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Chemistry

1. States of Matter
  1. Measurement: Physical quantities and SI units, Dimensional analysis, Precision, Significant figures.
  2. Chemical reactions: Laws of chemical combination, Dalton’s atomic theory; Mole concept; Atomic, molecular and molar masses; Percentage composition & molecular formula; Balanced chemical equations & stoichiometry
  3. Gaseous state: Kinetic theory – Maxwell distribution of velocities, Average, root mean square and most probable velocities and relation to temperature, Diffusion; Deviation from ideal behaviour – Critical temperature, Liquefaction of gases, van der Waals equation.
  4. Liquid state: Vapour pressure, surface tension, viscosity.
  5. Solid state: Classification; Space lattices & crystal systems; Unit cell – Cubic & hexagonal systems; Close packing; Crystal structures: Simple AB and AB2 type ionic crystals, covalent crystals – diamond & graphite, metals. Imperfections- Point defects, non-stoichiometric crystals; Electrical, magnetic and dielectric properties; Amorphous solids – qualitative description.
2. Atomic Structure
  1. Introduction: Subatomic particles; Rutherford’s picture of atom; Hydrogen atom spectrum and Bohr model.
  2. Quantum mechanics: Wave-particle duality – de Broglie relation, Uncertainty principle; Hydrogen atom: Quantum numbers and wavefunctions, atomic orbitals and their shapes (s, p, and d), Spin quantum number.
  3. Many electron atoms: Pauli exclusion principle; Aufbau principle and the electronic configuration of atoms, Hund’s rule.
  4. Periodicity: Periodic law and the modern periodic table; Types of elements: s, p, d, and f blocks; Periodic trends: ionization energy, atomic and ionic radii, electron affinity, and valency.
  5. Nucleus: Natural and artificial radioactivity; Nuclear reactions, Artificial transmutation ofelements.
3. Chemical Bonding & Molecular Structure
  1. Ionic Bond: Lattice Energy and Born-Haber cycle
  2. Molecular Structure: Lewis picture & resonance structures, VSEPR model & molecular shapes
  3. Covalent Bond: Valence Bond Theory- Orbital overlap, Directionality of bonds & hybridistaion (s & p orbitals only), Resonance; Molecular orbital theory- Methodology, Orbital energy level diagram, Bond order, Magnetic properties for homonuclear diatomic species.
  4. Metallic Bond: Qualitative description.
  5. Intermolecular Forces: Polarity; Dipole moments; Hydrogen Bond.
4. Thermodynamics
  1. Basic Concepts: Systems and surroundings; State functions; Intensive & Extensive Properties; Zeroth Law and Temperature
  2. First Law of Thermodynamics: Work, internal energy, heat, enthalpy, heat capacities; Enthalpies of formation, phase transformation, ionization, electron gain; Thermochemistry; Hess’s Law.
  3. Second and Third Laws: Spontaneous and reversible processes; entropy; Gibbs free energy related to spontaneity and non-mechanical work; Standard free energies of formation, free energy change and chemical equilibrium; Third Law and Absolute Entropies.
5. Physical and Chemical Equilibria
  1. Concentration Units: Mole Fraction, Molarity, and Molality
  2. Solutions: Solubility of solids and gases in liquids, Vapour Pressure, Raoult’s law, Relative lowering of vapour pressure, depression in freezing point; elevation in boiling point; osmotic pressure, determination of molecular mass.
  3. Physical Equilibrium: Equilibria involving physical changes (solid-liquid, liquid-gas, solid-gas), Adsorption, Physical and Chemical adsorption, Langmuir Isotherm.
  4. Chemical Equilibria: Equilibrium constants (KP, KC), Le-Chatelier’s principle.
  5. Ionic Equilibria: Strong and Weak electrolytes, Acids and Bases (Arrhenius, Lewis, Lowry and Bronsted) and their dissociation; Ionization of Water; pH; Buffer solutions; Acid-base titrations; Hydrolysis; Solubility Product of Sparingly Soluble Salts; Common Ion Effect.
