In the latest Chemistry Class 11 CBSE Syllabus 2020-21 (revised and reduced to 30%), has been cut by 30% due to Covid-19 so that all students don’t face any difficulty in studying and preparing for the exam. we will tell you about all those things that have been given in Chemistry Class 11 CBSE.
Chemistry Class 11 CBSE Syllabus 2020-21 (Revised & Reduced By 30% Due To Covid-19)
| Unit No. | Title | No. of Periods | Marks |
| Unit I | Some Basic Concepts of Chemistry | 10 | 11 |
| Unit II | Structure of Atom | 12 | |
| Unit III | Classification of Elements and Periodicity in Properties | 6 | 04 |
| Unit IV | Chemical Bonding and Molecular Structure | 14 | 21 |
| Unit V | States of Matter: Gases and Liquids | 9 | |
| Unit VI | Chemical Thermodynamics | 14 | |
| Unit VII | Equilibrium | 12 | |
| Unit VIII | Redox Reactions | 4 | 16 |
| Unit IX | Hydrogen | 4 | |
| Unit X | s ‐Block Elements | 5 | |
| Unit XI | Some p ‐Block Elements | 9 | |
| Unit XII | Organic Chemistry: Some basic Principles and Techniques | 10 | 18 |
| Unit XIII | Hydrocarbons | 10 | |
| Total | 119 | 70 |
General Introduction: Importance and scope of Chemistry subject.
Atomic and molecular masses, percentage composition, empirical and molecular formula, mole concept and molar mass, chemical reactions, stoichiometry, and calculations based on stoichiometry.
Unit II: Structure of Atom (12 Periods)
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, forms of s, p and d orbitals, rules for filling electrons in orbitals ‐ Aufbau system, Pauli’s exclusion principle and Hund’s rule, electronic configuration of atoms, stability of half-filled and filled orbitals.
Unit III: Classification of Elements and Periodicity in Properties (6 Periods)
Modern periodic law and the present form of the periodic table, periodic trends in properties of ingredients ‐atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic amounts higher than 100.
Unit IV: Chemical Bonding and molecule structure (4 Periods)
Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, the polar nature of the covalent bond, covalent nature of ionic bond, valence bond theory, resonance, the geometry of covalent fragments, VSEPR theory, the concept of hybridization, including s, p and d orbitals, and shapes of some simple units, molecular orbital theory of homonuclear diatomic bits(qualitative idea only), Hydrogen bond.
Unit V: States of Matter: Gases And Liquids (09 Periods)
Three states of matter, intermolecular synergies, kinds of bonding, melting and boiling periods, the role of gas laws in elucidating the concept of the unit, Boyle’s law, Charles law, Gay Lussac’s law, Avogadro’s law, ideal behavior, practical source of the gas equation, Avogadro’s number, ideal gas equation and deviation from ideal behavior.
Unit VI: Chemical Thermodynamics (14 Periods)
Concepts of Systems and types of systems, surroundings, work, heat, power, extensive and intensive resources, state functions.
The first law of thermodynamics ‐internal energy and enthalpy, measurement of ΔU and ΔH, Hess’s law of even heat summation, enthalpy of bond dissociation, fire, formation, atomization, sublimation, phase transition, ionization, solution, and dilution. The second law of Thermodynamics (brief introduction)
Introduction of entropy as a state party, Gibb’s energy change for spontaneous and non‐spontaneous processes.
3rd law of thermodynamics (brief introduction).
Unit VII: Equilibrium (12 Periods)
Equilibrium in physical and chemical methods, dynamic nature of equilibrium, the law of mass action, equilibrium constant, parts affecting equilibrium ‐ Le Chatelier’s principle, ionic equilibrium‐ ionization of acids and principles, strong and weak electrolytes, degree of ionization, ionization of polybasic acids, acid strength, the concept of pH, buffer solution, solubility product, natural ion effect (with illustrative examples).
Unit VIII: Redox Reactions (04Periods)
Concept of oxidation and loss, redox reactions, oxidation number, balancing redox reactions, in terms of loss and increase of electrons, and change in oxidation number.
