Utkal University, Odisha, Chemistry Semester 1, Inorganic Chemistry-I Syllabus

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INORGANIC CHEMISTRY-I

Unit-I: Atomic structure
Bohr’s theory, its limitations and atomic spectrum of hydrogen atom, Sommerfeld’s modification. Wave mechanics: de Broglie equation, Heisenberg’s Uncertainty Principle, Schrödinger’s wave equation (time independent) and its significance, Derivation of Schrödinger’s wave equation (for hydrogen atom) in Cartesian coordinate, significance of ψ and ψ2. Normalized and orthogonal wave functions. Sign of wave functions; Setting of Schrödinger’s equation in polar coordinates (derivation not required), radial and angular wave functions for hydrogen atom. Radial and angular distribution curves; Shapes of s, p, d and f orbitals; Quantum
numbers and their significance. Pauli’s Exclusion principle, Hund’s rule of maximum multiplicity, Aufbau’s principle and its limitations.

Unit-II: Periodicity of elements
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 & p-blocks. (a) Effective nuclear charge, shielding or screening effect, Slater rules, variation of effective nuclear charge in periodic table. (b) Atomic radii (van der Waals) (c) Ionic and crystal radii. (d) Covalent radii (octahedral and tetrahedral) (e) Ionization enthalpy, Successive ionization enthalpies and factors affecting ionization energy. Applications of ionization enthalpy. (f) Electron gain enthalpy, trends of electron gain enthalpy. (g) Electronegativity, Pauling’s/ Mulliken’s electronegativity scales. Variation of electronegativity with bond order, partial charge, hybridization. Sanderson’s electron density ratio.

Unit-III: Chemical bonding-I
(i) 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. Madelung constant, Born-Haber cycle and its application, Solvation energy.
(ii) Covalent bond: Valence Bond theory (Heitler-London approach). Hybridization with suitable examples of linear, trigonal planar, square planar, tetrahedral, trigonal bipyramidal and octahedral arrangements, equivalent and non-equivalent hybrid orbitals, Resonance and resonance energy.
Molecular orbital theory. Molecular orbital diagrams of diatomic and simple polyatomic molecules N2, O2, C2, B2, F2, CO, NO, and their ions (CO+, NO+, NO-).

Unit-IV: Chemical bonding-II
VSEPR theory, shapes of simple molecules and ions containing lone 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.

(i) Metallic Bond: Qualitative idea of valence bond and band theories. Semiconductors and insulators.
(ii) 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.

Oxidation-reduction: Redox equations, standard electrode potential and its applications to inorganic reactions. Principles involved in some volumetric analyses (iron and copper).

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