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.
COURSE STRUCTURE
CLASS–XI (THEORY) (2022-23)
Time:3Hours Total Marks70
S.NO UNIT PERIODS MARKS
1 Some Basic Concepts of Chemistry 18 7
2 Structure of Atom 20 9
3 Classification of Elements and
Periodicity in Properties
12 6
4 Chemical Bonding and Molecular
Structure
20 7
5 Chemical Thermodynamics 23 9
6 Equilibrium 20 7
7 Redox Reactions 9 4
8 Organic Chemistry: Some basic
Principles and Techniques
20 11
9 Hydrocarbons 18 10
TOTAL 160 70
Unit I: Some Basic Concepts of Chemistry 18 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 20 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, 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 12 Periods
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, Ionization enthalpy, electron gain
enthalpy, electronegativity, valency. Nomenclature of elements with atomic number
greater than 100.
Unit IV: Chemical Bonding and Molecular Structure 20 Periods
Valence electrons, ionic bond, covalent bond, bond parameters, Lewis’s 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 VI: Chemical Thermodynamics 23 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 ΔU and ΔH, 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 20 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 poly basic acids, acid strength, concept of pH, hydrolysis of salts
(elementary idea), buffer solution, Henderson Equation, solubility product, common ion
effect (with illustrative examples).
Unit VIII: Redox Reactions 09 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 XII: Organic Chemistry -Some Basic Principles and Techniques 20 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 18 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, the 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, the 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 the functional group in
monosubstituted benzene. Carcinogenicity and toxicity.
PRACTICALS
3 HOURS/ 30 Marks
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
1. Any one 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.
D. 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.
E. Quantitative Estimation
1. Using a mechanical balance/electronic 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.
F. Qualitative Analysis
1. Determination of one anion and one cation in a given salt
Cation:
Pb2+, Cu2+ As3+, Aℓ3+, Fe3+, Mn2+, Zn2+, Ni2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4
(Note: Insoluble salts excluded)
2. Detection of -Nitrogen, Sulphur, Chlorine in organic compounds.
G. PROJECTS
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
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 practical (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, standard flask,
pipette, burette, conical flask, clamp stand, dropper, wash bottle
• Odour 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 sulphate,
benzoic acid
C. 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.
D. 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.
E. 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.
F. Qualitative Analysis
1. Determination of one anion and one cation in a given salt
2. Cations – NH4
3. Detection of Nitrogen in the given organic compound.
4. Detection of Halogen in the given organic compound.
Note: The above practical 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.
3. Laboratory Manual of Chemistry, Class XI Published by NCERT
4. Other related books and manuals of NCERT including multimedia and online
sources
Note:
The content indicated in NCERT textbooks as excluded for the year 2022-23 is not to be
tested by schools.
CLASS XII (2022-23) (THEORY)
Time: 3 Hours 70 Marks
Unit II: Solutions 15 Periods
Types of solutions, expression of concentration of solutions of solids in liquids, solubility
of gases in liquids, solid solutions, Raoult’s law, colligative properties – relative lowering of
vapour pressure, elevation of boiling point, depression of freezing point, osmotic pressure,
determination of molecular masses using colligative properties, abnormal molecular mass,
Van’t Hoff factor.
Unit III: Electrochemistry 18 Periods
Redox reactions, EMF of a cell, standard electrode potential, Nernst equation and its
application to chemical cells, Relation between Gibbs energy change and EMF of a cell,
conductance in electrolytic solutions, specific and molar conductivity, variations of
conductivity with concentration, Kohlrausch’s Law, electrolysis and law of electrolysis
(elementary idea), dry cell-electrolytic cells and Galvanic cells, lead accumulator, fuel
cells, corrosion.
Unit IV: Chemical Kinetics 15 Periods
Rate of a reaction (Average and instantaneous), factors affecting rate of reaction:
concentration, temperature, catalyst; order and molecularity of a reaction, rate law and
specific rate constant, integrated rate equations and half-life (only for zero and first order
reactions), concept of collision theory (elementary idea, no mathematical treatment),
activation energy, Arrhenius equation.
