ISC Class 12 Chemistry Revised Syllabus for 2024 Exam: Download Syllabus PDF

ISC Class 12 Chemistry Revised Syllabus: In this article, students will get the ISC Chemistry revised syllabus for Class 12 2023-24. Download the ISC revised syllabus pdf here for Chemistry Class 12. 

Download ISC Class 12 Chemistry Revised Syllabus 2023-24 PDF
Download ISC Class 12 Chemistry Revised Syllabus 2023-24 PDF

ISC Class 12 Chemistry revised syllabus for 2024 examination: Indian School Certificate (ISC) is one of the examinations conducted by CISCE for classes 11 and 12. The examination before ISC Class 11 is called ICSE (Indian Certificate of Secondary Education). After the implementation of the National Education Policy 2020, educational boards are introducing changes to their curriculums. This same is followed by CISCE. The aim is to ensure the holistic growth of students without compromising their studies. To check further updates, go through the National Education Policy 2020 - 'School Education'. On June 02, 2023, CISCE released its revised syllabus for selected ISC subjects. It is observed that the revised ISC syllabus has less content to cover as compared to the previously released syllabus for the academic year 2023-24. Students and teachers should have a copy of the revised syllabus to take care of the course content accordingly. 

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Here, we are going to provide the revised ISC Class 12 Chemistry syllabus 2023-24. In the newly released ISC Class 12 Chemistry syllabus, the revision is major, as many of the units are now completely removed. Earlier, there were 16 units, which now reduced to 10. It means 6 of the units are now dropped from the syllabus. Check out the ISC Class 12 Chemistry revised syllabus 2023-24 here.

ISC Revised Syllabus 2023-24 For Classes 11 and 12 (All Subjects)

ISC Class 12 Chemistry Revised Course Structure

S. No.


Total Weightage



Physical Chemistry (25 Marks)




Chemical Kinetics


d -and f -Block Elements

Inorganic Chemistry (25 Marks)


Coordination Compounds


Haloalkanes and Haloarenes

Organic Chemistry (31 Marks)


Alcohols, Phenols and Ethers


Aldehydes, Ketones and Carboxylic Acids


Organic Compounds containing Nitrogen




70 Marks

ISC Class 12 Chemistry Old Course Structure





Solid State

Physical Chemistry

25 Marks






Chemical Kinetics


Surface Chemistry


General Principles and Processes of Isolation of Elements

Inorganic Chemistry

20 Marks


P-Block Elements


d -and f -Block Elements


Coordination Compounds


Haloalkanes and Haloarenes

Organic Chemistry

25 Marks


Alcohols, Phenols and Ethers


Aldehydes, Ketones and Carboxylic Acids


Organic Compounds containing Nitrogen






Chemistry in Everyday Life


70 Marks

ISC Class 12 Chemistry Revised Syllabus 2023-24

There will be two papers in the subject: 

Paper I: Theory - 3 hours (70 marks)

Paper II: 

  • Practical: 3 hours (15 marks) 
  • Project Work (10 marks) 
  • Practical File (5 marks)

1. Solutions 

Study of concentration of solutions of solids in liquids, liquid in liquid, solubility of gases in liquids, solid solutions, Colligative properties - Raoult's law of relative lowering of vapour pressure (1st & 2nd), elevation of boiling point, depression of freezing point, osmotic pressure. Use of colligative properties in determining molecular masses of solutes, abnormal molecular mass association and dissociation, van't Hoff factor. 

Normality, molality, molarity, mole fraction, ppm, as measures of concentration. Definition of the above with examples. Simple problems based on the above. 

(i) Solubility of gases in liquids – Henry’s Law, simple numericals based on the above. 

(ii) Raoult’s Law for volatile solutes and nonvolatile solutes, ideal solution, non-ideal solution. Azeotropic mixtures – definition, types, graphical representation, fractional distillation with examples. 

(iii) Colligative properties – definition and examples, and its use in determination of molecular mass. 

(a) Relative lowering of vapour pressure: Definition and mathematical expression of Raoult’s Law. Determination of relative molecular mass by measurement of lowering of vapour pressure. 

(b) Depression in freezing point: molal depression constant (cryoscopic constant) – definition and mathematical expression (derivation included). 

(c) Elevation in boiling point method: molal elevation constant (ebullioscopic constant) definition and mathematical expression (derivation included). 

(d) Osmotic pressure: definition and explanation. Natural and chemical semipermeable membranes, reverse osmosis, isotonic, hypotonic and hypertonic solutions. Comparison between diffusion and osmosis. Application of osmotic pressure in the determination of relative molecular mass. van’t Hoff- Boyle’s Law, van’t Hoff – Charles’ Law, van’t Hoff - Avogadro’s law. 

