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NEB Class 11 Chemistry Syllabus 2080

NEB Class 11 Chemistry Syllabus 2080; CDC Updated Grade 11th Chemistry Syllabus for NEB Exam 2080-2081.
NEB Class 11 Chemistry Syllabus 2080

NEB Class 11 Chemistry Syllabus 2080

NEB Grade 11 Updated Chemistry Course Content. CDC Latest Syllabus for Grade 11 Chemistry for NEB Exams 2080-2081.

Subject Chemistry
Grades 11
Subject code Che. 301 (Grade 11)
Credit hrs 5 hrs
Working hrs 160 hrs
Also Check: Class 11 Model Question (All Subject)

NEB Class 11 Chemistry Chapters List

Class 11

General and physical chemistry

1. Foundation and Fundamentals
2. Stoichiometry 
3. Atomic structure
4. Classification of elements and periodic table
5. Chemical bonding and shapes of molecules
6. Oxidation and reduction
7. States of matter
8. Chemical equilibrium

Inorganic chemistry

9. Chemistry of Non-metals
10. Chemistry of metals
11. Bio-inorganic chemistry

Organic chemistry

12. Basic concept of organic chemistry
13. Fundamental principles
14. Hydrocarbons
15. Aromatic hydrocarbons

Applied chemistry

16. Fundamentals of applied chemistry
17. Modern chemical manufactures

NEB Class 11 Chemistry Curriculum and Syllabus

Unit Content

General and physical chemistry

1. Foundation and Fundamentals (2 hr)

1.1 General introduction of chemistry

1.2 Importance and scope of chemistry

1.3 Basic concepts of chemistry (atoms, molecules, relative masses of atoms and molecules, atomic mass unit ( amu), radicals, molecular formula, empirical formula )

1.4 Percentage composition from molecular formula

2. Stoichiometry (8 hr)

2.1 Dalton’s atomic theory and its postulates

2.2 Laws of stoichiometry

2.3 Avogadro’s law and some deductions

2.3.1 Molecular mass and vapour density

2.3.2 Molecular mass and volume of gas

2.3.3 Molecular mass and no. of particles

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 (Solving related numerical problems)

