Central Universities Common Entrance Test [CUCET] 2012 : Syllabus – M. Sc. Chemistry (MSC)
M. Sc. Chemistry (MSC)
(Offered by CU Rajasthan)
The Question paper will have common Part A and subject specific Part B
Part A: It will be of 45 minutes duration and will have 35 Multiple Choice Questions (MCQs),
with four options: only one correct. Part A is intended to test the applicants; general
awareness, reasoning, basic language skills (English) and analytical skills.
Part B: will be subject specific, of 75 minutes duration and will have 65 MCQs with four
Options: only one correct.
Syllabus / Topics for Subject Specific Part B:
(a) Inorganic Chemistry
1. Periodic table: Periodic classification of elements, periodicity in properties. General methods of
isolation and purification of elements.
2. Chemical bonding: Types of bonding. VSEPR theory and shapes of molecules. Hybridization, VBT
and MOT of simple molecules, dipole moment. Ionic solids - lattice energy. Structure of diamond and
3. Main group elements (s and p block elements): Chemistry with emphasis on group relationship and
gradation in properties; structure of electron deficient compounds of main group elements and application
of main group elements.
4. Transition and inner transition elements (d and f block elements): Characteristics of d- and f-block
elements. Coordination compounds of first row transition elements, bonding in coordination compounds
– VBT and CFT of tetrahedral and octahedral complexes. Application of CFT to spectral and magnetic
properties. Electronic spectra of coordination compounds.
5. Organometallic compounds: Concept of hepticity, 18 electron rule. Carbonyl compounds of first row
of transition metals.
6. Non aqueous solvents: General characteristics, reactions with reference to ammonia and liquid
7. Acids and Bases: Lewis and HSAB concepts
8. Nuclear Chemistry: Radioactivity, nuclear reactions, applications of isotopes.
(b) Organic Chemistry
1. Nomenclature of Organic compounds.
2. Mechanism of Organic reactions: Electronic effects in Organic molecules – polarization effect
(Inductive effect), polarizability effect (Electromeric effect), resonance, hyperconjugation. Formal
charge. Generation, structure and general reactions of reactive intermediates –Carbocation, carbanion,
3. Stereochemistry: Types of isomerism. Projection formulae, chirality, assigning stereochemical
descriptors to chiral centres and geometric isomers. Optical isomerism in compounds containing one and
two asymmetric centres. Conformations of cyclohexanes.
4. Aromaticity and Huckel’s rule: Mono and bicyclic carbocyclic aromatic hydrocarbons and their
electrophilic substitution reactions.
5. Synthetic chemistry: Methods of preparation and characteristic reactions of alkanes, alkenes,
alkynes (including their cyclic analogues), arenes and their simple functional derivatives, such as alkyl,
halo, nitro, hydroxyl, alkoxy, formyl, amino, carbonyl, carboxyl (and carboxylic acid derivatives).
Functional group interconversions. Grignard reagents, acetoacetic and malonic ester chemistry. Synthesis
of simple compounds. Structure determination and synthetic problems using chemical reactions.
6. Mechanism (with stereochemistry): Aliphatic nucleophilic substitution, elimination, enolate reactions,
Claisen condensation, esterification and ester hydrolysis, Cannizzaro reaction, benzoin condensation,
Perkin reaction, Claisen rearrangement, Beckmann rearrangement, Wagner-Meerwein rearrangement.
7. Carbohydrates: Classification, nomenclature. Open and cyclic formulae. Chemistry of glucose.
8. Amino acids and peptides: Structure, stereochemistry, and characteristics reactions of amino acids.
Structure of peptides.
9. Heterocyclic chemistry: Monocyclic 5-membered heteroaromatic compounds with one hetero atom
(S,O,N) and pyridine. Their nomenclature, electronic structure, aromaticity, characteristic properties and
(c) Physical chemistry
1. Atomic structure: Fundamental particles. Bohr’s theory of hydrogen atom; Wave-particle duality;
Uncertainty principles; Schrodinger’s wave equation; Quantum numbers, shapes of orbitals; Hund’s rule
and Pauli’s exclusion principle. Idea of electromagnetic spectrum.
2. Theory of gases: Kinetic theory of gases. Real and ideal gases, critical phenomenon.
3. Chemical thermodynamics: Reversible and irreversible processes. First law and its application to
ideal and nonideal gases. Thermochemistry. Second law. Entropy and free energy, Criteria for
4. Chemical and Phase equilibria: Law of mass action; Kp , Kc, Kx and Kn ; Effect of temperature on
K; Ionic equilibria in solutions; pH and buffer solutions; Hydrolysis; Solubility product; Phase equilibria–
Phase rule and its application to one-component and two-component systems; Colligative properties.
5. Electrochemistry: Conductance and its applications; Transport number; Galvanic cells; types of
electrodes, EMF and Free energy. Liquid junction potential and concentration cells. Application of emf
measurement for determination of K, ΔG, ΔH, ΔS. Stability of complexes and determination of
6. Chemical kinetics: Reactions of various order, Arrhenius equation, Collision theory; Theory of
absolute reaction rate; Chain reactions - Normal and branched chain reactions; Enzyme kinetics;
Photophysical and photochemical processes; Catalysis.
7. Quantum chemistry: Black body radiation, Elementary quantum chemistry, state function, operators,
eigen values and eigen functions.
(d) Analytical Chemistry
Classification of analytical methods. Performance characteristics of analytical methods. Errors and their
types. Acid-base titrations and acid-base indicators, redox titrations, precipitation and complexometric
titrations, conductometric and potentiometric titrations. Basics of UV-VIS spectroscopy, Lambert-Beers
Sample Questions (Part B)
(1) The strongest acid among the following is –
(A) HCOOH (B) Cl3C-COOH (C) CH3-COOH (D) Br3C-COOH
(2) The species having tetrahedral shape is –
(A) [PdCl4]2- (B) [Ni(CN)4]2- (C) [Pd(CN)4]2- (D) [NiCl4]2-
(3) The hybridization of sulphur atom in sulphur hexafluoride is –
(A) sp3 (B) sp3d (C) sp2 (D) sp3d2
(4) The IUPAC name of the following compound is
(A) pentyl methanoate (B) methyl 4-oxohexanoate
(C) 2,5-heptanedione (D) methyl pentanoate-3-one
(5) The rate of a reaction doubles when the temperature is changed from 300K to 310 K. Hence, energy
of activation of the reaction is -
(A) 40kJ (B) 53.5 kJ (C) 48kJ (D) 56 kJ
(6) Change in entropy is defined as dS = dqrev/T, bacause
(A) entropy is a state function
(B) q is not a state function
(C) the path followed by the system is a reversible path
(D) entropy is a state function and hence entropy change is always calculated assuming the system follows a reversible path.
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