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Curriculum | B.Sc (Non- Medical) | Paper VI (Theory) Physical Chemistry code 09010608

Paper VI (Theory) Physical Chemistry  code 09010608

S.No. Topic Learning objectives Teaching Guidlines  Methodology Time (Hrs)
1 Electronic Spectrum:

1. Concept of potential energy curves for bonding and anti bonding molecular orbitals,

2. Qualitative description of selection rules and Franck-Condon principle.

3. Qualitative description of sigma and pie and n molecular orbital(MO)their energy level and respective transitions

Students will be able to

1. Understand that electronic spectra consist of various vibrational and rotational levels and to draw the potential energy curves

2. Understand the various selection rules and possibility of electronic transitions

To describe that potential energy curves consist of vibrational and rotational levels, complex nature of electronic spectra, selection rules along with the concepts multiplicity, gerade and ungerade orbitals, term symbols, types of molecular orbitals involved in electronic transitions (σ,  and n orbitals) ,1. Lecture

2. Seminar

3.Discussion with students

4. Assignment

5.discussion on assignment

6.Evaluation of assignment

 

 

 

4

2. Photochemistry:

1. Interaction of radiation with matter, difference between thermal and photochemical processes.

2. Laws of photochemistry: Grotthus-Drapperlaw, Stark- Einstein  law(law of photochemical equivalence)

4. Jablonski diagram depiciting various processes occurring in the excited state, qualitative description of fluorescence, phosphorescence, non-radiative processes (internal conversion, intersystem crossing), quantum yield,

5. Photosensitized reactions-energy transfer processes (simpleexamples), photoinhibitors, Photochemical equilibrium or Photostationary state

Students will be able to

1. Understand the importance of photochemistry and laws of photochemistry

2. Understand and Jablonski diagram

To describe the various photochemical and photophysical processes with suitable examples, laws of photochemistry, explain fluorescence, phosphorescence, internal conversion and intersystem crossing using Jablonski diagram, Quantum yield, photosensitizers and photoinhibitos using suitable examples. 1. Lecture

2. Seminar

3.Discussion with students

4. Assignment

5.discussion on assignment

6.Evaluation of assignment

 

 

 

 

 

8

3. Solutions:

Dilute Solutions and Colligative Properties

1. Ideal and non-ideal solutions, methods of expressing concentrations of solutions, activity and activity coefficient.

2. Dilute solution, Colligative properties,

3. Raolut’s law, relative lowering of vapour pressure, molelcular weight determination,

4. Osmosis law of osmotic pressure and its measurement, determination of molecular weight from osmotic pressure.

5. Elevation of boiling point and depression of freezingpoint

6. Thermodynamic derivation of relation between molecular weight and elevation in boiling point and depression  in freezing point.

7. Experimental methods for determining various colligative properties. Abnormal molar mass, degree of dissociation and association of solutes.

Students will be able to

1. Understand the difference between ideal and non-ideal solutions

2. Understand and derive colligative properties of solutions

 

To explain the difference between ideal and non-ideal solutions, colligative properties of solutions, Raolut’s law, relative lowering of vapour pressure, molelcular weight determination and their thermodynamic derivations.

 

1. Lecture

2. Seminar

3.Discussion with students

4. Assignment

5.discussion on assignment

6.Evaluation of assignment

 

 

 

 

10

4.

 

Phase Equillibrium:

1. Statement and meaning of the terms–phase, component and degree of freedom,

2. Thermodynamic derivation of Gibbs phase rule, phase equilibria of one component system –Example–water and Sulpher systems.

3. Phase equilibria of two component systems solid- liquid equilibria, simple eutectic

Example Pb-Ag system, desilverisation of lead

Students will be able to understand and explain the phase rule and phase diagrams of one and two component system To describe the phase, component and degree of freedom using various examples of the systems like, water, ice and vapour system, gases etc., derive Gibbs phase rule, Pahse equilibria of water sulphur, Pb-Ag system, desilverisation of lead. 1. Lecture

2. Seminar

3.Discussion with students

4. Assignment

5.discussion on assignment

6. Evaluation of assignment

 

 

 

8

Admission 2017