NEB Class 11 Chemistry: Complete Syllabus, Notes & Practicals

Class 11 Chemistry: The Ultimate Syllabus and Curriculum Guide

This guide provides a comprehensive overview of the Class 11 Chemistry curriculum, syllabus, and practicals as per the Secondary Education Curriculum 2076.

A visual representation for Class 11 Chemistry concepts.

1. Course Description

Secondary Education Curriculum 2076 – Chemistry

Grades: 11 and 12

Credit hrs: 5 | Working hrs: 160

Introduction

This curriculum for Chemistry is designed to provide students with a foundational understanding of the principles of chemistry, fostering scientific inquiry and critical thinking. It aims to develop a strong knowledge base that is essential for further studies in science and technology and for becoming an informed citizen in a world increasingly shaped by chemical science.

The Class 11 Chemistry course focuses on the core concepts of general, inorganic, organic, and applied chemistry. It encourages students to appreciate the role of chemistry in daily life, industry, and the environment. For official curriculum details, you can visit the official NEB website.

Level-wise Competencies

Upon completion, students are expected to:

  1. Understand fundamental chemical principles and their applications.
  2. Perform laboratory experiments safely and accurately, and interpret the results.
  3. Apply stoichiometric principles to solve quantitative problems.
  4. Understand the structure of atoms, chemical bonding, and the periodic properties of elements.
  5. Gain knowledge of organic compounds and their reactions.

2. Detailed Class 11 Chemistry Syllabus

Content Area: General and Physical Chemistry

  • 1. Foundation and Fundamentals
    • 1.1 General introduction of chemistry
    • 1.2 Importance and scope of chemistry
    • 1.3 Basic concepts of chemistry
    • 1.4 Percentage composition from molecular formula
  • 2. Stoichiometry
    • 2.1 Dalton’s atomic theory and its postulates
    • 2.2 Laws of stoichiometry
    • 2.3 Avogadro’s law and some deductions
    • 2.4 Mole and its relation with mass, volume and number of particles
    • 2.5 Calculations based on mole concept
    • 2.6 Limiting reactant and excess reactant
    • 2.7 Theoretical yield, experimental yield and % yield
    • 2.8 Calculation of empirical and molecular formula from % composition
  • 3. Atomic Structure
    • 3.1 Rutherford’s atomic model & its limitations
    • 3.2 Postulates of Bohr’s atomic model
    • 3.3 Spectrum of hydrogen atom
    • 3.4 Elementary idea of quantum mechanical model
    • 3.5 de Broglie’s wave equation & Heisenberg’s Uncertainty Principle
    • 3.6 Quantum Numbers, Orbitals and shape of s and p orbitals
    • 3.7 Aufbau Principle, Pauli’s exclusion principle, Hund’s rule
  • 4. Classification of elements and Periodic Table
    • 4.1 Modern periodic law and modern periodic table
    • 4.2 IUPAC classification of elements
    • 4.3 Nuclear charge and effective nuclear charge
    • 4.4 Periodic trend and periodicity (Atomic radii, Ionization energy, etc.)
  • 5. Chemical Bonding and Shapes of Molecules
    • 5.1 Ionic, Covalent and Coordinate covalent bond
    • 5.2 Lewis dot structure & Resonance
    • 5.3 VSEPR theory and shapes of some simple molecules
    • 5.4 Hybridization involving s and p orbitals
    • 5.5 Bond characteristics
    • 5.6 Vander Waal’s force, Hydrogen bonding, Metallic bonding
  • 6. Oxidation and Reduction
    • 6.1 General and electronic concept of oxidation and reduction
    • 6.2 Oxidation number
    • 6.3 Balancing redox reactions
    • 6.4 Electrolysis (Qualitative and Quantitative aspect)
  • 7. States of Matter
    • 7.1 Gaseous state (Kinetic theory, Gas laws, Ideal gas equation)
    • 7.2 Liquid state (Physical properties, Liquid crystals)
    • 7.3 Solid state (Types of solids, Crystal lattice)
  • 8. Chemical equilibrium
    • 8.1 Physical and chemical equilibrium
    • 8.2 Law of mass action
    • 8.3 Equilibrium constant (Kp and Kc)
    • 8.4 Le Chatelier’s Principle

