00088 - Chemistry (A-L)

Learning outcomes

Upon completion of the course, the student will have acquired fundamental knowledge of chemistry and will be able to apply this knowledge to the resolution of numerical problems. Furthermore, the student will recognize chemistry as an interdisciplinary, useful, and innovative science.

Course contents

Fundamental principles of chemistry: the scientific method, properties of matter, measurements and units, significant figures. Elements, compounds, and mixtures; states of matter; the Law of Conservation of Mass (Lavoisier), the Law of Definite Proportions (Proust), and Dalton’s atomic theory. Atoms and atomic mass. The concept of the mole and Avogadro’s number.

Atomic structure: subatomic particles, their mass and charge, atomic number, mass number, and isotopes. Empirical, molecular, and structural formulas; atomic and molecular weights; stoichiometric calculations.

Overview of atomic theory (Schrödinger, Heisenberg). Quantum numbers. Shape and orientation of orbitals. The concept of electron probability density. Multi-electron atoms. Aufbau principle, Hund’s rule, and Pauli exclusion principle. Construction of electronic configurations.

The Periodic Table: organization based on quantum level filling. Periodic trends in atomic properties: ionization energy, electron affinity, and electronegativity.

Chemical bonding: nomenclature and geometry of selected inorganic and organic molecules (as listed in course materials). Lewis structures and formal charges. The Valence Shell Electron Pair Repulsion (VSEPR) model. Bonding and lone pairs. Covalent and polar covalent bonds. Valence Bond Theory. Hybrid orbitals: sp, sp², sp³; examples include BeH₂, BH₃, CH₄, H₂O, and NH₃. Effect of lone pairs. Multiple bonds. Resonance structures with reference to benzene. Molecular Orbital Theory. Homonuclear diatomic molecules: bonding and antibonding orbitals, molecular orbital filling, single, double, and triple bonds. Paramagnetism in O₂. Heteronuclear diatomic molecules: bond polarity, electronegativity differences, ionic character, and dipole moments in diatomic and polyatomic molecules. Introduction to HOMO, LUMO, and delocalized orbitals.

Ionic bonding and lattice energy.

Metallic bonding and band theory: conductors, insulators, and semiconductors. Diodes and photovoltaic cells.

Intermolecular forces: hydrogen bonding, van der Waals interactions, dipole–dipole, and ion–dipole interactions.

States of matter: solid, liquid, and gas. Amorphous vs. crystalline solids. Crystal packing: metals and ionic solids. Body-centered and face-centered cubic lattices, interstitial sites, and defects.

Ionic solids: lattice types based on ionic radii. Brief overview of molecular solids and crystallography: crystal lattices, diffraction phenomena, and Bragg’s law.

Physical and chemical changes.

Chemical reactions: writing and balancing chemical equations; stoichiometric calculations; limiting reagents. Types of reactions: acid–base, redox, precipitation, and exchange reactions.

Concentration units: molarity, molality, mass percent, and mole fraction.

Thermochemistry: First Law of Thermodynamics, heat of reaction, enthalpy, Hess’s law, standard enthalpies of formation. Qualitative introduction to statistical derivation of entropy. Second and Third Laws of Thermodynamics, absolute entropy. Gibbs free energy: enthalpic and entropic contributions, temperature effects on spontaneity (ΔG).

Chemical equilibrium: chemical potential and equilibrium conditions, equilibrium constant (K) and reaction quotient (Q). Le Chatelier’s principle. Effect of temperature, pressure, and concentration on equilibrium. Homogeneous and heterogeneous equilibria. Solubility product (Ksp) and slightly soluble salts.

Phase equilibria overview: P–T diagrams, vapor pressure.

Colligative properties: boiling point elevation, freezing point depression, and osmotic pressure.

Electrochemistry: Galvanic cells, standard reduction potentials, free energy and useful work, Nernst equation. Batteries and accumulators (lead-acid batteries, lithium batteries, fuel cells). Electrolytic cells: electrolysis of molten salts and aqueous solutions. Corrosion.

Note: The syllabus may be subject to modifications during the course.

Readings/Bibliography

Authors: Balzani, Moggi, Prodi, Venturi
Title: Chemistry: Fundamentals and Perspectives
Publisher: Bononia University Press

Author: S. S. Zumdhal
Title: Chemistry
Publisher: Zanichelli

Teaching methods

Lectures and Blackboard Exercises

Assessment methods

The exam consists of a written test. Upon passing it, the student may request an additional oral examination.

The following materials will be allowed during the exam:

• a calculator;

• a periodic table;

• one A4 double-sided sheet with notes and formulas.

Students with certified disabilities or specific learning disorders (SLD) are encouraged—if they deem it appropriate—to contact the instructor in order to arrange for additional time during the exam. The request must be made by email at least 7 days prior to the exam date, with the relevant office in copy:

https://site.unibo.it/studenti-con-disabilita-e-dsa/en/contacts

Teaching tools

The teaching materials used during the lectures will be made available to students on the Virtuale platform.

Office hours

See the website of Giuseppe Falini