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Physical Chemistry JEE

Physical Chemistry is the unit with the highest weightage among all of chemistry and is a very calculation-oriented unit. The fundamentals are required to be coupled with formulas to be able to score well. Alongside, practice and revision are even more important because it requires speed to solve problems by recognizing patterns quickly. Some of the important chapters in this unit are Stoichiometry, Thermodynamics & Thermochemistry, Electrochemistry, and Equilibrium, specifically Ionic Equilibrium. Atomic Structure has a close resemblance with Atomic Physics and thus is naturally important. A total of 137 questions have been asked between 2010 and 2020.

Physical Chemistry JEE Chapter Wise Overview

Number of questions asked in each chapter of Physical Chemistry JEE from 2010 to 2020 in JEE


JEE Chemistry Chapter-wise weightage of Physical Chemistry 2020

Let's find out the chapter-wise weightage of the Unit Physical Chemistry

Chapters Weightage
STOICHIOMETRY Mole Concepts 3.33
Atomic Structure 3.5
States of Matter & Solutions 7.6
Thermodynamics 3.8
Equilibrium 3.6
Redox & Electrochemistry 3.0
Chemical Kinetics 3.6
Surface Chemistry 5.8


List of important topics for Physical Chemistry JEE

  • Mole concept & Stoichiometry
  • Dual nature of Radiation
  • Atomic Spectra
  • Bohr's Model for Hydrogen
  • States of Matter (Gases, Liquids & Solids)
  • Kinetic Theory of Gases
  • Crystal Lattice and Unit cells
  • Close packed structures and voids
  • Vapour Pressure of a solution
  • Colligative properties of Solutions
  • Law of Chemical equilibrium
  • Acids, Bases and Concept of pH
  • Hydrolysis of Salts
  • Buffer solutions & Crystal field theory
  • Redox Reactions
  • Conductance of Electrolytic Solutions
  • Chemical Kinetics
  • Radioactivity and Nuclear Reactions (Fission & Fusion)
  • Types and Isotherms
  • Catalysis

Physical Chemistry JEE Syllabus 2023,2024

  • Matter and its nature, Dalton's atomic theory: Concept of atom, molecule, element and compound: Physical quantities and their measurements in Chemistry, precision and accuracy, significant figures.
  • S.I.Units, dimensional analysis: Laws of chemical combination
  • Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae: Chemical equations and stoichiometry.
  • Classification of matter into solid, liquid and gaseous states.
  • Gaseous State: Measurable properties of gases: Gas laws - Boyle's law, Charle’s law.
  • Graham's law of diffusion.
  • Avogadro's law, Dalton's law of partial pressure
  • Concept of Absolute scale of temperature
  • Ideal gas equation
  • Kinetic theory of gases (only postulates)
  • Concept of average, root mean square and most probable velocities
  • Real gases, deviation from Ideal behaviour, compressibility factor and van der Waals equation.
  • Liquid State: Properties of liquids - vapour pressure, viscosity and surface tension and effect of temperature on them (qualitative treatment only).
  • Solid State: Classification of solids: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea)
  • Bragg's Law and its applications: Unit cell and lattices, packing in solids (fcc, bcc and hcp lattices), voids, calculations involving unit cell parameters, an imperfection in solids
  • Electrical and magnetic properties.
  • Thomson and Rutherford atomic models and their limitations
  • Nature of electromagnetic radiation, photoelectric effect
  • Spectrum of the hydrogen atom.
  • Bohr model of a hydrogen atom - its postulates, derivation of the relations for the energy of the electron and radii of the different orbits, limitations of Bohr's model
  • Dual nature of matter, de Broglie's relationship
  • Heisenberg uncertainty principle
  • Elementary ideas of quantum mechanics, quantum mechanics, the quantum mechanical model of the atom, its important features.
  • Elementary ideas of quantum mechanics, quantum mechanics, the quantum mechanical model of the atom, its important features.
  • Concept of atomic orbitals as one-electron wave functions: Variation of  and 2 with r for 1s and 2s orbitals; various quantum numbers (principal, angular momentum and magnetic quantum numbers) and their significance
  • Shapes of s, p and d - orbitals, electron spin and spin quantum number: Rules for filling electrons in orbitals – Aufbau principle.
  • Pauli's exclusion principle and Hund's rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals.
  • Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes.
  • The first law of thermodynamics - Concept of work, heat internal energy and enthalpy, heat capacity, molar heat capacity
  • Hess’s law of constant heat summation
  • Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization and solution.
  • The second law of thermodynamics - Spontaneity of processes; S of the universe and G of the system as criteria for spontaneity. G (Standard Gibbs energy change) and equilibrium constant.
  • Different methods for expressing the concentration of solution - molality, molarity, mole fraction, percentage (by volume and mass both), the vapour pressure of solutions and Raoult's Law - Ideal and non-ideal solutions, vapour pressure - composition, plots for ideal and non-ideal solutions
  • Colligative properties of dilute solutions - a relative lowering of vapour pressure, depression of freezing point, the elevation of boiling point and osmotic pressure
  • Determination of molecular mass using colligative properties
  • Abnormal value of molar mass, van’t Hoff factor and its significance.
  • Meaning of equilibrium, the concept of dynamic equilibrium.
  • Equilibria involving physical processes: Solid-liquid, liquid - gas and solid-gas equilibria, Henry's law. General characteristics of equilibrium involving physical processes. Equilibrium involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of G and G in chemical equilibrium, factors affecting equilibrium concentration, pressure, temperature, the effect of catalyst Le Chatelier’s principle. Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius. Bronsted - Lowry and Lewis) and their ionization, acid-base equilibria (including multistage ionization) and ionization constants, ionization of water. pH scale, common ion effect, hydrolysis of salts and pH of their solutions, the solubility of sparingly soluble salts and solubility products, buffer solutions.
  • Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, balancing of redox reactions.
  • Electrolytic and metallic conduction, conductance in electrolytic solutions, molar conductivities and their variation with concentration: Kohlrausch’s law and its applications.
  • Electrochemical cells - Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half - cell and cell reactions, emf of a Galvanic cell and its measurement: Nernst equation and its applications
  • Relationship between cell potential and Gibbs' energy change: Dry cell and lead accumulator Fuel cells.
  • Rate of a chemical reaction, factors affecting the rate of reactions: concentration, temperature, pressure and catalyst
  • Elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units, differential and integral forms of zero and first-order reactions, their characteristics and half-lives, the effect of temperature on the rate of reactions
  • Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions (no derivation).
  • Adsorption- Physisorption and chemisorption and their characteristics, factors affecting adsorption of gases on solids - Freundlich and Langmuir adsorption isotherms, adsorption from solutions.
  • Catalysis - Homogeneous and heterogeneous, activity and selectivity of solid catalysts, enzyme catalysis and its mechanism.
  • Colloidal state- distinction among true solutions, colloids and suspensions, classification of colloids - lyophilic.
  • Lyophobic; multimolecular, macromolecular and associated colloids (micelles), preparation and properties of colloids - Tyndall effect.
  • Brownian movement, electrophoresis, dialysis, coagulation and flocculation: Emulsions and their characteristics.

