Grade XI NEB Syllabus – NEB Chemistry Syllabus


Chemistry Syllabus



NEB Chemistry Syllabus is theory-cum-practical. It is intended to consolidate learning in chemistry achieved in secondary school. 


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               Grade XI NEB Syllabus – NEB Chemistry Syllabus




Grade: XI
Full marks: 100(75T+25P)

Pass Marks: 27T+10P

Teaching Hours: 150T+50P

I. Introduction of NEB Chemistry Syllabus

NEB Chemistry is concerned with the physical and chemical characteristics of substances, the nature of matter and the study of chemical reactions. Chemistry, thus, is a powerful process of uncovering and extending our understanding of various chemical phenomena. The power resides in the combination of concepts and experiments involving careful observation and quantitative measurements under controlled conditions. The resulting concepts suggest further experiments and investigations as a result; there will be a modification of the existing concept leading to the creativity of thought. This creativity involves the recognition of a problem formulation of ideas to solve the problem and ultimately refinement of the original ideas. The present curriculum aims to foster this uniqueness among students by enabling them to study both theoretical and practical aspects of chemistry.
 This course is theory-cum-practical. It is intended to consolidate learning in chemistry achieved in secondary school. Furthermore, it intends to provide a piece of concrete knowledge and appropriate skills for those students, continuing further studies in chemistry and the students not studying the subject beyond this stage. The course seeks to maintain a balance between useful facts concepts and theories which will facilitate understanding of the properties of substances, reactions, and processes. Emphasis is enforced to stimulate, create and sustain students’ interest in
Chemistry being an experimental science, the laboratory is an essential component of its syllabus. The course intends to make students aware of the importance of the scientific method for accurate experimental work and develop the abilities to interpret, organize and evaluate data in order to make decisions and solve problems.
II.      General Objectives of NEB Chemistry Syllabus

The general objectives of Chemistry Syllabus are to:
1. apply appropriate chemical principles, concepts, theories, definitions, laws, models and patterns to interpret, dear conclusion, make a generalization, and predictions from chemical facts, observations and experimental data;
2. select appropriate facts to illustrate a given principle, concept, theory, model and pattern;
3. present chemical ideas in a clear and logical form, and
4. select and organize data and perform calculations in which guidance on the method is not supplied.
III.  Specific Objectives of NEB Chemistry Syllabus

After studying the NEB Chemistry, the student shall be able to:
1. State and apply fundamental facts and principles of chemistry dealing with the  I. Methods of Preparation: general, laboratory and industrial process of the matters.

II. Physical and Chemical Properties,
III.Important applications
2. perform chemical calculations:
3. identify the mineral resources of Nepal;
4. understand chemical patterns and principles;
5. apply knowledge and understanding of chemistry in familiar and unfamiliar situations;
6. make accurate observations and measurements, being aware of possible sources of error;
7. record the results of experiments accurately and clearly; draw a conclusion and make a generalization from experiment; and
8.  appreciate the scientific, social, economic, environmental, and technological contributions and applications of chemistry.
General and Physical Chemistry Syllabus(Section A)

Unit 1: Language of Chemistry (Review Lecturers) 

                                                        3 Teaching hrs 

1.Chemical equations, their significances, and 


2. Balancing chemical equations by:

     i.   Hit and trial method 

ii. Partial equation method 

3. Types of chemical reaction


Unit 2. Chemical Arithmetic                           17 teaching hours

2.1 Dalton’s atomic theory and laws of Stoichiometry:
1.Postulates of Dalton’s atomic theory
2.Law of conservation of mass
3.Law of constant proportions
4.Law of multiple proportions
5.Law of reciprocal proportions
6.Law of gaseous volumes
7.Chemical calculations based on stoichiometry
2.2. Atomic Mass and Molecular Mass:
Definition of atomic mass and molecular mass
1.Mole concept
2.Mole in term of mass, volume number and ions
3.Calculation based on mole concept
2.3. Empirical, Molecular Formula and Limiting reactants:
1.Percentage compositions
2.Derivation of empirical and molecular formula from percentage composition
3.Chemical calculation based on the following the chemical equation
 Limiting reactants
 Mass-mass relationship
 Volume- volume relationship
 Mass volume relationship
(solving reacted numerical problems)
2.4. Avogadro’s Hypothesis and Its Applications:
1.  Development of Avogadro’s Hypothesis
2.  Definition of Avogadro’s Hypothesis
3.  Application of Avogadro’s Hypothesis
i. Deduction of atomicity of elementary gas 