(e) Abnormal molecular mass: Dissociation and Association with suitable examples 

(f) van’t Hoff factor for the electrolytes which dissociate and the molecules which associate in solution. Modification of the formula of colligative properties based on van’t Hoff factor. Simple problems. Calculation of degree of dissociation and association. Experimental details not required. 

Numerical problems based on all the above methods. Experimental details not required.

2. Electrochemistry

Electrolytic and electrochemical cells. Redox reactions in electrochemical cells. Electromotive Force (emf) of a cell, standard electrode potential, Nernst equation and its application to chemical cells. Relation between Gibbs energy change and emf of a cell. 

Conductance in electrolytic solutions, specific, equivalent and molar conductivity, variations of conductivity with concentration, graphs; Kohlrausch's Law of electrolysis and Faraday’s Laws of electrolysis. Dry cell and lead accumulator, fuel cells, corrosion. 

(i) Electrochemical cells: introduction, redox reactions (principle of oxidation and reduction in a cell). 

(ii) Galvanic cells - introduction; representation, principle – oxidation-reduction. Mechanism of production of electric current in a galvanic cell. 

(iii) Measurement of potential. Single electrode potentials. Standard hydrogen electrode (Eo) - definition, preparation, application and limitations. Standard electrode potential - Measurement of standard electrode potential of Zn++ / Zn, Cu++ / Cu, half cell (using standard hydrogen electrode). Cell notation – representation. Factors affecting electrode potential with explanation - main emphasis on the temperature, concentration and nature of the electrode. 

(iv) Electrochemical series. Its explanation on the basis of standard reduction potential. Prediction of the feasibility of a reaction. 

(v) Nernst equation and correlation with the free energy of the reaction with suitable examples. Prediction of spontaneity of a reaction based on the cell emf. Numericals on standard electrode potential of half-cells, cell emf, relationship between free energy and equilibrium constant, standard electrode potential and free energy. 

(vi) Comparison of metallic conductance and electrolytic conductance. Relationship between conductance and resistance. Specific resistance and specific conductance. Cell constant: Calculation of cell constant. Meaning of equivalent conductance. Meaning of molar conductance. General relationship between specific conductance, molar conductance and equivalent conductance (units and graphs). Units, numericals. Molar conductance of a weak electrolyte at a given concentration and at infinite dilution. Kohlrausch’s Law – definition, applications and numericals. 

(vii) Faraday’s laws of Electrolysis. Faraday’s First Law of electrolysis. Statement, mathematical form. Simple problems. Faraday’s Second Law of electrolysis: Statement, mathematical form. Simple problems. Relation between Faraday, Avogadro’s number and charge on an electron. F = NAe should be given (no details of Millikan’s experiment are required). 

(viii) Batteries: Primary and Secondary Cells: Leclanche cell, mercury cell, Lead storage battery and fuel cell – structure, reactions and uses. 

(ix) Corrosion: Concept, mechanism of electrochemical reaction, factors affecting it and its prevention. 

3. Chemical Kinetics

Meaning of Chemical Kinetics – slow and fast reactions. Rate of a reaction - average and instantaneous rate (graphical representation). Factors affecting rate of reaction: surface area, nature of reactants, concentration, temperature, catalyst and radiation. Order and molecularity of a reaction, rate law and specific rate constant. Integrated rate equations and half-life (only for zero and first order reactions), concept of collision theory (elementary idea, no mathematical treatment). Concept of threshold and activation energy, Arrhenious equation. 

(i) Meaning of chemical kinetics, Scope and importance of Kinetics of the reaction, slow and fast reactions – explanation in terms of bonds. 

(ii) Rate of Reaction: definition, representation of rate of reaction in terms of reactants and products, determination of rate of reactions graphically, instantaneous and average rate of reaction. Factors affecting rate of reaction. 

(iii)Law of mass Action: statement and meaning of active mass. Explanation with an example – general reactions. 

(iv) Effect of concentration of reactants on the rate of a reaction: Qualitative treatment, based on the law of mass Action, statement of rate law, General rate equation – Rate = k(concentration of the reactant)n , where k is rate constant and n is the order of the reaction, relationship between the rate of the reaction with rate constant with respect to various reactants. 

(v) Order of a reaction: meaning, relation between order and stoichiometric coefficients in balanced equations, order as an experimental quantity, rate equation for zero order reaction and its unit, mathematical derivation of rate equation for first order reaction, characteristics of first order reaction – rate constant is independent of the initial concentration, units to be derived, definition of half-life period, derivation of expression of half-life period from first order rate equation. Problems based on first order rate equation and half-life period. 

