JKCET 2022 Chemistry Syllabus (Available) – Get Chemistry Syllabus PDF Here


The Jammu and Kashmir Board of Professional Entrance Examination (JKBPEE) will be organized the Jammu and Kashmir Common Entrance Test (JKCET 2022).

which is the state level entrance test and it is offering various professional courses to the candidates through this entrance examination known as JKCET 2022.

JKCET is conducted for taking admission into the Various Engineering Professional courses. JKCET will help the candidates to get admission into the B.Tech and B.E courses across the Jammu and Kashmir Union Territory.

JKCET 2022 Chemistry Syllabus 

JKCET Chemistry Syllabus 2022 will be released officially by the JKCET 2022 authority online. Students can download the JKCET 2022 syllabus into PDF format.

Unit 1:

Chemical Arithmetic & Atomic Structure (Marks: 03)

Laws of chemical combination, Mole concept (numerical) Percentage composition, Chemical reactions, Stoichiometry and calculations based on stoichiometry.

Atomic structure:-

Bohr’s model of the Hydrogen atom, Quantum numbers, Pauli’s exclusion principle, Hund’s rule, and Aufbau principle. Heisenberg’s uncertainty principle, the de-Broglie wave equation, and its significance.

Unit 2:

Chemical Equilibrium (Marks: 04)

Law of mass action, Le-Chatelier’s principle, and its application to physical and chemical equilibria. Ionization of weak electrolytes (Ostwald’s dilution law)

Acids and bases: Acid-base equilibria. Bronsted-Lowry and Lewis concept, of acids and bases.Ionic product of water.pH and pOH scales, pKa&pKb values, Solubility product, Buffer solutions Common ion effect, Hydrolysis of salts

Unit 3:

Chemical Kinetics (Marks: 02)

Rate of chemical reaction, Average and instantaneous rate, Factors affecting the rate of reaction, Order and molecularity of reaction, Integrated rate equation and Half-life period (for zero and first-order) reaction, Activation energy, and Arrhenius equation.

Unit 4:

Solutions (Marks: 02)

Vapour pressure, Raoult’s law, Ideal and Non-ideal solutions, Colligative properties. Determination of the molecular mass of non-volatile solutes through colligative properties. Abnormal molecular masses and Can’t Hoff Factor.

Unit 5:

Chemical Thermodynamics (Marks: 04)

Energy changes taking place during chemical reactions, Internal Energy and Enthalpy changes, Enthalpy of combustion, Solution, and Neutralization.

Hess’s Law (Numerical problems) Laws of thermodynamics-first, second & third, Concepts of Entropy and Free energy, Spontaneity of a chemical reaction and Thermodynamic equilibrium.

Unit 6:

Redox Reactions and Electrochemistry (Marks: 03)

Dependence of electrode and cell potential on concentration (Nernst Equation), Electrode potential as a criterion for product formation in electrolysis.

E.M.F. of Galvanic cell, Relationship between free energy change and E.M.F. of a cell.Definition and units of Equivalent, Molar, and Specific conductivity.

Unit 7:

Solid State & States Of Matter (Marks: 04)

Boyle’s Law, Charle’s law, Dalton’s law of partial pressure, Graham’s law of diffusion of gases. Causes of deviation from ideal behavior, ideal gas equation, and nature of ‘R’, Vander Waal’s equation, surface tension, and viscosity of liquids. Crystalline and amorphous solids, Crystal lattice, Crystal types, Packing efficiency, calculation of density of unit cell,

A number of atoms per unit cell in a cubic cell. Co-ordination number, Stoichiometric defects: Schottky, Frenkel, and interstitial. Properties of solids: Electrical, Magnetic & Dielectric.

Unit 8:

Surface Chemistry (Marks: 02)

Freundlich Adsorption isotherm, preparation of colloidal solutions by physical and chemical methods.Electrical properties (cataphoresis, electroosmosis, coagulation, and protective colloids) Homogeneous and Heterogeneous Catalysis.

Unit 9:

Periodic Properties (Marks: 02)

Classification of elements as s, p, d, and f block elements.Variation of Ionization energy, Electron affinity, Electronegativity, Atomic and Ionic radii along the period and down the group in the periodic table.

Unit 10:

Chemical Bonding and Molecular Structure (Marks: 04)

Types of chemical bonds, Ionic & covalent bonds, Bond parameters, Quantum theory of a covalent bond, pi and sigma bonds, Hybridization involving s, p, and d-orbitals, Dipole moments and hydrogen bond.

