CTEVT diploma in engineering  first year (first and second semester) chemistry syllabus(course):  Complete note of diploma in engineering  is also available in this website.

First Semester : 45 teaching hours

Unit-1: Language of chemistry:  4 hrs

  1.1 Symbol:

• Definition
• Significance (qualitative and quantitative).

 1.2 Formula:

• Definition
• Significance (qualitative and quantitative)
• Concept of valency in terms of combining capacity with H₂, O₂, and Cl₂
• Variable valency (ref. Fe, Sn, Pb, Cu, Hg, S and N)
• Radicals (electro- positive and electro – negative)
• Writing a formula.

 1.3 Chemical equation:

• Definition
• Types requisites
• Significance and limitation
• Balancing of chemical equation by hit and trial method and Partial equation method.

Unit: 2: General chemistry: 8 hrs

2.1 Atom and molecule:

• Definition
• Dalton’s atomic theory and modern position of the theory.

2.2 Atomic weight:

• Definition
• Determination of atomic weight by Dulong and Petit’s method and Related numerical problems.

2.3 Molecular Weight:

• Definition
• Avogadro’s hypothesis
• Application of Avogadro’s hypotheses ( Mol. Wt=2×V.D., in the deduction of atomicity of elementary gases H₂ , Cl₂, O₂, and N₂)
• Molecular weight determination by Victor Meyer’s method and Related numerical problems.

2.4 Equivalent weight:

• Definition
• Equivalent weight of element, acid, base and salt
• Equivalent weight determination by hydrogen displacement method and oxide method.
• Numerical relation between equivalent weight, atomic weight and valency
• Some related problems of equivalent wt. (From Hydrogen displacement method and oxide method).

2.5 Simple mole concept:

• Mole of an atom
• Mole of a molecule
• Molar volume and
• Simple calculation on mole concept.

Unit – 3: System of classification: 33 hrs.

3.1 Acid, Base and Salt:

• Arrhenius concept of acid and base
• Lowry and Bronsted concept of acid and base
• Conjugate acid and base
• Amphoteric nature of water
• Lewis concept of acid and base
• Properties of acid and base.
• Definition of Salt
• Types of salt (normal, acidic and basic)
• Concept of hydrogen ion concentration, pH value and pH Scale
• Buffer solution.

3.2 Volumetric analysis:

• Definition of titration (acidimetry and alkalimetry),
• Indicator
• End-point (neutralization point)
• Standard solution (primary and secondary standard solution), Normal, Decinormal, Molar, Molal solution
• Requisites of primary standard substance
• Volumetric equation,
• Express the strength of solution Normality, Molarity, Molality, gram per litre and percentage and related numerical problems.

3.3 Periodic table:

• Mendeleev’s periodic law
• Mendeleev’s periodic table
• Characteristics of groups and periods in the table
• Advantages and anomalies of the periodic table
• Modern periodic law.

3.4 Electronic theory valency:

• Assumptions
• Types
• Electrovalency eg. NaCl, MgO, CaS
• Covalency eg. H₂, O₂, N₂, CH₄, H₂O, NH₃, C₂H₂
• Coordinate co-valency eg.H₂O₂, SO₂, O₃, SO₃)
• Electronic dot structure of some compounds eg.H₂SO₄, CaCO₃, K₂SO₃

3.5 Electrolysis:

• Definition of electrolyte, non-electrolyte and electrolysis
• Faraday laws of electrolysis,
• Application of electrolysis (electroplating and electro refining)
• Electrolysis of acidulated water.

3.6 Oxidation and reduction:

• Classical definition
• Electronic interpretation
• Oxidizing agent: Definition and eg O₂, O₃, oxyacids, halogens, K₂Cr₂O₇, KMnO₄
• Reducing agent: Definition and eg. H₂, H₂S with some examples,
• auto-oxidation eg.H₂O₂, HNO₂, SO₂
• Idea of oxidation number
• Balancing chemical equation by oxidation number method.

3.7 Atomic structure :

• Subatomic particles (electron, proton and neutron)
• Classical α – rays scattering experiment
• Rutherford’s atomic model and its drawbacks
• Bohr’s atomic model (postulates only)
• Composition of nucleus
• Mass number and atomic number
• Isotopes and isobar
• Arrangement of electron (Bohr – Bury Scheme)
• Concept of shell and sub shell,
• Electronic Configuration and atomic structure of Some elements (Atomic no. 1 to 30)
• Hund’s rule
• General idea of quantum number and Pauli’s exclusion principle.

