CBSE Class 11 Chemistry Syllabus 2024-25 PDF | Download Latest Curriculum

CBSE Class 11 Chemistry Syllabus 2024-25

The Central Board of Secondary Education has released the updated CBSE Class 11 Chemistry Syllabus 2024-25. Students appearing for their Class 11 annual exams should review this detailed curriculum to streamline their study plan. The syllabus provides a comprehensive overview of the course structure, highlighting all chapters and essential topics for the academic session. By aligning your preparation with the official syllabus, you can manage your time effectively and focus on high-weightage topics to maximize your scores. Explore this page for complete details on the Class 11 Chemistry curriculum for the 2024-25 academic year.

Chemistry Class 11 Syllabus 2024-25

The Chemistry Class 11 curriculum for 2024-25 is categorized into theory and practical assessments, carrying 70 and 30 marks, respectively. We have provided a detailed marks distribution for each chapter, acting as a blueprint for the annual examination structure. Review the table below to understand the scoring breakdown of the CBSE Class 11 Chemistry Syllabus 2024-25 and prioritize your revision accordingly.

Chemistry Class 11 Syllabus 2024-25
S.No.	Unit	Marks
1.	Some Basic Concepts of Chemistry	7
2.	Structure of Atom	9
3.	Classification of Elements and Periodicity in Properties	6
4.	Chemical Bonding and Molecular Structure	7
5.	Chemical Thermodynamics	9
6.	Equilibrium	7
7.	Redox Reactions	4
8.	Organic Chemistry: Some Basic Principles and Techniques	11
9.	Hydrocarbons	10
Total Marks		70

CBSE 11th Chemistry Syllabus 2024-25 (Chapter-wise)

The CBSE 11th Chemistry Syllabus 2024-25 is strategically designed to build a strong foundational knowledge, ensuring a smoother transition to the Class 12 curriculum. We have listed the chapter-wise details below alongside an official PDF download link. Students are encouraged to familiarize themselves with every topic outlined in the CBSE Class 11 Chemistry Syllabus 2024-25 to ensure thorough exam preparation.

Unit I: Some Basic Concepts of Chemistry

• General Introduction: Importance and scope of Chemistry.
• Nature of matter, laws of chemical combination,
• Dalton's atomic theory: the 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.

Unit II: Structure of Atom 

• Discovery of Electron, Proton, Neutron, atomic number, isotopes, and isobars.
• Thomson's model and its limitations.
• Rutherford's model and its limitations,
• Bohr's model and its limitations,
• Concept of shells and subshells,
• Dual nature of matter and light, de Broglie's relationship,
• Heisenberg uncertainty principle,
• Concept of orbitals, quantum numbers, shapes of s, p, and d orbitals,
• Rules for filling electrons in orbitals - Aufbau principle, Pauli's exclusion principle, and Hund's rule,
• Electronic configuration of atoms, stability of half-filled and completely filled orbitals.

Unit III: Classification of Elements and Periodicity in Properties 

• Significance of classification, a brief history of the development of the periodic table, modern periodic law, and the present form of the periodic table,
• Periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency.
• Nomenclature of elements with atomic number greater than 100.

Unit IV: Chemical Bonding and Molecular Structure 

• Valence electrons, ionic bond, covalent bond, bond parameters,
• Lewis’s structure,
• The polar character of the covalent bond,
• The covalent character of ionic bond,
• Valence bond theory,
• Resonance,
• The geometry of covalent molecules,
• VSEPR theory,
• Concept of hybridization involving s, p, and d orbitals, and shapes of some simple molecules,
• Molecular orbital theory of homonuclear diatomic molecules (qualitative idea only),
• Hydrogen bond.

Unit VI: Chemical Thermodynamics 

• Concepts of Systems and types of systems, surroundings, work, heat, energy, extensive and intensive properties, and state functions.
• The first law of thermodynamics -internal energy and enthalpy, heat capacity and specific heat, measurement of ΔU and ΔH, Hess's law of constant heat summation,
• Enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution, and dilution.
• Second law of Thermodynamics (brief introduction) Introduction of entropy as a state function,
• Gibb's energy change for spontaneous and non-spontaneous processes, criteria for equilibrium.
• Third law of thermodynamics (brief introduction).