Unit VIII: d and f Block Elements 18 Periods
General introduction, electronic configuration, occurrence and characteristics of transition
metals, general trends in properties of the first-row transition metals – metallic character,
ionization enthalpy, oxidation states, ionic radii, colour, catalytic property, magnetic
S.No. Title No. of Periods Marks
1 Solutions 15 7
2 Electrochemistry 18 9
3 Chemical Kinetics 15 7
4 d -and f -Block Elements 18 7
5 Coordination Compounds 18 7
6 Haloalkanes and Haloarenes 15 6
7 Alcohols, Phenols and Ethers 14 6
8 Aldehydes, Ketones and Carboxylic Acids 15 8
9 Amines 14 6
10 Biomolecules 18 7
Total 160 70
properties, interstitial compounds, alloy formation, preparation and properties of K2Cr2O7
and KMnO4.
Lanthanoids –
Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction
and its consequences.
Actinoids – Electronic configuration, oxidation states and comparison with lanthanoids.
Unit IX: Coordination Compounds 18 Periods
Coordination compounds – Introduction, ligands, coordination number, colour, magnetic
properties and shapes, IUPAC nomenclature of mononuclear coordination compounds.
Bonding, Werner’s theory, VBT, and CFT; structure and stereoisomerism, the importance
of coordination compounds (in qualitative analysis, extraction of metals and biological
system).
Unit X: Haloalkanes and Haloarenes. 15 Periods
Haloalkanes: Nomenclature, nature of C–X bond, physical and chemical properties,
optical rotation mechanism of substitution reactions.
Haloarenes: Nature of C–X bond, substitution reactions (Directive influence of halogen in
monosubstituted compounds only). Uses and environmental effects of – dichloromethane,
trichloromethane, tetrachloromethane, iodoform, freons, DDT.
Unit XI: Alcohols, Phenols and Ethers 14 Periods
Alcohols: Nomenclature, methods of preparation, physical and chemical properties (of
primary alcohols only), identification of primary, secondary and tertiary alcohols,
mechanism of dehydration, uses with special reference to methanol and ethanol.
Phenols: Nomenclature, methods of preparation, physical and chemical properties, acidic
nature of phenol, electrophilic substitution reactions, uses of phenols.
Ethers: Nomenclature, methods of preparation, physical and chemical properties, uses.
Unit XII: Aldehydes, Ketones and Carboxylic Acids 15 Periods
Aldehydes and Ketones: Nomenclature, nature of carbonyl group, methods of
preparation, physical and chemical properties, mechanism of nucleophilic addition,
reactivity of alpha hydrogen in aldehydes, uses.
Carboxylic Acids: Nomenclature, acidic nature, methods of preparation, physical and
chemical properties; uses.
Unit XIII: Amines 14 Periods
Amines: Nomenclature, classification, structure, methods of preparation, physical and
chemical properties, uses, identification of primary, secondary and tertiary amines.
Diazonium salts: Preparation, chemical reactions and importance in synthetic organic
chemistry.
Unit XIV: Biomolecules 18 Periods
Carbohydrates – Classification (aldoses and ketoses), monosaccharides (glucose and
fructose), D-L configuration oligosaccharides (sucrose, lactose, maltose), polysaccharides
(starch, cellulose, glycogen); Importance of carbohydrates.
Proteins -Elementary idea of – amino acids, peptide bond, polypeptides, proteins,
structure of proteins – primary, secondary, tertiary structure and quaternary structures
(qualitative idea only), denaturation of proteins; enzymes. Hormones – Elementary idea
excluding structure.
Vitamins – Classification and functions.
Nucleic Acids: DNA and RNA.
Note:
The content indicated in NCERT textbooks as excluded for the year 2022-23 is not to be
tested by schools.
PRACTICALS
3 HOURS/ 30 MARKS
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 60 Periods
Micro-chemical methods are available for several of practical experiments.
Wherever possible, such techniques should be used.
A. Surface Chemistry
(a) Preparation of one lyophilic and one lyophobic sol
Lyophilic sol – starch, egg albumin and gum
Lyophobic sol – aluminium hydroxide, ferric hydroxide, arsenous sulphide.
(b) Dialysis of sol-prepared in (a) above.
(c) Study of the role of emulsifying agents in stabilizing the emulsion of different oils.
B. Chemical Kinetics
(a) Effect of concentration and temperature on the rate of reaction between Sodium
Thiosulphate and Hydrochloric acid.
(b) Study of reaction rates of any one of the following:
(i) Reaction of Iodide ion with Hydrogen Peroxide at room temperature using
different concentrations of Iodide ions.
(ii) Reaction between Potassium Iodate, (KIO3) and Sodium Sulphite: (Na2SO3)
using starch solution as an indicator (clock reaction).
