Chemistry BSc Syllabus Sargodha University


 (Outlines of Courses for Session 2005-2006 and on wards)

Paper “A”            Physical Chemistry (Written)         50 Marks

Paper “B”            Inorganic Chemistry (Written)      50 Marks

Paper “C”            Organic Chemistry   (Written)       50 Marks

Practical:    (For three Days , Four Hours Duration each day as detailed below):

Paper “A”            Physical Chemistry (Practical)      16 Marks

Paper “B”            Inorganic Chemistry (Practical)    17 Marks

Paper “C”            Organic Chemistry (Practical)       17 Marks

Total Marks: 200


PAPER A:  PHYSICAL CHEMISTRY (Written)     50 marks

 Note. All units should be expressed in SI System



Ideal gas laws and general gas equation , Kinetic molecular theory of gases, Kinetic equation for ideal gases and deduction of gas laws, molecular velocities (Averages, root mean square and  most probable ), distribution of molecular velocities and experimental verification, molecular collisions, mean free path, collision frequency, heat capacity of gases ( Cp,Cv).

Thermal Energy:

Translational, rotational and vibrational contributions. Principle of equipartition of energy, Van der Waals  equation and its validity. Critical phenomenon and determination of constants. Van der experimental determination of critical temperature. Law of Waals corresponding states. Liquefaction of gases.


Structural differences between gases and liquids, Vapour pressure, surface tension, viscosity, refractive index, optical activity and dipole moment (their measurements and relation to chemical constitution).


Crystal lattice and unit cell, law of crystallography, crystal system. X-rays diffraction and the Bragg’s equation . Experimental methods for X ray structure determination. Closed – packed sphere structures, structure of ionic solids, Elementary treatment of metals, insulators and semi- conductors.


Classification, preparation, purification and properties of colloidal solutions, Brief ­­­treatment of Gels, Emulsions, Aerosols and Surface – active agents.


Raoult’s law, Henry’s law, activity and activity coefficients, Deviations of solutions from ideal behaviour . Colligative properties, lowering of vapour pressure, Boiling point elevation, Depression in freezing point and osmotic pressure (Their measurements and thermodynamic derivation of molecular masses). Abnormal colligative properties of solutions.


 Earlier developments, Nature of light radiations, Bohr’s theory of atomic structure. Interpretation of emission spectra of hydrogen atoms. Quantum mechanics, de Broglie equation and Eigen values. Interpretatin of (H-E). Eigen function and Eigen values. Heisenberg’s uncertainty principle. Particles in one dimensional box (permitted energies and values).

Quantum number of atomic orbitals, Pauli’s Exclusion Principle. Distributionof electons in atomic orbials.

Chemical Bonding (Elementary treatment of Lewis, Valence bond and Molecular orbital theories).


Thermodynamics terms and types of system. State and state function. Equilibrium states, nature of heat and work, Sign convention and units of work and q. Internal energy change, first law of the rmodynamics, enthalpy . Heat capacity  Cp – Cv – R.

Thermo-chemistry. Heat of reaction. Hess’s law. Heat of formation Standard enthalpy of combustion and its applications. Heat of neutralization. Heat of solution. Bond energies. Measurement of heat of reaction . Effect of temperature on heat of reaction (Kirchhoff’s equation ).

Types of thermodynamics processes. Reversibility and irreversibility. Isothermal reversible expansion of an ideal gas. Adiabatic process for an ideal gas. Spontaneous and non-spontaneous processes, Second law of thermdynamics. The Carnot’s cycle. Efficiency of an engine. Thermodynamics temperature scale Entropy and its calculations for phase transition, reversible and irreversible isothermal expansion. Temperature dependence entropy. Entropy and probability, Helmholtz and Gibb’s Free Energies. Standard free energy, G-RT In K. Van’t Hoffisochore, (intergrated form)Clausius – Claperyron equation.


