** UPDATED CBSE CLASS XI Chemistry Syllabus: 2018-19

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    CBSE Class 11th Chemistry Syllabus, CBSE Class 11th Chemistry Syllabus 2018, XIth Class Chemistry Theory Syllabus, XIth Class Chemistry Practical Syllabus, Syllabus of Class XI Chemistry Syllabus
    CBSE CLASS XI Chemistry Syllabus 2018-19

    Hi friends, today we are going to discuss you the latest Syllabus of Class XI Chemistry Syllabus. As you know very well that Central Board of Secondary Education (CBSE) has its own curriculum and they hold the supreme authority to change it further for the benefit of students.

    UPDATED CBSE CLASS XI Chemistry Syllabus 2018-19, CBSE Class 11th Chemistry Syllabus, CBSE Class 11th Chemistry Syllabus 2018, XIth Class Chemistry Theory Syllabus, XIth Class Chemistry Practical Syllabus, Syllabus of Class XI Chemistry Syllabus
    UPDATED CBSE CLASS XI Chemistry Syllabus 2018-19

    So it’s always a wise decision to keep an eye on what happening around with the subject you are going to learn. This year CBSE made little bit changes in class XI Chemistry Syllabus. Let us have a look at the updated CBSE Class XI Chemistry Syllabus for the academic year 2017-18


    CBSE Class XI Chemistry Syllabus (2018-19 Session)


    COURSE STRUCTURE
    CLASS–XI (THEORY) (2017-18)

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

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    Unit No. Title No. of Periods Marks
    Unit I Some Basic Concepts of Chemistry 12 11
    Unit II Structure of Atom 14
    Unit III Classification of Elements and Periodicity in Properties 08 04
    Unit IV Chemical Bonding and Molecular Structure 14 21
    Unit V States of Matter: Gases and Liquids 12
    Unit VI Chemical Thermodynamics 16
    Unit VII Equilibrium 14
    Unit VIII Redox Reactions 06 16
    Unit IX Hydrogen 08
    Unit X s -Block Elements 10
    Unit XI Some p -Block Elements 14
    Unit XII Organic Chemistry: Some Basic Principles and Techniques 14 18
    Unit XIII Hydrocarbons 12
    Unit XIV Environmental Chemistry 06
    Total 160           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: a 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)
    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, the concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship, Heisenberg uncertainty principle, a 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)
    The significance of classification, a 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 (14 Periods)
    Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of a covalent bond, the covalent character of ionic bond, valence bond theory, resonance, the geometry of covalent molecules, VSEPR theory, the concept of hybridization, involving s,p and d orbitals and shapes of some simple molecules, the 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 behavior, empirical derivation of gas equation, Avogadro’s number, ideal gas equation. Deviation from ideal behavior, liquefaction of gases, critical temperature, kinetic energy and molecular speeds (elementary idea), Liquid State- vapor 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. The second law of Thermodynamics (brief introduction)
    Introduction of entropy as a state function, Gibb’s energy change for spontaneous and nonspontaneous 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, the degree of ionization, ionization of polybasic acids, acid strength, the 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)
    The 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)
    A 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
    the 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 use.
    Preparation and Properties of Some Important Compounds:
    Sodium Carbonate, Sodium Chloride, Sodium Hydroxide and Sodium Hydrogencarbonate, The biological importance of Sodium and Potassium. Calcium Oxide and Calcium Carbonate and their industrial uses, biological importance of
    Magnesium and Calcium.

    Unit XI: Some p -Block Elements (14 Periods)
    General Introduction to p -Block Elements Group 13 Elements: General introduction, electronic configuration, occurrence, a variation of properties, oxidation states, trends in chemical reactivity, anomalous properties of the 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, the anomalous behavior 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 Technique (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 hyperconjugation. 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, a 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, the mechanism
    of electrophilic addition. Alkynes – Nomenclature, a 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 the 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

    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 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 glass jet
    4. Boring a cork

    B. 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.

    C. Experiments based on pH
    (a) Anyone of the following experiments:

    •  Determination of pH of some solutions obtained from fruit juices, a 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.

    (b) Study the pH change by common-ion in case of weak acids and weak bases.

    D. Chemical Equilibrium
    One of the following experiments:
    a) Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions.
    b) Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the concentration of either of the ions.

    E. Quantitative Estimation
    i) Using a chemical balance.
    ii) Preparation of standard solution of Oxalic acid.
    iii) Determination of strength of a given solution of Sodium Hydroxide by titrating it against a 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.

    F. 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 –
    (Note: Insoluble salts excluded)

    (b) 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 sulfide 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 the 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 in 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 based 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 XI

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

    A. 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

    •  Odor detection in qualitative analysis
    • Procedure/Setup of the apparatus

                                                                   Practical Examination for Visually Impaired Students
                                                                                                         Class XI

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

    A. 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

    •  Odor detection in qualitative analysis
    •  Procedure/Setup of the apparatus

    B. List of Experiments
     A. Characterization and Purification of Chemical Substances
    1. Crystallization of an impure sample of any one of the following: copper sulfate, benzoic acid

     B. 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 the same concentration.

    C. Chemical Equilibrium
    1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing
    the concentration of either ion.
    2. Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the
    concentration of either of the ions.

    D. 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
    a standard solution of oxalic acid.

    E. Qualitative Analysis
    1. Determination of one anion and one cation in a given salt
    2. Cations– (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-XI, Published by NCERT.
    2. Chemistry Part -II, Class-XI, Published by NCERT.

    Time 3 Hours                                                                                                                       Max. Marks: 70

    S.

    No.

    Typology of Questions Very Short

    Answer

    (VSA)

    (1 mark)

    Short

    Answer-I

    (SA-I)

    (2 marks)

    Short

    Answer –II

    (SA-II) (3

    marks)

    Value

    based

    question

    (4 marks)

    Long

    Answer

    (LA)

    (5 marks)

    Total

    Marks

    %

    Weightag

    e

    1 Remembering- (Knowledge-based Simple recall questions, to know specific facts, terms, concepts, principles, or theories, Identify, define, or recipe information) 2 1 1 7 10%
    2 Understanding- Comprehension –to be familiar with the meaning and to understand conceptually, interpret, compare, contrast, explain, paraphrase information) 2 4 1 21 30%
    3 Application (Use the abstract information in concrete the, to apply knowledge to new situations, Use given content to interpret a situation, provide an example, or solve a problem) 2 4 1 21 30%
    4 High order thinking skills (Analysis & Synthesis- Classify, compare, contrast, or differentiate between different pieces of information, Organize and/or integrate unique pieces of information from a variety of sources) 2 1 1 10 14%
    5 Evaluation- (Appraise, judge, and/or justify the value or worth of a decision of them, or to predict outcomes based on values) 1 2 1 11 16%
    TOTAL 5×1=5 5×2=10 12×3=36 1×4=4 3×5=15 70(26) 100%

    QUESTION WISE BREAK UP

    Type of Question Mark per Question Total No. of Questions Total Marks
    VSA 1 5 05
    SA-I 2 5 10
    SA-II 3 12 36
    VBQ 4 1 04
    LA 5 3 15
    Total 26 70

    1. Internal Choice: There is no overall choice in the paper. However, there is an internal choice in one a question of 2 marks weightage, one question of 3 marks weightage and all the three questions of 5 marks weightage.

    2. The above template is only a sample. Suitable internal variations may be made for generating similar templates keeping the overall weight to a different form of questions and typology of questions same.

    Note: NCERT Books Download for Free

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