CBSE Chemistry Class 11 Syllabus pdf Download 2021 -2022 : Class 11 is considered to be a vital stage in secondary education. 11th grade is all about laying foundations for topics to come in Class 12 Board exams as well as competitive entrance tests. Therefore, it’s important that you thoroughly understand Class 11 topics to ease your study.
Each and every detail is provided in this article related to the Central Board of Secondary Education. You just have to check out and read every detail to know about it.
CBSE Chemistry Class 11 Syllabus 2020-21
|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 VIII||Redox Reactions||4||16|
|Unit X||s -Block Elements||5|
|Unit XI||Some p -Block Elements||9|
|Unit XII||Organic Chemistry: Some Basic Principles andTechniques||10||18|
Download CBSE Chemistry Class 11 Syllabus 2020-21
CBSE Chemistry Class 11 Syllabus 2019-20
|Unit I||Some Basic Concepts of Chemistry||O8||08 Marks|
|Unit II||Structure of Atom||10|
|Unit III||Classification of Elements and Periodicity in Properties||06||04 Marks|
|Unit IV||Chemical Bonding and Molecular Structure||14||20 Marks|
|Unit V||States of Matter: Gases, Liquids and solids||18|
|Unit VI||Chemical Thermodynamics||16|
|Unit VIII||Redox Reactions||06||20 Marks|
|Unit X||s -Block Elements||10|
|Unit XI||p -Block Elements||18|
|Unit XII||Organic Chemistry: Some Basic Principles and Techniques||14||18 Marks|
|Unit XIV||Environmental Chemistry||06|
CBSE Class 11 Chemistry Syllabus 2018 – 19
Higher Secondary is the most crucial stage of school education because at this juncture specialized discipline-based, content-oriented courses are introduced. Students reach this stage after 10 years of general education and opt for Chemistry with the purpose of pursuing their career in basic sciences or professional courses like medicine, engineering, technology and other applied areas.
Therefore, there is a need to provide learners with sufficient conceptual background of Chemistry, which will make them competent to meet the challenges of academic and professional courses after the senior secondary stage. The new and updated curriculum is based on disciplinary approach with rigour and depth taking care that the syllabus is not heavy and at the same time it is comparable to the international level.
The knowledge related to the subject of Chemistry has undergone tremendous changes during the past decade. Many new areas like synthetic materials, biomolecules, natural resources, industrial chemistry are coming in a big way and deserve to be an integral part of chemistry syllabus at a senior secondary stage.
At the international level, new formulations and nomenclature of elements and compounds, symbols and units of physical quantities floated by scientific bodies like IUPAC and CGPM are of immense importance and need to be incorporated in the updated syllabus. The revised syllabus takes care of all these aspects. Greater emphasis has been laid on the use of new nomenclature, symbols and formulations, the teaching of fundamental concepts, application of concepts in chemistry to industry/ technology, logical sequencing of units, removal of obsolete content and repetition, etc.
Unit – I: 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 – II: Structure of Atom
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
Modern periodic law and the present form of the 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
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, Liquids and Solids
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) Solid-state: Classification of solids based on different binding forces: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea). Unit cell in two dimensional and three-dimensional lattices, calculation of density of unit cell, packing in solids, packing efficiency, voids, number of atoms per unit cell in a cubic unit cell, point defects, electrical and magnetic properties.
Unit – VI: Chemical Thermodynamics
Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions. The 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. The 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
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 polybasic acids, acid strength, concept of pH, Henderson Equation, hydrolysis of salts (elementary idea), buffer solution, solubility product, common ion effect (with illustrative examples).
Unit – VIII: Redox Reactions
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 – IX: Hydrogen
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)
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.
Preparation and Properties of Some Important Compounds: Sodium Carbonate, Sodium Chloride, Sodium Hydroxide and Sodium Hydrogencarbonate, Biological importance of Sodium and Potassium. Calcium Oxide and Calcium Carbonate and their industrial uses, biological importance of Magnesium and Calcium
Unit – XI : p -Block Elements
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 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, the variation of properties, oxidation states, trends in chemical reactivity, anomalous behaviour 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.
Group -15 Elements: General introduction, electronic configuration, occurrence, oxidation states, trends in physical and chemical properties; Nitrogen preparation properties and uses; compounds of Nitrogen, preparation and properties of Ammonia and Nitric Acid, Oxides of Nitrogen(Structure only) ; Phosphorus – allotropic forms, compounds of Phosphorus: Preparation and Properties of Phosphine, Halides and Oxoacids (elementary idea only).
Unit – XII: Organic Chemistry – Some Basic Principles and Techniques
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 – XIII: H hydrocarbons
Classification of 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.
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 the functional group in monosubstituted benzene. Carcinogenicity and toxicity.
Unit – XIV: Environmental Chemistry
Environmental pollution – air, water and soil pollution, chemical reactions in atmosphere, smogs, 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 :
Micro-chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used:
- 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 the 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
- Anyone of the following experiments:
- 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.
- Comparing the pH of solutions of strong and weak acids of the same concentration.
- Study the pH change in the titration of a strong base using universal indicator.
- Study the pH change by common-ion in case of weak acids and weak bases.
- Anyone of the following experiments:
- Chemical Equilibrium
One of the following experiments:
- Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions.
- Study the shift in equilibrium between [Co(H2O)6]2+and chloride ions by changing the concentration of either of the ions.
- Quantitative Estimation
- Using a chemical balance.
- Preparation of standard solution of Oxalic acid.
- Determination of strength of a given solution of Sodium Hydroxide by titrating it against a 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.
- Qualitative Analysis
- 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)
- Detection of -Nitrogen, Sulphur, Chlorine in organic compounds.
- Determination of one anion and one cation in a given salt
|Evaluation Scheme for Examination||Marks|
|Volumetric Analysis||08 Marks|
|Salt Analysis||08 Marks|
|Content-Based Experiment||06 Marks|
|Project Work||04 Marks|
|Class record and viva||04 Marks|
|Total Marks||30 Marks|
- Checking the bacterial contamination in drinking water by testing sulphide ion.
- Study of the methods of purification of water.
- Study the acidity of different samples of tea leaves.
- Determination of the rate of evaporation of different liquids.
- 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 the permissible limit (if any).
- Investigation of the foaming capacity of different washing soaps and the effect of the addition of Sodium Carbonate on it.
- Study the effect of acids and bases on the tensile strength of fibres.
- Study of acidity of fruit and vegetable juices.
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