Chemistry Class 11 CBSE Syllabus 2020-21 (Revised & Reduced By 30% Due To Covid-19): student read

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In the latest Chemistry Class 11 CBSE Syllabus 2020-21 (revised and reduced to 30%), has been cut by 30% due to Covid-19 so that all students don’t face any inconvenience in studying and preparing for the exam. we will tell you regarding all those things that have been given in Chemistry Class 11 CBSE.

Chemistry Class 11 CBSE Syllabus 2020-21 (Reviewed & Reduced By 30% Due To Covid-19)

Unit No.

Title

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

6

04

Unit IV

Chemical Bonding and Molecular Structure

14

21

Unit V

States of Matter: Gases and Liquids

9

Unit VI

Chemical Thermodynamics

14

Unit VII

Equilibrium

12

Unit VIII

Redox Reactions

4

16

Unit IX

Hydrogen

4

Unit X

s ‐Block Elements

5

Unit XI

Some p ‐Block Elements

9

Unit XII

Organic Chemistry: Some Basic Principles and Techniques

10

18

Unit XIII

Hydrocarbons

10

Total

119

70

General Introduction: Importance and scope of Chemistry subject.

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

Unit II: Structure of Atom (12 Periods)

Bohr’s model and its limitations, de Broglie’s relationship, Heisenberg uncertainty principle, the concept of orbitals, quantum numbers, forms of s, p and d orbitals, the concept of shells and subshells, dual nature of matter and light, rules for filling electrons in orbitals ‐ Aufbau system, Pauli’s exclusion principle and Hund’s rule, electronic configuration of particles, stability of half-filled and filled orbitals.

Unit III: Classification of Elements and Periodicity in Assets (6 Periods)

Modern periodic law and the existing form of the periodic table, periodic trends in properties of ingredients ‐atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electronegativity, valency. Nomenclature of elements with atomic electron gain enthalpy amounts higher than 100.

Unit IV: Chemical Bonding and molecule structure (4 Periods)

Valence electrons, bond parameters, Lewis structure, the polar nature of the covalent bond, covalent nature of ionic bond, valence bond theory, resonance, ionic bond, covalent bond, the geometry of covalent fragments, VSEPR theory, the concept of hybridization, including s, p and d orbitals, and shapes of some simple units, molecular orbital theory of homonuclear diatomic particles(qualitative idea only), Hydrogen bond.

Unit V: States of Matter: Gases And Liquids (09 Periods)

Three states of matter, kinds of bonding, melting and boiling periods, the role of gas laws in elucidating the concept of the unit, Boyle’s law, Charles law, intermolecular synergies, Gay Lussac’s law, Avogadro’s law, practical source of the gas equation, Avogadro’s number, ideal behavior, ideal gas equation and deviation from ideal behavior.

Unit VI: Chemical Thermodynamics (14 Periods) 

Concepts of Systems and types of systems, surroundings, work, heat, power, state functions.

The first law of thermodynamics ‐internal energy and enthalpy, measurement of ΔU and ΔH, extensive and intensive resources, Hess’s law of even heat summation, enthalpy of bond dissociation, fire, formation, atomization, ionization, solution, and dilution. The second law of Thermodynamics (brief introduction), sublimation, phase transition 

Introduction of entropy as a state party, Gibb’s energy change, and non‐spontaneous processes.

law of thermodynamics (brief introduction).

Unit VII: Equilibrium (12 Periods)

Equilibrium in physical and chemical methods, equilibrium constant, parts affecting equilibrium ‐ Le Chatelier’s principle, ionic equilibrium‐ ionization of acids and principles, dynamic nature of equilibrium, the law of mass action, strong and weak electrolytes, degree of ionization, ionization of polybasic acids, the concept of pH, buffer solution, solubility product, acid strength, natural ion effect (with illustrative examples).

Unit VIII: Redox Reactions (04Periods)

Concept of oxidation and loss, redox retreats, oxidation number, balancing redox reactions, in terms of loss and addition of electrons, and change in oxidation number.

Unit IX: Hydrogen (04 Periods)

The rank of hydrogen in the review table, occurrence, isotopes, hydrides‐ionic covalent and interstitial; heavy liquid, physical and biochemical properties of water.

Unit X: s‐Block Elements (Alkali and AlkalineEarth Metals) (5 Period)

Group 1 and Group 2 Elements General introduction, occurrence, anomalous properties of the first element of each group, oblique relationship, bearings in chemical reactivity with oxygen, electronic arrangement, trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii), water, hydrogen, and halogens, uses.

