ATOMIC STRUCTURE, PERIODICITY AND BONDING

Paper Code: 
CHY 101
Credits: 
3
Contact Hours: 
45.00
Max. Marks: 
100.00
Objective: 

Course Objective(s):

This course will enable the students to -

  • gain an in-depth knowledge about different types of bonding in main group elements.
  • understand the concept of hybridization, geometry of covalent molecules, shapes of atomic and molecular orbitals

Course Outcomes (COs):

Course Outcomes

Teaching Learning Strategies

Assessment

Strategies

On completion of this course, 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
  • Use of models
  • Assertion and reasoning
  • Technology enabled learning
  • Peer learning
  • Problem solving exercises
  •  Oral and written examinations
  • Assignments
  • Quiz
  • Efficient delivery using seminar presentations
  • Group activity
  • Multiple choice questions
  • Short answer type questions
  • Assertion and reasoning

 

 



 

 

9.00
Unit I: 
Atomic Structure

Bohr’s theory to hydrogen-like atoms and ions, quantum numbers, qualitative approach of Schrödinger equation and its application to hydrogen atom, 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 configuration.

9.00
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.

9.00
Unit III: 
Chemical Bonding-I

Ionic Bond - general characteristics, 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–Landé equation and its applications, Born-Haber cycle and its applications, solvation energy and solubilities of ionic compounds, polarizing power and polarizability, ionic potential, Fajans’ rules.

Covalent Bond- Lewis structures, octet rule and its exceptions, Valence Bond Theory (Heitler and London approach) and its limitations, concept of resonance and resonating structures of simple inorganic molecules, directional character of covalent bonds, hybridizations, 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.

Self-Study- defects in solids.

 

9.00
Unit IV: 
Chemical Bonding-II

Molecular orbital concept of bonding (elementary pictorial approach)-sigma and pi-bonds, multiple bonding, MO diagrams of homo diatomic (H2, Li2, Be2, B2 C2, N2, O2 and F2), and hetero diatomic molecules (CO, NO, CN and HF) and their ions, bond orders, bond lengths, coordinate bonding- Lewis acid-base adducts.

9.00
Unit V: 
Metallic Bonding and Weak Chemical Forces

Metallic bond- qualitative idea of free electron theory and band theory, conducting, semi conducting and insulating properties with examples from main group elements.
Weak Chemical Forces: Van der Waals interactions - ion-dipole, dipole-dipole, induced-dipole, instantaneous dipole – induced dipole interactions.
Hydrogen bonding- types, theories and properties of H-bond, effects of H-bond on physical properties.

Essential Readings: 
  • Concise Inorganic Chemistry, Fifth Edition; J.D. Lee; Wiley India(P) Ltd, New Delhi, 2008.
  • Principles of Inorganic Chemistry, Thirty Third Edition; B.R. Puri, L.R. Sharma, K.C. Sharma; Vishal Publishing Co., Delhi, 2020.

 

References: 

SUGGESTED READINGS:

  • Inorganic Chemistry, Seventh International Edition; M. Weller, T. Overton, J. Rourke, F. Armstrong; Oxford University Press, New York, 2018.
  • Inorganic Chemistry (Principle of Structure and Reactivity), Fourth Edition; J. E Huheey, E. A. Keiter, R. L. Keiter; Pearson India, New Delhi, 2013.
  • Inorganic Chemistry, Fifth Edition; G. L. Miessler and D. A. Tarr; Pearson Education Inc. Singapore, 2013.

 

e-RESOURCES:

 

Academic Year: 
2022-2023
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