NEB Class 12 Chemistry: Complete Syllabus, Notes & Practicals

Class 12 Chemistry: The Ultimate Syllabus and Curriculum Guide

This guide provides a comprehensive overview of the Class 12 Chemistry curriculum, syllabus, and practicals as per the Secondary Education Curriculum 2076.

A visual representation for Class 12 Chemistry concepts.

1. Course Description

Secondary Education Curriculum 2076 – Chemistry

Grades: 11 and 12

Credit hrs: 5 | Working hrs: 160

Introduction

The Grade 12 Chemistry curriculum builds upon the foundational concepts learned in Grade 11, delving deeper into advanced topics in physical, inorganic, organic, and applied chemistry. It is designed to equip students with a robust understanding of chemical principles and their practical applications, preparing them for higher education and careers in science, engineering, and medicine.

This Class 12 Chemistry course emphasizes analytical thinking, problem-solving skills, and laboratory proficiency. It aims to foster an appreciation for the role of chemistry in technological advancements and sustainable development. For official curriculum details, please refer to the official NEB website.

Level-wise Competencies

Upon completion, students are expected to:

  1. Analyze and solve complex problems in volumetric analysis, chemical kinetics, and thermodynamics.
  2. Understand the principles of ionic equilibrium and electrochemistry.
  3. Explain the properties and reactions of transition metals and important organic functional groups.
  4. Apply chemical principles to understand industrial processes and their environmental impact.
  5. Develop advanced laboratory skills through qualitative and quantitative experiments.

2. Detailed Class 12 Chemistry Syllabus

Content Area: General and Physical Chemistry

  • 1. Volumetric Analysis
    • 1.1 Introduction to gravimetric analysis, volumetric analysis and equivalent weight
    • 1.2 Relationship between equivalent weight, atomic weight and valency
    • 1.3 Equivalent weight of compounds
    • 1.4 Concentration of solution and its units
    • 1.5 Primary and secondary standard substances
    • 1.6 Law of equivalence and normality equation
    • 1.7 Titration and its types
  • 2. Ionic Equilibrium
    • 2.1 Introduction to Acids and Bases (Arrhenius, Bronsted-Lowry, Lewis concepts)
    • 2.2 Ionization of weak electrolyte (Ostwald’s dilution law)
    • 2.3 Ionic product of water ($K_w$)
    • 2.4 Dissociation constant ($K_a$ & $K_b$), pKa and pKb
    • 2.5 pH value
    • 2.6 Solubility and solubility product principle
    • 2.7 Common Ion effect
    • 2.8 Buffer solution and its application
    • 2.9 Indicators and selection of indicators
    • 2.10 Types of salts and Hydrolysis of salts
  • 3. Chemical Kinetics
    • 3.1 Rate of reactions
    • 3.2 Rate law, Rate constant, Order and molecularity
    • 3.3 Integrated rate equation for zero and first order reaction
    • 3.4 Half-life of reactions
    • 3.5 Collision theory, activation energy
    • 3.6 Factors affecting rate of reactions (Concentration, Temperature, Catalyst)
    • 3.7 Catalysis and its types
  • 4. Thermodynamics
    • 4.1 Internal energy and First law of thermodynamics
    • 4.2 Enthalpy and enthalpy changes
    • 4.3 Laws of thermochemistry (Laplace Law and Hess’s law)
    • 4.4 Entropy and spontaneity
    • 4.5 Second law of thermodynamics
    • 4.6 Gibbs’ free energy and prediction of spontaneity
    • 4.7 Relationship between $\Delta G$ and equilibrium constant
  • 5. Electrochemistry
    • 5.1 Electrode potential and standard electrode potential
    • 5.2 Types of electrodes
    • 5.3 Electrochemical series and its applications
    • 5.4 Voltaic cell
    • 5.5 Cell potential and its relationship with free energy
    • 5.6 Commercial batteries and fuel cells

