Gauhati University Question Papers for Chemistry 3rd Semester
Gauhati University Question Papers for Chemistry 3rd Semester
Question Paper from 2010 available
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Semester III
PAPER
M 301 Structure and Bonding
Unit 3.1 Atomic Structure
Learning
Structure of hydrogen-like atoms and their representation in
quantum mechanical terms. Basic quantum mechanical ideas and
principles leading
to atomic structure (outline only without details) :
a)
Particle character of radiation - black body radiation phenomenon - Planck’s
hypothesis : Postulates and explanation for black body
radiation.
b) Wave
character of particles-electron diffraction.
c)
Discrete nature of energy levels of atomic and molecular systems, line
spectra
of atoms (e.g., hydrogen) and molecules
(e.g.N2O).matter-de Broglie hypothesis.
d)
Dual nature of matter-de Broglie hypothesis. e) The defining limit
of
classical mechanics-the uncertainty principle.
f)
Definition of micro and macro particles.
g)
Necessity of quantum mechanical equation.
h)
Schrodinger equation-statement and identity of terms. Energy eigenvalues-
expression alone. Energy eigenfunctions: Setting up of expressions of radial(
R)
and angular( Y) parts for 1s,2s,2po,2p+1,2p-1,2px,2py,2pz orbital, Born
interpretation of the wave functions, Orbital concept-one electron wave
functions,
Plots of
and ψ2 for 1s,2s,2p,2px,2py,2pz,3dxy,3dzx orbital.n,l,m quantum numbers-
origin
and significance(outline only).
i)
The concept of spin and spin quantum numbers (outline only).Many
electron
atoms. Electron repulsion in the He atom. Pauli’s exclusion principle.
Aufbau
principle and electron configuration of many electron atoms.
j)
Effective nuclear charge-shielding and penetration effects. Electron
Configuration of atoms.
Unit
3. 2 Chemical Bonding I
Lewis
electron pair bond. Valence bond approach to bonding in
diatomic molecules- outline of concept of overlap ( HF
and H2 ). Resonance and
resonance energy in HF and
benzene. Bond moments and dipole moments (outline
with simple
pictorial representation). Percent ionic character of HCl and HF bonds.
Formal
charges on atoms
in molecules.
Concept of electro negativity -explanation of molecular properties on
the basis of electro negativity.
PAPER
M 302
Unit
3.3 Chemical Bonding II
Shapes
of molecules- VSEPR theory, hybrid orbital and hybridization in
polyatomic molecules-influence of hybridization on bond length, bond angle
and
other properties of molecules including shapes and
dipole moments. Effects of
structure on molecular
properties- steric effects and electronic effects.
Unit
3.4 Chemical Bonding III
Molecular
orbital theory of homonuclear diatomic molecules
( N2, O2, F2,CO, NO
etc).Graphical representation of
angular parts of the
wave function( H2+ molecule ion).
Energy levels,
electronic configuration of ground states of diatomic molecules.
Setting
up of the wave functions and energy level diagrams for H2 molecules
without calculations. Multicentre bonding( diborane);MOs of simple triatomic
systems ( BeH2,H2O,NO2);Multiple bonding, orbital
picture and energy of
ethane,ethyne and benzene; Huckel’ s aromaticity
rule.Delocalisition vs.
Resonance; bond energy; bond length and covalent radii.
Bonding in metals (band
theory); properties consequent from Band theory.
Unit
3.5 Ionic Bonds and Solids
Types of solids, macroscopic
properties of solids, properties of ionic compounds;
types of unit
cells; crystal lattices and Miller indices; crystal system and Bravais
lattices.Closed packed structures, ionic radii; radius ratio and structures;
Spinel and
Perovskite
structures,
Lattice energy of ionic solids; Born- Haber cycle-calculations; Covalent
character of ionic bonds-Fajan’s rules of polarization. Inter-molecular
forces-
dipole moment and molecular polarisability. Molecular solids;
Hydrogen bonding
and its effect on physical properties.
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