3.8 Corrosion:

• Definition
• Types
• Direct and indirect method and prevention against corrosion.

3.9 Activity and electrochemical series:

• Definition
• Action of water, acid and oxygen on metals.

Second Semester : 45 teaching hours

Unit- 1: Non-metals and their compounds: 20 hrs.

 1. Water:

• Source of water
• Hard and soft water
• Removal of temporary and permanent hardness of water
• Water treatment of domestic and industrial purpose

 2. Ammonia:

• Lab preparation
• Manufacture by Haber’s process
• Properties and uses

 3. Nitric acid:

• Manufacture by Ostwald’s process
• Properties and uses.
• Nitrogen cycle
• Fixation of Nitrogen
• Chemical fertilizers
• Oxides of nitrogen as pollutant (general concept)
• Acid rain (due to oxides of nitrogen and oxide of Sulphur “Sulphur dioxide”)

 4. Halogens (Chlorine): Lab preparation, Properties and uses.

 5. Hydrochloric acid: Lab preparation, Properties and uses.

 6. Hydrogen Sulphide: Lab preparation, Properties and uses.

 7. Sulphuric acid: Manufacture by contact process, Properties and uses.

 8. Carbon and its compounds:

• Allotropes of carbon (reference of diamond & graphite & their structure).
• Oxides of carbon (Ref. carbon dioxide & carbon mono oxide as pollutants)- general idea only.

Unit: 2: Metals and their compounds: 15 hrs.

2.1 General study of metals and their components:

• Difference between metal and non metal
• Combined & free state of metals
• Chemistry of Metallic Carbonates, Sulphates, Chlorides and Nitrates.

2.2 Alkali metals:

• General characteristics of Alkali metals
• Properties & uses of sodium.

2.3 Alkaline earth metals:

• General characteristics of the Alkaline earth metals
• Properties & uses of calcium.

 2.4 Aluminum: Properties and uses

2.5 Coinage metals:

• General properties of coinage metals
• Properties and uses of cupper

2.6 Zinc: Properties & uses

2.7 Iron: Properties & uses

2.8 Lead: Properties & uses

2.9 Alloys:

• Definition
• Purpose of making alloys
• Types of alloys

Unit: 3: Organic compounds and synthetic materials: 10hrs

3.1. Organic compounds

• Historical background, classification, and nomenclature
• Functional groups and homologous series
• Saturated hydrocarbon: Properties of Methane
• Unsaturated hydrocarbon: Properties of Ethylene and Acetylene
• Aromatic compounds: Definition , Comparison of aliphatic and aromatic compounds
• Properties of Benzene.

3.2. Synthetic materials:

• Polymer and polymerization – Definition , Types of polymer
• Rubber: Types (Natural and Synthetic ) ,Preparation and uses.
• Polyvinyl chloride (PVC): Preparation and uses
• Polythene: Preparation and uses.

REFERENCE :

http://www.ctevt.org.np/

The post CTEVT diploma in Engineering chemistry syllabus(course) : appeared first on Online Chemistry notes.

CTEVT first year Chemistry syllabus for Certificate/Diploma Level in Health Sciences : General Medicine(HA), Medical Laboratory Technology(MLT), Diagnostic Radiography, Homeopathy, Ayurveda, Amchi Science, Dental Science, Ophthalmic Science, Pharmacy, Physiotherapy and Acupuncture, Acupressure & Moxibustion.

⇐ See complete note of CTEVT chemistry…

SYLLABUS :

Total teaching hours :   240 hrs

Theory       :                    160 hrs

Practical    :                    80 hrs

PHYSICAL CHEMISTRY : 67 teaching hours.

Unit 1: Elements, compounds and chemical change : 3 hours

• Symbols for the atom,molecule, and compound ,radical and variable valency.
• Writing a chemical formula, molecular formula and empirical formulae.
• Significance of symbol and formula .
• Chemical compound and its differences from mechanical mixture.
• Pure and impure substances.
• The processes of separating the constituents of a mixture:

Unit 2 : Chemical equations: 3 hrs.

• Chemical formula, Chemical equation, reactant and product.
• Significance and limitations of chemical equations.
• Types of chemical reactions (seven-types) with examples.
• Balancing a chemical equation by: hit and trial method and partial equation method.

Unit 3 : Periodic table : 5 hrs.

• Historical development of periodic table.
• Periodic classification of elements.
• Location of s, p, d and f-block elements.
• Mendeleev’s periodic table, success and defects of Mendeleev’s periodic table
• Periodicity in properties by: Atomic radii, Electronegativity , Ionisational potential , Electron affinity.

