Chemistry

• General Introduction
• Measurement of Properties of Matter The International System of units Uncertainty in measurement
• Laws of Chemical Combination
  • Statement of laws of chemical combination
  • Importance of laws of chemical combination
  • Dalton’s Atomic Theory
• Empirical Formula and Molecular Formula
  • Atomic mass
  • Molar mass
  • Empirical formula
  • Molecular formula
• Mole Concept and Stoichiometry
  • Mole concept
  • Stoichiometric calculations

• Introduction to Structure of Atom
• Atomic models
  • Thomson model
  • Rutherford model
  • Bohr model
  • Dual behaviour
• Quantum Mechanical Model
  • Concept of orbitals
  • Heisenberg’s uncertainty principle
  • Quantum numbers
• Shapes of Atomic Orbitals
  • Shape of s, p and d orbitals
  • Node and nodal surface
  • Shielding effect
• Rules for Filling Electrons in Orbitals
  • Aufbau principle
  • Pauli’s exclusion principle
  • Hund’s rule
  • Electronic configuration of atoms
• Stability of Completely Filled and half-filled Orbitals

• General Introduction
• Historical Attempts towards Classification
  • Mendeleev Periodic table
• Modern Periodic Table
  • Periodicity of properties
  • Groups and periods
  • Nomenclature of elements with atomic numbers greater than 100
• Periodic Trends in Physical Properties
  • Atomic radii
  • Ionic radii
  • Lanthanide Contraction
  • Ionization enthalpy
  • Electron gain enthalpy
  • Electronegativity
• Periodic Trends in Physical Properties
  • Valency and oxidation state
  • Anomalous properties of second period elements
  • Periodic trends and chemical reactivity

• General Introduction
• Types of Chemical Bonds
  • Ionic bond
  • Covalent bond
  • Polar covalent bond
• Valence Bond Theory
  • Hybridization
  • VSEPR theory
  • Resonance
• Molecular Orbital Theory
  • Magnetic characteristics
  • Bond order
• Hydrogen Bond
  • Intermolecular hydrogen bonding
  • Intramolecular hydrogen bonding

• General Introduction to three States of Matter
• Intermolecular Forces
  • Types of intermolecular forces
  • Nature of intermolecular forces
• Laws Governing Gaseous State
  • Boyle’s law
  • Charles law
  • Gay-Lussac’s law
  • Avogadro law
• Ideal Behaviour
  • Ideal gas equation
  • Dalton’s law of partial pressure
  • Kinetic theory of gases
• Deviation from Ideal Behaviour
  • Compressibility factor
  • Boyle’s temperature
• Liquefaction of Gases
  • Critical temperature, critical pressure and critical volume
• Liquid State
  • Vapour pressure
  • Viscosity
  • Surface tension

• Introduction to Thermodynamics
• Thermodynamic Terms Concepts of :
  • system, surrounding
  • types of system
  • state of a system
  • state function and path function
  • extensive and intensive properties
  • reversible and irreversible process
• Thermodynamic Quantities
  • Work
  • Heat
• First Law of Thermodynamics
  • Internal Energy
  • Enthalpy
  • Heat capacity
  • Measurement of ΔU and ΔH
• Thermochemistry
  • Enthalpy change in a chemical reaction
  • Endothermic and Exothermic reactions
  • Standard enthalpy of reactions
  • Enthalpy changes during phase transformations
  • Standard enthalpy of formation
  • Thermochemical equations
  • Hess’s Law of Constant Heat Summation
  • Enthalpies for different types of reactions
• Spontaneity
  • Entropy
  • Second law of Thermodynamics
  • Gibb’s energy change for spontaneous and non-spontaneous processes
  • Criteria for equilibrium
  • Third Law of Thermodynamics

• Introduction to The students will be able to:
  • Dynamic nature of dynamic nature.
• Equilibrium in Physical Processes
  • Solid – liquid equilibrium
  • Liquid – vapour equilibrium
  • Solid – vapour equilibrium
  • Equilibrium involving dissolution of solid and gases in liquids
• Equilibrium in Chemical Processes
  • Dynamic nature of chemical equilibrium
  • Law of Chemical Equilibrium
  • Equilibrium constant
• Types of Chemical Equilibria
  • Homogenous Equilibria
  • Heterogeneous Equilibria
• Applications of Equilibrium Constant
  • Predicting the extent of a reaction
  • Predicting the direction of the reaction
  • Calculating Equilibrium Concentrations
• Factors Affecting Equilibria
  • Chatelier’s principle
• Ionic Equilibrium in Solution
  • Strong and weak electrolytes
  • Acids, bases and salts
• Ionization of Acids and Bases
  • Ionic product of Water
  • pH scale
  • Ionization constant of weak acids and bases
  • Factors affecting acid strength
  • Common ion effect
• Buffer Solutions
• Solubility Equilibria of Sparingly Soluble Salts
  • Solubility product
  • Common ion effect of solubility of ionic salts

• Introduction to Redox Reactions
• Oxidation and Reduction Reactions
• Redox Reactions in Terms of Electron Transfer Reactions
  • Competitive electron transfer reactions
• Oxidation Number
  • Calculation of oxidation number
• Types of Redox Reactions
• Balancing of Redox Reactions
  • Oxidation number method
  • Half reaction method
• Redox Titrations

