Unit 1: Some Basic Concepts in Chemistry | - Matter & its nature
- Dalton’s atomic theory
- Concept of atom/molecule/compound
- Physical quantities & their measurement in chemistry
- Precision & accuracy
- Significant figures
- SI Units
- Dimensional analysis
- Laws of Chemical Combination
- Atomic & molecular masses/molecular masses /molar mass/mole concept/percentage composition/empirical & molecular formulae
- Chemical equations & stoichiometry
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Unit 2: Atomic Structure | - Discovery of sub-atomic particles(electron, proton and neutron); Nature of electromagnetic radiation, photoelectric effect; Spectrum of hydrogen atom, Bohr model of hydrogen atom - its postulates, derivation of the relations for energy of the electron and radii of the different orbits, limitations of Bohr’s model; Dual nature of matter, de-Broglie’s relationship, Heisenberg uncertainty principle
- Elementary ideas of quantum mechanics, quantum mechanical model of atom, its important features, concept of atomic orbitals as one electron wave functions; Variation of Ψ and Ψ2 with r for 1s and 2s orbitals; various quantum numbers (principal, angular momentum and magnetic quantum numbers) and their significance; shapes of s, p and d - orbitals, electron spin and spin quantum number; Rules for filling electrons in orbitals - Aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals
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Unit 3: Chemical bonding & Molecular Structure | - Kossel - Lewis approach to chemical bond formation, concept of ionic and covalent bonds
- Covalent Bonding: Concept of electronegativity, Fajan’s rule, dipole moment; Valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules
- Quantum mechanical approach to covalent bonding: Valence bond theory - Its important features, concept of hybridization involving s, p and d orbitals; Resonance
- Molecular Orbital Theory - Its important features, LCAOs, types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, concept of bond order, bond length and bond energy.
- Elementary idea of metallic bonding. Hydrogen bonding and its applications
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Unit 4: Chemical Thermodynamics | - Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes
- First law of thermodynamics: Concept of work, heat internal energy and enthalpy, heat capacity, molar heat capacity; Hess’s law of constant heat summation; Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization and solution
- Second law of thermodynamics: Spontaneity of processes; ΔS of the universe and ΔG of the system as criteria for spontaneity, ΔGo (Standard Gibbs energy change) and equilibrium constant
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Unit 5: Solutions | - Different methods for expressing concentration of solution - molality, molarity, mole fraction, percentage (by volume and mass both), vapour pressure of solutions and Raoult’s Law - Ideal and non-ideal solutions, vapour pressure - composition, plots for ideal and non-ideal solutions; Colligative properties of dilute solutions - relative lowering of vapour pressure, depression of freezing point, elevation of boiling point and osmotic pressure; Determination of molecular mass using colligative properties; Abnormal value of molar mass, van’t Hoff factor and its significance.
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Unit 6: Equilibrium | - Meaning of equilibrium, concept of dynamic equilibrium
- Equilibria involving physical processes: Solid -liquid, liquid - gas and solid - gas equilibria, Henry’s law, general characteristics of equilibrium involving physical processes
- Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, significance of ΔG and ΔGo in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, effect of catalyst; Le Chatelier’s principle
- Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Bronsted - Lowry and Lewis) and their ionization, acid - base equilibria (including multistage ionization) and ionization constants, ionization of water, pH scale, common ion effect, hydrolysis of salts and pH of their solutions, solubility of sparingly soluble salts and solubility products, buffer solutions
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Unit 7: Redox Reactions and Electrochemistry - 1 | - Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, balancing of redox reactions.
- Electrolytic & metallic conduction, conductance in electrolytic solutions, specific & molar conductivities and their variation with concentration, Kohlrausch’s law & its applications
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Unit 8: Read Reactions and Electrochemistry - 2 | - Electrochemical cells - Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half - cell and cell reactions, emf of a Galvanic cell and its measurement; Nernst equation and its applications; Relationship between cell potential and Gibbs’ energy change; Dry cell and lead accumulator; Fuel cells; Corrosion and its prevention
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Unit 9: Chemical Kinetics | - Rate of a chemical reaction, factors affecting the rate of reactions: concentration, temperature, pressure and catalyst; elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units, differential and integral forms of zero and first order reactions, their characteristics and half - lives, effect of temperature on rate of reactions - Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions (no derivation).
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Unit 10: Classification of Elements & Periodicity in Properties | - Modem periodic law and present form of the periodic table, s, p, d and f block elements, periodic trends in properties of elements, atomic and ionic radii, ionization enthalpy, electron gain enthalpy, valence, oxidation states and chemical reactivity.