Content Area: Inorganic Chemistry

  • 9. Chemistry of Non-metals
    • 9.1 Hydrogen
    • 9.2 Allotropes of Oxygen
    • 9.3 Ozone
    • 9.4 Nitrogen
    • 9.5 Halogens
    • 9.6 Carbon
    • 9.7 Phosphorus
    • 9.8 Sulphur
  • 10. Chemistry of Metals
    • 10.1 Metals and Metallurgical Principles
    • 10.2 Alkali Metals
    • 10.3 Alkaline Earth Metals
  • 11. Bio-inorganic Chemistry
    • 11.1 Introduction to Bio-inorganic Chemistry
    • 11.2 Micro and macro nutrients
    • 11.3 Importance of metal ions in biological systems
    • 11.4 Ion pumps
    • 11.5 Metal toxicity

Content Area: Organic Chemistry

  • 12. Basic Concept of Organic Chemistry
    • 12.1 Introduction to organic chemistry
    • 12.2 Tetra-covalency and catenation properties of carbon
    • 12.3 Classification of organic compounds
    • 12.4 Functional groups and homologous series
    • 12.5 Cracking, reforming, octane number, cetane number
  • 13. Fundamental Principles of Organic Chemistry
    • 13.1 IUPAC Nomenclature
    • 13.2 Qualitative analysis of organic compounds
    • 13.3 Isomerism in Organic Compounds
    • 13.4 Preliminary Idea of Reaction Mechanism
  • 14. Hydrocarbons
    • 14.1 Saturated Hydrocarbons (Alkanes)
    • 14.2 Unsaturated hydrocarbons (Alkenes & Alkynes)
    • 14.3 Test of unsaturation
    • 14.4 Kolbe’s electrolysis methods
  • 15. Aromatic Hydrocarbons
    • 15.1 Introduction to aromatic compounds & Huckel’s rule
    • 15.2 Kekule structure of benzene
    • 15.3 Preparation of benzene
    • 15.4 Chemical properties of benzene

Content Area: Applied Chemistry

  • 16. Fundamentals of Applied Chemistry
    • 16.1 Chemical industry and its importance
    • 16.2 Economics of production
    • 16.3 Designing and running a chemical plant
    • 16.4 Environmental impact
  • 17. Modern Chemical Manufactures
    • 17.1 Manufacture of ammonia, nitric acid, sulphuric acid, sodium hydroxide, sodium carbonate
    • 17.2 Fertilizers (Urea)
  • 18. Nuclear Chemistry and Applications
    • 18.1 Natural and artificial radioactivity
    • 18.2 Nuclear fission and fusion
    • 18.3 Industrial and medical uses of radioactivity
    • 18.4 Radiocarbon dating
    • 18.5 Harmful effects of nuclear radiations

3. Practical Portion

Students should perform at least 10 experiments, with no more than three from any single category.

a) List of Experiments for Grade 11

A. Experiments based on laboratory techniques

  1. To separate insoluble components from a mixture (NaCl, sand, camphor).
  2. To separate a mixture of two soluble solids by fractional crystallization (KNO₃ + NaCl).
  3. To prepare a pure crystal of a salt by crystallization.
  4. To separate components of a mixture of two insoluble solids.
  5. To determine the number of water of crystallization.
  6. To determine the volume of 1 mole of hydrogen gas at NTP.
  7. To obtain pure water from an impure sample by distillation.

B. Experiments to study different types of reactions

  1. To carry out various chemical reactions and represent them in molecular and ionic forms.
  2. To perform precipitation reaction of BaCl₂ and H₂SO₄.
  3. To neutralize NaOH with HCl and recover NaCl crystals.
  4. To test for ferrous ions and oxidize them to ferric ions.
  5. To study the process of electrolysis and electroplating.

C. Experiments on quantitative analysis

  1. To determine the weight of Mg by hydrogen displacement.
  2. To determine the solubility of a given solid.
  3. To determine the relative surface tension by drop count method.
  4. To determine the relative viscosity using Ostwald’s viscometer.
  5. To determine the molecular weight of a metal carbonate.

D. Experiments on preparation of gas and study of properties

  1. To prepare and study the properties of hydrogen gas.
  2. To prepare and study the properties of ammonia gas.
  3. To prepare and study the properties of carbon dioxide gas.
  4. To study the properties of hydrogen sulphide.
  5. To study the properties of sulphuric acid.