(vi) Molecularity of the reaction: Meaning – physical picture, Relation between order, molecularity and the rate of a reaction, Differences between order and molecularity of a reaction. 

(vii) The concept of energy: Exothermic and endothermic reactions, concept of energy barrier, threshold and activation energy, formation of activated complex, effect of catalyst on activation energy and reaction rate. 

(viii)Collision Theory: Condition for a chemical change – close contact, particles should collide. Collisions to be effective – optimum energy and proper orientation during collision. Energy barrier built-up when the collision is about to take place, Activated complex formation, difference in energy of the reactant and the product – exothermic and endothermic reactions with proper graphs and labelling. 

(ix)Mechanism of the reaction: meaning of elementary reaction, meaning of complex and overall reaction, explanation of the mechanism of the reaction, slowest step of the reaction. Relationship between the rate expression, order of reactants and products at the rate-determining step, units of rate constant – explanation with suitable examples. 

(x) Effect of temperature on the rate constant of a reaction: Arrhenius equation – K=Ae-Ea/RT, Meaning of the symbols of Arrhenius equation, related graph, evaluation of Ea and A from the graph, meaning of slope of the graph, conversion from exponential to log form of the equation, relationship between the increase in temperature and the number of collisions. Numerical based on Arrhenius equation. 

4. d and f Block Elements

Position in the periodic table, occurrence, electronic configuration and characteristics of transition metals, general trends in properties of the 3d-series of transition metals - metallic character, ionisation enthalpy, oxidation states, ionic radii, colour of ions, catalytic property, magnetic properties, interstitial compounds, alloy formation, preparation and properties of K2Cr2O7 and KMnO4. Lanthanoids and actinoids. 

(i) d-Block: 3d, 4d and 5d series Study in terms of metallic character, atomic and ionic radii, ionisation enthalpy, oxidisation states, variable valency, formation of coloured compounds, formation of complexes, alloy formation. 

(ii) f-Block: 4f and 5f series Electronic configuration, atomic and ionic radii, oxidisation states, formation of coloured compounds, formation of complexes, alloy formation. Lanthanoid contraction and its consequences. Chemical reactivity – with oxygen, hydrogen, halogen, sulphur, nitrogen, carbon and water. Actinoids - oxidation states and comparison with lanthanoids. 

(iii)Potassium permanganate: structure, shape, equation of extraction from pyrolusite ore, its oxidising nature in acidic, basic and neutral medium, use in redox titration. Oxidising nature in acidic [FeSO4, (COOH)2.2H2O, KI], basic (KI) and neutral (H2S) mediums to be done.

 (iv) Potassium dichromate: structure, shape, equation of extraction from chromite ore and its use in titration. Oxidising nature in acidic, basic and neutral medium, use in redox titration. Interconversion of chromate and dichromate ion (effect of pH). 

5. Coordination Compounds

Concept of complexes, definition of ligands, coordination number, oxidation number. IUPAC nomenclature of mononuclear coordination compounds. Isomerism (structural and stereo). Bonding, Werner's theory, VBT and CFT. Colour, magnetic properties and shapes. Importance of coordination compounds (in qualitative analysis, extraction of metals and biological system). 

(i) Definition of coordination compounds / complex compounds, differences with a double salt, study of ligands – mono-, bi-, tri- , tetra-, penta-, hexa- and polydentate, chelating ligands, definition of coordination number, its calculation for a complex coordination sphere, study of oxidation state of an element in a complex, its calculation, IUPAC rules of nomenclature of coordination compounds. 

(ii) Isomerism – structural, stereo types and examples. 

(iii)Valence bond theory of coordination compounds – examples of formation of inner orbital and outer orbital complexes (high and low spin, octahedral, tetrahedral and square planar), prediction of magnetic character. 

(iv) Crystal field theory – crystal field splitting in tetra and octahedral systems. Explanation of colour and magnetic character. 

(v) Stability of coordination compounds (explain stability on the basis of magnitude of K) as mentioned above). 

(vi) Importance and uses.

6. Haloalkanes and Haloarenes.

Haloalkanes: General formula, nomenclature and classification. Nature of C–X bond, physical and chemical properties, mechanism of substitution reactions, optical rotation. 

Haloarenes: Basic idea, nature of C–X bond, substitution reactions (directive influence of halogen in monosubstituted compounds only). 

Uses and environmental effects of - dichloromethane, trichloromethane, tetrachloromethane, iodoform, freons and DDT. 

Nature of C-X bond 

Naming the halogen derivatives of alkanes by using common system and IUPAC system for mono, di and tri-halo derivatives. 

Preparation of haloalkanes from: 

- Alkane and halogen. 