Basic concepts, law of mass action, Relationship between Kc , Kp, Kx and Kn for gasseous reactions. Homogeneous gaseous equilibria. Effects of pressure, concentration on equilibrium changes. Examples of chemical equilibria. Degree of dissociation.

Le Chatelier’s Principle and its applications to homogeneous and heterogeneous equilibria, thermodynamic equations. Effect of temperature on chemical equilibrium.


Phases, components, degrees of freedem. Gibb’s phase rule and its derivation. Phase diagram, One component system, (Water and sulphur system). Two component systems, eutectic systems, cooling curves and cooling behaviour, silver-lead system, Compound formation with congruent m.p. Ferric chloride- water system, sodium sulphate- water system.

Solid solution and alloy systems, liquid-vapour systems. Three component systems. Partially miscible a three component systems. Liquid-liquid systems, Nernst’s distribution law, applications and deviations.


The reaction rate (average and instantaneous). Rate equation, velocity constant. Rate law expression, order and molecularity. Kinetic expressions for zero order, first order, pseudo-unimolecular and second order (with same 8 different initial conc.) with examples. Determination of order and rate const of a reaction. Effect of temperature. Activation energy and its determination.

Biomolecular collison theory of reaction rates (causes of its failure). Collision theory of unimolecular reactions (Lindemann’s mechanism). Some examples of m/re-action mechanisms.


Electrolytic conduction (definitions and measurements, specific, equivalent and molar conductances). Conductance of strong and weak electrolytes, Kohlrausch’s law and its applications. Ostwald’s dilution law. Transport number, Hittorf’s rule. Determination of transference numbers. Applications of conductance measurements.

Electromotive force and its measurements. Electrochemical cells; reversible and irreversible, classification of half cells. Electrode potential and its measurements (standard electrodes). Cell notations. Thermodynamic aspects of cell reactions. Liquid Junction potential. Types of Galvanic cells, concentration cells without and with transference


 Types of nuclear radiations, detection and measurement of radioactivity, stable and unstable isotopes. Half life, natural radioactivity. Artificial nuclear transformations. Applications of radioactive isotopes. Nuclear fission and fusion reactions. Brief description of nuclear reactor.


 1.  Surface Tension Measurements:

Determination of surface tension of different liquids. Parachor values. Composition of mixtures of two miscible liquids.

2.  Viscosity Measurements:

Determination of viscosity coefficients of different liquids. Rheochor values and composition of mixture of two miscible liquids.

 3. Refractometry:

Determination of specific and molar refractivities of different liquids, composition of two miscible liquids.

 4.  Thermochemical Measurements:

(i) Heat of neutralization of acids and bases.

(ii) Heat of solution of different salts.

5.  Molecular Mass:

Determination by ebullioscopic method.

6.  Chemical Kinetics:

Determination of reaction rate constant for a first order reaction (acid hydrolysis).

Conductance Measurement:

  • (i) Determination of cell constant and molar conductance.
  • (ii) Verification of Ostwald’s dilution law. Determination of degree of dissociation for weak electrolytes.


  1. Text Book of Physical Chemistry for B.Sc students by Ali Mohammad and Ghulam Rasool Chaudhry, Ameen Publishers, Urdu Bazar, Lahore.
  2. Text Book of Physical Chemistry for B.Sc students by G. Nabi, Publishers; Ilmi Kitab Khana, Urdu Bazar, Lahore.