3. Atomic structure (8 hr)

3.1 Rutherford's atomic model

3.2 Limitations of Rutherford's atomic model

3.3 Postulates of Bohr’s atomic model and its application

3.4 Spectrum of hydrogen atom

3.5 Defects of Bohr’s theory

3.6 Elementary idea of quantum mechanical model: de Broglie's wave equation

3.7 Heisenberg's Uncertainty Principle

3.8 Concept of probability

3.9 Quantum Numbers

3.10 Orbitals and shape of s and p orbitals only

3.11 Aufbau Principle

3.12 Pauli’s exclusion principle

3.13 Hund’s rule and electronic configurations of atoms and ions (up to atomic no. 30)

4. Classification of elements and periodic table (5 hr)

4.1 Modern periodic law and modern periodic table

4.1.1 Classification of elements into different groups, periods and blocks

4.2 IUPAC classification of elements

4.3 Nuclear charge and effective nuclear charge

4.4 Periodic trend and periodicity 4.4.1 Atomic radii

4.4.2 Ionic radii

4.4.3 Ionization energy 

4.4.4 Electron affinity 

4.4.5 Electronegativity

4.4.6 Metallic characters (General trend and explanation only)

5. Chemical bonding and shapes of molecules (9 hr)

5.1 Valence shell, valence electron and octet theory

5.2 Ionic bond and its properties

5.3 Covalent bond and coordinate covalent bond

5.4 Properties of covalent compounds

5.5 Lewis dot structure of some common compounds of s and p block elements

5.6 Resonance

5.7 VSEPR theory and shapes of some simple molecules (BeF2, BF3, CH4, CH3Cl, PCl5, SF6, H2O,NH3,CO2,H2S, PH3)

5.8 Elementary idea of Valence Bond Theory

5.9 Hybridization involving s and p orbitals only

5.10 Bond characteristics: 5.10.1 Bond length 5.10.2 Ionic character 5.10.3 Dipole moment

5.11 Vander Waal’s force and molecular solids

5.12 Hydrogen bonding and its application

5.13 Metallic bonding and properties of metallic solids

6. Oxidation and reduction (5 hr)

6.1 General and electronic concept of oxidation and reduction

6.2 Oxidation number and rules for assigning oxidation number

6.3 Balancing redox reactions by oxidation number and ion-electron (half reaction) method

6.4 Electrolysis

6.4.1 Qualitative aspect

6.4.2 Quantitative aspect(Faradays laws of electrolysis)

7. States of matter (8 hr)

7.1 Gaseous state

7.1.1 Kinetic theory of gas and its postulates

7.1.2 Gas laws

7.1.2.1 Boyle’s law and Charles' law

7.1.2.2 Avogadro's law

7.1.2.3 Combined gas equation

7.1.2.4 Dalton's law of partial pressure

7.1.2.5 Graham's law of diffusion

7.1.3 Ideal gas and ideal gas equation

7.1.4 Universal gas constant and its significance

7.1.5 Deviation of real gas from ideality (Solving related numerical problems based on gas laws)

7.2 Liquid state

7.2.1 Physical properties of liquids

7.2.1.1 Evaporation and condensation

7.2.1.2 Vapour pressure and boiling point

7.2.1.3 Surface tension and viscosity (qualitative

idea only)

7.2.2 Liquid crystals and their applications

7.3 Solid state

7.3.1 Types of solids

7.3.2 Amorphous and crystalline solids

7.3.3 Efflorescent, Deliquescent and Hygroscopic solids

7.3.4 Crystallization and crystal growth

7.3.5 Water of crystallization

7.3.6 Introduction to unit crystal lattice and unit cell

8. Chemical equilibrium (3 hr)

8.1 Physical and chemical equilibrium

8.2 Dynamic nature of chemical equilibrium

8.3 Law of mass action

8.4 Expression for equilibrium constant and its importance

8.5 Relationship between Kp and Kc

8.6 Le Chatelier’s Principle (Numericals not required)


Inorganic chemistry

9. Chemistry of Non-metals (22 hr)

9.1 Hydrogen

9.1.1 Chemistry of atomic and nascent hydrogen

9.1.2 Isotopes of hydrogen and their uses

9.1.3 Application of hydrogen as fuel

9.1.4 Heavy water and its applications

9.2 Allotropes of Oxygen

9.2.1 Definition of allotropy and examples

9.2.2 Oxygen: Types of oxides (acidic, basic, neutral, amphoteric, peroxide and mixed oxides)

9.2.3 Applications of hydrogen peroxide

9.2.4 Medical and industrial application of oxygen

9.3 Ozone

9.3.1 Occurrence

9.3.2 Preparation of ozone from oxygen

9.3.3 Structure of ozone

9.3.4 Test for ozone

9.3.5 Ozone layer depletion (causes, effects and control measures)

9.3.6 Uses of ozone

9.4 Nitrogen

9.4.1 Reason for inertness of nitrogen and active nitrogen

9.4.2 Chemical properties of ammonia [ Action with CuSO4 solution, water, FeCl3 solution, Conc. HCl, Mercurous nitrate paper, O2 ]

9.4.3 Applications of ammonia

9.4.4 Harmful effects of ammonia

9.4.5 Oxy-acids of nitrogen (name and formula)

9.4.6 Chemical properties of nitric acid [HNO3 as an acid and oxidizing agent (action with zinc, magnesium, iron, copper, sulphur, carbon, SO2 and H2S)