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Unit 11: p-Block Elements | - Group 13 to Group 18 Elements General Introduction: Electronic configuration and general trends in physical and chemical properties of elements across the periods and down the groups; unique behaviour of the first element in each group
- Group - 13 Preparation, properties and uses of Boron and Aluminium; Structure, properties and uses of Borax, Boric acid, Diborane, Boron tri-fluoride, Aluminium chloride and alums
- Group - 14 Tendency for catenation; Structure, properties and uses of allotropes and oxides of Carbon, Silicon tetrachloride, Silicates, Zeolites and Silicones
- Group - 15 Properties and uses of Nitrogen and Phosphorus; Allotrophic forms of Phosphorus; Preparation, properties, structure and uses of Ammonia, Nitric acid, Phosphine and Phosphorus halides, (PCl3, PCl5); Structures of oxides and oxoacids of Nitrogen and Phosphorus
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Unit 12: p-Block Elements | - Group - 16 Preparation, properties, structures and uses of dioxygen and ozone; Allotropic forms of Sulphur; Preparation, properties, structures and uses of Sulphur dioxide, Sulphuric acid (including its industrial preparation); Structures of oxoacids of Sulphur
- Group - 17 Preparation, properties and uses of hydrochloric acid; Trends in the acidic nature of hydrogen halides; Structures of Interhalogen compounds and oxides and oxoacids of halogens
- Group - 18 Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon
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Unit 13: d and f Block Elements | - Transition Elements General introduction, electronic configuration, occurrence and characteristics, general trends in properties of the first row transition elements - physical properties, ionization enthalpy, oxidation states, atomic radii, colour, catalytic behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation; Preparation, properties and uses of K2Cr2O7 and KMnO4
- Lanthanoids - Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction
- Actinoids - Electronic configuration and oxidation states
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Unit 14: Co-ordination Compounds | - Introduction to co-ordination compounds, Werner’s theory; ligands, co-ordination number, denticity, chelation; IUPAC nomenclature of mononuclear co-ordination compounds, isomerism; Bonding-Valence bond approach and basic ideas of Crystal field theory, colour and magnetic properties; Importance of co-ordination compounds (in qualitative analysis, extraction of metals and in biological systems)
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Unit 15: Purification & Characterization of Organic Compounds | - Purification - Crystallization, sublimation, distillation, differential extraction and chromatography - principles and their applications
- Qualitative analysis - Detection of nitrogen, Sulphur, phosphorus and halogens
- Quantitative analysis (basic principles only) - Estimation of Carbon, Hydrogen, Nitrogen, Halogens, Sulphur, Phosphorus
- Calculations of empirical formulae and molecular formulae; Numerical problems in organic quantitative analysis
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Unit 16: Some Basic Principles of Organic Chemistry - 1 | - Tetravalency of Carbon; Shapes of simple molecules - hybridization (s and p); Classification of organic compounds based on functional groups: - C = C - , - C ≡ C - and those containing Halogens, Oxygen, Nitrogen and Sulphur; Homologous series; Isomerism - structural and stereoisomerism
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Unit 17: Some Basic Principles of Organic Chemistry - 2 | - Nomenclature (Trivial and IUPAC) Covalent bond fission - Homolytic and heterolytic: free radicals, carbocations and carbanions; stability of carbocations and free radicals, electrophiles and nucleophiles
- Electronic displacement in a covalent bond - Inductive effect, electromeric effect, resonance and hyper conjugation
- Common types of organic reactions - Substitution, addition, elimination and rearrangement
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Unit 18: Hydrocarbons - 1 | - Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and reactions
- Alkanes - Conformations: Sawhorse and Newman projections (of ethane); Mechanism of halogenation of Alkanes
- Alkenes - Geometrical isomerism; Mechanism of electrophilic addition: addition of hydrogen, halogens, water, hydrogen halides (Markownikoff’s and peroxide effect); Ozonolysis, oxidation, and polymerization
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Unit 19: Hydrocarbons - 2 | - Alkynes - Acidic character; Addition of hydrogen, halogens, water and hydrogen halides; Polymerization
- Aromatic hydrocarbons - Nomenclature, benzene - structure and aromaticity; Mechanism of electrophilic substitution: halogenation, nitration, Friedel - Craft’s alkylation and acylation, directive influence of functional group in mono-substituted benzene
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Unit 20: Organic Compounds Containing Halogens | - General methods of preparation, properties and reactions; Nature of C-X bond; Mechanisms of substitution reactions
- Uses; Environmental effects of chloroform, iodoform, freons and DDT
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Unit 21: Organic Compounds Containing Oxygen - 1 | - General methods of preparation, properties, reactions and uses
- Alcohols, Phenols and Ethers
- Alcohols: Identification of primary, secondary and tertiary Alcohols; mechanism of dehydration
- Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration and sulphonation, Reimer - Tiemann reaction
- Ethers: Structure
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Unit 22: Organic Compounds Containing Oxygen - 2 | - General methods of preparation, properties, reactions and uses
- Aldehyde and Ketones Nature of carbonyl group; Nucleophilic addition to >C=O group, relative reactivities of aldehydes and ketones; Important reactions such as - Nucleophilic addition reactions (addition of HCN, NH3 and its derivatives), Grignard reagent; oxidation; reduction (Wolff Kishner and Clemmensen); acidity of - Hydrogen, aldol condensation, Cannizzaro reaction, Haloform reaction; Chemical tests to distinguish between Aldehydes and Ketones
- Carboxylic Acids: Acidic strength and factors affecting it
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Unit 23: Organic Compounds Containing Nitrogen | - General methods of preparation, properties, reactions and uses
- Amines: Nomenclature, classification, structure, basic character and identification of primary, secondary and tertiary amines and their basic character
- Diazonium Salts: Importance in Synthetic Organic Chemistry
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Unit 24: Principles related to practical chemistry | - Detection of extra elements (Nitrogen, Sulphur, halogens) in organic compounds; Detection of the following functional groups; hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketones) carboxyl, and amino groups in organic compounds
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Unit 25: Biomolecules | - General introduction and importance of biomolecules
- Carbohydrates - Classification: aldoses and ketoses; monosaccharides (glucose and fructose), constituent monosaccharides of oligosaccharides (sucrose, lactose, maltose) and polysaccharides (starch, cellulose, glycogen)
- Proteins - Elementary Idea of amino acids, peptide bond, polypeptides; Proteins: primary, secondary, tertiary and quaternary structure (qualitative idea only), denaturation of proteins, enzymes
- Vitamins - Classification and functions
- Nucleic Acids - Chemical constitution of DNA and RNA. Biological functions of nucleic acids
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