New syllabus (curriculam) of class 11 and 12 chemistry for NEB board Nepal..
Class – 11 Chemistry Syllabus(Nepal)
Subject code : 201
Total working hours : 160 hours.
Theory : 128 teaching hours.
Practical : 32 teaching hours.
Final exam : 100 marks- Out of 100, 75 from theoretical exam and 25 from practical exam+ viva ,records, project works and internal exams.
General and Physical Chemistry : 48 teaching hours.
Unit -1 . Foundation and Fundamentals : 2 teaching hours
General introduction of chemistry, Importance and scope of chemistry, Basic concepts of chemistry (atoms, molecules, relative masses of atoms and molecules, atomic mass unit ( amu), radicals, molecular formula, empirical formula ), Percentage composition from molecular formula.
Unit -2 . Stoichiometry : 8 teaching hours
Dalton’s atomic theory and its postulates , Laws of stoichiometry, Avogadro’s law and some deductions ( Molecular mass and vapour density , Molecular mass and volume of gas, Molecular mass and no. of particles) , Mole and its relation with mass, volume and number of particles; Calculations based on mole concept ; Limiting reactant and excess reactant ;Theoretical yield, experimental yield and % yield ; Calculation of empirical and molecular formula from % composition (Solving related numerical problems)
Unit -3 . Atomic Structure : 8 teaching hours
Rutherford’s atomic model ; Limitations of Rutherford’s atomic model; Postulates of Bohr’s atomic model and its application ; Spectrum of hydrogen atom ; Defects of Bohr’s theory; Elementary idea of quantum mechanical model: de Broglie’s wave equation; Heisenberg’s Uncertainty Principle ; Concept of probability; Quantum Numbers ; Orbitals and shape of s and p orbitals only; Aufbau Principle; Pauli’s exclusion principle; Hund’s rule and electronic configurations of atoms and ions (up to atomic no. 30)
Unit-4. Classification of elements and Periodic Table: 5 teaching hours
Modern periodic law and modern periodic table; Classification of elements into different groups, periods and blocks ; IUPAC classification of elements; Nuclear charge and effective nuclear charge ;Periodic trend and periodicity : Atomic radii ,Ionic radii , Ionization energy , Electron affinity ,Electronegativity , Metallic characters (General trend and explanation only)
Unit-5. Chemical Bonding and Shapes of Molecules : 9 teaching hours
Valence shell, valence electron and octet theory ; Ionic bond and its properties ; Covalent bond and coordinate covalent bond ;Properties of covalent compounds ; Lewis dot structure of some common compounds of s and p block elements ; Resonance ;VSEPR theory and shapes of some simple molecules (BeF2, BF3, CH4, CH3Cl, PCl5, SF6, H2O,NH3,CO2,H2S, PH3); Elementary idea of Valence Bond Theory; Hybridization involving s and p orbitals only ; Bond characteristics: Bond length, Ionic character, Dipole moment; Vander Waal’s force and molecular solids ; Hydrogen bonding and its application; Metallic bonding and properties of metallic solids
Unit-6. Oxidation and Reduction : 5 teaching hours
General and electronic concept of oxidation and reduction; Oxidation number and rules for assigning oxidation number ; Balancing redox reactions by oxidation number and ion-electron (half reaction) method ; Electrolysis : Qualitative aspect and Quantitative aspect(Faradays laws of electrolysis)
Unit-7. States of Matter : 8 teaching hours
7.1 Gaseous state : Kinetic theory of gas and its postulates ;Gas laws -Boyle’s law and Charles’ law, Avogadro’s law ;Combined gas equation ;Dalton’s law of partial pressure ;Graham’s law of diffusion; Ideal gas and ideal gas equation ; Universal gas constant and its significance; Deviation of real gas from ideality (Solving related numerical problems based on gas laws)
7.2 Liquid state : Physical properties of liquids- Evaporation and condensation ,Vapour pressure and boiling point ,Surface tension and viscosity (qualitative idea only) ; Liquid crystals and their applications
7.3 Solid state : Types of solids -Amorphous and crystalline solids, Efflorescent, Deliquescent and Hygroscopic solids ; Crystallization and crystal growth; Water of crystallization; Introduction to unit crystal lattice and unit cell .
