) preparation, chemical reactions; acidic character of Alkynes, addition reaction of – hydrogen, halogens, hydrogen halides and water.
  • Aromatic hydrocarbons – Introduction, IUPAC nomenclature; Benzene; resonance aromaticity; chemical properties; mechanism of electrophilic substitution – nitration, sulphonation, halogenations, Friedel-Crafts alkylation and acylation, carcinogenicity and toxicity.
• Unit-6 : Environmental Chemistry (04 Marks, 07 Hours) : Environmental pollution – air, water and soil pollution (cause and effects), Primary and secondary pollutants (solid and liquid), chemical reactions in the atmosphere, smog, pollution due to industrial wastes; solid waste management (elementary idea only), SPM, RSPM, green chemistry as an alternative tool for reducing pollution. Water preservation and protection, Strategy for control of environmental pollution.

সেমিস্টার – II : ব্যবহারিক (Practical) সিলেবাস 

• A. Basic Laboratory Techniques
  • i. Cutting glass tube and glass rod
  • ii. Bending a glass tube
  • iii. Drawing out a glass jet
  • iv. Boring a cork
• B. Characterization and purification of chemical substances
  • i. Determination of the melting point of an organic compound
  • ii. Determination of the boiling point of an organic compound
  • iii. Crystallization of impure sample of any of the following: Alum, Copper, Sulphate, Benzoic acid.
• C. Environment-related experiments
  • i. Calculation of pH of soil sample.
  • ii. Determination of turbidity for a given sample of water
  • iii. Determination of dissolved oxygen in a given sample of water
  • iv. Determination of TDS of water sample
• D. Quantitative estimation (Use of digital balance (precession up to 3 decimal points)) (Volumetric analysis)
  • i. Determination of strength of a given sodium hydroxide solution by titrating it against a standard oxalic acid solution.
  • ii. Determination of strength of a given hydrochloric acid solution by titrating it against standard sodium carbonate solution.
  • iii. Standardisation of KMnO₄ solution by using standard Oxalic acid solution.
  • iv. Estimation of Fe in Mohr’s salt solution using standard KMnO₄ solution or standard K₂Cr₂O₇ solution.

Project Work

• a) Preparation of standard solutions:
  • i) Preparation of (N/10) Oxalic acid solution.
  • ii) Preparation of (N/10) Mohr’s salt solution.
  • iii) Preparation of (N/10) Sodium carbonate solution.
  • iv) Preparation of (N/10) Hydrochloric acid solution.
  • v) Preparation of (N/10) Sodium hydroxide solution.
• b) Preparation of inorganic compounds:
  • i) Preparation of potash alum.
  • ii) Preparation of potassium ferric oxalate.
• c) Study of acidity of
  • i) Different samples of tea leaves.
  • ii) Fruit and vegetable juices.