Syllabus: Chemistry for Class 11 | Chemistry Class 11 - NEET PDF Download

 Page 1


 
 
COURSE STRUCTURE 
                              CLASS XI 
THEORY 
Time: 3 Hours                                                                                           Total Marks: 70 
 
S. No UNIT Marks 
1 Some Basic Concepts of Chemistry 7 
2 Structure of Atom 9 
3 Classification of Elements and Periodicity in Properties 6 
4 Chemical Bonding and Molecular Structure 7 
5 Chemical Thermodynamics 9 
6 Equilibrium 7 
7 Redox Reactions 4 
8 Organic Chemistry: Some basic Principles and 
Techniques 
11 
9 Hydrocarbons 10 
 TOTAL 70 
Unit 1: Some Basic Concepts of Chemistry                                                                    
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 2: 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'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 
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, valiancy, Nomenclature of elements with atomic number 
greater than 100. 
Page 2


 
 
COURSE STRUCTURE 
                              CLASS XI 
THEORY 
Time: 3 Hours                                                                                           Total Marks: 70 
 
S. No UNIT Marks 
1 Some Basic Concepts of Chemistry 7 
2 Structure of Atom 9 
3 Classification of Elements and Periodicity in Properties 6 
4 Chemical Bonding and Molecular Structure 7 
5 Chemical Thermodynamics 9 
6 Equilibrium 7 
7 Redox Reactions 4 
8 Organic Chemistry: Some basic Principles and 
Techniques 
11 
9 Hydrocarbons 10 
 TOTAL 70 
Unit 1: Some Basic Concepts of Chemistry                                                                    
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 2: 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'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 
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, valiancy, Nomenclature of elements with atomic number 
greater than 100. 
 
 
 
Unit 4: 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 homonuclear diatomic molecules (qualitative idea only), Hydrogen bond. 
Unit 5: Chemical Thermodynamics 
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 ?U and ?H, 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 6: 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 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 7: 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 8: Organic Chemistry – Some Basic Principles and Techniques 
General introduction, methods of purification, qualitative and quantitative analysis, 
classification and IUPAC nomenclature of organic compounds. Electronic displacements 
in a covalent bond: inductive effect, electrometric effect, resonance and hyper 
conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, 
carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions. 
Page 3


 
 
COURSE STRUCTURE 
                              CLASS XI 
THEORY 
Time: 3 Hours                                                                                           Total Marks: 70 
 
S. No UNIT Marks 
1 Some Basic Concepts of Chemistry 7 
2 Structure of Atom 9 
3 Classification of Elements and Periodicity in Properties 6 
4 Chemical Bonding and Molecular Structure 7 
5 Chemical Thermodynamics 9 
6 Equilibrium 7 
7 Redox Reactions 4 
8 Organic Chemistry: Some basic Principles and 
Techniques 
11 
9 Hydrocarbons 10 
 TOTAL 70 
Unit 1: Some Basic Concepts of Chemistry                                                                    
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 2: 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'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 
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, valiancy, Nomenclature of elements with atomic number 
greater than 100. 
 
 
 
Unit 4: 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 homonuclear diatomic molecules (qualitative idea only), Hydrogen bond. 
Unit 5: Chemical Thermodynamics 
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 ?U and ?H, 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 6: 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 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 7: 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 8: Organic Chemistry – Some Basic Principles and Techniques 
General introduction, methods of purification, qualitative and quantitative analysis, 
classification and IUPAC nomenclature of organic compounds. Electronic displacements 
in a covalent bond: inductive effect, electrometric 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 9: Hydrocarbons 
 
Aliphatic Hydrocarbons 
Alkanes - Nomenclature, isomerism, conformation (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 
 
 
Note: The following topics are included in the syllabus but will be assessed only 
formatively to reinforce understanding without adding to summative assessments. This 
reduces academic stress while ensuring meaningful learning. Schools can integrate 
these with existing chapters as they align well. Relevant NCERT textual material is 
enclosed for reference. 
 
1. s & p Block Elements 
Electronic configuration, atomic & Ionic radii, Ionization Enthalpy, Hydration 
Enthalpy and general trends in physical and chemical properties of s and p 
block elements across the periods and down the groups; unique behavior of the 
first element in each group. 
2. The Gaseous State 
Qualitative treatment of Gas laws, Ideal gas equation and deviations from it. 
 
 
 
 
 
 
 
 
 
 
Page 4


 
 
COURSE STRUCTURE 
                              CLASS XI 
THEORY 
Time: 3 Hours                                                                                           Total Marks: 70 
 
S. No UNIT Marks 
1 Some Basic Concepts of Chemistry 7 
2 Structure of Atom 9 
3 Classification of Elements and Periodicity in Properties 6 
4 Chemical Bonding and Molecular Structure 7 
5 Chemical Thermodynamics 9 
6 Equilibrium 7 
7 Redox Reactions 4 
8 Organic Chemistry: Some basic Principles and 
Techniques 
11 
9 Hydrocarbons 10 
 TOTAL 70 
Unit 1: Some Basic Concepts of Chemistry                                                                    
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 2: 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'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 
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, valiancy, Nomenclature of elements with atomic number 
greater than 100. 
 
