UNIT 1: BASIC CONCEPTS AND ATOMIC STRUCTURE
Laws of chemical combination: Law of conservation of mass. Law of definite proportion, Law of multiple proportions. Gay- Lussac’s law of combining volumes. Dalton’s atomic theory. Mole concept. Atomic, molecular and molar masses. Chemical equations. Balancing and calculation based on chemical equations.
Atomic structure: Fundamental particles. Rutherford model of atom. Nature of electromagnetic radiation. Emission spectrum of hydrogen atom. Bohr model of hydrogen atom. Drawbacks of Bohr model. Dual nature of matter and radiation. de Broglie relation. Uncertainty principle. Wave function (mention only). Atomic orbitals and their shapes (s, p and d orbitals only). Quantum numbers. Electronic configurations of elements. Pauli’s exclusion principle. Hund’s rule. Aufbau principle.
UNIT 2: BONDING AND MOLECULAR STRUCTURE
Kossel and Lewis approach of bonding. Ionic bond. Lattice energy. Born-Haber cycle. Covalent bond. Lewis structure of covalent bond. Concept of orbital overlap. VSEPR theory and geometry of molecules. Polarity of covalent bond. Valence bond theory and hybridization (sp, sp2, sp3, dsp2, d2sp3 and sp3d2). Resonance. Molecular orbital method. Bond order. Molecular orbital diagrams of homodiatomic molecules. Bond strength and magnetic behaviour. Hydrogen bond. Coordinate bond. Metallic bond.
UNIT 3: STATES OF MATTER
Gaseous state: Boyle’s law. Charles’ law. Avogadro’s hypothesis. Graham’s law of diffusion. Absolute scale of temperature. Ideal gas equation. Gas constant and its values. Dalton’s law of partial pressure. Aqueous tension. Kinetic theory of gases. Deviation of real gases from ideal behaviour. van der Waals equation. Liquefaction of gases. Joule-Thomson effect. Critical temperature. Liquid state: Properties of liquids. Vapour pressure and boiling point. Surface tension. Viscosity. Solid state: Types of solids (ionic, covalent and molecular). Space lattice and unit cells. Cubic crystal systems. X-ray studies of crystals. The Bragg equation. Close packing. Different voids (tetrahedral and octahedral only). Structures of simple ionic compounds of AB and AB2 types. Density calculations. Point defects (Frenkel and Schottky). Electrical properties of solids. Conductors, semiconductors and insulators. Piezoelectric and pyroelectric crystals. Magnetic properties of solids. Diamagnetic, paramagnetic, ferromagnetic, antiferromagnetic and ferrimagnetic substances.
UNIT 4: PERIODIC PROPERTIES OF ELEMENTS AND HYDROGEN
Classification of elements: Mendeleev’s periodic table. Atomic number and modern periodic law. Long form of periodic table. Electronic configurations of elements and their position in the periodic table. Classification into s-, p-, d- and f-block elements. Periodic properties: Ionization energy, electron affinity, atomic radii, valence and electronegativity. Hydrogen: Position in the periodic table, occurrence, isolation, preparation (including commercial), properties, reactions and uses. Isotopes of hydrogen. Hydrides: Molecular, saline and interstitial hydrides. Water: Structure of water molecule and its aggregates. Physical and chemical properties of water. Hard and soft water. Removal of hardness. Preparation and uses of heavy water: Liquid hydrogen as fuel.
UNIT 5: S-BLOCK ELEMENTS AND PRINCIPLES OF METALLURGY
Alkali metals: Occurrence, electronic configuration, trends in atomic and physical properties (ionization energy, atomic radii and ionic radii), electrode potential, and reactions with oxygen, hydrogen, halogens and liquid ammonia. Oxides, hydroxides and halides. Alkaline earth metals: Occurrence, electronic configuration, trends in atomic and physical properties, electrode potential, and reactions with oxygen, hydrogen and halogens. Oxides, hydroxides, halides and sulphides.Anomalous properties of lithium and beryllium. Compounds of s-block elements: Large scale preparation of NaOH and Na2CO3, their properties and uses. Preparation and properties of CaO, Ca(OH)2, Plaster of Paris and MgSO4. Industrial uses of
lime, limestone and cement. Principles of metallurgy: Occurrence of metals. Concentration of ores. General principles of extraction of metals from ore. Refining of metals. Extraction of sodium, aluminium, iron and copper. Manufacture of steel. Different types of steel. Heat treatment and uses of steel.