Unit-8. Chemical equilibrium: 3 teaching hours
Physical and chemical equilibrium; Dynamic nature of chemical equilibrium; Law of mass action; Expression for equilibrium constant and its importance; Relationship between Kp and Kc ; Le Chatelier’s Principle (Numericals not required)
Inorganic Chemistry : 35 teaching hours
Unit-9. Chemistry of Non-metal :
9.1. Hydrogen, Oxygen and ozone : 4 teaching hours
9.1.1 Hydrogen : Chemistry of atomic and nascent hydrogen ; Isotopes of hydrogen and their uses; Application of hydrogen as fuel ; Heavy water and its applications
9.1.2 Oxygen : Allotropes of Oxygen – Definition of allotropy and examples; Types of oxides (acidic, basic, neutral, amphoteric, peroxide and mixed oxides) ; Applications of hydrogen peroxide; Medical and industrial application of oxygen
9.1.3 Ozone: Occurrence ; Preparation of ozone from oxygen; Structure of ozone; Test for ozone; Ozone layer depletion (causes, effects and control measures) ; Uses of ozone
9.2 Nitrogen : 5 teaching hours
Reason for inertness of nitrogen and active nitrogen ; Chemical properties of ammonia [ Action with CuSO4 solution, water, FeCl3 solution, Conc. HCl, Mercurous nitrate paper, O2 ]; Applications of ammonia; Harmful effects of ammonia ; Oxy-acids of nitrogen (name andformula); Chemical properties of nitric acid [HNO3 as an acid and oxidizing agent (action with zinc, magnesium, iron, copper, sulphur, carbon, SO2 and H2S) ; Ring test for nitrate ion.
9.3 Halogens: 5 teaching hours
General characteristics of halogens; Comparative study on preparation (no diagram and description is required); Chemical properties [with water, alkali, ammonia, oxidizing character, bleaching action] and uses of halogens (Cl2, Br2 and I2); Test for Cl2, Br2 and I2 ; 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)
9.4 Carbon and Phosphorus : 3 teaching hours
9.4.1 Carbon : Allotropes of carbon (crystalline and amorphous) including fullerenes (structure, general properties and uses only) ; Properties (reducing action, reaction with metals and nonmetals) and uses of carbon monoxide
9.4.2 Phosphorus : Allotropes of phosphorus (name only); Preparation (no diagram and description is required), properties ( basic nature ,reducing nature , action with halogens and oxygen) and uses of phosphine.
9.5 Sulphur : 5 teaching hours
Allotropes of sulphur (name only) and uses of sulphur ; Hydrogen sulphide (preparation from Kipp’s apparatus with diagram,) properties (Acidic nature, reducing nature, analytical reagent) and uses ; Sulphur dioxide its properties (acidic nature, reducing nature, oxidising nature and bleaching action) and uses ; Sulphuric acid and its properties (acidic nature, oxidising nature, dehydrating nature) and uses ; Sodium thiosulphate (formula and uses) .
Unit-10. Chemistry of Metals
10.1 Metals and Metallurgical Principles : 5 teaching hours
Definition of metallurgy and its types (hydrometallurgy, pyrometallurgy, electrometallurgy) ; Introduction of ores ; Gangue or matrix, flux and slag, alloy and amalgam ; General principles of extraction of metals (different processes involved in metallurgy) – concentration, calcination and roasting, smelting, carbon reduction, thermite and electrochemical reduction ; Refining of metals (poling and electro-refinement)
10.2 Alkali and Alkaline earth Metals : 5 teaching hours
10.2.1 Alkali Metals : General characteristics of alkali metals ; Sodium [extraction from Down’s process, properties (action with Oxygen, water, acids nonmetals and ammonia) and uses] ; Properties (precipitation reaction and action with carbon monooxide) and uses of sodium hydroxide ; Properties (action with CO2, SO2, water, precipitation reactions) and uses of sodium carbonate
10.2.2 Alkaline Earth Metals : General characteristics of alkaline earth metals ; Molecular formula and uses of (quick lime, bleaching powder, magnesia, plaster of paris and epsom salt); Solubility of hydroxides, carbonates and sulphates of alkaline earth metals (general trend with explanation) ; Stability of carbonate and nitrate of alkaline earth metals (general trend with explanation).