ii. Deduction of the relationship between molecular mass and vapor density 

iii.  Deduction of molar volume of gases

iv. Deduction of molecular formula from its volumetric composition  (Solving related numerical problems)
2.5. Equivalent Masse:
1.Concept of equivalent mass
2.Equivalent weight of elements, and compounds (Salt, acid, base, oxidizing agent reducing agents)
3.Gram equivalent weight (GEW)
4.Relation between equivalent weight, valency and atomic weight
5.Determination of the equivalent weight of metal by
i.    Hydrogen displacement method 
ii. Oxide formation method (Solving related numerical problems)
Unit 3. State of Matter                                                              14 Teaching hours
3.1.  Gaseous State: 
1.Boyle’s law.
2.Charle’s law and Kelvin scale of temperature
3.application of Charles law and  Boyle’s law
4.Combined gas law, ideal gas equation an universal gas constant
5.Dalton’s law of partial pressure
6.Mathematical derivation of Dalton’s law and their applications
7.Graham’s law of diffusion and its applications
8.Kinetic model of gas and its postulates
9.Ideal and real gases
10.Deviation of gas from ideal behavior
(solving related numerical problems)
3.2.  Liquid State:
1.  Physical properties of liquid
i. Evaporation and condensation
ii.Vapor pressure of liquid and boiling
iii. Surface tension
2.  Solution and solubility:
i. Equilibrium in saturated solution 
ii. Solubility and solubility curve and its application.
(Solving related numerical problems)
3.3. Solid State
1.Crystalline and amorphous solids
2.water of crystallization
6.Seven types of crystal system
7.Simple cubic, face entered and body-centered

Unit 4: Atomic structure                                                                   10 teaching hrs
1.Discovery of fundamental particles of an atom (electron, proton, and neutron)
2.concept of atomic number, mass number, fractional atomic mass, isotopes, isobars
3.Rutherford’s   ray scattering experiment and nuclear model of atom; limitation 
4.Bohr’s model of atom and explanation of hydrogen spectra
5.Limitation of Bohr’s model of the atom
6.Elementary idea of quantum mechanical model
i. Dual nature of electron (de-Broglie equation) 

