UNIT-1: SOME BASIC CONCEPTS OF CHEMISTRY
General Introduction: Importance of studying chemistry, Historical approach to
particulate nature of matter, Laws of Chemical combination, Dalton’s Atomic Theory,
Concept of elements, atoms & molecules. Atomic and molecular masses, Mole concept and
molar mass, percentage composition, empirical and molecular formula; chemical reactions,
stoichiometry and calculation based on stoichiometry.
Unit-II: STRUCTURE OF ATOM
Discovery of electron, proton and neutron, atomic num
Thomson’s model and its limitations, Rutherford’s model and its limitations. Bohr’s mode
its limitations, concept of shells and sub
relationship. Heisenberg’s uncertainty principle, concept of orbitals, quantum numbers,
shapes of s, p and d- orbitals. Rules for filling electrons in orbi
exclusion principle and Hund’s rule. Electronic configuration of atoms, stability of
and completely filled orbitals.
Unit-III: CLASSIFICATION OF ELEMENT
Significance of classification, brief history of the development of periodic table.
Modern periodic law and the present form of the periodic table, periodic trends in
properties of elements: atomic radii, ionic radii, inert gas radii, ioniza
gain enthalpy, electronegativity, valency.
Unit-IV: CHEMICAL BONDING AND MOLECULAR STRUCTURE
Valence electrons, lonic bond, covalent bond, bond parameters, Lewis structure,
polar character of covalent bond,
molecules, VSEPR theory, concept of hybridization involving s, p and d
of some simple molecules, molecular orbital theory of homonuclear molecules (Qualitative
idea only), hydrogen bonding.
Unit-V: THERMODYNAMICS
Concepts of system, types of systems, surrounding, work, heat; energy intensive
and extensive properties, state functions. First Law of Thermodynamics, internal energy,
enthalpy, heat capacity, specific heat, molar heat capacity, measureme
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
and non-spontaneous process and
Unit-VI: EQUILIBRIUM
Equilibrium in physical and chemical processes, dynamic nature of equilibrium,
law of mass action, equilibrium constant, factors affecting equilibrium: Le
principle: ionic equilibrium-ionization of acids and bases, strong and
degree of ionization, Concept of pH. Hydrolysis of salts (elementary idea), buffer solutions
solubility product, common ion effect (with suitable examples).
Unit-VII: REDOX REACTIONS
Concept of oxidation and reduction, redox reactions, oxidation number,
balancing of chemical equations in redox reactions, applications of redox reactions.
39
CHEMISTRY
Time Allowed: 3hrs
Practicals: 30
1: SOME BASIC CONCEPTS OF CHEMISTRY 07 Marks
General Introduction: Importance of studying chemistry, Historical approach to
ture of matter, Laws of Chemical combination, Dalton’s Atomic Theory,
Concept of elements, atoms & molecules. Atomic and molecular masses, Mole concept and
molar mass, percentage composition, empirical and molecular formula; chemical reactions,
try and calculation based on stoichiometry.
Discovery of electron, proton and neutron, atomic number, isotopes and isobars.
son’s model and its limitations, Rutherford’s model and its limitations. Bohr’s mode
its limitations, concept of shells and sub-shells. Dual nature of matter and light, de
relationship. Heisenberg’s uncertainty principle, concept of orbitals, quantum numbers,
orbitals. Rules for filling electrons in orbitals- Aufbau’s principle, Pauli’s
exclusion principle and Hund’s rule. Electronic configuration of atoms, stability of
III: 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 the periodic table, periodic trends in
properties of elements: atomic radii, ionic radii, inert gas radii, ionization enthalpy, electron
gain enthalpy, electronegativity, valency.
IV: CHEMICAL BONDING AND MOLECULAR STRUCTURE
Valence electrons, lonic bond, covalent bond, bond parameters, Lewis structure,
polar character of covalent bond, valence bond theory, resonance, geometry of covalent
molecules, VSEPR theory, concept of hybridization involving s, p and d
of some simple molecules, molecular orbital theory of homonuclear molecules (Qualitative
.
Concepts of system, types of systems, surrounding, work, heat; energy intensive
and extensive properties, state functions. First Law of Thermodynamics, internal energy,
enthalpy, heat capacity, specific heat, molar heat capacity, measureme
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
spontaneous process and criteria for equilibrium.
Equilibrium in physical and chemical processes, dynamic nature of equilibrium,
law of mass action, equilibrium constant, factors affecting equilibrium: Le
ionization of acids and bases, strong and
degree of ionization, Concept of pH. Hydrolysis of salts (elementary idea), buffer solutions
olubility product, common ion effect (with suitable examples).
tion and reduction, redox reactions, oxidation number,
balancing of chemical equations in redox reactions, applications of redox reactions.
Time Allowed: 3hrs
Practicals: 30 Marks
07 Marks
General Introduction: Importance of studying chemistry, Historical approach to
ture of matter, Laws of Chemical combination, Dalton’s Atomic Theory,
Concept of elements, atoms & molecules. Atomic and molecular masses, Mole concept and
molar mass, percentage composition, empirical and molecular formula; chemical reactions,
09 Marks
ber, isotopes and isobars.
son’s model and its limitations, Rutherford’s model and its limitations. Bohr’s model &
shells. Dual nature of matter and light, de-Broglie’s
relationship. Heisenberg’s uncertainty principle, concept of orbitals, quantum numbers,
Aufbau’s principle, Pauli’s
exclusion principle and Hund’s rule. Electronic configuration of atoms, stability of half-filled
AND PERIODICITY IN PROPERTIES
06 Marks
Significance of classification, brief history of the development of periodic table.
