Chemistry Syllabus for AIEEE 2012

                           SECTION: A                    
                   PHYSICAL CHEMISTRY

UNIT 1: SOME BASIC CONCEPTS IN CHEMISTRY
Matter and its nature, Dalton’s atomic theory; Concept of atom, molecule, element andcompound; Physical quantities and their measurements in Chemistry, precision andaccuracy, significant figures, S.I. Units, dimensional analysis; Laws of chemicalcombination; Atomic and molecular masses, mole concept, molar mass, percentagecomposition, empirical and molecular formulae; Chemical equations and stoichiometry.

UNIT 2: STATES OF MATTER
Classification of matter into solid, liquid and gaseous states.
Gaseous State:Measurable properties of gases; Gas laws - Boyle’s law, Charle’s law, Graham’s law ofdiffusion, Avogadro’s law, Dalton’s law of partial pressure; Concept of Absolute scale oftemperature; Ideal gas equation; Kinetic theory of gases (only postulates); Concept ofaverage, root mean square and most probable velocities; Real gases, deviation fromIdeal behaviour, compressibility factor and van der Waals equation.
Liquid State:Properties of liquids - vapour pressure, viscosity and surface tension and effect oftemperature on them (qualitative treatment only).
Solid State:Classification of solids: molecular, ionic, covalent and metallic solids, amorphous andcrystalline solids (elementary idea); Bragg’s Law and its applications; Unit cell andlattices, packing in solids (fcc, bcc and hcp lattices), voids, calculations involving unitcell parameters, imperfection in solids; Electrical, magnetic and dielectric properties.

UNIT 3: ATOMIC STRUCTUREThomson and Rutherford atomic models and their limitations; Nature ofelectromagnetic radiation, photoelectric effect; Spectrum of hydrogen atom, Bohrmodel of hydrogen atom - its postulates, derivation of the relations for energy of theelectron and radii of the different orbits, limitations of Bohr’s model; Dual nature ofmatter, de-Broglie’s relationship, Heisenberg uncertainty principle. Elementary ideas ofquantum mechanics, quantum mechanical model of atom, its important features, ?? and??2, concept of atomic orbitals as one electron wave functions; Variation of ?? and ??2with r for 1s and 2s orbitals; various quantum numbers (principal, angular momentumand 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 – aufbauprinciple, Pauli’s exclusion principle and Hund’s rule, electronic configuration ofelements, extra stability of half-filled and completely filled orbitals.

UNIT 4: CHEMICAL BONDING AND MOLECULAR STRUCURE
Kossel - Lewis approach to chemical bond formation, concept of ionic and covalentbonds.Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds;calculation of lattice enthalpy.Covalent Bonding: Concept of electronegativity, Fajan’s rule, dipole moment; ValenceShell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules.Quantum mechanical approach to covalent bonding: Valence bond theory - Its importantfeatures, 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 configurationsof homonuclear diatomic molecules, concept of bond order, bond length and bondenergy.Elementary idea of metallic bonding. Hydrogen bonding and its applications.

UNIT 5: CHEMICAL THERMODYNAMICS
Fundamentals of thermodynamics: System and surroundings, extensive and intensiveproperties, state functions, types of processes.First law of thermodynamics - Concept of work, heat internal energy and enthalpy, heatcapacity, molar heat capacity; Hess’s law of constant heat summation; Enthalpies ofbond dissociation, combustion, formation, atomization, sublimation, phase transition,hydration, ionization and solution.Second law of thermodynamics; Spontaneity of processes; DS of the universe and DG ofthe system as criteria for spontaneity, Dgo (Standard Gibbs energy change) andequilibrium constant.

UNIT 6: SOLUTIONS
Different methods for expressing concentration of solution - molality, molarity, molefraction, percentage (by volume and mass both), vapour pressure of solutions andRaoult’s Law – Ideal and non-ideal solutions, vapour pressure - composition, plots forideal and non-ideal solutions; Colligative properties of dilute solutions - relativelowering of vapour pressure, depression of freezing point, elevation of boiling point andosmotic pressure; Determination of molecular mass using colligative properties;Abnormal value of molar mass, van’t Hoff factor and its significance.

UNIT 7: EQUILIBRIUM
Meaning of equilibrium, concept of dynamic equilibrium.Equilibria involving physical processes: Solid -liquid, liquid - gas and solid – gas equilibria,Henry’s law, general characterics of equilibrium involving physical processes.Equilibria involving chemical processes: Law of chemical equilibrium, equilibriumconstants (Kp and Kc) and their significance, significance of DG and DGo in chemicalequilibria, factors affecting equilibrium concentration, pressure, temperature, effect ofcatalyst; Le Chatelier’s principle.Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, variousconcepts of acids and bases (Arrhenius, Bronsted - Lowry and Lewis) and their ionization, acid - base equilibria (including multistage ionization) and ionizationconstants, ionization of water, pH scale, common ion effect, hydrolysis of salts and pHof their solutions, solubility of sparingly soluble salts and solubility products, buffersolutions.