E. Experiments on qualitative analysis

  1. To detect basic and acid radicals of a given salt.
  2. To detect the presence of Cl⁻, SO₄⁻⁻ and CO₃⁻⁻ in tap water.

b) Sample Project Works for Grade 11

  1. Observe and list organic and inorganic compounds in your surroundings.
  2. Study the methods of water purification.
  3. Test the hardness of drinking water from different sources.
  4. Study the acidity of different samples of tea leaves.
  5. Prepare molecular models using stick and clay.
  6. Study of adulteration of food materials.
  7. Study the effects of pesticides on human health.
  8. Study the effects of plastics on the environment.
  9. Analysis of soil samples (pH, humus content).
  10. Investigation on corrosion and rusting on iron.
  11. Compare ground and surface water quality of a given place.
  12. Design and development of a water filter.

4. Chapter-wise Notes for Class 11 Chemistry

Unit Chapter Name Notes
General and Physical Chemistry
1Foundation and Fundamentals
2Stoichiometry
3Atomic Structure
4Classification of elements and Periodic Table
5Chemical Bonding and Shapes of Molecules
6Oxidation and Reduction
7States of Matter
8Chemical equilibrium
Inorganic Chemistry
9Chemistry of Non-metals
10Chemistry of Metals
11Bio-inorganic Chemistry
Organic Chemistry
12Basic Concept of Organic Chemistry
13Fundamental Principles of Organic Chemistry
14Hydrocarbons
15Aromatic Hydrocarbons
Applied Chemistry
16Fundamentals of Applied Chemistry
17Modern Chemical Manufactures
18Nuclear Chemistry and Applications

5. Class 11 Chemistry Micro-Syllabus

Content Area: General and Physical Chemistry

1. Foundation and Fundamentals

  1. 1.1 Recognize the importance and scope of chemistry.
  2. 1.2 Explain the terms atom, molecule, radicals, valency molecular formula and empirical formula.
  3. 1.3 Calculate percentage composition of constituent elements from molecular formula.
  4. 1.4 Define and use the terms relative atomic mass, relative molecular mass and relative formula mass.

2. Stoichiometry

  1. 2.1 Explain Dalton’s atomic theory and its postulates.
  2. 2.2 State and explain laws of stoichiometry.
  3. 2.3 Explain Avogadro’s hypothesis and deduce some relationships.
  4. 2.4 Define mole and explain its relation with mass, volume and number of particles.
  5. 2.5 Interpret a balanced chemical equation and perform stoichiometric calculations.
  6. 2.6 Identify limiting and excess reagent in a reaction.
  7. 2.7 Calculate theoretical yield and percentage yield.
  8. 2.8 Find empirical and molecular formula from percentage composition.

3. Atomic Structure

  1. 3.1 Explain Rutherford atomic model and its limitations.
  2. 3.2 Summarize Bohr’s atomic theory and its importance.
  3. 3.3 Explain the origin of hydrogen spectra with the help of Bohr’s model.
  4. 3.4 Explain the general idea about Debroglie’s wave equation and probability.
  5. 3.5 Explain quantum numbers and Planck’s quantum theory.
  6. 3.6 Explain the concept and general shapes of s,p,d and f orbitals.
  7. 3.7 Use Aufbau principle, Pauli Exclusion Principle and Hund’s rule to write electronic configuration.

4. Classification of elements and Periodic Table

  1. 4.1 Explain modern periodic table and its features.
  2. 4.2 Classify the elements of periodic table in different blocks and groups.
  3. 4.3 Identify the elements as metals, non-metals and metalloids.
  4. 4.4 Define the term nuclear charge and effective nuclear charge.
  5. 4.5 Explain and interpret the Periodic trend of atomic radii, ionic radii, ionization energy, electronegativity, electron affinity and metallic characters.

5. Chemical Bonding and Shapes of Molecules

  1. 5.1 Show structure atoms and ions by Lewis dot method.
  2. 5.2 Explain the ionic bond and the properties of ionic compounds.
  3. 5.3 Explain the covalent bond, co-ordinate bond and the properties of covalent compound.
  4. 5.4 Describe the feature of sigma and Pi-bond.
  5. 5.5 Describe the co-ordinate covalent compounds with some examples.
  6. 5.6 Write the lewis dot diagrams of some ionic and covalent compounds.
  7. 5.7 Write the resonance structure of some covalent species.
  8. 5.8 Explain the properties of molecular and metallic solids.
  9. 5.9 Use VSEPR theory to describe the shapes of simple covalent molecules.
  10. 5.10 Describe the concept of hybridization in simple covalent molecules.
  11. 5.11 Explain the characteristics of bond in terms of dipole moment, Ionic character and bond length.
  12. 5.12 Describe the hydrogen bonding and its importance.

