CBSE 11th Class Chemistry Syllabus

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Course Structure

Course Syllabus

Unit I: Some Basic Concepts of Chemistry

• General Introduction −
  • Importance of Chemistry
  • Scope of chemistry
• Nature of matter
• Laws of chemical combination
• Dalton's atomic theory
• Concept of −
  • Elements
  • Atoms
  • Molecules
• Atomic and molecular masses −
  • Mole concept
  • Molar mass
  • Percentage composition
  • Empirical and molecular formula
  • Chemical reactions
  • Stoichiometry and calculations based on stoichiometry

Unit II: Structure of Atom

• Discovery of −
  • Electron
  • Proton
  • Neutron
  • Atomic number
  • Isotopes
  • Isobars
• Models −
  • Thomson's model and its limitations
  • Rutherford's model and its limitations
  • Bohr's model and its limitations
• Concept of shells and subshells
• Dual nature of matter and light
• de Broglie's relationship
• Heisenberg uncertainty principle
• Concept of orbitals
• Quantum numbers
• Shapes of s, p and d orbitals
• Rules for filling electrons in orbitals −
  • Aufbau principle
  • Pauli's exclusion principle
  • Hund's rule
  • Electronic configuration of atoms
  • Stability of half-filled and completely filled orbitals

Unit III: Classification of Elements and Periodicity in Properties

• Significance of classification
• Brief history of the development of periodic table
• Modern periodic law
• Present form of periodic table
• Periodic trends in properties of elements −
  • Atomic radii
  • Ionic radii
  • Inert gas radii
  • Ionization enthalpy
  • Electron gain enthalpy
  • Electronegativity
  • Valency
• Nomenclature of elements with atomic number greater than 100

Unit IV: Chemical Bonding and Molecular Structure

• Valence electrons

• Ionic bond

• Covalent bond

• Bond parameters

• Lewis structure

• Polar character of covalent bond

• Covalent character of ionic bond

• Valence bond theory

• Resonance

• Geometry of covalent molecules

• VSEPR theory

• Concept of hybridization

• Involving s, p and d orbitals

• Shapes of some simple molecules

• Molecular orbital theory of homonuclear diatomic molecules (qualitative idea only)

• Hydrogen bond

Unit V: States of Matter: Gases and Liquids

• Three states of matter
• Intermolecular interactions
• Types of bonding
• Melting and boiling points
• Role of gas laws in elucidating the concept of the molecule
• Boyle's law
• Charles law
• Gay-Lussac's law
• Avogadro's law
• Ideal behavior
• Empirical derivation of gas equation
• Avogadro's number
• Ideal gas equation
• Deviation from ideal behavior
• Liquefaction of gases
• Critical temperature
• Kinetic energy and molecular speeds (elementary idea)
• Liquid state
• Vapour pressure
• Viscosity
• Surface tension

Unit VI: Chemical Thermodynamics

• System
  • Concept
  • Types
  • Surroundings
  • Work
  • Heat
  • Energy
  • Extensive
  • Intensive properties
  • State functions
• First law of thermodynamics
• Internal energy and enthalpy
• Heat capacity and specific heat
• Measurement of δU and δH
• Hess's law of constant heat summation
• Enthalpy of bond dissociation
• Combustion
• Formation
• Atomization
• Sublimation
• Phase transition
• Ionization
• Solution
• Dilution
• Second law of Thermodynamics (brief introduction)
• Introduction of entropy as a state function
• Gibb's energy change for spontaneous and non-spontaneous processes
• Criteria for Equilibrium
• Third law of thermodynamics (brief introduction)

Unit VII: Equilibrium

• Equilibrium in physical and chemical processes
• Dynamic nature of equilibrium
• Law of mass action
• Equilibrium constant
• Factors affecting equilibrium
• Le chatelier's principle
• Ionic equilibrium-ionization of acids and bases
• Strong and weak electrolytes
• Degree of ionization
• Ionization of poly basic acids
• Acid strength
• Concept of pH
• Henderson equation
• Hydrolysis of salts (elementary idea)
• Buffer solution
• Solubility product
• Common ion effect (with illustrative examples)

Unit VIII: Redox Reaction

• Concept of oxidation and reduction
• Redox reactions
• Oxidation number
• Balancing redox reactions
• In terms of loss and gain of electrons and change in oxidation number
• Applications of redox reactions

Unit IX: Hydrogen

• Position of hydrogen in periodic table
• Occurrence
• Isotopes
• Preparation
• Properties and uses of hydrogen
• Hydrides-ionic covalent and interstitial
• Physical and chemical properties of water
• Heavy water
• Hydrogen peroxide –preparation, reactions and structure and use
• Hydrogen as a fuel

Unit X: s -Block Elements (Alkali and Alkaline Earth Metals)

Group 1 & Group 2 Elements

• General introduction
• Electronic configuration
• Occurrence
• Anomalous properties of the first element of each group
• Diagonal relationship
• Trends in the variation of properties - such as −
  • Ionization enthalpy
  • Atomic and ionic radii
• Trends in chemical reactivity with −
  • Oxygen
  • Water
  • Hydrogen
  • Halogens
• Preparation and Properties of Some Important Compounds −
  • Sodium Carbonate
  • Sodium Chloride
  • Sodium Hydroxide
  • Sodium Hydrogen carbonate
• Biological importance of −
  • Sodium
  • Potassium
  • Magnesium
  • Calcium
• Industrial uses of −
  • Calcium Oxide
  • Calcium Carbonate

