UP PGT Chemistry Syllabus 2026 PDF Download | UPSESSB Exam Pattern & Topics

UP PGT Chemistry Syllabus 2026

The comprehensive UP PGT Chemistry Syllabus 2026 encompasses essential domains including Physical, Organic, Inorganic, and Analytical Chemistry, providing a robust framework for mastery. The examination features 125 multiple-choice questions (MCQs) totaling 425 marks, with each question valued at 3.4 marks and a 2-hour completion window. Notably, there is no negative marking for the UP PGT Exam Date 2026. A strategic approach to this syllabus ensures optimized time management and improved accuracy, significantly increasing your competitive edge.

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UP PGT Chemistry Exam Pattern 2026

The UPSESSB UP TGT PGT Exam Pattern 2026 is conducted in an offline, pen-and-paper format comprising 125 MCQs. The TGT examination is evaluated out of 500 marks (4 marks per question), while the PGT examination is scored out of 425 marks (3.4 marks per question). Both assessments share a 2-hour duration and exclude negative marking, serving as the gateway for recruitment of teachers across Uttar Pradesh schools.

UP PGT Chemistry Marks Distribution 2026

Understanding the UP TGT PGT selection criteria is vital for strategic planning. For the PGT position, the final merit is determined by the written exam (425 marks/85%), the interview (50 marks/10%), and special qualifications (25 marks/5%), totaling 500 marks. In contrast, TGT selection relies exclusively on the written examination (500 marks/100%). This distinction underlines the significance of performance in the written test for both roles, with added weightage for PGT candidates possessing higher academic credentials.

UP PGT Chemistry Syllabus 2026 Detailed

The UP PGT Chemistry Syllabus 2026 is expertly curated to test advanced conceptual knowledge and practical application. Physical Chemistry segments cover thermodynamics, kinetics, electrochemistry, and states of matter. Inorganic Chemistry focuses on periodic trends, coordination chemistry, and transition metals, while Organic Chemistry emphasizes reaction mechanisms, stereochemistry, and biomolecules. This rigorous syllabus ensures candidates demonstrate the depth of knowledge required for high-level teaching roles.

(A) Physical Chemistry Syllabus:

• Gaseous State: Kinetic molecular theory of gases, Derivation of kinetic equation and verification of gas laws, Description of molecular velocities, Heat capacity of gases, Energy distribution law, Molecular collisions and transport phenomena, Mean free path and collision diameter, Non-ideal gases: van der Waals equation and other state equations, Law of corresponding states and Liquefaction of gases
• Liquid State: Intermolecular forces in liquids, Vapour pressure of liquids and its temperature dependence and Surface tension and viscosity of liquids and their temperature effects
• Solid State: Crystals: shape and symmetry, Space lattice and unit cell, Miller indices, Various crystal systems, Bragg’s equation, Crystal structure of sodium chloride, Packing of atoms in cubic systems and Bonding in solids and crystal defects
• Colloidal State: Lyophilic and lyophobic colloids, Formation and properties of colloids, Charge generation on colloidal particles, Coagulation and protection of colloids and Applications of colloids (aerosols, foams, emulsions)
• Molecular Structure: Dipole moment and molecular structure determination, Infrared and Raman spectroscopy and their application in molecular structure determination and Nuclear Magnetic Resonance (NMR) and Electron Spin Resonance (ESR) spectroscopy and their applications
• Thermodynamics and Thermochemistry: Zeroth and First Law of Thermodynamics, Enthalpy and internal energy, Applications of the First Law of Thermodynamics, Work done by an ideal gas in isothermal and adiabatic expansions, Joule-Thomson coefficient, Reaction enthalpies (combustion, formation, neutralization, phase change, and sublimation), Hess’s Law and its applications and Bond energy
• Second Law of Thermodynamics: Carnot cycle, Entropy and its physical concept and Entropy changes in reversible and irreversible processes
• Free Energy (Gibbs and Helmholtz): Maxwell’s relations, Partial molar quantities (chemical potential), Gibbs-Duhem relation and Clausius-Clapeyron equation and Gibbs-Helmholtz equation
• Molecular Thermodynamics: Partition function and its importance, Relationship between partition function and thermodynamic properties and Translational, rotational, vibrational, and electronic partition functions of ideal gases
• Surface Chemistry: Physical and chemical adsorption, Langmuir adsorption isotherm and BET equation and its applications
• Photochemistry: Primary and secondary processes, Einstein’s law of photochemical equivalence, Phosphorescence and fluorescence, Photochemical decomposition of hydrogen iodide and Chemical lasers
• Catalysis: Homogeneous and heterogeneous catalysis, Theory of heterogeneous catalysis and Enzyme catalysis
• Solutions: Ideal and non-ideal solutions, Raoult’s Law, Colligative properties (osmotic pressure, vapor pressure lowering, boiling point elevation, freezing point depression) and Determination of molecular weight from colligative properties
• Nuclear Chemistry: Fundamental particles and their classification, Nuclear forces, Liquid drop and shell models of atomic nuclei, Nuclear stability, Energy changes in nuclear reactions, Concept of nuclear cross-section and Nuclear fission, spallation, and fusion reactions
• Chemical Kinetics: Order and molecularity of reactions, Rate laws for first and second-order reactions, Temperature dependence of rate constants (Arrhenius equation), Methods for determining reaction order and Transition state theory
• Chemical Equilibrium: Relationship between Kp and Kc, Decomposition of phosphorus pentachloride, Formation of HI and NH3, Decomposition of CaCO3 and NH4HS and Le Chatelier’s principle and its applications
• Electrochemistry: Electrical conductivity, Arrhenius theory of electrolytic dissociation, Ostwald’s dilution law, Theory of strong electrolytes, Debye-Hückel-Onsager equation, Determination of conductance and its applications, Kohlrausch’s law of independent migration of ions, Electrochemical cells, Nernst equation and standard electrode potentials, Measurement of EMF and its applications, Fuel cells, Ionic equilibria (solubility product, hydrolysis of salts, pH, buffer solutions, acid-base indicators)