6. Oxidation and Reduction

  1. 6.1 Define oxidation and reduction in terms of electronic concept.
  2. 6.2 Define oxidation number and explain the rules of assigning it.
  3. 6.3 Calculate oxidation numbers of elements in compounds and ions.
  4. 6.4 Explain redox processes in terms changes in oxidation number.
  5. 6.5 Use oxidation number change to identify oxidizing and reducing agent.
  6. 6.6 Balance the given redox reaction by oxidation number change or half equation method.
  7. 6.7 Explain the qualitative and quantitative aspects of faradays laws of electrolysis.

7. States of Matter

  1. 7.1 List the postulates of kinetic molecular theory.
  2. 7.2 State and explain Gas laws and related numerical problems.
  3. 7.3 Explain Boyle’s law, Charle’s law, Avogadro law, combined gas law, etc.
  4. 7.4 State and use the general gas equation PV = nRT.
  5. 7.5 Explain the meaning of Universal gas constant.
  6. 7.6 Distinguish between real gas and ideal gas.
  7. 7.7 Explain conditions for a gas to approach ideal behavior.
  8. 7.8 Explain the cause of deviation of real gas from the gas laws.
  9. 7.9 Explain the physical properties of liquid.
  10. 7.10 Describe Liquid crystals and their applications.
  11. 7.11 Differentiate between amorphous and crystalline solids.
  12. 7.12 Describe the properties of crystalline solid.
  13. 7.13 Define unit cell, crystal lattice, efflorescence, etc.

8. Chemical equilibrium

  1. 8.1 Explain physical and chemical equilibrium.
  2. 8.2 Describe the meaning of dynamic nature of equilibrium.
  3. 8.3 Explain and deduce law of mass action.
  4. 8.4 Write equilibrium expression and equilibrium constant.
  5. 8.5 Derive the relation between Kp and Kc.
  6. 8.6 State Lechateliar’s Principle and apply it to systems in equilibrium.

Content Area: Inorganic Chemistry

9. Chemistry of Non-metals

  1. 9.1 Describe and compare the chemistry of atomic and nascent hydrogen.
  2. 9.2 Explain isotopes of hydrogen and their uses.
  3. 9.3 Explain types of oxides.
  4. 9.4 Recognize applications of hydrogen peroxide.
  5. 9.5 State medical and industrial application of oxygen.
  6. 9.6 Describe occurrence, preparation, structure and test of ozone.
  7. 9.7 Describe ozone layer depletion.
  8. 9.8 Give reason for inertness of nitrogen and active nitrogen.
  9. 9.9 Give chemical properties of ammonia.
  10. 9.10 Explain applications and harmful effects of ammonia.
  11. 9.11 Write the name and formula of oxy-acids of nitrogen.
  12. 9.12 Explain the chemical properties of nitric acid.
  13. 9.13 Detect nitrate ion in laboratory.
  14. 9.14 Explain general characteristics of halogens.
  15. 9.15 Compare the methods of preparation of halogens.
  16. 9.16 Explain chemical properties and uses of halogens (Cl₂, Br₂, I₂).
  17. 9.17 Explain laboratory preparation of Cl₂, Br₂ and I₂.
  18. 9.18 Show preparation and properties of haloacids.
  19. 9.19 State the uses of haloacids (HCl, HBr and HI).
  20. 9.20 Explain allotropes of carbon including fullerenes.
  21. 9.21 State properties and uses of carbon monoxide.
  22. 9.22 Name allotropes of phosphorus.
  23. 9.23 Show preparation, properties and uses of phosphine.
  24. 9.24 Explain allotropes of sulphur and uses of sulphur.
  25. 9.25 Prepare hydrogen sulphide using Kipp’s apparatus.
  26. 9.26 Explain properties and uses of hydrogen sulphide.
  27. 9.27 Explain properties of sulphur dioxide and its uses.
  28. 9.28 Explain sulphuric acid and its properties and uses.
  29. 9.29 Write formula and uses of sodium thiosulphate.