  6. Factors Affecting Equilibria: Concentration, Temperature, Pressure, Catalysts, Significance of DG and DG0 in Chemical Equilibria.
6. Electrochemistry
  1. Redox Reactions: Oxidation-reduction reactions (electron transfer concept); Oxidation number; Balancing of redox reactions; Electrochemical cells and cell reactions; Electrode potentials; EMF of Galvanic cells; Nernst equation; Gibbs energy change and cell potential; Concentration cells; Secondary cells; Fuel cells; Corrosion and its prevention.
  2. Electrolytic Conduction: Electrolytic Conductance; Specific, equivalent and molar conductivities; Kolhrausch’s Law and its application, Faraday’s laws of electrolysis; Electrode potential and electrolysis, Commercial production of the chemicals, NaOH, Na, Al, Cl2, & F2
7. Chemical Kinetics
  1. Aspects of Kinetics: Rate and Rate expression of a reaction; Rate constant; Order of reaction; Integrated rate expressions for zero and first order reactions; Half-life; Determination of rate constant and order of reaction
  2. Factor Affecting the Rate of the Reactions: Temperature dependence of rate constant; Activation energy; Catalysis, Surface catalysis, enzymes, zeolites; Factors affecting rate of collisions between molecules; Effect of light.
  3. Mechanism of Reaction: Elementary reactions; Complex reactions; Reactions involving two/three steps only; Photochemical reactions; Concept of fast reactions.
  4. Radioactive isotopes: Half-life period; Radiochemical dating.
8. Hydrogen and s-block elements
  1. Hydrogen: Element: unique position in periodic table, occurrence, isotopes; Dihydrogen: preparation, properties, reactions, and uses; Molecular, saline, interstitial hydrides; Water: Properties; Structure and aggregation of water molecules; Hard and soft water; Heavy water; Hydrogen peroxide.
  2. s-block elements: Abundance and occurrence; Anomalous properties of the first elements in each group; diagonal relationships.
  3. Alkali metals: Lithium, sodium and potassium: occurrence, extraction, reactivity, and electrode potentials; Reactions with oxygen, hydrogen, halogens and liquid ammonia; Basic nature of oxides and hydroxides; Halides; Properties and uses of compounds such as NaCl, Na2CO3, NaHCO3, NaOH, KCl, and KOH.
  4. Alkaline earth metals: Magnesium and calcium: Occurrence, extraction, reactivity and electrode potentials; Reactions with non-metals; Solubility and thermal stability of oxo salts; Properties and uses of important compounds such as CaO, Ca(OH)2, plaster of Paris, MgSO4, MgCl2, CaCO3, and CaSO4; Lime and limestone, cement.
9. p- d- and f-block elements
  1. General: Abundance, distribution, physical and chemical properties, isolation and uses of elements; Trends in chemical reactivity of elements of a group; Extraction and refining of metals.
  2. Group 13 elements: Boron; Properties and uses of borax, boric acid, boron hydrides & halides. Reaction of aluminum with acids and alkalis;
  3. Group 14 elements: Carbon: Uses, Allotropes (graphite, diamond, fullerenes), oxides, halides and sulphides, carbides; Silicon: Silica, silicates, silicones; Tin and lead: Extraction, halides and oxides.
  4. Group 15 elements: Dinitrogen; Reactivity and uses of nitrogen and its compounds; Industrial and biological nitrogen fixation; Ammonia: Haber’s process, properties and reactions; Oxides of nitrogen and their structures; Ostwald’s process of nitric acid production; Fertilizers – NPK type; Production of phosphorus; Allotropes of phosphorus; Preparation, structure and properties of hydrides, oxides, oxoacids and halides of phosphorus.
  5. Group 16 elements: Isolation and chemical reactivity of dioxygen; Acidic, basic and amphoteric oxides; Preparation, structure and properties of ozone; Allotropes of sulphur; Production of sulphur and sulphuric acid; Structure and properties of oxides, oxoacids, hydrides and halides of sulphur.
