96453 - General Chemistry and Laboratory

Learning outcomes

At the end of the course,

... the student understands the theoretical foundations necessary for understanding the structure of matter, including its atomic and molecular constituents. He/she possesses a method suited to the scientific treatment of phenomena, based on models adequate for the rigorous description of thermodynamic and kinetic aspects.

... the student is able to transfer a chemical problem to a stoichiometric calculation framework. In this framework, he/she is able to correctly consider both numerical aspects and units of measurement. The student has understood the importance of adequately considering the grammar and spelling of chemistry, consisting of all the conventions that describe atoms and the interactions between them.

Course contents

Theoretical teaching unit (39 hours)

General Chemistry

Atomic structure and characteristics of atoms. Concept of quantized energy. Quantum numbers and visualization of orbitals. Pauli and Hund principles. Organization of elements in the periodic table and periodic trends in their properties. Types of chemical bonds: ionic, covalent, and metallic. Formation of hybrid orbitals and molecular orbital theory. Three-dimensional structure of molecules, use of Lewis structures, and application of the VSEPR model. Physical states of matter: solid and gaseous. Fundamental laws of gases and behavior of real gases. Overview of thermodynamics and chemical kinetics. Liquid state and formation of solutions. Intermolecular forces and interpretation of phase diagrams. Definition and classification of acids and bases according to the Arrhenius, Brønsted-Lowry, and Lewis models. Acid and base intensity, the ionic product of water, and the concept of pH.

Stoichiometry

Fundamental concepts of matter and chemical measurements. Avogadro's constant and definition of the mole. Calculation of atomic and molecular masses, and use of molar mass. Quantitative interpretation of chemical formulas. Determination of the percent mass composition of elements within a compound. Analysis of molar and weight ratios in chemical reactions. Balancing chemical equations, both in the absence and presence of electron transfer. Quantitative value of a balanced chemical equation. Identifying the limiting reagent and determining the yield of a reaction. Preparing solutions and calculating concentration. Behavior of ideal gases and related physical laws. Study of chemical equilibrium: definition of equilibrium constants and analysis of the influence of changes in concentration, pressure, and temperature. Ionic equilibria in aqueous environments: distinction between strong and weak electrolytes; characteristics of neutral, acidic, and basic solutions; concepts of pH and pOH. Calculating the pH for solutions containing acids and bases, both strong and weak. Behavior of acid-base mixtures: hydrolysis phenomena and buffer solutions. Heterogeneous equilibria related to solubility: solubility product constant, influence of the common ion and pH on solubility equilibrium.

Organic Chemistry

Carbon structure and hybridization; Functional classes: alkanes, alkenes, alkynes, alcohols, acids, amines; Basic nomenclature; Isomerism: structural, geometric, optical; Main organic reactions: substitution, addition, elimination; Introduction to polymers or biomolecules.

Laboratory teaching unit (9 hours)

Students will be provided with explanations in class on how to set up a laboratory experiment to highlight specific properties of a substance or sample of interest. This will be followed by practical laboratory exercises with two objectives: to familiarize students with the instrumentation and safety regulations of the chemical laboratory; and to develop the ability to connect the results of an empirical experiment to the concepts acquired during lectures. The aspects that will be focused on are solubility issues, acid-base properties, and reactions between organic molecules.

Readings/Bibliography

Students are free to choose the textbook they wish to use for the exam, provided it is of a university level.

My favorite texts today are those that, contrary to the traditional approach, dedicate the first chapter to the description of the atom. Among them, I found

Del Zotto A. - General Chemistry Exercises - EdiSES

Anfuso F., Palmisano L. - Guide to Solving Chemistry Exercises - EdiSES

Bertini I., Luchinat C., Mani F. - Stoichiometry. An Introduction to the Study of Chemistry - CEA

Wade – Fundamentals of Organic Chemistry – Piccin

Teaching methods

Teaching Methods

The course consists of lectures, supported by slides and excerpts from textbooks, animations, and videos.

Classroom exercises involving the solution of numerical problems on the board and practical demonstrations are also included.

Finally, laboratory activities are included, with hands-on experience. Attendance at the laboratory activities requires all students to complete Modules 1 and 2 via e-learning [https://www.unibo.it/it/servizi-e-opportunita/salute-e-assistenza/salute-e-sicurezza/sicurezza-e-salute-nei-luoghi-di-studio-e-tirocinio] and to participate in Module 3, a specific training course on health and safety in the workplace. Information on the dates and attendance methods for Module 3 can be found in the relevant section of the program website.

Assessment methods

Assessment and Evaluation Methods

The exam consists of a written and an oral test. Each written exam is offered on two closely spaced dates, allowing students to choose the one that best fits their schedule. Each new exam cancels all previous ones. The result of the final written exam is valid for one year. Only students who have obtained a grade of 18/30 or higher in the written exam are admitted to the oral exam.

The end-of-course exam aims to assess the achievement of the following learning objectives:

• Transfer a chemical problem to a stoichiometric calculation setting. In this setting, both numbers and units of measurement must be correctly considered. Chemistry describes atoms and the interactions between them through conventions, such as lines that indicate chemical bonds, dots that indicate electrons, and subtraction and addition symbols that identify negative and positive charges. These conventions are the equivalent of grammar and spelling for the writer. Errors in these areas will be treated with equal severity.

• Describe the composition of matter and the phenomena that lead to its transformations with appropriate language and scientific rigor.

Teaching tools

Learning materials projected during class, of necessarily lower quality than textbook pages, will be made available to students in electronic format on Virtuale.

Office hours

See the website of Luca Laghi