Physical Chemistry JEE Video Lectures


Physical Chemistry JEE Books

List of Chapters of Physical Chemistry  
1-Mole Concept Download
2-Atomic Structure Download
3-Gases and Liquid Download
4-Dilute solutions Download
5-Solid State Download
6-Energetics Download
7-Chemical Kinetics Download
8-Equilibrium Download
9-Redox and Electrochemistry Download
10-Surface chemistry Download

Physical Chemistry JEE Test Series 2022,2023,2024

List of FREE Modern Physics & Electronics JEE Tests  
Paper set 1 (Easy) Download Questions Download Solutions
Paper set 2 (Moderate) Download Questions Download Solutions
Paper set 3 (Difficult) Download Questions Download Solutions

Question on Physical Chemistry For JEE Mains And Advanced 2022, 2023, 2024

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If 0.5 mole of  is mixed with 0.20 mole of , the maximum number of moles of  then can be formed is


The following diagram shows the arrangement of lattice points with  and . Choose the correct options


The solutions in which the blood cells retain their normal shape, with regard to the blood, are


The  for andare, and, respectively. The standard enthalpy change (in ) for the reaction



Which of the following will not change the concentration of ammonia in the equilibrium


Q. Is physical chemistry easy for JEE?

For the students who are good in maths, physical chemistry is their favourite, since it does not require memorization like Inorganic and organic. If your basics are clear you can score 100% in physical chemistry.

Q. Is physical chemistry important?

Yes, every year 12 to 15 questions are asked from physical chemistry in JEE. In physical chemistry Mole concept, thermodynamics, electrochemistry, ionic equilibrium and solid-state are important.

Q. Is NCERT enough for physical chemistry for jee?

30% of the syllabus asked in JEE are directly from NCERT level so you cannot skip it, but for the remaining 70%, NCERT will be of no use. So just being completely dependent on NCERT is not going to help you get a good rank in JEE. JEE will ask you concepts beyond NCERT so we will advance you to use other books to practice JEE level questions.

Q. How to study physical chemistry for jee main?

start with NCERT since that will give you an idea about the list of topics to be covered follow by topic by solving JEE level questions from books, you can also use kaysons practice platform since we have over 30000 questions along with solutions and doubt clearing for you to practice.

Q. Which all chapters are there in physical chemistry for JEE?

For JEE physical chemistry involves topics from 11th standard and 12th as well. So from the 11th standard Mole concept, Atomic Structure, Periodic properties, chemical bonding, gases and liquid, dilute solutions, solid-state. While from 12th standard Energetics, chemical kinetics, Equilibrium, Redox and electrochemistry, surface chemistry.

Q. Is physical chemistry harder than organic chemistry?

Depends if you are good with Math and physics Physical chemistry is going to be easy for you if you are good at memorising then organic chemistry is going to be easy for you. Physical chemistry has more calculation than organic chemistry.

Q. What is the weightage of physical chemistry for JEE?

12 to 15 questions are asked every year from Physical chemistry that is about 48 to 60 marks. It is a scoring topic so you should target 100% in this.

Q. Which are the important topics in physical chemistry for JEE?

Mole concept, thermodynamics, electrochemistry, ionic equilibrium and solid-state.