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States of Matter

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1.Course Title
2.Course Category 
3.Type of Course
4.Course Objectives 
5.Course Outcomes 
Unit 1.Gaseous State.
Unit 2. Liquid State.
Unit 3.Solid State.
Unit 4.Ionic equilibria.

1.Course Title.

  • States of Matter

2.Course Category.

  • Major

3.Type of Course.

  • Theory

4.Course Objectives.

  • Basics Concepts.
  • Advance Concepts
  • Derive expressions
  • Concepts of ionization, pH and buffers.
  • Applications of ionization


5.Course Outcomes.

  • Mathematical expressions
  • Understand physical significance.
  • Crystal Structures
  • Cubic System
  • Ionization
  • Weak Acids and bases.
  • Hydrolysis of salt
  • Gas Equation
  • Everyday life

Unit 1.Gaseous State.

Kinetic molecular model of a gas: postulates and derivation of the kinetic gas equation; collision frequency; collision diameter; mean free path. Maxwell distribution and its use in evaluating molecular velocities (average, root mean square and most probable) and average kinetic energy. Behaviour of real gases: Deviations from ideal gas behaviour, compressibility factor, Z, and its variation with pressure and temperature for different gases. Causes of deviation from ideal behaviour. Equation of states for real gases; van der Waals equation of state, its derivation and application in explaining real gas behaviour, van der Waals equation expressed in virial form and calculation of Boyle temperature. Isotherms of real gases and their comparison with van der Waals isotherms, continuity of states, critical state, relation between critical constants and van der Waals constants, law of corresponding states. 

Unit 2. Liquid State.

Qualitative treatment of the structure of the liquid state; physical properties of liquids; vapour pressure, surface tension and coefficient of viscosity, and their determination. Effect of addition of various solutes on surface tension and viscosity. Explanation of cleansing action of detergents. Temperature variation of viscosity of liquids and comparison with that of gases

Unit 3.Solid State.

Definition of space lattice, unit cell. symmetry elements and symmetry operations, qualitative idea of point and space groups, seven crystal systems and fourteen Bravais lattices. Laws of crystallography - (i) Law of constancy of interfacial angles (ii) Laws of rationality of indices (iii) Law of symmetry. Symmetry elements in crystals. X-ray diffraction by crystals. Derivation of Bragg’s equation. A simple account of rotating crystal method and powder pattern method. Analysis of powder diffraction patterns of NaCl, CsCl and KCl. Defects in crystals.

Unit 4.Ionic equilibria.

Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of ionization, ionization constant and ionic product of water. Ionization of weak acids and bases, pH scale, common ion effect; dissociation constants of mono and diprotic acids. Salt hydrolysis-calculation of hydrolysis constant, degree of hydrolysis and pH for different salts. Buffer solutions; derivation of Henderson equation and its applications. Solubility and solubility product of sparingly soluble salts – applications of solubility product principle. Qualitative treatment of acid – base titration curves (calculation of pH at various stages). Theory of acid–base indicators; selection of indicators and their limitations

.Books*/ 

References

.

References: 
  •  1. Atkins, P.W.; Paula, J.de. (2014), Atkin’s Physical Chemistry Ed., 10th Edition, Oxford 
  • 2. University Press. 
  • 3. Principles of Physical Chemistry, B.R. Puri & L.R. Sharma, Shoban Lal Nagin Chand & Co. 
  • 4. Castellan, G. W. (2004), Physical Chemistry, 4th Edition, Narosa. 
  • 5. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol 1, 6th Edition, McGraw Hill Education.

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