WEST BENGAL JOINT ENTRANCE EXAMINATIONS BOARD
JEM 2012 - SYLLABUS
Atoms, Molecules and Chemical Arithmetic:
Dalton’s atomic theory; Gay Lussac’s law of gaseous volume; Avogadro’s
Hypothesis and its applications. Atomic mass; Molecular mass; Equivalent weight;
Valency; Gram atomic weight; Gram molecular weight; Gram equivalent weight and
mole concept; Chemical formulae; Balanced chemical equations; Calculations
(based on mole concept) involving common oxidation-reduction, neutralization,
and displacement reactions; Concentration in terms of mole fraction, molarity,
molality and normality. Percentage composition, empirical formula and molecular
formula; Numerical problems.
Atomic Structure: Concept of Nuclear Atom – electron,
proton and neutron (charge and mass), atomic number; Rutherford’s model and its
limitations; Extra nuclear structure; Line spectra of hydrogen atom.
Quantization of energy (Planck’s equation E = hv); Bohr’s model of hydrogen atom
and its limitations, Sommerfelds modifications (elementary idea); The four
quantum numbers, ground state electronic configurations of many electron atoms
and mono-atomic ions; The Aufbau Principle; Pauli’s Exclusion Principle and
Uncertainty principle; The concept of atomic orbitals,
shapes of s, p and d orbitals (pictorial approach)
Radioactivity and Nuclear Chemistry
Radioactivity – α-, β-, γ-rays and their properties; Artificial
transmutation; Rate of radioactive decay, decay constant, half-life and average
life period of radio-elements; Units of radioactivity; Numerical problems.
Stability of the atomic nucleus – effect of neutron–proton (n/p) ratio on the
modes of decay, group displacement law, radioisotopes and their uses (C, P, Co
and I as examples) isobars and isotones (definition and examples), elementary
idea of nuclear fission and fusion reactions.
The Periodic Table and Chemical Families
Modern periodic law (based on atomic number); Modern periodic table based on
electronic configurations, groups (Gr. 1–18) and periods. Types of
elements-representative (s-block and p-block), transition (d-block) elements and
inner transition (f-block / lanthanides and actinides) and their general
characteristics. Periodic trends in physical and chemical properties–atomic
radii, valency, ionization energy, electron affinity, electronegativity,
metallic character, acidic and basic characters of oxides and hydrides of the
representative elements (up to Z = 36). Position of hydrogen and the noble gases
in the periodic table; Diagonal relationships.
Chemical Bonding and Molecular Structure
Valence electrons, the Octet rule, electrovalent, covalent and coordinate
covalent bonds with examples; Properties of electrovalent and covalent
compounds. Limitations of Octet rule (examples); Fajan’s Rule. Directionality of
covalent bonds, shapes of poly-atomic molecules (examples); Concept of
hybridization of atomic orbitals (qualitative pictorial approach) : sp, sp2, sp3
and dsp2. Molecular orbital energy diagrams for homonuclear diatomic species –
bond order and magnetic properties.
Valence Shell Electron Pair Repulsion (VSEPR) concept
(elementary idea) – shapes of molecules. Concept of resonance (elementary idea),
resonance structures (examples). Elementary idea about electronegativity, bond
polarity and dipole moment, inter- and intra- molecular hydrogen bonding and its
effects on physical properties (mp, bp and solubility); Hydrogen bridge bonds in
Double salts and complex salts, co-ordination compounds
(examples only), co-ordination number (examples of co-ordination number 4 and 6
Measurable properties of gases. Boyle’s Law and Charles Law, absolute scale
of temperature, kinetic theory of gases, ideal gas equation – average, root mean
square and most probable velocities and their relationship with temperature.
Dalton’s Law of partial pressure, Graham’s Law of gaseous
diffusion. Deviations from ideal behavior.
Liquefaction of gases, real gases, van der Waal’s equation;
Chemical Energetics and Chemical Dynamics
Chemical Energetics – conservation of energy principle, energy changes in
physical and chemical transformations. First law of thermodynamics; Internal
energy, work and heat, pressure-volume work; Enthalpy. Internal energy change (ΔE)
and Enthalpy change (ΔH) in a chemical reaction. Hess’s Law and its applications
(Numerical problems). Heat of reaction, fusion and vapourization; Second law of
thermodynamics; Entropy; Free energy; Criterion of spontaneity.
