WBCHSE Class 11 Chemistry Syllabus

Chemistry is an interesting subject which benefits students to learn and understand the complete chemical changes taking place in our life. Chemistry is a well-known branch of science that deals with the study of composition, structure, properties, and interaction of matter. There are different branches of chemistry such as organic chemistry, inorganic chemistry, physical chemistry, analytical chemistry, biochemistry, etc.

WBCHSE Class 11 Chemistry Syllabus for the present academic year are designed by the subject experts on the basis of all important topics. The Class 11 Chemistry Syllabus for the present academic year includes all the necessary and important topics including classification of elements and periodicity, S block elements, Organic chemistry- basic principles and lot more.

We at BYJU’S provide the syllabus for WBCHSE Class 11 Chemistry along with the mark-wise weightage for every chapter, so that students can have a good idea about the pattern of the exam.

Download West Bengal Board Class 11 Chemistry Syllabus

Unitwise Marking Scheme

Unit Name Marks
Unit I: Some Basic Concepts of Chemistry 03
Unit II: Structure of Atom 06
Unit III: Classification of Elements and Periodicity in properties 04
Unit IV: Chemical bonding and Molecular Structure 05
Unit V: State of Matter; Gases and Liquids 04
Unit VI: Thermodynamics 06
Unit VII: Equilibrium 06
Unit VIII: Redox Reactions 03
Unit IX: Hydrogen 03
Unit X: s-Block Elements 05
Unit XI: Some p-Block Elements 07
Unit XII: Organic Chemistry: some basic Principles and Techniques 07
Unit XIII: Hydrocarbons 08
Unit IV: Environmental Chemistry 03
Total 70

Students of Class 11 West Bengal Board can go through the Chemistry syllabus mentioned below:

Unit – I: Some Basic Concepts of chemistry

General Introduction: Importance and scope of chemistry.

Historical approach to particulate nature of matter, laws of chemical combination. Dalton’s atomic
theory: concept of elements, atoms and molecules.

Atomic and molecular masses. Mole concept and molar mass: percentage composition, empirical
and molecular formula; chemical reactions, stoichiometry and calculations based on stoichiometry.

Unit – II: Structure of atoms

Discovery of electrons, proton and neutron; atomic number, isotopes and isobars.

Rutherford’s model and its limitations. Bohr’s model and its limitations, concept of shell and sub
shells, 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 exclusion principle and Hund’s rule, electronic configuration of
atoms, stability of half filled, 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 and the present form of periodic table, periodic trends in properties of elements – atomic
radii, ionic radii, Ionization enthalpy, election gain enthalpy, electronegativity valency, nomenclature
of elements with atomic number greater than 100.

Unit – IV: Chemical Bonding and Molecular Structure

Valence electrons, ionic bond, bond parameters, covalent bond: Born Haber Cycle. 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 and shapes of some simple molecules, Molecular orbital theory of homonuclear diatomic
molecules and 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 Behaviour, empirical derivation of gas equation. Avogadro’s number,
Ideal gas equation. Derivation from ideal behaviour, Liquefaction of gases, critical temperature,
kinetic energy and molecular speeds (elementary idea)

Liquid state – vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical
derivations).

Unit – VI: Chemical Thermodynamics

Concepts of system, types of systems, surroundings. Work, heat, energy, extensive and intensive
properties, state functions.

First law of thermodynamics – internal energy change ( U) and enthalpy change ( H). Hess’s
law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomization,
sublimation, Phase transformation, ionization, and solution.

Introduction of entropy as a state function, Gibbs energy change for spontaneous and non spontaneous processes, criteria for equilibrium. Second and third laws of thermodynamics.

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 of polybasic
acids, acid strength, concept of pH Henderson Equation. Hydrolysis of salts (elementary idea).
Buffer solutions, solubility product, common ion effect ( with illustrative examples).

Unit – VIII: Red ox Reactions

Concept of oxidation and reduction, red ox reactions, oxidation number, balancing redox reactions
in terms of loss and gain of electrons and change in oxidation number.

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, properties, structure and use; hydrogen as a fuel.

Unit – X: s-Block Elements (alkali and Alkaline earth metals)

Group 1 and 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 and
halogens; uses.

Preparation and properties of some important compounds:

Sodium carbonate, sodium hydroxide and sodium hydrogen carbonate, biological importance of
sodium and potassium. CaO, CaCO3 and industrial use of lime and limestone, biological importance of Mg and Ca

Unit –X I: 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, Aluminium: reactions with acids and alkalis and uses.

Group 14 elements: General introduction, electronic configuration, occurrence, variation of
properties, oxidation state, trends in chemical reactivity, anomalous behaviour of first element,
carbon- catenation, allotropic forms, physical and chemical properties; uses of some important
compounds; oxides.

Important compounds of silicon and a few uses: silicon tetrachloride, silicones, silicates and
zeolites, their uses and structure of silicates.

Unit –XII: Organic chemistry – Some Basic Principles and Techniques

General introduction, methods of qualitative and quantitative analysis, classification and IUPAC
nomenclature of organic compounds

Electronic displacements in a covalent bond: inductive effect, electrometric effect, resonance
and hyper conjugation.

Homolytic and Heterolytic fission of a covalent bond: free radicals, carbocations, carbanions,
electrophiles and nucleophiles, types of organic reactions.

Unit –XIII: Hydrocarbons

Classification of hydrocarbons

Alkanes – Nomenclature, isomerism, conformations (ethane only), physical properties, chemical
reactions including halogenations, free radical mechanism, combustion and pyrolysis.

Alkenes – Nomenclature, structure of double bond (ethene), geometrical isomerism, physical
properties, methods of preparation; chemical reactions; addition of hydrogen, halogen, water,
hydrogen halides (markovnikov’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, carcinogenicity and toxicity.

Unit –XIV: Environmental chemistry

Environmental pollution – air, water and 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, strategy for control of environmental pollution.

West Bengal Board Class 11 Chemistry Practical syllabus

Evaluation Scheme for Examination Marks
Volumetric analysis 10
Salt Analysis 08
Content Based Experiment 06
Class Record, Viva and Project work 06
Total 30

Experiments

A. Basic Laboratory Techniques

I. Cutting glass tube and glass rod
II. Bending a glass tube
III. Drawing out a glass jet
IV. Boring a cork

B. Characterization and purification of chemical substances

I. Determination of melting point of an organic compound
II. Determination of boiling point of an organic compound
III. Crystallization of impure sample of anyone of the following: Alum, copper
sulphate, Benzoic acid.

C. Experiments related to pH change

a. Anyone of the following experiments:

  1. Determination of pH of some solutions obtained from fruit juices, varied concentrations of acids, bases and salts using pH paper or universal indicator.
  2. Comparing the pH of solutions of strong and weak acid of same concentration.
  3. Study the pH change in the titration of a strong base using universal indicator.

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

D. Chemical equilibrium

One of the following experiments:

  1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either ions.
  2. 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

  1. Using a chemical balance.
  2. Preparation of standard solution of oxalic acid.
  3. Determination of strength of a given solution of sodium hydroxide by titrating it against standard solution of oxalic acid.
  4. Preparation of standard solution of sodium carbonate.
  5. 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 caution in a given salt

Cautions:- Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+,Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+
Anions:-CO 32-, S 2-, SO 32-, SO42- , NO2-1 , NO3-1, Cl-1, Br-1, I-1, PO43- , CO42-, CH3COO
(Note: Insoluble salts excluded)

G. Detection of nitrogen, sulphur, chlorine

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