Unit- 11. Bio-inorganic Chemistry : 3 teaching hours
Introduction to Bio-inorganic Chemistry ; Introduction of Micro and macro nutrients ; Importance of metal ions in biological systems (ions of Na, K, Mg, Ca, Fe, Cu, Zn, Ni, Co, Cr) ; Ion pumps (sodium-potassium and sodium-glucose pump) 11.5 Metal toxicity (toxicity due to iron, arsenic, mercury, lead and cadmium)
Organic Chemistry : 30 teaching hours
Unit- 12. Basic Concept of Organic Chemistry : 6 teaching hours
Introduction to organic chemistry and organic compounds ; Reasons for the separate study of organic compounds from inorganic compounds ; Tetra-covalency and catenation properties of carbon ; Classification of organic compounds ; Alkyl groups, functional groups and homologous series ; Idea of structural formula, contracted formula and bond line structural formula ; Preliminary idea of cracking and reforming, quality of gasoline, octane number, cetane number and gasoline additive
Unit 13. Fundamental Principles of Organic Chemistry : 10 teaching hours
IUPAC Nomenclature of Organic Compounds (upto chain having 6 carbon atoms) ; Qualitative analysis of organic compounds (detection of N, S and halogens by Lassaigne’s test) ; Isomerism in Organic Compounds ; Definition and classification of isomerism ; Structural isomerism and its types: chain isomerism, position isomerism, functional isomerism, metamerism and tautomerism ; Concept of geometrical isomerism (cis & trans) & optical isomerism (d & l form)
Preliminary Idea of Reaction Mechanism : Homolytic and heterolytic fission ; Electrophiles, nucleophiles and free- radicals ; Inductive effect: +I and –I effect ; Resonance effect: +R and –R effect .
Unit 14. Hydrocarbons : 8 teaching hours
14.1 Saturated Hydrocarbons (Alkanes): Preparation from haloalkanes (Reduction and Wurtz reaction), Decarboxylation, Catalytic hydrogenation of alkene and alkyne ; Chemical properties: Substitution reactions (halogenation, nitration & sulphonation only), oxidation of ethane ; Unsaturated hydrocarbons (Alkenes & Alkynes) .
14.2 Alkenes: Preparation by Dehydration of alcohol, Dehydrohalogenation, Catalytic hydrogenation of alkyne ; 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 ; Chemical properties: Addition reaction with (H2, HX, H2O), Acidic nature (action with Sodium, ammoniacal AgNO3 and ammoniacal Cu2Cl2) ; Test of unsaturation (ethene & ethyne): bromine water test and Baeyer’s test ;
14.4 Comparative studies of physical properties of alkane, alkene and alkyne; Kolbe’s electrolysis methods for the preparation of alkane, alkene and alkynes
Unit 15. Aromatic Hydrocarbons : 6 teaching hours
Introduction and characteristics of aromatic compounds : Huckel’s rule of aromaticity : Kekule structure of benzene : Resonance and isomerism : Preparation of benzene from decarboxylation of sodium benzoate, phenol, and ethyne only ; Physical properties of benzene ; Chemical properties of benzene: Addition reaction: hydrogen, halogen, Electrophilic substitution reactions: orientation of benzene derivatives (o, m & p), nitration, sulphonation, halogenations, Friedal-Craft’s reaction (alkylation and acylation), combustion of benzene ( free combustion only) and uses.
Applied Chemistry : 15 teaching hours
Unit: 16 Fundamentals of Applied Chemistry : 4 teaching hours
Fundamentals of Applied Chemistry ; Chemical industry and its importance ; Stages in producing a new product ; Economics of production ; Cash flow in the production cycle ; Running a chemical plant; Designing a chemical plant ; Continuous and batch processing ; Environmental impact of the chemical industry.
Unit: 17 Modern Chemical Manufactures : 11 teaching hours
Modern Chemical Manufactures (principle and flow sheet diagram only) ; Manufacture of ammonia by Haber’s process ; Manufacture of nitric acid by Ostwald’s process ; Manufacture of sulphuric acid by contact process ; Manufacture of sodium hydroxide by Diaphragm Cell ; Manufacture of sodium carbonate by ammonia soda or Solvay process ; Fertilizers (Chemical fertilizers, types of chemical fertilizers, production of urea with flow-sheet diagram)
Class- 12 Chemistry syllabus(Nepal)
Subject code : 202
Total working hours : 160 hours.
Theory : 128 teaching hours.
Practical : 32 teaching hours.
Final exam mark : 100 marks- Out of 100, 75 from theoretical exam and 25 from practical exam+ viva ,records, project works and internal exams.
