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ICSE 11th Chemistry Tuition

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What will you learn in this course?
    • To foster acquisition of knowledge and understanding of terms, concepts, facts, processes, techniques and principles relating to the subject of Chemistry.
    • To develop the ability to apply the knowledge of contents and principles of Chemistry in new or unfamiliar situations.
    • To develop skills in proper handling of apparatus and chemicals.
    • To develop an ability to appreciate achievements in the field of Chemistry and its role in nature and society.
    • To develop an interest in activities involving usage of the knowledge of Chemistry.
    • To develop a scientific attitude through the study of Physical Sciences.
    • To acquaint students with the emerging frontiers and interdisciplinary aspects of the subject.
    • To develop skills relevant to the discipline.
    • To apprise students with interface of Chemistry with other disciplines of Science, such as, Physics, Biology, Geology, Engineering, etc.
₹ 12000
Course Teacher
Course Information
₹ 12000

* Exclusive of 18% GST

    • Assignments every week
    • 200+ MCQs
    • Courseware prepared by experts
    • Assessments to give you the level of improvement

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.

Course Features

120 hours of Live Classes
200+ MCQ Test Series
Live Doubt Resolution
Individual Attention

Course Structure

Units Topics Marks
I Some Basic Concepts of Chemistry 10
II Structure of Atom
III Classification of Elements and Periodicity in Properties
IV Chemical Bonding and Molecular Structure
V States of Matter: Gases and Liquids
VI Chemical Thermodynamics
VI Equilibrium
VIII Redox Reactions 15
IX Hydrogen
X s -Block Elements
XI Some p -Block Elements 15
XII Organic Chemistry: Some basic Principles and Techniques
XIII Hydrocarbons
XIV Environmental Chemistry
Practicals 30
Total 100

Course Lessons

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.

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.

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.

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.

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.

(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.

(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.

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

Hydrogen and its compounds: hydrides, water, heavy water, hydrogen peroxide.

(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.

(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.

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.

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.

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.


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