Modern periodic law and the present form of the periodic table, periodic trends in
tion enthalpy, electron
07 Marks
Valence electrons, lonic bond, covalent bond, bond parameters, Lewis structure,
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 molecules (Qualitative
09 Marks
Concepts of system, types of systems, surrounding, work, heat; energy intensive
and extensive properties, state functions. First Law of Thermodynamics, internal energy,
enthalpy, heat capacity, specific heat, molar heat capacity, measurement of E and H,
Hess’s law of constant heat summation, enthalpy of bond dissociation, combustion;
formation, atomization, sublimation, phase transition ionization and dilution.
change for spontaneous
07 Marks
Equilibrium in physical and chemical processes, dynamic nature of equilibrium,
law of mass action, equilibrium constant, factors affecting equilibrium: Le-Chatelier’s
ionization of acids and bases, strong and weak electrolytes,
degree of ionization, Concept of pH. Hydrolysis of salts (elementary idea), buffer solutions,
04 Marks
tion and reduction, redox reactions, oxidation number,
balancing of chemical equations in redox reactions, applications of redox reactions.
38
Unit-VIII: ORGANIC CHEMISTRY
: ORGANIC CHEMISTRY-SOME BASIC PRINCIPLES AND TECHNIQUES
SOME BASIC PRINCIPLES AND TECHNIQUES
11 Marks
roduction to organic chemistry, methods of purification, qualitative
and quantitative analysis, classification and IUPAC nomenclature of organic compounds.
Electronic displacement in a covalent bond: inductive effect, electromeric effect,
conjugation. Homolytic and heterolytic fission of a covalent bond,
free radicals, electrophiles, nucleophiles, carbocations and carbanions. Types of organic
roduction to organic chemistry, methods of purification, qualitative
and quantitative analysis, classification and IUPAC nomenclature of organic compounds.
Electronic displacement in a covalent bond: inductive effect, electromeric effect,
conjugation. Homolytic and heterolytic fission of a covalent bond,
free radicals, electrophiles, nucleophiles, carbocations and carbanions. Types of organic
General introduction to organic chemistry, methods of purification, qualitative
and quantitative analysis, classification and IUPAC nomenclature of organic compounds.
Electronic displacement in a covalent bond: inductive effect, electromeric effect,
resonance and hyper-conjugation. Homolytic and heterolytic fission of a covalent bond,
free radicals, electrophiles, nucleophiles, carbocations and carbanions. Types of organic
reactions.
Unit-IX: HYDROCARBONS
Classification of hydrocarbons
Alkanes: Nomenclature, isomerism, conformations (ethane only),
physical properties. Chemical reactions including free radical mechanism of halogenation,
combustion and pyrolysis
Methods of preparation,
physical properties. Chemical reactions including free radical mechanism of halogenation,
Nomenclature, isomerism, conformations (ethane only), Methods of preparation,
physical properties. Chemical reactions including free radical mechanism of halogenation,
Nomenclature, structure of double bond (ethene), geometrical isomerism,
addition of hydrogen.
halogen, water, hydrogen halides (Markownikov’s addition and peroxide effect).
: Nomenclature, structure of triple bond (ethyne), physical properties, methods of
preparation, chemical reactions: acidic character of alkynes, addition reaction of hydrogen,
10 Marks
Nomenclature, structure of double bond (ethene), geometrical isomerism,
methods of preparation, physical properties, chemical reactions- addition of hydrogen.
halogen, water, hydrogen halides (Markownikov’s addition and peroxide effect).
tion, mechanism of electrophilic addition.
: Nomenclature, structure of triple bond (ethyne), physical properties, methods of
preparation, chemical reactions: acidic character of alkynes, addition reaction of hydrogen,
ns, hydrogen halides and water.
ntroduction, IUPAC nomenclature, Benzene resonance,
aromaticity, chemical properties, mechanism of electrophilic substitution
sulphonation, halogenations Friedel Craft’s alkylation and acylation, directive infl
functional group in mono substituted benzene.
Alkenes: Nomenclature, structure of double bond (ethene), geometrical isomerism,
methods of preparation, physical properties, chemical reactions
halogen, water, hydrogen halides (Markownikov’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
Aromatic hydrocarbons: Introduction, IUPAC nomenclature, Benzene resonance,
aromaticity, chemical properties, mechanism of electrophilic substitution
sulphonation, halogenations Friedel Craft’s alkylation and acylation, directive infl
functional group in mono substituted benzene.
ntroduction, IUPAC nomenclature, Benzene resonance,
aromaticity, chemical properties, mechanism of electrophilic substitution-nitration,
sulphonation, halogenations Friedel Craft’s alkylation and acylation, directive influence of
Units of measurements, System of Units, , S I Units, fundamental and derived units, least count,significant figures, Errors in measurements , Dimensions of Physics quantities, dimensional analysis, and its applications.