NTA CUET (PG) 2023 syllabus for chemistry

Are you looking for CUET (PG) chemistry syllabus for admission in Msc courses of various central universities ? Here you will get CUET (PG) syllabus of chemistry in details as provided by NTA on their official website . Below we have provided the NTA CUET (PG) chemistry syllabus in a easy and explained way so that it would be easier for applicants to understand . The syllabus is a first step to start preparation of any exam by understanding the areas which you need to study .

NTA CUET (PG) 2023 syllabus for chemistry
NTA CUET (PG) 2023 syllabus for chemistry

CUET (PG) stands for common university entrance test for postgraduate courses , It is a national level examination for candidates looking for admission in postgraduate (PG) courses of various central universities . The Common University Entrance Test (CUET) will provide a common platform and equal opportunities to candidates across the country . The CUET exam is a computer based test (CBT) taken only on computer at NTA centers you choose in your application form .

In CUET (PG) chemistry domain knowledge exam there will be 75 questions given in your questions paper . For every correct answer you will get 4 marks , for every incorrect answer 1 marks will be deducted as negative marking .For Un-answered/un-attempted response will be given no marks. Te exam is conducted of total 300 marks . The exam can be given in english or hindi language based on your choice .

CUET (PG) official Chemistry syllabus p,df download

The syllabus is divided into physical , organic , inorganic chemistry as follows :


Quantum numbers and their significance. s, p, d, f block elements, the long form of periodic table. Detailed discussion of the following properties of the elements, with reference to s & p-block. Effective nuclear charge, shielding or screening effect, Slater rules, variation of effective nuclear charge in periodic table. General characteristics, types of ions, size effects, radius ratio rule and its limitations. Packing of ions in crystals. Born-Landé equation with derivation and lattice energy. Madelung constant, Born-Haber cycle and its application, solvation energy. Lewis structure, Valence Bond theory, Molecular orbital theory. Formal charge, Valence shell electron pair repulsion theory (VSEPR), Redox equations, Standard Electrode Potential and its application to inorganic reactions.

Bronsted-Lowry concept of acidbase reactions, solvated proton, relative strength of acids, types of acid-base reactions, levelling solvents, Lewis acid-base concept, Classification of Lewis acids, Hard and Soft Acids and Bases (HSAB) Application of HSAB principle. Inert pair effect, diagonal relationship Allotropy and catenation. Complex formation tendency of s and p block elements. Study of the compounds with emphasis on structure, bonding, preparation, properties and uses.

Boric acid and borates, boron nitrides, borohydrides (diborane) carboranes and graphitic compounds, silanes, oxides and oxoacids of nitrogen, Phosphorus and chlorine. Peroxo acids of Sulphur, interhalogen compounds, polyhalide ions, pseudo halogens and basic properties of halogens. Werner’s theory, valence bond theory (inner and outer orbital complexes), electro neutrality principle and back bonding. Crystal field theory, measurement of 10 Dq (Δo), CFSE in weak and strong fields, pairing energies, factors affecting the magnitude of 10 Dq (Δo, Δt). Octahedral vs. tetrahedral coordination, tetragonal distortions from octahedral geometry Jahn-Teller theorem, square planar geometry. Qualitative aspect of Ligand field and MO Theory.


Intensive and extensive variables; state and path functions; isolated, closed and open systems; zeroth law of thermodynamics. First law: Concept of heat, q, work, w, internal energy, U, and statement of first law; enthalpy, H, relation between heat capacities, calculations of q, w, U and H for reversible, irreversible and free expansion of gases (ideal and van der Waals) under isothermal and adiabatic conditions. Heats of reactions: standard states; enthalpy of formation of molecules and ions and enthalpy of combustion and its applications; calculation of bond energy.

Second Law: Concept of entropy; thermodynamic scale of temperature, statement of the second law of thermodynamics; molecular and statistical interpretation of entropy. Calculation of entropy change for reversible and irreversible processes. Third Law: Statement of third law, concept of residual entropy, calculation of absolute entropy of molecules. Free Energy Functions: Gibbs and Helmholtz energy; variation of S, G, A with T, V, P; Free energy change and spontaneity. Relation between Joule-Thomson coefficient and other thermodynamic parameters; inversion temperature. Miller indices, elementary ideas of symmetry, symmetry elements and symmetry operations, qualitative idea of point and space groups, seven crystal systems and fourteen Bravais lattices.

Ionization of weak acids and bases, pH scale, common ion effect, Salt hydrolysis-calculation of hydrolysis constant, degree of hydrolysis and pH for different salts. Buffer solutions; derivation of Henderson equation and its applications; buffer capacity, buffer range. Kinetic molecular model of a gas: postulates and derivation of the kinetic gas equation; collision frequency. Maxwell distribution and its use in evaluating molecular velocities (average, root mean square and most probable) and average kinetic energy. Order and Molecularity of a reaction, rate laws in terms of the advancement of a reaction, differential and integrated form of rate expressions up to second order reactions, experimental methods of the determination of rate laws, kinetics of complex reactions.


Hemolytic and Heterolytic fission with suitable examples. Curly arrow rules, formal charges; Electrophiles and Nucleophiles; Nucleophlicity and basicity; Types, shape and their relative stability of Carbocations, Carbanions, Free radicals and Carbenes. Introduction to types of organic reactions and their mechanism: Addition, Elimination and Substitution reactions.

Fischer Projection, Newman and Sawhorse Projection formulae and their inter conversions; Geometrical isomerism: cis–trans and, synanti isomerism E/Z notations with C.I.P rules. Optical Isomerism: Optical Activity, Specific Rotation, Chirality/Asymmetry, Enantiomers, Molecules with two or more chiral-centres, Distereoisomers, meso structures, Racemic mixture and resolution. Relative and absolute configuration: D/L and R/S designations


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