Physical Chemistry: 40 teaching hours
Unit-1. Volumetric Analysis : 8 teaching hrs
Introduction to gravimetric analysis, volumetric analysis and equivalent weight ; Relationship between equivalent weight, atomic weight and valency ; Equivalent weight of compounds (acid, base, salt, oxidizing and reducing agents) ; Concentration of solution and its units in terms of : Percentage, g/L , molarity, molality, normality and formality, ppm and ppb ; Primary and secondary standard substances ; Law of equivalence and normality equation ; Titration and its types: Acid-base titration, redox titration ( related numerical problems)
Unit 2. Ionic Equilibrium : 10 hrs
Introduction to Acids and Bases ; Limitation of Arrhenius concepts of acids and bases ; Bronsted –Lowry definition of acids and bases ; Relative strength of acids and bases ; Conjugate acid –base pairs ; Lewis definition of acids and bases ; Ionization of weak electrolyte (Ostwald’s dilution law) ; Ionic product of water(Kw) ; Dissociation constant of acid and base, (Ka& Kb) ; Concept of pKa and pKb ; pH value: pH of strong and weak acids, pH of strong and weak bases ; Solubility and solubility product principle ; Common Ion effect ; Application of solubility product principle and common ion effect in precipitation reactions ; Buffer solution and its application ; Indicators and selection of indicators in acid base titration; Types of salts: Acidic salts, basic salts, simple salts, complex salts (introduction and examples) ; Hydrolysis of salts : Salts of strong acid and strong base , Salts of weak acid and strong base , Salts of weak base and strong acid (solving related numerical problems)
Unit 3. Chemical Kinetics : 7 hrs
Introduction ; Rate of reactions: Average and instantaneous rate of reactions ; Rate law and its expressions ; Rate constant and its unit and significance; Order and molecularity ; Integrated rate equation for zero and first order reaction ; Half-life of zero and first order reactions ; Collision theory, concept of activation energy and activated complex ; Factors affecting rate of reactions: Effect of concentration, temperature (Arrhenius Equation) and effect of catalyst (energy profile diagram) ; Catalysis and types of catalysis: homogeneous, heterogeneous and enzyme catalysis (solving related numerical problems based on rate, rate constant and order of zero and first order reactions)
Unit 4. Thermodynamics : 8 hrs
Introduction ; Energy in chemical reactions ; Internal energy ; First law of thermodynamics ; Enthalpy and enthalpy changes: Endothermic and exothermic processes) ; Enthalpy of reaction, enthalpy of solution, enthalpy of formation, enthalpy of combustion ; Laws of thermochemistry (Laplace Law and Hess’s law) ; Entropy and spontaneity ; Second law of thermodynamics ; Gibbs’ free energy and prediction of spontaneity ; Relationship between ∆G and equilibrium constant (Solving related numerical problems)
Unit 5. Electrochemistry : 7 hrs
Electrode potential and standard electrode potential ; Types of electrodes: Standard hydrogen electrode and calomel electrodes ; Electrochemical series and its applications ; Voltaic cell: Zn-Cu cell, Ag- Cu cell ; Cell potential and standard cell potential ; Relationship between cell potential and free energy ; Commercial batteries and fuel cells (hydrogen/oxygen)
Inorganic Chemistry : 20 teaching hours.
Unit 6.Transition Metals : 5 hrs
Introduction ; Characteristics of transition metals ; Oxidation states of transition metals ; Complex ions and metal complexes ; Shapes of complex ions ; d-orbitals in complex ions (simple explanation by crystal field theory) for octahedral complex ; Reasons for the colour of transition metal compounds ; Catalytic properties of transition metals
Unit 7. Studies of Heavy Metals : 15 hrs
7.1 Copper : Occurrence and extraction of copper from copper pyrite ; Properties (with air, acids, aqueous ammonia and metal ions) and uses of copper ; Chemistry (preparation, properties and uses) of blue vitriol ; Other compounds of copper (red oxide and black oxide of copper) formula and uses only
7.2 Zinc : Occurrence and extraction of zinc from zinc blende ; Properties (with air, acid, alkali, displacement reaction) and uses of zinc ; Chemistry (preparation, properties and uses) of white vitriol
7.3 Mercury : Occurrence and extraction of mercury from cinnabar ; Properties of mercury ; Chemistry (preparation, properties and uses) of calomel and corrosive sublimate
7.4 Iron : Occurrence and extraction of iron ; Properties and uses of iron ; Manufacture of steel by Basic Oxygen Method and Open Hearth Process ; Corrosion of iron and its prevention
7.5 Silver : Occurrence and extraction of silver by cyanide process ; Preparation and uses of silver chloride and silver nitrate.
Organic Chemistry : 55 teaching hours.
