CBSE Class 11 Chemistry Syllabus 2024-25

Table of Contents

CBSE Class 11 Chemistry Syllabus: The newly released Central Board of Secondary Education (CBSE) Class 11 Chemistry syllabus is now available. Published on the official website, students can access and download their complete chemistry syllabus and curriculum here. Alongside course content, practical details, and evaluation scheme are provided. The downloadable link is sourced directly from the official website, ensuring reliability. Dive into the complete article to discover more, brought to you by Infinity Learn.

Class 11 Chemistry Syllabus 2024-25

The table below contains a unit-by-unit Class 11 Chemistry Syllabus for students in grade 11. Students can refer to the table for more information on the CBSE Class 11 Chemistry Syllabus.

Also Check: CBSE Syllabus for Class 1 to 12

Unit	Topic	Sub-Topic
I	Some Basic Concepts of Chemistry	Chemistry’s significance and scope. – Nature of matter, chemical laws, and Dalton’s atomic theory: elements, atoms, and molecules. – Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formulas, chemical reactions, stoichiometry, and calculations based on stoichiometry.
II	Structure of Atom	– Discoveries of the electron, proton, and neutron, as well as the atomic number, isotopes, and isobars. – The limitations of Thomson’s model. – 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.
III	Classification of Elements and Periodicity in Properties	– Importance of classification, a brief history of periodic table development, modern periodic law and the current form of the periodic table, periodic trends in element properties -atomic radii, ionic radii, inert gas radii, ionization enthalpy, electron gain enthalpy, electronegativity, and valency. – The classification of elements with atomic numbers greater than 100.
IV	Chemical Bonding and Molecular Structure	– Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, 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.
V	Chemical Thermodynamics	– Concepts of systems and types of systems, surroundings, work, heat, energy, extensive and intensive properties, and state functions. – First law of thermodynamics – internal energy and enthalpy, measurement of U and H, 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 to entropy as a state function and Gibb’s energy change for spontaneous and nonspontaneous processes. – Third law of thermodynamics (brief introduction).
VI	Equilibrium	– Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, equilibrium constant, and 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 (an elementary idea), buffer solution, Henderson Equation, solubility product, common ion effect (with illustrative examples).
VII	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.
VIII	Organic Chemistry: Some basic Principles and Techniques	Organic compound introduction, classification, and IUPAC nomenclature. – Covalent bond electronic displacements: inductive effect, electromeric effect, resonance, and hyperconjugation. – Covalent bond homolytic and heterolytic fission: free radicals, carbocations, carbanions, electrophiles and nucleophiles, organic reactions.
IX	Hydrocarbons	– Hydrocarbon categorization – Hydrocarbons of the aliphatic type: – Alkanes – Nomenclature, isomerism, conformation (ethane only), physical properties, and chemical reactions. – Alkenes – Nomenclature, double bond structure (ethene), geometrical isomerism, physical properties, methods of preparation, chemical reactions: hydrogen, halogen, water, hydrogen halides (Markovnikov’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition. – Nomenclature of alkynes, triple bond structure (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, and functional group influence on monosubstituted benzene. Carcinogenesis and toxicity.

CBSE Class 11 Chemistry Syllabus and Practical Syllabus 2024-25

The practicals are an essential component of science education. The CBSE has included some practicals in the curriculum to provide students with hands-on experience. The following are some of the CBSE Class 11 Chemistry Syllabus experiments:

Category	Experiment	Details
A. Basic Laboratory Techniques	1. Cutting glass tubes and glass rods	– Description of the process for cutting glass tubes and rods.
	2. Bending a glass tube	– Procedure for bending a glass tube.
	3. Drawing out a glass jet	– Steps for drawing out a glass jet.
	4. Boring a cork	– Explanation of how to bore a cork.
B. Characterization and Purification of Chemical Substances	1. Determination of the melting point of an organic compound.	– Experimental details for determining the melting point of an organic compound.
	2. Determination of the boiling point of an organic compound.	– Procedure for determining the boiling point of an organic compound.
	3. Crystallization of an impure sample (choose one): a. Alum b. Copper Sulfate c. Benzoic Acid	– Steps for the crystallization of the chosen impure sample.
C. Experiments based on pH	1. Determination of pH (choose one): a. Solutions obtained from fruit juices, acids, bases, and salts using pH paper or a universal indicator. b. Comparing the pH of solutions of strong and weak acids of the same concentration. c. Study the pH change in the titration of a strong base using a universal indicator.	– Detailed procedure for the chosen experiment.
	2. Study the pH change by common ion in the case of weak acids and weak bases.	– Experimental steps for studying the pH change with common-ion.
D. Chemical Equilibrium	1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions. OR 2. Study the shift in equilibrium between [Co(H2O)6] 2+ and chloride ions by changing the concentration of either of the ions.	– Detailed procedure for the selected chemical equilibrium experiment.
E. Quantitative Estimation	i. Using a mechanical balance/electronic balance.	– Explanation of using a mechanical or electronic balance.
	ii. preparation of a standard solution of oxalic acid.	– Step-by-step process for preparing a standard solution of oxalic acid.
	iii. determination of the strength of a given solution of sodium hydroxide by titrating it against a standard solution of oxalic acid.	– Procedure for determining the strength of sodium hydroxide.
	iv. preparation of a standard solution of sodium carbonate.	– Detailed steps for preparing a standard solution of sodium carbonate.
	v. determination of the strength of a given solution of hydrochloric acid by titrating it against a standard sodium carbonate solution.	– Experimental details for determining the strength of hydrochloric acid.
F. Qualitative Analysis	1. Determination of one cation and one anion in a given salt (choose one): a. Cations: Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+ b. Anions: (CO3)2-, S2-, NO2-, SO32-, SO2-, NO-, Cl-, Br-, I-, PO43-, C2O2-, CH3COO-	– Steps for the qualitative analysis of the chosen cation and anion in a salt.
	2. detection of nitrogen, sulfur, and chlorine in organic compounds.	– Procedure for detecting nitrogen, sulfur, and chlorine in organic compounds.