C. Thermochemistry
Any one of the following experiments
(a) Enthalpy of dissolution of Copper Sulphate or Potassium Nitrate.
(b) Enthalpy of neutralization of strong acid (HCI) and strong base (NaOH).
(c) Determination of enthaply change during interaction (Hydrogen bond formation)
between Acetone and Chloroform.
D. Electrochemistry
Variation of cell potential in Zn/Zn2+|| Cu2+/Cu with change in concentration of
electrolytes (CuSO4 or ZnSO4) at room temperature.
E. Chromatography
(a) Separation of pigments from extracts of leaves and flowers by paper
chromatography and determination of Rf values.
(b) Separation of constituents present in an inorganic mixture containing two cations
only (constituents having large difference in Rf values to be provided).
F. Preparation of Inorganic Compounds
Preparation of double salt of Ferrous Ammonium Sulphate or Potash
Alum. Preparation of Potassium Ferric Oxalate.
G. Preparation of Organic Compounds
Preparation of any one of the following compounds
i) Acetanilide ii) Di -benzalAcetone iii) p-Nitroacetanilide iv) Aniline yellow or 2 –
Naphthol Anilinedye.
H. Tests for the functional groups present in organic compounds:
Unsaturation, alcoholic, phenolic, aldehydic, ketonic, carboxylic and amino (Primary)
groups.
I. Characteristic tests of carbohydrates, fats and proteins in pure samples and
their detection in given foodstuffs.
J. Determination of concentration/ molarity of KMnO4 solution by titrating it
against a standard solution of:
(a) Oxalic acid,
(b) Ferrous Ammonium Sulphate
(Students will be required to prepare standard solutions by
weighing themselves).
K. Qualitative analysis
Determination of one anion and one cation in a given salt
Cation:
Pb2+, Cu2+ As3+, Aℓ3+
, Fe3+, Mn2+, Zn2+, Ni2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4
(Note: Insoluble salts excluded)
INVESTIGATORY PROJECT
Scientific investigations involving laboratory testing and collecting information
from other sources A few suggested Projects.
• Study of the presence of oxalate ions in guava fruit at different stages of ripening.
• Study the quantity of casein present in different samples of milk.
• Preparation of soybean milk and its comparison with natural milk with respect to curd
formation, the effect of temperature, etc.
• Study of the effect of Potassium Bisulphate as a food preservative under various
conditions (temperature, concentration, time, etc.)
• Study of digestion of starch by salivary amylase and effect of pH and temperature on it.
• Comparative study of the rate of fermentation of the following materials: wheat flour,
gram flour, potato juice, carrot juice, etc.
• Extraction of essential oils present in Saunf (aniseed), Ajwain (carum), Illaichi
(cardamom).
• Study of common food adulterants in fat, oil, butter, sugar, turmeric power, chilli
powder and pepper.
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 of Classes XI and XII
Evaluation Scheme
Topic Marks
Identification/Familiarity with the apparatus 5
Written test (based on given/prescribed practicals) 10
Practical Record
General Guidelines
• The practical examination will be of two hours duration.
• A separate list of ten experiments is included here.
• The written examination in practicals for these students will be conducted at the
time of the practical examination of all other students.
• The written test will be of 30 minutes duration.
• The question paper given to the students should be legibly typed. It should contain
a total of 15 practical skill-based very short answer type questions. A student would
be required to answer any 10 questions.
• A writer may be allowed to such students as per CBSE examination rules.
• All questions included in the question papers should be related to the listed
practical. Every question should require about two minutes to be answered.
• These students are also required to maintain a practical file. A student is expected
to record at least five of the listed experiments as per the specific instructions for
each subject. These practicals should be duly checked and signed by the internal
examiner.
• The format of writing any experiment in the practical file should include aim,
apparatus required, simple theory, procedure, related practical skills, precautions
etc.
• Questions may be generated jointly by the external/internal examiners and used
for assessment.
• The viva questions may include questions based on basic
theory/principle/concept, apparatus/materials/ chemicals required, procedure,
precautions, sources of error etc.
1. Items for Identification/Familiarity of the apparatus for assessment in practical
(All experiments)
Beaker, glass rod, tripod stand, wire gauze, Bunsen burner, Whatman filter paper,
gas jar, capillary tube, pestle and mortar, test tubes, tongs, test tube holder, test
tube stand, burette, pipette, conical flask, standard flask, clamp stand, funnel, filter paper
Hands-on Assessment
• Identification/familiarity with the apparatus
• Odour detection in qualitative analysis