Content Area: Inorganic Chemistry

  • 6. Transition Metals
    • 6.1 Characteristics, Oxidation states
    • 6.2 Complex ions and metal complexes
    • 6.3 Shapes of complex ions and d-orbitals in complex ions
    • 6.4 Colour of transition metal compounds
    • 6.5 Catalytic properties
  • 7. Studies of Heavy Metals
    • 7.1 Copper (Extraction, properties, uses, compounds)
    • 7.2 Zinc (Extraction, properties, uses, compounds)
    • 7.3 Mercury (Extraction, properties, uses, compounds)
    • 7.4 Iron (Extraction, properties, uses, steel manufacturing, corrosion)
    • 7.5 Silver (Extraction, properties, uses, compounds)

Content Area: Organic Chemistry

  • 8. Haloalkanes
    • 8.1 Introduction
    • 8.2 Nomenclature, isomerism and classification of monohaloalkanes
    • 8.3 Preparation of monohaloalkanes from alkanes, alkenes and alcohols
    • 8.4 Physical properties of monohaloalkanes
    • 8.5 Chemical properties, substitution reactions SN1 and SN2 reactions (basic concept only)
    • 8.6 Formation of alcohol, nitrile, amine, ether, thioether, carbylamines, nitrite and nitro alkane using haloalkanes
    • 8.7 Elimination reaction (dehydrohalogenation- Saytzeff’s rule), Reduction reactions, Wurtz reaction
    • 8.8 Preparation of trichloromethane from ethanol and propanone
    • 8.9 Chemical properties of trichloromethane: oxidation, reduction, action on silver powder, conc. nitric acid, propanone, and aqueous alkali
  • 9. Haloarenes
    • 9.1 Introduction
    • 9.2 Nomenclature and isomerism of haloarenes
    • 9.3 Preparation of chlorobenzene from benzene and benzene diazonium chloride
    • 9.4 Physical properties
    • 9.5 Chemical properties
    • 9.6 Uses of haloarenes
  • 10. Alcohols
    • 10.1 Introduction
    • 10.2 Nomenclature, isomerism and classification of monohydric alcohol
    • 10.3 Distinction of primary, secondary and tertiary alcohols by Victor Meyer’s Method
    • 10.4 Preparation of monohydric alcohols
    • 10.5 Industrial preparation alcohol
    • 10.6 Definition of common terms: Absolute alcohol, power alcohol, etc.
    • 10.7 Physical properties monohydric alcohols
    • 10.8 Chemical properties of monohydric alcohols
  • 11. Phenols
    • 11.1 Introduction and nomenclature
    • 11.2 Preparation of phenol
    • 11.3 Physical properties of phenol
    • 11.4 Chemical properties (Acidic nature, various reactions)
    • 11.5 Test of phenol
    • 11.6 Uses of phenol
  • 12. Ethers
    • 12.1 Introduction
    • 12.2 Nomenclature, classification and isomerism of ethers
    • 12.3 Preparation of aliphatic and aromatic ethers from Williamson’s synthesis
    • 12.4 Physical properties of ether
    • 12.5 Chemical properties of ethoxyethane
    • 12.6 Uses of ethers
  • 13. Aldehydes and Ketones
    • 13.1 Aliphatic aldehydes and ketones
    • 13.2 Aromatic aldehydes and Ketones
  • 14. Carboxylic Acid and its Derivatives
    • 14.1 Aliphatic and aromatic carboxylic acids
    • 14.2 Derivatives of Carboxylic acids (acid halides, amides, esters and anhydrides)
  • 15. Nitro Compounds
    • 15.1 Nitroalkanes
    • 15.2 Nitrobenzene
  • 16. Amines
    • 16.1 Aliphatic amines
    • 16.2 Aromatic amine (Aniline)
  • 17. Organometallic Compounds
    • 17.1 Introduction
    • 17.2 Nature of Metal-Carbon bond
    • 17.3 Grignard reagent

Content Area: Applied Chemistry

3. Practical Portion

Students should perform experiments from the following categories.

a) List of Experiments for Grade 12

A. Recovery and preparation of salt

  1. To recover blue vitriol crystals from a mixture.
  2. To recover CaCO₃ from dolomite.
  3. To obtain hydrated calcium sulphate from marble chips.

