Degree 1st Year 1st Semester Chemistry Full Syllabus Information

                           

        SEMESTER – I

Course I (Inorganic &Physical Chemistry) 60 hrs.(4h/w)

Course outcomes:

At the end of the course, the student will be able to;

1. Understand the basic concepts of p-block elements

2. Explain the difference between solid, liquid and gasesinterms of intermolecular interactions.

3. Applytheconceptsofgasequations,pHandelectrolyteswhilestudyingotherchemistrycour

ses.

INORGANIC CHEMISTRY 24 h

UNIT –I

Chemistry of p-block elements 8h

Group 13: Preparation & structure of Diborane, Borazine

Group 14: Preparation, classification and uses of silicones

Group 15: Preparation & structures of Phosphonitrilic halides {(PNCl2)nwhere

n=3, 4

Group 16: Oxides and Oxoacids of Sulphur (structures only)

Group 17: Pseudohalogens, Structures of Interhalogen compounds.

UNIT-II

1. Chemistry of d-block elements: 6h

Characteristics of d-block elements with special reference to electronic configuration,

variable valence, magnetic properties, catalytic properties and ability to form complexes.

Stability of various oxidation states.

2. Chemistry of f-block elements: 6h

Chemistry of lanthanides - electronic structure, oxidation states, lanthanide contraction,

consequences of lanthanide contraction, magnetic properties. Chemistry of actinides -

electronic configuration, oxidation states, actinide contraction, comparison of lanthanides and

actinides.

3. Theories of bonding in metals: 4h

Valence bond theory andFree electron theory, explanation of thermal and electrical

conductivity of metals based on these theories, explanation of conductors, semiconductors

and insulato

PHYSICAL CHEMISTRY 36h

UNIT-III

Solidstate 10h

Symmetry in crystals. Law of constancy of interfacial angles. The law of rationality of

indices. The law of symmetry. Miller indices, Definition of lattice point, space lattice, unit

cell. Bravais lattices and crystal systems. X-ray diffraction and crystal structure. Bragg's law.

Powder method. Defects in crystals. Stoichiometric and non-stoichiometric defects.

UNIT-IV

1. Gaseous state 6h

van der Waal's equation of state. Andrew's isotherms of carbon dioxide, continuity of state.

Critical phenomena. Relationship between critical constants and vander Waal's constants.

Lawof corresponding states. Joule- Thomson effect. Inversion temperature.

2.Liquid state 4h

Liquid crystals,mesomorphicstate. Differences between liquid crystal and solid/liquid.

Classification of liquid crystals into Smectic and Nematic. Application of liquid crystals as

LCD devices.

UNIT-V

Solutions, Ionic equilibrium& dilute solutions

1. Solutions 6h

Azeotropes-HCl-H2O system and ethanol-water system. Partially miscible liquids-phenol-

water system. Critical solution temperature (CST), Effect of impurity on consulate

temperature. Immiscible liquids and steam distillation.Nernst distribution law. Calculation of

the partition coefficient. Applications of distribution law.

2. Ionic equilibrium 3h

Ionic product, common ion effect, solubility and solubility product. Calculations based on

solubility product.

3. Dilute solutions 7h

Colligative properties- RLVP, Osmotic pressure, Elevation in boing point and depression in

freezing point. Abnormal colligative properties. Van't Hoff factor.