Unit 4 : States of matter : Gaseous state : 5 hrs.

• Differences between solids, liquids and gases.
• Kinetic theory of gases.
• Effect of pressure and temperature on volume of gas.
• Simple derivation of ideal gas equation (PV=nRT)
• Dalton’s law of partial pressure.
• Graham’s law of diffusion.
• Law of stoichiometry, Avogardo’s hypothesis .
• Simple chemical calculations.

Unit 5 : States of matter : Liquid State: 4 hrs.

• Solution and its types (Unsaturated, saturated and supersaturated solution).
• Solubility and related numerical problems.
• Viscosity and surface tension.
• Raoult’s law
• Colligative properties of solution.

Unit 6 : States of matter : Solid State : 1 hr.

• Classification of solids.
• The difference between amorphous and crystalline solids.
• Molecular crystal, Covalent crystal, Ionic crystal, Water of crystallization.

Unit 7 : Atomic structure : 5 hrs.

• Fundamental particles of atoms.
• Bohr’s postulates of atomic model, Bohr’s explanation of hydrogen spectrum.
• Rutherford’s nuclear model of atom.
• Afbau’s principle, Hund’s rule.
• Atomic number, mass number, atomic weight and gram atomic weight, Isotopes and isobars.

Unit 8 : Electronic theory of valency: 3 hrs.

• Electronic theory of valency
• Types of chemical bond : Electrovalent , Covalent , Co-ordinate covalent
• Factors affecting the formation of ionic and covalent bond; Hydrogen bond.

Unit 9 : Oxidation and Reduction : 5 hrs.

• Classical concept of oxidation and reduction.
• Electronic concept of oxidation and reduction.
• Oxidant and reductant and oxidation number
• Examples of redox reaction.
• Balancing the chemical equation by oxidation number method and ion electron method.

Unit 10 : Electrochemistry : 5 hrs.

• Electrolytes, Non-electrolytes, strong and weak electrolytes.
• Arrhenius theory of ionization.
• Faradays’ laws of electrolysis.
• Electrolysis of water, Ionic product of water,PH, POH, Buffer solution
• Importance of PH and buffer in human body.
• Simple numerical problems.

Unit 11 : Acid, base and salt : 2 hrs.

• Characteristics of acids, bases and salts.
• Arrhenious and Bronsted-Lowry concept of acids and bases.
• Salts and their types.
• Antacids and antabases and their medical uses.

Unit 12 : Solution- True solution : 2 hrs.

• Types of solution, Solubility, Solubility product, Solubility curve, Henry’s law.
• Osmosis, osmotic pressure, isotonic, hypotonic and hypertonic solution.
• Biological importance of osmosis.

Unit 13 : Solution – Colloids : 3 hrs.

• Comparison between true solution, colloidal solution and suspension.
• Difference between lyophilic and lyophobic solutions.
• Coagulation of solutions by – boiling, electrophoresis, addition of electrolyte.
• Dialysis, and associated colloids.
• Application of colloids in the medical field and in everyday life.
• Precipitation of smoke, kidney dialysis machines.
• Emulsions, gels and gelation.

Unit 14 : Mole concept and chemical arithmetic : 4 hrs.

• Mole concept, Mole in the term of mass, volume and ion.
• Relationships based upon chemical equation-

        Mass – Mass relationship

        Mass – volume relationship

        Volume – volume relationship

• Limiting reagent.
• Calculation of related numerical problems.

Unit 15 : Volumetric analysis : 5 hrs.

• Types of chemical analysis.
• Equivalent and gram equivalent weight of Element, acid, base, and salt; Determination of equivalent weight by hydrogen displacement method.
• Titration, acidimetry, alkalimetry, end point, indicator, primary and secondary standard substance
• Ways of expressing concentration of solution in terms of – Normality, Molarity, molality ,%by mass, % by volume, parts per million (PPm), Normality factor.
• pH change in acid base titration and choice of indicator.
• Calculations to prepare different concentrations of solution.

Unit 16 : Chemical kinetics : 7 hrs.

• Molecularity of reaction, Difference between order of reaction and molecularity of reaction.
• Reversible and irreversible reaction.
• Variation of reactant, product and rate o freaction with progress of reaction (graphicalre presentation).
• Law of mass action.
• Le-Chateliers’ principle and its application
• Activation energy and activated complex.
• Zero, first and second order reactions
• Catalysis: Enzyme catalysis, characteristics of enzyme catalysis, promoter, autocatalysis, negative catalysis, catalytic poisoning.

