CHEMISTRY SYLLABUS
Class XI & XII
AIMS -
The knowledge in chemistry during the last decade has under gone revolutionary change. Many new areas like synthetic materials, Bio molecules, new industrial chemicals have arrived in a big way. At senior Secondary level it deserve
to be an integral part of chemistry syllabus. At the International level new formulations, nomenclature of elements and compounds, symbols and units of Physical quantities floated by Scientific bodies like TUPAC, IUPAC and CGPM are of no less importance and need to be incorporated in the syllabus.
The revised syllabus has been prepared keeping in mind the NCF (National curriculum Frame work) 2005, CBSE, NCERT and the present state syllabus takes care of all these aspects listed above. Greater emphasis has been laid on use
of new nomenclature, symbols and formulations, teaching of fundamental concepts, applications of concepts in industry/ Technology, logical sequencing of units, removal of irrelevent contents of the present syllabus and avoiding
unnecessary repetition of things already studied in the previous classes has been kept in mind while forming this new syllabus.
OBJECTIVES -
The broad objectives of teaching Chemistry at Senior Secondary Stage are to help the learners as follows:
• to promote understanding of basic facts and concepts in chemistry while retaining the excitement of chemistry.
• to make students capable of studying chemistry in academic and professional courses (such as medicine, engineering, techonology) at higher level.
• to expose the students to emerging various new areas of chemistry and apprise them with the relevance in their future studies and their application in various spheres of chemical science and technology.
• to equip students to face various chalanges related to health, nutrition, environment, population, weather, industries and agriculture.
• to develop problem solving skills in students.
• to expose the students to different processes used in industries and their technological applications.
• to apprise students with interface of chemistry with other disciplines of science such as physics, biology, geology, engineering etc.
• to acquaint students with different aspects of chemistry used in daily life.
• to develop an interest in students to study chemistry as a discipline.
• to develop a disciplinary habbit while working with chemistry.
CHEMISTRY
TIME - 3 HRS. CLASS – XI Theo. – 75 M.M. 100
THEORY
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Unit Topics Marks Periods
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1. History of chemistry and some basic concepts 4 14
2. Atomic structure 5 16
3. Classifiction of elements and periodicity in 4 08
their properties
4. Chemical bonding and molecular structure 5 16
5. States of Matter 4 14
6. Thermodynamics & chemical energetics 5 14
7. Chemical Equilibrium 4 08
I - Equilibrium processes and phase
equilibrium
II - Ionic eqnilibrium in solutions 4 08
8. I - Oxidation - Reduction Reactions 3 06
II - Principles of metallurgical operations 3 06
9. Hydrogen 3 08
10. S-Block Elements (Group I and II elements) 5 08
11. Some p Block elements I (Elements of Group 13) 5 12
12. Some p Block elements II (Elements of Group 14) 5 12
13. Organic chemistry - some basic principles 5 14
14. Hydrocarbons 5 16
15. Environmental Chemistry 3 06
16. Polymers 3 08
Revision --- 20
Total: 75 200
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Unit 1 History of chemistry and some basic concepts : 04
History of chemistry : General introduction History of Chemistry in light of Indian Scenerio, importance and scope of chemistry, Historical approach to particulate nature of matter (ancient concept).
some basic concepts : laws of chemical combination, Dalton's atomic theroy; concept of elements, atoms and molecules.
Atomic and molecular masses, Mole concept and molar mass; percentage composition, empirical and molecular formulae; chemical reactions, stoichiometry and calculations based on it.
Unit 2 Structure of Atom : 05
Discovery of electron, Proton and Neutron; atomic number, isotops and isobars. Thompson's model and its limitations, Rutherford's model and its limitations, hydrogen spectrum, Bohr's model and its limitations, modern concept of atomic structure, 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 3 Classification of Elements and Periodicity in Properties : 04
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, inert gas radii, ionisation enthalpy, electron gain enthalpy, electronegativity, valency.
Unit 4. Chemical bonding and molecular structure- 05
Valence electrons, ionic bond, covalent bond and co-ordinate bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, Born-Haber cycle, 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 5. States of Matter (gases and liquids) 04
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, Charle's law, Gay Lussac's law, Avogadro's law, Ideal behaviour of gases, Avogadro's number, kinetic theory of gases, Ideal gas equation, Deviation from ideal behaviour, liquifaction of gases, critical temperature.
Liquid State - Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations)
Unit 6. Thermodynamics and chemical energetics 05
Reversible and irreversible processes, concept of system, types of systems,surrounding, work, heat, energy, extensive and itensive properties, state functions.
First law of thermodynamics - internal energy and enthalpy, heat capacity and specific heat, measurement of D U and D H, Hess's law of constant heat summation, enthalpy of : bond dissociation, combustion, formation, atomization,
sublimation, phase transition, ionization and dilution.
Introduction of entropy as a state function, free energy change for spontaneous and non-spontaneous processes.
