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

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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.

CTEVT diploma level chemistry syllabus and complete note

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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.

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