29225 - Basics of Chemistry T

Learning outcomes

The course provides students with the basic principles of Chemistry, in order to understand the properties of the materials and the characteristics of the energetic processes employed in the field of Mechanical Engineering.

Course contents

1. The atomic structure of matter. Atoms and molecules. The fundamental particles of matter and the former atomic models: the Rutherford model. Atomic number and mass number; nuclides and isotopes. Relative and absolute atomic mass; the atomic mass unit. The mole and Avogadro’s number.
2. The structure of the atomic nucleus. Stable nuclides and radionuclides. Radioactivity; the kinetics of radioactive decay. Overview of natural radioactive families. The mass defect. Nuclear fission and its applications; nuclear fusion.
3. The electronic configurations of atoms. The photoelectric effect. The emission spectrum of the hydrogen atom. The Heisenberg uncertainty principle. De Broglie waves. The Schrödinger equation and its application to the hydrogen atom case. Atomic orbitals and quantum numbers. Atoms with more electrons: the spin of the electron and the quantum number of spin; the exclusion principle of Pauli and the Hund rule. The electronic configuration of the main elements. The Periodic Table of the elements; the main periodic properties and their trend along groups and periods.
4. The chemical bond. The ionic bond. The covalent bond. Simple and multiple bonds: sigma and pigreco type bonds. Coordination bonds. The valence bond theory (VB). The valence of the elements. Hybrid orbitals and molecular geometry; the sp, sp², sp³ hybrids; other types of hybridization. Introduction to the VSEPR theory. Polar and apolar molecules. The theory of molecular orbitals (MO). The metallic bond; the band model in solids. Conductors and insulators. Semiconductors and their doping. The weak bonds.
5. Chemical reactions. The stoichiometric equation and its meaning. The nomenclature of the most common inorganic and organic compounds. Redox reactions and their balancing. Stoichiometric calculations.
6. Aggregation states of matter. The gaseous state: the ideal gas model and the gas state equation. The laws of Dalton and Amagat. The compressibility factor. The critical temperature. The liquid state: the vapor pressure and the boiling temperature. Solutions. The solubility of a solid and a gas in a liquid. The solid state: amorphous and crystalline solids; the crystal lattice and the elementary cell. Outline of crystallographic systems and various types of elementary cells. The compact crystalline cells: HCP, BCC, CFC. The main characteristics of the various types of crystalline solids (metallic, ionic, molecular, covalent, etc.). Main defects in crystals: point, line and surface defects.
7. State diagrams. The phase rule and the state diagrams of pure substances. The colligative properties of solutions. Main types of the two-component state diagrams related to the liquid-solid and liquid-vapor equilibria.
8. Chemical kinetics. The reaction rate. The kinetic equation. The order of reaction. Effect of temperature on the reaction rate: the Arrhenius equation; activation energy. Catalysts: general properties; homogeneous and heterogeneous catalysts.
9. Thermochemistry. The first principle of Thermodynamics; internal energy and enthalpy. The thermochemical equations; the standard enthalpy of formation and the standard enthalpy of reaction. Overview of combustion. Hess law.
10. Chemical equilibrium. The chemical equilibrium from a kinetic point of view. Expressions of the equilibrium constants for ideal gaseous systems: K_P and K_c. Calculation of the equilibrium composition. The shift of equilibrium position. Van't Hoff equation.
11. Ionic equilibria in solution. The autoprotolysis of water. Acid, neutral and basic solutions: the pH definition. Acids and bases according to Arrhenius and according to Bronsted and Lowry. Solubility equilibria.
12. Electrochemistry. The Daniell cell. The electromotive force of a battery. The electrochemical series. The Nernst equation. Electrolytic processes: the potential for decomposition; the laws of Faraday. Corrosion in metals and methods of protection.

Readings/Bibliography

R.A. Michelin, A. Munari - " Fondamenti di Chimica ", III Ed., CEDAM, Padova, 2016.

R.A. Michelin, P. Sgarbossa, M. Mozzon, A. Munari - "CHIMICA, Test ed Esercizi", Casa Editrice Ambrosiana, Milano, 2018.

Teaching methods

Lectures. The course is composed by two parts, a theoretical and an exercise one. This latter concerns the resolution of simple exercises regarding stoichiometry, redox reactions and chemical equilibrium

Assessment methods

The assessment methods are a written work and an optional oral interview. The written examination work consists of a number of multiple choice theory quiz (typically 40) and exercises (usually 2), these latter regarding arguments treated in the classroom exercises. To be able to access the optional oral examination, students must obtain a passing grade (at least 18) in the written work, with at least 8 in the quiz part and 5 in the exercises.

Teaching tools

Overhead projector. Copies of a typical examination paper will be available at the copying office near the entrance of the Library 'G.P. Dore'.

Office hours

See the website of Andrea Munari