Unit 7. Chemical Equilibrium 04
I - Equilibrium in physical and chemical processes, Dynamic nature of equilibrium, Law of mass action, equilibrium constant, kP and kC , factors affecting equilibrium - Le Chatelier's principle;
II - 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 8. I - Oxidation - Reduction Reactions 03
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, applications of redox reactions.
II - Principles of metallurgical operations 03
Modes of occurance, concentration of ores, chemical principles underlying extraction and Refining.
Unit 9 Hydrogen 03
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; representing strength, or concentration hydrogen as a fuel.
Unit10 S-Block Elements (Group I and Group II elements) 05
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; reaction with ammonia, uses.
Preparation and properties of some important compounds:
Sodium carbonate, sodium hydroxide and sodium hydrogen carbonate, (Sodium bi carbonate) biological importance of sodium and potassium. CaO, CaCO3 and industrial use of lime, limestone and plaster of paris, biological importance of Mg and Ca.
Unit11 Some p-Block Elements, I (Group 13 elements) 05
General introduction, electronic configuration, occurence, 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, Alum.
Unit12 Some p-Block elements, II (Group 14 elements) 05
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 compunds: oxides.
Important compunds of silicon and a few uses, silicon tetrachloride, silicones, silicates and zeolites.
Unit13 Organic Chemistry- Some Basic Principles and Techniques 05
General introducion, methods of purification, qualitative and quantitative analysis. Tetra valency of carbon, classification and IUPAC nomenclature of organic compounds. structural isomerism.
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, carboanions; electrophiles and nucleophiles, types of organic reactions.
Unit14 Hydrocarbons 05
Classification of hydrocarbons
Alkanes - Nomenclature, isomerism, conformations (In reference to ethane). physical properties, chemical reactions including free radicals, 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 ( Markonikoffs addition rule 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, suphonation, halogenation, Friedel Craft's alkylation and acylation; directive infuence of functional group in mono- subsitituted benzene; carcinogenicity and toxicity.
Unit15 Environmental Chemistry 03
Environmental pollution - air, water and soil pollution, chemical reactions in atomosphere, 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.
Importance of medicianal plants in pollution control and its medicinal use.
Unit16 Polymers 03
Classification - Natural and synthetic, methods of polymerisation (addition and condensation), co-polymerisation, some important polymers (Natural and synthetic) like polythene, nylon, polyester, bakelite, rubber & its vulcanisation, PVC, Teflon.
Chemistry Practical
Class - XIth
M.M. 25 Periods: 120
Micro- chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used.
A. Basic Laboratory Techniques 04
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 substance 12
1. Determination of melting points of organic compounds
2. Determination of boiling point of organic compound
3. Crystalization involving impure sample of any one of the following: Alum, copper sulphate, Benzoic acid.
C. Experiments related to pH change 12
a. Any one of the following experiments:
• Determination of pH of some solutions obtained from fruit juices, solutions 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 acid with a strong base using indicator.
b. Study of pH change by common-ion effect in case of weak acids and weak bases.
D. Chemical equilibrium 08
One of the following experiments:
a. Study the shift in equilibrium between ferric ions and thiocynate ions by increasing/ decreasing the concentration of either ions.
b. Study the shift in equilibrium between [Co(H20)6]3+ and chloride ions by changing the concentration of either of the ions.
E. Quantitative estimation 32
• Using a chemical balance
• Preparation of standard solution of oxalic acid
• Determination of strength of a given solution of sodium hydroxide by
titrating it agianst 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 32
Determination of one anion and one cation in a given salt 6 Acid radicals - (Note : Insoluble salts to be excluded)
G. Detection of any one of the following elements. With preparation of sodium extract must be taught to the student:- 4
elements - N, S, Cl, Br, I
K. Determing strength of given unknown solution by titrating nutralisation reaction between 
against 
using phenolphthelene as an indicator and 
as an intermediate solutions OR oxalic acid and ferrous
ammonium sulphate where 
is an intermediate solution as well as self indicator. 5
PROJECT 20
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 ions.
• Study of the methods of purification of water.
• Testing the hardness, presence of iron, fluoride, chloride ions etc. depending upon the regional variation in drinking water and the 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 them.
• Study of the acidity/basicity of different samples of the tea leaves.
• Determination of the rate of evaporation of different liquids.
• Study of the effect of acids and bases on the tensile strength of fibers.
• Analysis of fruit and vegetable juices for their acidity/basicity
• Prepare a table of atleast ten medicinal plants showing the uses of various parts useful for curing diseases.
Note: Any other investigatory project, which involves about 10 periods of work,
can be chosen with the approval of the teacher.
Subject - Chemistry (Practical)
Class - XI
Examination Scheme
Time - 3 Hrs. M.M. 25
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S.No. Syllabus Marks
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1. Vlumetric analysis - Acid - base double titration with the 05
help of 
solution against 
solution.
2. Qualitative analysis - Analysis of Inorganic salt containing 06
one acidic and one basic radical.
3. Element detection in an organic compound (any one) 04
N , S , Cl , Br , I
4. Project work - To write four or five projects based on every 04
day life, after doing these projects in laboratory, they are to
be recorded in practical note book.
5. Practical Record 03
6. Viva voce 03
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