9.4.7 Ring test for nitrate ion 

9.5 Halogens

9.5.1 General characteristics of halogens

9.5.2 Comparative study on preparation (no diagram and description is required),

9.5.2.1 Chemical properties [with water, alkali, ammonia, oxidizing character, bleaching action] and uses of halogens (Cl2, Br2 and I2)

9.5.3 Test for Cl2, Br2 and I2

9.5.4 Comparative study on preparation (no diagram and description is required), properties ( reducing strength, acidic nature and solubility) and uses of haloacids (HCl, HBr and HI)

9.6 Carbon

9.6.1 Allotropes of carbon (crystalline and amorphous) including fullerenes (structure, general properties and uses only)

9.6.2 Properties (reducing action, reaction with metals and nonmetals) and uses of carbon monoxide

9.7 Phosphorus

9.7.1 Allotropes of phosphorus (name only)

9.7.2 Preparation (no diagram and description is required), properties ( basic nature ,reducing nature , action with halogens and oxygen) and uses of phosphine

9.8 Sulphur

9.8.1 Allotropes of sulphur (name only) and uses of sulphur

9.8.2 Hydrogen sulphide (preparation from Kipp's apparatus with diagram,) properties (Acidic nature, reducing nature, analytical reagent) and uses

9.8.3 Sulphur dioxide its properties (acidic nature, reducing nature, oxidising nature and bleaching action) and uses

9.8.4 Sulphuric acid and its properties (acidic nature, oxidising nature, dehydrating nature) and uses

9.8.5 Sodium thiosulphate (formula and uses)

10. Chemistry of metals (10 hr)

10.1 Metals and Metallurgical Principles

10.1.1 Definition of metallurgy and its types (hydrometallurgy, pyrometallurgy, electrometallurgy)

10.1.2 Introduction of ores

10.1.3 Gangue or matrix, flux and slag, alloy and amalgam

10.1.4 General principles of extraction of metals (different processes involved in metallurgy) – concentration, calcination and roasting, smelting, carbon reduction, thermite and electrochemical reduction

10.1.5 Refining of metals (poling and electro-refinement)

10.2 Alkali Metals

10.2.1 General characteristics of alkali metals

10.2.2 Sodium [extraction from Down's process, properties (action with Oxygen, water, acids nonmetals and ammonia) and uses]

10.2.3 Properties (precipitation reaction

and action with carbon monoxide) and uses of sodium hydroxide

10.2.4 Properties (action with CO2, SO2, water, precipitation reactions) and uses of sodium carbonate

10.3 Alkaline Earth Metals

10.3.1 General characteristics of alkaline earth metals

10.3.2 Molecular formula and uses of (quick lime, bleaching powder, magnesia, plaster of paris and epsom salt)

10.3.3 Solubility of hydroxides, carbonates and sulphates of alkaline earth metals (general trend with explanation)

10.3.4 Stability of carbonate and nitrate of alkaline earth metals (general trend with explanation)

11. Bio-inorganic chemistry (3 hr)

11. Introduction to Bio-inorganic Chemistry

11.1 Introduction

11.2 Micro and macro nutrients

11.3 Importance of metal ions in biological systems (ions of Na, K, Mg, Ca, Fe, Cu, Zn, Ni, Co, Cr)

11.4 Ion pumps (sodium-potassium and sodium-glucose pump)

11.5 Metal toxicity (toxicity due to iron, arsenic, mercury, lead and cadmium)


Organic chemistry

12. Basic concept of organic chemistry (6 hr)

12.1 Introduction to organic chemistry and organic compounds

12.2 Reasons for the separate study of organic compounds from inorganic

compounds

12.3 Tetra-covalency and catenation properties of carbon

12.4 Classification of organic compounds

12.5 Alkyl groups, functional groups and homologous series

12.6 Idea of structural formula, contracted formula and bond line structural formula

12.7 Preliminary idea of cracking and reforming, quality of gasoline, octane number, cetane number and gasoline additive

13. Fundamental principles of organic chemistry (10 hr)

13.1 IUPAC Nomenclature of Organic Compounds (upto chain having 6- carbon atoms)

13.2 Qualitative analysis of organic compounds (detection of N, S and halogens by Lassaigne's test)

13.3 Isomerism in Organic Compounds

13.4 Definition and classification of isomerism

13.5 Structural isomerism and its types: chain isomerism, position isomerism, functional isomerism, metamerism and tautomerism

