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CBSE Class XI / XII, 2015, 2016, 2017

Download CBSE Class XI (NCERT), 2015, 2016, 2017, Chemistry Syllabus (8676 Downloads so far)
CHEMISTRY
COURSE STRUCTURE
CBSE XI (NCERT), 2015, 2016, 2017 (Theory)
One Paper Three Hours Max Marks. 70
Unit Titles Weightage
I Some Basic concepts of chemistry 03
II Structure of Atom 06
III Classification of Elements and Periodicity in Properties 04
IV Chemical Bonding and molecular Structure 05
V States of Matter: Gases and Liquids 04
VI Thermodynamics 06
VII Equilibrium 06
VIII Redox Reactions 03
IX Hydrogen 03
X S-Block Elements 05
XI Some p-Block Elements 07
XII Organic Chemistry: some basic Principles and Techniques 07
XIII Hydrocarbons 08
XIV Environmental Chemistry 03
Total 70


Unit I: Some Basic Concepts of Chemistry
General Introduction: Importance and scope of chemistry.
Historical approach to particulate 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
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, 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 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
Significance of classification, 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. Ionization enthalpy, electron gain enthalpy, electro negativity, valence, 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 homo nuclear diatomic molecules, hydrogen bond.

Unit V: States of Matter: Gases and Liquids
Three states of matter. Intermolecular interactions, type 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. Derivation 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: Thermodynamics
Concepts Of System, types of systems, surroundings. Work, heat, energy, extensive and intensive properties, state functions.
First law of thermodynamics - internal energy (U) and enthalpy change (H), 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 transformation, ionization, and solution.
Introduction of entropy as a state function, Gibbs energy change for spontaneous and nonspontaneous processes, criteria for equilibrium.
Second and Third Law of Thermodynamics.

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, acide strength, concept of pH. Henderson Equation. Hydrolysis of salts (elementary idea). Buffer solutions, 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, properties and structure; 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 hydrogen carbonate, biological importance of sodium and potassium. CaO, CaCO3 and industrial use of lime and limestone, biological importance of Mg and Ca.

Unit XI: Some 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 acids, boron hydrides. Aluminium: uses, reactions with acids and alkalies and uses.

Group 14 elements:
General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous behaviour of first element, 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 and structure of silicates.

Unit XII: Organic Chemistry - Some Basic Principles and Techniques
General introduction, methods of 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
Classification of hydrocarbons
Alkanes - Nomenclature, isomerism, conformations (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 (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.

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 mono-substituted benzene; carcinogenicity and toxicity.

Unit XIV: Environmental Chemistry
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, strategy for control of environmental pollution.

Practicals

PRACTICALS SYLLABUS

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 anyone of the following: Alum, copper sulphate, Benzoic acid.

C. Experiments related to pH change
(a) Anyone of the following experiments:
  • Determination of pH of some solutions obtained from fruit juices, varied concentrations of acids. ,bases and salts using pH paper or universal indicator.
  • Comparing the pH of solutions of strong and weak acid of same concentration.
  • Study the pH change in the titration of a strong base using universal indicator.
    b) Study of pH change by common-ion effect 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 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
  • 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 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.

    F. Qualitative analysis
    Determination of one anion and one cation in a given salt
    Cations: Pb2+, Cu2+sup>, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+

    Anions: CO32-, S2-, SO32-, SO42-, NO2-, Cl-, Br-, I-, PO43-, C2O42-, CH3COO-

    (Note: Insoluble salts excluded)

    G. Detection of nitrogen, sulphur, Chlorine,bromine and iodine in an organic compound.

    Recommended Textbooks.
    1. Chemistry Part - I, Published by NCERT
    2. Chemistry Part - II, Published by NCERT


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