CHEMISTRY SYLLABUS AIEEE 2012 ALL INDIA ENGINEERING ENTRANCE EXAMINATION

chemistry syllabus of aieee 2012 all india engineering entrance examination 

 CHEMISTRY
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 and van der Waals equation.
  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
  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 STRUCURE
  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.

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.
  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; 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 and  sodium  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 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;  properties  of  boric acid, diborane, boron trifluoride, aluminium chloride and alums.
   Group – 14
  Allotropes  of  carbon,  tendency  for  catenation;  Structure  &  properties  of silicates, and zeolites. 
  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 phosphorus.
  Group – 16
  Preparation,  properties,  structures  and  uses  of  ozone;  Allotropic  forms  of sulphur;  Preparation,  properties,  structures  and  uses  of  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.

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  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 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 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.

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 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. 

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)  and  constituent  monosaccharides  of  oligosacchorides (sucrose, lactose and 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 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.