(Syllabus) CBSE Syllabus of Chemistry for Class 11th For March 2009 Examination

Syllabus : CBSE Syllabus of Chemistry for Class 11th For March 2009 Examination

Class XI  CHEMISTRY (Theory)
One Paper             Time: 3 Hours                     70 marks



Unit 									Marks 
1. Some Basic concepts of chemistry 					03 
2. Structure of Atom  							06 
3. Classification of Elements and Periodicity in Properties		04 
4. Chemical Bonding and molecular Structure				05 
5. States of Matter: Gases and Liquids					04 
6. Thermodynamics							06 
7. Equilibrium								06 
8. Redox Reactions							03 
9. Hydrogen								03 
10. S-Block Elements							05 
11. Some P-Block Elements						07 
12. Organic Chemistry: some basic Principles and Techniques		07 
13. Hydrocarbons							08 
14. Environmental Chemistry						03 
TOTAL:									70 


Unit I: Some Basic Concepts of Chemistry (Periods 14)
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 (Periods 16)

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 (Periods 8)

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.
Unit IV: Chemical Bonding and Molecular Structure (Periods 16)

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 (qualitative idea only), hydrogen bond.
Unit V: States of Matter: Gases and Liquids (Periods 14)
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’snumber. Ideal gas equation. Derivation from ideal behaviour, liquefaction of gases, critical temperature.
Liquid State - Vapour pressure, viscosity and surface tension (qualitative idea only, no  mathematical derivations).

Unit VI: Thermodynamics (Periods16)
Concepts Of System, 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 transformation, ionization, and solution.
Introduction of entropy as a state function, free energy change for spontaneous and nonspontaneous processes, criteria for equilibrium.
Unit VII: Equilibrium (Periods 16)
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, concept of pH. Hydrolysis of salts (elementary idea). Buffer solutions, solubility product, common ion effect (with illustrative examples).
Unit VIII: Redox Reactions (Periods 6)
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, applications of redox reactions.
Unit IX : Hydrogen (Periods 8)
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) (Periods 14)
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 (Periods 16)
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.
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.
Unit XII: Organic Chemistry - Some Basic Principles and Techniques (Periods 14)
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 (Periods 16)
Classification of hydrocarbons
Alkanes - Nomenclature, isomerism, conformations (ethane only), physical properties, chemical reactions including halogenation, free radical mechanism, 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 (Periods 6)
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.

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