  1.  Chaudhry, G. R., ;Text Book of Physical Chemistry, New Kitab Markaz, Aminpur Bazar, Faisalabad, Pakistan, 2nd Edition (2001)
  2. Maron S. H. & B. Jerome, “Fundamentals of Physical Chemistry”, Macruthan Publishing co. Inc. New York. (Also published by National Book Foundation).
  3. Atkins P.W. & M. J. Clugston, “Principles of Physical Chemistry” Pitman Publishing Company.(1998)
  4. Moore W. J., “Physical Chemistry”, 5th Ed. Longmans Publishers.
  5. Jones M., “Elements of Physical Chemistry”, Addison-Sesky Publishing Company.
  6. Adamson A. W.,”Understanding Physical Chemistry” 3rd Ed. Benjamin Cummings Publishing Company Inc.
  7. Heald C. & A.C.K. Smith, Applied Physical Chemistry English Language Book Society and MacMillan.
  8. Akhtar M.N. & Ghulam Nabi ,”Text Book of Physical Chemistry”
  9. Bhatti H. N. and K. Hussain, “Principles of Physical Chemistry”; Carwan Book House, Lahore.
  10. Levitt B.P., “Findlay’s Practical Physical Chemistry”, 9th Ed., Longman Group Limited.
  11. Das R.C. and B. Behera, “Experimental Physical Chemistry”, Tata McGraw Hill Publishing Company Limited.
  12. Crocleford H.D., H.W. Biard, F.W. Getzen & J.W. Nowell, “Laboratory Manual of Physical Chemistry”, 2nd Ed., John Wiley & Sons London.



 Atomic Structure and periodic Table:

 Electromagnetic radiations, Atomic spectra, the wave nature of electron, electron spin and the Pauli’s exclusion Principle, the special distribution of electrons, the electronic configuration of elements. The variation of properties with atomic structure, atomic size, ionization energy, electron affinities and electronegativities. Modern trends in periodic table based upon chemical re-activities of elements.

Metals as reducing agents and non-metals as oxidizing agents. Redox actions, redox potential (elementary treatment). Electrochemical series and its applications.

Chemical Bonding:

Nature and types of chemical bond, energetic of chemical bond, bond energies, bond length, polarity of molecules, dipolemoment. Theories of chemical bonding Valence bond theory. Interpretation of pictorial pictures of molecules based on hybridization and resonance. Interpretation of shapes of molecules based on valence shell electron pair repulsion (VSEPR) treatment. Molecular orbital theory as applied to homonuclear and heterounclear diatomic molecules. Hydrogen and metallic bonding.

Acid- Base Equilibria in Aqueous Solutions:

General concepts of acids and bases including soft and hard acid-base concepts. Relative strength of acids and bases, significance of PK, ionization of water and pH concept. Buffers. Relationship between acid-base equilibria and redox processes.

Ionic Reaction in six Solution:

 Hydrolysis of salts, applications of law of mass action and the principle of solubility product and common ion effect in inorganic qualitative analysis.

Chemistry of p-block Elements:

General characteristics of the following groups of p-block elements with reference to the aspects given against each.

a. Boron and Aluminum:

Gradation of the characteristic properties within group III. Metallurgy of aluminium and its chemical characteristics. Electron deficient molecules such as boranes aluminium hydrides and halides, including their structure onding. Boric acid, borax and alums.

b. Carbon and Silicon:

Gradation of the characteristic properties within group IV. Green-house effect. Production of pure silicon chips for solar energy cells, silicones. Structural aspects of metasilicates / ortho and meta silicates. Industrial applications of Zeolites. Cement and Glass Industry. Water glass.

c. Nitrogen and Phosphorus:

Gradation of the characteristics properties within group V. Oxides and oxyacids of nitrogen and their role in environmental pollution. Nitrogen and phosphorus based fertilizers.

d. Oxygen and Sulphur:

Gradation of the characteristics properties within group VI. Oxides and Oxyacids of sulphur. Role of sulphur dioxide in air pollution. Thionic acids. Use of “hypo” in photography.

e. Halogens:

Gradation of the characteristic properties within group VII. Oxyacids of chlorine. Structural and chemical aspects of interhalogons and pseudohalogens.

f. Zero Group Elements:

Basis of reactivity of noble gases. Nature of bonding and structure of xenon compounds (fluorides, oxides and oxyflourides), laboratory and commercial utilization of noble gases.

