NCERT Solutions and Notes for CBSE Class 11 Chemistry

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CBSE Class 11 Chemistry Syllabus

The Central Board of Secondary Education (CBSE) has released new CBSE Class 11 Chemistry Syllabus 2020-21 (Revised & Reduced By 30%). With this article, you can view  CBSE Class 11 Chemistry Syllabus.  

CBSE Class 11 Chemistry Syllabus 2020 – 21

Latest CBSE Class 11 Chemistry Syllabus 2020-21 (Revised & Reduced By 30%) is available here for view. . New CBSE Class 11 Chemistry Syllabus contains complete details about course structure (Theory and Practicals), design of question paper, prescribed textbook.

CBSE Class 11 Chemistry Syllabus 2020-21 (Revised & Reduced By 30%)

Unit No.


No. of Periods


Unit I

Some Basic Concepts of Chemistry



Unit II

Structure of Atom


Unit III

Classification of Elements and Periodicity in Properties



Unit IV

Chemical Bonding and Molecular Structure



Unit V

States of Matter: Gases and Liquids


Unit VI

Chemical Thermodynamics


Unit VII




Redox Reactions



Unit IX



Unit X

s ‐Block Elements


Unit XI

Some p ‐Block Elements


Unit XII

Organic Chemistry: Some basic Principles and Techniques










Unit I: Some Basic Concepts of Chemistry (10Periods)


General Introduction: Importance and scope of Chemistry.

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 (12 Periods)

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 (06 Periods)

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, valency. Nomenclature of elements with atomic number greater than 100.

Unit IV: Chemical Bonding and Molecular Structure (14Periods)

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 V: States of Matter: Gases And Liquids (9 Periods)

Three states of matter, intermolecular interactions, types of bonding, melting and boiling points, role of gas laws in elucidating the concept of the molecule, Boyle’s law, Charles law, Gay Lussac’s law, Avogadro’s law, ideal behaviour, empirical derivation of gas equation, Avogadro’s number, ideal gas equation and deviation from ideal behavior.

Unit VI: Chemical Thermodynamics (14 Periods)

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, 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.

Third law of thermodynamics (brief introduction).

Unit VII:  Equilibrium (12 Periods)

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, buffer solution, solubility product, common ion effect (with illustrative examples).

Unit VIII: Redox Reactions (04Periods)

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.

Unit IX: Hydrogen (04 Periods)

Position of hydrogen in periodic table, occurrence, isotopes, hydrides‐ionic covalent and interstitial; physical and chemical properties of water, heavy water, hydrogen as a fuel.

Unit X: s‐Block Elements (Alkali and AlkalineEarth Metals)  5 Period

Group 1 and Group 2 Elements

General introduction, electronic configuration, occurrence, anomalous properties of the first element of each group, diagonal relationship, trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii), trends in chemical reactivity with oxygen, water, hydrogen and halogens, uses.

Unit XI: Some p‐Block Elements (9 Periods)

General Introduction to p ‐Block Elements

Group  13  Elements:  General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous properties of the first element of the group, Boron ‐ physical and chemical properties.

Group  14  Elements:  General introduction, electronic configuration, occurrence, variation of properties,  oxidation  states,  trends  in  chemical  reactivity,  anomalous  behaviour  of  first elements. Carbon‐catenation, allotropic forms, physical and chemical properties.

Unit XII: Organic Chemistry ‐ Some Basic Principles and Techniques (10 Periods)

General introduction, classification andIUPACnomenclatureoforganiccompounds.Electronicdisplacementsinacovalentbond: 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 (10 Periods)

Classification of Hydrocarbons

Aliphatic Hydrocarbons:

Alkanes ‐ Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions.

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 monosubstituted benzene. Carcinogenicity and toxicity.

CBSE Class 11 Chemistry Syllabus 2020-21:

Evaluation Scheme for Examination


Volumetric Analysis


Salt Analysis


Content Based Experiment


Project Work


Class record and viva




PRACTICAL SYLLABUS (Total Periods: 60) 

Micro-chemical methods are available for several of the practical experiments, wherever possible such techniques should be used.

A. Basic Laboratory Techniques

1. Cutting glass tube and glass rod

2. Bending a glass tube

3. Drawing out a glassjet

4. Boring a cork

B. Characterization and Purification of ChemicalSubstances

1. Determination of melting point of an organic compound.

2. Determination of boiling point of an organic compound.

3. Crystallization of impure samples of any one of the following: Alum, Copper Sulphate, BenzoicAcid.

C. Quantitative Estimation 

i. Using a mechanical balance/electronic balance. 

ii. Preparation of standard solution of Oxalic acid. 

iii. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard solution of Oxalic acid. 

iv. Preparation of standard solution of Sodium carbonate. 

v. Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonate solution. 

D. Qualitative Analysis 

a) Determination of one anion and one cation in a given salt 

Cations- Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+ 

Anions – (CO3)2- , S2-, NO2- , SO32-, SO2-4, NO3- , Cl- , Br-, I-, PO43- , C2O2-4, CH3COO- (Note: Insoluble salts excluded) 

b) Detection of -Nitrogen, Sulphur, Chlorine in organic compounds. 


Scientific investigations involving laboratory testing and collecting information from other sources.

A few suggested Projects 

  • Checking the bacterial contamination in drinking water by testing sulphide 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 presence of these ions above permissible limit (if any). 

  • Investigation of the foaming capacity of different washing soaps and the effect of 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. 

Note: Any other investigatory project, which involves about 10 periods of work, can be chosen with the approval of the teacher.

Prescribed Books: 

  1. Chemistry Part – I, Class-XI, Published by NCERT. 
  2. Chemistry Part – II, Class-XI, Published by NCERT.
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