VSEPR: Shapes of simple molecules ( H2O, NH3, SO2, CO2, PCl3, PCl5, CIF3, BF3, SF4, XeF2, XeF4 ).

Molecular orbital theory: Energy Levels and M.O. diagrams of H2, H2+, He2, O2, O1- 2, O2 2-& F2. Bond order and its significance.

Unit 11:

Chemistry Of Representative Elements (Marks: 04)

S and P Block Elements: Electron configuration, Oxidation states, and trends in various properties like ionization energy, electron affinity, atomic radii, electronegativity, and diagonal relationship.

Alkali metals: Hydration of ions, action with ammonia, flame coloration, the solubility of hydroxides, carbonates, and sulfates.

Alkaline Earth Metals: Solubility of carbonates, hydroxides, and sulfates.

Boron Family: Structure of halides, relative acid strength of trihalides of boron.

Carbon family: Hydrides and oxides.

Nitrogen family: Oxides of Nitrogen and Phosphorous, reducing nature, basic strength, and boiling points of their halides.

Oxygen family: volatility, thermal stability, acid character, reducing character and bond angles of their hydrides, oxyacids of sulfur.

Halogen family: Bond energy, color, and oxidizing power, boiling point, acid strength and dipole moment, thermal stability, reducing the power of hydracids, relative acidity, and oxidizing power of oxyacids of halogens.

Unit 12:

Transition Elements Including Lanthanoids (Marks: 02)

Electron configuration, Oxidation states, Colour, and Magnetic properties. Oxides of Vanadium, Chromium and Manganese Alloys of Copper, Silver, and Iron. Metallurgy of Iron, Copper, and Zinc.

Unit 13:

Co-Ordination Chemistry (Marks: 04)

Introduction, Ligands, Co-ordination Number, IUPAC Nomenclature.

Bonding theories: Werner’s, VBT, and CFT.
Isomerism in Coordination compounds (Ionization, Linkage, Hydrate, Geometrical, and Optical). Applications of Coordination complexes in Biology, Medicine, and Analytical Chemistry.

Unit 14:

Nomenclature And Basic Concepts Inorganic Chemistry (Marks: 03)

Nomenclature of organic compounds (monofunctional and polyfunctional groups), inductive, electromeric resonance and hyperconjugation effects, reaction intermediates, carbocations, carbanions and free radicals with their general stability order, types of organic reactions (addition, substitution, elimination, and redox reactions), aromaticity on the basis
of Huckel rule. Ortho, meta, and para directing groups.

Unit 15:

Hydrocarbons (Marks: 03)

Structural isomerism in alkanes, alkenes, alkynes and arenas, stereoisomerism: geometrical and optical isomerism, chirality, the origin of chirality, specific rotation, racemization, and the resolution, conformations in ethane and cyclohexane, relative configuration (D, L- Nomenclature), absolute (R and S system of nomenclature).

Unit 16:

Organic Chemistry Based On Functional Group-I (Marks: 02)

Haloalkanes, haloarenes, alcohols, and phenols: General methods of preparation and
properties. Chloroform and Iodoform.

Unit 17:

Organic Chemistry Based On Function Group-Ii (Marks: 03)

Ethers, Aldehydes, Ketones, Monocarboxylic acids:

General methods of preparation and properties. Derivatives of monocarboxylic acids like acid halides, acid anhydrides acid amides and esters. The relative strength of carboxylic acids

Unit 18:

Organic Chemistry Based On Functional Group-Iii (Marks: 03)

Cyanides, Isocyanides, Nitrocompounds, and Amines: General methods of preparation and properties. The relative basic character of amines.

Unit 19:

Molecules Of Life (Marks: 03)

Carbohydrates: Definition, Classification, Mutarotation, Structure of Animo-acids, Peptides, and Proteins (Molish and ninhydrin tests). Classification and uses of vitamins.

Chemicals in medicine and health care, Dyes, and drugs. Chemical reactions in the atmosphere, ozone depletion, and its effects.Acid rain, Green House effect & Global warming.

Unit 20:

Polymers (Marks: 03)

Introduction, Classification, Methods of Polymerisation (Addition, Condensation, Free Radical, Cationic & Anionic). Natural & Synthetic Polymers: Polythene, Nylon, Polyester, Bakelite, and Rubber. Biodegradable and Non-Biodegradable Polymers.

If you have any other queries regarding JKCET 2022 Chemistry Syllabus, you can ask us by leaving your comment below.

Leave a comment