(Syllabus) AIEEE CHEMISTRY SYLLABUS - 2009
AIEEE
2009 CHEMISTRY SYLLABUS
SECTION: A
PHYSICAL CHEMISTRY
UNIT 1: SOME BASIC CONCEPTS IN CHEMISTRY:
Matter and its nature, Dalton’s atomic theory; Concept of atom, molecule,
element and compound; Physical quantities and their measurements in Chemistry,
precision and accuracy, significant figures, S.I. Units, dimensional analysis;
Laws of chemical combination; Atomic and molecular masses, mole concept, molar
mass, percentage composition, 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 of diffusion, Avogadro’s law, Dalton’s law of partial
pressure; Concept of Absolute scale of temperature; Ideal gas equation; Kinetic
theory of gases (only postulates); Concept of average, root mean square and most
probable velocities; Real gases, deviation from Ideal behaviour, compressibility
factor, van der Waals equation, liquefaction of gases, critical constants.
Liquid State: Properties of liquids - vapour pressure, viscosity and surface
tension and effect of temperature on them (qualitative treatment only). Solid
State: Classification of solids: molecular, ionic, covalent and metallic solids,
amorphous and crystalline solids (elementary idea); Bragg’s Law and its
applications; Unit cell and lattices, packing in solids (fcc, bcc and hcp
lattices), voids, calculations involving unit cell parameters, imperfection in
solids; Electrical, magnetic and dielectric properties.
UNIT 3: ATOMIC STRUCTURE:
Discovery of sub-atomic particles (electron, proton and neutron); Thomson and
Rutherford atomic models and their limitations; 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, ?? and ??2, concept of atomic orbitals as one electron wave
functions; Variation of ?? and ??2 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.
UNIT 4: CHEMICAL BONDING AND MOLECULAR STRUCTURE:
Kossel - Lewis approach to chemical bond formation, concept of ionic and
covalent bonds. 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; 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.
UNIT 5: 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; DS of the universe and DG of the system as criteria for spontaneity,
Dgo (Standard Gibbs energy change) and equilibrium constant.
UNIT 6: 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.
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,
equilibrium constants (Kp and Kc) and their significance, significance of DG and
DGo 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, Br??nsted - 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.
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 and molar conductivities and their variation with
concentration: Kohlrausch’s law and its applications. 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.
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).
UNIT-10 : SURFACE CHEMISTRY:
Adsorption- Physisorption and chemisorption and their characteristics, factors
affecting adsorption of gases on solids - Freundlich and Langmuir adsorption
isotherms, adsorption from solutions. Catalysis - Homogeneous and heterogeneous,
activity and selectivity of solid catalysts, enzyme catalysis and its mechanism.
Colloidal state - distinction among true solutions, colloids and suspensions,
classification of colloids - lyophilic, lyophobic; multi molecular,
macromolecular and associated colloids (micelles), preparation and properties of
colloids - Tyndall effect, Brownian movement, electrophoresis, dialysis,
coagulation and flocculation; Emulsions and 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 the
extraction of metals - concentration, reduction (chemical and electrolytic
methods) and refining with special reference to the extraction of Al, Cu, Zn and
Fe; Thermodynamic and electrochemical principles involved in the extraction of
metals.
UNIT 13: HYDROGEN:
Position of hydrogen in periodic table, isotopes, preparation, properties and
uses of hydrogen; Physical and chemical properties of water and heavy water;
Structure, preparation, reactions and uses of hydrogen peroxide; Classification
of hydrides - ionic, covalent and interstitial; Hydrogen as a fuel.
UNIT 14: S - BLOCK ELEMENTS (ALKALI AND
ALKALINE EARTH METALS):
Group - 1 and 2 Elements General introduction, electronic configuration and
general trends in physical and chemical properties of elements, anomalous
properties of the first element of each group, diagonal relationships.
Preparation and properties of some important compounds - sodium carbonate,
sodium chloride, sodium hydroxide and sodium hydrogen carbonate; 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 and chemical properties of elements across the
periods and down the groups; unique behaviour of the first element in each
group. Groupwise study of the p – block elements Group – 13 Preparation,
properties and uses of boron and aluminium; Structure, properties and uses of
borax, boric acid, diborane, boron trifluoride, 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. 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 chlorine and
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.
UNIT 16: 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 K2
Cr2 O7 and KMnO4. Inner Transition Elements Lanthanoids - Electronic
configuration, oxidation states, chemical reactivity and lanthanoid contraction.
Actinoids - Electronic configuration and oxidation states.
UNIT 17: 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
coordination 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 Stratospheric Tropospheric pollutants – Gaseous pollutants:
Oxides of carbon, nitrogen and sulphur, hydrocarbons; their sources, harmful
effects and prevention; Green house effect and Global warming; Acid rain;
Particulate pollutants: Smoke, dust, smog, fumes, mist; their sources, harmful
effects and prevention. Stratospheric pollution- Formation and breakdown of
ozone, depletion of ozone layer - its mechanism and effects. Water Pollution -
Major pollutants such as, pathogens, organic wastes and chemical pollutants;
their harmful effects and prevention. Soil pollution - Major pollutants such as:
Pesticides (insecticides,. herbicides and fungicides), 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 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.
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 and carbanions; stability of carbocations and free
radicals, electrophiles and nucleophiles. Electronic displacement in a covalent
bond - Inductive effect, electromeric effect, resonance and hyperconjugation.
Common types of organic reactions Substitution, addition, elimination and
rearrangement.
UNIT 21: HYDROCARBONS:
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. 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.
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, freons and DDT.
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 of dehydration. Phenols: Acidic nature, electrophilic
substitution reactions: halogenation, nitration and sulphonation, 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), 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.
UNIT 24: 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.
UNIT 25: POLYMERS:
General introduction and classification of polymers, general methods of
polymerization- addition and condensation, copolymerization; Natural and
synthetic rubber and vulcanization; some important polymers with emphasis 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 (glucose and fructose),
constituent monosaccharides of oligosacchorides (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.
UNIT 27: CHEMISTRY IN EVERYDAY LIFE:
Chemicals in medicines - Analgesics, tranquilizers, antiseptics,
disinfectants, antimicrobials, antifertility drugs, antibiotics, antacids,
antihistamins - their meaning and 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 the
following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde
and ketone), 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
of
indicators, 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 CuSO4
2. 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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