INORGANIC CHEMISTRY I: ATOMIC STRUCTURE & CHEMICAL BONDING

Paper Code: 
C-CHY 111
Credits: 
4
Contact Hours: 
60.00
Max. Marks: 
100.00
Objective: 

Course Objective(s):
This course will enable the students to-

understand the fundamental concepts of atomic structure, comprehend the general characteristics of s, p, d, and f block elements including periodic trends in physical properties, acquire a thorough understanding of various bonding types in main group elements, explore the concept of hybridization, analyze the geometry of covalent molecules, and examine the 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: describe the principles of quantum mechanics and predict electronic configurations of atoms, and their stability.

CO2: discuss the periodicity of chemical and physical properties of elements across the periodic table.

CO3: discuss the general characteristics and properties of ionic and covalent bonding, explain the shapes of inorganic molecules and ions using VSEPR theory and hybridization.

CO4: construct molecular orbital diagrams of homo and hetero nuclear diatomic and triatomic molecules and determine the bond order.

CO5: discuss the different theories of metallic bonding, hydrogen bonding and Vander Waals interaction.
  • Interactive lectures
  • Tutorials
  • Group discussions
  • Use of models
  • Digital learning
  • Peer learning
  • Problem solving sessions

 

 
  • Oral and written examinations
  • Assignments
  • Quiz

 

 

12.00
Unit I: 
Atomic Structure

Bohr’s theory, its limitations and atomic spectrum of hydrogen atom. Wave mechanics: de Broglie equation, Heisenberg’s uncertainty principle and its significance, Schrödinger’s wave equation, significance of ψ and ψ2, quantum numbers and their significance, normalized and orthogonal wave functions, sign of wave functions, radial and angular wave functions for hydrogen atom, radial and angular distribution curves, shapes of s, p, d and f orbitals, contour boundary and probability diagrams. Pauli’s exclusion principle, Hund’s rule of maximum multiplicity, Aufbau’s principle and its limitations, variation of orbital energy with atomic number.

12.00
Unit II: 
Periodicity of Elements

s, p, d, f block elements, the long form of periodic table. Detailed discussion of the following properties of the elements, with reference to s and p-block:

  • Effective nuclear charge, shielding or screening effect, Slater rules, variation of effective nuclear charge in periodic table.
  • Atomic radii (van der Waals)
  • Ionic and crystal radii.
  • Covalent radii (octahedral and tetrahedral)
  • Ionization enthalpy, successive ionization enthalpies and factors affecting ionization energy, applications of ionization enthalpy.
  • Electron gain enthalpy, trends of electron gain enthalpy.
  • Electronegativity, Pauling’s/ Mulliken’s/ Allred Rachow’s/ and Mulliken-Jaffé’s electronegativity scales, variation of electronegativity with bond order, partial charge, hybridization, group electronegativity, Sanderson’s electron density ratio.

 

18.00
Unit III: 
Chemical Bonding

Ionic bond: General characteristics, types of ions, size effects, radius ratio rule and its limitations,packing of ions in crystals, Born-Landé equation with derivation and importance of Kapustinskii expression for lattice energy, Madelung constant, Born-Haber cycle and its application, solvation energy.

Covalent bond: Lewis structure, Valence Bond theory (Heitler-London approach). energetics of hybridization, equivalent and non-equivalent hybrid orbitals, Bent’s rule, resonance and resonance energy, formal charge, Valence Shell Electron Pair Repulsion theory (VSEPR), shapes of simple molecules and ions containing lone pairs and bond pairs of electrons, multiple bonding (σ and π bond approach) and bond lengths, covalent character in ionic compounds, polarizing power and polarizability, Fajan’s rules and consequences of polarization.

Ionic character in covalent compounds: Bond moment and dipole moment, percentage ionic character from dipole moment and electronegativity difference.

12.00
Unit IV: 
Molecular Orbital Theory

  LCAO approach, molecular orbital diagrams of diatomic and simple polyatomic molecules N2, O2, C2, B2, F2, CO, NO, and their ions, HCl, BeF2, CO2(idea of s-p mixing and orbital interaction to be given).

8.00
Unit V: 
Metallic Bonding and Weak Chemical Forces

Metallic Bond: Qualitative idea of valence bond and band theories, semiconductors and insulators, defects in solids.

Weak Chemical Forces: van der Waals forces, ion-dipole forces, dipole-dipole interactions, induced dipole interactions, instantaneous dipole-induced dipole interactions, repulsive forces. Hydrogen bonding (theories of hydrogen bonding, valence bond treatment),effects of chemical force, melting and boiling points, solubility energetics of dissolution process.

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. Kalia; 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, Fifth Edition; G. L. Miessler and D. A. Tarr; Pearson Education Inc. Singapore, 2013.

e-RESOURCES:

Academic Year: 
2023-2024
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