(B) Inorganic Chemistry Syllabus:

• Atomic Structure: Wave-particle duality, Heisenberg uncertainty principle, Schrödinger wave equation, Atomic orbitals, Quantum numbers, Shapes of s, p, and d orbitals, Aufbau principle, Pauli’s exclusion principle, Hund’s rule, Electronic configuration of elements and Periodic table and periodic properties (atomic and ionic radii, ionization energy, electron affinity, electronegativity)
• Chemical Bonding: Ionic bonding (lattice energy, Born-Haber cycle, salvation energy), Covalent bonding (hybridization, molecular orbital theory) and VSEPR theory and molecular shapes of NH3, H3O+, SF6, and IF7
• s-Block Elements: General characteristics, Chemistry of lithium and beryllium, Diagonal relationships
• p-Block Elements: General properties, Oxides and oxyacids of nitrogen, phosphorus, and sulfur, Phosphazenes, silicates, and silicones and Diboranes, interhalogens, and polyhalides
• d-Block Elements: Characteristics of 3d, 4d, and 5d transition metals, Coordination compounds (Werner’s theory, IUPAC nomenclature, isomerism, metal-ligand bonding), Crystal field theory (crystal field splitting in tetrahedral and octahedral complexes, CFSE, magnetism) and Electronic spectra of transition metal complexes
• Lanthanides and Actinides: Electronic configuration, Oxidation states, Separation techniques, and Magnetic and spectroscopic properties
• Bioinorganic Chemistry: Role of alkali and alkaline earth metal ions in biological systems and Metal porphyrins (hemoglobin and myoglobin)

(C) Organic Chemistry Syllabus:

• General Organic Chemistry: Orbital representation of methane, ethane, ethene, ethyne, and benzene, Polarization of bonds (inductive, resonance, and steric effects), Acidity and basicity of organic compounds, Nucleophilic and electrophilic substitutions, additions, and eliminations and Isomerism (structural and stereoisomerism)
• Important Functional Groups: Alkyl halides, alcohols, aldehydes, ketones, carboxylic acids, and their derivatives, Preparation and reactions of Grignard reagents and Keto-enol tautomerism
• Carbohydrates: Classification and Ring structure and mutarotation of glucose and fructose
• Aromatic Compounds: General methods of preparation and Electrophilic substitution reactions (nitration, halogenation, sulfonation, Friedel-Crafts reactions)

UP PGT Chemistry Syllabus 2026 PDF

Utilize the table provided below to download the official UP PGT Chemistry Syllabus PDF. A thorough review of these topics before commencing your preparation will allow you to prioritize core areas and maintain a disciplined, efficient study schedule for optimal results.