ISC Syllabus for Class 11 Chemistry plays an important role in exam preparation. So, it’s crucial to know the syllabus right at the beginning of the academic session. Here, students can find the Chemistry ISC Class 11 Syllabus for the academic year 2023-24. Along with the syllabus, they will also find the marks weightage of the theory paper. They can download the ISC Class 11 Chemistry Syllabus PDF from the link below.
Download PDF of ISC Class 11 Chemistry Syllabus 2023-24
In the PDF, students will find the ISC Class 12 Chemistry Practical Syllabus, along with the project work and practical file assessment, in detail. So, go through it before creating the study plan.
Marks Distribution of the ISC Class 11 Chemistry Syllabus Paper 1 (Theory)
There will be no overall choice in the paper. Students will be required to answer all questions. The internal choice will be available in two questions of 2 marks each, two questions of 3 marks each and all three questions of 5 marks each. The Chemistry question paper will be based on the following pattern:
| S.No. | Unit | Total Weightage |
| 1 | Some Basic Concepts of Chemistry | Physical Chemistry
32 Marks |
| 2 | Structure of Atom | |
| 3 | Classification of Elements and Periodicity in Properties | |
| 4 | Chemical Bonding and Molecular Structure | |
| 5 | States of Matter: Gases and Liquids | |
| 6 | Chemical Thermodynamics | |
| 7 | Equilibrium | |
| 8 | Redox Reactions | Inorganic Chemistry
15 Marks |
| 9 | Hydrogen | |
| 10 | s -Block Elements | |
| 11 | Some p -Block Elements | |
| 12 | Organic Chemistry: Some Basic Principles and Techniques | Organic Chemistry
23 Marks |
| 13 | Hydrocarbons | |
| 14 | Environmental Chemistry | |
| Total | 70 Marks | |
ISC Syllabus for Class 11 Chemistry
1. Some Basic Concepts of Chemistry
General introduction: Importance and scope of chemistry.
Study of matter. Understanding laws of chemical combination. Dalton’s atomic theory: concept of elements, atoms and molecules.
Isotopic (atomic) and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula. Stoichiometry and calculations based on chemical reactions.
2. Structure of Atom
Discovery of fundamental particles electron, proton and neutron), atomic number, isotopes and isobars. Thomson’s model and its limitations. Rutherford’s experimental model and its limitations. Dual nature of matter and light. Bohr’s atomic model and its limitations (de Broglie’s equation, Heisenberg’s uncertainty principle), concept of shells, subshells, orbitals. Quantum numbers, shapes of s, p and d orbitals. Rules for filling electrons in orbitals -aufbau principle, Pauli’s exclusion principle and Hund’s rule of maximum multiplicity. Electronic configuration of atoms, stability of half- filled and completely filled orbitals.
3. Classification of Elements and Periodicity in Properties
Significance of classification; study of Mendeleev’s periodic law and its limitations; Modern Periodic Law and the present form of periodic table leading to periodic trends in properties of elements – atomic radii, ionic radii,
valency, ionisation enthalpy, electron gain enthalpy, electronegativity. Nomenclature of elements with atomic number greater than 100.
4. Chemical Bonding and Molecular Structure
Valence electrons, ionic bond character, covalent bond of ionic bond, covalent bond, bond parameters, lewis structure, polar character of covalent bond, VSEPR theory, geometry of covalent molecules, valence bond theory, concept of hybridisation involving s, p and d orbitals and shapes of some simple molecules. Coordinate bond. Molecular orbital theory of homonuclear diatomic molecules (qualitative idea only). Resonance and hydrogenbond.
5. States of Matter: Gases and Liquids
States of matter and their characteristic properties to establish the concept of the molecule. Boyle’s law, Charles law, GayLussac’s law, Avogadro’s law, Avogadro’s number, ideal behaviour of gases and derivation of ideal gas
equation. Kinetic Theory of gases, kinetic energy and molecular speeds (elementary idea). Deviation from ideal behaviour, van der Waal’s equation, liquefaction of gases, critical temperature. Liquid state – vapour pressure,
viscosity and surface tension (qualitative idea only, no mathematical derivations).
6. Chemical Thermodynamics
(i) Introduction, concepts, types of system, surroundings, extensive, intensive properties and state functions.
(ii) First Law of Thermodynamics and its significance, work, heat, internal energy, enthalpy (∆U or ∆E and ∆H), heat capacity and specific heat. Hess’s law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomisation, sublimation, phase transition, ionisation, solution and dilution.
