CBSE Class 11 Chemistry Syllabus 2025-26: Download PDF, Topics & Marking Scheme

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

70

Unit

Topics covered

Unit 1: Some Basic Concepts of Chemistry

General Introduction: Importance and scope of Chemistry, Nature of matter, laws of chemical combination, Dalton's atomic theory: 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 2: Structure of Atom

Discovery of Electron, Proton and 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 3: Classification of Elements and Periodicity in Properties

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

Unit 4: 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.

Unit 5: Chemical Thermodynamics

Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions. First law of thermodynamics -internal energy and enthalpy, heat capacity and specific heat, 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 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 6: Equilibrium

Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, 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 poly basic acids, acid strength, concept of pH, hydrolysis of salts (elementary idea), buffer solution, Henderson Equation, solubility product, common ion effect (with illustrative examples).

Unit 7: 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 8: 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, electrometric effect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.

Unit 9: Hydrocarbons

Aliphatic Hydrocarbons Alkanes - Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions including free radical mechanism of halogenation, combustion and pyrolysis. Alkenes - Nomenclature, 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, 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 functional group in mono-substituted benzene, carcinogenicity and toxicity

Section

Content

A. Basic Laboratory Techniques

1. Cutting glass tube and a glass rod

2. Bending a glass tube

3. Drawing out a glass jet

4. Boring a cork

B. Characterisation and Purification of Chemical Substances

1. Determination of the melting point of an organic compound

2. Determination of the boiling point of an organic compound

3. Crystallisation of an impure sample (choose one): Alum, Copper Sulphate, Benzoic Acid

C. Experiments Based on pH

1. Any one experiment:

– Determination of pH of solutions from fruit juices or known concentrations using pH paper/universal indicator

– Comparing the pH of strong and weak acids of the same concentration

– pH change in the titration of a strong base with universal indicator

2. Study pH change by common-ion effect in weak acids and bases

D. Chemical Equilibrium

Perform one of the following:

– Study the equilibrium shift between ferric and thiocyanate ions with varying concentrations

– Study equilibrium shift between [Co(H₂O)₆]²⁺ and chloride ions by altering ion concentrations

E. Quantitative Estimation

1. Use of mechanical/electronic balance

2. Preparation of a standard solution of Oxalic acid

3. Titration: NaOH solution vs. standard Oxalic acid

4. Preparation of standard Sodium Carbonate solution

5. Titration: HCl solution vs. standard Sodium Carbonate

F. Qualitative Analysis

1. Identification of one cation and one anion in a salt sample:

Cations: Pb²⁺, Cu²⁺, Al³⁺, Fe³⁺, Mn²⁺, Ni²⁺, Zn²⁺, Co²⁺, Ca²⁺, Sr²⁺, Ba²⁺, Mg²⁺, NH₄⁺

Anions: CO₃²⁻, S²⁻, SO₃²⁻, NO₃⁻, NO₂⁻, Cl⁻, Br⁻, I⁻, SO₄²⁻, PO₄³⁻, CH₃COO⁻

(Insoluble salts excluded)

2. Detection of Nitrogen, Sulphur, and Chlorine in organic compounds