Madhya Pradesh Public Service Commission
Syllabus For Chemistry Mains Examination (Optional)
CHEMISTRY ( CODE NO. 05 )
PAPER - I
Symmetry elements and symmetry operations. Recognition of symmetry point group
and symmetry elements in AB2 and AB3 molecules.
2. Atomic structure
Idea of de Broglie matter waves. Heisenberg's uncertainity principle,
Schrodinger wave equation (time independent). Significance of ? and ? 2,
particle in one- imensional box, quantum numbers, radial and angular wave
functions, shapes of s. p, d and orbitals, Aufbau principle, Hund's multiplicity
rule, Pauli exclusion principle. Effective nuclear charge.
3. Chemical bonding
Ionic bond, percent ionic character from dipole moment and electronegativity
difference, characteristics of ionic compounds, factors affecting stability of
ionic compounds, lattice energy, Born- Haber cycle; covalent bond and its
general characteristics, polarities of bonds in molecules and their dipole
moments. Valency bond theory, concept of resonance and resonance energy.
Molecular orbital theory (LCAO method); bonding in homonuclear and heteronuclear
molecules: H2+, H2 to Ne2, NO, CO. The concept of hybridization, character of
bonds, bond angles and bond length. Hydrogen bonding and van der Waals forces.
4. Solid State
Forms of solids, law of constancy of interfacial angles, crystal systems and
crystal classes (crystallographic groups). Designation of crystal faces, lattice
structures and unit cell. Laws of rational indices. Bragg's law. X-ray
diffraction by crystals. Close packing, radious ratio rules, calculation of some
limiting radius ratio values. Structures of NaCl, CsCl, and KCl. crystal
Imperfections in crystals. Elementary study of liquid crystals.
Thermodynamic systems, states and processes, work, heat and internal energy;
first law of thermodynamics, work done on the systems and heat absorbed in
different types of processes;calorimetry, energy and enthalpy changes in various
processes and their temperature dependence. Second law of thermodynamics;
entropy as a state function, entropy changes in various process,
entropy–reversibility and irreversibility, Free energy functions; criteria for
equilibrium, relation between equilibrium constant and thermodynamic quantities;
Nernst heat theorem and third law of thermodynamics. Thermodynamics derivations
of - Gibbs- Helmholtz equation, law of mass action and Clapeyron-Clausius
Conductivity and its applications to determine - Dissociation constant of weak
electrolyte Solubility product of sparingly soluble salts Conductrometric
titration. Debye-Huckel theory of strong electrolytes. Galvanic cells,
concentration cells; electrochemical series, measure - ment of e.m.f. of cells,
fuel cells and batteries. Processes at electrodes; double layer at the interface
of metal and solvent; rate of charge transfer, current density; overpotential.
7. Chemical kinetics
Concentration dependence of rate of reaction; defferential and integral rate
equations for zeroth, first, and second order of reactions. Effect of
temperature and pressure on rate constant. Collisions and transition state
Absorption of light; decay of excited state by different routes; photochemical
reactions between hydrogen and halogens and theirquantum yields.
9. Surface phenomena and catalysis
Absorption from gases and solutions on solid adsorbents,
Freundlich and Langmuir adsorption isotherm; determination of surface area,
characteristics and mechanism of reaction on heterogeneous catalysts.
10. Bio-inorganic chemistry
Essential and trace elements in biological processes, metalloporphyrins with
special reference to haemoglobin and myoglobin. nitrogen fixation, oxygen-uptake
proteins, cytochromes and ferredoxins. Biological role of alkali and alkaline
earth metal ions.
11. Coordination chemistry
(1) Introduction to bonding theories in transition metal complexes:Valency bond
theory, crystal field theory, Ligand field theory
and molecular orbital theory.
(2) Magnetic properties of transition metal complexes:
Magnetic moment (spin only and with L-S coupling), orbital contribution to
(3) Electronic spectra of transition metal complexes:
Spectroscopic ground and excited states, types of electronic transitions,
selection rules for d-d transitions. Spectrochemical series. Orgel-energy level
diagram for d1 to d9 states.
(4) Isomerism in coordination compounds. IUPAC nomenclature
of coordination compounds; stereochemistry of complexes with 4, 5 and 6
coordination numbers; chelate effect and polynuclear complexes; trans effect and
its theories; thermodynamic and kinetic stability of complexes.
(5) Organometallic chemistry: Synthesis, structure and
bonding in metal carbonyl complexes, metal olefin complexes and metal alkyne
complexes. Oxidative addition reactions.
12. General chemistry of inner transition elements
Lanthanides and actinides: Occurrence, separation, oxidation states and magnetic
properties; lanthanide contraction.
CHEMISTRY (CODE NO. 05 )
PAPER - II
1. Reaction mechanisms
General methods (both kinetic and non-kinetic) of study of mechanism of organic
reactions illustrated by examples–use of isotopes, intermediate trapping,
stereochemistry; energy diagrams of simple organic reactions–transition states
and intermediates; energy of activation; thermodynamic control and kinetic
control of reactions.
2. Reactive intermediates
Generation, geometry, stability and reactions of carbonium ions, carbanions,
free radicals, carbenes and benzynes.
3. Name reactions
Aldol condensation, Claisen condensation, Perkin reaction, Knoevenagel reaction,
Wittig reaction, Wolff-Kishner reduction, Cannizzaro reaction and von Richter
reaction; benzoin condensation; Fischer indole synthesis, Skraup synthesis,
Sandmeyer reaction, Reimer-Tiemann reaction and Reformatsky reaction.
4. Synthetic polymers
Addition or chain growth polymerization free radical vinyl polymerization, ionic
vinyl polymerization, Ziegler-Natta polymerization, viryl polymerization
Condensation or step growth polymerization. Polyesters, polyamides,
phenol-formaldehyde resins, urea-formaldehyde resins, epoxy resins.
Photochemical reactions of simple organic compounds, excited and ground states,
singlet and triplet states, Jablonski diagram. Fluorescence and phosphorescence.
Quantum yield and energy transfer process.
6. Organic spectroscopy
Problems pertaining to the structure elucidation of simple organic compounds
using UV-visible, IR and NMR spectroscopy.7. Heterocyclic compounds Molecular
orbital picture and aromatic characteristic of pyrrole, furane, thiophene and
pyridene. Methods of synthesis and chemical reactions with particular emphasis
on the mechanism of electrophilic substitution. Comparison of basicity of
pyridene, piperidene and pyrrole. Preparation and reactions of indole, quinoline
8. Stereochemistry of carbon compounds
Elements of symmetry, chiral and achiral compounds. Fischer projection formulae;
optical isomerism of lactic and tartaric acids, enantiomerism and
diastereoisomerism; configuration (relative and absolute); conformations of
ethane and n-butane, and cyclohexane. D, L-and R, S-notations of compounds
containing chiral centres; projection formulae-Fischer, Newman and Sawhorse of
compounds containing two adjacent chiral centres; meso and dl-isomers, erythro
and threo isomers; racemization nd resolution; geometrical isomers; E and Z
9. Organometallic compounds
Preparation and synthetic uses of Grignard reagents, alkyl lithium compounds.
10. Active methylene compounds
Diethyl malonate and ethyl acetoacetate-applications in organic synthesis;
11. Analytical chemistry
Errors in quantitative analysis, classification of errors, minimization of
errors, precision and accuracy, significance of figures, coprecipitation and
post-precipitation, optimum conditions for precipitation, choice of indicators
in the acid –base titration, theories of indicators, principle of EDTA
titration. Numerical questions on Quantitative estimation of pyrolusite,
iodometry, silver coin, acidbase titration, redox titration.