Chemical Structure and Bonding
At the end of this curricular unit, students should have aquired knowledge and skills which will allow them to:
Apply general concepts of quantum mechanics
Predict atomic and mlecular properties
Predic Lewis Strucutures.
Predict electronic structure and molecular geometry through Valence Bond Theory and Molecular Orbital Theory
Predict molecular properties (bond order and distance, paramagnetism, acid/base behaviour, nucleofilicity and electrofilicity, ioniztion energy, electron afinity, conductor, semi-conductor or insulating properties, etc.)
Use Molecular Orbital Theory to predict and rationalize chemical reactivity in simple molecules.
António Gil de Oliveira Santos
Weekly - 4
Total - 57
R. L. Deckock, H. B. Gray, Chemical Structure and Bonding, University Science Books, Sausalito, California,1989
The program of Chemical Structure and Bonding is transmitted in Portuguese during 39 hours of theoretic-practical classes (3 hours per week), followed by 18 hour of pratical classes (1.5 hours per week) dedicated to the resolution of typical exercises and discussion with the students.
Atomic structure: Historical revision. Bohr''''s model applied to the hydrogen atom. Wavelike behaviour. Heisenberg''''s uncertainty principle. Schrödinger''''s equation. Eigenvalues and eigenfunctions. Wavefunction normalization. Particle in a one-dimensional box. Quantic numbers and the boxs dimensionality. Atomic orbitals and energy levels. Radial distribution function. Angular moments. Polielectronic atoms. Periodic properties.
Molecules. Lewis structures. Molecular geometry. Molecular structure: Ionic bonding and crystal lattice energy. Covalent bonding. Valence bond theory. Linear combination of atomic orbitals, Molecular orbital theory. Molecular orbital energy diagrams of diatomic and poliatomic molecules. Chemical reactivity according to the frontier orbital theory. Lewis acids and bases. Formation of aducts. Nucleophiles and electrophiles.