CBSE Syllabus

CBSE Syllabus for Class 11 Chemistry

CBSE Syllabus for Class 11 Chemistry

Biology is a subject in which one topic is related to the other topic, so it is important that students should study the topics according to the syllabus provide by NCERT. Here we have categorised all the chapters in a separate unit, which is given in the table below.

NCERT syllabus for class 11 Chemistry is important for the students of class 12th, as it gives a brief knowledge about the topics of biology.

Chemistry is one of the vital subjects in Science stream and it is also of very much importance while preparing for various competitive exams and hence it is essential to prepare it from the very beginning. Understanding the concepts and applying them in the provided situation can improvise your learning as well as knowledge ability.

Chemistry is a very important resource for students of CBSE Class 11.Chemistry is an interesting subject for the enhancement of analytical and problem solving skills.

Unfortunately, many students find it difficult because of no interest or lack of better knowledge to comprehend.  Chemistry is really a difficult subject but very interesting when comprehended well and practice with easy to hard problems and students find it difficult because most of them do not have their basics clear for the subject. Lack of sufficient practice tool is a major reason why solving Mathematical problems seems a tough nut to crack.

School Connect Online students are not only solving and understanding questions from Chemistry from NCERT or Syllabus but also they are solving questions to practice Chemistry Olympiad this helps students to become expert

To help you with this, we have learning notes and videos, Practice questions for  NCERT, NEET, with Solutions for Class 11 Chemistry.

Below is the CBSE class 11 Chemistry Syllabus. It is very important to understand the syllabus before you start preparing for the exam.

NCERT Syllabus for Class 11 Chemistry



Some Basic Concepts of Chemistry

  1. Importance of Chemistry
  2. Nature of Matter
  3. Properties of Matter and their Measurement
  4. Uncertainty in Measurement
  5. Laws of Chemical Combinations
  6. Dalton’s Atomic Theory
  7. Atomic and Molecular Masses
  8. Mole Concept and Molar Masses
  9. Percentage Composition
  10. Stoichiometry and Stoichiometric Calculations

Structure of Atom

  1. Discovery of Subatomic Particles
  2. Atomic Models
  3. Developments Leading to the Bohr’s Model of Atom
  4. Bohr’s Model for Hydrogen Atom
  5. Towards Quantum Mechanical Model of the Atom
  6. Quantum Mechanical Model of Atom

Classification of Elements and Periodicity in Properties

  1. Why do we Need to Classify Elements ?
  2. Genesis of Periodic Classification
  3. Modern Periodic Law and the present form of the Periodic Table
  4. Nomenclature of Elements with Atomic Numbers > 100
  5. Electronic Configurations of Elements and the Periodic Table
  6. Electronic Configurations and Types of Elements: s-, p-, d-, f- Blocks
  7. Periodic Trends in Properties of Elements

Chemical Bonding and Molecular Structure

  1. Kössel-Lewis Approach to Chemical Bonding
  2. Ionic or Electrovalent Bond
  3. Bond Parameters
  4. The Valence Shell Electron Pair Repulsion (VSEPR) Theory
  5. Valence Bond Theory
  6. Hybridisation
  7. Molecular Orbital Theory
  8. Bonding in Some Homonuclear Diatomic Molecules
  9. Hydrogen Bonding

States of Matter

  1. Intermolecular Forces
  2. Thermal Energy
  3. Intermolecular Forces vs Thermal Interactions
  4. The Gaseous State
  5. The Gas Laws
  6. Ideal Gas Equation
  7. Kinetic Energy and Molecular Speeds
  8. Kinetic Molecular Theory of Gases
  9. Behaviour of Real Gases: Deviation from Ideal Gas Behaviour
  10. Liquefaction of Gases
  11. Liquid State


  1. Thermodynamic Terms
  2. Applications
  3. Measurement of ?U and ?H: Calorimetry
  4. Enthalpy Change, ?rH of a Reaction – Reaction Enthalpy
  5. Enthalpies for Different Types of Reactions
  6. Spontaneity
  7. Gibbs Energy Change and Equilibrium


  1. Equilibrium in physical process
  2. Equilibrium in chemical process
  3. Law of chemical equilibrium and equilibrium constant
  4. Homogeneous equilibria
  5. Heterogeneous equilibria
  6. Applications of Equilibrium Constants
  7. Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G
  8. Factors Affecting Equilibria
  9. Ionic Equilibrium in Solution
  10. Acids, Bases and Salts
  11. Ionization of Acids and Bases
  12. Buffer Solutions
  13. Solubility Equilibria of Sparingly Soluble Salts


Class 11 Chemistry Practical Marking Scheme

Evaluation Scheme for Examination


Volumetric Analysis


Salt Analysis


Content Based Experiment


Project Work


Class record and viva





Chemistry Practical Syllabus

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 glass jet
  4. Boring a cork

B. Characterization and Purification of Chemical Substances

  1. Determination of melting point of an organic compound.
  2. Determination of boiling point of an organic compound.
  3. 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:
  2. Determination of pH of some solutions obtained from fruit juices, solution of known and varied concentrations of acids, bases and salts using pH paper or universal indicator.
  3. Comparing the pH of solutions of strong and weak acids of same concentration.
  4. Study the pH change in the titration of a strong base using universal indicator.
  5. Study the pH change by common-ion in case of weak acids and weak bases.

D. Chemical Equilibrium

  1. One of the following experiments:
  2. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions.
  3. 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

  1. Using a chemical balance.
  2. Preparation of standard solution of Oxalic acid.
  3. Determination of strength of a given solution of Sodium Hydroxide by titrating it against standard solution of Oxalic acid.
  4. Preparation of standard solution of Sodium Carbonate.
  5. Determination of strength of a given solution of Hydrochloric acid by titrating it against standard
  6. Sodium Carbonate solution.

F. Qualitative Analysis

  1. Determination of one anion and one cation in a given salt Cations- Pb2+, Cu2+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+,Ba2+, Mg2+, [NH4]+

Anions – [CO3]2-, S2-, [SO3]2-, [SO4]2-, [NO3], Cl,Br, I, [PO4]3-, [C2O4]2-, CH3COO

(Note: Insoluble salts excluded)

  1. Detection of -Nitrogen, Sulphur, Chlorine in organic compounds.

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