UNIT 8: REDOX REACTIONS AND ELECTROCHEMISTRY
Electronic concepts of oxidation and reduction, redox reactions, oxidation number,rules for assigning oxidation number, balancing of redox reactions.Eectrolytic and metallic conduction, conductance in electrolytic solutions, specific andmolar conductivities and their variation with concentration: Kohlrausch’s law and itsapplications.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 leadaccumulator; Fuel cells.

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 andmolecularity of reactions, rate law, rate constant and its units, differential and integralforms of zero and first order reactions, their characteristics and half - lives, effect oftemperature on rate of reactions – Arrhenius theory, activation energy and itscalculation, collision theory of bimolecular gaseous reactions (no derivation).


UNIT-10 : SURFACE CHEMISTRYAdsorption- Physisorption and chemisorption and their characteristics, factors affectingadsorption of gases on solids - Freundlich and Langmuir adsorption isotherms,adsorption from solutions.Colloidal state - distinction among true solutions, colloids and suspensions,classification of colloids - lyophilic, lyophobic; multi molecular, macromolecular andassociated colloids (micelles), preparation and properties of colloids - Tyndall effect,Brownian movement, electrophoresis, dialysis, coagulation and flocculation; Emulsionsand their characteristics.                                                

                  SECTION – B                
          INORGANIC CHEMISTRY


UNIT 11: CLASSIFICATON OF ELEMENTS AND 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.

UNIT 12: GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF METALS
Modes of occurrence of elements in nature, minerals, ores; Steps involved in theextraction of metals - concentration, reduction (chemical and electrolytic methods) andrefining with special reference to the extraction of Al, Cu, Zn and Fe; Thermodynamicand electrochemical principles involved in the extraction of metals.

UNIT 13: HYDROGEN
Position of hydrogen in periodic table, isotopes, preparation, properties and uses ofhydrogen; Physical and chemical properties of water and heavy water; Structure,preparation, reactions and uses of hydrogen peroxide; Hydrogen as a fuel.

UNIT 14: S - BLOCK ELEMENTS (ALKALI AND ALKALINE EARTH METALS)
Group - 1 and 2 ElementsGeneral introduction, electronic configuration and general trends in physical andchemical properties of elements, anomalous properties of the first element of eachgroup, diagonal relationships.Preparation and properties of some important compounds - sodium carbonate andsodium hydroxide; Industrial uses of lime, limestone, Plaster of Paris and cement;Biological significance of Na, K, Mg and Ca.

UNIT 15: P - BLOCK ELEMENTS
Group - 13 to Group 18 Elements
General Introduction: Electronic configuration and general trends in physical andchemical properties of elements across the periods and down the groups; uniquebehaviour of the first element in each group.Groupwise study of the p – block elements
Group – 13Preparation, properties and uses of boron and aluminium; properties of boric acid,diborane, boron trifluoride, aluminium chloride and alums.
Group – 14Allotropes of carbon, tendency for catenation; Structure & properties of silicates, andzeolites.
Group – 15Properties and uses of nitrogen and phosphorus; Allotrophic forms of phosphorus;Preparation, properties, structure and uses of ammonia, nitric acid, phosphine andphosphorus halides, (PCl3, PCl5); Structures of oxides and oxoacids of phosphorus.
Group – 16Preparation, properties, structures and uses of ozone; Allotropic forms of sulphur;Preparation, properties, structures and uses of sulphuric acid (including its industrialpreparation); Structures of oxoacids of sulphur.
Group – 17Preparation, properties and uses of hydrochloric acid; Trends in the acidic nature ofhydrogen halides; Structures of Interhalogen compounds and oxides and oxoacids ofhalogens.
Group –18Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon.

UNIT 16: d – and f – BLOCK ELEMENTS
Transition Elements
General introduction, electronic configuration, occurrence and characteristics, generaltrends in properties of the first row transition elements - physical properties, ionizationenthalpy, oxidation states, atomic radii, colour, catalytic behaviour, magneticproperties, complex formation, interstitial compounds, alloy formation; Preparation,properties and uses of K2 Cr2 O7 and KMnO4.
Inner Transition Elements
Lanthanoids - Electronic configuration, oxidation states and lanthanoid contraction.
Actinoids - Electronic configuration and oxidation states.

UNIT 17: CO-ORDINATION COMPOUNDS
Introduction to co-ordination compounds, Werner’s theory; ligands, co-ordinationnumber, denticity, chelation; IUPAC nomenclature of mononuclear co-ordinationcompounds, isomerism; Bonding-Valence bond approach and basic ideas of Crystalfield theory, colour and magnetic properties; Importance of co-ordination compounds(in qualitative analysis, extraction of metals and in biological systems).

UNIT 18: ENVIRONMENTAL CHEMISTRY
Environmental pollution - Atmospheric, water and soil.Atmospheric pollution - Tropospheric and StratosphericTropospheric pollutants – Gaseous pollutants: Oxides of carbon, nitrogen and sulphur,hydrocarbons; their sources, harmful effects and prevention; Green house effect andGlobal warming; Acid rain;Particulate pollutants: Smoke, dust, smog, fumes, mist; their sources, harmful effects andprevention.Stratospheric pollution- Formation and breakdown of ozone, depletion of ozone layer - itsmechanism and effects.Water Pollution - Major pollutants such as, pathogens, organic wastes and chemicalpollutants; their harmful effects and prevention.Soil pollution - Major pollutants such as: Pesticides (insecticides,. herbicides andfungicides), their harmful effects and prevention.Strategies to control environmental pollution.