6. Transition Elements (d-block elements):

General characteristics of d-block elements, Electronic configuration, coordinate bond formation, Development of coordination compounds, nomenclature. Applications of valence bond, crystal field theories to explain the structures of coordination compounds. Colour and magnetic behaviour of coordination compounds.

7. Modern Materials:

Introduction to liquid crystals, inorganic polymers, engineering ceramics, fiber glass, thin films and semiconductors.

Paper ‘B’   B.Sc. Inorganic Chemistry (Practical) Marks  17

1.  Qualitative Analysis:

i. Mixture of four radicals (cations and anions) from standard samples as well as from water, soil and simple ores by semi-micro techniques/macro-techniques.

ii. Spot tests for the following cations:

Ni  (II), Ag  (i)  Hg (II)   Cd  (II)

2.  Separation of cations:-

Ni  (II),  Co  (II), Mn  (II),  Cu (II), by paper chromatography

3.  Quantitative Analysis:-

(Calculations should be based on morality). Multistage exercises based on iodometry, iodometry, complexometry and redox reactions, e.g.,

  • Preparation of Ferrous Sulphate from Kipp’s Waste and determining the percentage purity of the sample by estimating Fe (II) with K2 Cr2 O7.
  • Preparations of CuZo4, from copper turnings and determining parity of the sample by Iodometry and Iodimetry.
  • Determinations of hardness of water using EDTA and other relevant exercises

4.  Gravimetric Analysis:-

Estimations of Ba +2  and Pb +2  ions as BaSO4 and as PbCrO4


  • Text Books of Inorganic Chemistry (for B.Sc students) by Muhammad Zafar Iqbal, Illmi Kitab Khana, Lahore.


  1.  Iqbal, M. Z., ‘Text Book of Inorganic Chemistry’, Ilmi Kitab Khana, Revised Edition (1998).
  2. Chaudhry, G. R., ;Text Book of Inorganic Chemistry, New Kitab Markaz, Aminpur Bazar, Faisalabad, Pakistan, 2nd Edition (2001)
  3. Bhatti, H. N. and B.A. Nasir, Modern Inorganic Chemistry, The Carvan Book House, Lahore, Pakistan, 1st Edition (2000)
  4. Cotton, F. Albert, Geoffrey Wilkinson and Paul L. Gaus, ‘Basic Inorganic Chemistry’, John Wiley & Sons, Inc. 3rd Edition (1995).
  5. Lee, J.D., ‘Concise Inorganic Chemistry’, Chapman & Hall, 5th Edition, (1996).
  6. Jolly, William. L., ‘Modern Inorganic Chemistry’, McGraw Hill, 2nd Edition (1991).
  7. Shriver, D.F., P.W. Atkins and C.H. Langford, ‘Inorganic Chemistry’, Oxford, 2nd Edition (1994).
  8. Sharpe, A.G., ‘Inorganic Chemistry’, Longman, 3rd Edition (1992).
  9. Rayner-Canham, Geof., ‘Descriptive Inorganic Chemistry’, W.H. Freeman & Co. (1995).
  10. Jefferey, G.H., J.Bassett, J.Mendham and R.C.Denney, ‘Vogel’s Textbook of Quantitative Chemical Analysis’, 5th Edition, Benjamin-Cummings, (1989).
  11. Vogel, A.I, ‘A Text Book of Macro and Semimicro Qualitative Inorganic Analysis’, Longman Green & Co, (1995).
  12. Skoog, D.A., D.M.West and F.J.Holler, Analytical Chemistry, 6th Edition, Saunders College Publications, (1994).
  13. Graham, H and J.H. Man, Chemistry in Context. 5th Edition, Thomas Nelson Ltd., (2000), U.K.
  14. Philp M., Advance Chemistry, Combridge Low Price Edition, (1996) U.K.
  15. David H. Modern Analytical Chemistry, McGraw Hill International Edition, (2000).