ii.Heisenberg’s uncertainty principle 

iii.Probability concept
7.The shape of atomic orbital ( s and p orbitals only)
8.Quantum numbers
9.Pauli’s exclusion principle
10.Hund’s rule of Maximum multiplicity
11.Aufbau principle and Bohr Bury rule
12.Electronic configuration of the atoms and ions(Z= 1 to 30)
Unit 5: Nuclear Chemistry                                       3 Teaching hrs
1.Concept radioactivity
2.Radioactive rays (alpha ray, Beta ray & gamma ray)
3.Meaning of natural and artificial radioactivity
4.Nuclear reactions, Nuclear energy (fission and fusion)
5. Nuclear isotopes and uses
Unit 6: Electronic Theory of Valency and Bonding                         8 Teaching hrs
1.The basic assumption of electronic theory of valency
2. Octet rule
3. Ionic bonds, ionic compounds, and characteristics of ionic compounds. Lewis symbol to represent the formation of ionic compounds
4.Covalent bonds, covalent compounds, and characteristics of the covalent compound- Lewis structure of some typical covalent compounds
5.coordinate covalent bonds. Lewis structures of some typical co-ordinate covalent compounds
6.The exception of the octet rule
7.Partial ionic characters of covalent compounds. Non-polar and polar covalent molecules
8.Dipole moments and its application
9.Some special types of bonds: hydrogen bond and its types, metallic bond, Vander Waal’s bond, resonance, and resonance hybrid structures of O3, SO3, SO2, CO3-2, SO4-2, PO4-2, NO3-
10.Classification of crystalline solids
i. Ionic solid
ii.Covalent solid
iii.Molecular solid
iv.Metallic solid
Unit 7: Periodic classification of Elements                 6 Teaching hrs
1.      Introduction
2.      Mendeleev’s periodic law and the periodic table
3.      Anomalies of Mendeleev’s periodic table
4.      Modern periodic law and the modern periodic table
5.      Advantages of the modern periodic table
6.      Division of elements into s, p, d and f blocks
7.      Periodicity of physical properties: valency, atomic radii, ionic radii ionization energy, electron affinity and electronegativity (general trends only)
Unit 8: Oxidation and Reduction                                                           6 teaching hours
1.      The classical concept of oxidation and reduction
2.      Electronic interpretation of oxidation and reduction
3.      Oxidation number and rules for the assignment of oxidation number
4.      Differentiate between oxidation number and valency
5.      The oxidizing and reducing agent
6.      Redox reaction
7.      Balancing redox reactions by
i.                    Oxidation number method
ii.                  ion-electron method
Unit 9: Equilibria                                                                                     5 Teaching hrs
1.      Introduction
2.      Equilibrium involving in physical change 3. Chemical equilibrium
          Reversible and irreversible reactions
          Dynamic nature of chemical equilibrium and its characteristics
          Law of Mass action
          The equilibrium constant (Kc) and its characteristics
          Homogenous and heterogeneous equilibrium
          The relation between Kp and Kc (derivation)
          Le-chatelier’s Principle and its application
(No numerical is required)
Inorganic NEB Chemistry Syllabus
Section B
Unit 10: Non- Metals I                                                                   12 Teaching hrs
10.1. Hydrogen.
1.      Position in Periodic table
2.      Atomic hydrogen, Nascent hydrogen
3.      Isotopes o Hydrogen
4.      Ortho and parahydrogen
5.      Applications
10.2. Oxygen
1.      Position in Periodic table
2.      Types of oxides
3.      Uses of oxygen
10.3. Ozone:
1.      Occurrence
2.      Preparation from oxygen
3.      Structure of ozone
4.      Important properties of  ozone
5.      Ozone layer and the ozone hole
6.      Uses of ozone
10.4. Water:
1.      Structure 
2.      Solvent property of water
3.      Heavy water and uses
4.      Uses
10.5. Nitrogen and Its Compounds:
1.      Position of nitrogen in the periodic table
2.      Uses of nitrogen
3.      Types of nitrogen oxides (name and Lewis structure)
4.      Ammonia
          manufacture by Haber’s synthesis method
          Physical properties, chemical properties and uses
5.      Oxyacids of nitrogen (type)
6.      Technical production of nitric acid by Ostwald method
          Properties of nitric acid and uses
          Taste of nitrate ion