B. Volumetric analysis (Titration)

  1. To prepare a primary standard solution of Na₂CO₃ and standardize HCl.
  2. To determine the strength of NaOH solution.
  3. To determine the strength of bench sulphuric acid (Double titration).
  4. To standardize KMnO₄ solution with standard oxalic acid (Redox titration).

C. Organic chemistry

  1. To detect foreign elements (N, S, X) in an organic compound.
  2. To identify functional groups (-OH, -COOH, CHO, –CO–, –NH₂, –COO–).
  3. To test for carbohydrates, fats, proteins, and phenol.

D. Thermochemistry

  1. To determine the enthalpy of neutralization.
  2. To determine the molar enthalpy change of ammonium chloride solution.

E. Chemical kinetics

  1. To study the kinetics of the reaction between sodium thiosulphate and HCl.
  2. To study the kinetics of the reaction between propanone and iodine.

F. Salt analysis

  1. To perform complete salt analysis to detect acid and basic radicals (at least three samples).

G. Applied and analytical Chemistry

  1. To separate ink components by paper chromatography and determine R_f values.
  2. To determine acetic acid content in vinegar.
  3. To prepare common compounds: Potash alum, Iodoform, Fehling’s solution.
  4. To isolate hippuric acid from cow urine.
  5. To demonstrate the pH value of unknown samples.

b) Sample Project Works for Grade 12

  1. Investigate environmental impacts of chemical pollution from various sources.
  2. Prepare a report on a paper or cement industry.
  3. Observe the setting duration of different cement brands.
  4. Study the effect of heat on different types of plastics.
  5. Extraction of essential oils from plants.
  6. Preparation of soap from vegetable oil.
  7. Study the quantity of casein in different milk samples.
  8. Study the formation of rust under various conditions.
  9. Study food preservatives and adulterants in common food items.
  10. Investigate the foaming capacity of different washing soaps.

4. Chapter-wise Notes for Class 12 Chemistry

Unit Chapter Name Notes
General and Physical Chemistry
1Volumetric Analysis
2Ionic Equilibrium
3Chemical Kinetics
4Thermodynamics
5Electrochemistry
Inorganic Chemistry
6Transition Metals
7Studies of Heavy Metals
Organic Chemistry
8Haloalkanes
9Haloarenes
10Alcohols
11Phenols
12Ethers
13Aldehydes and Ketones
14Carboxylic Acid and its Derivaties
15Nitro Compounds
16Amines
17Organometallic Compounds
Applied Chemistry
18Chemistry in the service of mankind
19Cement
20Paper and Pulp
21Nuclear Chemistry and Applications of Radioactivity

5. Class 12 Chemistry Micro-Syllabus

Content Area: General and Physical Chemistry

1. Volumetric Analysis

  1. 1.1 Define and explain the terms volumetric and gravimetric analysis.
  2. 1.2 Express the concentration of solutions in terms of percentage, g/l, molarity, molality, normality, ppm, ppb.
  3. 1.3 Define and calculate the equivalent weight of elements, acids, bases, salts, oxidising and reducing agents.
  4. 1.4 Express the concentration of solution in terms of normality.
  5. 1.5 Explain and apply the concept of law of equivalence in chemical calculation.
  6. 1.6 Define and explain primary and secondary standard substance.
  7. 1.7 Explain different types of titration and their applications.

