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

 Page 1


 COURSE STRUCTURE  
CLASS –XI (THEORY) (2023-24)  
 Time: 3 Hours                    Total Marks70  
  
S.No  UNIT No. of 
Periods 
Marks 
1 Some Basic Concepts of Chemistry 12 7 
2 Structure of Atom 14 9 
3 Classification of Elements and Periodicity in 
Properties 
8 6 
4 Chemical Bonding and Molecular Structure 14 7 
5 Chemical Thermodynamics 16 9 
6 Equilibrium 14 7 
7 Redox Reactions 6 4 
8 Organic Chemistry: Some basic Principles and 
Techniques 
14 11 
9 Hydrocarbons 12 10 
  TOTAL  70 
 
 
Unit I:  Some Basic Concepts of Chemistry  12 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    14 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.  
  
 
Page 2


 COURSE STRUCTURE  
CLASS –XI (THEORY) (2023-24)  
 Time: 3 Hours                    Total Marks70  
  
S.No  UNIT No. of 
Periods 
Marks 
1 Some Basic Concepts of Chemistry 12 7 
2 Structure of Atom 14 9 
3 Classification of Elements and Periodicity in 
Properties 
8 6 
4 Chemical Bonding and Molecular Structure 14 7 
5 Chemical Thermodynamics 16 9 
6 Equilibrium 14 7 
7 Redox Reactions 6 4 
8 Organic Chemistry: Some basic Principles and 
Techniques 
14 11 
9 Hydrocarbons 12 10 
  TOTAL  70 
 
 
Unit I:  Some Basic Concepts of Chemistry  12 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    14 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  08 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      14 Periods  
  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 VI:  Chemical Thermodynamics      16 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 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 VII:   Equilibrium      14 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      06 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      14 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.  
 
Page 3


 COURSE STRUCTURE  
CLASS –XI (THEORY) (2023-24)  
 Time: 3 Hours                    Total Marks70  
  
S.No  UNIT No. of 
Periods 
Marks 
1 Some Basic Concepts of Chemistry 12 7 
2 Structure of Atom 14 9 
3 Classification of Elements and Periodicity in 
Properties 
8 6 
4 Chemical Bonding and Molecular Structure 14 7 
5 Chemical Thermodynamics 16 9 
6 Equilibrium 14 7 
7 Redox Reactions 6 4 
8 Organic Chemistry: Some basic Principles and 
Techniques 
14 11 
9 Hydrocarbons 12 10 
  TOTAL  70 
 
 
Unit I:  Some Basic Concepts of Chemistry  12 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    14 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  08 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      14 Periods  
  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 VI:  Chemical Thermodynamics      16 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 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 VII:   Equilibrium      14 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      06 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      14 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    12 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, 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 monosubstituted benzene. 
Carcinogenicity and toxicity.  
  
PRACTICALS  
  
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  
Page 4


 COURSE STRUCTURE  
CLASS –XI (THEORY) (2023-24)  
 Time: 3 Hours                    Total Marks70  
  
S.No  UNIT No. of 
Periods 
Marks 
1 Some Basic Concepts of Chemistry 12 7 
2 Structure of Atom 14 9 
3 Classification of Elements and Periodicity in 
Properties 
8 6 
4 Chemical Bonding and Molecular Structure 14 7 
5 Chemical Thermodynamics 16 9 
6 Equilibrium 14 7 
7 Redox Reactions 6 4 
8 Organic Chemistry: Some basic Principles and 
Techniques 
14 11 
9 Hydrocarbons 12 10 
  TOTAL  70 
 
 
Unit I:  Some Basic Concepts of Chemistry  12 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    14 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  08 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      14 Periods  
  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 VI:  Chemical Thermodynamics      16 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 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 VII:   Equilibrium      14 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      06 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      14 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    12 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, 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 monosubstituted benzene. 
Carcinogenicity and toxicity.  
  
