HBSE Class 11 Syllabus 2025 Chemistry

Haryana Board
Syllabus
2024-25

BOARD OF SCHOOL EDUCATION HARYANA
Syllabus and Chapter wise division of marks (2024-25)
Class- 11th Subject: Chemistry Code:856
General Instructions:
1. There will be an Annual Examination based on the entire syllabus.
2. The annual examination (Theory) will be of 70 Marks whereas Practical
examination will be of 30 marks (Internal). Therefore, Total annual evaluation
(70+30) will be of 100 marks.
3. For Practical examination the criteria are as follows:

Total Time: 3 Hours
Evaluation Scheme Marks
Marks allocated for Internal Assessment 15
1. Student Assessment Test 10
Weightage of marks (06 marks of SAT, 02
marks of half yearly test, 02 marks for
attendance and classroom participation)
2. Practical file/ Record 03
3. Project Record 02

Marks allocated for Annual Examination 15
Volumetric Analysis 05
Salt Analysis 04
Activity (One from Syllabus) 03
Viva Voce 03
Total marks 30

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Course Structure (2024-25)
Class- 11th Subject: Chemistry Code:856

Sr. Name of Chapter Marks
No.
1 Unit 1: Some Basic Concepts of Chemistry 7

2 Unit 2: Structure of Atom 8

3 Unit 3: Classification of Elements and Periodicity in 6
properties

4 Unit 4: Chemical Bonding and Molecular Structure 9

5 Unit 5: Chemical Thermodynamics 7

6 Unit 6: Equilibrium 7

7 Unit 7: Redox Reactions 6

8 Unit 8: Organic Chemistry: Some Basic Principles and 10
Techniques.

9 Unit 9: Hydrocarbons 10

Total 70

Practical 30

Grand Total 100

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Unit 1: Some Basic Concepts of Chemistry
General Introduction: Importance and scope of Chemistry. 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 2: Structure of Atom
Discovery of Electron, Proton and Neutron, atomic number, isotopes and
isobars. Thomson's model and its limitations. Rutherford's model and its
limitations, Bohr's model and its limitations, concept of shells 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's exclusion
principle and Hund's rule, electronic configuration of atoms, stability of half-
filled and completely filled orbitals.
Unit 3: 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, inert gas radii, Ionization
enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of
elements with atomic number greater than 100.
Unit 4: Chemical Bonding and Molecular Structure
Valence electrons, ionic bond, covalent bond, bond parameters, Lewis’s
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
(qualitative idea only), Hydrogen bond
Unit 5: Thermodynamics
Concepts of System and types of systems, surroundings, work, heat, energy,
extensive and 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

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dissociation, combustion, formation, atomization, sublimation, phase transition,
ionization, solution and 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 6: 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, hydrolysis of salts (elementary idea), buffer solution,
Henderson Equation, solubility product, common ion effect (with illustrative
examples).
Unit 7: Redox Reactions
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 8: Organic Chemistry -Some Basic Principles and Techniques
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 and
nucleophiles, types of organic reactions.
Unit 9: Hydrocarbons
Classification of Hydrocarbons Aliphatic Hydrocarbons: Alkanes -
Nomenclature, isomerism, conformation (ethane only), physical properties,
chemical reactions including free radical mechanism of halogenation,
combustion and pyrolysis. Alkenes - Nomenclature, the 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, the structure of triple bond

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(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 the functional group in mono-
substituted benzene. Carcinogenicity and toxicity.

PRACTICALS:
1. Basic Laboratory Techniques.
2. Purification of sample of a compound by crystallisation.
3. Study of shift in equilibrium in the reaction of ferric ions and thiocyanate ions
by increasing the concentration of any one of these ions.
4. Determine the pH of some fruit juices.
5. Study the variation in pH by common ion effect in the case of weak acids and
weak bases.
6. Determination of the concentration (strength) of a given sodium hydroxide
solution by titrating it against a standard solution of oxalic acid
7. Determination of the strength of a given solution of dilute hydrochloric acid by
titrating it against a standard solution of sodium carbonate
8. Detect one cation and one anion in the given salt from the following ions:
Cations - Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+,
Mg2+, NH4+
Anions - CO32-, S2–, SO32- , SO42- , NO2- , NO3- , Cl–, Br–, I–, PO43- , C2O42-,
CH3COO–. (Insoluble salts to be excluded)

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Monthwise Syllabus Teaching Plan (2024-25)
Class- 11th Subject: Chemistry Code:856
Chapter / Topic Teaching Revision Practical
Month Periods periods Periods
Unit 1: Some Basic Concepts of 16 4
Chemistry

Practical: Basic Laboratory 8
April
Techniques.

Unit 2: Structure of Atom 20 5

Practical: Purification of
May 4
sample of a compound by
crystallisation.

Summer Vacations:-
June Investigatory Projects, charts and working innovative models
should be given during the summer vacations
Unit 3: Classification of 12 4
July Elements and Periodicity in
properties
Unit 4: Chemical Bonding and 20 5
August Molecular Structure

Unit 5: Thermodynamics 18 4
September Half Yearly Exam

Unit 6: Equilibrium 14 4

Practical: Study of shift in
October
equilibrium in the reaction of 2
ferric ion and thiocyanate ions.

6

Practical: To determine the pH
of some fruit juices. 1

Practical: Study the variation in
pH by common ion effect in the
2
case of weak acids and weak
bases.

Unit 7: Redox Reactions 8 2

Practical: Determination of the
4
concentration (strength) of a
given sodium hydroxide
solution by titrating it against a
standard solution of oxalic acid.

Practical: Determination of the
4
strength of a given solution of
dilute hydrochloric acid by
titrating it against a standard
solution of sodium carbonate

Practical: Detect one cation and
one anion in the given salt 8
Unit 8: Organic Chemistry: 17 4
November Some Basic Principles and
Techniques.
December Unit 9: Hydrocarbons 20 3
Revision -- -- --
January

7

Revision and Annual Practical -- -- --
February Exams

Annual Exams
March

Note:
• Subject teachers are advised to direct the students to prepare notebook of
the Terminology/Definitional Words used in the chapters for enhancement
of vocabulary for clarity of the concept.

• The NCERT textbooks present information in boxes across the book. These
help students to get conceptual clarity. However, the information in these
boxes would not be assessed in the year-end examination.
Prescribed Books:
1. Chemistry Part-I and Part II, Class XI, BSEH Publications © NCERT
2. Laboratory Manual of Chemistry, Class XI published by (NCERT)

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Question Paper Design(2024-25)
Class- 11th Subject: Chemistry Code: 856
Time: 3 Hours
Type of Marks Number Description Total Marks
Question of
Question
1 18 09 Multiple Choice 18
Objective Questions,
Questions 03 Fill in the blanks
03 One Word
Answer based.
03 Assertion-Reason
Questions
Very Short 2 7 Internal choice will 14
Answer Type be given in any 3
Question questions
Short Answer 3 5 Internal choice will 15
Type Question be given in any 2
questions
Case Study 4 2 Internal choice will 8
be given only in one
part of both
questions
Long Answer 5 3 Internal choice will 15
Type Question be given in all the
questions and may
be given in the parts
Total 35 70

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