  6. Group 17 and group 18 elements: Structure and properties of hydrides, oxides, oxoacids of chlorine; Inter halogen compounds; Bleaching Powder; Preparation, structure and reactions of xenon fluorides, oxides, and oxoacids.
  7. d-block elements: General trends in the chemistry of first row transition elements; Metallic character; Oxidation state; Ionic radii; Catalytic properties; Magnetic properties; Interstitial compounds; Occurrence and extraction of iron, copper, silver, zinc, and mercury; Alloy formation; Steel and some important alloys; preparation and properties of CuSO4, K2Cr2O7, KMnO4, Mercury halides; Silver nitrate and silver halides; Photography.
  8. f-block elements: Lanthanides and actinides; Oxidation states and chemical reactivity of lanthanide compounds; Lanthanide contraction; Comparison of actinides and lanthanides.
  9. Coordination Compounds: Coordination number; Ligands; Werner’s coordination theory; IUPAC nomenclature; Application and importance of coordination compounds (in qualitative analysis, extraction of metals and biological systems e.g. chlorophyll, vitamin B12, and hemoglobin); Bonding: Valence-bond approach, Crystal field theory (qualitative); Stability constants; Shapes, color and magnetic properties; Isomerism including stereoisomerisms; Organometallic compounds.
10. Principles of Organic Chemistry and Hydrocarbons
  1. Classification: Based on functional groups, trivial and IUPAC nomenclature.
  2. Electronic displacement in a covalent bond: Inductive, resonance effects, and hyperconjugation; free radicals; carbocations, carbanion, nucleophile and electrophile; types of reactions.
  3. Alkanes and cycloalkanes: Structural isomerism and general properties.
  4. Alkenes and alkynes: General methods of preparation, physical properties, electrophilic and free radical additions, acidic character of alkynes and (1,2 and 1,4) addition to dienes.
  5. Aromatic hydrocarbons: Sources; Isomerism; Resonance delocalization; polynuclear hydrocarbons; mechanism of electrophilic substitution reaction, directive influence and effect of substituents on reactivity.
  6. Haloalkanes and haloarenes: Physical properties, chemical reactions.
  7. Petroleum: Composition and refining, uses of petrochemicals.
11. Stereochemistry
  1. Introduction: Chiral molecules; Optical activity; Polarimetry; R,S and D,L configurations; Fischer projections; Enantiomerism; Racemates; Diastereomerism and meso structures.
  2. Conformations: Ethane, propane, n-butane and cyclohexane conformations; Newman and sawhorse projections.
  3. Geometrical isomerism in alkenes
12. Organic Compounds with Functional Groups Containing Oxygen and Nitrogen
  1. General: Electronic structure, important methods of preparation, important reactions and physical properties of alcohols, phenols, ethers, aldehydes, ketones, carboxylic acids, nitro compounds, amines, diazonium salts, cyanides and isocyanides.
  2. Specific: Effect of substituents on alpha-carbon on acid strength, comparative reactivity of acid derivatives, basic character of amines and their separation, importance of diazonium salts in synthetic organic chemistry
13. Biological and Industrial chemistry
  1. The Cell: Concept of cell and energy cycle.
  2. Carbohydrates: Classification; Monosaccharides; Structures of pentoses and hexoses; Anomeric carbon; Mutarotation; Simple chemical reactions of glucose, Disaccharides: reducing and non-reducing sugars – sucrose, maltose and lactose; Polysaccharides: elementary idea of structures of starch and cellulose.
  3. Proteins: Amino acids; Peptide bond; Polypeptides; Primary structure of proteins; Simple idea of secondary and tertiary structures of proteins; Denaturation of proteins and enzymes.
  4. Nucleic Acids: Types of nucleic acids; Primary building blocks of nucleic acids (chemical composition of DNA & RNA); Primary structure of DNA and its double helix; Replication; Transcription and protein synthesis; Genetic code.