• General Introduction
  • Position of hydrogen in the periodic table
• Dihydrogen
  • Occurrence of dihydrogen
  • Isotopes of hydrogen
  • Methods of preparation of hydrogen
  • Properties of hydrogen
  • Uses of hydrogen
• Hydrides
  • Classification
  • General methods of preparation
  • General properties
• Water
  • General characteristics
  • Hard and soft water
  • Heavy water
• Hydrogen peroxide
  • Preparation
  • Properties
  • Uses

• General Introduction
• Group 1 Elements
  • Electronic configuration
  • Physical Properties
  • Chemical properties
  • Diagonal relationship
  • Biological importance
  • Some Alkali metal compounds
• Group 2 Elements
  • Electronic configuration
  • Physical Properties
  • Chemical properties
  • Diagonal relationship
  • Biological importance
  • Some Alkaline earth metal compounds

• General Introduction
• Group 13 Elements
  • Electronic configuration
  • Occurrence
  • Inert pair effect
  • Reactivity
  • Some compounds of Group 13 elements
• Group 14 Elements
  • Electronic configuration
  • General properties
  • Catenation
  • Allotropic forms of carbon
  • Carbides
  • Some compounds of Group 14 elements

• General Introduction
  • Origin of organic chemistry
  • Organic chemistry as a separate discipline
• Types of Hybridization of Carbon
  • Types of hybridization in carbon compounds
  • Shapes of organic molecules
  • 2D and 3D structural representations of organic compounds
• Classification of Organic Compounds
  • based on functional groups
  • based on structure
• IUPAC Nomenclature of Organic Compounds
  • Priority order of functional groups
  • Prefixes and suffixes for functional groups
  • Derivation of structural formula from a given IUPAC name and vice-versa
• Stereochemistry and Isomerism
  • Structural isomerism
  • Stereochemistry and stereoisomerism
  • Projection formulae
  • Interconversion of projection formulas
  • Conformations and their relative stabilities (ethane and butane)
  • Geometrical isomerism (cis and trans)
  • Optical isomerism
  • Absolute and relative nomenclature of optical isomers
• Homolytic and Heterolytic Fission of a Covalent Bond
  • carbocation
  • carbanion
  • free radical
• Basics of Organic Reaction
  • Electrophilic and nucleophilic
  • reagents Types of organic reactions
• Electronic Displacements in a Covalent Bond
  • inductive effect
  • electromeric effect
  • resonance
  • hyperconjugation
• Aromaticity
  • Huckel’s rule
  • Stability of aromatic compounds
• Acidity and Basicity (Bronsted and Lowry’s Concept)
  • Relative acidity of carboxylic acids, phenols and alcohols
  • Relative basicity of amines

• General Introduction
  • Classification of hydrocarbons
• Alkanes (Upto 5 Carbon Atoms)
  • Methods of preparation (Reduction, Wurtz reaction, Kolbe’s electrolysis)
  • Physical properties Chemical reactions (Halogenation, Isomerisation, Oxidation, Aromatization, Combustion, Pyrolysis)
• Alkenes (Upto 5 Carbon Atoms)
  • Methods of preparation (Partial reduction, dehydrohalogenati on, dehydration, dehalogenation)
  • Physical properties Chemical reactions (Addition of H2, X2, Markovnikov’s and anti-Markovnikov’s addition of HX, and H2O, ozonolysis, xidation and polymerisation)
• Alkynes (Upto 5 Carbon Atoms)
  • Methods of preparation (Hydrolysis of calcium carbide, dehydrohalogenation)
  • Physical properties Chemical reactions (Addition of H2, X2, HX, and H2O and polymerisation)

• General Introduction
• Environmental Pollution
  • Environmental pollution
  • Conservation of natural resources
• Air Pollution
  • Greenhouse effect
  • Depletion of stratospheric ozone
  • Sulphur oxides
  • Nitrogen oxides
• Water Pollution
  • Types of water pollutants
  • Treatment of water pollution
  • BOD
• Industrial Pollution
  • Industrial and agricultural chemicals that cause environmental
  • degradation Industrial waste management

• Cutting glass tube and glass rod
• Bending a glass tube
• Drawing out a glass jet
• Boring a cork

• Determination of melting point of an organic compound.
• Determination of boiling point of an organic compound.
• Crystallization involving impure sample of any one of the following:
  • Alum, Copper Sulphate, Benzoic Acid.

• 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.
• Study of pH change by common-ion effect in case of weak acids and weak bases.

One of the following experiments:

• Study the shift in equilibrium between ferric ions and thiocynate ions by increasing /decreasing the concentration of either of the ions.
• Study the shift in equilibrium between [Co (H2 O)6 ] 2+and chloride ions by changing the concentration of either of the ions.

One of the following experiments:

• 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.
• Determination of strength of a given solution of hydrochloric acid by titrating it against standard sodium carbonate solution.

• 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,NO−2,NO−3,Cl−,I−,PO3−4,C2O2−4,CH3COO−
  (Note: Insoluble salts excluded)
• Detection of nitrogen, sulphur, chlorine, in organic compounds.