Unit VII: Equilibrium

• Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, the equilibrium constant, Factors affecting equilibrium - Le Chatelier's principle,
• Ionic equilibrium- ionization of acids and bases,
• Strong and weak electrolytes, degree of ionization,
• Ionization of polybasic acids, acid strength, the concept of pH, hydrolysis of salts (elementary idea), buffer solution,
• Henderson Equation, solubility product, common ion effect (with illustrative examples).

Unit VIII: Redox Reactions 

• 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.

Unit XII: Organic Chemistry - Some Basic Principles and Techniques 

• General introduction,
• Methods of purification,
• Qualitative and quantitative analysis,
• Classification and IUPAC nomenclature of organic compounds.
• Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance, and hyperconjugation.
• Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.

Unit XIII: Hydrocarbons 

Classification of Hydrocarbons

Aliphatic Hydrocarbons:

• Alkanes - Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions including free radical mechanism of halogenation, combustion, and pyrolysis.
• Alkenes - Nomenclature, the structure of double bond (ethene), geometrical isomerism, physical properties, 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, the structure of triple bond (ethyne), physical properties, methods of 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,
• Halogenation,
• Friedel Craft's alkylation and acylation,
• Directive influence of the functional group in monosubstituted benzene.
• Carcinogenicity and toxicity.

CBSE Class 11 Chemistry Syllabus 2024-25 for Practical

The practical assessment accounts for 30 marks, covering experimental activity and a viva-voce. The CBSE Class 11 Chemistry practical syllabus includes Volumetric Analysis (8 marks), Salt Analysis (8 marks), Content-Based Experiments (6 marks), Project Work (4 marks), and Lab Record/Viva (4 marks).

Class 11th Chemistry Practical Evaluation Scheme
Evaluation Scheme for Examination	Marks
Volumetric Analysis	08
Salt Analysis	08
Content-Based Experiment	06
Project Work	04
Class record and viva	04
Total	30

Experiments

A. Basic Laboratory Techniques 

• Cutting glass tube and glass rod
• Bending a glass tube
• Drawing out a glass jet
• Boring a cork

B. Characterization and Purification of Chemical Substances 

• Determination of the melting point of an organic compound.
• Determination of boiling point of an organic compound.
• Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.

C. Experiments based on pH 

1. Any one of the following experiments:

• Determination of pH of some solutions obtained from fruit juices, solutions of known and varied concentrations of acids, bases, and salts using pH paper or universal indicator.
• Comparing the pH of solutions of strong and weak acids of the same concentration. Study the pH change in the titration of a strong base using a universal indicator.

    2. Study the pH change by common-ion in case of weak acids and weak bases. 

D. Chemical Equilibrium: Select one of the following experiments: 

• Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions.
• Study the shift in equilibrium between [Co(H2O)6] 2+ and chloride ions by changing the concentration of either of the ions.

E. Quantitative Estimation 

• Using a mechanical balance/electronic balance.
• Preparation of standard solution of Oxalic acid.
• Determination of strength of a given solution of Sodium hydroxide by titrating it against a standard solution of Oxalic acid. Preparation of standard solution of Sodium carbonate.
• Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonate solution.

F. Qualitative Analysis 

• Determination of one anion and one cation in a given salt Cation: Pb2+, Cu2+ As3+, Aℓ3+, Fe3+, Mn2+, Zn2+, Ni2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4 + Anions: (CO3) 2- , S2- , (SO3) 2- , (NO2) - , (SO4) 2- , Cℓ- , Br- , I- , (PO4) 3- , (C2O4) 2- , CH3COO-, NO3 - (Note: Insoluble salts excluded)
• Detection of -Nitrogen, Sulphur, and Chlorine in organic compounds.

G. PROJECTS 

• Scientific investigations involve laboratory testing and collecting information from other sources.

A few suggested Projects: 

• Checking the bacterial contamination in drinking water by testing sulfide ion
• Study of the methods of purification of water
• Testing the hardness, presence of Iron, Fluoride, Chloride, etc., depending upon the regional variation in drinking water, and study of causes of the presence of these ions above the permissible limit (if any).
• Investigation of the foaming capacity of different washing soaps and the effect of the addition of Sodium carbonate on it
• Study the acidity of different samples of tea leaves.
• Determination of the rate of evaporation of different liquids.
• Study the effect of acids and bases on the tensile strength of fibers.
• Study of acidity of fruit and vegetable juices.