Unit 8. Haloalkanes : 8 hrs
Introduction ; Nomenclature, isomerism and classification of monohaloalkanes ; Preparation of monohaloalkanes from alkanes, alkenes and alcohols ; Physical properties of monohaloalkanes ; Chemical properties, substitution reactions SN1 and SN2 reactions (basic concept only) ; Formation of alcohol, nitrile, amine, ether, thioether, carbylamines, nitrite and nitro alkane using haloalkanes ; Elimination reaction (dehydrohalogenation- Saytzeff’s rule), Reduction reactions, Wurtz reaction ; Preparation of trichloromethane from ethanol and propanone ; Chemical properties of trichloromethane: oxidation, reduction, action on silver powder, conc. nitric acid, propanone, and aqueous alkali.
Unit 9. Haloarenes : 3 hrs
Introduction ; Nomenclature and isomerism of haloarenes ; Preparation of chlorobenzene from benzene and benzene diazonium chloride ; Physical properties ; Chemical properties : Low reactivity of haloarenes as compared to haloalkanes in term of nucleophilic substitution reaction , Reduction of chlorobenzene , Electrophilic substitution reactions , Action with Na (Fittig and Wurtz- Fittig reaction) ; Action with chloral ; Uses of haloarenes.
Unit 10. Alcohols : 7 hrs
Introduction ; Nomenclature; isomerism and classification of monohydric alcohol ; Distinction of primary, secondary and tertiary alcohols by Victor Meyer’s Method ; Preparation of monohydric alcohols from Haloalkane, primary amines, and esters ; Industrial preparation alcohol from: oxo process, hydroboration-oxidation of ethene & fermentation of sugar ; Definition of common terms: Absolute alcohol, power alcohol, denatured alcohol (methylated spirit), rectified spirit; alcoholic beverage ; Physical properties monohydric alcohols ; Chemical properties of monohydric alcohols : Reaction with HX, PX3, PCl5, SOCl2 ; Action with reactive metals like Na, K, Li ; Dehydration of alcohols ; Oxidation of primary, secondary and tertiary alcohol with mild oxidizing agents like acidified KMnO4 or K2Cr2O7 ; Catalyic dehydrogenation of 1⁰ and 2⁰ alcohol and dehydration of 3⁰ alcohol. ; Esterification reaction ; Test of ethanol.
Unit 11. Phenols : 4 hrs
Introduction and nomenclature ; Preparation of phenol from i. chlorobenzene ii. Diazonium salt and iii. benzene sulphonic acid ; Physical properties of phenol ; Chemical properties : Acidic nature of phenol (comparison with alcohol and water) ; Action with NH3, Zn, Na, benzene diazonium chloride and phthalic anhydride ; Acylation reaction, Kolbe’s reaction, Reimer-Tiemann’s reaction ; Electrophilic substitution: nitration, sulphonation, brominaiton and Friedal-Craft’s alkylation ; Test of phenol: (FeCl3 test, aq. Bromine test & Libermann test) ; Uses of phenol .
Unit 12. Ethers : 2 hrs
Introduction ; Nomenclature, classification and isomerism of ethers ; Preparation of aliphatic and aromatic ethers from Williamson’s synthesis ; Physical properties of ether ; Chemical properties of ethoxyethane: action with HI , Conc. HCl, Conc. H2SO4, air and Cl2 , Uses of ethers
Unit 13. aldehydes and Ketones : 10 hrs
Introduction, nomenclature and isomerism ; Preparation of aldehydes and ketones from: Dehydrogenation and oxidation of alcohol, Ozonolysis of alkenes, Acid chloride, Gem dihaloalkane, Catalytic hydration of alkynes ; Physical properties of aldehydes and ketones ; Chemical properties ; Structure and nature of carbonyl group ; Distinction between aldehyde and ketones by using 2,4- DNP reagent, Tollen’s reagent, Fehling’s solution ; Addition reaction: addition of H2, HCN and NaHSO3 13.1.4.4 Action of aldehyde and ketone with ammonia derivatives; NH2OH, NH2-NH2, phenyl hydrazine, semicarbazide ; Aldol condensation ; Cannizzaro’s reaction ; Clemmensen’s reduction 13.1.4.8 Wolf-Kishner reduction ; Action with PCl5 and action with LiAlH4 ; Action of methanal with ammonia and phenol ; Formalin and its uses .
Aromatic aldehydes and Ketones : Preparation of benzaldehyde from toluene and acetophenone from benzene ; Properties of benzaldehyde ; Perkin condensation ; Benzoin condensation ; Cannizzaro’s reaction ; Electrophilic substitution reaction .
