Inorganic Chemistry I

Paper Code: 
CHY-111
Credits: 
3
Contact Hours: 
45.00
Objective: 

Course Objectives:

This course will enable the students to -

 

  1. have an in-depth knowledge about different types of bonding in main group elements.

  2. be acquainted with the concept of hybridization and geometry of covalent molecules, shapes of atomic and molecular orbitals

Course Outcomes (COs):

Course

Learning outcomes

(at course level)

Learning and teaching strategies

Assessment

Strategies

Paper Code

Paper Title

CHY-111

Inorganic Chemistry

 

 

The students will be able to –

 

CO1: explain Bohr’s theory and concept of    wave function and quantum numbers

CO2: calculate the radius ratio of ionic molecules and determine the ionic structures of the type AX and AX2

 CO3: appraise the concept of Born-Haber cycle and predict the lattice energy, ionization energy and stability of the ionic compounds.

CO4: predict physical and chemical characteristics of elements in various groups and periods according to ionic size, charge, etc. and position in periodic table and describe various types of hybridization and geometry of molecules.

CO5: construct molecular orbital diagrams of homo and hetero nuclear diatomic molecules and determine the bond order with the help of M.O. diagram.

CO6: discuss the different theories of metallic bonding, hydrogen bonding and Van der Waals interaction.

Class lectures

Tutorials

Group discussions

Model Study

Question preparation

  • Subjective type
  • Long answer
  • Short answer
  • Objective type
  • Multiple choice questions
  • One answer/two answer type questions
  • Assertion and reasoning

Oral and written examinations (Scheduled and surprise tests)

 

 Closed-book and open book tests

 

Problem solving exercises

 

 Assignments

 

Quiz

 

Semester End Examination

 

 

10.00
Unit I: 
Atomic Structure

Bohr’s theory to hydrogen-like atoms and ions; spectrum of hydrogen atom. Quantum numbers. Introduction to the concept of atomic orbitals; shapes, radial and angular probability diagrams of s, p and d orbitals (qualitative idea). Many electron atoms and ions: Pauli’s exclusion principle, Hund’s rule, exchange energy, Aufbau principle and its limitation. Electronic energy level diagram and electronic configurations of hydrogen-like and polyelectronic atoms and ions up to atomic number 30.

 

12.00
Unit II: 
Chemical Periodicity

Periodic table, group trends and periodic trends in physical properties.Classification of elements on the basis of electronic configuration. Modern IUPAC Periodic table. General characteristic of s, p, d and f block elements. Position of hydrogen and noble gases in the periodic table. Effective nuclear charges, screening effects, Slater’s rules, atomic radii, ionic radii (Pauling’s univalent), covalent radii. Ionization potential, electron affinity and electronegativity (Pauling, Mulliken and Allred-Rochow scales) and factors influencing these properties. Inert pair effect. 

7.00
Unit III: 
Ionic Bonding

Size effects, radius ratio rules and their limitations. Packing of ions in crystals, ionic compounds of the type AX (ZnS, NaCl, CsCl) and AX2 (CaF2-fluorite) lattice energy, Born–Landéequation and its applications, Born-Haber cycle and its applications. Solvation energy, polarizing power and polarizability, ionic potential, Fajans’ rules. Defects in solids.

8.00
Unit IV: 
Covalent Bonding

Lewis structures, formal charge. Valence Bond Theory, directional character of covalent bonds, hybridizations, equivalent and non-equivalent hybrid orbitals, Bent’s rule, VSEPR theory, shapes of molecules and ions containing lone pairs and bond pairs (examples from main groups chemistry), partial ionic character of covalent bonds, bond moment, dipole moment and electronegativity differences. Concept of resonance, resonance energy, resonance structures.

 

8.00
Unit V: 
Other Types of Bonding

Molecular orbital concept of bonding (elementary pictorial approach):sigma and pi-bonds, multiple bonding, MO diagrams of H2, F2, O2, C2, B2, CO, NO, HF, and H2O; bond orders, bond lengths, Walsh Diagram. Coordinate bonding: Lewis acid-base CN-,adducts (examples), double salts and complex salts.

Hydrogen bonding: Effect on the physical properties of compounds of the main group elements.

Metallic bonding: Qualitative idea of band theory, conducting, semi conducting and insulating properties with examples from main group elements.

 

References: 
  • Concise Inorganic Chemistry; Fifth Edition; J.D. Lee; Wiley India(P) Ltd, New Delhi, 2008.
  • Inorganic Chemistry; Seventh International Edition; M. Weller,T. Overton, J. Rourke, F. Armstrong; OxfordUniversity Press, New York, 2018.

 

Academic Year: 
2021-2022
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