(iii) Second Law of Thermodynamics and its significance, spontaneity of a chemical change; Entropy, Free Energy. Inadequacy of First Law and need for Second Law; Ideas about reversible (recapitulation), spontaneous and non-spontaneous processes.
(iv) Third Law of Thermodynamics – statement only.
7. Equilibrium
(i) Chemical Equilibrium
Introduction of physical and chemical equilibrium and its characteristics.
Dynamic nature of equilibrium, law of mass action, equilibrium constant and
factors affecting equilibrium. Le Chatelier’s principle and its applications.
(ii) Ionic equilibrium
Introduction, electrolyte (strong and weak), non-electrolyte, ionisation, degree of ionisation of polybasic acids, acid strength, concept of pH, pH indicators,
buffer solution, common ion effect (with illustrative examples). Henderson equation, hydrolysis of salts, solubility and solubility product.
8. Redox Reactions
Concept of oxidation and reduction, redox reactions, oxidation number, change in oxidation number, balancing redox reactions (in terms of loss and gain of electrons). Applications of redox in various types of chemical reactions.
9. Hydrogen
Hydrogen and its compounds: hydrides, water, heavy water, hydrogen peroxide.
10. s-Block Elements (Alkali and Alkaline Earth Metals)
(i) Group 1 and 2 elements
General characterises of Group 1 and 2 should include the following:
Occurrence; physical state; electronic configuration; atomic and ionic radii; common oxidation state; electropositive /electronegative character; ionisation enthalpy; reducing/oxidising nature.
(ii) Preparation and properties of some important compounds
Sodium chloride, sodium hydroxide, Sodium carbonate, sodium bicarbonate, sodium thiosulphate; biological importance of sodium and potassium.
Magnesium chloride hexahydrate, calcium oxide, calcium hydroxide, calcium carbonate, plaster of Paris and cement. Industrial uses of the above, biological importance of magnesium and calcium.
11. Some p -Block Elements
(i) Group 13 Elements
General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, physical and chemical properties.
(ii) Preparation and properties of some important compounds, borax, boric acid, boron hydrides, aluminium: Reactions with acids and alkalies. Lewis acid character of boron halides; amphoteric nature of aluminium, alums.
(iii) Group 14 Elements
General characteristics, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity.
(iv) Some important compounds; oxides of carbon and silicon, silicon carbide, silicon tetra chloride, silicones, silicates and zeolites.
12. Organic Chemistry – Some Basic Principles and Techniques
General introduction, classification and IUPAC nomenclature of organic compounds and isomerism.
Methods of purification, qualitative and quantitative analysis. Electron displacement in a covalent bond: inductive effect, electromeric effect, resonance and hyperconjugation.
Homolytic and heterolytic bond fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.
13. Hydrocarbons
Classification of Hydrocarbons
I. Aliphatic Hydrocarbons
(i) Alkanes – Nomenclature, isomerism, conformation (methane and ethane),
physical properties, chemical properties including free radical mechanism of
halogenation, combustion and pyrolysis.
(ii) Alkenes – Nomenclature, structure of double bond (ethene), isomerism; methods of preparation; physical properties, chemical properties; addition of hydrogen, halogen, water, hydrogen halides (Markownikoff’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition.
(iii) Alkynes – Nomenclature, structure of triple bond (ethyne), methods of preparation; physical properties, chemical properties: acidic character of alkynes, addition reactions – hydrogen, halogens, hydrogen halides and water.
II. Aromatic Hydrocarbons
Introduction, IUPAC nomenclature, benzene: resonance, aromaticity, chemical properties: mechanism of electrophilic substitution. Nitration, sulphonation, halogenation, Friedel Crafts alkylation and acylation, directive influence of functional group in monosubstituted benzene. Carcinogenicity and toxicity.
14. Environmental Chemistry
Types of environmental pollution (air, water and soil pollution); various types of pollutants: smog, acid rain; effects of depletion of ozone layer, greenhouse effect and global warming. Pollution due to industrial wastes, green chemistry as an alternative tool for reducing pollution; strategies for control of environmental pollution.
We hope students have found this information on the ISC Class 11 Chemistry Syllabus useful for their studies. To get the syllabus for all the subjects of Classes 11 and 12, visit the ISC Syllabus page. Stay tuned for the latest update on ICSE/ISC/CBSE/State Board and competitive exams.
Comments