CBSE Class 11 chemistry syllabus & Recommended books

    cbse class 11 chemistry syllabus
    cbse class 11 chemistry syllabus

    Hi Friends, today we are going to discuss you about CBSE class 11 Chemistry syllabus with all the best books recommended to score great in the particular subject.This updated syllabus for CBSE class 11 Chemistry, focuses on reducing the curriculum load while ensuring that ample opportunities and scope for learning within its framework.

    As you know very well that Central Board of Secondary Education (CBSE) has its own curriculum and syllabus designed for the students and they hold the supreme authority to change it further for the benefit of students. So it is always a wise decision to keep an eye on what happening around with the subject you are going to learn. This year CBSE made little bit changes in class 11 Chemistry syllabus.

    Chemistry Books for class 11th 

    For Chemistry of class XI, one can opt from the list of books listed below.

    • NCERT Chemistry for class 11 (NCERT Publication)
    • Pradeep Chemistry
    • Numerical Chemistry by P. Bahadur
    • Arihant Organic Chemistry (Arihant Publications)
    • Organic Chemistry by O.P. Tandon
    • Inorganic Chemistry by O.P. Tandon
    • Modern approach to chemical calculations by R.C. Mukherjee

    Overview of CBSE Class 11 Chemistry Syllabus, Chapter wise Chemistry syllabus for class 11, Class XI Chemistry syllabus for session 2016-2017.

    CBSE class 11 Chemistry syllabus chapter details in brief

    Now Let us have a brief look at the salient features asked in CBSE class 11 Chemistry syllabus. 


    THEORY: Theory paper for class 11 Chemistry, will be of 70 marks and will consist of following topics.

    Unit Title Periods Marks
    1. Some Basic Concepts of Chemistry





    2. Structure of Atom 14
    3. Classification of Elements and Periodicity in Properties 08 04
    4. Chemical Bonding and Molecular Structure 14  



    5. States of Matter: Gases and Liquids 12
    6. Chemical Thermodynamics 16
    7. Equilibrium 14
    8. Redox Reactions O6  



    9. Hydrogen 08
    10. S-Block Elements 10
    11. Some p -Block Elements 14
    12. Organic Chemistry: Some basic Principles and Techniques 14  


    13. Hydrocarbons 12
    14. Environmental Chemistry O6
                                           Total 160 70

    Unit l: 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 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, the concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship.
    • Heisenberg uncertainty principle, the 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, the stability of half filled and completely filled orbitals.

    Unit 3: Classification of Elements and Periodicity in Properties

    • The significance of classification, a 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, valency. 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 a covalent bond, the covalent character of an ionic bond.
    • Valence bond theory, resonance, the geometry of covalent molecules, VSEPR theory, the 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: States of Matter: Gases and Liquids

    • Three states of matter, intermolecular interactions, types of bonding, melting and boiling points, the role of gas laws in elucidating the concept of the molecule.
    • Boyle’s law, Charles; law, Gay Lussac’s law, Avogadro’s law, ideal behavior, empirical derivation of gas equation, Avogadro’s number, ideal gas equation.
    • Deviation from ideal behavior, liquefaction of gasses, critical temperature, kinetic energy and molecular speeds (elementary idea), Liquid State- vapor pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations)

    Unit-6: 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 AU and AH, 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)
    • The introduction of entropy as a state function, Gibb’s energy change for spontaneous and nonspontaneous processes, criteria for equilibrium.
    • Third law of thermodynamics (brief introduction).

    unit-7: Equilibrium

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

    unit-8: Redox Reactions

    • The 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-9: Hydrogen

    • The position of hydrogen in periodic table, occurrence, isotopes, preparation, properties, and uses of hydrogen.
    • Hydrides-ionic, covalent and interstitial; physical and chemical properties of water, heavy water, hydrogen peroxide -preparation, reactions and structure and use; hydrogen as a fuel.

    unit-10: S-Block Elements (Alkali and Alkaline Earth Metals)

    (i) 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 nd halogens, use.

    (ii) Preparation and Properties of Some important Compounds:

    • Sodium Carbonate, Sodium Chloride, Sodium Hydroxide and Sodium Hydrogencarbonate, the Biological importance of Sodium and Potassium.
    • Calcium Oxide and Calcium Carbonate and their industrial uses, biological importance of Magnesium and Calcium.

    Unit- 11: Some p -Block Elements

    Group 13 Elements: General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous properties of first element of the group, Boron – physical and chemical properties, some important compounds, Borax, Boric acid, Boron Hydrides, Aluminium: Reactions with acids and alkalies, uses.

    Group 14 Elements: General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, the anomalous behavior of first elements. Carbon-catenation, allotropic forms, physical and chemical properties; uses of some important compounds: oxides. Important compounds of Silicon and a few uses: Silicon Tetrachloride, Silicones, Silicates and Zeolites, their uses.

    unit-12: Organic Chemistry-Some Basic Principles and Technique

    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-13: Hydrocarbons

    Classification of Hydrocarbons

    (i) 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 (Markownikov’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.

    (ii) 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.

    Unit-14: Environmental Chemistry 

    Environmental pollution – air, water and soil pollution, chemical reactions in atmosphere, smog, major atmospheric pollutants, acid rain, ozone and its reactions, effects of depletion of ozone layer, greenhouse effect and global warming pollution due to industrial wastes, green chemistry as an alternative tool for reducing pollution, strategies for control of environmental pollution.

    Practical syllabus for class 11 Chemistry

    Practical syllabus for class 11 Chemistry will be of 30 marks and consist of following listed events.

    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

    List of Experiments for CBSE Class 11 Chemistry 

    These are the Experiments designed for CBSE Class 11 Chemistry.

    • Basic Laboratory Techniques
    • Cutting glass tube and glass rod
    • Bending a glass tube
    • Drawing out a glass jet
    • Boring a cork
    • Characterization and Purification of Chemical Substances
    • Determination of 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.
    • Experiments based on pH
    • Determination of one anion and one cation in a given salt
    • Detection of -Nitrogen, Sulphur, Chlorine in organic compounds.
    • Investigation of the foaming capacity of different washing soaps and the effect of the addition of Sodium Carbonate on it.
    • Determination of the rate of evaporation of different liquids.
    • Study the effect of acids and bases on the tensile strength of fibers.


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