Unit XI: Some p‐Block Elements (9 Periods)

General Introduction to p ‐Block Elements Group 13 Elements: General meeting, appearance, variation of properties, oxidation states, courses in chemical reactivity, electronic configuration, anomalous properties of the first part of the group, Boron ‐ physical and chemical features.

Group 14 Elements: General introduction, electronic arrangement, occurrence, variation of properties, trends in chemical reactivity, anomalous behavior of first components. Carbon‐catenation, allotropic forms, oxidation states, physical and biochemical properties.

Unit XII: Organic Chemistry ‐ Some Basic Principles and Techniques (10 Periods)

General introduction, and IUPAC nomenclature of organic compounds. Electronic displacements in bond: inductive effect, electromeric effect, and hyperconjugation. Homolytic and heterolytic cleavage of a bond: free radicals, carbanions, electrophiles, and nucleophiles, carbocations, examples of organic reactions.

Unit XIII: Hydrocarbons (10 Periods)

Classification of Hydrocarbons

Aliphatic Hydrocarbons:

Alkanes ‐ conformation (ethane only), physical properties, isomerism, Nomenclature, chemical reactions.

Alkenes ‐ Nomenclature, state structure of double bond (ethene), geometrical isomerism, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides, mechanism of electrophilic addition, physical properties, ozonolysis, methods of preparation, (Markovnikov’s addition and peroxide effect), oxidation.

Alkynes ‐ the structure of triple bond (ethyne), Nomenclature, physical properties, chemical reactions: acidic character of alkynes, increasing reaction of ‐ hydrogen, methods of construction, halogens, hydrogen halides, and water.

Aromatic Hydrocarbons:

Introduction, IUPAC classification, benzene: resonance, chemical features: mechanism of electrophilic exchange. Nitration, sulphonation, aromaticity, halogenation, Craft’s alkylation, and acylation, directive leadership of the functional group in monosubstituted benzene. Carcinogenicity & toxicity.

CBSE Class 11 Chemistry Syllabus 2020-21:

Evaluation System for Examination

Marks

Volumetric Analysis

08

Salt Analysis

08

Content-Based Experiment

06

Project Work

04

Class record and viva

04

Total

30

PRACTICAL SYLLABUS (Total Periods: 60) 

Micro-chemical methods are ready for sundry practical experiments, wherever possible such techniques should be used.

A. Basic Laboratory Techniques

1. Cutting glass tube and glass rod

2. Bending a glass tube

3. Drawing out a glass jet

4. Boring a cork

B. Characterization and Purification of Chemical Substances

1. Determination of melting limit of an essential compound.

2. Determination of boiling limit of organic synthesis.

3. Crystallization of mixed samples of any 1 of the following: Alum, Copper Sulphate, BenzoicAcid.

C. Quantitative Estimation 

i. Using a mechanical balance/electronic balance. 

ii. Preparation of standard resolution of Oxalic acid. 

iii. Determination of strength of a mediated solution of Sodium hydroxide by titrating it upon a conventional solution of Oxalic acid. 

iv. Preparation of regular water of Sodium carbonate. 

v. Determination of strength of a given intention of hydrochloric acid by titrating it against conventional Sodium Carbonate suspension. 

D. Qualitative Analysis 

a) Determination of one anion and one cation in a collapsed salt 

Cations- Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Co2+, Ca2+, Zn2+, Sr2+, Ba2+, Mg2+, NH4+ 

Anions – (CO3)2- , S2-, NO2- , SO32-, SO2-4, NO3- , Br-, Cl- , I-, PO43- , CH3COO-,C2O2-4 (Note: Insoluble salts excluded) 

b) Detection of -Nitrogen, Sulphur, Chlorine in natural aggregates. 

c) PROJECTS 

Scientific investigations including scullery testing and collecting information from other sources.

A few suggested Projects 

  • Checking the bacterial poisoning in drinking water by testing sulfide ion 
  •  
  • Study of the methods of purification of water 
  • Investigation of the foaming ability of another washing soaps and the effect of interest of Sodium carbonate on it 
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  • Study the acidity of various samples of tea leaves. 
  • Determination of the rate of withdrawal of different liquids 
  • Study the effect of acids and authorities on the tensile force of fibers. 
  • Study of acidity of fruit and green juices. 

Note: Any other investigatory project, which covers about 10 periods of work, can be chosen with the support of the teacher.

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