  5. Lipids, Hormones, Vitamins: Classification, structure, functions in biosystems.
  6. Polymers: Classification of polymers; General methods of polymerization; Molecular mass of polymers; Biopolymers and biodegradable polymers; Free radical, cationic and anionic addition polymerizations; Copolymerization: Natural rubber; Vulcanization of rubber; Synthetic rubbers. Condensation polymers.
  7. Pollution: Environmental pollutants; soil, water and air pollution; Chemical reactions in atmosphere; Smog; Major atmospheric pollutants; Acid rain; Ozone and its reactions; Depletion of ozone layer and its effects; Industrial air pollution; Green house effect and global warming; Green Chemistry.
  8. Chemicals in medicine, health-care and food: Analgesics, Tranquilizers, antiseptics, disinfectants, anti-microbials, anti-fertility drugs, antihistamines, antibiotics, antacids; Cosmetics: Creams, perfumes, talcum powder, deodorants; Preservatives, artificial sweetening agents, antioxidants, and edible colours.
  9. Other Industrial Chemicals: Dyes: Classification with examples – Indigo, methyl orange, aniline yellow, alizarin, malachite green; Advanced materials: Carbon fibers, ceramics, micro alloys; Detergents; Insect repellents, pheromones, sex attractants; Rocket Propellants.
14. Theoretical Principles of Experimental Chemistry
  1. Volumetric Analysis: Principles; Standard solutions of sodium carbonate and oxalic acid; Acidbase titrations; Redox reactions involving KI, H2SO4, Na2SO3 and H2S; Potassium permanganate in acidic, basic and neutral media; Titrations of oxalic acid, ferrous ammonium sulphate with KMnO4; Estimation of calcium and magnesium by EDTA titrations.
  2. Qualitative analysis of Inorganic Salts: Principles in the determination of the cations Pb2+, Cu2+, As3+, Mn2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+, Fe3+, Ni2+ and the anions CO32-, S2-, SO42-, SO32-, NO2-, NO3-, Cl-, Br-, I-, PO43-, CH3COO-, C2O42-.
  3. Physical Chemistry Experiments: crystallization of alum, copper sulphate, ferrous sulphate, double salt of alum and ferrous sulphate, potassium ferric sulphate; Temperature vs. solubility; pH measurements; Lyophilic and lyophobic sols; Dialysis; Role of emulsifying agents in emulsification. Equilibrium studies involving (i) ferric and thiocyanate ions (ii) [Co(H2O)6]2+ and chloride ions; Enthalpy determination for (i) strong acid vs. strong base neutralization reaction (ii) hydrogen bonding interaction between acetone and chloroform; Rates of the reaction between (i) sodium thiosulphate and hydrochloric acid, (ii) potassium iodate and sodium sulphite (iii) iodide vs. hydrogen peroxide, concentration and temperature effects in these reactions;
  4. Purification Methods: Filtration, crystallization, sublimation, distillation, differential extraction, and chromatography. Principles of melting point and boiling point determination; principles of paper chromatographic separation – Rf values.
  5. Qualitative Analysis of Organic Compounds: Detection of nitrogen, sulphur, phosphorous and halogens; Detection of carbohydrates, fats and proteins in foodstuff; Detection of alcoholic, phenolic, aldehydic, ketonic, carboxylic, amino groups and unsaturation.
  6. Quantitative Analysis of Organic Compounds: Basic principles for the quantitative estimation of carbon, hydrogen, nitrogen, halogen, sulphur and phosphorous; Molecular mass determination by silver salt and chloroplatinate salt methods; Elementary idea of mass spectrometer for accurate molecular mass determination; Calculations of empirical and molecular formulae.
  7. Principles of Organic Chemistry Experiments: Preparation of iodoform, acetanilide, p-nitro acetanilide, di-benzyl acetone, aniline yellow, beta-naphthol; Preparation of acetylene and study of its acidic character.
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