UNIT 6: p-BLOCK ELEMENTS
General characteristics of p-block elements: atomic and physical properties. Oxidation states. Trends in chemical reactivity of Groups 13, 14, 15, 16 and 17 elements. Boron: Occurrence, isolation, physical and chemical properties. Borax and boric acid. Boron hydrides. Structure of diborane. Uses of boron and its compounds. Carbon: Allotropes, properties, carbides, halides and sulphide. Nitrogen: Terrestrial abundance and distribution, isolation, properties and chemical reactivity. Fixation of nitrogen. Ammonia: Haber process of manufacture, properties and uses. Nitric acid: Ostwald process of manufacture and important uses. Oxides of nitrogen: Preparation and structures (skeletal only). Oxygen: Terrestrial abundance, isolation, properties and chemical reactivity. Oxides: Acidic, basic and amphoteric oxides. Preparation, structure, properties and uses of ozone and hydrogen peroxide. Silica: Different forms and uses. Structures of silicates. Phosphorus: Production, allotropes and phosphine. Preparation and structures of PCl3, PCl5, P4O6, P4O10, oxyacids of phosphorus. Comparison of halides, hydrides and oxides of Group 15 elements. Sulphur: Production, allotropes, oxides and halides. Hydrogen sulphide: Preparation, properties and uses in qualitative analysis. Sulphuric acid: Manufacture, properties and uses. Preparation and properties of Na2S2O3. Comparison of oxides, halides and hydrides of Group 17 elements. Hydrides, oxides and oxyacids of chlorine. Preparation and properties of bleaching powder. Interhalogen compounds. Group 18 elements: Occurrence, isolation, atomic and physical properties, uses. Compounds of xenon: Preparation of fluorides and oxides, and their reactions with water.
UNIT 7: d-BLOCK AND f-BLOCK ELEMENTS
d-Block elements: Electronic configuration and general characteristics. Metallic properties, ionization energy, electrode potential, oxidation states, ionic radii, catalytic properties, coloured ions, complex formation, magnetic properties, interstitial compounds and alloys. Preparation and properties of KMnO4, K2Cr2O7, CuSO4.5H2O, AgNO3, and halides of silver and mercury. Photography. f-Block elements: Lanthanides: Occurrence, electronic configuration and oxidation states. Lanthanide contraction. Uses.
Actinides: Occurrence, electronic configuration and comparison with lanthanides.
UNIT 8: NUCLEAR CHEMISTRY
Natural radioactivity: Properties of alpha, beta and gamma radiations. Group displacement law. Nuclear stability and binding energy. Nuclear reactions. Radioactive disintegration series. Rate of radioactive disintegration and half life. Artificial radioactivity: Transmutation of elements. Nuclear energy. Nuclear fission and nuclear fusion. Nuclear reactors. Radio isotopes and their uses. Radiochemical dating. Synthetic elements.
UNIT 9: THERMODYNAMICS
System and surrounding: Types of systems. Types of processes. Intensive and extensive properties. State functions and path functions. Reversible and irreversible processes. Zeroth law. First law of thermodynamics: Internal energy and enthalpy. Application of first law of thermodynamics. Enthalpy changes during phase transition. Enthalpy changes in chemical reactions. Standard enthalpy of formation. Hess’s law of constant heat summation and numerical problems. Second law of thermodynamics: Entropy and Gibbs free energy. Free energy change and chemical equilibrium. Criteria for spontaneity.
UNIT 10: CHEMICAL EQUILIBRIUM
Physical and chemical equilibria: Dynamic nature of equilibrium. Equilibria involving physical changes (solid-liquid, liquidgas, dissolution of solids in liquids and dissolution of gases in liquids). General characteristics of equilibria involving physical processes. Equilibria involving chemical systems: Law of chemical equilibrium. Magnitude of equilibrium constant.Numerical problems. Effect of changing conditions of systems at equilibrium (changes of concentration, temperature and pressure). Effect of catalyst. The Le Chatelier principle and its applications. Relationship between Kp and Kc. Ionic equilibrium.
Ionization of weak and strong electrolytes. Concepts of acids and bases: Those of Arrhenius, Bronsted-Lowry and Lewis. Acid-base equilibrium. Ionization of water. pH scale. Salt hydrolysis. Theory of acid-base indicators. Solubility product. Common ion effect. Buffer action and buffer solutions.
UNIT 11: SOLUTIONS
Types of solutions: Different concentration terms (normality, molarity, molality, mole fraction and mass percentage). Solubility of gases and solids. Vapour pressure of solutions and Raoult’s law. Deviation from Raoult’s law. Colligative properties: Lowering of vapour pressure, elevation in boiling point, depression in freezing point and osmotic pressure. Ideal and non-ideal solutions. Determination of molecular mass. Abnormal molecular mass. The van’t Hoff factor and related numerical problems
UNIT 12: REDOX REACTIONS AND ELECTROCHEMISTRY
Oxidation and reduction: Electron transfer concept. Oxidation number. Balancing equations of redox reactions: Oxidation number method and ion electron method (half reaction method). Faraday’s laws of electrolysis: Quantitative aspects. Electrolytic conduction. Conductance. Molar conductance. ohlrausch’s law and its applications. Electrode potential and electromotive force (e.m.f.). Reference electrode (SHE only). Electrolytic and Galvanic cells. Daniel cell. The Nernst equation. Free energy and e.m.f. Primary and secondary cells. Fuel cell (H2-O2 only). Corrosion and its prevention: Electrochemical theory of rusting of iron. Methods of prevention of corrosion. Galvanization and cathodic protection.