CTEVT Chemistry syllabus(curriculum) for Certificate/Diploma Level in Health Sciences

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.

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⇐ See complete note of CTEVT chemistry…

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SYLLABUS :

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Total teaching hours :   240 hrs

Theory       :                    160 hrs

Practical    :                    80 hrs

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PHYSICAL CHEMISTRY : 67 teaching hours.

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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.

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ORGANIC CHEMISTRY : 52 teaching hours.

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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.

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Environmental Chemistry ( Pollution) :  5 hrs.

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• 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.

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INORGANIC CHEMISTRT : 36 teaching hours.

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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.

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⇐ See complete note of CTEVT diploma level chemistry..

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REFERENCE :

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