Unit 11: Non- Metals II                                                          23 teaching hours
11.1 Halogens: (Chlorine, Bromine, and Iodine)
1.  Position in the periodic table
2.  Comparative study on preparation, properties, and uses
3.  Manufacture of bromine from carnallite process and manufacture of iodine from,
  i. Seaweeds (Principle only) ii. Caliche (Principle only)
4.  Uses of halogens
5.  Comparative study on; preparation, properties, and uses of haloacids (HCl, HBr, and HI)
11.2 Carbon:
1.  Position in the periodic table
2.  Allotropes of carbon including fullerenes
3.  Laboratory preparation, properties and uses of carbon monoxides
11.3  Phosphorous:
1.Occurrence, position in the periodic table
2.Allotropes of phosphorous and uses of phosphorus
3.preparation, properties, and uses of phosphine
4.Oxides and oxyacids of phosphorous (structure and uses)
5.Preparation, properties, and uses of orthophosphoric acid
11.4  Sulphur:
Position in periodic table and allotropes
1.Hydrogen Sulphide : (Laboratory methods and Kipp’s apparatus), properties and uses of
2.Sulphur dioxide: Laboratory preparation, preparation, and uses
3.Sulphuric acid: Manufacture by contact process, properties and uses
4.Sodium thiosulphate (hypo): formula and uses
11.5  Boron and silicon :
1.  Occurrences, position in the periodic table
2.  Properties and uses
3.  Formula and uses of burax, boric acid, silicate and silica 11.6 Noble gas: Position in the periodic table, occurrence and uses
11.7. Environmental pollution:
     Air pollution, photochemical smog
     Acid rain, water pollution
     Greenhouse effect
Unit 12: Metal and metallurgical principles                                       6 teaching hours
1.      Characteristics of metals, non-metals, and metalloids
2.      Minerals and ores
3.      Important minerals deposit in Nepal
4.      The different process involved in metallurgical process
5.      Concentration
6.      Calcination and roasting
7.      Smelting
8.      Carbon reduction process
9.      Thermite process
10.  Electrochemical reduction
11.  Refining of metals: poling, electro-refinement, etc
Unit 13: Alkali and Alkaline Earth Metals                              10 teaching hours
1.      Periodic discussion and general characteristics.
2.      Sodium: Occurrence, Extraction from Downs process, properties and uses.
3.      Sodium hydroxide: Manufacture, properties and uses 4. Sodium carbonate: Manufacture, properties, and uses.
13.1 Alkaline Earth Metals :
1.  Periodic discussion and general characteristics
2.  Preparation, properties, and uses of 
i. quick lime 
ii. Plaster of Paris
iii. bleaching powder 
 iv. magnesia v. Epsom salt.
Organic chemistry Syllabus
Section C
Unit 14. Introduction to Organic Chemistry
14.1 Fundamental principles                                                 6 teaching hours
1.   Definition of organic chemistry and organic compounds
2.   Origin of organic compounds (vital force theory)
3.   Reasons for the separate study of organic compounds
4.   Tetra covalency and catenation property of carbon
5.   Classification of organic compounds 
6.   Functional groups and homologous series
7.   Meaning of empirical formula, molecular formula, structural formula and contracted formula
8.   Qualitative analysis of organic compounds. (detection of N, S, and halogens by Lassaegne’s test
14.2 Nomenclature of Organic Compounds: 6 teaching hours
1.  Common names
2.  IUPAC system and IUPAC rules of naming hydrocarbons, alcohols, ethers, aldehydes, ketones carboxylic acid, amines, ester, acid derivative halogen derivatives, nitriles etc.)
14.3 Structure Isomerism in Organic Compounds: 2 teaching hours
1.  Definition of structure isomerism
2.  Types of structure isomerism: chain isomerism, position, isomerism, functional isomerism and metamerism
14.4 Preliminary Idea of reaction mechanism                         2 teaching hours
1.  Concept of homolytic and heterolytic fission
2.  Electrophile, nucleophiles and free- radicals
3.  Inductive the effect, +I, -I effect
Unit 15: Hydrocarbons
15.1  Sources :                                                                                               4 teaching hours
Origin of coal and petroleum, hydrocarbon from petroleum cracking and reforming, aliphatic and aromatic hydrocarbon form coal, quality of gasoline, octane member and gasoline additive.
15.2  Alkanes (saturated hydrocarbons):
1. General methods of preparations:
   Catalytic Hydrogenation
   Reduction of haloalkane
   Kolbe’s electrolysis method
   Using Grigrand’s reagent
   Wurtz reaction
   Form aldehydes and ketones
2.  Physical properties
3.  Chemical properties: Substitutions reaction, oxidation, pyrolysis or cracking aromatization
15.3 Alkenes: 4 teaching hours
1. General methods of preparation
         Dehydration of alcohol
         Catalytic hydrogenation of alkyne   Kolbe’s electrolysis
2.  Laboratory preparation of alkene
3.  Chemical properties of alkene: addition reaction  (H2, X2, HX2, H2O, O3, H2SO4)
4.  Oxidation with alkaline KMnO4 (Baeyer’s reaction)
5.  Polymerization
6.  Test of ethene and uses
15.4 Alkynes :                                                                                                 3 teaching hours
1.            Preparation form i. carbon and hydrogen ii. Kolbe’s electrolysis iii. 1,2 dibromoethane
2.            Lab preparation of ethyne
3.            Physical properties
4.            Chemical Properties: Addition (H2, X2, HX, H2O, O3), Acidic nature (action with ammonical AgNO3and ammonical Cu2Cl2), Oxidation with alkaline KMnO4,
Polymerization uses of ethyne
5.            Practical
Full marks: 25
Pass marks: 10
Students are required to secure the pass marks in the practical paper separately. The following is a list of experiments. The students are required to perform in the practical classes in Grade XI.
A. Experiments based on laboratory techniques:NEB Chemistry Syllabus
1.      To separate the insoluble component in the pure and dry state from the given mixture of soluble and insoluble solids. (NaCl and sand)
2.      To separate volatile component from the given mixture of volatile and non-volatile (demonstration of sublimation process)
3.      To separate a mixture of two soluble solids by fractional crystallization (KNO3+NaCl)
4.      To prepare a saturated solution of impure salt and obtain the pure crystal of the same salt by crystallization
5.      To separate the component of a mixture of two insoluble solids (the being soluble in dil acids)
6.      To obtain pure water from a given sample of water (Distillation)
B. Experiment to study the different reactions (Neutralization, Precipitation, Redox reaction, electrolysis) :
7.         To perform precipitation reaction of BaCl2and H2SO4 and obtain solid BaSO4,,
8.         To neutralize sodium hydroxide with hydrochloric acid solution  and recover the crystal of sodium chloride
9.         To test the ferrous ions in the given aqueous solution and oxidize it to ferric ion
(FerrousFerric system) Redox Reaction
10.     To study the process of electrolysis and electroplating C. Experiments on quantitative analysis :
11.     To determine the equivalent weight or weight of metal by hydrogen displacement method:
12.     To determine the solubility of the given soluble solid at laboratory temperature
13.     To determine the relative surface tension of unknown liquid by frop count method; and
14.     To study the rate of flow of liquid through Ostwald’s viscometer and determine the relative viscosity of the unknown liquid
D. Experiments on the preparation of gas and study of properties:
15.    To prepare and collect hydrogen gas and study the following properties;
a.       Solubility with water, color, odor;
b.      Litmus test;
c.       burning match stick test; and
d.      Reducing properties of nascent hydrogen.
16.    To prepare and collect ammonia gas and investigate the following properties :
a.       Solubility with water/color/odor;
b.      Litmus test;
c.       Action with copper sulphate solution; and
d.      Action with mercurous nitrate paper.
17.    To prepare carbon dioxide gas and investigate the following properties:
a.       Solubility, Colour, odour,
b.      Litmus paper test
c.       Lime water test; and
d.      Action with burning magnesium ribbon.
18.    To study the properties of hydrogen sulphide (Physical, analytical and reducing);
19.    To study the following properties of sulphuric acid:
a.       Solubility with water;
b.      Litmus paper test;
c.       Precipitating reaction; and
d.      Dehydrating reaction.
E. Experiments of qualitative analysis:

