Chemistry in class 11 is a large subject that requires a thorough comprehension of the principles and themes. Knowing the CBSE Class 11 Chemistry syllabus would assist students in comprehending the Chemistry course structure for the academic year 2023-2024. Class 11 students learn what they need to study, how much each unit is worth, and how long it will take them to complete it by going over the syllabus. Students can design their study schedule based on this information. The final exam question paper will be framed according to the CBSE Class 11 Chemistry syllabus, so students must adhere to it.
The CBSE Syllabus for Class 11 Chemistry contains information on practicals, projects, assignments, and other topics that must be covered during the academic year.
Unit No. | Unit Name | No. of Periods | Marks |
---|---|---|---|
Unit I |
Some Basic Concepts of Chemistry |
10 |
11 |
Unit II |
Structure of Atom |
12 |
|
Unit III |
Classification of Elements and Periodicity in Properties |
06 |
04 |
Unit IV |
Chemical Bonding and Molecular Structure |
14 |
06 |
Unit V |
Redox Reactions |
04 |
05 |
Unit VI |
Hydrogen |
04 |
|
Unit VII |
Organic Chemistry: Some Basic Principles and Techniques |
10 |
9 |
Total |
60 |
35 |
General Introduction: Importance and scope of Chemistry. Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry and calculations based on stoichiometry.
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 and Hund’s rule, electronic configuration of atoms, stability of half-filled and completely filled orbitals.
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.
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 and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules(qualitative idea only), Hydrogen bond.
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.
Position of hydrogen in periodic table, occurrence, isotopes, hydrides-ionic covalent and interstitial; physical and chemical properties of water, heavy water, hydrogen as a fuel
General introduction, 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 No. | Unit Name | No. of Periods | Marks |
---|---|---|---|
Unit V |
States of Matter: Gases and Liquids |
09 |
15 |
Unit VI |
Chemical Thermodynamics |
14 |
|
Unit VII |
Equilibrium |
12 |
|
Unit X |
s -Block Elements |
05 |
11 |
Unit XI |
p -Block Elements |
09 |
|
Unit XIII |
Hydrocarbons |
10 |
9 |
Total |
59 |
35 |
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 and deviation from ideal behaviour.
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, measurement of U and H, Hess’s law of constant heat summation, enthalpy of bond 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 nonspontaneous processes.
Third law of thermodynamics (brief introduction).
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, buffer solution, solubility product, common ion effect (with illustrative examples).
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.
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. 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.
Classification of Hydrocarbons Aliphatic Hydrocarbons: Alkanes – Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions.
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.
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 monosubstituted benzene. Carcinogenicity and toxicity.
Practical work is equally important in the Chemistry class. Students gain a better understanding of the theory by carrying out experiments in the lab. As a result, students must be familiar with the CBSE Chemistry Practical Syllabus as well as the list of experiments included in it. In addition, each term's Chemistry practical is worth 15 points. As a result, students must do their best in practicals as well. It will aid in the improvement of their overall score.
CBSE Term I Chemistry Practical is of 15 marks. It will be conducted under the supervision of subject teacher. This contribute to the overall practical marks for the subject.
The table below shows the evaluation scheme of term 1 practical exams.
Evaluation Scheme for Term 1 | Marks |
---|---|
Volumetric Analysis |
08 |
Content Based Experiment |
02 |
Class record and viva (Internal Examiner) |
05 |
Total |
15 |
Micro-chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used:
A. Basic Laboratory Techniques
B. Characterization and Purification of Chemical Substances
CBSE Term II Chemistry Practical is of 15 marks. It will be conducted under the supervision of subject teacher. This contribute to the overall practical marks for the subject.
Evaluation Scheme for Term 2 | Marks |
---|---|
Salt Analysis |
08 |
Content Based Experiment |
02 |
Project Work and Viva(Internal) |
05 |
Total |
15 |
Cations‐ Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4 +
Anions – (CO3)2‐ , S2‐, NO2‐ , SO32‐, SO2‐ , NO ‐ , Cl‐ , Br‐, I‐, PO43‐ , C2O2‐ ,CH3COO‐
(Note: Insoluble salts excluded)
Scientific investigations involving laboratory testing and collecting information from other sources.
There are 9 chapters in the CBSE Class 11 syllabus for Chemistry.
You can get the free PDF for CBSE Syllabus Class 11 Chemistry on the website of Orchids International School.
To prepare for the Class 11 Chemistry exam effectively, learn the key concepts given in the syllabus. Additionally, practice each question given in the textbook and revise the topics thoroughly.
Some of the good resources for studying Class 11 Chemistry are NCERT textbooks, worksheets, and practice materials from some reputed schools like the Orchids International School.
The concepts covered in the CBSE Class 11 syllabus are very basic which helps students to understand the fundamentals and lay a solid foundation for higher classes.
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