2. Ionic Equilibrium

  1. 2.1 Explain the limitations of Arrhenius concepts of acids and bases.
  2. 2.2 Define Bronsted and Lowry concepts for acids and bases.
  3. 2.3 Define conjugate acids and conjugate base.
  4. 2.4 Identify conjugate acid-base pairs of Bronsted acid and base.
  5. 2.5 Define and explain Lewis acids and bases.
  6. 2.6 Use the extent of ionization and dissociation constant of acid ($k_a$) and base ($k_b$).
  7. 2.7 Explain ionization constant of water and calculate pH and pOH in aqueous medium using $K_w$ values.
  8. 2.8 Show understanding of, and use, the concept of solubility product $K_{sp}$.
  9. 2.9 Calculate $K_{sp}$ from concentrations and vice versa.
  10. 2.10 Show understanding of the common ion effect.
  11. 2.11 Describe the application of solubility product principle and common ion effect in precipitation reactions.
  12. 2.12 Define a Buffer and show with equations how a Buffer system works.
  13. 2.13 Explain the choice of suitable indicators for acid-base titrations.
  14. 2.14 Define and differentiate different types of salts.
  15. 2.15 Explain hydrolysis of salts.

3. Chemical Kinetics

  1. 3.1 Define chemical kinetics.
  2. 3.2 Explain and use the terms rate of reaction, rate equation, rate constant.
  3. 3.3 Explain qualitatively factors affecting rate of reaction.
  4. 3.4 Use collision theory to explain the influence of temperature, concentration and particle size on reaction rate.
  5. 3.5 Explain the meaning of activation energy and activated complex.
  6. 3.6 Derive and explain integrated rate equation and half life for zero, and first order reaction.
  7. 3.7 Construct and use rate equations.
  8. 3.8 Explain the significance of Arrhenius equation and solve related problems.
  9. 3.9 Explain and use the terms catalyst and catalysis (homogenous, heterogeneous).
  10. 3.10 Describe enzyme as biological catalyst.
  11. 3.11 Explain the role of catalyst in the reaction mechanism.
  12. 3.12 Solve related numerical problems.

4. Thermodynamics

  1. 4.1 Define thermodynamics.
  2. 4.2 Explain the energy change in chemical reactions.
  3. 4.3 Define the terms internal energy and state function.
  4. 4.4 State and explain first law of thermodynamics.
  5. 4.5 State and explain enthalpy and enthalpy changes in various process.
  6. 4.6 Explain endothermic and exothermic process.
  7. 4.7 State laws of thermo-chemistry and solve numerical problems related to Hess law.
  8. 4.8 Define the term entropy and spontaneity.
  9. 4.9 State and explain second law of thermodynamics.
  10. 4.10 Define standard Gibbs free energy change by means of the equation $\Delta G = \Delta H – T\Delta S$.
  11. 4.11 Calculate $\Delta G$ for a reaction using the equation.
  12. 4.12 State whether a reaction or process will be spontaneous by using the sign of $\Delta G$.
  13. 4.13 Explain the relationship between $\Delta G$ and equilibrium constant.

5. Electrochemistry

  1. 5.1 Define the terms: standard electrode (redox) potential.
  2. 5.2 Explain about standard hydrogen electrode and calomel electrodes.
  3. 5.3 Calculate a standard cell potential.
  4. 5.4 Describe the applications of electrochemical series.
  5. 5.5 Use standard cell potentials to deduce the direction of electron flow and predict the feasibility of a reaction.
  6. 5.6 Define and explain standard cell potential with reference to voltaic cells.
  7. 5.7 Explain the relationship between cell potential and free energy change.
  8. 5.8 State the possible advantages of fuel cells and rechargeable batteries.

Content Area: Inorganic Chemistry

6. Transition Metals

  1. 6.1 Explain characteristics of transition metals.
  2. 6.2 Explain oxidation states of transition metals.
  3. 6.3 Describe complex ions and metal complexes.
  4. 6.4 Show shapes of complex ions.
  5. 6.5 Describe d-orbitals in complex ions (simple explanation by crystal field theory).
  6. 6.6 Explain reasons for the colour of transition metal compounds.
  7. 6.7 Explain catalytic properties of transition metals.

