GOVERNMENT COLLEGE (AUTONOMOUS), RAJAMAHENDRAVARAM DEPARTMENT OF CHEMISTRY CBCS Syllabus for B.Sc. III Year Effective from onwards

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1 GOVERNMENT COLLEGE (AUTONOMOUS), RAJAMAHENDRAVARAM DEPARTMENT OF CHEMISTRY CBCS Syllabus for B.Sc. III Year Effective from onwards Paper VI Semester V Applied Physical Chemistry and Organic Chemistry Course Code: 106 MODULE I (Applied Physical Chemistry) 1. Chemical Kinetics: 8 Hrs. Rate of reaction, factors influencing the rate of a reaction concentration, temperature, light, catalyst. Any one experimental method to determine the rate of reaction. Definition of order and molecularity of simple reactions with two examples each. Derivation rate constants and time half change for first, second (where 2A Products i.e., when both reactants are same and two reactants are different A + B products) and zero order reactions. Two examples each for first, second and zero order reactions. Any one method to determine the order of reactions. Effect of temperature on rate of reaction, Arrhenius equation, concept of activation energy. Theories of reaction rates collision theory of bimolecular gaseous reactions. The transition state theory of bimolecular reactions (elementary treatment). Additional Input : Order and molecularity of complex reactions. 2. Thermodynamics: 16 Hrs. Some basic concepts of Thermodynamics 1. System and surroundings 2. Types of thermodynamic systems 3. Macroscopic system and macroscopic properties

2 4. State of a system and state variables 5. Extensive and intensive properties 6. Types of thermodynamic processes 7. Reversible and irreversible processes 8. Internal energy and enthalpy 9. State and path functions The first law of thermodynamics statement Heat capacities and their relationship Joule s law Joule Thomson coefficient Calculation of w, q for the expansion of perfect ideal gas under isothermal and adiabetic conditions for reversible processes. Temperature dependence of enthalpy of formation Kirchoff s equation. Second law of thermodynamics Different statements of the law. Carnot cycle and its efficiency Carnot theorem Concept of entropy entropy as a state function Entropy changes in reversible, and irreversible processes. The Gibbs (G) and Helmholtz (A) energies Variation of G with P, V and T. Gibbs Helmholtz equations one application of Gibbs Helmholtz equations. Additional Input : Different statements of First Law of Thermodynamics. 3. Photochemistry : 8 Hrs. Differences between thermal and photochemical processes. Laws of photochemistry Grothus Draper s Law and Stark Einstein s law of photochemical equivalence. Quantum Yield

3 Photochemical hydrogen chlorine, hydrogen bromine reactions. Jablonski diagram depicting various processes occurring in the excited state, qualitative description of fluorescence, phosphorescence, nonradiative processes (internal conversion, intersystem crossing). Photosensitized reactions energy transfer processes (simple example). Additional Input : Applications of fluorescence & Phosphorescence Processes. MODULE II (Applied Organic Chemistry) 1. Carbohydrates : 6 Hrs. Monosaccharides : All discussion to be confined to (+) glucose as an example of aldohexoses and (-) fructose as example of ketohexoses. Structural Elucidation of D-(+) glucose : Evidences for straight chain pentahydroxy aldehyde structure (Acetylation, reduction to n-hexane, cyanohydrins formation, reduction of Tollen s and Fehling s reagents and oxidation to gluconic and saccharic acid). Configuration of glucose based on D-glyceraldehyde as primary standard (no proof for configuration is required). Evidence for cyclic structure of glucose (some negative aldehydes tests and mutarotation). Cyclic structure of glucose. Decomposition of cyclic structure (Pyranose structure, anomeric Carbon and anomers). Proof for the ring size (methylation, hydrolysis and oxidation reactions). Different ways of writing pyranose structure (Haworth formula and chair conformational formula). Structural Elucidation of Fructose: Evidences of 2 Keto Hexose structure, formation of Penta Acetate, formation of Cyanohydrin its hydrolysis and reduction by HI. Cyclic structure of

4 Fructose (Furanose structure and Haworth formula) Osazone formation from Glucose and Fructose. Definition of Anomers with examples. Interconversion of Monosaccharides : Aldopentose to aldo hexose. Ex : Arabinose to D-Glucose, D-Mannose (Kiliani Fischer method). Epiers, Epimerisation Lobry de bruyn van Ekenstein rearrangement. Aldohexose to Aldopentose. Eg : D-glucose to D-arabinose by Ruff s degradation. Aldohexose (+) (glucose) to ketohexose (-) (Fructose) and Ketohexose (fructose) to aldohexose (Glucose). Additional Input : Disaccharide Sucrose (Elementary treatment) 2. Biomolecules : Amino acids and proteins Nucleic acids : 6 Hrs. Amino acids Introduction : Definition of Amino acids Classification of Amino acids into : 1. Alpha, beta, and gama amino acids. 2. Natural and essential amino acids definition and examples, 3. Classification of alpha amino acids into acidic, basic and neutral amino acids with two examples each. Methods of Synthesis : General methods of synthesis of alpha amino acids (specific examples Glycine, and leucine) by following methods : a) From halogenated carboxylic acid (without mechanism) b) Malonic ester synthesis (without mechanism) c) Strecker s synthesis (without mechanism) Physical Properties : Optical activity of naturally occurring amino acids : L-configuration, irrespective of sign rotation. Zwitterion structure salt like character Solubility, melting points, amphoteric character Definition of isoelectric point.

5 Chemical Properties : Two reactions of alpha aminoacids involving both amino and carboxyl groups Action of heat, action with metallic ions. (without mechanism). Peptides and Proteins : Definition and primary structures with two examples each. Nucleicacids Elementary treatment : Definition and two examples of the following : Nucleic acids Nucleosides Nucleotides Nitrogen bases Additional Input : Importance of amino acids in biological systems. 3. Material Science: 5 Hrs.