10. Chemistry of Metals

  1. 10.1 Define metallurgy and its types.
  2. 10.2 Define ores, gangue, flux, slag, alloy and amalgam.
  3. 10.3 Explain general principles of extraction of metals.
  4. 10.4 Give general characteristics of alkali metals.
  5. 10.5 State and explain extraction of sodium from Down’s process.
  6. 10.6 Describe properties and uses of sodium.
  7. 10.7 Explain properties and uses of sodium hydroxide.
  8. 10.8 State and explain properties and uses of sodium carbonate.
  9. 10.9 Give general characteristics of alkaline earth metals.
  10. 10.10 Write molecular formula and uses of quick lime, bleaching powder, etc.
  11. 10.11 Explain solubility of hydroxides, carbonates and sulphates of alkaline earth metals.
  12. 10.12 Explain stability of carbonate and nitrate of alkaline earth metals.

11. Bio-inorganic Chemistry

  1. 11.1 Explain bio-inorganic chemistry.
  2. 11.2 Define micro and macro nutrients with examples.
  3. 11.3 State and explain importance of metal ions in biological systems.
  4. 11.4 Elaborate ion pumps (sodium-potassium and sodium-glucose pump).
  5. 11.5 Explain metal toxicity (due to iron, arsenic, mercury, lead and cadmium).

Content Area: Organic Chemistry

12. Basic concept of organic chemistry

  1. 12.1 Define organic chemistry and organic compounds.
  2. 12.2 State and explain origin of organic compounds.
  3. 12.3 Describe reasons for the separate study of organic compounds.
  4. 12.4 Explain tetra-covalency and catenation property of carbon.
  5. 12.5 Describe classification of organic compounds.
  6. 12.6 Define functional groups and homologous series with examples.
  7. 12.7 State and explain the structural formula, contracted formula and bond line structural formula.
  8. 12.8 Introduce preliminary idea of cracking and reforming, quality of gasoline, octane number, etc.

13. Fundamental principles

  1. 13.1 State IUPAC name of the organic compounds.
  2. 13.2 Detect N, S and halogens by Lassaigne’s test.
  3. 13.3 Define and classify isomerism in organic compounds.
  4. 13.4 State and explain the concept of geometrical and optical isomerism.
  5. 13.5 Give preliminary idea of reaction mechanism.

14. Hydrocarbons

  1. 14.1 Define and describe saturated hydrocarbons (Alkanes).
  2. 14.2 Show preparation of alkanes.
  3. 14.3 Explain chemical properties of alkanes.
  4. 14.4 Define and describe unsaturated hydrocarbons (Alkenes & Alkynes).
  5. 14.5 Show preparation of alkenes.
  6. 14.6 Explain chemical properties of alkenes.
  7. 14.7 Show preparation of alkynes.
  8. 14.8 Describe chemical properties of alkynes.
  9. 14.9 Test unsaturation of hydrocarbons.
  10. 14.10 Compare physical properties of alkane, alkene and alkyne.
  11. 14.11 Describe Kolbe’s electrolysis methods.

15. Aromatic Hydrocarbons

  1. 15.1 Define aromatic compounds and their characteristics.
  2. 15.2 State and explain Huckel’s rule, Kekule structure of benzene, resonance and isomerism.
  3. 15.3 Show the preparation of benzene.
  4. 15.4 Explain physical and chemical properties of benzene.

Content Area: Applied Chemistry

16. Fundamentals of Applied Chemistry

  1. 16.1 Explain chemical industry and its importance.
  2. 16.2 Explain stages in producing in the development of a new product.
  3. 16.3 Explain economics of production.
  4. 16.4 Explain cash flow in the production cycle.
  5. 16.5 Describe running a chemical plant.
  6. 16.6 Design a chemical plant.
  7. 16.7 Describe continuous and batch processing.
  8. 16.8 Explain environmental impact of the chemical industry.

17. Modern Chemical Manufactures

  1. 17.1 State and show manufacture of ammonia by Haber’s process.
  2. 17.2 State and show manufacture of nitric acid by Ostwald’s process.
  3. 17.3 State and show manufacture of sulphuric acid by contact process.
  4. 17.4 State and show manufacture of sodium hydroxide by Diaphragm Cell.
  5. 17.5 State and show manufacture of sodium carbonate by ammonia soda or Solvay process.
  6. 17.6 Describe fertilizers (Chemical fertilizers, types, production of urea).
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