7. Studies of Heavy Metals

  1. 7.1 Explain occurrence of heavy metals.
  2. 7.2 Describe extraction of heavy metals.
  3. 7.3 Describe properties and uses of copper.
  4. 7.4 Explain chemistry of blue vitriol.
  5. 7.5 Write formula and uses red and black oxide of copper.
  6. 7.6 Describe properties and uses of zinc.
  7. 7.7 Explain chemistry of white vitriol.
  8. 7.8 State properties of mercury.
  9. 7.9 Explain chemistry of calomel and corrosive sublimate.
  10. 7.10 Explain properties and uses of iron.
  11. 7.11 Explain manufacture of steel.
  12. 7.12 Explain corrosion of iron and its prevention.
  13. 7.13 Explain preparation and uses of silver chloride and silver nitrate.

Content Area: Organic Chemistry

8. Haloalkanes

  1. 8.1 Describe nomenclature, isomerism and classification of monohaloalkanes.
  2. 8.2 Show the preparation of monohaloalkanes.
  3. 8.3 State physical properties of monohaloalkanes.
  4. 8.4 Describe chemical properties of haloalkanes: SN1 and SN2 reactions.
  5. 8.5 Show the formation of various compounds using haloalkanes.
  6. 8.6 Describe elimination, reduction, and Wurtz reaction.
  7. 8.7 Show the preparation of trichloromethane.
  8. 8.8 Explain the chemical properties of trichloromethane.

9. Haloarenes

  1. 9.1 Describe nomenclature and isomerism of haloarenes.
  2. 9.2 Show the preparation of chlorobenzene.
  3. 9.3 State physical properties of haloarens.
  4. 9.4 Describe low reactivity of haloarenes in nucleophilic substitution.
  5. 9.5 Explain the chemical properties of haloarenes.
  6. 9.6 Describe uses of haloarenes.

10. Alcohols

  1. 10.1 Describe nomenclature, isomerism and classification of monohydric alcohol.
  2. 10.2 Distinguish primary, secondary and tertiary alcohols by Victor Meyer’s Method.
  3. 10.3 Show the preparation of monohydric alcohols.
  4. 10.4 Explain the industrial preparation of alcohol.
  5. 10.5 Define various terms related to alcohol.
  6. 10.6 State physical properties of monohydric alcohols.
  7. 10.7 Explain chemical properties of monohydric alcohols.

11. Phenols

  1. 11.1 Describe nomenclature of phenol.
  2. 11.2 Show the preparation of phenol.
  3. 11.3 State physical properties of phenol.
  4. 11.4 Describe acidic nature of phenol.
  5. 11.5 Explain the chemical properties of phenol.
  6. 11.6 Describe test of phenol.
  7. 11.7 State important uses of phenol.

12. Ethers

  1. 12.1 Describe nomenclature, classification and isomerism of ethers.
  2. 12.2 Show the preparation of ethers by Williamson’s synthesis.
  3. 12.3 State physical properties of ether.
  4. 12.4 Explain chemical properties of ethoxyethane.
  5. 12.5 State important uses of ethers.

13. Aldehydes and Ketones

  1. 13.1 Describe nomenclature and isomerism of aliphatic aldehydes and ketones.
  2. 13.2 Show the preparation of aldehydes and ketones.
  3. 13.3 State physical properties of aldehydes and ketones.
  4. 13.4 Describe structure and nature of carbonyl group.
  5. 13.5 Explain chemical properties of aliphatic aldehydes and ketones.
  6. 13.6 Action of aldehyde and ketone with ammonia derivatives.
  7. 13.7 Aldol condensation, Cannizzaro’s reaction, etc.
  8. 13.8 Other reactions of aldehydes and ketones.
  9. 13.9 Distinguish between aliphatic aldehydes and ketones.
  10. 13.10 Define formalin and state its uses.
  11. 13.11 Show the preparation of benzaldehyde and acetophenone.
  12. 13.12 Explain chemical properties of benzaldehyde.