PRACTICALS  
  
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  
a) 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.  
b) Study the pH change by common-ion in case of weak acids and weak bases.  
D. Chemical Equilibrium  
   One of the following experiments:  
a) Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing 
the concentration of either of the ions.  
b) Study the shift in equilibrium between [Co(H 2O) 6]
2+
 and chloride ions by changing the 
concentration of either of the ions.  
     E.      Quantitative Estimation  
i. Using a mechanical balance/electronic balance. ii. 
Preparation of standard solution of Oxalic acid.  
iii. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard 
solution of Oxalic acid.  
iv. Preparation of standard solution of Sodium carbonate.  
v. Determination of strength of a given solution of hydrochloric acid by titrating it against standard 
Sodium Carbonate solution.  
 F.       Qualitative Analysis  
a) Determination of one anion and one cation in a given salt  
Cations- Pb
2+
, Cu
2+
, As
3+
, Al
3+
, Fe
3+
, Mn
2+
, Ni
2+
, Zn
2+
, Co
2+
, Ca
2+
, Sr
2+
, Ba
2+
, Mg
2+
, NH 4
+ 
 
Anions – CO 3
2- -
 , S
2-
,  NO 2
-
 , SO 3
2-
-, SO 4
2-
, NO 3
-
 , Cl- , Br-, I-, PO 4
3-
 , ,  CH 3COO
-
 (Note: Insoluble salts 
excluded)  
 
b) Detection of -Nitrogen, Sulphur, Chlorine in organic compounds.   
  
c) 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  
Page 5


 COURSE STRUCTURE  
CLASS –XI (THEORY) (2023-24)  
 Time: 3 Hours                    Total Marks70  
  
S.No  UNIT No. of 
Periods 
Marks 
1 Some Basic Concepts of Chemistry 12 7 
2 Structure of Atom 14 9 
3 Classification of Elements and Periodicity in 
Properties 
8 6 
4 Chemical Bonding and Molecular Structure 14 7 
5 Chemical Thermodynamics 16 9 
6 Equilibrium 14 7 
7 Redox Reactions 6 4 
8 Organic Chemistry: Some basic Principles and 
Techniques 
14 11 
9 Hydrocarbons 12 10 
  TOTAL  70 
 
 
Unit I:  Some Basic Concepts of Chemistry  12 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    14 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  08 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      14 Periods  
  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 VI:  Chemical Thermodynamics      16 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 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 VII:   Equilibrium      14 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      06 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      14 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    12 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, 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 monosubstituted benzene. 
Carcinogenicity and toxicity.  
  
PRACTICALS  
  
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  
a) 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.  
b) Study the pH change by common-ion in case of weak acids and weak bases.  
D. Chemical Equilibrium  
   One of the following experiments:  
a) Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing 
the concentration of either of the ions.  
b) Study the shift in equilibrium between [Co(H 2O) 6]
2+
 and chloride ions by changing the 
concentration of either of the ions.  
     E.      Quantitative Estimation  
i. Using a mechanical balance/electronic balance. ii. 
Preparation of standard solution of Oxalic acid.  
iii. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard 
solution of Oxalic acid.  
iv. Preparation of standard solution of Sodium carbonate.  
v. Determination of strength of a given solution of hydrochloric acid by titrating it against standard 
Sodium Carbonate solution.  
 F.       Qualitative Analysis  
a) Determination of one anion and one cation in a given salt  
Cations- Pb
2+
, Cu
2+
, As
3+
, Al
3+
, Fe
3+
, Mn
2+
, Ni
2+
, Zn
2+
, Co
2+
, Ca
2+
, Sr
2+
, Ba
2+
, Mg
2+
, NH 4
+ 
 
Anions – CO 3
2- -
 , S
2-
,  NO 2
-
 , SO 3
2-
-, SO 4
2-
, NO 3
-
 , Cl- , Br-, I-, PO 4
3-
 , ,  CH 3COO
-
 (Note: Insoluble salts 
excluded)  
 
b) Detection of -Nitrogen, Sulphur, Chlorine in organic compounds.   
  
c) 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   
Class XI  
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 practicals (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  
B. 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.  
C. Chemical Equilibrium  
1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing 
the concentration of eitherions.  
2. Study the shift in equilibrium between [Co(H 2O) 6]
2+
 and chloride ions by changing the 
concentration of either of the ions.  
D. 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.  
E. Qualitative Analysis  
1. Determination of one anion and one cation in a given salt  
2. Cations - NH
+
4  
Anions – (CO 3)
2-
, S
2-
, (SO 3)
2-
, Cl
-
, CH 3COO
-
  
(Note: insoluble salts excluded)