Unit XI: Some p -Block Elements

General Introduction to p - Block Elements

• Group 13 Elements −

  • General introduction

  • Electronic configuration

  • Occurrence

  • Variation of properties

  • Oxidation states

  • Trends in chemical reactivity

  • Anomalous properties of first element of the group

  • Boron - physical and chemical properties

  • Some important compounds Borax, Boric acid, Boron Hydrides, Aluminum

  • Reactions with acids and alkalis

• Group 14 Elements −

  • General introduction

  • Electronic configuration

  • Occurrence

  • Variation of properties

  • Oxidation states

  • Trends in chemical reactivity

  • Anomalous behaviour of first elements

  • Carbon-catenation

  • Allotropic forms

  • Physical and chemical properties

  • Uses of some important compounds: oxides

  • Important compounds of Silicon and a few uses

  • Uses of Silicon Tetrachloride, Silicones, Silicates and Zeolites

Unit XII: Organic Chemistry

• Some Basic Principles and Technique
• General introduction
• Methods of purification
• Qualitative and quantitative analysis
• Classification and IUPAC nomenclature of organic compounds
• Electronic displacements in a covalent bond
• Inductive effect
• Electromeric effect
• Resonance and hyper conjugation
• Homolytic and heterolytic fission of a covalent bond
• Free radicals
• Carbocations
• Carbanions
• Electrophiles
• Nucleophile
• Types of organic reactions

Unit XIII: Hydrocarbons - Classification

• Aliphatic Hydrocarbons

• Alkanes

  • Nomenclature

  • Isomerism

  • Conformation (ethane only)

  • Physical properties

  • Chemical reactions including free radical mechanism of halogenation

  • Combustion

  • Pyrolysis

• Alkenes

  • Nomenclature

  • Structure of double bond (ethene)

  • Geometrical isomerism

  • Physical properties

  • Methods of preparation

  • Chemical reactions

  • Addition of hydrogen, halogen, water, hydrogen halides (markownikov's addition and peroxide effect)

  • Ozonolysis

  • Oxidation

  • Mechanism of electrophilic addition

• Alkynes

  • Nomenclature

  • Structure of triple bond (ethyne)

  • Physical properties

  • Methods of preparation

  • Chemical reactions

  • Acidic character of alkynes

  • Addition reaction of - hydrogen, halogens, hydrogen halides and water

• Aromatic Hydrocarbons

  • Introduction

  • IUPAC nomenclature

  • Benzene

  • Resonance

  • Aromaticity

  • Chemical properties

  • Mechanism of electrophilic substitution

  • Nitration

  • Sulphonation

  • Halogenation

  • Friedel Craft's alkylation and acylation

  • directive influence of functional group in mono-substituted benzene

  • Carcinogenicity and toxicity

Unit XIV: Environmental Chemistry

• Environmental pollution −
  • Air
  • Water
  • Soil pollution
• Chemical reactions in atmosphere
• Smog
• Major atmospheric pollutants
• Acid rain
• Ozone and its reactions
• 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

Practical Syllabus

Course Structure

Practical Syllabus

A. Basic Laboratory Techniques

• Cutting glass tube and glass rod
• Bending a glass tube
• Drawing out a glass jet
• Boring a cork

B. Characterization and Purification of Chemical Substances

• Determination of melting point of an organic compound.

• Determination of boiling point of an organic compound.

• Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.

C. Experiments based on pH

(a) Any one of the following experiments −

• Determination of pH of some solutions obtained from fruit juices, solution of known and varied

• concentrations of acids, bases and salts using pH paper or universal indicator.

• Comparing the pH of solutions of strong and weak acids of same concentration.

• Study the pH change in the titration of a strong base using universal indicator.

(b) Study the pH change by common-ion in case of weak acids and weak bases.

D. Chemical Equilibrium

One of the following experiments −

• Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions.

• Study the shift in equilibrium between [Co(H₂O)₆]²⁺ and chloride ions by changing the concentration of either of the ions.

E. Quantitative Estimation

• Using a chemical balance

• Preparation of standard solution of Oxalic acid

• Determination of strength of a given solution of Sodium Hydroxide by titrating it against standard solution of Oxalic acid

• Preparation of standard solution of Sodium Carbonate

• Determination of strength of a given solution of Hydrochloric acid by titrating it against standard Sodium Carbonate solution

F. Qualitative Analysis

• Determination of one anion and one cation in a given salt

  Cations − Pb²⁺, Cu²⁺ As³⁺A1³⁺, Fe³⁺, Mn²⁺, Ni²⁺, Zn²⁺, Co²⁺Ca²⁺, Sr²⁺, Ba²⁺, Mg²⁺,

  Anions − C₃^2-, S^2-, S₃^2-, NO₃^-, Cl^-, Br, I^-, PO³⁺, C₂O₄^2-, CH₃ COO^-

  (Note − Insoluble salts excluded)

• Detection of -Nitrogen, Sulphur, Chlorine in organic compounds.

PROJECT WORK

Scientific investigations involving laboratory testing and collecting information from other sources.

A few suggested Projects −

• Checking the bacterial contamination in drinking water by testing sulphide ion.

• Study of the methods of purification of water.

• Testing the hardness, presence of Iron, Fluoride, Chloride, etc., depending upon the regional variation

• in drinking water and study of causes of presence of these ions above permissible limit (if any).

• Investigation of the foaming capacity of different washing soaps and the effect of addition of Sodium Carbonate on it.

• Study the acidity of different samples of tea leaves.

• Determination of the rate of evaporation of different liquids.

• Study the effect of acids and bases on the tensile strength of fibers.

• Study of acidity of fruit and vegetable juices

Note − Any other investigatory project, which involves about 10 periods of work, can be chosen with the approval of the teacher.

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