WEST BENGAL JOINT ENTRANCE EXAMINATIONS BOARD
SYLLABUS FOR JEM
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;
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 Hund’s Rule.
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 only).
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; Numerical