Chemical Equilibria – The Law of mass action, dynamic
nature of chemical equilibria. Equilibrium constants, Le Chatelier’s Principle.
Equilibrium constants of gaseous reactions (Kp and Kc) and relation between them
(examples). Significance of ΔG and ΔG°.
Chemical Dynamics – Factors affecting the rate of chemical reactions
(concentration, pressure, temperature, catalyst). Arrhenius equation and concept
of activation energy. Order and molecularity (determination excluded); First
order reactions, rate constant, half-life (numerical problems), examples of
first order and second order reactions.
Physical Chemistry of Solutions
Colloidal Solutions – differences from true solutions; Hydrophobic and
hydrophilic colloids (examples and uses); Coagulation and peptization of
colloids; Dialysis and its applications; Brownian motion; Tyndall effect and its
applications; Elementary idea of emulsion, surfactant and micelle. Electrolytic
Solutions – Specific conductance, equivalent conductance, ionic conductance,
Kohlrausch’s law, Faraday’s laws of electrolysis, applications. Numerical
Non-electrolytic Solutions – Types of solution, vapour
pressure of solutions. Raoult’s Law; Colligative properties – lowering of vapour
pressure, elevation of boiling point, depression of freezing point, osmotic
pressure and their relationships with molecular mass (without derivations);
Ionic and Redox Equilibria
Ionic equilibria – ionization of weak electrolytes, Ostwald’s dilution law.
Ionization constants of weak acids and bases, ionic product of water, the pH –
scale, pH of aqueous solutions of acids and bases; Buffer solutions, buffer
action and Henderson equation. Acid-base titrations, acid-base indicators
(structures not required).
Solubility and Solubility Products.
Common ion effect (no numerical problems).
Redox Equilibria – Oxidation-Reduction reactions as electron transfer processes,
oxidation numbers, balancing of redox reactions by oxidation number and
ion-electron methods. Standard electrode potentials (E°), Electrochemical
series, feasibility of a redox reaction. Significance of Gibb’s equation : ΔG° =
– nFΔE° (without derivation), no numerical problems. Redox titrations with
(examples); Nernst equations (Numerical problems).
Chemistry of Non-metallic Elements and their Compounds
Carbon – occurrence, isotopes, allotropes (graphite, diamond, fullerene); CO
and CO2 production, properties and uses.
Nitrogen and Phosphorus – occurrence, isotopes, allotopes, isolation from
natural sources and purification, reactivity of the free elements. Preparation,
properties, reactions of NH3, PH3 , NO, NO2 , HNO2, HNO3, P4O10, H3PO3 and
H3PO4. Oxygen and Sulfur – Occurrence, isotopes, allotropic forms, isolation
from natural sources and purification, properties and reactions of the free
elements. Water, unusual properties of water, heavy water (production and uses).
Hydrogen peroxide and ozone (production, purification, properties and uses).
Halogens – comparative study, occurrence, physical states and chemical
reactivities of the free elements, peculiarities of fluorine and iodine;
Hydracids of halogens (preparation, properties, reactions and uses),
inter-halogen compounds (examples); Oxyacids of chlorine.
Chemistry of metals :
General principles of metallurgy – occurrence, concentration of ores,
production and purification of metals, mineral wealth of India. Typical metals
(Na, Ca, Al, Fe, Cu and Zn) – occurrence, extraction, purification (where
applicable), properties and reactions with air, water, acids and non-metals.
Manufacture of steels and alloy steel (Bessemer, Open-Hearth and L.D. process).
Principles of chemistry involved in electroplating, anodizing and galvanizing.
Chemistry in Industry
Large scale production (including physicochemical principles where
applicable omitting technical details and uses of individual items).
Heavy chemicals : Sulfuric acid (contact process),
Ammonia (Haber’s process), Nitric acid (Ostwald’s process), sodium bi-carbonate
and sodium carbonate (Solvey process). Polymers, Polythene, Nylon-66, rubber
from natural source, vulcanization. Electrochemicals – sodium hydroxide,
chlorine, bleaching powder as by-products. Fuel Gases – LPG, CNG.
Silicon carbide and silicones.
Common modes of pollution of air, water and soil. Ozone layer, ozone hole –
important chemical reactions. Green House effect; Smog; Pollution of water by
domestic and industrial effluents; Pollutants–pesticides, fertilizers and
Chemistry of carbon compounds
Hybridization of carbon – σ- and π-bonds.