Unit IX: Hydrogen (04 Periods)
The rank of hydrogen in the periodical table, occurrence, isotopes, hydrides‐ionic covalent and interstitial; physical and biochemical properties of water, heavy liquid, hydrogen as a fuel.
Unit X: s‐Block Elements (Alkali and AlkalineEarth Metals) (5 Period)
Group 1 and Group 2 Elements
General introduction, electronic arrangement, occurrence, anomalous properties of the first element of each group, oblique relationship, trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii), bearings 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 meeting, electronic configuration, appearance, variation of properties, oxidation states, courses in chemical reactivity, anomalous properties of the first part of the group, Boron ‐ physical and chemical properties.
Group 14 Elements: General introduction, electronic arrangement, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous behavior of first components. Carbon‐catenation, allotropic forms, physical and biochemical properties.
Unit XII: Organic Chemistry ‐ Some Basic Principles and Techniques (10 Periods)
General introduction, classification, and IUPAC nomenclature of organic compounds.Electronic displacements in a covalent bond: inductive effect, electromeric effect, noise, and hyperconjugation. Homolytic and heterolytic cleavage of a covalent bond: free radicals, carbocations, carbanions, electrophiles, and nucleophiles, examples of organic reactions.
Unit XIII: Hydrocarbons (10 Periods)
Classification of Hydrocarbons
Aliphatic Hydrocarbons:
Alkanes ‐ Nomenclature, conformation (ethane only), physical properties, isomerism, chemical reactions.
Alkenes ‐ Nomenclature, strthe ucture of double bond (ethene), geometrical isomerism, physical properties, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides, methods of preparation, (Markovnikov’s addition and peroxide effect), ozonolysis, mechanism of electrophilic addition, oxidation.
Alkynes ‐ the structure of triple bond (ethyne), Nomenclature, physical properties, methods of construction, chemical reactions: acidic character of alkynes, increasing reaction of ‐ hydrogen, halogens, hydrogen halides, and water.
Aromatic Hydrocarbons:
Introduction, IUPAC classification, benzene: resonance, aromaticity, chemical features: mechanism of electrophilic exchange. Nitration, sulphonation, halogenation, Friedel Craft’s alkylation, and acylation, directive leadership of the functional group in monosubstituted benzene. Carcinogenicity and toxicity.
CBSE Class 11 Chemistry Syllabus 2020-21:
| 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 |
PRACTICAL SYLLABUS (Total Periods: 60)
Micro-chemical methods are ready for several of the practical experiments, wherever feasible 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 ChemicalSubstances
1. Determination of melting limit of an organic compound.
2. Determination of boiling limit of an organic synthesis.
3. Crystallization of impure samples of any 1 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 negotiated solution of Sodium hydroxide by titrating it upon a standard solution of Oxalic acid.
iv. Preparation of regular solution of Sodium carbonate.
v. Determination of strength of a given resolution of hydrochloric acid by titrating it against conventional Sodium Carbonate solution.
D. Qualitative Analysis
a) Determination of one anion and one cation in a collapsed salt
Cations- Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Co2+, Ca2+, Zn2+, Sr2+, Ba2+, Mg2+, NH4+
Anions – (CO3)2- , S2-, NO2- , SO32-, SO2-4, NO3- , Br-, Cl- , I-, PO43- , CH3COO-,C2O2-4 (Note: Insoluble salts excluded)
b) Detection of -Nitrogen, Sulphur, Chlorine in natural aggregates.
c) PROJECTS
Scientific investigations involving scullery testing and collecting information from other sources.
A few suggested Projects
- Checking the bacterial infection in drinking water by testing sulfide ion
- Study of the methods of cleaning of water
- Investigation of the foaming ability of different washing soaps and the effect of interest of Sodium carbonate on it
- Study the acidity of various samples of tea leaves.
- Determination of the rate of escape of different liquids
- Study the effect of acids and bases on the tensile force of fibers.
- Study of acidity of fruit and green juices.
Note: Any other investigatory project, which includes about 10 periods of work, can be chosen with the support of the teacher.