Unit 17 : Thermochemistry : 5 hrs.

• Introduction
• Enthalpy and enthalpy change, exothermic and endothermic reactions, heat of combustion and its application, heat of formation, heat of neutralization and heat of solution, bond energy.
• First law of thermodynamics
• Hess’s law.

ORGANIC CHEMISTRY : 52 teaching hours.

Unit 1 : An introduction of organic chemistry: 2 hrs.

• Introduction
• Organic chemistry as a separate branch, Reason for large number of organic compounds.
• Difference between organic and inorganic compounds.
• Sources of organic compound
• Importance of organic chemistry in medical field
• Structure and uses of simple drugs- Antipyretics, antiseptics, analgesics, antibiotic, antimalarials, tranquilizers, germicides and fungicides.

Unit 2 : Nomenclature of organic compounds : 4 hrs.

• Functional group and Homologous series.
• IUPAC rule, IUPAC system of aliphatic compounds.
• Nomenclature of compounds containing functional and poly-functional groups.

Unit 3 : Isomerism : 2 hrs.

• Definition of isomerism.
• Structural isomerism of the types possitional, functional, chain ,metamerism and tautomerism with example.

Unit 4 : Organic reaction: 4 hrs.

• Carbocation and carbanion.
• Inductive effect (+I and –I effect), Significance of inductive effect
• Homolytic and Heterolytic bond fission
• Electrophiles and Nucleophiles.
• Resonance, VSEPR theory
• The types of organic reactions – Electrophilic and nucleophilic substitution, addition, elimination; Types of hybridization (sp, sp² and sp³)

Unit 5 : Hydrocarbons : 6 hrs.

Alkene :

• Introduction
• Laboratory preparation of ethene from ethanol.
• Physical and chemical properties and uses of alkenes.
• Markovnikov’s rule and anti-Markovnikov’s rule.

Alkyne :

• Introduction
• Laboratory preparation of ethyne from calcium carbide.
• Chemical properties–Combustion, hydrogenation,catalytic hydration, with Br₂ solution,with Na, polymerization
• Uses of ethyne.

Unit 6 : Alkyl halides : 3 hrs.

• Laboratorypreparation of chloroform.
• Physical and chemical properties and uses of chloroform.

Unit 7 : Alcohol : 4 hrs.

• Introduction
• Classification of alcohol as-monohydric, dihydric, polyhydric, primary, secondary and tertiary.
• Identification of primary, secondary and tertiary alcohol by oxidation method.
• Preparation of ethyl alcohol from molasses by fermentation.
• Physical and chemical properties of ethanol (oxidation with sodium, bleaching powder, oxygen, sulphuric acid, CH₃COOH, phosphorus halide).

Unit 8 : Carbonyl compounds : 5 hrs.

• General methods of preparation of aldehydes and ketone.
• Physical and chemical properties (NH₂OH, NH₂CONH₂, C₆H₅NHNH₂, NH₂NH₂, NaHSO₃; 2,4-DNP, Formaline, Oxidation of ammonia)
• Uses.

Unit 9 : Carboxylic acid : 2 hrs.

• Preparation of carboxylic acid from alcohol, aldehyde and alkyl benzene.
• Physical and Chemical properties (acidic character, NaHSOCl₂, NH₃,C₂H₅OH, P₂O₅)
• Uses.

Unit 10 : Ether : 2 hrs.

• Laboratory preparation from ethanol.
• Physical properties.
• Chemical properties – Combustion, hydrolysis, reaction with excess HI and PCl₅.
• Uses in medicine.

Unit 11 : Aromatic compounds:

Introduction : 4 hrs.

• Introduction
• Aromatic compound.
• Explain benzene nucleus and side chain.
• Characteristics of aromatic compound.
• Preparation of benzene, physical and chemical properties (halogenation, nitration, sulfonation, Freidel Craft’s reaction)
• Uses.

Nitrobenzene : 2 hrs.

• Introduction
• Laboratory preparation of nitrobenzene.
• Physical properties
• Reduction reaction of Nitrobenzene in different medium.
• Uses in everyday life.

Aniline : 3 hrs.

• Introduction
• Laboratory preparation of pure aniline
• Physical and Chemical properties- basic nature, alkylation, acylation, sulfonation, halogenation, nitration
• Uses.

Phenol : 2hrs.

• Introduction
• Preparation of phenol.
• Physical and Chemical properties (action with zinc dust, NaOH, NH₃, PCl₅, Kolbe’s reaction, Condensation with formaldehyde).

Benzoic acid : 2 hrs.

