CBSE Class 11 Chemistry Study Materials All Chapters
Class 11 Chemistry Chapters
- Chapter 1 Some Basic Concepts of Chemistry
- Chapter 2 Structure of The Atom
- Chapter 3 Classification of Elements and Periodicity in Properties
- Chapter 4 Chemical Bonding and Molecular Structure
- Chapter 5 States of Matter
- Chapter 6 Thermodynamics
- Chapter 7 Equilibrium
- Chapter 8 Redox Reactions
- Chapter 9 Hydrogen
- Chapter 10 The sBlock Elements
- Chapter 11 The pBlock Elements
- Chapter 12 Organic Chemistry: Some Basic Principles and Techniques
- Chapter 13 Hydrocarbons
- Chapter 14 Environmental Chemistry
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.
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%)
No. of Periods
Some Basic Concepts of Chemistry
Structure of Atom
Classification of Elements and Periodicity in Properties
Chemical Bonding and Molecular Structure
States of Matter: Gases and Liquids
s ‐Block Elements
Some p ‐Block Elements
Organic Chemistry: Some basic Principles and Techniques
Unit I: Some Basic Concepts of Chemistry (10Periods)
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‐
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
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.
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
Content Based Experiment
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.
- Chemistry Part – I, Class-XI, Published by NCERT.
- Chemistry Part – II, Class-XI, Published by NCERT.