                            
                     SECTION-C                  
            ORGANIC CHEMISTRY


UNIT 19: PURIFICATION AND CHARACTERISATION OF ORGANIC COMPOUNDS
Purification - Crystallization, sublimation, distillation, differential extraction andchromatography - 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 inorganic quantitative analysis.

UNIT 20: SOME BASIC PRINCIPLES OF ORGANIC CHEMISTRY
Tetravalency of carbon; Shapes of simple molecules - hybridization (s and p);Classification of organic compounds based on functional groups: - C = C - , - C h C –and those containing halogens, oxygen, nitrogen and sulphur; Homologous series;Isomerism - structural and stereoisomerism.Nomenclature (Trivial and IUPAC)Covalent bond fission - Homolytic and heterolytic: free radicals, carbocations andcarbanions; stability of carbocations and free radicals, electrophiles and nucleophiles.Electronic displacement in a covalent bond- Inductive effect, electromeric effect, resonance and hyperconjugation.

UNIT 21: HYDROCARBONS
Classification, isomerism, IUPAC nomenclature, general methods of preparation,properties and reactions.Alkanes - Conformations: Sawhorse and Newman projections (of ethane); Mechanism ofhalogenation of alkanes.Alkenes - Geometrical isomerism; Mechanism of electrophilic addition: addition ofhydrogen, halogens, water, hydrogen halides (Markownikoff’s and peroxide effect);Ozonolysis and polymerization.Alkynes - Acidic character; Addition of hydrogen, halogens, water and hydrogen halides;Polymerization.Aromatic hydrocarbons - Nomenclature, benzene - structure and aromaticity; Mechanismof electrophilic substitution: halogenation, nitration, Friedel – Craft’s alkylation andacylation, directive influence of functional group in mono-substituted benzene.

UNIT 22: 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.

UNIT 23: ORGANIC COMPOUNDS CONTAINING OXYGEN
General methods of preparation, properties, reactions and uses.
ALCOHOLS, PHENOLS AND ETHERS
Alcohols: Identification of primary, secondary and tertiary alcohols; mechanism ofdehydration.
Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration andsulphonation, Reimer - Tiemann reaction.
Ethers: Structure.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), Grignardreagent; oxidation; reduction (Wolff Kishner and Clemmensen); acidity of ? - hydrogen,aldol condensation, Cannizzaro reaction, Haloform reaction; Chemical tests todistinguish between aldehydes and Ketones.
CARBOXYLIC ACIDSAcidic strength and factors affecting it.

UNIT 24: ORGANIC COMPOUNDS CONTAINING NITROGEN
General methods of preparation, properties, reactions and uses.Amines: Nomenclature, classification, structure, basic character and identification ofprimary, secondary and tertiary amines and their basic character.Diazonium Salts: Importance in synthetic organic chemistry.

UNIT 25: POLYMERS
General introduction and classification of polymers, general methods of polymerisation addition and condensation, copolymerization;Natural and synthetic rubber and vulcanization; some important polymers withemphasis on their monomers and uses - polythene, nylon, polyester and bakelite.

UNIT 26: BIOMOLECULES
General introduction and importance of biomolecules.CARBOHYDRATES - Classification: aldoses and ketoses; monosaccharides (glucoseand fructose) and constituent monosaccharides of oligosacchorides (sucrose, lactoseand maltose).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.

UNIT 27: CHEMISTRY IN EVERYDAY LIFE
Chemicals in medicines - Analgesics, tranquilizers, antiseptics, disinfectants,antimicrobials, antifertility drugs, antibiotics, antacids, antihistamins - their meaningand common examples.Chemicals in food - Preservatives, artificial sweetening agents - common examples.Cleansing agents - Soaps and detergents, cleansing action.

UNIT 28: PRINCIPLES RELATED TO PRACTICAL CHEMISTRY

• Detection of extra elements (N,S, halogens) in organic compounds; Detection of thefollowing functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde andketone), carboxyl and amino groups in organic compounds.
• Chemistry involved in the preparation of the following:Inorganic compounds: Mohr’s salt, potash alum.Organic compounds: Acetanilide, pnitroacetanilide, aniline yellow, iodoform.
• Chemistry involved in the titrimetric excercises - Acids bases and the use ofindicators, oxalic-acid vs KMnO4, Mohr’s salt vs KMnO4.
• Chemical principles involved in the qualitative salt analysis:Cations - Pb2+ , Cu2+, AI3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, NH4+.Anions- CO3 2-, S2-, SO4 2-, NO2-, NO3-, CI -, Br, I.(Insoluble salts excluded).
• Chemical principles involved in the following experiments:1. Enthalpy of solution of CuSO42. Enthalpy of neutralization of strong acid and strong base.3. Preparation of lyophilic and lyophobic sols.4. Kinetic study of reaction of iodide ion with hydrogen peroxide at room temperature.

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