13.6 Concept of geometrical isomerism (cis & trans) & optical isomerism (d & l form)

13.7 Preliminary Idea of Reaction Mechanism

13.7.1 Homolytic and heterolytic fission

13.7.2 Electrophiles, nucleophiles and free- radicals

13.7.3 Inductive effect: +I and –I effect

13.7.4 Resonance effect: +R and –R effect

14. Hydrocarbons (8 hr)

14.1 Saturated Hydrocarbons (Alkanes)

14.1.1 Alkanes: Preparation from haloalkanes (Reduction and Wurtz reaction), Decarboxylation, Catalytic hydrogenation of alkene and alkyne

14.1.2 Chemical properties: Substitution reactions (halogenation, nitration & sulphonation only), oxidation of ethane

14.2 Unsaturated hydrocarbons (Alkenes & Alkynes)

14.2.1 Alkenes: Preparation by Dehydration of alcohol, Dehydrohalogenation, Catalytic hydrogenation of alkyne

14.2.1.1 Chemical properties: Addition reaction with HX (Markovnikov’s addition and peroxide effect), H2O, O3, H2SO4 only

14.3 Alkynes: Preparation from carbon and hydrogen, 1,2 dibromoethane, chloroform/iodoform only

14.3.1 Chemical properties: Addition reaction with (H2, HX, H2O), Acidic nature (action with Sodium, ammoniacal AgNO3 and ammoniacal Cu2Cl2)

14.4 Test of unsaturation (ethene & ethyne): bromine water test and Baeyer's test

14.5 Comparative studies of physical properties of alkane, alkene and alkyne

14.6 Kolbe's electrolysis methods for the preparation of alkane, alkene and alkynes

15. Aromatic hydrocarbons (6 hr)

15.1 Introduction and characteristics of aromatic compounds

15.2 Huckel's rule of aromaticity 15.3 Kekule structure of benzene 15.4 Resonance and isomerism

15.5 Preparation of benzene from decarboxylation of sodium benzoate, phenol, and ethyne only

15.6 Physical properties of benzene

15.7 Chemical properties of benzene: Addition reaction: hydrogen, halogen, Electrophilic substitution reactions: orientation of benzene derivatives (o, m & p), nitration, sulphonation, halogenations, Friedel-Craft's reaction (alkylation and acylation), combustion of benzene ( free combustion only) and uses Phenols


Applied chemistry

16. Fundamentals of applied chemistry (4 hr)

16.1 Fundamentals of Applied Chemistry

16.1.2 Chemical industry and its importance

16.1.3 Stages in producing a new product

16.1.4 Economics of production

16.1.5 Cash flow in the production cycle 

16.1.6 Running a chemical plant

16.1.7 Designing a chemical plant 

16.1.8 Continuous and batch processing

16.1.9 Environmental impact of the chemical industry

17. Modern chemical manufactures (11 hr)

17.1 Modern Chemical Manufactures (principle and flow sheet diagram only)

17.1.1 Manufacture of ammonia by Haber's process,

17.1.2 Manufacture of nitric acid by Ostwald's process,

17.1.3 Manufacture of sulphuric acid by contact process,

17.1.4 Manufacture of sodium hydroxide by Diaphragm Cell

17.1.5 Manufacture of sodium carbonate by ammonia soda or Solvay process

17.2 Fertilizers (Chemical fertilizers, types of chemical fertilizers, production of urea with flow-sheet diagram)


NEB Class 11 Chemistry Syllabus PDF 2080

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