- Alkene and hydrogen halide. 

- Alcohols with PX3, PCl5 and SOCl2

- Halide exchange method (Finkelstein and Swarts) 

- Silver salt of fatty acids (Hunsdiecker). 

Physical properties: State, melting point, boiling point and solubility. 

Chemical properties: nucleophilic substitution reactions (SN1, SN2 mechanism in terms of primary, secondary and tertiary halides) Reaction with: sodium hydroxide, water, sodium iodide, ammonia, primary amine, secondary amine, potassium cyanide, silver cyanide, potassium nitrite, silver nitrite, silver salt of fatty acid and lithium-aluminium hydride. Elimination reaction (Saytzeff’s rule) / β elimination. Reaction with metals: sodium and magnesium (Wurtz’s reaction, Grignard’s reagent preparation). Chloroform and iodoform: preparation and properties. Structure of freons. Preparation of haloarenes by Sandmeyer’s and Gattermann’s reaction, by electrophilic substitution. Physical properties: State, melting point, boiling point and solubility. 

Chemical properties: 

- Electrophilic substitution (chlorination nitration and sulphonation) with mechanism. 

- Nucleophilic substitution (replacement of chlorine with -OH, -NH2) with mechanism. 

- Reduction to benzene. 

- Wurtz-Fittig reaction. 

- Fittig reaction. 

- Addition reaction with magnesium (formation of Grignard reagent). 

- Structure of DDT

7. Alcohols, Phenols and Ethers

Alcohols: Classification, general formula, structure and nomenclature. Methods of preparation, physical and chemical properties (of primary alcohols only), identification of primary, secondary and tertiary alcohols, mechanism of dehydration, uses with special reference to methanol andethanol. 

(i) Classification into monohydric, dihydric and polyhydric alcohols, general formulae, structure and nomenclature of alcohols. Difference between primary, secondary and tertiary alcohols in terms of structure, physical properties and chemical properties. 

(ii) Methods of preparation: 

- Hydration of Alkenes – direct hydration, indirect hydration, hydroboration oxidation. 

- From Grignard’s reagent. 

- Hydrolysis of alkyl halides. 

- Reduction of carbonyl compounds. 

- From primary amines. 

Manufacture of methanol by Bosch process and ethanol by fermentation of carbohydrates, chemical equations required (only outline of the method of manufacture, detail not required). 


- Acidic nature of alcohols: 

- Reaction with sodium. 

- Esterification with mechanism. 

- Reaction with hydrogen halides. 

- Reaction with PCl3, PCl5, and SOCl2

- Reaction with acid chlorides and acid anhydrides 

- Oxidation. 

- Dehydration with mechanism. 

Uses of alcohols. 

(iii) Conversion of one alcohol into another. 

(iv) Distinction between primary, secondary and tertiary alcohols by Lucas’ Test.

Phenols: Classification and nomenclature. Methods of preparation, physical and chemical properties, acidic nature of phenol, electrophilic substitution reactions, uses of phenols. 

Preparation of phenol from diazonium salt, chlorobenzene (Dow’s process) and from benzene sulphonic acid. 

Manufacture from Cumene. 

Physical properties: state and solubility. 

Chemical properties: 

- Acidic character of phenol. 

- Reaction with sodium hydroxide. 

- Reaction with sodium. 

- Reaction with zinc. 

- Reaction with acetyl chloride and acetic anhydride. 

- Reaction with phosphorus penta chloride. 

- Bromination, nitration and sulphonation (Electrophilic substitution reactions). 

- Kolbe’s reaction (formation of salicylic acid). 

- Reimer – Tiemann reaction 

- Test for phenol – FeCl3 test, azo dye test. 

Aliphatic Ethers: General formula, structure and nomenclature. Methods of preparation, physical and chemical properties, uses. 

Ethers: structure of ethereal group. 

Preparation from alcohol (Williamson’s synthesis). 

Physical properties: state, miscibility. 

Chemical properties: 

- Reaction with chlorine. 

- Oxidation (peroxide formation). 

- Reaction with HI. 

- Reaction with PCl5

Aryl ethers 

Physical properties – state and solubility. 

Chemical properties – preparation of anisole (Williamson’s synthesis), electrophilic substitution (halogenation, nitration and Friedel-Crafts reaction.) 

Uses of ether.

Download the pdf to get Units 8, 9 and 10, ISC Chemistry revised syllabus 2023-24



To download the complete revised syllabus 2023-24 for units 8, 9 10 and the practical part click on the link below and download the pdf. 


Download ISC Class 12 Revised Chemistry Syllabus 2023-24 PDF



ISC Class 12 Chemistry Syllabus 2023-24 (Unrevised)

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