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…
Contents
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..