• Laboratory preparation of benzoic acid
• Physical and Chemical properties (action with alcohol, PCl₅, NH₃ and soda-lime)
• Uses.

Unit 12: Molecules of life : 5 hrs.

Carbohydrate:

• Definition and classification,
• Structure (Linear, Cyclic) of glucose,
• Functions of Carbohydrates

Protein:

• Amino acid and Peptide bond
• Essential and non-essential amino acid
• Denaturation of protein
• Functions of Protein
• Enzymes (Definition and importance).

Lipid:

• Introduction of lipid, fat and oil and their natural sources.
• Hydrolysis
• Functions of fat and oil .

Vitamins and coenzymes:

• Introduction
• Fat soluble and insoluble vitamins
• Importance and functions.

Environmental Chemistry ( Pollution) :  5 hrs.

• The sources and adverse effects due to the following air pollutants- CO₂, SO₂, O₃, H₂S, CO, hydrocarbon,lead, cadmium dust, CFC, oxides of nitrogen.
• Air pollution and its effects on : human health, materials and climate, Green house effect, Ozone layer depletion
• Acid rain and its adverse effects.
• Water pollution and its effects.
• Nuclear and pesticide pollution.

INORGANIC CHEMISTRT : 36 teaching hours.

Unit 1 : Hydrogen : 3 hrs.

• Laboratory preparation of Hydrogen
• Physical properties.
• Preparation of Vanaspati  
• Nascent hydrogen and molecular hydrogen
• Reaction of nascent hydrogen with KMnO₄, FeCl₃, K₂Cr₂O₇;
• Ortho and Para hydrogen, Isotopes
• Uses of hydrogen.

Unit 2 : Water : 7 hrs.

• Introduction of soft and hard water.
• The process of removal of hardness -Boiling, Clark’s process, using washing soda, permutit process, soda – ash method, deionisation of water.
• The advantage and disadvantage of hard water.
• The meaning of drinking water.
• Method of purification of drinking water by-  boiling, candle filtration, chemical disinfection, bleaching powder,Cl₂ solution,iodine,KMnO₄, ozonisation, using potash alum.
• The solvent property of water.
• Difference between soft and hard water.

Unit 3 : Carbon and its oxides : 2 hrs.

• Introduction
• Allotropes of carbon
• Laboratory preparation of carbon monoxide
• Physical properties of CO.
• Chemical properties  : reaction with – O₂, Cl₂, Ni, NaOH and haemoglobin.

Unit 4 : Ammonia : 3 hrs.

• Laboratory preparation of ammonia.
• Physical and chemical properties of ammonia (action with metals, Nessler’s reagent, ammonia as a Lewis base, basic nature)
• Uses of ammonia.

Unit 5 : Phosphorus : 2hrs.

• Introduction
• Occurrence of phosphorous in animal bones, ATP and ADP.
• Properties of white phosphorous –reactions  with O₂, with Cl₂,with caustic alkali.
• Uses of phosphorous.

Unit 6 : Sulphur : 5 hrs.

• Laboratory preparation of SO₂
• Chemical properties of SO₂ (action with lime water, sodium carbonate, oxidizing and reducing properties, bleaching properties)
• Laboratory preparation of H₂
• Reducing properties of H₂

Unit 7 : Halogens : 5 hrs.

• Laboratory preparation of Cl₂, Br₂ and I₂
• Physical properties of Chlorine, bromine and iodine.
• Compare the chemical properties of halogens
• Oxidizing action, bleaching action,  reaction with H₂, with slaked lime, and with organic compounds.
• Uses of Cl₂

Unit 8 : Metallic compounds : 7 hrs.

• Difference between minerals and ores, flux and slag, calcination and roasting.
• Preparation, properties and uses of HgCl₂, Hg₂Cl₂, Plaster of Paris, Epsom salt, Bleaching powder, Cu₂O, AgNO₃, AuCl₃, ZnCl₂.2H₂O
• Biological importance of Na and K.

Unit 9 : Minerals : 2hrs.

• Sources of the following minerals- Na, K, Ca, Mg, Fe, Zn, Ni, Cobalt.
• Biological importance and effects due to their deficiency.

⇐ See complete note of CTEVT diploma level chemistry..

REFERENCE :

• http://ctevt.org.np/files/curriculum/Diploma/1%20st%20Year%20curriculum%20of%20Health%20science%20all.pdf

The post CTEVT Chemistry syllabus(curriculum) for Certificate/Diploma Level in Health Sciences appeared first on Online Chemistry notes.

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 .

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