 
 
Unit 4: 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 homonuclear diatomic molecules (qualitative idea only), Hydrogen bond. 
Unit 5: Chemical Thermodynamics 
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 ?U and ?H, 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 6: 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 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 7: 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 8: Organic Chemistry – Some Basic Principles and Techniques 
General introduction, methods of purification, qualitative and quantitative analysis, 
classification and IUPAC nomenclature of organic compounds. Electronic displacements 
in a covalent bond: inductive effect, electrometric 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 9: Hydrocarbons 
 
Aliphatic Hydrocarbons 
Alkanes - Nomenclature, isomerism, conformation (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 
 
 
Note: The following topics are included in the syllabus but will be assessed only 
formatively to reinforce understanding without adding to summative assessments. This 
reduces academic stress while ensuring meaningful learning. Schools can integrate 
these with existing chapters as they align well. Relevant NCERT textual material is 
enclosed for reference. 
 
1. s & p Block Elements 
Electronic configuration, atomic & Ionic radii, Ionization Enthalpy, Hydration 
Enthalpy and general trends in physical and chemical properties of s and p 
block elements across the periods and down the groups; unique behavior of the 
first element in each group. 
2. The Gaseous State 
Qualitative treatment of Gas laws, Ideal gas equation and deviations from it. 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
PRACTICAL 
 
PRACTICAL SYLLABUS                                                                                   
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 a universal 
indicator. 
2. Study the pH change by common-ion in case of weak acids and weak bases. 
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 
Page 5


 
 
COURSE STRUCTURE 
                              CLASS XI 
THEORY 
Time: 3 Hours                                                                                           Total Marks: 70 
 
S. No UNIT Marks 
1 Some Basic Concepts of Chemistry 7 
2 Structure of Atom 9 
3 Classification of Elements and Periodicity in Properties 6 
4 Chemical Bonding and Molecular Structure 7 
5 Chemical Thermodynamics 9 
6 Equilibrium 7 
7 Redox Reactions 4 
8 Organic Chemistry: Some basic Principles and 
Techniques 
11 
9 Hydrocarbons 10 
 TOTAL 70 
Unit 1: Some Basic Concepts of Chemistry                                                                    
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 2: 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'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 
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, valiancy, Nomenclature of elements with atomic number 
greater than 100. 
 
 
 
Unit 4: 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 homonuclear diatomic molecules (qualitative idea only), Hydrogen bond. 
Unit 5: Chemical Thermodynamics 
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 ?U and ?H, 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 6: 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 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 7: 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 8: Organic Chemistry – Some Basic Principles and Techniques 
General introduction, methods of purification, qualitative and quantitative analysis, 
classification and IUPAC nomenclature of organic compounds. Electronic displacements 
in a covalent bond: inductive effect, electrometric 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 9: Hydrocarbons 
 
Aliphatic Hydrocarbons 
Alkanes - Nomenclature, isomerism, conformation (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 
 
 
Note: The following topics are included in the syllabus but will be assessed only 
formatively to reinforce understanding without adding to summative assessments. This 
reduces academic stress while ensuring meaningful learning. Schools can integrate 
these with existing chapters as they align well. Relevant NCERT textual material is 
enclosed for reference. 
 
1. s & p Block Elements 
Electronic configuration, atomic & Ionic radii, Ionization Enthalpy, Hydration 
Enthalpy and general trends in physical and chemical properties of s and p 
block elements across the periods and down the groups; unique behavior of the 
first element in each group. 
2. The Gaseous State 
Qualitative treatment of Gas laws, Ideal gas equation and deviations from it. 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
PRACTICAL 
 
PRACTICAL SYLLABUS                                                                                   
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 a universal 
indicator. 
2. Study the pH change by common-ion in case of weak acids and weak bases. 
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 
 
 
 
 
D. Chemical Equilibrium 
      Any one of the following experiments: 
? Study the shift in equilibrium between ferric ions and thiocyanate ions by 
increasing/decreasing the concentration of either of the ions. 
? 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 
Cations:  ????
?? +
,????
?? +
, ????
?? +
, ????
?? +
,????
?? +
, ???? ?? +
,  ????
?? +
, ????
?? +
, ????
?? +
, ????
?? +
, ????
?? +
, ????
?? +
, 
???? ?? +
 
Anions: ????
?? ?? -
,?? ?? -
 , ????
?? ?? -
, ???? ?? -
, ???? ?? -
 ,  ????
-
, ????
-
, ?? -
 ,????
?? ?? -
, ????
?? ?? -
 , ????
?? ?????? -
    
    (Note: Insoluble salts excluded) 
2. Detection of -Nitrogen, Sulphur, Chlorine in organic compounds. 
 
 
PROJECTS 
Scientific investigations involving laboratory testing and collecting information from other 
sources. 
A few suggested Projects 
a) Checking the bacterial contamination in drinking water by testing sulphide ion 
b) Study of the methods of purification of water 
c) 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).