ISC Class 11 Chemistry Syllabus

Syllabus plays an important role in exam preparation. So, it’s important to know the syllabus right at the beginning of the academic session. Here, students can find the ISC Class 11 Chemistry Syllabus for the year 2020. Along with the syllabus, students will also find the marks weightage of the theory paper. They can download the ISC Class 11 Chemistry Syllabus PDF 2020 from the link below.

ISC Class 11 Reduced Chemistry Syllabus 2020-21: Download PDF

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 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 the 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.

2. Structure of Atom

Bohr’s atomic model and its limitations (deBroglie’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; 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 molecule s, 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 hydrogen bond.

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, Gay Lussac’s law, Avogadro’s law, Avogadro’s number, ideal behaviour of gases and derivation of ideal gas equation. Kinetic Theory of gases. Deviation from ideal behaviour, van der Waal’s equation, liquefaction of gases, critical temperature.

6. Chemical Thermodynamics

(i) First Law of Thermodynamics and its significance, work, heat, internal energy, enthalpy (ΔU or ΔE and ΔH), 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.

(ii) 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

(iii) Third Law of Thermodynamics – statement only.
Self-explanatory

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

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, boric acid, aluminium: Reactions with acids and alkalies. Lewis acid character of boron halides; amphoteric nature of aluminium, alums. Boric acid – preparation and action of heat. Aluminium: Reactions with acids and alkalies. Alums – preparation and uses.

iii. Group 14 Elements
General characteristics, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity.
iv. Preparation and properties of: Silicon carbide – preparation from silica. Uses. Silicones – general method of preparation. Uses.

12. Organic Chemistry – Some Basic Principles and Techniques

General introduction, classification and IUPAC nomenclature of organic compounds and isomerism. Qualitative and quantitative analysis. Electron displacement in a covalent bond:  inductive effect,  electrometric 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, 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

(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: Nitration, sulphonation,
halogenation, Friedel Crafts alkylation and acylation, directive influence of functional group in monosubstituted benzene.

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 ISC Class 11 Chemistry Syllabus useful for their studies. To get the syllabus for all the subjects of class 11 and 12, visit ISC Syllabus page. Stay tuned for the latest update on ICSE/ISC/CBSE/State Board and competitive exams.

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