Chemistry XI Syllabus CBSE Board


Unit I: Some Basic Concepts of Chemistry

  1. General Introduction: Importance and scope of Chemistry.
    Nature of matter, laws of chemical combination, Dalton's atomic theory: concept of elements, atoms and molecules.

Unit II: Structure of Atom

  1. 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 III: Classification of Elements and Periodicity in Properties

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

Unit IV: Chemical Bonding and Molecular Structure


Unit V: States of Matter: Gases and Liquids

  1. 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. Deviation from ideal behaviour, liquefaction of gases, critical temperature, kinetic energy and molecular speeds (elementary idea), Liquid State- vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations).

Unit VI: Chemical Thermodynamics

    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 VII: Equilibrium

  1. 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 VIII: Redox Reactions


Unit IX: Hydrogen

  1. 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 X: s-Block Elements (Alkali and Alkaline Earth Metals)

  1. Group 1 and Group 2 Elements

Unit XI: Some p-Block Elements 14 Periods General Introduction to p -Block Elements

  1. 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.

Unit XII: Organic Chemistry -Some Basic Principles and Techniques


Unit XIII: Hydrocarbons 12 Periods Classification of Hydrocarbons

  1. 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.
  2. 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 XIV: Environmental Chemistry

  1. 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 should be conducted alongside the concepts taught in theory classes

  1. Basic Laboratory Techniques
    • Cutting glass tube and glass rod.
    • Bending a glass tube.
    • Dilute Ethanoic Acid solution
    • Drawing out a glass jet.
    • Boring a cork.
  2. 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.
  3. Experiments based on pH
    • Any one of the following experiments:
      • Comparing the pH of solutions of strong and weak acids of same concentration.
      • Study the pH change in the titration of a strong base using universal indicator.
  4. Chemical Equilibrium
    • One of the following experiments:
  5. Quantitative Estimation
    • Using a mechanical balance/electronic balance.
    • Preparation of standard solution of Oxalic acid.
    • Determination of strength of a given solution of Sodium hydroxide by titrating it against standard solution of Oxalic acid.
    • Preparation of standard solution of Sodium carbonate.
    • Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonate solution.
  6. Qualitative Analysis
    • 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).
    • Detection of -Nitrogen, Sulphur, Chlorine in organic compounds.
  7. Projects
      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.