Unit 14. Carboxylic Acid and its Derivaties : 9 hrs
Aliphatic and aromatic carboxylic acids : Introduction, nomenclature and isomerism ; Preparation of monocarboxylic acids from: aldehydes, nitriles, dicarboxylic acid, sodium alkoxide and trihaloalkanes ; Preparation of benzoic acid from alkyl benzene ; Physical properties of monocarboxylic acids ; Chemical properties: Action with alkalies, metal oxides, metal carbonates, metal bicarbonates, PCl3, LiAlH4 and dehydration of carboxylic acid ; Hell-Volhard-Zelinsky reaction ; Electrophilic substitution reaction of benzoic acid bromination, nitration and sulphonation) ; Effect of constituents on the acidic strength of carboxylic acid ; Abnormal behaviour of methanoic acid
Derivatives of Carboxylic acids (acid halides, amides, esters and anhydrides) : Preparation of acid derivatives from carboxylic acid ; Comparative physical properties of acid derivatives ; Comparative chemical properties of acid derivatives (hydrolysis, ammonolysis, amines (RNH2), alcoholysis, and reduction only) ; Claisen condensation ; Hofmann bromamide reaction ; Amphoteric nature of amide ; Relative reactivity of acid derivatives.
Unit 15. Nitro Compounds : 3 hrs
Nitroalkanes : Introduction, nomenclature and isomerism ; Preparation from haloalkane and alkane ; Physical properties ; Chemical properties: Reduction ; Nitrobenzene : Preparation from benzene ; Physical properties ; Chemical properties : Reduction in different media ; Electrophilic substitution reactions (nitration, sulphonation & bromination) ; Uses of nitro-compounds .
Unit 16. Amines : 7 hrs
Aliphatic amines : Introduction, nomenclature, classification and isomerism ; Separation of primary, secondary and tertiary amines by Hoffmann’s method ; Preparation of primary amines from haloalkane, nitriles, nitroalkanes and amides ; Physical properties ; Chemical properties: basicity of amines, comparative study of basic nature of 10, 20 and 30 amines ; Reaction of primary amines with chloroform, conc. HCl, R-X, RCOX and nitrous acid (NaNO2 / HCl) ; Test of 10, 20 and 30 amines (nitrous acid test)
Aromatic amine (Aniline) : Preparation of aniline from nitrobenzene, phenol ; Physical properties ; Chemical properties: basicity of aniline, comparison of basic nature of aniline with aliphatic amines and ammonia, alkylation, acylation, diazotization, carbylamine and coupling reaction, electrophilic substitution: Nitration sulphonation and bromination ; Uses of aniline.
Unit 17. Organometallic Compounds : 2 hrs
Introduction, general formula and examples of organolithium, organocopper and organocadmium compounds ; Nature of Metal-Carbon bond ; Grignard reagent : Preparation (using haloalkane and haloarene) ; Reaction of Grignard reagent with water, aldehydes and ketones ( preparation of primary, secondary and tertiary alcohols), carbon dioxide, HCN, RCN, ester and acid chloride
Applied Chemistry : 13 teaching hours.
Unit 18. Chemistry in the Service of Mankind : 4 hrs
Polymers : Addition and condensation polymers ; Elastomers and fibres ; Natural and synthetic polymers ; Some synthetic polymers (polythene, PVC, Teflon, polystyrene, nylon and bakelite ; Dyes : Introduction; Types of dyes on the basis of structure and method of application; Drugs :Characteristics of drugs; Natural and synthetic drugs ; Classification of some common drugs; Habit forming drugs and drug addiction ; Pesticides : Introduction to insecticides, herbicides and fungicides
Unit 19. Cement : 4 hrs
Introduction ; Raw materials for cement production ; Main steps in cement production (crushing and grinding, strong heating and final grinding) ; Types of cement- OPC and PPC ; Portland cement process with flow-sheet diagram ; Cement Industry in Nepal.
Unit 20. Paper and Pulp : 3 hrs
Introduction ; Raw materials ; Sources of raw materials; Stages in production of paper; Flow-sheet diagram for paper production ; Quality of paper.
Unit 21. Nuclear Chemistry and Applications of Radioactivity : 2 hrs
Natural and artificial radioactivity ; Units of radioactivity; Nuclear reactions ; Nuclear fission and fusion reactions ; Nuclear power and nuclear weapons ; Industrial uses of radioactivity ; Medical uses of radioactivity ; Radiocarbon dating ; Harmful effects of nuclear radiations .