14. Carboxylic Acid and its Derivatives

  1. 14.1 Describe nomenclature and isomerism of carboxylic acids.
  2. 14.2 Show the preparation of monocarboxylic acids.
  3. 14.3 Show the preparation of benzoic acid.
  4. 14.4 State physical properties of monocarboxylic acids.
  5. 14.5 Explain chemical properties of carboxylic acids.
  6. 14.6 Hell Volhard-Zelinsky reaction and electrophilic substitution.
  7. 14.7 Explain effect of constituents on the acidic strength.
  8. 14.8 Describe abnormal behaviour of methanoic acid.
  9. 14.9 Show the preparation of acid derivatives.
  10. 14.10 Explain the comparative physical properties of acid derivatives.
  11. 14.11 Explain the comparative chemical properties of acid derivatives.
  12. 14.12 Claisen condensation and Hofmann bromamide reaction.
  13. 14.13 Describe amphoteric nature of amide and relative reactivity of acid derivatives.

15. Nitro Compounds

  1. 15.1 Describe nomenclature and isomerism of nitro compounds.
  2. 15.2 Show the preparation from haloalkane and alkane.
  3. 15.3 State physical properties of nitro compounds.
  4. 15.4 Explain chemical properties of nitro compounds.
  5. 15.5 Show preparation of nitrobenzene.
  6. 15.6 State physical properties of nitrobenzene.
  7. 15.7 Explain chemical properties of nitrobenzene.
  8. 15.8 State important uses of nitro compounds.

16. Amines

  1. 16.1 Describe nomenclature, classification and isomerism of amines.
  2. 16.2 Show the separation of amines by Hoffmann’s method.
  3. 16.3 Show preparation of primary amines.
  4. 16.4 State physical properties of aliphatic amines.
  5. 16.5 Explain chemical properties of aliphatic amines.
  6. 16.6 Reaction and test of primary, secondary and tertiary amines.
  7. 16.7 Show preparation of aniline.
  8. 16.8 State physical properties of aromatic amine.
  9. 16.9 Explain chemical properties of aromatic amine.
  10. 16.10 State important uses of aniline.

17. Organometallic Compounds

  1. 17.1 Describe general formula and examples of organometallic compounds.
  2. 17.2 Explain the nature of Metal-Carbon bond.
  3. 17.3 Define Grignard reagent.
  4. 17.4 Show the preparation of Grignard reagent.
  5. 17.5 Explain reactions of Grignard reagent.

Content Area: Applied Chemistry

18. Chemistry in the Service of Mankind

  1. 18.1 Explain addition and condensation polymers.
  2. 18.2 Explain elastomers and fibres.
  3. 18.3 Describe natural and synthetic polymers.
  4. 18.4 Explain some synthetic polymers.
  5. 18.5 Explain types of dyes.
  6. 18.6 Describe characteristics of drugs.
  7. 18.7 Differentiate natural and synthetic drugs.
  8. 18.8 Classify some common drugs.
  9. 18.9 Be aware of adverse effect of drug addiction.
  10. 18.10 Explain insecticides, herbicides and fungicides.

19. Cement

  1. 19.1 Explain introduction and raw materials for cement production.
  2. 19.2 Give main steps in cement production.
  3. 19.3 Explain OPC and PPC cement.
  4. 19.4 Explain Portland cement process with flow-sheet diagram.
  5. 19.5 Explain cement Industry in Nepal.

20. Paper and Pulp

  1. 20.1 Explain raw materials, sources of raw materials and stages in production of paper.
  2. 20.2 Give flow-sheet diagram for paper production.
  3. 20.3 Describe quality of paper.

21. Nuclear Chemistry and Applications of Radioactivity

  1. 21.1 Describe natural and artificial radioactivity.
  2. 21.2 Give units of radioactivity.
  3. 21.3 Explain nuclear reactions.
  4. 21.4 Distinguish between nuclear fission and fusion reactions.
  5. 21.5 Describe nuclear power and nuclear weapons.
  6. 21.6 Explain industrial uses of radioactivity.
  7. 21.7 State the medical uses of radioactivity.
  8. 21.8 Explain radiocarbon dating.
  9. 21.9 Describe harmful effects of nuclear radiations.
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