CBSE Syllabus for Class 11 Chemistry 2019-20

CBSE Syllabus of Class 11 Chemistry – in PDF

CBSE Syllabus for Class 11 Chemistry 2019-20 contains all the topics of this session. myCBSEguide provides you latest Syllabus for Class 11 Chemistry. Chemistry is the study of the materials that make up our bodies and everything in the world around us. It is important because everything you do is chemistry, Even your body is made of chemicals. Now you can Download Latest CBSE Syllabus for class 11 in PDF format is available in myCBSEguide mobile app. The curriculum for March 2020 exams is designed by CBSE, New Delhi as per NCERT textbooks for the session 2019-20.

CBSE Syllabus for class 11 Chemistry 2019-20

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CBSE Syllabus Class 11 Chemistry

Rationale 
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 a 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 one 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 senior secondary stage. At 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 use of new nomenclature, symbols and formulations, teaching of fundamental concepts, application of concepts in chemistry to industry/ technology, logical sequencing of units, removal of obsolete content and repetition, etc.
Objectives
The curriculum of Chemistry at Senior Secondary Stage aims to:

• promote understanding of basic facts and concepts in chemistry while retaining the excitement of chemistry.
• make students capable of studying chemistry in academic and professional courses (such as medicine, engineering, technology) at tertiary level.
• expose the students to various emerging new areas of chemistry and apprise them with their relevance in future studies and their application in various spheres of chemical sciences and technology.
• equip students to face various challenges related to health, nutrition, environment, population, weather, industries and agriculture.  develop problem-solving skills in students.
• expose the students to different processes used in industries and their technological applications.
• apprise students with interface of chemistry with other disciplines of science such as physics, biology, geology, engineering, etc.
• acquaint students with different aspects of chemistry used in daily life.
• develop an interest in students to study chemistry as a discipline.
• integrate life skills and values in the context of chemistry.

Class-11 (Theory) (2019-20)
Course Structure

Total Periods (Theory 160+ Practical 60)
Time: 3 Hours
Total Marks 70

Unit I: Some Basic Concepts of Chemistry
12 Periods
General Introduction: Importance and scope of chemistry. Nature of matter, laws of chemical combination, Dalton’s atomic theory: 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
14 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
08 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
14 Periods
alence 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.
12 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.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
16 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, 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
14 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 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
06 Periods
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
08 Periods
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)
10 Periods
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
14 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 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, 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
Unit XII: Organic Chemistry – Some Basic Principles and Techniques
14 Periods
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 hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.
Unit XIII: Hydrocarbons
12 Periods
Classification of Hydrocarbons
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 (Markownikov’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.
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
06 Periods
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.

Practicals

Practical Syllabus
Total Periods 60
Micro-chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used:

1. 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
2. Characterization and Purification of Chemical Substances
   1. Determination of melting point of an organic compound.
   2. Determination of boiling point of an organic compound.
   3. Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.
3. Experiments based on pH
   1. 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 same concentration.
      • Study the pH change in the titration of a strong base using universal indicator.
   2. Study the pH change by common-ion in case of weak acids and weak bases.
4. Chemical Equilibrium
   One of the following experiments:
   1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions.
   2. Study the shift in equilibrium between [Co(H2O)6] ²⁺ and chloride ions by changing the concentration of either of the ions.
5. Quantitative Estimation
   1. Using a chemical balance.
   2. Preparation of standard solution of Oxalic acid.
   3. Determination of strength of a given solution of Sodium Hydroxide by titrating it against standard solution of Oxalic acid.
   4. Preparation of standard solution of Sodium Carbonate.
   5. Determination of strength of a given solution of Hydrochloric acid by titrating it against standard Sodium Carbonate solution.
6. Qualitative Analysis
   1. 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- , S^2- , [SO₃]^2- , [SO₄]^2- , [NO₃] ^– , Cl^– ,Br^– , I^– , [PO₄]³– , [C₂O₄]²– , CH₃COO^– (Note: Insoluble salts excluded)
   2. Detection of -Nitrogen, Sulphur, Chlorine inorganic compounds.

PROJECT 
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.

Practical Examination for Visually Impaired Students Class 11

Note: Same Evaluation scheme and general guidelines for visually impaired students as given for Class 12 may be followed.

1. List of apparatus for identification for assessment in practicals (All experiments) Beaker, Tripod stand, Wire gauze, glass rod, funnel, filter paper, Bunsen burner, test tube, test tube stand, dropper, test tube holder, ignition tube, china dish, tongs, funnel, tripod stand, wire gauze, Bunsen burner, standard flask, pipette, burette, conical flask, funnel, clamp stand, dropper, wash bottle, filter paper
   • Odour detection in qualitative analysis
   • Procedure/Setup of the apparatus
2. List of Experiments
   1. Characterization and Purification of Chemical Substances
      1. Crystallization of an impure sample of any one of the following: copper sulphate, benzoic acid
   2. Experiments based on pH
      1. Determination of pH of some solutions obtained from fruit juices, solutions of known and varied concentrations of acids, bases and salts using pH paper
      2. Comparing the pH of solutions of strong and weak acids of same concentration.
   3. Chemical Equilibrium
      1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either ions.
      2. Study the shift in equilibrium between [Co(H2O)6] 2+and chloride ions by changing the concentration of either of the ions.
   4. Quantitative estimation
      1. Preparation of standard solution of oxalic acid.
      2. Determination of molarity of a given solution of sodium hydroxide by titrating it against standard solution of oxalic acid.
   5. Qualitative Analysis
      1. Determination of one anion and one cation in a given salt
      2. Cations- [NH]4 + Anions – [CO3] 2- ,S2- , [SO3] 2- , Cl- , CH3COO- (Note: insoluble salts excluded)
      3. Detection of Nitrogen in the given organic compound.
      4. Detection of Halogen in the given organic compound.

Note: The above practicals may be carried out in an experiential manner rather than recording observations. Prescribed Books:

1. Chemistry Part -I, Class-11, Published by NCERT.
2. Chemistry Part -II, Class-11, Published by NCERT.
3. Chemistry Lab Manual, Class 11, Published by NCERT

Question Wise Break up

1. No chapter wise weightage.Care to be taken to cover all the chapters.
2. Suitable internal variations may be made for generating various templates keeping the overall weightage to different form of questions and typology of questions same.
   Choice(s): 
   There will be no overall choice in the question paper.
   However, 33 % internal choices will be given in all the sections