20. To detect the basic radical of the given salt by the dry way and the acid radical by dry and wet ways.
Basic radicals : Zn++, Al++, NH4+, Ca++, Na+
Acid radicals: CO3, SO4,  NO3, Br, I, Cl
Note: Experiment from 1 to 19 requires one practical period of each experiment and the experiment no 20 requires four practical periods. (Two theory periods will be equivalent to one practical period)
Evaluation scheme
The chemistry theory paper (XI) will consist of three types of questions:
(a)               Very short answer questions (weightage of 2 marks of each)
(b)               Short answer questions (weightage of 5 marks of each); and
(c)               Long answer questions (weightage of 10 marks of each)
According to the manner of questions, groups are divided into group ‘A’, group ‘B’ and group ‘C’
1.      Group ‘A’ will consist of twenty-two (22) very short questions, out of which, examinees are required to answer only fifteen (15) questions.
2.      Group ‘B’ will consist of seven (7) short questions out of which examinees are required to answer five (5) questions.
3.      Group ‘C’ will consist of four (4) questions, out of which examinees are required to answer 2 questions.
The weightage of content distribution for the three types of questions form different sections of the curriculum will be as follows:
Teaching hours

Reference book of NEB Chemistry 

1. Acharya, Suk Dev,, Fundamentals of Chemistry-XI, Bhudipuran Prakashan, Ktm


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One thought on “Grade XI NEB Syllabus – NEB Chemistry Syllabus

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