Theory Total Periods 180
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 and 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. Thompson’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,
inert gas radii, ionization enthalpy, electron gain enthalpy,
electronegativity, 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,
Syllabus
for
Secondary
and
Higher
Secondary
Levels
24
molecular orbital theory of homonuclear 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’s number,
ideal gas equation, deviation 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 (Periods 16)
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 ΔU and ΔH, 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 nonspontaneous
process, 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, reactions 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.
25
Syllabus
for
Secondary
and
Higher
Secondary
Levels
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 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 (Periods 16)
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 (Periods 6)
Environmental pollution : Air, water and soil pollution, chemical reactions in atmosphere, smogs,
major atmospheric pollutants; acid rain, ozone and its reactions, effects of depletion of ozone
Syllabus
for
Secondary
and
Higher
Secondary
Levels
26
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 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 (Periods 2)
1. Cutting glass tube and glass rod
2. Bending a glass tube
3. Drawing out a glass jet
4. Boring a cork
B. Characterisation and Purification of Chemical Substance (Periods 6)
1. Determination of melting point of organic compound.
2. Determination of boiling point of organic compound.
3. Crystallization involving impure sample of any one of the following: Alum, Copper
sulphate, Benzoic acid.
C. Experiments Related to pH Change (Periods 6)
(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 acid of same concentration.
• Study the pH change in the titration of a strong acid with 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 (Periods 4)
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 (H2O)6]2+ and chloride ions by changing the
concentration of either of the ions.
E. Quantitative Estimation (Periods 16)
• 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.
27
Syllabus
for
Secondary
and
Higher
Secondary
Levels
XII
• Determination of strength of a given solution of hydrochloric acid by titrating it against
standard sodium carbonate solution.
F. Qualitative Analysis (Periods 16)
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+, NH+
4
Anions – CO2– 3, S2–, SO2– 3, SO2– 4, NO– 2, NO– 3, Cl–, Br–, I–, PO3– 4, C2O2– 4 CH3COO–
(Note : Insoluble salts excluded)
Project (Periods 10)
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 etc. depending upon the regional
variation in drinking water and the study of causes of presences 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 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.
Note: Any other investigatory project, which involves about 10 periods of work, can be chosen
with the approval of the teacher.
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 and 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. Thompson’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,
inert gas radii, ionization enthalpy, electron gain enthalpy,
electronegativity, 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,
Syllabus
for
Secondary
and
Higher
Secondary
Levels
24
molecular orbital theory of homonuclear 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’s number,
ideal gas equation, deviation 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 (Periods 16)
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 ΔU and ΔH, 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 nonspontaneous
process, 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, reactions 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.
25
Syllabus
for
Secondary
and
Higher
Secondary
Levels
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 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 (Periods 16)
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 (Periods 6)
Environmental pollution : Air, water and soil pollution, chemical reactions in atmosphere, smogs,
major atmospheric pollutants; acid rain, ozone and its reactions, effects of depletion of ozone
Syllabus
for
Secondary
and
Higher
Secondary
Levels
26
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 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 (Periods 2)
1. Cutting glass tube and glass rod
2. Bending a glass tube
3. Drawing out a glass jet
4. Boring a cork
B. Characterisation and Purification of Chemical Substance (Periods 6)
1. Determination of melting point of organic compound.
2. Determination of boiling point of organic compound.
3. Crystallization involving impure sample of any one of the following: Alum, Copper
sulphate, Benzoic acid.
C. Experiments Related to pH Change (Periods 6)
(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 acid of same concentration.
• Study the pH change in the titration of a strong acid with 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 (Periods 4)
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 (H2O)6]2+ and chloride ions by changing the
concentration of either of the ions.
E. Quantitative Estimation (Periods 16)
• 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.
27
Syllabus
for
Secondary
and
Higher
Secondary
Levels
XII
• Determination of strength of a given solution of hydrochloric acid by titrating it against
standard sodium carbonate solution.
F. Qualitative Analysis (Periods 16)
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+, NH+
4
Anions – CO2– 3, S2–, SO2– 3, SO2– 4, NO– 2, NO– 3, Cl–, Br–, I–, PO3– 4, C2O2– 4 CH3COO–
(Note : Insoluble salts excluded)
Project (Periods 10)
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 etc. depending upon the regional
variation in drinking water and the study of causes of presences 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 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.
Note: Any other investigatory project, which involves about 10 periods of work, can be chosen
with the approval of the teacher.
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