Isomerism – constitutional and stereoisomerism; Geometrical
and optical isomerism of compounds containing upto two asymmetric carbon atoms.
IUPAC nomenclature of simple organic compounds– hydrocarbons, mono and
bifunctional molecules only (alicyclic and heterocyclic compounds excluded).
Conformations of ethane and n-butane (Newman projection only).
Electronic effects – inductive, resonance and
hyperconjugation. Stability of carbocation, carbanion and free radicals;
Rearrangement of carbocation; Electrophiles and nucleophiles, tautomerism in β-
dicarbonyl compounds, acidity and basicity of simple organic compounds.
Alkanes – Preparation from alkyl halides and carboxylic acids; Reactions –
halogenation and combustion.
Alkenes and Alkynes – Preparation by elimination of alcohols,
alkyl halides and quaternary ammonium hydroxides, Saytzeff and Hofmann rules;
Reactions – electrophilic addition of X2, HX, HOX, H2O (X = halogen), ozonolysis,
epoxidation and oxidation with KMnO4, OsO4 (stereochemistry of addition
excluded). Markownikoff’s and anti-Markownikoff’s additions; Hydroboration;
Oxymercuration – demercuration, reduction of alkenes and alkynes (H2/Lindler
catalyst and Na in liquid NH3), metal acetylides.
Alkyl halides – Preparation from alcohols; Formation of
Grignard reagents and their synthetic applications for the preparation of
alkanes, alcohols, aldehydes, ketones and acids; SN1 and SN2 reactions
Alcohols – Preparation from carbonyl compounds and esters.
Reaction – dehydration, oxidation, esterification, reaction with sodium, ZnCl2 /
HCl, phosphorous halides.
Ethers – Preparation by Williamson’s synthesis; Cleavage
with HCl and HI.
Aldehydes and Ketones – Preparation from esters, acid chlorides, gem-dihalides,
Ca-salt of carboxylic acids. Reaction – Nucleophilic addition with HCN,
hydrazine, hydroxyl amines, semi carbazides, alcohols; Aldol condensation,
Clemmensen and Wolff-Kishner reduction, haloform, Cannizzaro and Wittig
Carboxylic Acids – Hydrolysis of esters (mechanism
excluded) and cyanides; Hunsdicker and HVZ reactions.
Aliphatic Amines – Preparation from nitro, cyano and amido compounds.
Distinction of 1º, 2º and 3º amines (Hinsberg method); Reaction with HNO2;
Carbyl amine reaction.
Benzene – Kekule structure, aromaticity and Hückel rule. Electrophilic
substitution – halogenation, sulfonation, nitration, Friedel Crafts reaction,
ozonolysis. Directive influence of substituents in monosubstituted benzenes.
Amines – Preparation from reduction of nitro compounds;
Formation of diazonium salts and their stability; Replacement of diazonium group
with H, OH, X (halogen), CN and NO2, diazocoupling and reduction.
Haloarenes – Nucleophilic substitution, cine
substitution (excluding mechanism).
Phenols – halogenation, sulfonation, nitration, Reimer-Tiemann and Kolbe
Aromatic Aldehydes – Preparation by Gattermann, Gattermann – Koch,
Rosenmund and Stephen’s method. Reactions – Perkin, Benzoin and Cannizzaro.
Application Oriented chemistry
Main ingredients, their chemical natures (structures excluded) and their side
effects, if any, of common antiseptics, analgesics, antacids, vitamin-C.
Introduction to Bio-molecules
Carbohydrates – Pentoses and hexoses. Distinctive chemical reactions of
glucose. Aminoacids – glycine, alanine, aspartic acid, cysteine (structures).
Zwitterion structures of amino acids, peptide bond.
ADP and ATP – structures and role in bioenergetics; Nucleic
acids – DNA and RNA skeleton structures. Names of essential elements in
Principles of qualitative analysis
Detection of water soluble noninterfaring Acid and Basic Radicals by dry and
wet tests from among :
(a) Acid Radicals : Cl-, S2-, SO4
2-, NO– 3, CO3 2-
(b) Basic Radicals: Cu2+, Al3+, Fe3+, Fe2+,
Zn2+, Ca2+, Mg2+, Na+, NH4+
Detection of special elements (N, Cl, Br, I and S) in organic compounds by
chemical tests. Identification of functional groups in : phenols, aromatic
amines, aldehydes, ketones and carboxylic acids.